Chemistry Matter and Change

Problem 7

Explain how an ionic compound forms from these elements.
sodium and nitrogen

Ronald Prasad

Numerade Educator

00:52

Problem 8

Explain how an ionic compound forms from these elements.
lithium and oxygen

Erwin Ni

Numerade Educator

01:07

Problem 9

Explain how an ionic compound forms from these elements.
strontium and fluorine

David Collins

Numerade Educator

01:15

Problem 10

Explain how an ionic compound forms from these elements.
aluminum and sulfur

Erwin Ni

Numerade Educator

Problem 11

Challenge Explain how elements
in the two groups shown on the
periodic table at the right combine
to form an ionic compound.

David Collins

Numerade Educator

00:26

Problem 12

Explain how an ionic compound made up of charged particles can
be electrically neutral.

Erwin Ni

Numerade Educator

00:26

Problem 13

Describe the energy change associated with ionic bond formation, and relate it
to stability.

Amy Jiang

Numerade Educator

02:18

Problem 14

Identify three physical properties of ionic compounds that are associated with
ionic bonds, and relate them to bond strength.

Rebecca Wallace

Numerade Educator

01:30

Problem 15

Explain how ions form bonds, and describe the structure of the resulting
compound.

David Collins

Numerade Educator

00:47

Problem 16

Relate lattice energy to ionic-bond strength.

Erwin Ni

Numerade Educator

Problem 17

Apply Use electron configurations, orbital notation, and electron-dot structures
to represent the formation of an ionic compound from the metal strontium and
the nonmetal chlorine.

Miguel Perez

Numerade Educator

05:58

Problem 18

Design a concept map that shows the relationships among ionic bond strength,
physical properties of ionic compounds, lattice energy, and stability.

Caroline Basil

Numerade Educator

01:09

Problem 19

Write formulas for the ionic compounds formed by the following ions.
potassium and iodide

David Collins

Numerade Educator

00:35

Problem 20

Write formulas for the ionic compounds formed by the following ions.
magnesium and chloride

Erwin Ni

Numerade Educator

01:11

Problem 21

Write formulas for the ionic compounds formed by the following ions.
aluminum and bromide

David Collins

Numerade Educator

00:31

Problem 22

Write formulas for the ionic compounds formed by the following ions.
cesium and nitride

Erwin Ni

Numerade Educator

00:48

Problem 23

Challenge Write the general formula
for the ionic compound formed by
elements from the two groups shown
on the periodic table at the right.

Amy Jiang

Numerade Educator

00:27

Problem 24

Write formulas for ionic compounds composed of the following ions.
sodium and nitrate

Erwin Ni

Numerade Educator

01:24

Problem 25

Write formulas for ionic compounds composed of the following ions.
calcium and chlorate

David Collins

Numerade Educator

00:37

Problem 26

Write formulas for ionic compounds composed of the following ions.
aluminum and carbonate

Erwin Ni

Numerade Educator

Problem 27

Challenge Write the formula for an ionic compound formed by ions from a group 2
element and polyatomic ions composed of only carbon and oxygen.

David Collins

Numerade Educator

00:32

Problem 28

Name the following compounds.
NaBr

Erwin Ni

Numerade Educator

01:06

Problem 29

Name the following compounds.
$\mathrm{CaCl}_{2}$

David Collins

Numerade Educator

00:36

Problem 30

Name the following compounds.
$\mathrm{KOH}$

Erwin Ni

Numerade Educator

01:09

Problem 31

Name the following compounds.
$\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}$

David Collins

Numerade Educator

00:42

Problem 32

Name the following compounds.
$\mathrm{Ag}_{2} \mathrm{CrO}_{4}$

Erwin Ni

Numerade Educator

00:33

Problem 33

Challenge The ionic compound $\mathrm{NH}_{4} \mathrm{ClO}_{4}$ is a key reactant used in
solid rocket boosters, such as those that power the Space Shuttle into
orbit. Name this compound.

