Introductory Chemistry

Steven S. Zumdahl, Donald J. DeCoste

Chapter 12 Chemical Bonding - all with Video Answers

Educators

Chapter Questions

04:07

Problem 1

In general terms, what is a chemical bond?

Ethan Brown

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01:39

Problem 2

The energy required to break a given chemical bond is called the

Lottie Adams

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01:41

Problem 3

What sorts of elements react to form ionic compounds?

Lottie Adams

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02:14

Problem 4

In general terms, what is a covalent bond?

Ethan Brown

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03:55

Problem 5

Describe the type of bonding that exists in the $\mathrm{Cl}_{2}(g)$ molecule. How does this type of bonding differ from that found in the $\mathrm{HCl}(g)$ molecule? How is it similar?

Ethan Brown

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03:35

Problem 6

Compare and contrast the bonding found in the $\mathrm{H}_{2}(g)$ and $\mathrm{HF}(g)$ molecules with that found in $\mathrm{NaF}(s)$.

Ethan Brown

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01:11

Problem 7

The relative ability of an atom in a molecule to attract electrons to itself is called the atom's __________

Lottie Adams

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01:35

Problem 8

What does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.

Lottie Adams

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01:20

Problem 9

A bond between atoms having a (small/large) difference in electronegativity will be ionic.

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01:09

Problem 10

What factor determines the relative level of nolarity of a nolar covalent bond?

Lottie Adams

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01:30

In each of the following groups, which element is the most electronegative? Which is the least electronegative?
a. $\mathrm{K}, \mathrm{Na}, \mathrm{H}$
b. $\mathrm{F}, \mathrm{Br}, \mathrm{Na}$
c. B , N , F

Lottie Adams

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01:54

Problem 12

In each of the following groups, which element is the most electronegative? Which is the least electronegative?
a. $\mathrm{Cs}, \mathrm{Ba}, \mathrm{At}$
b. Ba , Sr, Ra
c. $\mathrm{O}, \mathrm{Rb}, \mathrm{Mg}$

Lottie Adams

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01:37

Problem 13

On the basis of the electronegativity values given in Fig. 12.3 , indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent.
a. $\mathrm{O}-\mathrm{O}$
b. Al

Lottie Adams

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01:22

Problem 14

On the basis of the electronegativity values given in Fig. 12.3 , indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic.
a. $\mathrm{S}-\mathrm{S}$
b. $\mathrm{S}-\mathrm{H}$
c. $S-K$

Lottie Adams

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00:52

Problem 15

Which of the following molecules contain polar covalent bonds
a. water, $\mathrm{H}_{2} \mathrm{O}$
b. carbon monoxide, CO
c. fluorine, $\mathrm{F}_{2}$
d. nitrogen, $\mathrm{N}_{2}$

Lottie Adams

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02:15

Problem 16

Which of the following molecules contain polar covalent bonds?
a. phosphorus, $\mathrm{P}_{4}$
b. oxygen, $\mathrm{O}_{2}$
c. ozone, $\mathrm{O}_{3}$
d. hydrogen fluoride, HF

Arpit Gupta

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01:47

Problem 17

On the basis of the electronegativity values given in Fig. 12.3 , indicate which is the more polar bond in each of the following pairs.
a. $\mathrm{H}-\mathrm{F}$ or $\mathrm{H}-\mathrm{Cl}$
b. $\mathrm{H}-\mathrm{Cl}$ or $\mathrm{H}-\mathrm{I}$
c. $\mathrm{H}-\mathrm{Br}$ or $\mathrm{H}-\mathrm{Cl}$
d. $\mathrm{H}-\mathrm{I}$ or $\mathrm{H}-\mathrm{Br}$

Lottie Adams

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01:37

Problem 18

On the basis of the electronegativity values given in Fig. $12.3,$ indicate which is the more polar bond in each of the following pairs.
a. $\mathrm{O}-\mathrm{Cl}$ or $\mathrm{O}-\mathrm{Br}$
b. $\mathrm{N} \longrightarrow \mathrm{O}$ or $\mathrm{N}-\mathrm{F}$
c. $\mathrm{P}-\mathrm{S}$ or $\mathrm{P}-\mathrm{O}$
d. $\mathrm{H}-\mathrm{O}$ or $\mathrm{H}-\mathrm{N}$

