Chemistry Principles and Practice

Problem 3

Graph the atomic radii versus atomic number of the first 18 elements. Explain the trends in radii across the second period and down Group $1 \mathrm{~A}$.

Crystal Wang

Numerade Educator

03:10

Problem 4

Explain why carbon atoms are larger than oxygen atoms even though oxygen contains more electrons.

Lane Francis

Numerade Educator

01:48

Problem 5

Why are sulfur atoms larger than oxygen atoms?

Lane Francis

Numerade Educator

01:04

Problem 6

Define ionization energy. Write an equation for the first ionization energy for lithium. Write the electron configuration of each species in the equation.

Crystal Wang

Numerade Educator

01:58

Problem 7

How many different values of ionization energy does an atom have? What determines this number?

Crystal Wang

Numerade Educator

02:43

Problem 8

Graph ionization energy versus atomic number for the second-period elements. Explain the trends and any discontinuities in the graph.

Crystal Wang

Numerade Educator

01:17

Problem 9

Even though ionization energies generally increase from left to right across the periodic table, the first ionization energy for aluminum is lower than that for magnesium. How can this observation be explained?

Crystal Wang

Numerade Educator

View

Problem 10

Explain why the first ionization energy of sodium is slightly lower than that of lithium.

Ashley Brady

Numerade Educator

02:52

Problem 11

Explain why the first ionization energies of manganese, iron, and cobalt increase very slightly, whereas in the series of gallium, germanium, and arsenic, the first ionization energy increases considerably.

Crystal Wang

Numerade Educator

02:23

Problem 12

Explain why the second ionization energy of magnesium is about twice the first, but the third ionization energy is more than four times the second.

Ashley Brady

Numerade Educator

01:24

Problem 13

The first ionization energy of boron is $800 \mathrm{~kJ} / \mathrm{mol}$. Qualitatively discuss the expected values of the next three ionization energies of boron. Discuss the reasons for any big differences between them.

Crystal Wang

Numerade Educator

03:20

Problem 14

Explain why the first ionization energy of magnesium is greater than the first ionization energies of both sodium and aluminum.

Crystal Wang

Numerade Educator

01:16

Problem 15

Aluminum atoms are larger than silicon atoms, and the first ionization energy of silicon is greater than that of aluminum. Explain these trends, using differences in the effective nuclear charges.

Crystal Wang

Numerade Educator

01:28

Problem 16

Define electron affinity.

Crystal Wang

Numerade Educator

01:33

Problem 17

In which group in the periodic table would you expect the elements to have strongly exothermic electron affinities? Explain your answer.

Crystal Wang

Numerade Educator

02:46

Problem 18

How do electron affinities vary down a group?

Crystal Wang

Numerade Educator

02:40

Problem 19

Explain why the electron affinity of lithium is slightly favorable (exothermic), whereas the electron affinity of beryllium is unfavorable (endothermic). Contrast these trends with the ionization energy trends of these two elements.

Crystal Wang

Numerade Educator

01:10

Problem 20

Describe the physical properties of the elements in Group $1 \mathrm{~A}$.

Lane Francis

Numerade Educator

01:10

Problem 21

Describe the physical properties of the elements in Group $2 \mathrm{~A}$.

Lane Francis

Numerade Educator

01:05

Problem 22

Describe the physical properties of the elements in Group 7A.

Lane Francis

Numerade Educator

02:32

Problem 23

State the reactivity trend down the group for the elements in the following groups.
(a) $1 \mathrm{~A}$
(b) $2 \mathrm{~A}$
(c) $7 \mathrm{~A}$

Ashley Brady

Numerade Educator

00:57

Problem 24

Using Figure 8.18 , suggest compounds from Group $1 \mathrm{~A}$ to put in fireworks that would burn
(a) red.
(b) yellow.

