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Chemistry

Kenneth W. Whitten, Raymond E. Davis, Larry Peck

Chapter 4

The Structure of Atoms - all with Video Answers

Educators

Chapter Questions

01:08

Problem 1

List the three fundamental particles of atoms, and indicate the mass and charge associated with each.

Nicole Smina
Nicole Smina
Numerade Educator
01:29

Problem 1

Define and illustrate the following terms clearly and concisely: (a) representative elements; (b) $d$ -transition elements; (c) inner transition elements.

Lottie Adams
Lottie Adams
Numerade Educator
03:07

Problem 2

In the oil-drop experiment, how did Millikan know that none of the oil droplets he observed were ones that had a deficiency of electrons rather than an excess?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:42

Problem 2

The third shell $(n=3)$ has $s, p$, and $d$ subshells. Why does Period 3 contain only eight elements?

Lottie Adams
Lottie Adams
Numerade Educator
01:09

Problem 3

How many electrons carry a total charge of $1.20$ coulombs?

Sima Sarker
Sima Sarker
Numerade Educator
01:10

Problem 3

Account for the number of elements in Period 5.

Lottie Adams
Lottie Adams
Numerade Educator
03:30

Problem 4

(a) How do we know that canal rays have charges opposite in sign to cathode rays? What are canal rays? (b) Why are cathode rays from all samples of gases identical, whereas canal rays are not?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:09

Problem 4

What would be the atomic number of the as-yet undiscovered alkali metal of Period 8 ?

Lottie Adams
Lottie Adams
Numerade Educator
04:23

Problem 5

The following data are measurements of the charges on oil droplets using an apparatus similar to that used by Millikan:
$$
\begin{array}{ll}
3.364 \times 10^{-19} \mathrm{C} & 4.327 \times 10^{-19} \mathrm{C} \\
3.843 \times 10^{-19} \mathrm{C} & 7.211 \times 10^{-19} \mathrm{C}
\end{array}
$$
$$
\begin{array}{ll}
4.326 \times 10^{-19} \mathrm{C} & 2.886 \times 10^{-19} \mathrm{C} \\
3.844 \times 10^{-19} \mathrm{C} & 4.803 \times 10^{-19} \mathrm{C}
\end{array}
$$
Each should be a whole-number ratio of some fundamental charge. Using these data, determine the largest possible value of the fundamental charge.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:20

Problem 5

Identify the group, family, or other periodic table location of each element with the outer electron configuration
(a) $n s^{2} n p^{3} ;$ (b) $n s^{2}$
(c) $n s^{2}(n-1) d^{0-2}(n-2) f^{1-14}$.

Lottie Adams
Lottie Adams
Numerade Educator
04:12

Problem 6

A Suppose we discover a new positively charged particle, which we call the "whizatron." We want to determine its charge. (a) What modifications would we have to make to the Millikan oil-drop apparatus to carry out the corresponding experiment on whizatrons? (b) In such an experiment, we observe the following charges on five different droplets:
$$
\begin{array}{ll}
4.88 \times 10^{-19} \mathrm{C} & 8.53 \times 10^{-19} \mathrm{C} \\
6.10 \times 10^{-19} \mathrm{C} & 7.32 \times 10^{-19} \mathrm{C} \\
2.44 \times 10^{-19} \mathrm{C} &
\end{array}
$$
What is the largest possible value of the charge on the whizatron?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:38

Problem 6

Repeat Exercise 5 for (a) $n s^{2} n p^{5} ;$ (b) $n s^{1} ;$ (c) $n s^{2}(n-1) d^{1-10}$;
(d) $n s^{2} n p^{1}$.

Lottie Adams
Lottie Adams
Numerade Educator
03:28

Problem 7

Outline Rutherford's contribution to understanding the nature of atoms.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:10

Problem 7

Write the outer electron configurations for the (a) alkaline earth metals; (b) first column of $d$ -transition metals; and
(c) alkali metals.

Lottie Adams
Lottie Adams
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04:06

Problem 8

Why was Rutherford so surprised that some of the $\alpha$ -particles were scattered backward in the gold foil experiment?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:36

Problem 8

Which of the elements in the following periodic table is (are)
(a) alkali metals; (b) an element with the outer configuration of $d^{7} s^{2} ;$ (c) lanthanides; (d) $p$ -block representative elements;
(e) elements with partially filled $f$ -subshells; (f) halogens;
(g) s-block representative elements; (h) actinides; (i) $d$ -transition elements; (j) noble gases; (k) alkaline earth elements?

Lottie Adams
Lottie Adams
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03:15

Problem 9

Summarize Moseley's contribution to our knowledge of the structure of atoms.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:05

Problem 9

Identify the elements and the part of the periodic table in which the elements with the following configurations are found. (a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} ;$ (b) $[\operatorname{Kr}] 4 d^{8} 5 s^{2} ;$ (c) [Xe]
$4 f^{14} 5 d^{5} 6 s^{1} ;$ (d) $[\mathrm{Xe}] 4 f^{9} 6 s^{2} ;(\mathrm{e})[\mathrm{Kr}] 4 d^{10} 5 s^{2} 5 p^{4} ;$ (f) $[\mathrm{Kr}]$
$4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{1}$

Lottie Adams
Lottie Adams
Numerade Educator
04:23

Problem 10

The approximate radius of a hydrogen atom is $0.0529 \mathrm{~nm}$, and that of a proton is $1.5 \times 10^{-15} \mathrm{~m}$. Assuming both the hydrogen atom and the proton to be spherical, calculate the fraction of the space in an atom of hydrogen that is occupied by the nucleus. $V=(4 / 3) \pi r^{3}$ for a sphere.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:59

Problem 10

(a) Which ions in this list are likely to be formed: $\mathrm{K}^{2+}$, $\mathrm{Cs}^{+}, \mathrm{Al}^{4+}, \mathrm{F}^{2-}, \mathrm{Se}^{2-} ?(\mathrm{~b})$ Which, if any, of these ions have a
noble gas configuration?

Lottie Adams
Lottie Adams
Numerade Educator
02:28

Problem 11

The approximate radius of a neutron is $1.5 \times 10^{-15} \mathrm{~m}$, and the mass is $1.675 \times 10^{-27} \mathrm{~kg}$. Calculate the density of a neutron. $V=(4 / 3) \pi r^{3}$ for a sphere.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:21

Problem 11

Give the electron configurations of these ions, and indicate which ones are isoelectronic. (a) $\mathrm{Ca}^{2+}$ (b) $\mathrm{K}^{+}(\mathrm{c}) \mathrm{O}^{2-}$

Lottie Adams
Lottie Adams
Numerade Educator
01:23

Problem 12

Arrange the following in order of increasing ratio of charge to mass: ${ }^{12} \mathrm{C}^{+},{ }^{12} \mathrm{C}^{2+},{ }^{14} \mathrm{~N}^{+},{ }^{14} \mathrm{~N}^{2+}$.

Nicole Smina
Nicole Smina
Numerade Educator
02:39

Problem 12

What is meant by nuclear shielding? What effect does it have on trends in atomic radii?

Lottie Adams
Lottie Adams
Numerade Educator
05:59

Problem 13

Refer to Exercise 12. Suppose all of these high-energy ions are present in a mass spectrometer. For which one will its path be changed (a) the most and (b) the least by increasing the external magnetic field? Which of the ions would take (c) the longest time and (d) the shortest time to travel a given distance in a time-of-flight mass spectrometer?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:58

Problem 13

Why do atomic radii decrease from left to right within a period in the periodic table?

Lottie Adams
Lottie Adams
Numerade Educator
01:38

Problem 14

Estimate the percentage of the total mass of a ${ }^{58} \mathrm{Ni}$ atom that is due to (a) electrons, (b) protons, and
(c) neutrons by assuming that the mass of the atom is simply the sum of the masses of the appropriate numbers of subatomic particles.

Nicole Smina
Nicole Smina
Numerade Educator
01:55

Problem 14

Consider the elements in Group 6A. Even though it has not been isolated or synthesized, what can be predicted about the atomic radius of element number $116 ?$

Lottie Adams
Lottie Adams
Numerade Educator
03:55

Problem 15

(a) How are isotopic abundances determined experimentally? (b) How do the isotopes of a given element differ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:52

Problem 15

Variations in the atomic radii of the transition elements are not as pronounced as those of the representative elements. Why?

Lottie Adams
Lottie Adams
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02:14

Problem 16

Clearly define and provide examples that illustrate the meaning of each: (a) atomic number, (b) isotope, (c) mass number, (d) nuclear charge.

Nicole Smina
Nicole Smina
Numerade Educator
01:53

Problem 16

Arrange each of the following sets of atoms in order of increasing atomic radii: (a) the alkaline earth elements; (b) the noble gases; (c) the representative elements in the third period; (d) C, Si, Sn, and Pb.

Lottie Adams
Lottie Adams
Numerade Educator
00:43

Problem 17

Write the composition of one atom of each of the three isotopes of silicon: ${ }^{28} \mathrm{Si}$, ${ }^{29} \mathrm{Si}$, ${ }^{30} \mathrm{Si}$.

Nicole Smina
Nicole Smina
Numerade Educator
01:39

Problem 17

Arrange the following species in order of decreasing radius: $\mathrm{S}, \mathrm{Cl}^{-}, \mathrm{Ar}, \mathrm{K}^{+} .$ Explain your answer

Lottie Adams
Lottie Adams
Numerade Educator
00:51

Problem 18

Write the composition of one atom of each of the four isotopes of strontium: ${ }^{84} \mathrm{Sr},{ }^{86} \mathrm{Sr},{ }^{87} \mathrm{Sr},{ }^{88} \mathrm{Sr}$.

Nicole Smina
Nicole Smina
Numerade Educator
01:11

Problem 18

Define (a) first ionization energy and (b) second ionization energy.

Lottie Adams
Lottie Adams
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02:56

Problem 19

Complete Chart A for neutral atoms.

