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Chemistry

Paul Flowers, Klaus Theopold, Richard Langley

Chapter 7

Chemical Bonding and Molecular Geometry - all with Video Answers

Educators

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Chapter Questions

01:27

Problem 1

Does a cation gain protons to form a positive charge or does it lose electrons?

Linhan Yang
Linhan Yang
Numerade Educator
01:24

Problem 2

Iron(III) sulfate $\left[\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}\right]$ is composed of $\mathrm{Fe}^{3+}$ and $\mathrm{SO}_{4}^{2-}$ ions. Explain why a sample of iron(III) sulfate is uncharged.

Connor Hudson
Connor Hudson
Numerade Educator
03:22

Problem 3

Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions: $\mathrm{P}, \mathrm{I}, \mathrm{Mg}, \mathrm{Cl}, \mathrm{In}, \mathrm{Cs}, \mathrm{O}, \mathrm{Pb}, \mathrm{Co} ?$

Linhan Yang
Linhan Yang
Numerade Educator
00:50

Problem 4

Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions: Br, Ca, Na, N, F, Al, Sn, S, Cd?

Aadit Sharma
Aadit Sharma
Numerade Educator
05:40

Problem 5

Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:
(a) $\mathrm{P}$
(b) Mg
(c) Al
(d) O
(e) Cl
(f) Cs

Linhan Yang
Linhan Yang
Numerade Educator
01:14

Problem 6

Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds:
(a) I
(b) Sr
(c) K
(d) $\mathrm{N}$
(e) $\mathrm{S}$
(f) In

Aadit Sharma
Aadit Sharma
Numerade Educator
13:24

Problem 7

Write the electron configuration for each of the following ions:
(a) $\mathrm{As}^{3-}$
(b) I $^{-}$
(c) $\mathrm{Be}^{2+}$
(d) $\mathrm{Cd}^{2+}$
(e) $\mathrm{O}^{2-}$
(f) $\mathrm{Ga}^{3+}$
(g) $\mathrm{Li}^{+}$
(h) $\mathrm{N}^{3-}$
(i) $\mathrm{Sn}^{2+}$
(j) $\mathrm{Co}^{2+}$
(k) $\mathrm{Fe}^{2+}$
(l) $\mathrm{As}^{3+}$

Connor Hudson
Connor Hudson
Numerade Educator
02:51

Problem 8

Write the electron configuration for the monatomic ions formed from the following elements (which form the greatest concentration of monatomic ions in seawater):
(a) Cl
(b) $\mathrm{Na}$
(c) Mg
(d) Ca
(e) $K$
(f) Br
(g) Sr
(h) $\mathrm{F}$

Aadit Sharma
Aadit Sharma
Numerade Educator
11:40

Problem 9

Write out the full electron configuration for each of the following atoms and for the monatomic ion found in binary ionic compounds containing the element:
(a) Al
(b) Br
(c) Sr
(d) Li
(e) As
(f) $\mathrm{S}$

Anupa Sharad Medhekar
Anupa Sharad Medhekar
Numerade Educator
00:46

Problem 10

From the labels of several commercial products, prepare a list of six ionic compounds in the products. For each compound, write the formula. (You may need to look up some formulas in a suitable reference.)

Aadit Sharma
Aadit Sharma
Numerade Educator
01:23

Problem 11

Why is it incorrect to speak of a molecule of solid $\mathrm{NaCl}$ ?

Linhan Yang
Linhan Yang
Numerade Educator
01:13

Problem 12

What information can you use to predict whether a bond between two atoms is covalent or ionic?

Aadit Sharma
Aadit Sharma
Numerade Educator
06:19

Problem 13

Predict which of the following compounds are ionic and which are covalent, based on the location of their constituent atoms in the periodic table:
(a) $\mathrm{Cl}_{2} \mathrm{CO}$
(b) MnO
(c) $\mathrm{NCl}_{3}$
(d) CoBr $_{2}$
(e) $\mathrm{K}_{2} \mathrm{S}$
(f) CO
(g) $\mathrm{CaF}_{2}$
(h) HI
(i) CaO
(j) IBr
(k) $\mathrm{CO}_{2}$

Connor Hudson
Connor Hudson
Numerade Educator
00:48

Problem 14

Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond.

Aadit Sharma
Aadit Sharma
Numerade Educator
03:10

Problem 15

From its position in the periodic table, determine which atom in each pair is more electronegative:
(a) Br or Cl
(b) $\mathrm{N}$ or $\mathrm{O}$
(c) S or O
(d) $\mathrm{P}$ or $\mathrm{S}$
(e) Si or $\mathbf{N}$
(f) Ba or $P$
(g) N or K

Connor Hudson
Connor Hudson
Numerade Educator
02:23

Problem 16

From its position in the periodic table, determine which atom in each pair is more electronegative:
(a) $\mathrm{N}$ or $\mathrm{P}$
(b) $\mathrm{N}$ or $\mathrm{Ge}$
(c) S or F
(d) Cl or S
(e) $\mathrm{H}$ or $\mathrm{C}$
(f) Se or $P$
(g) C or Si