Crystal Wang

Numerade Educator

05:19

Problem 25

Write the electron configurations of the following elements after finding their locations in the periodic table.
(a) $\mathrm{P}$
(b) $\mathrm{Sr}$
(c) $\mathrm{Sm}$
(d) $\mathrm{Ra}$

Ashley Brady

Numerade Educator

03:04

Problem 26

Write the electron configurations of the following elements after finding their locations in the periodic table.
(a) $\mathrm{B}$
(b) $\mathrm{Bi}$
(c) $\mathrm{Ba}$
(d) $\mathrm{Cd}$

Crystal Wang

Numerade Educator

Problem 27

Identify the block of the periodic table where each of the following elements is.
(a) $\mathrm{Gd}$
(b) $\mathrm{Ir}$
(c) $\mathrm{As}$
(d) $\mathrm{Sc}$

Lane Francis

Numerade Educator

02:11

Problem 28

Identify the block of the periodic table where each of the following elements is.
(a) $\mathrm{Tl}$
(b) $\mathrm{B e}$
(c) $\mathrm{Xe}$
(d) $U$

Lane Francis

Numerade Educator

01:35

Problem 29

Using the abbreviated notation, write the ground-state electron configuration of the following ions.
(a) $\mathrm{S}^{2-}$
(b) $\mathrm{Mn}^{2+}$
(c) $\mathrm{Ge}^{2+}$

Crystal Wang

Numerade Educator

01:49

Problem 30

Using the abbreviated notation, write the ground-state electron configuration of the following ions.
(a) $Y^{3+}$
(b) $\mathrm{Br}^{-}$
(c) $\mathrm{Rh}^{2+}$

Crystal Wang

Numerade Educator

Problem 31

Using the abbreviated notation, write the ground-state electron configuration of the following ions.
(a) $\mathrm{P}^{2-}$
(b) $\mathrm{Fe}^{2+}$
(c) $\mathrm{Co}^{3+}$

Crystal Wang

Numerade Educator

01:56

Problem 32

Using the abbreviated notation, write the ground-state electron configuration of the following ions.
(a) $\mathrm{Ga}^{2+}$
(b) $\mathrm{Se}^{2-}$
(c) $\mathrm{Ru}^{2+}$

Crystal Wang

Numerade Educator

02:10

Problem 33

Identify the cations with a $1+$ charge that have the following electron configurations.
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$
(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10}$

Crystal Wang

Numerade Educator

01:36

Problem 34

Identify the cations with a $2+$ charge that have the following electron configurations.
(a) $[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{1}$
(b) $1 s^{2} 2 s^{2} 2 p^{1}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$

Crystal Wang

Numerade Educator

Problem 35

Identify the anions with a $2-$ charge that have the following electron configurations.
(a) $[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{6}$
(b) $1 s^{2} 2 s^{2} 2 p^{5}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}$

Crystal Wang

Numerade Educator

01:28

Problem 36

Identify the anions with a $1-$ charge that have the following electron configurations.
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}$
(b) $1 s^{2} 2 s^{2} 2 p^{5}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{5}$

Crystal Wang

Numerade Educator

01:21

Problem 37

Write the ground-state electron configurations for $\mathrm{Fe}^{3+}$ and $\mathrm{Cr}^{3+}$

Crystal Wang

Numerade Educator

01:21

Problem 38

Which transition-metal ion with a $3+$ charge has the ground-state electron configuration $[\mathrm{Kr}] 4 d^{5}$ ?

Crystal Wang

Numerade Educator

02:04

Problem 39

Write the symbols for a cation and an anion that are isoelectronic with Se.

Lane Francis

Numerade Educator

02:26

Problem 40

Write the symbols for two cations and two anions that are isoelectronic with $\mathrm{Kr}$

Lane Francis

Numerade Educator

02:17

Problem 41

What neutral atoms are isoelectronic with the following ions?
(a) $\mathrm{O}^{2-}$
(b) $\mathrm{Fe}^{2+}$
(c) $\mathrm{Fe}^{3+}$
(d) $\mathrm{In}^{+}$

Lane Francis

Numerade Educator

02:11

Problem 42

What neutral atoms are isoelectronic with the following ions?
(a) $\mathrm{Pb}^{4+}$
(b) $\mathrm{Br}^{-}$
(c) $\mathrm{S}^{2-}$
(d) $\mathrm{Ni}^{3+}$

Lane Francis

Numerade Educator

01:24

Problem 43

Which of the following species are not isoelectronic with the rest: $\mathrm{F}^{-}, \mathrm{Ne}, \mathrm{Na}^{+}, \mathrm{Ca}^{2+} ?$