Lottie Adams

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01:35

Problem 19

19. Which bond in each of the following pairs has the greater ionic character?
a. $\mathrm{Na}-\mathrm{F}$ or $\mathrm{Na}-\mathrm{I}$
b. $\mathrm{Ca}-\mathrm{S}$ or $\mathrm{Ca}-\mathrm{O}$
c. $\mathrm{Li}-\mathrm{Cl}$ or $\mathrm{Cs}-\mathrm{Cl}$
d. $\mathrm{Mg}-\mathrm{N}$ or $\mathrm{Mg}-\mathrm{P}$

Lottie Adams

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01:43

Problem 20

Which bond in each of the following pairs has less ionic character?
a. $\mathrm{Na}-\mathrm{O}$ or $\mathrm{Na}-\mathrm{N}$
b. $\mathrm{K}-\mathrm{S}$ or $\mathrm{K}-\mathrm{P}$
c. $\mathrm{Na}-\mathrm{Cl}$ or $\mathrm{K}-\mathrm{Cl}$
d. $\mathrm{Na}-\mathrm{Cl}$ or $\mathrm{Mg}-\mathrm{Cl}$

Lottie Adams

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01:36

Problem 21

What is a dipole moment? Give four examples of molecules that possess dipole moments, and draw the direction of the dipole as shown in Section 12.3 .

Lottie Adams

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01:32

Problem 22

Why is the presence of a dipole moment in the water molecule so important? What are some properties of water that are determined by its polarity?

Lottie Adams

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01:30

Problem 23

In each of the following diatomic molecules, which end of the molecule is negative relative to the other end?
a. hydrogen chloride, HCl
b. carbon monoxide, CO
c. bromine monofluoride, BrF

Lottie Adams

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01:10

Problem 24

In each of the following diatomic molecules, which end of the molecule is positive relative to the other end? a. hydrogen fluoride, HF
b. chlorine monofluoride, ClF
c. iodine monochloride, ICl
ach of th

Lottie Adams

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01:11

Problem 26

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative.
a. $C-F$
b. $\mathrm{Si}-\mathrm{C}$
c. $C-O$
d. $B-C$

Lottie Adams

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01:24

Problem 26

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative.
a. $\mathrm{S}-\mathrm{P}$
b. $\mathrm{S}-\mathrm{F}$
$\begin{array}{l}\text { c. S } & \text { Cl }\end{array}$
d. $\mathrm{S}-\mathrm{Br}$

Lottie Adams

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00:59

Problem 27

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative.
a. $\mathrm{Si}-\mathrm{H}$
b. $P-H$
d. $\mathrm{Cl}-\mathrm{H}$

Lottie Adams

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01:20

Problem 28

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative.
a. $\mathrm{H}-\mathrm{C}$
b. $\mathrm{N} \longrightarrow \mathrm{O}$
c. $\mathrm{N}-\mathrm{S}$
d. $\mathrm{N}-\mathrm{C}$

Lottie Adams

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02:13

Problem 29

What does it mean when we say that in forming bonds, atoms try to achieve an electron configuration analogous to a noble gas?

Ethan Brown

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04:48

Problem 30

The metallic elements lose electrons when reacting, and the resulting positive ions have an electron configuration analogous to the noble gas element.

Ethan Brown

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04:47

Problem 31

Nonmetals form negative ions by (losing/gaining) enough electrons to achieve the electron configuration of the next noble gas.

Ethan Brown

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09:54

Problem 32

Explain how the atoms in covalent molecules achieve electron configurations similar to those of the noble gases. How does this differ from the situation in ionic compounds?

Ethan Brown

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06:45

Problem 33

Which simple ion would each of the following elements be expected to form? What noble gas has an analogous electron configuration to each of the ions?
a. chlorine, $Z=17$
b. strontium, $Z=38$
c. oxygen, $Z=8$
d. rubidium, $Z=37$

Ethan Brown

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01:44

Problem 34

34. Which simple ion would each of the following elements be expected to form? Which noble gas has an analogous electron configuration to each of the ions?
a. bromine, $Z=35$
b. cesium, $Z=55$

Lottie Adams

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01:42

Problem 35

For each of the following numbers of electrons, give the formula of a positive ion that would have that number of electrons, and write the complete electron configuration for each ion.
a. 10 electrons
b. 2 electrons
c. 18 electrons
d. 36 electrons

Lottie Adams

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02:57

Problem 36

What is the expected ground-state electron configuration for $\mathrm{Te}^{2-}$ ?

