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Chemistry

Paul Flowers, Klaus Theopold, Richard Langley

Chapter 6

Electronic Structure and Periodic Properties of Elements - all with Video Answers

Educators


Chapter Questions

00:47

Problem 1

The light produced by a red neon sign is due to the emission of light by excited neon atoms. Qualitatively
describe the spectrum produced by passing light from a neon lamp through a prism.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
00:37

Problem 2

An FM radio station found at 103.1 on the FM dial broadcasts at a frequency of $1.031 \times 10^{8} \mathrm{s}^{-1}(103.1 \mathrm{MHz})$ What is the wavelength of these radio waves in meters?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:46

Problem 3

FM-95, an FM radio station, broadcasts at a frequency of 9.51 $\times 10^{7} \mathrm{s}^{-1}(95.1 \mathrm{MHz})$. What is the wavelength of these radio waves in meters?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
01:08

Problem 4

A bright violet line occurs at $435.8 \mathrm{nm}$ in the emission spectrum of mercury vapor. What amount of energy, in joules, must be released by an electron in a mercury atom to produce a photon of this light?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:36

Problem 5

Light with a wavelength of $614.5 \mathrm{nm}$ looks orange. What is the energy, in joules, per photon of this orange light? What is the energy in eV $\left(1 \mathrm{eV}=1.602 \times 10^{-19} \mathrm{J}\right) ?$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:21

Problem 6

Heated lithium atoms emit photons of light with an energy of $2.961 \times 10^{-19} \mathrm{J}$. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the
emitted light?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
05:45

Problem 7

A photon of light produced by a surgical laser has an energy of $3.027 \times 10^{-19} \mathrm{J}$. Calculate the frequency and wavelength of the photon. What is the total energy in 1 mole of photons? What is the color of the emitted light?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:06

Problem 8

When rubidium ions are heated to a high temperature, two lines are observed in its line spectrum at wavelengths (a) $7.9 \times 10^{-7} \mathrm{m}$ and $(\mathrm{b}) 4.2 \times 10^{-7} \mathrm{m} .$ What are the frequencies of the two lines? What color do we see when we heat a rubidium compound?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
06:47

Problem 9

The emission spectrum of cesium contains two lines whose frequencies are (a) $3.45 \times 10^{14} \mathrm{Hz}$ and (b) $6.53 \times$ $10^{14} \mathrm{Hz} .$ What are the wavelengths and energies per photon of the two lines? What color are the lines?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
04:01

Problem 10

Photons of infrared radiation are responsible for much of the warmth we feel when holding our hands before a fire. These photons will also warm other objects. How many infrared photons with a wavelength of $1.5 \times 10^{-6} \mathrm{m}$ must be absorbed by the water to warm a cup of water (175 g) from $25.0^{\circ} \mathrm{C}$ to $40^{\circ} \mathrm{C} ?$

Rabia Shuaib
Rabia Shuaib
Numerade Educator
02:32

Problem 11

One of the radiographic devices used in a dentist's office emits an X-ray of wavelength $2.090 \times 10^{-11} \mathrm{m}$. What is the energy, in joules, and frequency of this X-ray?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:43

Problem 12

The eyes of certain reptiles pass a single visual signal to the brain when the visual receptors are struck by photons of a wavelength of $850 \mathrm{nm} .$ If a total energy of $3.15 \times 10^{-14} \mathrm{J}$ is required to trip the signal, what is the minimum number of photons that must strike the receptor?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
05:54

Problem 13

RGB color television and computer displays use cathode ray tubes that produce colors by mixing red, green, and blue light. If we look at the screen with a magnifying glass, we can see individual dots turn on and off as the colors change. Using a spectrum of visible light, determine the approximate wavelength of each of these colors. What is the frequency and energy of a photon of each of these colors?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
09:46