Aadit Sharma
Aadit Sharma
Numerade Educator
02:58

Problem 17

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity:
(a) $\mathrm{C}, \mathrm{F}, \mathrm{H}, \mathrm{N}, \mathrm{O}$
(b) $\mathrm{Br}, \mathrm{Cl}, \mathrm{F}, \mathrm{H}, \mathrm{I}$
(c) $\mathrm{F}, \mathrm{H}, \mathrm{O}, \mathrm{P}, \mathrm{S}$
(d) Al, H, Na, O, P
(e) $\mathrm{Ba}, \mathrm{H}, \mathrm{N}, \mathrm{O}, \mathrm{As}$

Linhan Yang
Linhan Yang
Numerade Educator
03:35

Problem 18

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity:
(a) $\mathrm{As}, \mathrm{H}, \mathrm{N}, \mathrm{P}, \mathrm{Sb}$
(b) Cl, H, P, S, Si
(c) $\mathrm{Br}, \mathrm{Cl}, \mathrm{Ge}, \mathrm{H}, \mathrm{Sr}$
(d) Ca, H, K, N, Si
(e) Cl, Cs, Ge, H, Sr

Aadit Sharma
Aadit Sharma
Numerade Educator
04:47

Problem 19

Which atoms can bond to sulfur so as to produce a positive partial charge on the sulfur atom?

Ronald Prasad
Ronald Prasad
Numerade Educator
01:39

Problem 20

Which is the most polar bond?
(a) $\mathrm{C}-\mathrm{C}$
(b) C-H
(c) $\mathrm{N}-\mathrm{H}$
(d) $\mathrm{O}-\mathrm{H}$
(e) $\mathrm{Se}-\mathrm{H}$

Connor Hudson
Connor Hudson
Numerade Educator
06:15

Problem 21

Identify the more polar bond in each of the following pairs of bonds:
(a) HF or HCl
(b) NO or CO
(c) SH or OH
(d) PCl or SCl
(e) CH or NH
(f) SO or PO
(g) CN or NN

Linhan Yang
Linhan Yang
Numerade Educator
04:30

Problem 22

Which of the following molecules or ions contain polar bonds?
(a) $\mathrm{O}_{3}$
(b) $\mathrm{S}_{8}$
(c) $\mathrm{O}_{2}^{2-}$
(d) $\mathrm{NO}_{3}^{-}$
(e) $\mathrm{CO}_{2}$
(f) $\mathrm{H}_{2} \mathrm{S}$
(g) $\mathrm{BH}_{4}^{-}$

Ian Lee
Ian Lee
Numerade Educator
03:30

Problem 23

Write the Lewis symbols for each of the following ions:
(a) $\mathrm{As}^{3-}$
(b) I $^{-}$
(c) $\mathrm{Be}^{2+}$
(d) $\mathrm{O}^{2-}$
(e) $\mathrm{Ga}^{3+}$
(f) $\mathrm{Li}^{+}$
(g) $\mathrm{N}^{3-}$

Connor Hudson
Connor Hudson
Numerade Educator
08:21

Problem 24

Many monatomic ions are found in seawater, including the ions formed from the following list of elements. Write the Lewis symbols for the monatomic ions formed from the following elements:
(a) Cl
(b) $\mathrm{Na}$
(c) Mg
(d) Ca
(e) K
(f) Br
(g) Sr
(h) $\mathrm{F}$

Shalini Tyagi
Shalini Tyagi
Numerade Educator
05:06

Problem 25

Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed:
(a) MgS
(b) $\mathrm{Al}_{2} \mathrm{O}_{3}$
(c) $\mathrm{GaCl}_{3}$
(d) $\mathrm{K}_{2} \mathrm{O}$
(e) $\mathrm{Li}_{3} \mathrm{N}$
(f) KF

Heath Mclean
Heath Mclean
Numerade Educator
02:42

Problem 26

In the Lewis structures listed here, $M$ and $X$ represent various elements in the third period of the periodic table. Write the formula of each compound using the chemical symbols of each element:

Cheryl Glor
Cheryl Glor
Numerade Educator
04:15

Problem 27

Write the Lewis structure for the diatomic molecule $P_{2}$, an unstable form of phosphorus found in high temperature phosphorus vapor.

Ian Lee
Ian Lee
Numerade Educator
06:17

Problem 28

Write Lewis structures for the following:
(a) $\mathrm{H}_{2}$
(b) HBr
(c) $\mathrm{PCl}_{3}$
(d) $\mathrm{SF}_{2}$
(e) $\mathrm{H}_{2} \mathrm{CCH}_{2}$
(f) HNNH
(g) $\mathrm{H}_{2} \mathrm{CNH}$
(h) $\mathrm{NO}^{-}$
(i) $\mathrm{N}_{2}$
(j) CO
(k) CN $^{-}$

Nicholas Sacco
Nicholas Sacco
Numerade Educator
07:23

Problem 29

Write Lewis structures for the following:
(a) $\mathrm{O}_{2}$
(b) $\mathrm{H}_{2} \mathrm{CO}$
(c) $\mathrm{AsF}_{3}$
(d) CINO
(e) $\operatorname{SiCl}_{4}$
(f) $\mathrm{H}_{3} \mathrm{O}^{+}$
(g) $\mathrm{NH}_{4}+$
(h) $\mathrm{BF}_{4}^{-}$
(i) HCCH
(j) CICN
(k) $\mathrm{C}_{2}^{2+}$