Vasu Makani

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02:39

Problem 37

On the basis of their electron configurations, predict the formula of the simple binary ionic compounds likely to form when the following pairs of elements react with each other.
a. aluminum, Al, and sulfur, S
b. radium, $\mathrm{Ra}$, and oxygen, $\mathrm{O}$
c. calcium, Ca, and fluorine, $\mathrm{F}$
d. cesium, Cs , and nitrogen, $\mathrm{N}$
e. rubidium, $\mathrm{Rb}$, and phosphorus, $\mathrm{P}$

Lottie Adams

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01:28

Problem 38

Lottie Adams

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01:20

Problem 39

Name the noble gas atom that has the same electron configuration as each of the ions in the following compounds.

Lottie Adams

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01:33

Problem 40

Atoms form ions so as to achieve electron configurations similar to those of the noble gases. For the following pairs of noble gas configurations, give the formulas of two simple ionic compounds that would have comparable electron configurations.
a. [He] and [Ne]
b. $[\mathrm{Ne}]$ and $[\mathrm{Ne}]$
c. [He] and [Ar]
d. $[\mathrm{Ne}]$ and $[\mathrm{Ar}]$

Lottie Adams

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00:26

Problem 41

Is the formula we write for an ionic compound the molecular formula or the empirical formula? Why?

Lottie Adams

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02:12

Problem 42

Describe in general terms the structure of ionic solids such as $\mathrm{NaCl}$. How are the ions packed in the crystal?

Arpit Gupta

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00:23

Problem 43

Why are cations always smaller than the atoms from which they are formed?

Lottie Adams

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00:24

Problem 44

Why are anions always larger than the atoms from which they are formed?

Lottie Adams

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00:53

Problem 45

For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms of the electron structure of each species.
a. H or $\mathrm{H}^{-}$
b. $\mathrm{N}$ or $\mathrm{N}^{3-}$
c. Al or $\mathrm{Al}^{3+}$
d. F or Cl

Lottie Adams

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01:58

Problem 46

For each of the following pairs, indicate which species is larger. Explain your reasoning in terms of the electron structure of each species.
a. $\mathrm{Mg}^{2+}$ or $\mathrm{Mg}$
b. $\mathrm{Ca}^{2+}$ or $\mathrm{K}^{+}$
c. $\mathrm{Rb}^{+}$ or $\mathrm{Br}^{-}$
d. $\mathrm{Se}^{2-}$ or $\mathrm{Se}$

Lottie Adams

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00:49

Problem 47

For each of the following pairs, indicate which is smaller.
a. Fe or $\mathrm{Fe}^{3+}$
b. Cl or $\mathrm{Cl}^{-}$
c. $\mathrm{Al}^{3+}$ or $\mathrm{Na}^{+}$

Lottie Adams

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01:33

Problem 48

For each of the following pairs, indicate which is larger.
a. I or F
b. F or $\mathrm{F}^{-}$
c. $\mathrm{Na}^{+}$ or $\mathrm{F}^{-}$

Lottie Adams

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01:41

Problem 49

Why are the valence electrons of an atom the only electrons likely to be involved in bonding to other atoms?

Arpit Gupta

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01:22

Problem 50

Explain what the "duet" and "octet" rules are and how they are used to describe the arrangement of electrons in a molecule.

Lottie Adams

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01:52

Problem 51

What type of structure must each atom in a compound usually exhibit for the compound to be stable?

Lottie Adams

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02:39

Problem 52

When elements in the second and third periods occur in compounds, what number of electrons in the valence shell represents the most stable electron arrangement? Why?

Lottie Adams

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02:25

Problem 53

How many electrons are involved when two atoms in a molecule are connected by a "double bond"? Write the Lewis structure of a molecule containing a double bond.

Arpit Gupta

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00:44

Problem 54

What does it mean when two atoms in a molecule are connected by a "triple bond"? Write the Lewis structure of a molecule containing a triple bond.

Lottie Adams

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01:10

Problem 55

Write the simple Lewis structure for each of the following atoms.
a. I $(Z=53)$
b. $\mathrm{Al}(Z=13)$
c. Xe $(Z=54)$
d. $\operatorname{Sr}(Z=38)$

Lottie Adams

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01:00

Problem 56

Write the simple Lewis structure for each of the following atoms.
a. $\operatorname{Mg}(Z=12)$
b. $\operatorname{Br}(Z=35)$
c. $\mathrm{S}(Z=16)$
d. $\mathrm{Si}(Z=14)$

Lottie Adams

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01:23

Problem 57

Give the total number of valence electrons in each of the following molecules.
a. $\mathrm{N}_{2} \mathrm{O}$
b. $\mathrm{B}_{2} \mathrm{H}_{6}$
c. $\mathrm{C}_{3} \mathrm{H}_{8}$
d. $\mathrm{NCl}_{3}$