Problem 14

Answer the following questions about a Blu-ray laser:
(a) The laser on a Blu-ray player has a wavelength of $405 \mathrm{nm}$. In what region of the electromagnetic spectrum is this radiation? What is its frequency?
(b) A Blu-ray laser has a power of 5 milliwatts (1 watt $=1 \mathrm{J} \mathrm{s}^{-1}$ ). How many photons of light are produced by the laser in 1 hour?
(c) The ideal resolution of a player using a laser (such as a Blu-ray player), which determines how close together data can be stored on a compact disk, is determined using the following formula: Resolution $=0.60(\lambda \text { (NA), where } \lambda$ is the wavelength of the laser and NA is the numerical aperture. Numerical aperture is a measure of the size of the spot of light on the disk; the larger the NA, the smaller the spot. In a typical Blu-ray system, NA = 0.95. If the 405-nm laser is used in a Blu-ray player, what is the closest that information can be stored on a Blu-ray disk?
(d) The data density of a Blu-ray disk using a 405-nm laser is 1.5 $\times 10^{7}$ bits $\mathrm{mm}^{-2}$. Disks have an outside diameter
of $120 \mathrm{mm}$ and a hole of $15-\mathrm{mm}$ diameter. How many data bits can be contained on the disk? If a Blu-ray disk can hold 9,400,000 pages of text, how many data bits are needed for a typed page? (Hint: Determine the area of the disk that is available to hold data. The area inside a circle is given by $\mathrm{A}=\pi r^{2},$ where the radius $r$ is one-half of the diameter.)

Rabia Shuaib
Rabia Shuaib
Numerade Educator
10:42

Problem 15

What is the threshold frequency for sodium metal if a photon with frequency $6.66 \times 10^{14} \mathrm{s}^{-1}$ ejects an electron with $7.74 \times 10^{-20} \mathrm{J}$ kinetic energy? Will the photoelectric effect be observed if sodium is exposed to orange light?

Dr.  Satish  Ingale
Dr. Satish Ingale
Numerade Educator
01:06

Problem 16

Why is the electron in a Bohr hydrogen atom bound less tightly when it has a quantum number of 3 than when
it has a quantum number of 1?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
00:44

Problem 17

What does it mean to say that the energy of the electrons in an atom is quantized?

Will Li
Will Li
Numerade Educator
01:27

Problem 18

Using the Bohr model, determine the energy, in joules, necessary to ionize a ground-state hydrogen atom. Show
your calculations.

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:42

Problem 19

The electron volt (eV) is a convenient unit of energy for expressing atomic-scale energies. It is the amount of energy that an electron gains when subjected to a potential of 1 volt; $1\ \mathrm{eV}=1.602 \times 10^{-19} \mathrm{J} .$ Using the Bohr model, determine the energy, in electron volts, of the photon produced when an electron in a hydrogen atom moves from the orbit with $n=5$ to the orbit with $n=2 .$ Show your calculations.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
01:47

Problem 20

Using the Bohr model, determine the lowest possible energy, in joules, for the electron in the $L$ i $^{2+}$ ion.

Rabia Shuaib
Rabia Shuaib
Numerade Educator
01:28

Problem 21

Using the Bohr model, determine the lowest possible energy for the electron in the $\mathrm{He}^{+}$ ion.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
00:55

Problem 22

Using the Bohr model, determine the energy of an electron with $n=6$ in a hydrogen atom.

Matthew Hurlock
Matthew Hurlock
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01:15

Problem 23

Using the Bohr model, determine the energy of an electron with $n=8$ in a hydrogen atom.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:39

Problem 24

How far from the nucleus in angstroms (1 angstrom $=1 \times 10^{-10} \mathrm{m}$ ) is the electron in a hydrogen atom if it has an energy of $-8.72 \times 10^{-20} \mathrm{J} ?$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:48

Problem 25

What is the radius, in angstroms, of the orbital of an electron with $n=8$ in a hydrogen atom?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
01:37

Problem 26

Using the Bohr model, determine the energy in joules of the photon produced when an electron in a $\mathrm{He}^{+}$ ion moves from the orbit with $n=5$ to the orbit with $n=2$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:54

Problem 27

Using the Bohr model, determine the energy in joules of the photon produced when an electron in a $\mathrm{Li}^{2+}$ ion moves from the orbit with $n=2$ to the orbit with $n=1$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
06:54

Problem 28

Consider a large number of hydrogen atoms with electrons randomly distributed in the $n=1,2,3,$ and 4 orbits.
(a) How many different wavelengths of light are emitted by these atoms as the electrons fall into lower-energy orbitals?
(b) Calculate the lowest and highest energies of light produced by the transitions described in part (a).
(c) Calculate the frequencies and wavelengths of the light produced by the transitions described in part (b).

Rabia Shuaib
Rabia Shuaib
Numerade Educator
01:56

Problem 29

How are the Bohr model and the Rutherford model of the atom similar? How are they different?