Sima Sarker
Sima Sarker
Numerade Educator
01:53

Problem 19

Why is the second ionization energy for a given element always greater than the fi rst ionization energy?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:44

Problem 20

Complete Chart B for neutral atoms.

Sima Sarker
Sima Sarker
Numerade Educator
01:52

Problem 20

What is the usual relationship between atomic radius and first ionization energy, other factors being equal?

Lottie Adams
Lottie Adams
Numerade Educator
01:44

Problem 21

Prior to 1962 , the atomic weight scale was based on the assignment of an atomic weight of exactly 16 amu to the naturally occurring mixture of oxygen. The atomic weight of cobalt is $58.9332$ amu on the carbon-12 scale. What was it on the older scale?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:21

Problem 21

What is the usual relationship between nuclear charge and first ionization energy, other factors being equal?

Lottie Adams
Lottie Adams
Numerade Educator
01:52

Problem 22

Determine the number of protons, neutrons, and electrons in each of the following species: (a) ${ }^{24} \mathrm{Mg}$,
(b) ${ }^{51} \mathrm{~V},(\mathrm{c})^{91} \mathrm{Zr}$
(d) ${ }^{27} \mathrm{Al}$,
(e) ${ }^{65} \mathrm{Zn}^{2+}$
(f) ${ }^{108} \mathrm{Ag}^{+}$.

Nicole Smina
Nicole Smina
Numerade Educator
06:22

Problem 22

Going across a period on the periodic table, what is the relationship between shielding and fi rst ionization energy?

Evelyn Clay
Evelyn Clay
Numerade Educator
01:43

Problem 23

Determine the number of protons, neutrons, and electrons in each of the following species: (a) ${ }^{52} \mathrm{Cr}$,
(b) ${ }^{112} \mathrm{Cd}$,
(c) ${ }^{137} \mathrm{Ba}^{2+}$,
(d) ${ }^{63} \mathrm{Cu}^{+}$
(e) ${ }^{56} \mathrm{Fe}^{2+}$
(f) ${ }^{55} \mathrm{Fe}^{3+}$

Nicole Smina
Nicole Smina
Numerade Educator
07:22

Problem 23

Within a group on the periodic table, what is the relationship between shielding and fi rst ionization energy?

Evelyn Clay
Evelyn Clay
Numerade Educator
04:06

Problem 24

- What is the symbol of the species composed of each of the following sets of subatomic particles?
(a) $24 p, 28 n, 24 e$;
(b) $20 p, 20 n, 20 e$;
(c) $33 p, 42 n, 33 e$;
(d) $53 p, 74 n, 53 e$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:08

Problem 24

Arrange the members of each of the following sets of elements in order of increasing first ionization energies:
(a) the alkali metals; (b) the halogens; (c) the elements in the second period; (d) $\mathrm{Br}, \mathrm{F}, \mathrm{B}, \mathrm{Ga}, \mathrm{Cs}$, and $\mathrm{H}$.

Lottie Adams
Lottie Adams
Numerade Educator
05:23

Problem 25

What is the symbol of the species composed of each of the following sets of subatomic particles? (a) $94 p, 150 n$, $94 e ;$ (b) $79 p, 118 n, 76 e ;$ (c) $34 p, 45 n, 34 e ;$ (d) $56 p, 80 n, 56 e$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:22

Problem 25

The following series of five ionization energies pertains to an element in the second period: $\mathrm{IE}_{1}=1.33 \times 10^{-21} \mathrm{~kJ} /$ atom; $\mathrm{IE}_{2}=4.03 \times 10^{-21} \mathrm{~kJ} /$ atom $; \mathrm{IE}_{3}=6.08 \times 10^{-21} \mathrm{~kJ} /$ atom
$\mathrm{IE}_{4}=4.16 \times 10^{-20} \mathrm{~kJ} /$ atom $; \mathrm{IE}_{5}=5.45 \times 10^{-20} \mathrm{~kJ} /$ atom
Identify the element, and explain why you selected that

Lottie Adams
Lottie Adams
Numerade Educator
02:52

Problem 26

The atomic weight of lithium is $6.941$ amu. The two naturally occurring isotopes of lithium have the following masses: ${ }^{6} \mathrm{Li}, 6.01512$ amu; ${ }^{7} \mathrm{Li}, 7.01600$ amu. Calculate the percent of ${ }^{6} \mathrm{Li}$ in naturally occurring lithium.

Sima Sarker
Sima Sarker
Numerade Educator
02:47

Problem 26

What is the general relationship between the sizes of the atoms of Period 2 and their fi rst ionization energies? Rationalize the relationship.

Evelyn Clay
Evelyn Clay
Numerade Educator
03:00

Problem 27

The atomic weight of rubidium is $85.4678$ amu. The two naturally occurring isotopes of rubidium have the following masses: ${ }^{85} \mathrm{Rb}, 84.9118 \mathrm{amu} ;{ }^{87} \mathrm{Rb}, 86.9092$ amu. Calculate
the percent of ${ }^{85} \mathrm{Rb}$ in naturally occurring rubidium.

Sima Sarker
Sima Sarker
Numerade Educator
02:13

Problem 27

In a plot of first ionization energy versus atomic number for Periods 2 and 3 , "dips" occur at the $3 \mathrm{~A}$ and $6 \mathrm{~A}$ elements. Account for these dips.

Lottie Adams
Lottie Adams
Numerade Educator
03:47

Problem 28

Strontium has four isotopes with the following masses:
$83.9134$ amu $(0.56 \%), 85.9094$ amu $(9.86 \%), 86.9089$ amu
$(7.00 \%)$, and $87.9056(82.58 \%) .$ Calculate the atomic mass of strontium.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:10

Problem 28

On the basis of electron configurations, would you expect a $\mathrm{Li}^{2+}$ ion to exist in compounds? Why or why not? How about $\mathrm{Be}^{2+}$ ?

Lottie Adams
Lottie Adams
Numerade Educator
01:54

Problem 29

What is the atomic weight of a hypothetical element that consists of the following isotopes in the indicated relative abundances?

Sima Sarker
Sima Sarker
Numerade Educator
01:29

Problem 29

How much energy, in kilojoules, must be absorbed by $1.35$ mol of gaseous lithium atoms to convert all of them to gaseous $\mathrm{Li}^{+}$ ions?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:33

Problem 30

Naturally occurring iron consists of four isotopes with the abundances indicated here. From the masses and relative abundances of these isotopes, calculate the atomic weight of naturally occurring iron.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:12

Problem 30

Arrange the following elements in order of increasing negative values of electron affinity: $\mathrm{P}, \mathrm{S}, \mathrm{Cl}$, and $\mathrm{Br}$.

Lottie Adams
Lottie Adams
Numerade Educator
01:47

Problem 31

Calculate the atomic weight of nickel from the following information.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:19

Problem 31

Arrange the members of each of the following sets of elements in order of increasingly negative electron affinities: (a) the Group 1A metals; (b) the Group $4 \mathrm{~A}$ elements; (c) the elements in the second period; (d) Li, K, $\mathrm{C}, \mathrm{F}$, and $\mathrm{Cl}$

Lottie Adams
Lottie Adams
Numerade Educator
04:28

Problem 32

The atomic weight of copper is $63.546$ amu. The two naturally occurring isotopes of copper have the following masses: ${ }^{63} \mathrm{Cu}, 62.9298$ amu; ${ }^{65} \mathrm{Cu}, 64.9278$ amu. Calculate the percent of ${ }^{63} \mathrm{Cu}$ in naturally occurring copper.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:34

Problem 32

The electron affinities of the halogens are much more negative than those of the Group 6 A elements. Why is this so?

Lottie Adams
Lottie Adams
Numerade Educator
05:26

Problem 33

Silver consists of two naturally occurring isotopes: ${ }^{107} \mathrm{Ag}$, which has a mass of $106.90509$ amu, and ${ }^{109} \mathrm{Ag}$, which has a mass of $108.9047$ amu. The atomic weight of silver is $107.8682$ amu. Determine the percent abundance of each isotope in naturally occurring silver.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:14

Problem 33

The addition of a second electron to form an ion with a $2-$ charge is always endothermic. Why is this so?

Lottie Adams
Lottie Adams
Numerade Educator
04:10

Problem 34

Refer to Table $4-3$ only and calculate the atomic weights of oxygen and chlorine. Do your answers agree with the atomic weights given in that table?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:52

Problem 34

Write the equation for the change described by each of the following, and write the electron configuration for each atom or ion shown: (a) the electron affinity of oxygen;
(b) the electron affinity of chlorine; (c) the electron affinity of magnesium.

Lottie Adams
Lottie Adams
Numerade Educator
02:22

Problem 35

The following is a mass spectrum of the $1+$ charged ions of an element. Calculate the atomic weight of the element. What is the element?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:59

Problem 35

Select the smaller member of each pair. (a) $\mathrm{N}$ and $\mathrm{N}^{3-} ;$
(b) $\mathrm{Ba}$ and $\mathrm{Ba}^{2+} ;(\mathrm{c}) \mathrm{Se}$ and $\mathrm{Se}^{2-} ;(\mathrm{d}) \mathrm{Co}^{2+}$ and $\mathrm{Co}^{3+}$

Lottie Adams
Lottie Adams
Numerade Educator
03:59

Problem 36

Suppose you measure the mass spectrum of the $1+$ charged ions of germanium, atomic weight $72.61$ amu. Unfortunately, the recorder on the mass spectrometer jams at the beginning and again at the end of your experiment. You obtain only the following spectrum, which may or may not be complete. From the information given here, can you tell whether one of the germanium isotopes is missing? If one is missing, at which end of the plot should it appear?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:58

Problem 36

Arrange the members of each of the following sets of cations in order of increasing ionic radii: (a) $\mathrm{K}^{+}, \mathrm{Ca}^{2+}$, $\mathrm{Ga}^{3+} ;(\mathrm{b}) \mathrm{Ca}^{2+}, \mathrm{Be}^{2+}, \mathrm{Ba}^{2+}, \mathrm{Mg}^{2+} ;(\mathrm{c}) \mathrm{Al}^{3+}, \mathrm{Sr}^{2+}, \mathrm{Rb}^{+}, \mathrm{K}^{+}$
(d) $\mathrm{K}^{+}, \mathrm{Ca}^{2+}, \mathrm{Rb}^{+}$.