Lottie Adams

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01:28

Problem 58

Give the total number of valence electrons in each of the following molecules.
a. $\mathrm{B}_{2} \mathrm{O}_{3}$
b. $\mathrm{CO}_{2}$
c. $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}$
d. $\mathrm{NO}_{2}$

Lottie Adams

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01:36

Problem 59

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots.
a. $\mathrm{NBr}_{3}$
b. HF
c. CBr $_{4}$
d. $\mathrm{C}_{2} \mathrm{H}_{2}$

Lottie Adams

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01:02

Problem 60

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electrons pairs as lines and all nonbonding valence electron pairs as dots.
a. $\mathrm{H}_{2} \mathrm{~S}$
b. $\mathrm{SiF}_{4}$
c. $\mathrm{C}_{2} \mathrm{H}_{4}$
d. $\mathrm{C}_{3} \mathrm{H}_{8}$

Lottie Adams

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01:25

Problem 61

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots.
a. $\mathrm{C}_{2} \mathrm{H}_{6}$
b. $\mathrm{NF}_{3}$
c. $\mathrm{C}_{4} \mathrm{H}_{10}$
d. $\mathrm{SiCl}_{4}$

Lottie Adams

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01:55

Problem 62

Which of the following species exhibits resonance?
$\mathrm{CH}_{4}, \mathrm{OCl}_{2}, \mathrm{NO}_{2}^{-}, \mathrm{HCN}$ (is the central atom)

David Collins

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01:16

Problem 63

$\mathrm{B}$ The "Chemistry in Focus" segment Broccoli-Miracle Food? discusses the health benefits of eating broccoli and gives a Lewis structure for sulforaphane, a chemical in broccoli. Draw possible resonance structures for sulforaphane.

Lottie Adams

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00:56

Problem 64

The "Chemistry in Focus" segment Hiding Carbon Dioxide discusses attempts at sequestering (storing) underground $\mathrm{CO}_{2}$ produced at power plants so as to diminish the greenhouse effect. Draw all resonance structures of the $\mathrm{CO}_{2}$ molecule.

Lottie Adams

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05:41

Problem 65

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms.
a. sulfate ion, $\mathrm{SO}_{4}^{2-}$
b. phosphate ion, $\mathrm{PO}_{4}^{3-}$
c. sulfite ion, $\mathrm{SO}_{3}{ }^{2-}$

Arpit Gupta

Numerade Educator

01:52

Problem 66

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms.
a. chlorate ion, $\mathrm{ClO}_{3}^{-}$
b. peroxide ion, $\mathrm{O}_{2}^{2-}$
c. acetate ion, $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}$

Lottie Adams

Numerade Educator

01:14

Problem 67

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms.
a. chlorite ion, $\mathrm{ClO}_{2}^{-}$
b. perbromate ion, $\mathrm{BrO}_{4}^{-}$
c. cyanide ion, CN $^{-}$

Lottie Adams

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01:06

Problem 68

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms.
a. carbonate ion, $\mathrm{CO}_{3}^{2-}$
b. ammonium ion, $\mathrm{NH}_{4}^{+}$
c. hypochlorite ion, $\mathrm{ClO}^{-}$

Lottie Adams

Numerade Educator

01:10

Problem 69

What is the geometric structure of the water molecule? How many pairs of valence electrons are there on the oxygen atom in the water molecule? What is the approximate $\mathrm{H}-\mathrm{O}-\mathrm{H}$ bond angle in water?

Lottie Adams

Numerade Educator

02:45

Problem 70

What is the geometric structure of the ammonia molecule? How many pairs of electrons surround the nitrogen atom in $\mathrm{NH}_{3} ? \mathrm{What}$ is the approximate $\mathrm{H}-\mathrm{N}-\mathrm{H}$ bond angle in ammonia?

Arpit Gupta

Numerade Educator

01:26

Problem 71

What is the geometric structure of the boron trifluoride molecule, $\mathrm{BF}_{3}$ ? How many pairs of valence electrons are present on the boron atom in $\mathrm{BF}_{3}$ ? What are the approximate $\mathrm{F}-\mathrm{B}-\mathrm{F}$ bond angles in $\mathrm{BF}_{3} ?$

Lottie Adams

Numerade Educator

00:53

Problem 72

What is the geometric structure of the $\mathrm{SiF}_{4}$ molecule? How many pairs of valence electrons are present on the silicon atom of $\mathrm{SiF}_{4} ?$ What are the approximate $\mathrm{F}-\mathrm{Si}-\mathrm{F}$ bond angles in $\mathrm{SiF}_{4} ?$

Lottie Adams

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01:24

Problem 73

Why is the geometric structure of a molecule important, especially for biological molecules?