Rabia Shuaib
Rabia Shuaib
Numerade Educator
02:59

Problem 30

The spectra of hydrogen and of calcium are shown here.What causes the lines in these spectra? Why are the colors of the lines different? Suggest a reason for the observation that the spectrum of calcium is more complicated than the spectrum of hydrogen.

Rabia Shuaib
Rabia Shuaib
Numerade Educator
08:23

Problem 31

How are the Bohr model and the quantum mechanical model of the hydrogen atom similar? How are they
different?

Dr.  Satish  Ingale
Dr. Satish Ingale
Numerade Educator
02:24

Problem 32

What are the allowed values for each of the four quantum numbers: $n, l, m_{l},$ and $m_{s} ?$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
05:06

Problem 33

Describe the properties of an electron associated with each of the following four quantum numbers: $n, l, m_{l}$, and
$m_{\mathrm{s}}$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:56

Problem 34

Answer the following questions:
(a) Without using quantum numbers, describe the differences between the shells, subshells, and orbitals of an atom.
(b) How do the quantum numbers of the shells, subshells, and orbitals of an atom differ?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:17

Problem 35

Identify the subshell in which electrons with the following quantum numbers are found:
(a) $n=2, I=1$
(b) $n=4, l=2$
(c) $n=6,1=0$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
00:45

Problem 36

Which of the subshells described in the previous question contain degenerate orbitals? How many degenerate
orbitals are in each?

Nicole Smina
Nicole Smina
Numerade Educator
02:21

Problem 37

Identify the subshell in which electrons with the following quantum numbers are found:
(a) $n=3,1=2$
(b) $n=1, l=0$
(c) $n=4, l=3$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
00:45

Problem 38

Which of the subshells described in the previous question contain degenerate orbitals? How many degenerate
orbitals are in each?

Nicole Smina
Nicole Smina
Numerade Educator
02:13

Problem 39

Sketch the boundary surface of a $d_{x^{2}-y^{2}}$ and a $p_{y}$ orbital. Be sure to show and label the axes.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
01:58

Problem 40

Sketch the $p_{x}$ and $d_{x z}$ orbitals. Be sure to show and label the coordinates.

Matthew Hurlock
Matthew Hurlock
Numerade Educator
05:27

Problem 41

Consider the orbitals shown here in outline.(a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)?
(b) How many orbitals of type (x) are found in a shell with $n=2$ ? How many of type (y)? How many of type (z)?
(c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell with $n=4 .$ Of an orbital of type
(y) in a shell with $n=2 .$ Of an orbital of type $(z)$ in a shell with $n=3$
(d) What is the smallest possible $n$ value for an orbital of type (x)? Of type (y)? Of type (z)?
(e) What are the possible $l$ and $m_{l}$ values for an orbital of type (x)? Of type (y)? Of type (z)?

Rabia Shuaib
Rabia Shuaib
Numerade Educator
02:17

Problem 42

State the Heisenberg uncertainty principle. Describe briefly what the principle implies.

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:58

Problem 43

How many electrons could be held in the second shell of an atom if the spin quantum number $m_{s}$ could have three values instead of just two? (Hint: Consider the Pauli exclusion principle.)

Jasmine Haskell
Jasmine Haskell
Numerade Educator
04:07

Problem 44

Which of the following equations describe particle-like behavior? Which describe wavelike behavior? Do any involve both types of behavior? Describe the reasons for your choices.
(a) $c=\lambda v$
(b) $E=\frac{m \nu^{2}}{2}$
(c) $r=\frac{n^{2} a_{0}}{Z}$
(d) $E=h v$
(e) $\lambda=\frac{h}{m \nu}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
04:58

Problem 45

Write a set of quantum numbers for each of the electrons with an $n$ of 4 in a Se atom.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
03:58

Problem 46

Read the labels of several commercial products and identify monatomic ions of at least four transition elements
contained in the products. Write the complete electron configurations of these cations.