Amy Jiang

Numerade Educator

02:26

Problem 34

State the order in which the ions associated with a compound
composed of potassium and bromine would be written in the chemical formula
and the compound name.

Rebecca Wallace

Numerade Educator

Problem 35

Describe the difference between a monatomic ion and a polyatomic ion, and
give an example of each.

David Collins

Numerade Educator

00:42

Problem 36

Apply lon $X$ has a charge of $2+,$ and ion $Y$ has a charge of $1-.$ Write the
formula unit of the compound formed from the ions.

Erwin Ni

Numerade Educator

01:31

Problem 37

State the name and formula for the compound formed from Mg and Cl.

David Collins

Numerade Educator

00:43

Problem 38

Write the name and formula for the compound formed from sodium ions and
nitrite ions.

Erwin Ni

Numerade Educator

02:08

Problem 39

Analyze What subscripts would you most likely use if the following substances
formed an ionic compound?
a. an alkali metal and a halogen
b. an alkali metal and a nonmetal from group 16
c. an alkaline earth metal and a halogen
d. an alkaline earth metal and a nonmetal from group 16

Jia Lu

Numerade Educator

02:14

Problem 40

Contrast the structures of ionic compounds and metals.

Rebecca Wallace

Numerade Educator

01:09

Problem 41

Explain how the conductivity of electricity and the high boiling points of metals
are explained by metallic bonding.

David Collins

Numerade Educator

Problem 42

Contrast the cause of the attraction in ionic bonds and metallic bonds.

Rebecca Wallace

Numerade Educator

Problem 43

Summarize alloy types by correctly pairing these terms and phrases: substitutional, interstitial, replaced, and filled in.

David Collins

Numerade Educator

02:40

Problem 44

Design an experiment that could be used to distinguish between a metallic
solid and an ionic solide at least two different methods for comparing the
solids. Explain your reasoning.

Rebecca Wallace

Numerade Educator

Problem 45

Model Draw a model to represent the physical property of metals known as
ductility, or the ability to be drawn into a wire. Base your drawing on the electron
sea model shown in Figure $7.11 .$

Rebecca Wallace

Numerade Educator

00:48

Problem 46

How do positive ions and negative ions form?

Erwin Ni

Numerade Educator

01:25

Problem 47

When do chemical bonds form?

David Collins

Numerade Educator

00:53

Problem 48

Why are halogens and alkali metals likely to form ions?
Explain your answer.

Erwin Ni

Numerade Educator

01:37

Problem 49

The periodic table shown in Figure 7.14 contains elements
labeled $A-G .$ For each labeled element, state the
number of valence electrons and identify the ion that
will form.

David Collins

Numerade Educator

01:26

Problem 50

Discuss the importance of electron affinity and ionization energy in the formation of ions.

Rebecca Wallace

Numerade Educator

01:04

Problem 51

The orbital notation of sulfur is shown in Figure 7.15.
Explain how sulfur forms its ion.

David Collins

Numerade Educator

02:53

Problem 52

Give the number of valence electrons in an atom of
each element.
$\begin{array}{ll}{\text { a. cesium }} & {\text { d. zinc }} \\ {\text { b. rubidium }} & {\text { e. strontium }} \\ {\text { c. gallium }}\end{array}$

Rebecca Wallace

Numerade Educator

01:06

Problem 53

Explain why noble gases are not likely to form chemical
bonds.

David Collins

Numerade Educator

00:24

Problem 54

Discuss the formation of the barium ion.

Erwin Ni

Numerade Educator

01:07

Problem 55

Explain how an anion of nitrogen forms.

David Collins

Numerade Educator

00:52

Problem 56

The more reactive an atom, the higher its potential
energy. Which atom has higher potential energy,
neon or fluorine? Explain.

Erwin Ni

Numerade Educator

02:11

Problem 57

Explain how the iron atom can form both an iron $2+$
ion and an iron $3+$ ion.