Lottie Adams
Lottie Adams
Numerade Educator
03:36

Problem 37

Calculate the atomic weight of silicon using the following data for the percent natural abundance and mass of each isotope: $92.23 \%^{28} \mathrm{Si}(27.9769 \mathrm{amu}) ; 4.67 \%{ }^{29} \mathrm{Si}$
$(28.9765 \mathrm{amu}) ; 3.10 \%{ }^{30} \mathrm{Si}(29.9738 \mathrm{amu})$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:18

Problem 37

Prepare sketches similar to Figure $4-18$ a that show the radii of $\mathrm{Cl}$ and $\mathrm{Cl}^{-}$. Why is one larger than the other?

Ronald Prasad
Ronald Prasad
Numerade Educator
04:09

Problem 38

Calculate the atomic weight of chromium using the following data for the percent natural abundance and mass of each isotope: $4.35 \%{ }^{50} \mathrm{Cr}(49.9461 \mathrm{amu}) ; 83.79 \%{ }^{52} \mathrm{Cr}$
$(51.9405 \mathrm{amu}) ; 9.50 \%{ }^{53} \mathrm{Cr}(52.9406 \mathrm{amu}) ; 2.36 \%{ }^{54} \mathrm{Cr}$
$(53.9389 \mathrm{amu})$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:02

Problem 38

Arrange the following sets of an?ons 1 n order of increasing ionic radii: (a) $\mathrm{Cl}^{-}, \mathrm{S}^{2-}, \mathrm{P}^{3-} ;$ (b) $\mathrm{O}^{2-}, \mathrm{S}^{2-}, \mathrm{Se}^{2-}$;
(c) $\mathrm{N}^{3-}, \mathrm{S}^{2-}, \mathrm{Br}^{-}, \mathrm{P}^{3-}$
(d) $\mathrm{Cl}^{-}, \mathrm{Br}^{-}, \mathrm{I}^{-}$.

Ronald Prasad
Ronald Prasad
Numerade Educator
00:53

Problem 39

State the periodic law. What does it mean?

Nicole Smina
Nicole Smina
Numerade Educator
01:31

Problem 39

Select the atom or ion in each pair that has the smaller radius. (a) Cs or $\mathrm{Rb} ;$ (b) $\mathrm{O}^{2-}$ or $\mathrm{O} ;$ (c) $\mathrm{Br}$ or $\mathrm{As} ;(\mathrm{d}) \mathrm{Ba}$ or $\mathrm{Ba}^{2+} ;(\mathrm{e}) \mathrm{Cl}^{-}$ or $\mathrm{Ca}^{2+}$

Lottie Adams
Lottie Adams
Numerade Educator
00:55

Problem 40

What was Mendeleev's contribution to the construction of the modern periodic table?

Nicole Smina
Nicole Smina
Numerade Educator
01:09

Problem 40

Most transition metals can form more than one simple positive ion. For example, iron forms both $\mathrm{Fe}^{2+}$ and $\mathrm{Fe}^{3+}$ ions, and tin forms both $\mathrm{Sn}^{2+}$ and $\mathrm{Sn}^{4+}$ ions. Which is the smaller ion of each pair, and why?

Lottie Adams
Lottie Adams
Numerade Educator
03:46

Problem 41

Consult a handbook of chemistry or a suitable website, and look up melting points of the elements of Periods 2 and $3 .$ Show that melting point is a property that varies periodically for these elements.

Ronald Prasad
Ronald Prasad
Numerade Educator
00:59

Problem 41

What is electronegativity?

Ronald Prasad
Ronald Prasad
Numerade Educator
00:40

Problem 42

Mendeleev's periodic table was based on increasing atomic weight. Argon has a higher atomic weight than potassium, yet in the modern table argon appears before potassium. Explain how this can be.

Nicole Smina
Nicole Smina
Numerade Educator
02:11

Problem 42

Arrange the members of each of the following sets of elements in order of increasing electronegativities:
(a) $\mathrm{Pb}, \mathrm{C}$,
$\mathrm{Sn}, \mathrm{Ge} ;(\mathrm{b}) \mathrm{S}, \mathrm{Na}, \mathrm{Mg}, \mathrm{Cl} ;(\mathrm{c}) \mathrm{P}, \mathrm{N}, \mathrm{Sb}, \mathrm{Bi} ;(\mathrm{d}) \mathrm{Se}, \mathrm{Ba}, \mathrm{F}, \mathrm{Si}, \mathrm{Sc} .$

Lottie Adams
Lottie Adams
Numerade Educator
03:17

Problem 43

Estimate the density of antimony from the following densities $\left(\mathrm{g} / \mathrm{cm}^{3}\right): \mathrm{As}, 5.72 ; \mathrm{Bi}, 9.8 ; \mathrm{Sn}, 7.30 ; \mathrm{Te}, 6.24 .$
Show how you arrived at your answer. Using a reference other than your textbook, look up the density of antimony. How does your predicted value compare with the reported value?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:47

Problem 43

Which of the following statements is better? Why?
(a) Magnesium has a weak attraction for electrons in a chemical bond because it has a low electronegativity. (b) The electronegativity of magnesium is low because magnesium has a weak attraction for electrons in a chemical bond.

Lottie Adams
Lottie Adams
Numerade Educator
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Problem 44

Estimate the density of selenium from the following densities $\left(\mathrm{g} / \mathrm{cm}^{3}\right): \mathrm{S}, 2.07 ; \mathrm{Te}, 6.24 ; \mathrm{As}, 5.72 ; \mathrm{Br}, 3.12 .$
Show how you arrived at your answer. Using a reference other than your textbook, look up the density of selenium. How does your predicted value compare with the reported value?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:36

Problem 44

Arrange the elements $\mathrm{Na}, \mathrm{Si}$, and $\mathrm{S}$ in order of
(a) increasing atomic radius; (b) increasing first ionization energy; (c) decreasing electronegativity.

Lottie Adams
Lottie Adams
Numerade Educator
03:14

Problem 45

Estimate the specific heat of antimony from the following specific heats $\left(\mathrm{J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right): \mathrm{As}, 0.34 ; \mathrm{Bi}, 0.14 ; \mathrm{Sn}, 0.23 ; \mathrm{Te}, 0.20 .$
Show how you arrived at your answer.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:37

Problem 45

One element takes on only a negative oxidation number when combined with other elements. From the table of electronegativity values, determine which element this is.

Lottie Adams
Lottie Adams
Numerade Educator
03:55

Problem 46

Given the following melting points in ${ }^{\circ} \mathrm{C}$, estimate the value for $\mathrm{CBr}_{4}: \mathrm{CF}_{4},-184 ; \mathrm{CCl}_{4},-23 ; \mathrm{CI}_{4}, 171$
(decomposes). Using a reference other than your textbook, look up the melting point of $\mathrm{CBr}_{4}$. How does your predicted value compare with the reported value?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
07:44

Problem 46

Assign oxidation states to the element specified in each group of compounds.
(a) $\mathrm{P}$ in $\mathrm{PCl}_{3}, \mathrm{P}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{HPO}_{3}, \mathrm{H}_{3} \mathrm{PO}_{3}$,
$\mathrm{POCl}_{3}, \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}, \mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2} ;(\mathrm{b}) \mathrm{Br}$ in $\mathrm{Br}^{-}, \mathrm{BrO}^{-}, \mathrm{BrO}_{2}^{-}$
$\mathrm{BrO}_{3}^{-}, \mathrm{BrO}_{4}^{-} ;(\mathrm{c}) \mathrm{Mn}$ in $\mathrm{MnO}, \mathrm{MnO}_{2}, \mathrm{Mn}(\mathrm{OH})_{2}, \mathrm{~K}_{2} \mathrm{MnO}_{4}$
$\mathrm{KMnO}_{4}, \mathrm{Mn}_{2} \mathrm{O}_{7} ;(\mathrm{d}) \mathrm{O}$ in $\mathrm{OF}_{2}, \mathrm{Na}_{2} \mathrm{O}, \mathrm{Na}_{2} \mathrm{O}_{2}, \mathrm{KO}_{2}$

Lottie Adams
Lottie Adams
Numerade Educator
00:49

Problem 47

Calcium and magnesium form the following compounds:
$\mathrm{CaCl}_{2}, \mathrm{MgCl}_{2}, \mathrm{CaO}, \mathrm{MgO}, \mathrm{Ca}_{3} \mathrm{~N}_{2}$, and $\mathrm{Mg}_{3} \mathrm{~N}_{2} .$ Predict
the formula for a compound of (a) magnesium and sulfur,
(b) barium and bromine.

Nicole Smina
Nicole Smina
Numerade Educator
03:42

Problem 47

Assign oxidation states to the element specified in each group of compounds. (a) $\mathrm{N}$ in $\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}_{3}, \mathrm{~N}_{2} \mathrm{O}_{4}$
$\mathrm{NH}_{4} \mathrm{Cl}, \mathrm{N}_{2} \mathrm{H}_{4}, \mathrm{NH}_{2} \mathrm{OH}, \mathrm{HNO}_{2}, \mathrm{HNO}_{3} ;$ (b) $\mathrm{C}$ in $\mathrm{CO}$
$\mathrm{CO}_{2}, \mathrm{CH}_{2} \mathrm{O}, \mathrm{CH}_{4} \mathrm{O}, \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{C}_{6} \mathrm{H}_{6} ;(\mathrm{c}) \mathrm{S}$ in $\mathrm{S}^{2-}$,
$\mathrm{SO}_{3}^{2-}, \mathrm{SO}_{4}^{2-}, \mathrm{S}_{2} \mathrm{O}_{3}^{2-}, \mathrm{S}_{4} \mathrm{O}_{6}^{2-}, \mathrm{H}_{2} \mathrm{~S} .$

Lottie Adams
Lottie Adams
Numerade Educator
00:30

Problem 48

The formulas of some hydrides of second-period representative elements are as follows: $\mathrm{BeH}_{2}, \mathrm{BH}_{3}$, $\mathrm{CH}_{4}, \mathrm{NH}_{3}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HF}$. A famous test in criminology
laboratories for the presence of arsenic (As) involves the formation of arsine, the hydride of arsenic. Predict the formula of arsine.