Matthew Hurlock
Matthew Hurlock
Numerade Educator
07:00

Problem 47

Read the labels of several commercial products and identify monatomic ions of at least six main group
elements contained in the products. Write the complete electron configurations of these cations and anions.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:35

Problem 48

Using complete subshell notation (not abbreviations, $1 s^{2} 2 s^{2} 2 p^{6},$ and so forth), predict the electron configuration of each of the following atoms:
(a) $\mathrm{C}$
(b) $\mathrm{P}$
(c) V
(d) Sb
(e) Sm

Dr.  Satish  Ingale
Dr. Satish Ingale
Numerade Educator
05:13

Problem 49

Using complete subshell notation $ (1 s^{2} 2 s^{2} 2 p^{6},$ and so forth), predict the electron configuration of each of the \right. following atoms:
(a) $\mathrm{N}$
(b) Si
(c) $\mathrm{Fe}$
(d) Te
(e) Tb

Will Li
Will Li
Numerade Educator
01:49

Problem 50

Is $1 s^{2} 2 s^{2} 2 p^{6}$ the symbol for a macroscopic property or a microscopic property of an element? Explain your
answer.

Rabia Shuaib
Rabia Shuaib
Numerade Educator
02:53

Problem 51

What additional information do we need to answer the question "Which ion has the electron configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} ”$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
03:36

Problem 52

Draw the orbital diagram for the valence shell of each of the following atoms:
(a) $\mathrm{C}$
(b) $\mathrm{P}$
(c) V
(d) Sb
(e) Ru

Matthew Hurlock
Matthew Hurlock
Numerade Educator
06:46

Problem 53

Use an orbital diagram to describe the electron configuration of the valence shell of each of the following atoms:
(a) $\mathrm{N}$
(b) Si
(c) Fe
(d) Te
(e) Mo

Jasmine Haskell
Jasmine Haskell
Numerade Educator
06:55

Problem 54

Using complete subshell notation $ (1 s^{2} 2 s^{2} 2 p^{6},$ and so forth), predict the electron configurations of the following \right. ions.

(a) $\mathrm{N}^{3-}$
(b) $\mathrm{Ca}^{2+}$
(c) $\mathrm{S}^{-}$
(d) $\mathrm{Cs}^{2+}$
(e) $\mathrm{Cr}^{2+}$
(f) $\mathrm{Gd}^{3+}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
00:54

Problem 55

Which atom has the electron configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6} 5 s^{2} 4 d^{2} ?$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
01:10

Problem 56

Which atom has the electron configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{7} 4 s^{2} ?$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:54

Problem 57

Which ion with a +1 charge has the electron configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} ?$ Which ion with a -2 charge has this configuration?

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
01:18

Problem 58

Which of the following atoms contains only three valence electrons: Li, $\mathrm{B}, \mathrm{N}, \mathrm{F}, \mathrm{Ne} ?$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:39

Problem 59

Which of the following has two unpaired electrons?
(a) Mg
(b) Si
(c) $\mathrm{S}$
(d) Both Mg and S
(e) Both Si and S.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
01:10

Problem 60

Which atom would be expected to have a half-filled 6p subshell?

Matthew Hurlock
Matthew Hurlock
Numerade Educator
00:48

Problem 61

Which atom would be expected to have a half-filled 4s subshell?

Will Li
Will Li
Numerade Educator
04:36

Problem 62

In one area of Australia, the cattle did not thrive despite the presence of suitable forage. An investigation showed the cause to be the absence of sufficient cobalt in the soil. Cobalt forms cations in two oxidation states, $\mathrm{Co}^{2+}$ and $\mathrm{Co}^{3+} .$ Write the electron structure of the two cations.

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:01

Problem 63

Thallium was used as a poison in the Agatha Christie mystery story “The Pale Horse." Thallium has two possible cationic forms, +1 and $+3 .$ The +1 compounds are the more stable. Write the electron structure of the +1 cation of thallium.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
05:43

Problem 64

Write the electron configurations for the following atoms or ions:
(a) $\mathrm{B}^{3+}$
(b) $\mathrm{O}^{-}$
(c) $\mathrm{Cl}^{3+}$
(d) $\mathrm{Ca}^{2+}$
(e) Ti

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
05:22

Problem 65

Cobalt- 60 and iodine- 131 are radioactive isotopes commonly used in nuclear medicine. How many protons,
neutrons, and electrons are in atoms of these isotopes? Write the complete electron configuration for each isotope.

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
03:28

Problem 66

Write a set of quantum numbers for each of the electrons with an $n$ of 3 in a Sc atom.