Amy Jiang

Numerade Educator

01:14

Problem 58

Predict the reactivity of each atom based on its electron
configuration.
a. potassium $\quad$ b. fluorine $\quad$ c. neon

Erwin Ni

Numerade Educator

01:02

Problem 59

Discuss the formation of a $3+$ scandium ion using its
orbital notation, shown in Figure $7.16 .$

Amy Jiang

Numerade Educator

01:36

Problem 60

What does the term electrically neutral mean when
discussing ionic compounds?

Rebecca Wallace

Numerade Educator

01:24

Problem 61

Discuss the formation of ionic bonds.

David Collins

Numerade Educator

00:10

Problem 62

Explain why potassium does not bond with neon to
form a compound.

Erwin Ni

Numerade Educator

01:13

Problem 63

Briefly discuss three physical properties of ionic solids
that are linked to ionic bonds.

David Collins

Numerade Educator

00:49

Problem 64

Describe an ionic crystal, and explain why ionic crystals
for different compounds might vary in shape.

Rebecca Wallace

Numerade Educator

Problem 65

How does lattice energy change with a change in the size
of an ion?

David Collins

Numerade Educator

00:34

Problem 66

In Figure 7.14 , the element labeled $B$ is barium, and the
element labeled $E$ is iodine. Explain why the compound
formed between these elements will not be BaI.

Erwin Ni

Numerade Educator

01:28

Problem 67

Determine the ratio of cations to anions in each.
a. potassium chloride, a salt substitute
b. calcium fluoride, used in the steel industry
c. calcium oxide, used to remove sulfur dioxide from power-plant exhaust
d. strontium chloride, used in fireworks

David Collins

Numerade Educator

01:41

Problem 68

Look at Figure $7.14 ;$ describe the ionic compound that
form from the elements represented by $\mathrm{C}$ and $\mathrm{D}$ .

Rebecca Wallace

Numerade Educator

01:24

Problem 69

Discuss the formation of an ionic bond between zinc
and oxygen.

David Collins

Numerade Educator

02:03

Problem 70

Using orbital notation, diagram the formation of an
ionic bond between aluminum and fluorine.

Rebecca Wallace

Numerade Educator

01:08

Problem 71

Using electron configurations, diagram the formation of
an ionic bond between barium and nitrogen.

David Collins

Numerade Educator

02:11

Problem 72

Conductors Under certain conditions, ionic compounds conduct an electric current. Describe these conditions, and explain why ionic compounds are not always used as conductors.

Rebecca Wallace

Numerade Educator

01:22

Problem 73

Which compounds are not likely to occur: CaKr, $\mathrm{Na}_{2}$S,
$\mathrm{BaCl}_{3}, \mathrm{MgF}$ ? Explain your choices.

David Collins

Numerade Educator

01:41

Problem 74

Use Table 7.6 dettermine which ionic compound has
the highest melting point: MgO, KI, or AgCl. Explain
your answer.

Erwin Ni

Numerade Educator

03:23

Problem 75

Which has the greater lattice energy, CsCl or KCl? $\mathrm{K}_{2} \mathrm{O}$
or CaO? Explain your choices.

Amy Jiang

Numerade Educator

00:47

Problem 76

What information do you need to write a correct chemical formula to represent an ionic compound?

Rebecca Wallace

Numerade Educator

01:26

Problem 77

When are subscripts used in formulas for ionic
compounds?

David Collins

Numerade Educator

02:58

Problem 78

Discuss how an ionic compound is named.

Rebecca Wallace

Numerade Educator

Problem 79

Using oxidation numbers, explain why the formula $\mathrm{NaF}_{2}$
is incorrect.

David Collins

Numerade Educator

00:50

Problem 80

Explain what the name scandium(III) oxide means
in terms of electrons lost and gained, and identify
the correct formula.