Nicholas Sacco
Nicholas Sacco
Numerade Educator
05:25

Problem 30

Write Lewis structures for the following:
(a) CIF $_{3}$
(b) $\mathrm{PCl}_{5}$
(c) $\mathrm{BF}_{3}$
(d) $\mathrm{PF}_{6}^{-}$

Ian Lee
Ian Lee
Numerade Educator
05:07

Problem 31

Write Lewis structures for the following:
(a) $\operatorname{Se} F_{6}$
(b) $\mathrm{XeF}_{4}$
(c) $\mathrm{SeCl}_{3}^{+}$
(d) $\mathrm{Cl}_{2} \mathrm{BBCl}_{2}$ (contains a B-B bond)

Heath Mclean
Heath Mclean
Numerade Educator
00:26

Problem 32

Write Lewis structures for:
(a) $\mathrm{PO}_{4}^{3-}$
(b) $\mathrm{ICl}_{4}^{-}$
(c) $\mathrm{SO}_{3}^{2-}$
(d) HONO

Aadit Sharma
Aadit Sharma
Numerade Educator
04:46

Problem 33

Correct the following statement: "The bonds in solid $\mathrm{PbCl}_{2}$ are ionic; the bond in a HCl molecule is covalent. Thus, all of the valence electrons in $\mathrm{PbCl}_{2}$ are located on the $\mathrm{Cl}^{-}$ ions, and all of the valence electrons in a $\mathrm{HCl}$ molecule are shared between the H and Cl atoms."

Heath Mclean
Heath Mclean
Numerade Educator
00:37

Problem 34

Write Lewis structures for the following molecules or ions:
(a) $\mathrm{SbH}_{3}$
(b) $\mathrm{XeF}_{2}$
(c) $\mathrm{Se}_{8}$ (a cyclic molecule with a ring of eight Se atoms)

Aadit Sharma
Aadit Sharma
Numerade Educator
09:21

Problem 35

=Methanol, H $_{3} \mathrm{COH}$, is used as the fuel in some race cars. Ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$, is used extensively as motor fuel in Brazil. Both methanol and ethanol produce $\mathrm{CO}_{2}$ and $\mathrm{H}_{2} \mathrm{O}$ when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

Heath Mclean
Heath Mclean
Numerade Educator
07:41

Problem 36

Many planets in our solar system contain organic chemicals including methane (CH $_{4}$ ) and traces of ethylene $\left(\mathrm{C}_{2} \mathrm{H}_{4}\right),$ ethane $\left(\mathrm{C}_{2} \mathrm{H}_{6}\right),$ propyne $\left(\mathrm{H}_{3} \mathrm{CCCH}\right),$ and diacetylene (HCCCCH). Write the Lewis structures for each of these molecules.

Heath Mclean
Heath Mclean
Numerade Educator
03:24

Problem 37

Carbon tetrachloride was formerly used in fire extinguishers for electrical fires. It is no longer used for this purpose because of the formation of the toxic gas phosgene, $\mathrm{Cl}_{2} \mathrm{CO}$. Write the Lewis structures for carbon tetrachloride and phosgene.

Heath Mclean
Heath Mclean
Numerade Educator
05:53

Problem 38

Identify the atoms that correspond to each of the following electron configurations. Then, write the Lewis symbol for the common ion formed from each atom:
(a) $1 s^{2} 2 s^{2} 2 p^{5}$
(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10}$
(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{4}$
(e) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{1}$

Connor Hudson
Connor Hudson
Numerade Educator
10:58

Problem 39

The arrangement of atoms in several biologically important molecules is given here. Complete the Lewis structures of these molecules by adding multiple bonds and lone pairs. Do not add any more atoms.
(a) the amino acid serine:
(b) urea:
(c) pyruvic acid:
(d) uracil:
(e) carbonic acid:

Linhan Yang
Linhan Yang
Numerade Educator
08:01

Problem 40

A compound with a molar mass of about 28 g/mol contains 85.7\% carbon and 14.3\% hydrogen by mass. Write the Lewis structure for a molecule of the compound.

Heath Mclean
Heath Mclean
Numerade Educator
07:08

Problem 41

A compound with a molar mass of about 42 g/mol contains 85.7\% carbon and 14.3\% hydrogen by mass. Write the Lewis structure for a molecule of the compound.

Heath Mclean
Heath Mclean
Numerade Educator
08:21

Problem 42

Two arrangements of atoms are possible for a compound with a molar mass of about $45 \mathrm{g} / \mathrm{mol}$ that contains 52.2\% C, 13.1\% H, and 34.7\% O by mass. Write the Lewis structures for the two molecules.

Heath Mclean
Heath Mclean
Numerade Educator
01:37

Problem 43

How are single, double, and triple bonds similar? How do they differ?