Arpit Gupta

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01:37

Problem 74

What general principles determine the molecular structure (shape) of a molecule?

Arpit Gupta

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01:31

Problem 75

How is the structure around a given atom related to repulsion between valence electron pairs on the atom?

Alyssa Iryami

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00:35

Problem 76

Why are all diatomic molecules linear, regardless of the number of valence electron pairs on the atoms involved?

Alyssa Iryami

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01:47

Problem 77

Although the valence electron pairs in ammonia have a tetrahedral arrangement, the overall geometric structure of the ammonia molecule is not described as being tetrahedral. Explain.

Alyssa Iryami

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02:55

Problem 78

Although both the $\mathrm{BF}_{3}$ and $\mathrm{NF}_{3}$ molecules contain the same number of atoms, the $\mathrm{BF}_{3}$ molecule is flat, whereas the $\mathrm{NF}_{3}$ molecule is trigonal pyramidal. Explain.

Alyssa Iryami

Numerade Educator

05:55

Problem 79

For the indicated atom in each of the following molecules or ions, give the number and arrangement of the electron pairs around that atom.
a. $\mathrm{As}$ in $\mathrm{AsO}_{4}^{3-}$
b. Se in $\mathrm{SeO}_{4}^{2-}$
c. $\mathrm{S}$ in $\mathrm{H}_{2} \mathrm{~S}$

Alyssa Iryami

Numerade Educator

02:23

Problem 80

For the indicated atom in each of the following molecules or ions, give the number and arrangement of the electron pairs around that atom.
a. $\mathrm{S}$ in $\mathrm{SO}_{3}^{2-}$
b. $\mathrm{S}$ in $\mathrm{HSO}_{3}^{-}$
c. $\mathrm{S}$ in $\mathrm{HS}^{-}$

Lottie Adams

Numerade Educator

03:03

Problem 81

Using the VSEPR theory, predict the molecular structure of each of the following molecules.
a. $\mathrm{NCl}_{3}$
b. $\mathrm{H}_{2} \mathrm{Se}$
c. $\mathrm{SiCl}_{4}$

Alyssa Iryami

Numerade Educator

01:56

Problem 82

Using the VSEPR theory, predict the molecular structure of each of the following molecules.
a. $\mathrm{CBr}_{4}$
b. $\mathrm{PH}_{3}$
c. $\mathrm{OCl}_{2}$

Lottie Adams

Numerade Educator

03:57

Problem 83

Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions.
a. sulfate ion, $\mathrm{SO}_{4}{ }^{2-}$
b. phosphate ion, $\mathrm{PO}_{4}^{3-}$
c. ammonium ion, $\mathrm{NH}_{4}^{+}$

Alyssa Iryami

Numerade Educator

03:59

Problem 84

Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions.
a. dihydrogen phosphate ion, $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$
b. perchlorate ion, $\mathrm{ClO}_{4}^{-}$
c. sulfite ion, $\mathrm{SO}_{3}^{2-}$

Alyssa Iryami

Numerade Educator

02:41

Problem 85

For each of the following molecules or ions, indicate the bond angle expected between the central atom and any two adjacent hydrogen atoms.
a. $\mathrm{H}_{2} \mathrm{O}$
b. $\mathrm{NH}_{3}$
c. $\mathrm{NH}_{4}^{+}$
d. $\mathrm{CH}_{4}$

Arpit Gupta

Numerade Educator

04:53

Problem 86

For each of the following molecules or ions, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms.
a. $\mathrm{Cl}_{2} \mathrm{O}$
b. $\mathrm{NCl}_{3}$
c. CCl $_{4}$
d. $\mathrm{C}_{2} \mathrm{Cl}_{4}$

Alyssa Iryami

Numerade Educator

01:36

Problem 87

The "Chemistry in Focus" segment Taste- It's the Structure That Counts discusses artificial sweeteners. What are the expected bond angles around the nitrogen atom in aspartame?
88. For each of the following molecules, predict both the molecular structure and bond angles around the central atom.
a. $\mathrm{SeS}_{2}$
b. $\mathrm{SeS}_{3}$
c. $\mathrm{SO}_{2}$
d. $\mathrm{CS}_{2}$

Lottie Adams

Numerade Educator

01:51

Problem 88

For each of the following molecules, predict both the molecular structure and bond angles around the central atom.
a. $\mathrm{SeS}_{2}$
b. $\mathrm{SeS}_{3}$
c. $\mathrm{SO}_{2}$
d. $\mathrm{CS}_{2}$

Lottie Adams

Numerade Educator

02:07

Problem 89

Consider the following order: $\mathrm{Li}<\mathrm{N}<\mathrm{F}$.
For which of the following properties does the order show the correct trend?
a. size
b. electronegativity
c. metallic character
d. number of unpaired electrons
e. More than one of the above properties (a-d) shows the correct trend.