Lane Francis

Numerade Educator

01:33

Problem 44

Which of the following species are not isoelectronic with the rest: $\mathrm{Ar}, \mathrm{K}^{+}, \mathrm{Ca}^{2+}, \mathrm{Y}^{3+} ?$

Lane Francis

Numerade Educator

01:49

Problem 45

Which species in each of the following pairs is larger? Explain your answer.
(a) $\mathrm{Na}$ or $\mathrm{Na}^{+}$
(b) $\mathrm{O}^{2-}$ or $\mathrm{F}^{-}$
(c) $\mathrm{Ni}^{2+}$ or $\mathrm{Ni}^{3+}$

Crystal Wang

Numerade Educator

02:17

Problem 46

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

Crystal Wang

Numerade Educator

01:32

Problem 47

Which species in each of the following pairs is larger? Explain your answer.
(a) $\mathrm{Na}$ or $\mathrm{Mg}$
(b) $B$ or $\mathrm{O}$
(c) $\mathrm{Be}^{2+}$ or $\mathrm{Be}^{3+}$

Crystal Wang

Numerade Educator

02:18

Problem 48

Which species in each of the following pairs is larger? Explain your answer.
(a) $\mathrm{Li}$ or $\mathrm{Na}$
(b) $\mathrm{O}$ or $\mathrm{P}$
(c) $\mathrm{Rb}$ or $\mathrm{Rb}^{+}$

Crystal Wang

Numerade Educator

02:56

Problem 49

Using only a periodic table as a guide, arrange each of the following series of atoms in order of increasing size.
(a) $\mathrm{B}, \mathrm{O}, \mathrm{Li}$
(b) $\mathrm{C}, \mathrm{N}, \mathrm{Si}$
(c) $\mathrm{S}, \mathrm{As}, \mathrm{Sn}$

Lane Francis

Numerade Educator

03:28

Problem 50

Using only a periodic table as a guide, arrange each of the following series of atoms in order of increasing size.
(a) $\mathrm{Na}, \mathrm{Be}, \mathrm{Li}$
(b) $\mathrm{P}, \mathrm{N}, \mathrm{F}$
(c) $\mathrm{I}, \mathrm{O}, \mathrm{Sn}$

Lane Francis

Numerade Educator

01:35

Problem 51

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.
(a) $\mathrm{Li}, \mathrm{Be}^{2+}, \mathrm{Be}$
(b) $\mathrm{S}, \mathrm{S}^{2-}, \mathrm{Cl}$
(c) $\mathrm{O}, \mathrm{S}, \mathrm{Si}$

Crystal Wang

Numerade Educator

02:43

Problem 52

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing size.
(a) $\mathrm{F}, \mathrm{F}^{-}, \mathrm{O}^{2-}$
(b) $\mathrm{Al}^{3+}, \mathrm{Mg}, \mathrm{Na}$
(c) $\mathrm{N}, \mathrm{P}, \mathrm{Si}$

Crystal Wang

Numerade Educator

01:23

Problem 53

Which element in the second period has the largest atomic radius? Why?

Ashley Brady

Numerade Educator

01:34

Problem 54

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

Numerade Educator

01:06

Problem 55

Of the atoms with the electron configurations $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$ and $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3},$ which is larger?

Crystal Wang

Numerade Educator

Problem 56

Of the atoms with the electron configurations $1 s^{2} 2 s^{2} 2 p^{4}$ and $1 s^{2} 2 s^{2} 2 p^{2},$ which is smaller?