Rebecca Wallace

Numerade Educator

Problem 81

Give the formula for each ionic compound.
a. calcium iodide
b. silver(I) bromide
c. copper (II) chloride
d. potassium periodate
e. silver(I) acetate

David Collins

Numerade Educator

02:27

Problem 82

Name each of the following ionic compounds.
$$
\begin{array}{l}{\text { a. } \mathrm{K}_{2} \mathrm{O}} \\ {\text { b. } \mathrm{CaCl}_{2}} \\ {\text { c. } \mathrm{Mg}_{3} \mathrm{N}_{2}} \\ {\text { d. } \mathrm{NaClO}_{2}} \\ {\text { e. } \mathrm{KNO}_{3}}\end{array}
$$

Erwin Ni

Numerade Educator

01:54

Problem 83

Complete Table 7.14 by placing the symbols, formulas,
and names in the blanks.

Amy Jiang

Numerade Educator

01:32

Problem 84

Chrome Chromium, a transition metal used in chrome
plating, forms both the $C r^{2+}$ and $C r^{3+}$ ions. Write the
formulas for the ionic compounds formed when each of
these ions react with fluorine and oxygen ions.

Rebecca Wallace

Numerade Educator

01:25

Problem 85

Which are correct formulas for ionic compounds? For
those that are not correct, give the correct formula and
justify your answer.
$$
\begin{array}{ll}{\text { a. AlCl }} & {\text { c. BaOH }_{2}} \\ {\text { b. } \mathrm{Na}_{3} \mathrm{SO}_{4}} & {\text { d. } \mathrm{Fe}_{2} \mathrm{O}}\end{array}
$$

David Collins

Numerade Educator

04:15

Problem 86

Write the formulas for all of the ionic compounds that
can be formed by combining each of the cations with
each of the anions listed in Table $7.15 .$ Name each
compound formed.

Rebecca Wallace

Numerade Educator

01:12

Problem 87

Describe a metallic bond.

David Collins

Numerade Educator

00:57

Problem 88

Briefly explain why metallic alloys are made.

Erwin Ni

Numerade Educator

01:42

Problem 89

Briefly describe how malleability and ductility of metals
are explained by metallic bonding.

David Collins

Numerade Educator

01:05

Problem 90

Compare and contrast the two types of metal alloys.

Erwin Ni

Numerade Educator

Problem 91

Explain how a metallic bond is similar to an ionic bond.

David Collins

Numerade Educator

00:37

Problem 92

Brass Copper and zinc are used to form brass, an alloy.
Briefly explain why these two metals form a substitutional alloy and not an interstitial alloy.

Erwin Ni

Numerade Educator

Problem 93

How is a metallic bond different from an ionic bond?

David Collins

Numerade Educator

00:41

Problem 94

Silver Briefly explain why silver is a good conductor of
electricity.

Rebecca Wallace

Numerade Educator

01:31

Problem 95

Steel Briefly explain why steel, an alloy of iron, is used
to build the supporting structure of many buildings.

David Collins

Numerade Educator

01:14

Problem 96

The melting point of beryllium is $1287^{\circ} \mathrm{C}$ , while that of
lithium is $180^{\circ} \mathrm{C}$ . Explain the large difference in values.

Rebecca Wallace

Numerade Educator

01:15

Problem 97

Titanium has a boiling point of $3287^{\circ} \mathrm{C}$ , and copper has
a boiling point of $2567^{\circ} \mathrm{C}$ . Explain why there is a difference in the boiling points of these two metals.

David Collins

Numerade Educator

Problem 98

Alloys Describe the difference between the metal alloy
sterling silver and carbon steel in terms of the types of
alloys involved.

Erwin Ni

Numerade Educator

01:23

Problem 99

Give the number of valence electrons for atoms of oxygen, sulfur, arsenic, phosphorus, and bromine.

David Collins

Numerade Educator

00:26

Problem 100

Explain why calcium can form a $\mathrm{Ca}^{2+}$ ion but not a
$\mathrm{Ca}^{3+}$ ion.