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:28

Problem 67

Based on their positions in the periodic table, predict which has the smallest atomic radius: Mg, Sr, Si, Cl, I.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
02:01

Problem 68

Based on their positions in the periodic table, predict which has the largest atomic radius: Li, Rb, $\mathrm{N}, \mathrm{F}, \mathrm{I}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:02

Problem 69

Based on their positions in the periodic table, predict which has the largest first ionization energy: Mg, Ba, B, O, Te.

Jasmine Haskell
Jasmine Haskell
Numerade Educator
03:03

Problem 70

Based on their positions in the periodic table, predict which has the smallest first ionization energy:
$\mathrm{Li}, \mathrm{Cs}, \mathrm{N}, \mathrm{F}, \mathrm{I}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:56

Problem 71

Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: $\mathbf{F}, \mathbf{L i}, \mathbf{N}, \mathbf{R b}$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
03:56

Problem 72

Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: $\mathrm{Mg}, \mathrm{O}, \mathrm{S}, \mathrm{Si}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:38

Problem 73

Atoms of which group in the periodic table have a valence shell electron configuration of $n s^{2} n p^{3} ?$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
02:24

Problem 74

Atoms of which group in the periodic table have a valence shell electron configuration of $n s^{2} ?$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:19

Problem 75

Based on their positions in the periodic table, list the following atoms in order of increasing radius: $\mathrm{Mg}, \mathrm{Ca}, \mathrm{Rb}, \mathrm{Cs}$

Will Li
Will Li
Numerade Educator
03:05

Problem 76

Based on their positions in the periodic table, list the following atoms in order of increasing radius: $\mathrm{Sr}, \mathrm{Ca}, \mathrm{Si}, \mathrm{Cl}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
01:51

Problem 77

Based on their positions in the periodic table, list the following ions in order of increasing radius: $\mathrm{K}^{+}, \mathrm{Ca}^{2+}$ $\mathrm{Al}^{3+}, \mathrm{Si}^{4+}$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
04:04

Problem 78

List the following ions in order of increasing radius: $\mathrm{Li}^{+}, \mathrm{Mg}^{2+}, \mathrm{Br}^{-}, \mathrm{Te}^{2-}$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
04:38

Problem 79

Which atom and/or ion is (are) isoelectronic with $\mathrm{Br}^{+}: \mathrm{Se}^{2+},$ Se, $\mathrm{As}^{-}, \mathrm{Kr}, \mathrm{Ga}^{3+}, \mathrm{Cl}^{-}$ ?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
03:46

Problem 80

Which of the following atoms and ions is (are) isoelectronic with $S^{2+}: S_{i}^{4+}, C^{3+}, A r, A s^{3+}, S i, A I^{3+} ?$

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
02:50

Problem 81

Compare both the numbers of protons and electrons present in each to rank the following ions in order of increasing radius: $\mathrm{As}^{3-}, \mathrm{Br}^{-}, \mathrm{K}^{+}, \mathrm{Mg}^{2+}$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
04:10

Problem 82

Of the five elements $\mathrm{Al}, \mathrm{Cl}, \mathrm{I}, \mathrm{Na}, \mathrm{Rb},$ which has the most exothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? Hint: Note the process depicted does not correspond to electron affinity.) $\mathrm{E}^{+}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{E}(g)$

Matthew Hurlock
Matthew Hurlock
Numerade Educator
02:22

Problem 83

Of the five elements $\mathrm{Sn}, \mathrm{Si}, \mathrm{Sb}, \mathrm{O}, \mathrm{Te}$ which has the most endothermic reaction? (E represents an atom.) What name is given to the energy for the reaction? $\mathrm{E}(g) \longrightarrow \mathrm{E}^{+}(g)+\mathrm{e}^{-}$

Jasmine Haskell
Jasmine Haskell
Numerade Educator
03:09

Problem 84

The ionic radii of the ions $S^{2-}, C l^{-},$ and $K^{+}$ are 184,181,138 pm respectively. Explain why these ions have different sizes even though they contain the same number of electrons.

Daniel Kyinakwa
Daniel Kyinakwa
Numerade Educator
02:53

Problem 85

Which main group atom would be expected to have the lowest second ionization energy?

Jasmine Haskell
Jasmine Haskell
Numerade Educator
00:54

Problem 86

Explain why Al is a member of group 13 rather than group $3 ?$

Matthew Hurlock
Matthew Hurlock
Numerade Educator