Crystal Wang

Numerade Educator

01:48

Problem 57

Indicate which species in each pair has the higher first ionization energy. Explain your answer.
(a) $\mathrm{Si}$ or $\mathrm{Cl}$
(b) $\mathrm{Na}$ or $\mathrm{Rb}$
(c) $\mathrm{O}^{2-}$ or $\mathrm{F}^{-}$

Crystal Wang

Numerade Educator

01:51

Problem 58

Indicate which species in each pair has the higher ionization energy. Explain your answer.
(a) $\mathrm{N}$ or $\mathrm{F}$
(b) $\mathrm{Mg}^{2+}$ or $\mathrm{Na}^{+}$
(c) $\mathrm{K}$ or $\mathrm{Si}$

Crystal Wang

Numerade Educator

01:50

Problem 59

Indicate which species in each pair has the higher ionization energy. Explain your answer.
(a) Ge or $\mathrm{Cl}$
(b) $\mathrm{B}$ or $\mathrm{F}$
(c) $\mathrm{Al}^{3+}$ or $\mathrm{Na}^{+}$

Crystal Wang

Numerade Educator

02:05

Problem 60

Indicate which species in each pair has the higher ionization energy. Explain your answer.
(a) $\mathrm{K}$ or I
(b) $\mathrm{Al}$ or $\mathrm{Al}^{+}$
(c) $\mathrm{Cl}^{-}$ or $\mathrm{Ar}$

Crystal Wang

Numerade Educator

02:46

Problem 61

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.
(a) $\mathrm{O}, \mathrm{O}^{2-}, \mathrm{F}$
(b) $\mathrm{C}, \mathrm{Si}, \mathrm{N}$
(c) $\mathrm{Te}, \mathrm{Ru}, \mathrm{Sr}$

Crystal Wang

Numerade Educator

02:25

Problem 62

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.
(a) $\mathrm{S}, \mathrm{Se}^{2-}, \mathrm{O}$
(b) Fe, $\mathrm{Br}, \mathrm{F}$
(c) $\mathrm{Cl}, \mathrm{Cl}^{-}, \mathrm{F}$

Crystal Wang

Numerade Educator

01:30

Problem 63

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.
(a) $\mathrm{N}, \mathrm{N}^{3-}, \mathrm{Ne}$
(b) $\mathrm{P}, \mathrm{Si}, \mathrm{Cl}$
(c) $\mathrm{Ga}, \mathrm{O}, \mathrm{Se}$

Crystal Wang

Numerade Educator

01:37

Problem 64

Using only a periodic table as a guide, arrange each of the following series of species in order of increasing first ionization energy.
(a) $\mathrm{K}, \mathrm{Se}, \mathrm{S}$
(b) $\mathrm{Cr}, \mathrm{As}, \mathrm{O}$
(c) $\mathrm{O}, \mathrm{O}^{-}, \mathrm{F}$

Crystal Wang

Numerade Educator

01:04

Problem 65

Which second ionization energy is greater, that of aluminum or that of magnesium? Explain your answer.

Crystal Wang

Numerade Educator

01:04

Problem 66

Predict which of these elements would have the greatest difference between the first and second ionization energies: $\mathrm{Si}, \mathrm{Na}, \mathrm{P}, \mathrm{Mg} .$ Briefly explain your answer.

Nicole Mabante

Numerade Educator

01:10

Problem 67

Which third ionization energy is greater, that of aluminum or that of magnesium? Explain your answer.

Crystal Wang

Numerade Educator

01:08

Problem 68

Which second ionization energy is greater, that of oxygen or that of fluorine? Explain your answer.

Crystal Wang

Numerade Educator

01:02

Problem 69

$\mathrm{Li}^{2+}$ is not a common charge for a lithium ion. Use the ionization energies of lithium to explain why.

Crystal Wang

Numerade Educator

02:30

Problem 70

Suggest a reason for the lack of metal cations with a 4+ charge.

Crystal Wang

Numerade Educator

01:02

Problem 71

What is the electron configuration of the $\mathrm{Ba}^{3+}$ ion? Suggest a reason why this ion is not normally found in nature.

Crystal Wang

Numerade Educator

Problem 72

On which ionization (first, second, third, fourth, etc.) will the ionization energy of an $\mathrm{Al}$ atom increase dramatically? Explain why.