Nicole Smina
Nicole Smina
Numerade Educator
02:20

Problem 48

Assign oxidation states to the element specified in each group of ions. (a) $\mathrm{N}$ in $\mathrm{N}^{3-}, \mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}, \mathrm{N}_{3}^{-}, \mathrm{NH}_{4}^{+}$;
(b) Cl in $\mathrm{Cl}_{2}, \mathrm{HCl}, \mathrm{HClO}, \mathrm{HClO}_{2}, \mathrm{KClO}_{3}, \mathrm{Cl}_{2} \mathrm{O}_{7}$,
$\mathrm{Ca}\left(\mathrm{ClO}_{4}\right), \mathrm{PCl}_{5}$

Lottie Adams
Lottie Adams
Numerade Educator
00:50

Problem 49

Clearly distinguish between the following terms and provide specific examples of each: groups (families) of elements and periods of elements.

Nicole Smina
Nicole Smina
Numerade Educator
02:38

Problem 49

Assign oxidation states to the element specified in each group. (a) $\mathrm{S}$ in $\mathrm{S}_{8}, \mathrm{H}_{2} \mathrm{~S}, \mathrm{SO}_{2}, \mathrm{SO}_{3}, \mathrm{Na}_{2} \mathrm{SO}_{3}, \mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{~K}_{2} \mathrm{SO}_{4}$;
(b) $\mathrm{Cr}$ in $\mathrm{CrO}_{2}^{-}, \mathrm{Cr}(\mathrm{OH})_{4}^{-}, \mathrm{CrO}_{4}^{2-}, \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} ;(\mathrm{c}) \mathrm{B}$ in
$\mathrm{BO}_{2}^{-}, \mathrm{BO}_{3}^{3-}, \mathrm{B}_{4} \mathrm{O}_{7}^{2-}$

Lottie Adams
Lottie Adams
Numerade Educator
01:03

Problem 50

Write names and symbols for (a) the alkaline earth metals,
(b) the Group $4 \mathrm{~A}$ elements,
(c) the Group 2B elements.

Nicole Smina
Nicole Smina
Numerade Educator
02:12

Problem 50

Compare the respective values of the first ionization energy (see Table $5-1)$ and electron affinity (see Table $5-2$ ) for several elements. Which energy is greater? Why?

Lottie Adams
Lottie Adams
Numerade Educator
01:27

Problem 51

Write names and symbols for (a) the alkali metals, (b) the noble gases, (c) the Group 4A elements.

Nicole Smina
Nicole Smina
Numerade Educator
01:54

Problem 51

Compare the respective values of the first ionization energy (see Table $5-1$ ) and electron affinity (see Table $5-2$ ) for nitrogen to those for carbon and oxygen. Explain why the nitrogen values are considerably different.

Lottie Adams
Lottie Adams
Numerade Educator
01:23

Problem 52

Clearly and concisely define the following terms and provide examples of each: (a) metals, (b) nonmetals,
(c) halogens.

Nicole Smina
Nicole Smina
Numerade Educator
01:17

Problem 52

Summarize the physical properties of hydrogen.

Lottie Adams
Lottie Adams
Numerade Educator
02:04

Problem 53

Calculate the wavelengths, in meters, of radiation of the following frequencies: (a) $5.00 \times 10^{15} \mathrm{~s}^{-1}$;
(b) $2.11 \times 10^{14} \mathrm{~s}^{-1}$;
(c) $5.44 \times 10^{12} \mathrm{~s}^{-1}$.

Sima Sarker
Sima Sarker
Numerade Educator
01:43

Problem 53

Write balanced equations for (a) the reaction of iron with steam, (b) the reaction of calcium with hydrochloric acid, (c) the electrolysis of water, and (d) the “water gas” reaction

Lottie Adams
Lottie Adams
Numerade Educator
05:48

Problem 54

Calculate the frequency of radiation of each of the following wavelengths: (a) $8973 \AA$, (b) $442 \mathrm{~nm}$, (c) $4.92 \mathrm{~cm}$,
(d) $4.55 \times 10^{-9} \mathrm{~cm}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
00:48

Problem 54

Write a balanced equation for the preparation of (a) an ionic hydride and (b) a molecular hydride.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:40

Problem 55

What is the energy of a photon of each of the radiations in Exercise 53 ? Express your answer in joules per photon. In which regions of the electromagnetic spectrum do these radiations fall?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
00:36

Problem 55

Classify the following hydrides as molecular or ionic:
(a) $\mathrm{NaH},(\mathrm{b}) \mathrm{H}_{2} \mathrm{~S}$, (c) $\mathrm{AlH}_{3}$,
(d) RbH,
(e) $\mathrm{NH}_{3}$.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:26

Problem 56

Excited lithium ions emit radiation at a wavelength of $670.8 \mathrm{~nm}$ in the visible range of the spectrum. (This characteristic color is often used as a qualitative analysis test for the presence of $\mathrm{Li}^{+} .$ ) Calculate (a) the frequency and (b) the energy of a photon of this radiation. (c) What color is this light?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:45

Problem 56

Explain why NaH and H2S are different kinds of hydrides.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:43

Problem 57

Calculate the energy, in joules per photon, of the red line, $6573 \AA$ A, in the discharge spectrum of atomic calcium.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:12

Problem 57

Write balanced equations for the reactions with water of
(a) $\mathrm{CaH}_{2}$, (b) $\mathrm{AlH}_{3}$, and
(c) $\mathrm{NaH}$.

Lottie Adams
Lottie Adams
Numerade Educator
03:33

Problem 58

Ozone in the upper atmosphere absorbs ultraviolet radiation, which induces the following chemical reaction:
$$
\mathrm{O}_{3}(\mathrm{~g}) \rightarrow \mathrm{O}_{2}(\mathrm{~g})+\mathrm{O}(\mathrm{g})
$$
What is the energy of a $3400-\AA$ photon that is absorbed? What is the energy of a mole of these photons?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:43

Problem 58

Name the following (pure) compounds: (a) $\mathrm{H}_{2} \mathrm{~S}$, (b) $\mathrm{HCl}$,
(c) $\mathrm{KH}$,
(d) $\mathrm{NH}_{3}$,
(e) $\mathrm{H}_{2} \mathrm{Se},(\mathrm{f}) \mathrm{MgH}_{2},(\mathrm{~g}) \mathrm{AlH}_{3} .$

Lottie Adams
Lottie Adams
Numerade Educator
07:07

Problem 59

During photosynthesis, chlorophyll- $\alpha$ absorbs light of wavelength $440 \mathrm{~nm}$ and emits light of wavelength $670 \mathrm{~nm}$. How much energy is available for photosynthesis from the absorption-emission of a mole of photons?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:09

Problem 59

Write a balanced equation for the reaction of an ionic hydride with water. What products are always formed during these reactions?

Lottie Adams
Lottie Adams
Numerade Educator
03:35

Problem 60

Alpha Centauri is the star closest to our solar system. It is 4.3 light-years away. How many miles is this? A light year is the distance that light travels (in a vacuum) in one year. Assume that space is essentially a vacuum.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:35

Problem 60

Briefly compare and contrast the properties of oxygen with those of hydrogen.

Lottie Adams
Lottie Adams
Numerade Educator
04:08

Problem 61

What evidence supports the idea that electromagnetic radiation is (a) wave-like:
(b) particle-like?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:04

Problem 61

Write molecular equations to show how oxygen can be prepared from (a) mercury(II) oxide, $\mathrm{HgO} ;$ (b) hydrogen peroxide, $\mathrm{H}_{2} \mathrm{O}_{2}$; and (c) potassium chlorate, $\mathrm{KClO}_{3}$.

Lottie Adams
Lottie Adams
Numerade Educator
02:42

Problem 62

Describe the influence of frequency and intensity of electromagnetic radiation on the current in the photoelectric effect.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:38

Problem 62

A Which of the following elements form normal oxides as the major products of reactions with oxygen? (a) $\mathrm{Li}$,
(b) $\mathrm{Ba},(\mathrm{c}) \mathrm{Rb},(\mathrm{d}) \mathrm{Mg},(\mathrm{e}) \mathrm{Zn}$ (exhibits only one common
oxidation state), (f) Al.

Lottie Adams
Lottie Adams
Numerade Educator
02:33

Problem 63

Cesium is often used in "electric eyes" for selfopening doors in an application of the photoelectric ef fect. The amount of energy required to ionize (remove an electron from) a cesium atom is $3.89$ electron volts $\left(1 \mathrm{eV}=1.60 \times 10^{-19} \mathrm{~J}\right)$. Show by calculation whether a beam of yellow light with wavelength 5830 Å would ionize a cesium atom.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:22

Problem 63

Oxygen has a positive oxidation number when combined with which element? Compare the electronegativity values of oxygen and that element.

Lottie Adams
Lottie Adams
Numerade Educator
03:58

Problem 64

Refer to Exercise 63 . What would be the wavelength, in nanometers, of light with just sufficient energy to ionize a cesium atom? What color would this light be?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:13

Problem 64

Write balanced equations for the reactions of the following elements with a limited amount of oxygen: (a) C,
(b) $\mathrm{As}_{4},(\mathrm{c})$ Ge.