Linhan Yang
Linhan Yang
Numerade Educator
02:01

Problem 44

Write resonance forms that describe the distribution of electrons in each of these molecules or ions.
(a) selenium dioxide, OSeO
(b) nitrate ion, $\mathrm{NO}_{3}^{-}$
(c) nitric acid, HNO $_{3}$ (N is bonded to an OH group and two O atoms)
(d) benzene, $\mathrm{C}_{6} \mathrm{H}_{6}$ :
(e) the formate ion:

Crystal Wang
Crystal Wang
Numerade Educator
02:56

Problem 45

Write resonance forms that describe the distribution of electrons in each of these molecules or ions.
(a) sulfur dioxide, $\mathrm{SO}_{2}$
(b) carbonate ion, $\mathrm{CO}_{3}^{2-}$
(c) hydrogen carbonate ion, $\mathrm{HCO}_{3}^{-}$ (C is bonded to an OH group and two O atoms)
(d) pyridine:
(e) the allyl ion:

Crystal Wang
Crystal Wang
Numerade Educator
02:54

Problem 46

Write the resonance forms of ozone, $\mathrm{O}_{3}$, the component of the upper atmosphere that protects the Earth from ultraviolet radiation.

Ian Lee
Ian Lee
Numerade Educator
View

Problem 47

Sodium nitrite, which has been used to preserve bacon and other meats, is an ionic compound. Write the resonance forms of the nitrite ion, $\mathrm{NO}_{2}^{-}$

Heath Mclean
Heath Mclean
Numerade Educator
04:58

Problem 48

In terms of the bonds present, explain why acetic acid, $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$, contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbonoxygen bond. The skeleton structures of these species are shown:

Heath Mclean
Heath Mclean
Numerade Educator
06:44

Problem 49

Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.
(a) $\mathrm{CO}_{2}$
(b) CO

Heath Mclean
Heath Mclean
Numerade Educator
00:59

Problem 50

Toothpastes containing sodium hydrogen carbonate (sodium bicarbonate) and hydrogen peroxide are widely used. Write Lewis structures for the hydrogen carbonate ion and hydrogen peroxide molecule, with resonance forms where appropriate.

Aadit Sharma
Aadit Sharma
Numerade Educator
15:08

Problem 51

Determine the formal charge of each element in the following:
(a) HCl
(b) $\mathrm{CF}_{4}$
(c) $\mathrm{PCl}_{3}$
(d) $\mathrm{PF}_{5}$

Anupa Sharad Medhekar
Anupa Sharad Medhekar
Numerade Educator
02:22

Problem 52

Determine the formal charge of each element in the following:
(a) $\mathrm{H}_{3} \mathrm{O}^{+}$
(b) $\mathrm{SO}_{4}^{2-}$
(c) $\mathrm{NH}_{3}$
(d) $\mathrm{O}_{2}^{2-}$
(e) $\mathrm{H}_{2} \mathrm{O}_{2}$

Aadit Sharma
Aadit Sharma
Numerade Educator
02:13

Problem 53

Calculate the formal charge of chlorine in the molecules $\mathrm{Cl}_{2}, \mathrm{BeCl}_{2}$, and $\mathrm{ClF}_{5}$.

Ian Lee
Ian Lee
Numerade Educator
03:37

Problem 54

Calculate the formal charge of each element in the following compounds and ions:
(a) $\mathrm{F}_{2} \mathrm{CO}$
(b) $\mathrm{NO}^{-}$
(c) $\mathrm{BF}_{4}^{-}$
(d) $\operatorname{SnCl}_{3}^{-}$
(e) $\mathrm{H}_{2} \mathrm{CCH}_{2}$
(f) ClF $_{3}$
(g) $\operatorname{Se} F_{6}$
(h) $\mathrm{PO}_{4}^{3-}$

Crystal Wang
Crystal Wang
Numerade Educator
03:26

Problem 55

Draw all possible resonance structures for each of these compounds. Determine the formal charge on each ato in each of the resonance structures:
(a) $\mathrm{O}_{3}$
(b) $\mathrm{SO}_{2}$
(c) $\mathrm{NO}_{2}^{-}$
(d) $\mathrm{NO}_{3}^{-}$

Crystal Wang
Crystal Wang
Numerade Educator
01:11

Problem 56

Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in nitrosyl chloride: ClNO or ClON?

Aadit Sharma
Aadit Sharma
Numerade Educator
05:32

Problem 57

Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in hypochlorous acid: HOCl or OCIH?

Heath Mclean
Heath Mclean
Numerade Educator
00:58

Problem 58

Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in sulfur dioxide: OSO or SOO?

Aadit Sharma
Aadit Sharma
Numerade Educator
05:10

Problem 59

Draw the structure of hydroxylamine, $\mathrm{H}_{3} \mathrm{NO},$ and assign formal charges; look up the structure. Is the actual structure consistent with the formal charges?

Heath Mclean
Heath Mclean
Numerade Educator
08:47

Problem 60

Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule:
(a) IF
(b) IF $_{3}$
(c) IF $_{5}$
(d) IF $_{7}$

Heath Mclean
Heath Mclean
Numerade Educator
08:24

Problem 61

Write the Lewis structure and chemical formula of the compound with a molar mass of about $70 \mathrm{g} / \mathrm{mol}$ that contains $19.7 \%$ nitrogen and $80.3 \%$ fluorine by mass, and determine the formal charge of the atoms in this compound.

Heath Mclean
Heath Mclean
Numerade Educator
01:37

Problem 62

Which of the following structures would we expect for nitrous acid? Determine the formal charges:

Aadit Sharma
Aadit Sharma
Numerade Educator
05:48

Problem 63

Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion pounds are produced each year in the United States alone. Write the Lewis structure for sulfuric acid, $\mathrm{H}_{2} \mathrm{SO}_{4},$ which has two oxygen atoms and two OH groups bonded to the sulfur.