David Collins

Numerade Educator

02:05

Problem 90

In ionic bonding,
a. the electrons are shared between the atoms.
b. the process of forming an ionic bond is highly endothermic overall.
c. the bonding that occurs is usually between two nonmetal atoms.
d. a noble gas configuration is formed for each element or ion.
e. At least two of the above statements are correct.

David Collins

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00:59

Problem 91

The geometric arrangement of electron pairs around a given atom is determined principally by the tendency to minimize between the electron pairs.

Alyssa Iryami

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01:38

Problem 92

Arrange the following bonds from the least polar to the most polar bond:
$$
\mathrm{C}-\mathrm{F}, \mathrm{Na}-\mathrm{F}, \mathrm{Ga}-\mathrm{F}, \mathrm{Si}-\mathrm{F}
$$

Nicole Smina

Numerade Educator

02:42

Problem 93

In each case, which of the following pairs of bonded elements forms the more polar bond?
a. $\mathrm{Br}-\mathrm{Cl}$ or $\mathrm{Br}-\mathrm{F}$
b. As $-\mathrm{S}$ or $\mathrm{As}-\mathrm{O}$
c. $\mathrm{Pb}-\mathrm{C}$ or $\mathrm{Pb}-\mathrm{Si}$

Alyssa Iryami

Numerade Educator

01:44

Problem 94

Which of the following statements is false concerning bonding?
Elements with extremely different electronegativities tend to form ionic bonds with each other.
b. In an $\mathrm{N}-\mathrm{O}$ bond, electron density is greater near the $\mathrm{O}$ atom.
c. An $\mathrm{N}-\mathrm{O}$ bond is an example of a polar covalent bond.
d. In general, chemical bonds form to minimize energy.
e. The bond in $\mathrm{KBr}$ is formed by sharing electrons.

David Collins

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01:02

Problem 95

$\mathrm{A}(\mathrm{n}) \quad$ chemical bond represents the equal sharing of a pair of electrons between two nuclei.

Lottie Adams

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01:21

Problem 96

For each of the following pairs of elements, identify which element would be expected to be more electronegative. It should not be necessary to look at a table of actual electronegativity values.
a. Be or Ba
b. $\mathrm{N}$ or $\mathrm{P}$
c. F or Cl

Alyssa Iryami

Numerade Educator

01:39

Problem 97

Alyssa Iryami

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01:24

Problem 98

Which of the following molecules contain polar covalent bonds?
a. carbon monoxide, CO
b. chlorine, $\mathrm{Cl}_{2}$
c. iodine monochloride, ICl
d. phosphorus, $\mathrm{P}_{4}$

Lottie Adams

Numerade Educator

03:21

Problem 99

On the basis of the electronegativity values given in Fig. $12.3,$ indicate which is the more polar bond in each of the following pairs.
a. $\mathrm{N}-\mathrm{P}$ or $\mathrm{N}-\mathrm{O}$
b. $\mathrm{N}-\mathrm{C}$ or $\mathrm{N}-\mathrm{O}$
c. $\mathrm{N}-\mathrm{S}$ or $\mathrm{N}-\mathrm{C}$
d. $\mathrm{N}-\mathrm{F}$ or $\mathrm{N}-\mathrm{S}$

Alyssa Iryami

Numerade Educator

00:55

Problem 100

The electrons involved in a $\mathrm{C}-\mathrm{F}$ bond could be considered
a. closer to C because carbon has a larger radius and thus exerts greater control over the shared electrons.
b. closer to F because fluorine has a higher electronegativity than carbon.
c. closer to C because carbon has a lower ionization energy than fluorine.
d. an inadequate model because the bond is ionic.
e. centrally located directly between the $\mathrm{C}$ and $\mathrm{F}$ because the electrons are shared.