Lottie Adams
Lottie Adams
Numerade Educator
04:13

Problem 65

(a) Distinguish between an atomic emission spectrum and an atomic absorption spectrum. (b) Distinguish between a continuous spectrum and a line spectrum.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:14

Problem 65

Write balanced equations for the reactions of the following elements with an excess of oxygen: (a) $\mathrm{C},(\mathrm{b}) \mathrm{As}_{4},(\mathrm{c})$ Ge.

Lottie Adams
Lottie Adams
Numerade Educator
02:10

Problem 66

Prepare a sketch similar to Figure $4-18 b$ that shows a ground energy state and three excited energy states. Using vertical arrows, indicate the transitions that would correspond to the absorption spectrum for this system.

Crystal Wang
Crystal Wang
Numerade Educator
01:24

Problem 66

Distinguish among normal oxides, peroxides, and superoxides. What is the oxidation state of oxygen in each case?

Lottie Adams
Lottie Adams
Numerade Educator
00:53

Problem 67

Why is the Bohr model of the hydrogen atom referred to as the solar system model?

Nicole Smina
Nicole Smina
Numerade Educator
02:44

Problem 67

Which of the following can be classified as basic anhydrides?
(a) $\mathrm{CO}_{2},(\mathrm{~b}) \mathrm{Li}_{2} \mathrm{O},(\mathrm{c}) \mathrm{SeO}_{3},(\mathrm{~d}) \mathrm{CaO}$
(e) $\mathrm{N}_{2} \mathrm{O}_{5}$

Lottie Adams
Lottie Adams
Numerade Educator
03:48

Problem 68

If each atom in one mole of atoms emits a photon of wavelength $5.50 \times 10^{3} \AA$, how much energy is lost? Express the answer in $\mathrm{kJ} / \mathrm{mol}$. As a reference point, burning one mole $\left(16 \mathrm{~g}\right.$ ) of $\mathrm{CH}_{4}$ produces $819 \mathrm{~kJ}$ of heat.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:03

Problem 68

Write balanced equations for the following reactions and name the products: (a) carbon dioxide, $\mathrm{CO}_{2}$, with water;
(b) sulfur trioxide, $\mathrm{SO}_{3}$, with water; (c) selenium trioxide, $\mathrm{SeO}_{3}$, with water; (d) dinitrogen pentoxide, $\mathrm{N}_{2} \mathrm{O}_{5}$, with water; and (e) dichlorine heptoxide, $\mathrm{Cl}_{2} \mathrm{O}_{7}$, with water

Lottie Adams
Lottie Adams
Numerade Educator
03:18

Problem 69

What is the Balmer-Rydberg equation? Why is it called an empirical equation?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:33

Problem 69

Write balanced equations for the following reactions and name the products: (a) sodium oxide, $\mathrm{Na}_{2} \mathrm{O}$, with water;
(b) calcium oxide, $\mathrm{CaO}$, with water; (c) lithium oxide, $\mathrm{Li}_{2} \mathrm{O}$, with water; (d) magnesium oxide, $\mathrm{MgO}$, with sulfur dioxide. $\mathrm{SO}_{2} ;$ and (e) calcium oxide, $\mathrm{CaO}$, with carbon dioxide, $\mathrm{CO}_{2}$.

Lottie Adams
Lottie Adams
Numerade Educator
04:21

Problem 70

Hydrogen atoms absorb energy so that the electrons are excited to the energy level $n=7 .$ Electrons then undergo these transitions: (1) $n=7 \rightarrow n=1 ;$ (2) $n=7 \rightarrow n=2$;
(3) $n=2 \rightarrow n=1$. Which of these transitions will produce the photon with (a) the smallest energy; (b) the highest frequency; (c) the shortest wavelength? (d) What is the frequency of a photon resulting from the transition $n=6 \rightarrow n=1 ?$

Crystal Wang
Crystal Wang
Numerade Educator
01:07

Problem 70

Identify the acid anhydrides of the following ternary acids:
(a) $\mathrm{H}_{2} \mathrm{SO}_{4}$
(b) $\mathrm{H}_{2} \mathrm{CO}_{3}$
(c) $\mathrm{H}_{2} \mathrm{SO}_{3}$
(d) $\mathrm{H}_{3} \mathrm{PO}_{4}$
(e) $\mathrm{HNO}_{2}$.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:53

Problem 71

Five energy levels of the He atom are given in joules per atom above an arbitrary reference energy:
(1) $6.000 \times 10^{-19} ;(2) 8.812 \times 10^{-19}$
(3) $9.381 \times 10^{-19}$;
(4) $10.443 \times 10^{-19} ;$ (5) $10.934 \times 10^{-19}$. Construct an energy level diagram for He, and find the energy of the photon (a) absorbed for the electron transition from level 1 to level 5 and (b) emitted for the electron transition from level 4 to level 1 .

Ronald Prasad
Ronald Prasad
Numerade Educator
01:20

Problem 71

Identify the basic anhydrides of the following metal hydroxides: (a) $\mathrm{NaOH},(\mathrm{b}) \mathrm{Mg}(\mathrm{OH})_{2},(\mathrm{c}) \mathrm{Fe}(\mathrm{OH})_{2}$,
(d) $\mathrm{Al}(\mathrm{OH})_{3}$.

Lottie Adams
Lottie Adams
Numerade Educator
04:26

Problem 72

The following are prominent lines in the visible region of the emission spectra of the elements listed. The lines can be used to identify the elements. What color is the light responsible for each line? (a) lithium, $4603 \AA$;;
(b) neon, $540.0 \mathrm{~nm}$; (c) calcium, $6573 \mathrm{~A}$;
(d) potassium, $\nu=3.90 \times 10^{14} \mathrm{~Hz}$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:20

Problem 72

Define combustion. Write a balanced equation for the combustion of diatomic hydrogen.

Lottie Adams
Lottie Adams
Numerade Educator
01:41

Problem 73

Hydrogen atoms have an absorption line at $1026 \AA$. What is the frequency of the photons absorbed, and what is the energy difference, in joules, between the ground state and this excited state of the atom?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:34

Problem 73

Write equations for the complete combustion of the following compounds: (a) methane, $\mathrm{CH}_{4}(\mathrm{~g}) ;$ (b) propane, $\mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{~g}) ;$ (c) ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\ell)$.

Lottie Adams
Lottie Adams
Numerade Educator
02:18

Problem 74

An argon laser emits blue light with a wavelength of $488.0 \mathrm{~nm}$. How many photons are emitted by this laser in $2.00$ seconds, operating at a power of 515 milliwatts? One watt (a unit of power) is equal to 1 joule/second.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:31

Problem 74

Write equations for the incomplete combustion of the following compounds to produce carbon monoxide: (a) methane, $\mathrm{CH}_{4}(\mathrm{~g}) ;$ (b) propane, $\mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{~g})$. As we have seen, two substances may react to form different products when they are mixed in different proportions under different conditions.

Lottie Adams
Lottie Adams
Numerade Educator
01:18

Problem 75

(a) What evidence supports the idea that electrons are particle-like? (b) What evidence supports the idea that electrons are wave-like?

Nicole Smina
Nicole Smina
Numerade Educator
02:36

Problem 75

In Exercises 75 and 76, draw molecular representations of the materials before and after reaction as described in the quantitative descriptions.
Ethane, $\mathrm{C}_{2} \mathrm{H}_{6}$, burns in excess oxygen to form carbon dioxide and water. To illustrate this reaction, two molecules of ethane will react in the presence of nine molecules of oxygen, $\mathrm{O}_{2}$, to yield four molecules of carbon dioxide, six molecules of water, and two molecules of excess oxygen left unreacted.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:20

Problem 76

(a) What is the de Broglie wavelength of a proton moving at a speed of $2.50 \times 10^{7} \mathrm{~m} / \mathrm{s}$ ? The proton mass is $1.67 \times 10^{-24} \mathrm{~g} .$ (b) What is the de Broglie wavelength of a stone with a mass of $30.0 \mathrm{~g}$ moving at $2.00 \times 10^{5} \mathrm{~m} / \mathrm{h}$ $(\approx 100 \mathrm{mph}) ?(\mathrm{c})$ How do the wavelengths in parts
(a) and (b) compare with the typical radii of atoms? (See the atomic radii in Figure $5-1 .$ )

Ronald Prasad
Ronald Prasad
Numerade Educator
02:09

Problem 76

Draw molecular representations of the materials before and after reaction as described in the quantitative descriptions.
Propane, $\mathrm{C}_{3} \mathrm{H}_{8}$, burns in excess oxygen to form carbon dioxide and water. To illustrate this reaction, a molecule of propane reacts in the presence of seven molecules of oxygen, $\mathrm{O}_{2}$, to yield three molecules of carbon dioxide, four molecules of water, and two molecules of excess oxygen left unreacted.

Crystal Wang
Crystal Wang
Numerade Educator
01:01

Problem 77

What is the wavelength corresponding to a neutron of mass $1.67 \times 10^{-27} \mathrm{~kg}$ moving at $2360 \mathrm{~m} / \mathrm{s}$ ?

Nicole Smina
Nicole Smina
Numerade Educator
04:01

Problem 77

(a) How much $\mathrm{SO}_{2}$ would be formed by burning $1.00 \mathrm{~kg}$ of bituminous coal that is $5.15 \%$ sulfur by mass? Assume that all of the sulfur is converted to $\mathrm{SO}_{2}$. (b) If $18.0 \%$ of the $\mathrm{SO}_{2}$ escaped into the atmosphere and $75.0 \%$ of the escaped $\mathrm{SO}_{2}$ were converted to $\mathrm{H}_{2} \mathrm{SO}_{4}$, how many grams of $\mathrm{H}_{2} \mathrm{SO}_{4}$ would be produced in the atmosphere?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:16

Problem 78

What is the velocity of an $\alpha$ -particle (a helium nucleus) that has a de Broglie wavelength of $0.529$ Å?

Nicole Smina
Nicole Smina
Numerade Educator
01:54

Problem 78

Write equations for the complete combustion of the following compounds. Assume that sulfur is converted to $\mathrm{SO}_{2}$ and nitrogen is converted to NO. (a) $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}(\ell)$,
(b) $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{SH}(\ell)$,
(c) $\mathrm{C}_{7} \mathrm{H}_{10} \mathrm{NO}_{2} \mathrm{~S}(\ell)$.