Heath Mclean
Heath Mclean
Numerade Educator
01:07

Problem 64

Which bond in each of the following pairs of bonds is the strongest?
(a) $\mathrm{C}-\mathrm{C}$ or $\mathrm{C}=\mathrm{C}$
(b) C-N or C $\equiv \mathrm{N}$
(c) $\mathrm{C} \equiv \mathrm{O}$ or $\mathrm{C}=\mathrm{O}$
(d) H-F or H-Cl
(e) $\mathrm{C}-\mathrm{H}$ or $\mathrm{O}-\mathrm{H}$
(f) C-N or C-O

Aadit Sharma
Aadit Sharma
Numerade Educator
04:23

Problem 65

Using the bond energies in Table $7.2,$ determine the approximate enthalpy change for each of the following reactions:
(a) $\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \longrightarrow 2 \mathrm{HBr}(g)$
(b) $\mathrm{CH}_{4}(g)+\mathrm{I}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{I}(g)+\mathrm{HI}(g)$
(c) $\mathrm{C}_{2} \mathrm{H}_{4}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$

Linhan Yang
Linhan Yang
Numerade Educator
01:44

Problem 66

Using the bond energies in Table $7.2,$ determine the approximate enthalpy change for each of the following reactions:
(a) $\mathrm{Cl}_{2}(g)+3 \mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{C} \operatorname{IF}_{3}(g)$
(b) $\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{H}_{3} \mathrm{CCH}_{3}(g)$
(c) $2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$

Aadit Sharma
Aadit Sharma
Numerade Educator
04:20

Problem 67

When a molecule can form two different structures, the structure with the stronger bonds is usually the more stable form. Use bond energies to predict the correct structure of the hydroxylamine molecule:

Anupa Sharad Medhekar
Anupa Sharad Medhekar
Numerade Educator
01:20

Problem 68

How does the bond energy of HCl( $g$ ) differ from the standard enthalpy of formation of $\mathrm{HCl}(g)$ ?

Aadit Sharma
Aadit Sharma
Numerade Educator
03:42

Problem 69

Using the standard enthalpy of formation data in Appendix G, show how the standard enthalpy of formation of $\mathrm{HCl}(g)$ can be used to determine the bond energy.

Linhan Yang
Linhan Yang
Numerade Educator
05:31

Problem 70

Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in $\mathrm{CS}_{2}$

Heath Mclean
Heath Mclean
Numerade Educator
09:10

Problem 71

Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the S-F bond in $\mathrm{SF}_{4}(g)$ or in $\mathrm{SF}_{6}(g) ?$

Heath Mclean
Heath Mclean
Numerade Educator
08:57

Problem 72

Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the P-Cl bond in $\mathrm{PCl}_{3}(g)$ or in $\mathrm{PCl}_{5}(g) ?$

Heath Mclean
Heath Mclean
Numerade Educator
01:41

Problem 73

Complete the following Lewis structure by adding bonds (not atoms), and then indicate the longest bond:

Linhan Yang
Linhan Yang
Numerade Educator
03:42

Problem 74

Use the bond energy to calculate an approximate value of $\Delta H$ for the following reaction. Which is the more stable form of FNO_?

Heath Mclean
Heath Mclean
Numerade Educator
08:37

Problem 75

Use principles of atomic structure to answer each of the following: $^{[1]}$
(a) The radius of the Ca atom is 197 pm; the radius of the $C a^{2+}$ ion is 99 pm. Account for the difference.
(b) The lattice energy of $\mathrm{CaO}(s)$ is $-3460 \mathrm{kJ} / \mathrm{mol}$; the lattice energy of $\mathrm{K}_{2} \mathrm{O}$ is $-2240 \mathrm{kJ} / \mathrm{mol}$. Account for the difference.
(c) Given these ionization values, explain the difference between $\mathrm{Ca}$ and $\mathrm{K}$ with regard to their first and second ionization energies.
(d) The first ionization energy of $\mathrm{Mg}$ is $738 \mathrm{kJ} / \mathrm{mol}$ and that of $\mathrm{Al}$ is $578 \mathrm{kJ} / \mathrm{mol}$. Account for this difference.

Heath Mclean
Heath Mclean
Numerade Educator
04:24

Problem 76

The lattice energy of LiF is 1023 kJ/mol, and the Li-F distance is 200.8 pm. NaF crystallizes in the same structure as LiF but with a Na-F distance of 231 pm. Which of the following values most closely approximates the lattice energy of NaF: 510, 890, 1023, 1175, or 4090 kJ/mol? Explain your choice.