Lottie Adams

Numerade Educator

01:19

Problem 101

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative.
a. $\mathrm{N}-\mathrm{Cl}$
b. $\mathrm{N}-\mathrm{P}$
c. $\mathrm{N}-\mathrm{S}$
d. $\mathrm{N}-\mathrm{C}$

Lottie Adams

Numerade Educator

01:36

Problem 102

Which of the following contains a metal ion that does not have a noble gas electron configuration?
$$
\mathrm{AgCl}, \mathrm{BaCl}_{2}, \mathrm{TiO}_{2}, \mathrm{ScF}_{3}, \mathrm{KNO}_{3}
$$

David Collins

Numerade Educator

01:56

Problem 103

What simple ion does each of the following elements most commonly form?
a. Sodium
b. iodine
c. potassium
d. calcium
e. sulfur
f. magnesium
g. aluminum
h. nitrogen

Alyssa Iryami

Numerade Educator

02:03

Problem 104

On the basis of their electron configurations, predict the formula of the simple binary ionic compound likely to form when the following pairs of elements react with each other.
a. sodium, $\mathrm{Na}$, and selenium, Se
b. rubidium, $\mathrm{Rb}$, and fluorine, $\mathrm{F}$
c. potassium, $\mathrm{K}$, and tellurium, Te
d. barium, $\mathrm{Ba}$, and selenium, Se
e. potassium, $\mathrm{K},$ and astatine, $\mathrm{At}$
f. francium, $\mathrm{Fr}$, and chlorine, $\mathrm{Cl}$

Lottie Adams

Numerade Educator

01:38

Problem 105

Which noble gas has the same electron configuration as each of the ions in the following compounds?
a. calcium bromide, $\mathrm{CaBr}_{2}$
b. aluminum selenide, $\mathrm{Al}_{2} \mathrm{Se}_{3}$
c. strontium oxide, $\mathrm{SrO}$
d. potassium sulfide, $\mathrm{K}_{2} \mathrm{~S}$

Lottie Adams

Numerade Educator

01:41

Problem 106

For each of the following pairs, indicate which is smaller.
a. $\mathrm{Rb}^{+}$ or $\mathrm{Na}^{+}$
b. $\mathrm{Mg}^{2+}$ or $\mathrm{Al}^{3+}$
c. $\mathrm{F}^{-}$ or $\mathrm{I}^{-}$
d. $\mathrm{Na}^{+}$ or $\mathrm{K}^{+}$

Lottie Adams

Numerade Educator

03:46

Problem 107

Write the Lewis structure for each of the following atoms.
a. He $(Z=2)$
b. Br $(Z=35)$
c. $\operatorname{Sr}(Z=38)$
d. Ne $(Z=10)$
e. I $(Z=53)$
f. $\operatorname{Ra}(Z=88)$

Dr. Satish Ingale

Numerade Educator

01:36

Problem 108

What is the total number of valence electrons in each of the following molecules?
a. $\mathrm{HNO}_{3}$
b. $\mathrm{H}_{2} \mathrm{SO}_{4}$
c. $\mathrm{H}_{3} \mathrm{PO}_{4}$
d. $\mathrm{HClO}_{4}$

Lottie Adams

Numerade Educator

01:50

Problem 109

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots.
a. $\mathrm{GeH}_{4}$
b. ICl
c. $\mathrm{NI}_{3}$
d. $\mathrm{PF}_{3}$

Lottie Adams

Numerade Educator

01:48

Problem 110

Select which of the following ions has the Lewis structure:
$$
[: \ddot{\mathrm{X}}-\ddot{\mathrm{X}}:\rfloor^{2-}
$$
a. $\mathrm{B}_{2}^{2-}$
b. $\mathrm{C}_{2}^{2-}$
c. $\mathrm{N}_{2}^{2-}$
d. $\mathrm{O}_{2}^{2-}$
e. $\mathrm{F}_{2}^{2-}$

David Collins

Numerade Educator

02:58

Problem 111

111. Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules that exhibit resonance, draw the various possible resonance forms.
a. $\mathrm{SO}_{2}$
b. $\mathrm{N}_{2} \mathrm{O}(\mathrm{N}$ in center $)$
c. $\mathrm{O}_{3}$

Lottie Adams

Numerade Educator

01:05

Problem 112

Chemicals placed in a microwave oven and exposed to microwave radiation can increase in temperature if they possess a net dipole moment. Which of the following molecules can get hot in an operating microwave oven?
$$
\mathrm{CCl}_{4}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HCl}, \mathrm{BH}_{3}, \mathrm{CO}_{2}
$$

Lottie Adams

Numerade Educator

01:11

Problem 113

Why is the molecular structure of $\mathrm{H}_{2} \mathrm{O}$ nonlinear, whereas that of $\mathrm{BeF}_{2}$ is linear, even though both molecules consist of three atoms?