Ronald Prasad
Ronald Prasad
Numerade Educator
00:55

Problem 79

(a) What is a quantum number? What is an atomic orbital?
(b) How many quantum numbers are required to specify a single atomic orbital? What are they?

Nicole Smina
Nicole Smina
Numerade Educator
01:51

Problem 79

Write the electron configuration for the product of the second ionization of the third largest alkaline earth metal.

Lottie Adams
Lottie Adams
Numerade Educator
00:31

Problem 80

How are the possible values for the angular momentum quantum number for a given electron restricted by the value of $n$ ?

Nicole Smina
Nicole Smina
Numerade Educator
02:07

Problem 80

You are given the atomic radii of $110 \mathrm{pm}, 118 \mathrm{pm}, 120 \mathrm{pm}$, $122 \mathrm{pm}$, and $135 \mathrm{pm}$, but do not know to which element (As, Ga, Ge, P, and Si) these values correspond. Which must be the value of Ge?

Lottie Adams
Lottie Adams
Numerade Educator
03:39

Problem 81

Without giving the ranges of possible values of the four quantum numbers, $n, \ell, m_{l}$, and $m_{s}$, describe briefly what information each one gives.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:34

Problem 81

Which is larger, $\mathrm{Na}^{+}$ or $\mathrm{F}^{-} ?$ For each of these ions, draw a representation of the shape of the highest energy occupied orbital.

Lottie Adams
Lottie Adams
Numerade Educator
01:40

Problem 82

Draw an orbital that has the following quantum numbers:
$n=3, \ell=1, m_{\ell}=-1$, and $m_{s}=-\frac{1}{2} .$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:52

Problem 82

Write the electron configurations of beryllium and magnesium. What similarities in their chemical properties can you predict on the basis of their electron configurations? Compare the sizes of their most stable ions.

Lottie Adams
Lottie Adams
Numerade Educator
04:15

Problem 83

What is the maximum number of electrons in an atom that can have the following quantum numbers? (a) $n=2$;
(b) $n=3$ and $\ell=1 ;$ (c) $n=3, \ell=1$, and $m_{\ell}=0$;
(d) $n=3, \ell=1, m_{\ell}=-1$, and $m_{s}=-\frac{1}{2}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:15

Problem 83

Dolostone is often more porous than limestone. One explanation of the origin of dolostone is that it results from partial replacement of calcium by magnesium in an original limestone sediment. Is this explanation reasonable, given what vou know of the ionic radii of magnesium and calcium ions?

Ronald Prasad
Ronald Prasad
Numerade Educator
04:30

Problem 84

What is the maximum number of electrons in an atom that can have the following quantum numbers? (a) $n=3$ and $\ell=1 ;$ (b) $n=3$ and $\ell=2 ;$ (c) $n=3, \ell=0$ and $m_{\ell}=-1$;
(d) $n=3, \ell=1$, and $m_{\ell}=-1 ;$ (e) $n=3, \ell=1, m_{\ell}=0$,
and $m_{s}=-\frac{1}{2}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:35

Problem 84

On an outline of the periodic table like the one below, label the areas in which the "last" electron assigned in the electron configuration is in a filled orbital of each of the following types: $1 s, 2 s, 2 p, 3 s, 3 p, 3 d, 4 s, 4 p, 4 d, 4 f, 5 s, 5 p, 5 d$,
$5 f, 6 s, 6 p, 6 d, 7 s$, and $7 p$.

Lottie Adams
Lottie Adams
Numerade Educator
01:06

Problem 85

What are the values of $n$ and $\ell$ for the following subshells?
(a) $1 s ;(\mathrm{b}) 4 s ;$ (c) $3 p ;(\mathrm{d}) 4 d ;(\mathrm{e}) 4 f$.

Sima Sarker
Sima Sarker
Numerade Educator
01:29

Problem 85

Generally, elements with very negative electron affinities gain electrons easily to form negative ions. Which group of elements tends to form anions most easily?

Lottie Adams
Lottie Adams
Numerade Educator
03:41

Problem 86

(a) How many sublevels are in the third main energy level? (b) Which, if any, of these sublevels contain a set of equivalent orbitals? (c) Sketch, on the same relative scale, at least one orbital from each of these sublevels.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:13

Problem 86

Identify all the elements that have an electronegativity of $3.0$ or greater. Where are they located on the periodic table? Identify all the elements that have an electronegativity of $1.0$ or less. Except for $\mathrm{Yb}$, where are they located on the periodic table?

Lottie Adams
Lottie Adams
Numerade Educator
03:29

Problem 87

(a) How many sublevels are in the second main energy level? (b) Which, if any, of these sublevels contain a set of equivalent orbitals? (c) Sketch, on the same relative scale, at least one orbital from each of these sublevels.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:41

Problem 87

Figure 5-9 includes the formulas of the normal oxides of the representative elements in their maximum oxidation states. Use these formulas to determine the oxidation state of each element, assuming an oxidation state of $-2$ for oxygen. What is the oxidation state of every element in Groups $1 \mathrm{~A}$, $2 \mathrm{~A}, 3 \mathrm{~A}, 4 \mathrm{~A}, 5 \mathrm{~A}$, and $6 \mathrm{~A}$ ? What is the oxidation state of most elements in Group 7A? Which element is the exception?

Lottie Adams
Lottie Adams
Numerade Educator
03:54

Problem 88

How many individual orbitals are there in the third shell? Write out $n, \ell$, and $m_{\ell}$ quantum numbers for each one, and label each set by the $s, p, d, f$ designations.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:17

Problem 88

Hydrogen can be obtained from water by electrolysis. Hydrogen may someday be an important replacement for current fuels. Describe some of the problems that you would predict if hydrogen were used in today's motor vehicles.

Lottie Adams
Lottie Adams
Numerade Educator
02:34

Problem 89

(a) Write the possible values of $\ell$ when $n=3 .$ (b) Write the allowed number of orbitals (1) with the quantum numbers $n=4, \ell=1 ;$ (2) with the quantum numbers $n=4, \ell=2$;
(3) with the quantum numbers $n=3, \ell=0, m_{l}=0$;
(4) with the quantum numbers $n=1$.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:23

Problem 89

The only chemically stable ion of rubidium is $\mathrm{Rb}^{+}$. The most stable monoatomic ion of bromine is $\mathrm{Br}^{-}$. Krypton $(\mathrm{Kr})$ is among the least reactive of all elements. Compare the electron configurations of $\mathrm{Rb}^{+}, \mathrm{Br}^{-}$, and $\mathrm{Kr}$. Then predict the most stable monatomic ions of strontium (Sr) and selenium (Se).

Lottie Adams
Lottie Adams
Numerade Educator
03:27

Problem 90

What are the possible values for $m_{\ell}$ for (a) the $p$ sublevel? (b) the $f$ sublevel? (c) all sublevels where $n=3$ ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:19

Problem 90

The first ionization energy of potassium, $\mathrm{K}$, is $419 \mathrm{~kJ} / \mathrm{mol}$. What is the minimum frequency of light required to ionize gaseous potassium atoms?

Lottie Adams
Lottie Adams
Numerade Educator
03:07

Problem 91

Write a complete set of quantum numbers $\left(n, \ell\right.$, and $\left.m_{t}\right)$ for each of the following orbitals: (a) $5 f$, (b) $4 d$, and (c) 2 s.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:20

Problem 91

Potassium and argon would be anomalies in a periodic table in which elements are arranged in order of increasing atomic weights. Identify two other elements among the transition elements whose positions in the periodic table would have been reversed in a "weight-sequence" arrangement. Which pair of elements would most obviously be out of place on the basis of their chemical behavior? Explain your answer in terms of the current atomic model, houring electron confiourations for these elemen

Ronald Prasad
Ronald Prasad
Numerade Educator
02:19

Problem 92

How many orbitals correspond to each of the following designations? (a) $3 p,(\mathrm{~b}) 4 p,(\mathrm{c}) 4 p_{x},(\mathrm{~d}) 6 d,(\mathrm{e}) 5 d,(\mathrm{f}) 5 f$,
(g) $n=5$, (h) $7 s$

Katherine Mccandless
Katherine Mccandless
Numerade Educator
01:56

Problem 92

The second ionization energy for magnesium is $1451 \mathrm{~kJ} / \mathrm{mol}$. How much energy, in kilojoules, must be absorbed by $1.75 \mathrm{~g}$ of gaseous magnesium atoms to convert them to gaseous $\mathrm{Mg}^{2+}$ ions?

Lottie Adams
Lottie Adams
Numerade Educator
02:47

Problem 93

The following incorrect sets of quantum numbers in the order $n, \ell, m_{\ell}, m_{s}$ are written for paired electrons or for one electron in an orbital. Correct them, assuming the $n$ values are correct. (a) $1,0,0,+\frac{1}{2},+\frac{1}{2} ;$ (b) $2,2,1, \frac{1}{2} ;$ (c) $3,2,3, \pm \frac{1}{2}$;
(d) $3,1,2,+\frac{1}{2} ;$ (e) $2,1,-1,0 ;$ (f) $3,-0,-1,-\frac{1}{2}$.

Nicole Mabante
Nicole Mabante
Numerade Educator
02:12

Problem 93

The chemical reactivities of carbon and lead are similar, but there are also major differences. Using their electron configurations, explain why these similarities and differences may exist.

Lottie Adams
Lottie Adams
Numerade Educator
04:11

Problem 94

(a) How are a $1 s$ orbital and a $2 s$ orbital in an atom similar? How do they differ? (b) How are a $3 p_{x}$ orbital and a $2 p_{y}$ orbital in an atom similar? How do they differ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:05

Problem 94

Go to physchem.ox.ac.uk/MSDS/ or another site on the web and locate "MSDS Data Sheets." Find the MSDS for sodium nitrate. (a) What does LDLo stand for? (b) What does mus stand for?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:03

Problem 95

Draw representations of ground state electron configurations using the orbital notation $(\uparrow \downarrow)$ for the following elements. (a) $\mathrm{N},(\mathrm{b}) \mathrm{V}$, (c) $\mathrm{Cl},(\mathrm{d}) \mathrm{Rh}$.