Heath Mclean
Heath Mclean
Numerade Educator
02:04

Problem 77

For which of the following substances is the least energy required to convert one mole of the solid into separate ions?
(a) MgO
(b) SrO
(c) KF
(d) CsF
(e) $\mathrm{MgF}_{2}$

Linhan Yang
Linhan Yang
Numerade Educator
03:03

Problem 78

The reaction of a metal, M, with a halogen, $\mathrm{X}_{2}$, proceeds by an exothermic reaction as indicated by this equation: $\mathrm{M}(s)+\mathrm{X}_{2}(g) \longrightarrow \mathrm{M} \mathrm{X}_{2}(s) .$ For each of the following, indicate which option will make the reaction more exothermic. Explain your answers.
(a) a large radius vs. a small radius for $\mathrm{M}^{+2}$
(b) a high ionization energy vs. a low ionization energy for $M$
(c) an increasing bond energy for the halogen
(d) a decreasing electron affinity for the halogen
(e) an increasing size of the anion formed by the halogen

Crystal Wang
Crystal Wang
Numerade Educator
01:53

Problem 79

The lattice energy of LiF is 1023 kJ/mol, and the Li-F distance is 201 pm. MgO crystallizes in the same structure as LiF but with a Mg-O distance of 205 pm. Which of the following values most closely approximates the lattice energy of $\mathrm{MgO}: 256 \mathrm{kJ} / \mathrm{mol}, 512 \mathrm{kJ} / \mathrm{mol}, 1023 \mathrm{kJ} / \mathrm{mol}, 2046 \mathrm{kJ} / \mathrm{mol},$ or $4008 \mathrm{kJ} / \mathrm{mol} ?$ Explain your choice.

David Collins
David Collins
Numerade Educator
05:11

Problem 80

80. Which compound in each of the following pairs has the larger lattice energy? Note: $\mathrm{Mg}^{2+}$ and $\mathrm{Li}^{+}$ have similar radii; $\mathrm{O}^{2-} \text { and } \mathrm{F}^{-}$ have similar radii. Explain your choices.
(a) MgO or MgSe
(b) LiF or MgO
(c) $\mathrm{Li}_{2} \mathrm{O}$ or $\mathrm{LiCl}$
(d) Li_Se or MgO

Heath Mclean
Heath Mclean
Numerade Educator
04:13

Problem 81

Which compound in each of the following pairs has the larger lattice energy? Note: $\mathrm{Ba}^{2+}$ and K $^{+}$ have similar radii; $S^{2-}$ and $C l^{-}$ have similar radii. Explain your choices.
(a) $\mathrm{K}_{2} \mathrm{O}$ or $\mathrm{Na}_{2} \mathrm{O}$
(b) $\mathrm{K}_{2} \mathrm{S}$ or $\mathrm{BaS}$
(c) KCl or BaS
(d) BaS or BaCl

Heath Mclean
Heath Mclean
Numerade Educator
00:44

Problem 82

Which of the following compounds requires the most energy to convert one mole of the solid into separate ions?
(a) MgO
(b) SrO
(c) KF
(d) CsF
(e) $\mathrm{MgF}_{2}$

Crystal Wang
Crystal Wang
Numerade Educator
02:16

Problem 83

Which of the following compounds requires the most energy to convert one mole of the solid into separate ions?
(a) $\mathrm{K}_{2} \mathrm{S}$
(b) $\mathrm{K}_{2} \mathrm{O}$
(c) CaS
(d) $\mathrm{Cs}_{2} \mathrm{S}$
(e) CaO

Linhan Yang
Linhan Yang
Numerade Educator
03:55

Problem 84

The lattice energy of $\mathrm{KF}$ is $794 \mathrm{kJ} / \mathrm{mol}$, and the interionic distance is $269 \mathrm{pm}$. The $\mathrm{Na}-\mathrm{F}$ distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: $682 \mathrm{kJ} / \mathrm{mol}, 794 \mathrm{kJ} / \mathrm{mol}, 924 \mathrm{kJ} / \mathrm{mol}, 1588 \mathrm{kJ} / \mathrm{mol},$ or $3175 \mathrm{kJ} / \mathrm{mol} ?$
Explain your answer.

Heath Mclean
Heath Mclean
Numerade Educator
01:29

Problem 85

Explain why the HOH molecule is bent, whereas the HBeH molecule is linear.

Linhan Yang
Linhan Yang
Numerade Educator
03:34

Problem 86

What feature of a Lewis structure can be used to tell if a molecule's (or ion's) electron-pair geometry and molecular structure will be identical?

Heath Mclean
Heath Mclean
Numerade Educator
01:54

Problem 87

Explain the difference between electron-pair geometry and molecular structure.

Linhan Yang
Linhan Yang
Numerade Educator
04:51

Problem 88

Why is the H-N-H angle in $\mathrm{NH}_{3}$ smaller than the $\mathrm{H}-\mathrm{C}-\mathrm{H}$ bond angle in $\mathrm{CH}_{4}$ ? Why is the H-N-H angle in $\mathrm{NH}_{4}^{+}$ identical to the H-C-H bond angle in $\mathrm{CH}_{4}$ ?

Heath Mclean
Heath Mclean
Numerade Educator
01:09

Problem 89

Explain how a molecule that contains polar bonds can be nonpolar.

Linhan Yang
Linhan Yang
Numerade Educator
05:09

Problem 90

As a general rule, MX_nolecules (where M represents a central atom and X represents terminal atoms; $n=2$ 5) are polar if there is one or more lone pairs of electrons on $\mathrm{M} . \mathrm{NH}_{3}(\mathrm{M}=\mathrm{N}, \mathrm{X}=\mathrm{H}, \mathrm{n}=3$ ) is an example. There are two molecular structures with lone pairs that are exceptions to this rule. What are they?