Crystal Wang

Numerade Educator

01:22

Problem 73

Indicate which species in each pair has the more negative electron affinity. Explain your answer.
(a) $\mathrm{S}$ or $\mathrm{Cl}$
(b) $\mathrm{N}$ or $\mathrm{O}$
(c) $\mathrm{S}$ or $\mathrm{F}$

Crystal Wang

Numerade Educator

01:05

Problem 74

Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answer.
(a) Se or $\mathrm{Br}$
(b) $\mathrm{S}$ or $\mathrm{P}$
(c) $\mathrm{Br}$ or $\mathrm{As}$

Crystal Wang

Numerade Educator

01:20

Problem 75

Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answer.
(a) $\mathrm{O}$ or $\mathrm{F}$
(b) $P$ or $\mathrm{Cl}$
(c) Se or $\mathrm{Br}$

Crystal Wang

Numerade Educator

02:03

Problem 76

Indicate which species in each pair has the more favorable (more negative) electron affinity. Explain your answer.
(a) $\mathrm{Br}$ or $\mathrm{Te}$
(b) $O$ or $B$
(c) In or Se

Crystal Wang

Numerade Educator

05:48

Problem 77

Write the equation for the reaction, if any, of sodium with the following substances.
(a) oxygen
(b) nitrogen
(c) chlorine
(d) water

Lane Francis

Numerade Educator

02:33

Problem 78

Write the equation for the reaction, if any, of lithium with the following substances.
(a) oxygen
(b) nitrogen
(c) chlorine
(d) water

Lane Francis

Numerade Educator

04:06

Problem 79

Write the equation for the reaction, if any, of barium with the following substances.
(a) oxygen
(b) water

Lane Francis

Numerade Educator

01:13

Problem 80

Write the equation for the reaction, if any, of calcium with the following substances.
(a) oxygen
(b) water

Crystal Wang

Numerade Educator

01:48

Problem 81

What is the trend in reactivity as you go down from $\mathrm{Li}$ to Cs in the periodic table? Give a reason for this trend.

Ashley Brady

Numerade Educator

01:55

Problem 82

What is the trend in reactivity as you go down from $\mathrm{F}$ to I in the periodic table? Give a reason for this trend.

Lane Francis

Numerade Educator

01:05

Problem 83

One way to generate hydrogen gas in the laboratory is to combine a reactive metal with water. The ensuing chemical reaction produces hydrogen gas as one product. Which element would generate hydrogen gas more vigorously when combined with water: potassium or calcium? Explain your answer. Write the balanced chemical reaction for both processes.

Crystal Wang

Numerade Educator

Problem 84

The presence of radioactive strontium in nuclear fallout (which is residue from atmospheric testing of nuclear bomb testing) is a major health concern because of strontium's periodic table relationship with calcium, a necessary nutrient. What is the reason for this concern?

Crystal Wang

Numerade Educator

02:31

Problem 85

What are the changes in (a) size, (b) ionization energy, and (c) electron affinity from potassium to calcium?

Crystal Wang

Numerade Educator

Problem 86

Write the electron configuration for the $3+$ cation of titanium.

Crystal Wang

Numerade Educator

Problem 87

Write the electron configuration for the $2+$ cation of calcium.

Ashley Brady

Numerade Educator

01:01

Problem 88

One sphere below represents a boron atom, while the other sphere represents an oxygen atom. Select the one that represents the boron atom. Explain your choice.

Crystal Wang

Numerade Educator

01:51

Problem 89

Three elements have the electron configurations $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$, $[\mathrm{Ar}] 4 s^{2}$, and $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$. The atomic radii of these elements (not necessarily in the same order) are 99,160 , and $231 \mathrm{pm}$. Identify the elements from the electron configurations, and match the sizes with these elements.

Crystal Wang

Numerade Educator

Problem 90

Write the electron configuration of the copper atom and the $2+$ cation of copper. Remember that the electron configuration of copper atom is unusual. Does the fact that copper is an exception to the aufbau principle influence the electron configuration of $\mathrm{Cu}^{2+} ?$

Crystal Wang

Numerade Educator

Problem 91

Palladium, with an electron configuration of $[\mathrm{Kr}] 4 d^{10},$ is an exception to the aufbau principle. Write the electron configuration of the $2+$ cation of palladium. Does the fact that palladium is an exception influence the electron configuration of $\mathrm{Pd}^{2+} ?$

Crystal Wang

Numerade Educator

Problem 92

List the element for which the $2+$ cation has the electron configuration $[\mathrm{Ar}] 3 d^{4}$.