Sima Sarker
Sima Sarker
Numerade Educator
02:06

Problem 95

While at the MSDS sheet for sodium nitrate required for Exercise 94 , answer the following: (a) What does the Risk Phrase "R8" indicate? (b) What does the Safety Phrase "S39" indicate?

Crystal Wang
Crystal Wang
Numerade Educator
08:03

Problem 96

Draw representations of ground state electron configurations using the orbital notation $(\uparrow \downarrow)$ for the following elements. (a) $\mathrm{P},(\mathrm{b}) \mathrm{Ni},(\mathrm{c}) \mathrm{Ga},(\mathrm{d}) \mathrm{Cd}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:13

Problem 96

Go to physics.nist.gov/PhysRefData/IonEnergy/ periodic-table.pdf or another site on the web and locate values given for the first ionization energies for $\mathrm{Al}$ and $\mathrm{P}$. Are the values different than those given in Table $5-1 ?$ Explain.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:36

Problem 97

Determine the number of electrons in the outer occupied shell of each of the following elements, and indicate the principal quantum number of that shell. (a) $\mathrm{Na}$, (b) Al,
(c) Ca,
(d) $\mathrm{Sr},(\mathrm{e}) \mathrm{Ba},(\mathrm{f}) \underline{\mathrm{Br}}$.

Sima Sarker
Sima Sarker
Numerade Educator
01:10

Problem 97

Use the Handbook of Cbemistry and Pbysics or a suitable website to find the Crystal Ionic Radii of the Elements. Plot atomic number versus radius of the $2+$ ions of the first $d$ -transition series. Is there a trend? Is a minimum size formed during the transition from $\mathrm{Sc}^{2+}$ to $\mathrm{Zn}^{2+} ?$ Do the values for the second and third $d$ -transition series appear to form a similar minimum at about the same group number?

Manik Pulyani
Manik Pulyani
Numerade Educator
01:11

Problem 98

Explain why each of the following ground state configurations is incorrect, and correct it.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:24

Problem 99

Explain why each of the following ground state configurations is incorrect, and correct it.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:16

Problem 100

A neutral atom has two electrons with $n=1$, eight electrons with $n=2$, eight electrons with $n=3$, and two electrons with $n=4$. Assume this element is in its ground state configuration.
(a) What are the atomic number, symbol, and name of this element?
(b) In which period of the periodic table does this element appear?
(c) In which group of the periodic table does this element appear?
(d) What is the total number of $s$ electrons in this atom?
(e) What is the total number of $p$ electrons in this atom?
(f) What is the total number of $d$ electrons in this atom?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:18

Problem 101

A neutral atom has two electrons with $n=1$, eight electrons with $n=2$, sixteen electrons with $n=3$, and two electrons with $n=4$. Assume this element is in its ground state configuration.
(a) What are the atomic number, symbol, and name of this element?
(b) In which period of the periodic table does this element appear?
(c) In which group of the periodic table does this element appear?
(d) What is the total number of $s$ electrons in this atom?
(e) What is the total number of $p$ electrons in this atom?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:40

Problem 102

With the help of Appendix B, list the symbols for the first five elements, by atomic number, that have an unpaired electron in an $s$ orbital. Identify the group in which most of these are found in the periodic table.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:58

Problem 103

List the elements having an atomic number of 20 or less that have one or more unpaired $p$ orbital electrons. Indicate the group to which each of these elements belongs in the periodic table.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:16

Problem 104

Identify the element or elements possible, given only the number of electrons in the outermost shell and the principal quantum number of that shell. (a) 1 electron, first shell; (b) 3 electrons, second shell; (c) 3 electrons, third shell; (d) 2 electrons, seventh shell; (e) 4 electrons, third shell; (f) 8 electrons, fifth shell.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:19

Problem 105

Give the ground state electron configurations for the elements of Exercise 95 using shorthand notation-that is, $1 s^{2} 2 s^{2} 2 p^{6}$, and so on.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:36

Problem 106

Give the ground state electron configurations for the elements of Exercise 96 using shorthand notation-that is, $1 s^{2} 2 s^{2} 2 p^{6}$, and so on.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:11

Problem 107

State the Pauli Exclusion Principle. Would any of the following electron configurations violate this rule: (a) $1 s^{3}$;
(b) $1 s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{3}$;
(c) $1 s^{2} 2 s^{2} 2 p_{x}^{2}$;
(d) $1 s^{2} 2 s^{2} 3 s^{2} ?$ Explain.

Nicole Mabante
Nicole Mabante
Numerade Educator
02:19

Problem 108

State Hund's Rule. Would any of the following electron configurations violate this rule: (a) $1 s^{2}$; (b) $1 s^{2} 2 s^{2} 2 p_{x}^{2}$;
(c) $1 s^{2} 2 s^{2} 2 p_{x}^{1} 2 p_{y}^{1}$;
(d) $1 s^{2} 2 s^{1} 2 p_{x}^{1} 2 p_{z}^{1}$;
(e) $1 s^{2} 2 s^{1} 2 p_{x}^{2} 2 p_{y}^{1} 2 p_{z}^{1}$ ?
Explain.

Nicole Mabante
Nicole Mabante
Numerade Educator
01:24

Problem 109

Classify each of the following atomic electron configurations as (i) a ground state, (ii) an excited state, or
(iii) a forbidden state: (a) $1 s^{2} 2 s^{2} 2 p^{5} 3 s^{1}$;
(b) $[\mathrm{Kr}] 4 d^{10} 5 s^{3}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{12} 4 s^{2}$;
(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 2 d^{1}$;
(e) $1 s^{2} 2 s^{2} 2 p^{8} 3 s^{2} 3 p^{5}$.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:40

Problem 110

Which of the elements with atomic numbers of 11 or less are paramagnetic when in the atomic state?

Sima Sarker
Sima Sarker
Numerade Educator
04:26

Problem 111

Semiconductor industries depend on such elements as $\mathrm{Si}$, Ga, As, Ge, B, Cd, and S. Write the predicted electron configuration of each element.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:33

Problem 112

The manufacture of high-temperature ceramic superconductors depends on such elements as $\mathrm{Cu}$, O, La, Y, Ba, Tl, and Bi. Write the predicted electron configuration of each element. (Consult Appendix $\mathrm{B}$ if necessary.)

Nicole Mabante
Nicole Mabante
Numerade Educator
03:36

Problem 113

In nature, potassium and sodium are often found together. (a) Write the electron configurations for potassium and for sodium. (b) How are they similar?
(c) How do they differ?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:04

Problem 114

Which elements are represented by the following electron configurations?
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{5}$
(b) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{4}$
(c) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 5 f^{14} 6 s^{2} 6 p^{6} 7 s^{2}$
(d) $[\mathrm{Kr}] 4 d^{5} 5 s^{2}$
(e) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{2} 4 s^{2}$

Sima Sarker
Sima Sarker
Numerade Educator
00:50

Problem 115

Repeat Exercise 114 for
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{2} 4 s^{2}$
(b) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{4}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}$
(d) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{6} 7 s^{2}$

Ronald Prasad
Ronald Prasad
Numerade Educator
03:15

Problem 116

Find the total number of $s, p$, and $d$ electrons in each of the following: (a) $\mathrm{P}$; (b) $\mathrm{Kr}$; (c) $\mathrm{Ni}$; (d) $\mathrm{Zn} ;$ (e) Ti.

Ronald Prasad
Ronald Prasad
Numerade Educator
03:18

Problem 117

Write the electron configurations of the Group $2 \mathrm{~A}$ elements Be, Mg, and Ca (see inside front cover). What similarities do you observe?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:38

Problem 118

Construct a table in which you list a possible set of values for the four quantum numbers for each electron in the following atoms in their ground states. (a) $\mathrm{K} ;$ (b) $\mathrm{O} ;$ (c) $\mathrm{Ca}$.

Nicole Mabante
Nicole Mabante
Numerade Educator
02:11

Problem 119

Construct a table in which you list a possible set of values for the four quantum numbers for each electron in the following atoms in their ground states. (a) $\mathrm{Sr} ;$ (b) $\mathrm{S} ;$ (c) Sc.

Nicole Mabante
Nicole Mabante
Numerade Educator
02:10

Problem 120

Draw general electron structures for the A group elements using the $\uparrow \downarrow$ notation, where $n$ is the principal quantum number for the highest occupied energy level.

Ronald Prasad
Ronald Prasad
Numerade Educator
01:19

Problem 121

Repeat Exercise 120 using $n s^{x} n p^{y}$ notation.

Ronald Prasad
Ronald Prasad
Numerade Educator
View

Problem 122

List $n, \ell$, and $m_{\ell}$ quantum numbers for the highest energy electron (or one of the highest energy electrons if there are more than one) in the following atoms in their ground states. (a) $\mathrm{Si} ;(\mathrm{b}) \mathrm{Ac} ;$ (c) $\mathrm{Cl} ;$ (d) $\mathrm{Pr}$.

Susan Hallstrom
Susan Hallstrom
Numerade Educator
04:03

Problem 123

List $n, \ell$, and $m_{\ell}$ quantum numbers for the highest energy electron (or one of the highest energy electrons if there are more than one) in the following atoms in their ground states. (a) Se; (b) $\mathrm{Zn} ;$ (c) $\mathrm{Mg}$; (d) $\mathrm{Pu}$.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:55

Problem 124

Write the ground state electron configurations for elements $\mathrm{A}-\mathrm{E}$.

Ronald Prasad
Ronald Prasad
Numerade Educator
02:49

Problem 125

Repeat Exercise 124 for elements F-J.