Erwin Ni

Numerade Educator

01:45

Problem 101

Which ionic compounds would have the greatest
lattice energy: NaCl, KCl, or MgCl $_{2} ?$ Explain your
answer.

Amy Jiang

Numerade Educator

02:55

Problem 102

Give the formula for each ionic compound.
a. sodium sulfide
b. iron $(\mathrm{III})$ chloride
c. sodium sulfate
d. calcium phosphate
e. zinc nitrate

Erwin Ni

Numerade Educator

01:19

Problem 103

Cobalt, a transition metal, forms both the $\mathrm{Co}^{2+}$ and
$\mathrm{Co}^{3+}$ ions. Write the correct formulas, and give the
name for the oxides formed by the two different ions.

Amy Jiang

Numerade Educator

02:14

Problem 104

Complete Table 7.16.

Rebecca Wallace

Numerade Educator

01:01

Problem 105

Gold Briefly explain why gold can be used both in jewelry and as a conductor in electronic devices.

Amy Jiang

Numerade Educator

00:50

Problem 106

Discuss the formation of the nickel ion with a $2+$ oxidation number.

Rebecca Wallace

Numerade Educator

00:40

Problem 107

Compare the oxyanions sulfate and sulfite.

Amy Jiang

Numerade Educator

00:33

Problem 108

Using electron-dot structures, diagram the formation of
an ionic bond between potassium and iodine.

Erwin Ni

Numerade Educator

00:48

Problem 109

Magnesium forms both an oxide and a nitride when
burned in air. Discuss the formation of magnesium
oxide and magnesium nitride when magnesium atoms
react with oxygen and nitrogen atoms.

Amy Jiang

Numerade Educator

01:55

Problem 110

An external force easily deforms sodium metal, while
sodium chloride shatters when the same amount of
force is applied. Why do these two solids behave so
differently?

Rebecca Wallace

Numerade Educator

01:13

Problem 111

Name each ionic compound.
a. $\mathrm{CaO}$
b. BaS
c. AlPO $_{4}$
d. $\operatorname{Ba}(\mathrm{OH})_{2}$
e. $\operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}$

Amy Jiang

Numerade Educator

05:22

Problem 112

Design a concept map to explain the physical properties
of both ionic compounds and metallic solids.

Shazia Naz

Numerade Educator

02:23

Problem 113

Predict which solid in each pair will have the higher
melting point. Explain your answers.
$$
\begin{array}{l}{\text { a. } \mathrm{NaCl} \text { or } \mathrm{CsCl}} \\ {\text { b. Ag or } \mathrm{Cu}} \\ {\text { c. } \mathrm{Na}_{2} \mathrm{O} \text { or } \mathrm{MgO}}\end{array}
$$

Amy Jiang

Numerade Educator

00:22

Problem 114

Compare and contrast cations and anions.

Erwin Ni

Numerade Educator

03:47

Problem 115

Observe and Infer Identify the mistakes in the incorrect formulas and formula names, and design a flowchart to prevent the mistakes.
$$
\begin{array}{ll}{\text { a. copper acetate }} & {\text { d. disodium oxide }} \\ {\text { b. } \operatorname{Mg}_{2} \mathrm{O}_{2}} & {\text { e. } \mathrm{Al}_{2} \mathrm{SO}_{43}} \\ {\text { c. } \mathrm{Pb}_{2} \mathrm{O}_{5}}\end{array}
$$

Amy Jiang

Numerade Educator

Problem 116

Apply Examine the ions in the beaker shown in
Figure 7.17 . Identify two compounds that could form
using the available ions, and explain why this is possible.