Heath Mclean
Heath Mclean
Numerade Educator
07:00

Problem 91

Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:
(a) $\mathrm{SF}_{6}$
(b) $\mathrm{PCl}_{5}$
(c) $\mathrm{BeH}_{2}$
(d) $\mathrm{CH}_{3}^{+}$

Heath Mclean
Heath Mclean
Numerade Educator
02:49

Problem 92

Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:
(a) $\mathrm{IF}_{6}^{+}$
(b) $\mathrm{CF}_{4}$
(c) $\mathrm{BF}_{3}$
(d) $\mathrm{SiF}_{5}^{-}$
(e) $\mathrm{BeCl}_{2}$

Crystal Wang
Crystal Wang
Numerade Educator
05:05

Problem 93

Predict the electron pair geometry and the molecular structure of each of the following ions:
(a) ClF $_{5}$
(b) $\mathrm{ClO}_{2}^{-}$
(c) $\operatorname{Te} \mathrm{Cl}_{4}^{2-}$
(d) $\mathrm{PCl}_{3}$
(e) $\operatorname{Se} F_{4}$
(f) $\mathrm{PH}_{2}^{-}$

Crystal Wang
Crystal Wang
Numerade Educator
01:41

Problem 94

Predict the electron pair geometry and the molecular structure of each of the following ions:
(a) $\mathrm{H}_{3} \mathrm{O}^{+}$
(b) $\mathrm{PCl}_{4}^{-}$
(c) $\operatorname{sn} C \operatorname{l}_{3}-$
(d) $\mathrm{BrCl}_{4}^{-}$
(e) ICl $_{3}$
(f) $\mathrm{XeF}_{4}$
(g) $\mathrm{SF}_{2}$

Crystal Wang
Crystal Wang
Numerade Educator
09:29

Problem 95

Identify the electron pair geometry and the molecular structure of each of the following molecules:
(a) ClNO (N is the central atom)
(b) $\mathrm{CS}_{2}$
(c) $\mathrm{Cl}_{2} \mathrm{CO}$ (C is the central atom)
(d) $\mathrm{Cl}_{2} \mathrm{SO}$ (S is the central atom)
(e) $\mathrm{SO}_{2} \mathrm{F}_{2}$ (S is the central atom)
(f) $\mathrm{XeO}_{2} \mathrm{F}_{2}$ (Xe is the central atom)
(g) $\mathrm{ClOF}_{2}^{+}$ (Cl is the central atom)

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
03:39

Problem 96

Predict the electron pair geometry and the molecular structure of each of the following:
(a) IOF $_{5}$ (I is the central atom)
(b) $\mathrm{POCl}_{3}$ (P is the central atom)
(c) $\mathrm{Cl}_{2} \mathrm{SeO}$ (Se is the central atom)
(d) $\mathrm{ClSO}^{+}$ (S is the central atom)
(e) $\mathrm{F}_{2} \mathrm{SO}$ (S is the central atom)
(f) $\mathrm{NO}_{2}^{-}$
(g) $\operatorname{SiO}_{4}^{4-}$

Crystal Wang
Crystal Wang
Numerade Educator
05:54

Problem 97

Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?
(a) ClF $_{5}$
(b) $\mathrm{ClO}_{2}$
(c) $\operatorname{Te} \mathrm{Cl}_{4}^{2-}$
(d) $\mathrm{PCl}_{3}$
(e) $\operatorname{Se} F_{4}$
(f) $\mathrm{PH}_{2}^{-}$
(g) $\mathrm{XeF}_{2}$

Crystal Wang
Crystal Wang
Numerade Educator
01:39

Problem 98

Which of these molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?
(a) $\mathrm{H}_{3} \mathrm{O}^{+}$
(b) $\mathrm{PCl}_{4}^{-}$
(c) $\operatorname{sn} C l_{3}^{-}$
(d) $\mathrm{BrCl}_{4}^{-}$
(e) ICl $_{3}$
(f) $\mathrm{XeF}_{4}$
(g) $\mathrm{SF}_{2}$

Cheryl Glor
Cheryl Glor
Numerade Educator
10:33

Problem 99

Which of the following molecules have dipole moments?
(a) $\mathrm{CS}_{2}$
(b) $\operatorname{Se} S_{2}$
(c) $\mathrm{CCl}_{2} \mathrm{F}_{2}$
(d) $\mathrm{PCl}_{3}$ (P is the central atom)
(e) ClNO (N is the central atom)

Heath Mclean
Heath Mclean
Numerade Educator
01:53

Problem 100

Identify the molecules with a dipole moment:
(a) $\mathrm{SF}_{4}$
(b) $\mathrm{CF}_{4}$
(c) $\mathrm{Cl}_{2} \mathrm{CCBr}_{2}$
(d) $\mathrm{CH}_{3} \mathrm{Cl}$
(e) $\mathrm{H}_{2} \mathrm{CO}$

Aadit Sharma
Aadit Sharma
Numerade Educator
01:56

Problem 101

The molecule XF $_{3}$ has a dipole moment. Is X boron or phosphorus?

Arun Bana
Arun Bana
Numerade Educator
03:48

Problem 102

The molecule XCl_ has a dipole moment. Is X beryllium or sulfur?