Lottie Adams

Numerade Educator

01:52

Problem 114

For the indicated atom in each of the following molecules, give the number and the arrangement of the electron pairs around that atom.
a. $\mathrm{C}$ in $\mathrm{CCl}_{4}$
b. Ge in GeH $_{4}$
c. B in BF $_{3}$

Lottie Adams

Numerade Educator

02:00

Problem 115

Using the VSEPR theory, predict the molecular structure of each of the following molecules.
a. $\mathrm{Cl}_{2} \mathrm{O}$
b. $\mathrm{OF}_{2}$
c. $\mathrm{SiCl}_{4}$

Lottie Adams

Numerade Educator

03:00

Problem 116

Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions.
a. chlorate ion
b. chlorite ion
c. perchlorate ion

Lottie Adams

Numerade Educator

01:15

Problem 117

For each of the following molecules, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms.
a. $\mathrm{Cl}_{2} \mathrm{O}$
b. CCl $_{4}$
c. $\mathrm{BeCl}_{2}$

Lottie Adams

Numerade Educator

01:21

Problem 118

Using the VSEPR theory, predict the molecular structure of each of the following molecules or ions containing multiple bonds.
a. $\mathrm{SO}_{2}$
b. $\mathrm{SO}_{3}$
c. $\mathrm{HCO}_{3}^{-}$ (hydrogen is bonded to oxygen)
d. HCN

Arpit Gupta

Numerade Educator

01:23

Problem 119

Using the VSEPR theory, predict the molecular structure of each of the following molecules or ions containing multiple bonds.
a. $\mathrm{CO}_{3}^{2-}$
b. HNO $_{3}$ (hydrogen is bonded to oxygen)
c. $\mathrm{NO}_{2}^{-}$
d. $\mathrm{C}_{2} \mathrm{H}_{2}$

Lottie Adams

Numerade Educator

01:42

Problem 120

What is the expected ground-state electron configuration for the element with one unpaired $5 p$ electron that forms a covalent compound with fluorine?

Nicole Smina

Numerade Educator

02:03

Problem 121

Consider the following series of atoms or ions: $\mathrm{S}^{2-}, \mathrm{S}, \mathrm{S}^{2+}, \mathrm{Cs}^{+}, \mathrm{Sr}^{2+}$
a. Which of the species has the smallest size?
b. Which of the species has the largest ionization energy?

David Collins

Numerade Educator

01:36

Problem 122

Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar covalent.
a. $\mathrm{H}_{2}$
b. $\mathrm{K}_{3} \mathrm{P}$
c. NaI
d. $\mathrm{SO}_{2}$
e. HF
f. CCl
g. CF $_{4}$
h. $\mathrm{K}_{2} \mathrm{~S}$

Lottie Adams

Numerade Educator

01:21

Problem 123

Compare the electronegativities of each pair of atoms. State the element of each pair that has the greater electronegativity.

Lottie Adams

Numerade Educator

04:20

Problem 124

List the bonds $\mathrm{P}-\mathrm{Cl}, \mathrm{P}-\mathrm{F}, \mathrm{O}-\mathrm{F},$ and $\mathrm{Si}-\mathrm{F}$ from least polar to most polar.

Lena Jake

Numerade Educator

02:05

Problem 125

Arrange the atoms and/or ions in the following groups in order of decreasing size.
a. $\mathrm{O}, \mathrm{O}^{-}, \mathrm{O}^{2-}$
b. $\mathrm{Fe}^{2+}, \mathrm{Ni}^{2+}, \mathrm{Zn}^{2+}$
$\mathrm{c} \cdot \mathrm{Ca}^{2+}, \mathrm{K}^{+}, \mathrm{Cl}^{-}$

Lottie Adams

Numerade Educator

01:50

Problem 126

Write electron configurations for the most stable ion formed by each of the following elements. Do not use the noble gas notation. Write out the complete electron configuration.

Lottie Adams

Numerade Educator

01:02

Problem 127

Which of the following compounds or ions exhibit resonance?
a. $\mathrm{O}_{3}$
b. $\mathrm{CNO}^{-}$
c. AsI $_{3}$
d. $\mathrm{CO}_{3}^{2-}$
e. AsF $_{3}$

Lottie Adams

Numerade Educator

01:13

Problem 128

The formulas of several chemical substances are given in the table below. For each substance in the table, give its chemical name and predict its molecular structure.

Lottie Adams

Numerade Educator