Susan Hallstrom

Numerade Educator

00:50

Problem 117

Apply Praseodymium is a lanthanide element that
reacts with hydrochloric acid, forming
praseodymium (III) chloride. It also reacts with nitric
acid, forming praseodymium(II) nitrate.
Praseodymium has the electron configuration
$[\mathrm{Xe}] 4 \mathrm{f}^{3} 6 \mathrm{s}^{2}$
a. Examine the electron configuration, and explain how
praseodymium forms a $3+$ ion.
b. Write the correct formulas for both compounds
formed by praseodymium.

Amy Jiang

Numerade Educator

01:25

Problem 118

Hypothesize Look at the locations of potassium and
calcium on the periodic table. Form a hypothesis to
explain why the melting point of calcium is considerably
higher than the melting point of potassium.

Rebecca Wallace

Numerade Educator

00:42

Problem 119

Assess Explain why the term delocalized is an appropriate term for the electrons involved in metallic bonding.

Amy Jiang

Numerade Educator

01:20

Problem 120

Apply All uncharged atoms have valence electrons.
Explain why elements such as iodine and
sulfur do not have metallic bonds.

Rebecca Wallace

Numerade Educator

00:29

Problem 121

Analyze Explain why lattice energy is a negative
quantity.

Amy Jiang

Numerade Educator

02:03

Problem 122

Ionic Compounds Chrysoberyl is a transparent or
translucent mineral that is sometimes opalescent. It is
composed of beryllium aluminum oxide, BeAl. $\mathrm{O}_{4}$ .
Identify the oxidation numbers of each of the ions found
in this compound. Explain the formation of this ionic
compound.

Rebecca Wallace

Numerade Educator

01:04

Problem 123

You are given a liquid of unknown density. The mass of
a graduated cylinder containing 2.00 $\mathrm{mL}$ of the liquid is
34.68 $\mathrm{g} .$ The mass of the empty graduated cylinder is
30.00 $\mathrm{g} .$ Given this information, determine the density
of the liquid. (Chapter 2$)$

Amy Jiang

Numerade Educator

02:19

Problem 124

In the laboratory, students used a balance and a graduated cylinder to collect the data shown in Table 7.17 . Calculate the density of the sample. If the accepted value
of this sample is 7.01 $\mathrm{g} / \mathrm{mL}$ , calculate the percent error.
(Chapter 2$)$

Rebecca Wallace

Numerade Educator

02:31

Problem 125

A mercury atom drops in energy from $1.413 \times 10^{-18} \mathrm{J}$
to $1.069 \times 10^{-18} \mathrm{J.(Chapter} 5 )$
a. What is the energy of the photon emitted by the
mercury atom?
b. What is the frequency of the photon emitted by the
mercury atom?
c. What is the wavelength of the photon emitted by the
mercury atom?

Amy Jiang

Numerade Educator

02:56

Problem 126

Which element has the greater ionization energy, chlorine or carbon? (Chapter 6$)$

Rebecca Wallace

Numerade Educator

01:05

Problem 127

Compare and contrast the ways in which metals and
nonmetals form ions, and explain why they are different.
(Chapter 6$)$

Amy Jiang

Numerade Educator

00:57

Problem 128

What are transition elements? (Chapter 6$)$

Erwin Ni

Numerade Educator

Problem 129

Write the symbol and name of the element that fits each
description. (Chapter 6$)$
a. the second-lightest of the halogens
b. the metalloid with the lowest period number
c. the only group 16 element that is a gas at room temperature
d. the heaviest of the noble gases
e. the group 15 nonmetal that is a solid at room temperature

Amy Jiang

Numerade Educator

01:57

Problem 130

Free Radicals Many researchers believe that free
radicals are responsible for the effects of aging and
cancer. Research free radicals, and write about the
cause and what can be done to prevent free radicals.

Rebecca Wallace

Numerade Educator

00:33

Problem 131

Growing Crystals Crystals of ionic compounds can
be easily grown in the laboratory setting.
Research the growth of crystals, and design an experiment to grow a crystal in the laboratory.

Amy Jiang

Numerade Educator