Crystal Wang

Numerade Educator

01:06

Problem 93

Determine the number of unpaired electrons for a $\mathrm{Cr}^{4+}$ cation.

Crystal Wang

Numerade Educator

Problem 94

Identify which member of Group 5 A has the following characteristics:
(a) largest size
(b) smallest ionization energy

Crystal Wang

Numerade Educator

01:43

Problem 95

Of the following electron configurations:
(1) $1 s^{2} 2 s^{2} 2 p^{1}$
(2) $1 s^{2} 2 s^{2} 2 p^{4}$
(3) $1 s^{2} 2 s^{2} 2 p^{5}$
which represents the element with the
(a) largest size?
(b) smallest ionization energy?
(c) greatest electron affinity?

Crystal Wang

Numerade Educator

01:07

Problem 96

The mineral magnetite has the overall formula $\mathrm{Fe}_{3} \mathrm{O}_{4}$ (as $\left.\mathrm{Fe}_{2} \mathrm{O}_{3} \cdot \mathrm{FeO}\right)$ and contains both $\mathrm{Fe}^{2+}$ and $\mathrm{Fe}^{3+}$. Write the electron configurations of both cations of iron.

Crystal Wang

Numerade Educator

01:26

Problem 97

Which of the cations $\mathrm{Ga}^{4+}$ and $\mathrm{Mn}^{4+}$ is not a stable species? Why?

Crystal Wang

Numerade Educator

03:50

Problem 98

Rank the following ions in order of increasing sizes and increasing ionization energies: $\mathrm{S}^{2-}, \mathrm{K}^{+}, \mathrm{Ca}^{2+}$.

Crystal Wang

Numerade Educator

04:02

Problem 99

Arrange the elements lithium, carbon, and oxygen in order of
(a) increasing size.
(b) increasing first ionization energy.
(c) increasing second ionization energy.
(d) number of unpaired electrons.

Crystal Wang

Numerade Educator

01:02

Problem 100

Chlorine gas can be prepared by passing electricity through a solution of $\mathrm{NaCl}$. What volume of chlorine at standard temperature and pressure can be prepared from 2.44 g $\mathrm{NaCl} ?$

Crystal Wang

Numerade Educator

01:08

Problem 101

Write the electron configuration and orbital diagram for the noble gas that has a density of $1.62 \mathrm{~g} / \mathrm{L}$ at $27^{\circ} \mathrm{C}$ and 1.00 atm pressure.

Crystal Wang

Numerade Educator

01:18

Problem 102

Write the electron configuration of the alkali metal (M) that reacts with oxygen to yield an oxide, $\mathrm{M}_{2} \mathrm{O},$ if $1.22 \mathrm{~g}$ of the metal reacts with $1.41 \mathrm{~g}$ of oxygen to form $2.63 \mathrm{~g}$ of the oxide.

Crystal Wang

Numerade Educator

02:25

Problem 103

Write an equation for the reaction with water of a metal that, in its ground state, has one electron in a $3 s$ orbital. What mass of water is needed to react with $2.34 \mathrm{~g}$ of this metal?

Ashley Brady

Numerade Educator

03:10

Problem 104

What is the mass percent of a transition metal, $\mathrm{M},$ in a compound of the formula $\mathrm{MCl}_{3}$ if the electron configuration of the metal cation in this compound is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} ?$

Ashley Brady

Numerade Educator

01:46

Problem 105

What masses of iron and $\mathrm{Cl}_{2}$ are needed to prepare $7.88 \mathrm{~g}$ of the metal halide product if, under the conditions of the reaction, the electron configuration of the iron cation in the product is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{6} ?$

Crystal Wang

Numerade Educator

02:02

Problem 106

Given the following two equations, where the metals (M and $M^{\prime}$ ) are from the second period, what are the metals, and which metal cation in the product has a larger radius?
$$
\begin{array}{l}
2 \mathrm{M}+\mathrm{F}_{2} \rightarrow 2 \mathrm{MF} \\
\mathrm{M}^{\prime}+\mathrm{F}_{2} \rightarrow \mathrm{M}^{\prime} \mathrm{F}_{2}
\end{array}
$$

Ashley Brady

Numerade Educator