Ronald Prasad
Ronald Prasad
Numerade Educator
06:35

Problem 126

How many unpaired electrons are in atoms of Na, Ne, Al, Be, Br, As, and Ti?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:37

Problem 127

(a) Distinguish between the terms "diamagnetic" and "paramagnetic," and provide an example that illustrates the meaning of each. (b) How is paramagnetism measured experimentally?

Ronald Prasad
Ronald Prasad
Numerade Educator
02:20

Problem 128

Which of the following ions or atoms possess paramagnetic properties? (a) $\mathrm{F},(\mathrm{b}) \mathrm{Kr},(\mathrm{c}) \mathrm{Ne}^{+}$
(d) Fe, (e) Cl-

Sima Sarker
Sima Sarker
Numerade Educator
03:18

Problem 129

Which of the following ions or atoms possess paramagnetic properties? (a) $\mathrm{Na}^{+}$, (b) $\mathrm{Ca}^{21+},(\mathrm{c}) \mathrm{Ca}$,
(d) $\mathrm{Ar}^{-},(\mathrm{e}) \mathrm{S} \mathrm{i}$.

Ronald Prasad
Ronald Prasad
Numerade Educator
00:58

Problem 130

The atomic mass of chlorine is reported to be $35.5$, yet no atom of chlorine has the mass of $35.5$ amu. Explain.

Nicole Smina
Nicole Smina
Numerade Educator
00:59

Problem 131

Chemists often use the terms "atomic weight" and "atomic mass" interchangeably. Explain why it would be more accurate if, in place of either of these terms, we used the phrase "average atomic mass."

Nicole Smina
Nicole Smina
Numerade Educator
02:43

Problem 132

The diameter of an atom is about 100,000 times larger than the diameter of the nucleus of the atom. Suppose an atom is enlarged until its nucleus is the size of a basketball, which has a diameter of $9.39$ inches. What would be the diameter of this enlarged atom?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:41

Problem 133

Using the electron configurations of the elements, given in Appendix B, and Hund's Rule, determine which elements have a pair of electrons in every occupied orbital (no singles). Are they about half of the elements, rather small in number, or rather large in number? To what groups of elements do they belong?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:25

Problem 134

Draw a three-dimensional representation of each of the following orbitals: (a) $3 p_{x}$, (b) $2 s$, (c) $3 d_{x y}$, (d) $3 d_{z^{2}}$.

Ian Lee
Ian Lee
Numerade Educator
04:40

Problem 135

We often show the shapes of orbitals as drawings. What are some of the limitations of these drawings?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:56

Problem 136

An atom in its ground state contains 18 electrons. How many of these electrons are in orbitals with $\ell=0$ values?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:27

Problem 137

Suppose that scientists were to discover a new element, one that has the chemical properties of the noble gases,and positioned directly below radon on the periodic table. Assuming that the $g$ orbitals of the elements preceding it in the period had not yet begun to fill, what would be the atomic number and ground state electron configuration of this new element?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
00:50

Problem 138

For a lithium atom, give (a) its ground state electron configuration; (b) the electron configuration for one of its lowest energy excited states; and (c) an electron configuration for a forbidden or impossible state.

Nicole Smina
Nicole Smina
Numerade Educator
01:16

Problem 139

Suppose we could excite all of the electrons in a sample of hydrogen atoms to the $n=6$ level. They would then emit light as they relaxed to lower energy states. Some atoms might undergo the transition $n=6$ to $n=1$, and others might go from $n=6$ to $n=5$, then from $n=5$ to $n=4$, and so on. How many lines would we expect to observe in the resulting emission spectrum?

Ronald Prasad
Ronald Prasad
Numerade Educator
04:25

Problem 140

Examine each of the following statements. What is incorrect about each statement? How can each statement be changed to make it a correct statement?
(a) A hydrogen atom has one energy level.
(b) A lithium atom has three electrons, two in the 1 s sublevel and one in the $2 p$ sublevel.
(c) The angular momentum quantum number, $\ell$, of an electron in a $p$ sublevel has a value of 2 .
(d) Three electrons in a $p$ sublevel will occupy separate orbitals, so one will be positive $(+1)$, one will be neutral
(0), and one will be negative $(-1)$.
(e) Two electrons in the same orbital must have the same spin.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:55

Problem 141

Antimatter is composed of antiparticles in the same way that normal matter is composed of particles. For every subatomic particle there exists an antiparticle with the same mass but opposite charge. The antielectron (or positron) has a positive charge, and the antiproton has a negative charge. In 1995 the European Organization for Nuclear Research (commonly known as CERN) announced that it had successfully created nine antihydrogen atoms using these antiparticles. Describe the composition of an antihydrogen atom. What's in the nucleus and what's outside the nucleus?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
04:56

Problem 142

Two isotopes of hydrogen occur naturally $\left({ }^{1} \mathrm{H},>99 \%,\right.$, and $\left.{ }^{2} \mathrm{H},<1 \%\right)$ and two of chlorine occur naturally ${ }^{35} \mathrm{Cl}$, $76 \%$, and $\left.{ }^{37} \mathrm{Cl}, 24 \%\right)$. (a) How many different masses of HCl molecules can be formed from these isotopes?
(b) What is the approximate mass of each of the molecules, expressed in atomic mass units? (Use atomic weights rounded to the nearest whole number.) (c) List these $\mathrm{HCl}$ molecules in order of decreasing relative abundance.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:37

Problem 143

$\mathrm{CH}_{4}$ is methane. If ${ }^{1} \mathrm{H},{ }^{2} \mathrm{H},{ }^{12} \mathrm{C}$, and ${ }^{13} \mathrm{C}$ were the only
isotopes present in a given sample of methane, show the different formulas and formula weights that might exist in that sample. (Use atomic weights rounded to the nearest whole number.)

Ronald Prasad
Ronald Prasad
Numerade Educator
04:23

Problem 144

Sodium is easily identified in a solution by its strong emission at $\lambda=589 \mathrm{~nm}$. According to Einstein's equation, $E=m c^{2}$ (where $m$ is mass), this amount of energy can be converted into mass. What is the mass equivalent of one photon emitted by an excited sodium atom? $\left(1 \mathrm{~J}=1 \mathrm{~kg} \cdot \mathrm{m}^{2} / \mathrm{s}^{2}\right)$

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:51

Problem 145

A student was asked to calculate the wavelength and frequency of light emitted for an electron making the following transitions:
(a) $n=6 \rightarrow n=2$, and
(b) $n=6 \rightarrow n=3$. She was asked to determine whether she would be able to visually detect either of these electron transitions. Are her responses below correct? If not, make the necessary corrections.
(a) $1 / \lambda=\left(1.097 \times 10^{7} / \mathrm{m}\right)\left(1 / 2^{2}-1 / 6^{2}\right)=$
$2.44 \times 10^{6} / \mathrm{m} ; \lambda=244 \mathrm{~nm}$
(b) $1 / \lambda=\left(1.907 \times 10^{7} / \mathrm{m}\right)\left(1 / 3^{2}-1 / 6^{2}\right)=$
$9.14 \times 10^{5} / \mathrm{m} ; \lambda=1090 \mathrm{~nm}$
She concluded that she couldn't see either of the transitions because neither is in the visible region of the spectrum.

Ronald Prasad
Ronald Prasad
Numerade Educator
04:41

Problem 146

When compounds of barium are heated in a flame, green light of wavelength $554 \mathrm{~nm}$ is emitted. How much energy is lost when one mole of barium atoms each emit one photon of this wavelength?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:21

Problem 147

A 60 -watt light bulb consumes energy at the rate of $60 \mathrm{~J} \cdot \mathrm{s}^{-1}$. Much of the light is emitted in the infrared region, and less than $5 \%$ of the energy appears as visible light. Calculate the number of visible photons emitted per second. Make the simplifying assumptions that $5.0 \%$ of the light is visible and that all visible light has a wavelength of $550 \mathrm{~nm}$ (yellow-green).

Ronald Prasad
Ronald Prasad
Numerade Educator
02:21

Problem 148

Classical music radio station KMFA in Austin broadcasts at a frequency of $89.5 \mathrm{MHz}$. What is the wavelength of its signal in meters?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:37

Problem 149

(a) How many electrons are in $30.0 \mathrm{~g}$ of copper?
(b) How many electrons are in one mole of fluorine molecules?

Ronald Prasad
Ronald Prasad
Numerade Educator
04:35

Problem 150

(a) How many electrons are in one mole of nitrogen molecules? (b) How many electrons are in $30.0 \mathrm{~g}$ of water?

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
02:10

Problem 151

At www.chemsoc.org/viselements or another suitable website, locate information on scandium, vanadium, chromium, and copper that will assist you in answering the following questions.
(a) Which of the four elements listed was first isolated in a laboratory in Mexico?
(b) Which was discovered first?
(c) Which of the four elements are (is) not essential in our diet?
(d) Which has only two known nonzero oxidation states?

Ronald Prasad
Ronald Prasad
Numerade Educator
03:19

Problem 152

Use an internet search engine (such as http://www .google.com) to locate a table of isotopes found in naturally occurring samples of nickel. From these data, calculate the atomic mass of nickel. How does your answer compare to the value found on the Periodic Table? How do the values you found compare to those in Exercise $31 ?$

Ronald Prasad
Ronald Prasad
Numerade Educator
01:59

Problem 153

Use an internet search engine (such as http://www .google.com) to locate a table of isotopes found in naturally occurring samples of chromium. How many neutrons are present in an atom of each stable isotope of chromium? How does the data you found compare to that in Exercise 38 ?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:11

Problem 154

Use an internet search engine (such as http://www.google .com) to locate a biography of Sir Isaac Newton. How old was he when he entered college? How old was he when he died?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:30

Problem 155

Go to home.att.net/ numericana/answer/humor .htm#units. (a) Locate the value for microcentury expressed in minutes. (b) Locate the so-called "New Scientific Units" and give your favorite one.

Ronald Prasad
Ronald Prasad
Numerade Educator