Heath Mclean
Heath Mclean
Numerade Educator
01:33

Problem 103

Is the $\mathrm{Cl}_{2} \mathrm{BBCl}_{2}$ molecule polar or nonpolar?

Linhan Yang
Linhan Yang
Numerade Educator
03:40

Problem 104

There are three possible structures for $\mathrm{PCl}_{2} \mathrm{F}_{3}$ with phosphorus as the central atom. Draw them and discuss how measurements of dipole moments could help distinguish among them.

Heath Mclean
Heath Mclean
Numerade Educator
02:52

Problem 105

Describe the molecular structure around the indicated atom or atoms:
(a) the sulfur atom in sulfuric acid, $\mathrm{H}_{2} \mathrm{SO}_{4}\left[(\mathrm{HO})_{2} \mathrm{SO}_{2}\right]$
(b) the chlorine atom in chloric acid, $\mathrm{HClO}_{3}\left[\mathrm{HOClO}_{2}\right]$
(c) the oxygen atom in hydrogen peroxide, HOOH
(d) the nitrogen atom in nitric acid, $\mathrm{HNO}_{3}\left[\mathrm{HONO}_{2}\right]$
(e) the oxygen atom in the OH group in nitric acid, $\mathrm{HNO}_{3}\left[\mathrm{HONO}_{2}\right]$
(f) the central oxygen atom in the ozone molecule, $\mathrm{O}_{3}$
(g) each of the carbon atoms in propyne, $\mathrm{CH}_{3} \mathrm{CCH}$
(h) the carbon atom in Freon, $\mathrm{CCl}_{2} \mathrm{F}_{2}$
(i) each of the carbon atoms in allene, $\mathrm{H}_{2} \mathrm{CCCH}_{2}$

Crystal Wang
Crystal Wang
Numerade Educator
01:45

Problem 106

Draw the Lewis structures and predict the shape of each compound or ion:
(a) $\mathrm{CO}_{2}$
(b) $\mathrm{NO}_{2}^{-}$
(c) $\mathrm{SO}_{3}$
(d) $\mathrm{SO}_{3}^{2-}$

Aadit Sharma
Aadit Sharma
Numerade Educator
05:08

Problem 107

A molecule with the formula $\mathrm{AB}_{2}$, in which $\mathrm{A}$ and $\mathrm{B}$ represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion for each shape.

Heath Mclean
Heath Mclean
Numerade Educator
03:38

Problem 108

A molecule with the formula $\mathrm{AB}_{3}$, in which $\mathrm{A}$ and $\mathrm{B}$ represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion that has each shape.

Heath Mclean
Heath Mclean
Numerade Educator
04:51

Problem 109

Draw the Lewis electron dot structures for these molecules, including resonance structures where appropriate:
(a) $\mathrm{CS}_{3}^{2-}$
(b) $\mathrm{CS}_{2}$
(c) CS
(d) predict the molecular shapes for $\mathrm{CS}_{3}^{2-}$ and $\mathrm{CS}_{2}$ and explain how you arrived at your predictions

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
00:39

Problem 110

What is the molecular structure of the stable form of $\mathrm{FNO}_{2}$ ? ( $\mathrm{N}$ is the central atom.)

Aadit Sharma
Aadit Sharma
Numerade Educator
07:03

Problem 111

A compound with a molar mass of about 42 g/mol contains 85.7\% carbon and 14.3\% hydrogen. What is its molecular structure?

Heath Mclean
Heath Mclean
Numerade Educator
04:22

Problem 112

Use the simulation (http://openstaxcollege.org/I/16MolecPolarity) to perform the following exercises for a two-atom molecule:
(a) Adjust the electronegativity value so the bond dipole is pointing toward $\mathrm{B}$. Then determine what the electronegativity values must be to switch the dipole so that it points toward A.
(b) With a partial positive charge on $A$, turn on the electric field and describe what happens.
(c) With a small partial negative charge on A, turn on the electric field and describe what happens.
(d) Reset all, and then with a large partial negative charge on $\mathrm{A}$, turn on the electric field and describe what happens.

Jennifer Hudspeth
Jennifer Hudspeth
Numerade Educator
01:39

Problem 113

Use the simulation (http:Ilopenstaxcollege.org/I/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles.
(a) Sketch the bond dipoles and molecular dipole (if any) for $\mathrm{O}_{3}$. Explain your observations.
(b) Look at the bond dipoles for $\mathrm{NH}_{3}$. Use these dipoles to predict whether $\mathrm{N}$ or $\mathrm{H}$ is more electronegative.
(c) Predict whether there should be a molecular dipole for $\mathrm{NH}_{3}$ and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

Crystal Wang
Crystal Wang
Numerade Educator
02:42

Problem 114

Use the Molecule Shape simulator (http:/lopenstaxcollege.org/l/16MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.

Crystal Wang
Crystal Wang
Numerade Educator
01:59

Problem 115

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select H_0. Switch between the "real" and "model" modes. Explain the difference observed.

Crystal Wang
Crystal Wang
Numerade Educator
01:12

Problem 116

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select "model" mode and S_0. What is the model bond angle? Explain whether the "real" bond angle should be larger or smaller than the ideal model angle.

Crystal Wang
Crystal Wang
Numerade Educator