Introductory Chemistry

Stephen S. Zumdahl

Chapter 4

Chemical Foundations: Elements, Atoms, and Ions - all with Video Answers

Educators

Chapter Questions

Problem 1

The ancient Greeks believed that all matter was composed of four fundamental substances: earth, air, fire, and water. How does this early conception of matter compare with our modern theories about matter?

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Problem 2

Who was the first scientist generally accredited with putting the study of chemistry on a firm experimental basis?

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Problem 3

In addition to his important work on the properties of gases, what other valuable contributions did Robert Boyle make to the development of the study of chemistry?

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Problem 4

How many elements are presently known? How many of these elements occur naturally, and how many are synthesized artificially? What are the most common elements present on the earth?

Lottie Adams

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Problem 5

What is the most abundant element on the earth in terms of mass? Where are several places where this element is commonly found?

Dr. Satish Ingale

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Problem 6

What are the most abundant elements found in living creatures? Are these elements also the most abundant elements found in the nonliving world?

Cole Hogan

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Problem 7

The letters $C, S,$ and $T$ have been very popular when naming the elements, and there are ten or more elements whose names begin with each of these letters. Without looking in your textbook, see if you can list the symbol and name of five elements for each letter.

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Problem 8

In some cases, the symbol of an element does not seem to bear any relationship to the name we use for the element. Generally, the symbol for such an element is based on its name in another language. Give the symbols and names for five examples of such elements.

Cole Hogan

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Problem 9

Match the name in column 1 with the chemical symbol in column 2
Column 1
a. hydrogen
b. cobalt
c. potassium
d. bromine
e. barium
f. sulfur
g. silver
h. sodium
i. helium
¡. carbon
Column 2
1. He
2. $\mathrm{H}$
3. Na
4. So
5. $\mathrm{Ag}$
6. $\mathrm{S}$
7. B
8. Ba
9. Br
10. Co
11. C
12. $K$
13. Po
14. Ne

Dr. Satish Ingale

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Problem 10

Match the chemical symbol in column 1 with the name in column 2.
Column 1
a. $\mathrm{Al}$
b. Ne
C. Ni
d. $\mathrm{Si}$
e. $\mathrm{Cu}$
f. Fe
$g . F$
h. Au
1. $\mathrm{Zn}$
i. $U$
Column 2
1. silicon
2. gold
3. sulfur
4. aluminum
5. copper
6. neon
7. iron
8. silver
9. nickel
10. magnesium
11. barium
12. fluorine
13. uranium
14. zinc

Dr. Satish Ingale

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Problem 11

Use the periodic table inside the front cover of this book to look up the symbol or name for each of the following elements.

Dr. Satish Ingale

Dr. Satish Ingale

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Problem 12

Use the periodic table found inside the front cover of this book to look up the symbol or name for each of the following less common elements.

Dr. Satish Ingale

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Problem 13

For each of the following chemical symbols, give the name of the corresponding element.
a. $K$
b. $G e$
c. $P$
d. $C$
e. $\mathrm{N}$
f. $\mathrm{Na}$
g. Ne
h. I

Dr. Satish Ingale

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Problem 14

Several elements have chemical symbols beginning with the letter $B$. For each of the following chemical symbols, give the name of the corresponding element.
a. $\mathrm{Br}$
b. $\mathrm{B}$
c. $\mathrm{Be}$
d. $\mathrm{Bi}$
e. Ba

Dr. Satish Ingale

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Problem 15

Indicate whether each of the following statements is true or false. If a statement is false, correct the statement so that it becomes true.
a. Most materials occur in nature as pure substances.
b. A given compound usually contains the same relative number of atoms of its various elements.
c. Atoms are made up of tiny particles called molecules.

Cole Hogan

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Problem 16

State the main idea of the law of constant composition in your own words, using an example to illustrate your understanding of this important idea.

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Problem 17

What is a compound?

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Problem 18

A given compound always contains the same relative masses of its constituent elements. How is this related to the relative numbers of each kind of atom present?

Lottie Adams

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Problem 19

Write the formula for each of the following substances, listing the elements in the order given.
a. a molecule containing three carbon atoms and eight hydrogen atoms
b. a compound containing two nitrogen atoms for every oxygen atom
c. a compound containing half as many barium atoms as iodine atoms
d. a compound containing aluminum atoms and also three times as many chlorine atoms as there are aluminum atoms
e. a sugar whose molecules contain 12 carbon atoms,
22 hydrogen atoms, and 11 oxygen atoms
f. a compound that contains twice as many potassium atoms as carbon atoms, and three times as many oxygen atoms as carbon atoms

Dr. Satish Ingale

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Problem 20

Write the formula for each of the following substances, listing the elements in the order given.
a. a molecule containing six carbon atoms and six hydrogen atoms
b. a molecule containing two nitrogen atoms and four oxygen atoms
c. a compound containing half as many calcium atoms as chlorine atoms
d. a compound containing one iron atom for every three bromine atoms
e. a compound containing equal numbers of sodium and nitrogen atoms, but three times as many oxygen atoms as there are sodium atoms
f. a compound containing three calcium atoms for every two nitrogen atoms

Dr. Satish Ingale

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Problem 21

Scientists J. J. Thomson and William Thomson (Lord Kelvin) made numerous contributions to our understanding of the atom's structure.
a. What subatomic particle did J. J. Thomson discover, and what did this lead him to postulate about the nature of the atom?
b. William Thomson postulated what became known
as the "plum pudding" model of the atom's structure. What did this model suggest?

Natalie Britton

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Problem 22

Indicate whether each of the following statements is true or false. If false, correct the statement so that it becomes true.
a. Rutherford's bombardment experiments with metal foil suggested that the alpha particles were being deflected by coming near a large, negatively charged atomic nucleus.
b. The proton and the electron have similar masses but opposite electrical charges.
c. Most atoms also contain neutrons, which are slightly heavier than protons but carry no charge.

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Problem 23

Where are neutrons found in an atom? Are neutrons positively charged, negatively charged, or electrically uncharged?

Natalie Britton

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Problem 24

What two common types of particles are found in the nucleus of the atom? What are the relative charges of these particles? What are the relative masses of these particles?

Lottie Adams

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Problem 25

Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare to the mass of the electron? Which particles make the greatest contribution to the mass of an atom? Which particles make the greatest contribution to the chemical properties of an atom?

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Problem 26

The proton and the (electron/neutron) have almost equal masses. The proton and the (electron/neutron) have charges that are equal in magnitude but opposite in nature.

Lottie Adams

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Problem 27

An average atomic nucleus has a diameter of about___________$\mathrm{m}$.

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Problem 28

Which particles in an atom are most responsible for the chemical properties of the atom? Where are these particles located in the atom?

Lottie Adams

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Problem 29

Explain what do we mean when we say that a particular element consists of several isotopes?

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Problem 30

True or false? The mass number of a nucleus represents the number of protons in the nucleus.

Cole Hogan

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Problem 31

For an atom, the number of protons and electrons is (different/the same).

Dr. Satish Ingale

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Problem 32

The _________ number represents the sum of the number of protons and neutrons in a nucleus.

Dr. Satish Ingale

Dr. Satish Ingale

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Problem 33

Was Dalton's original atomic theory consistent with the discovery that many elements consist of several isotopes? Why or why not?

Dr. Satish Ingale

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Problem 34

Are all atoms of the same element identical? If not, how can they differ?

Lottie Adams

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Problem 35

For each of the following elements, use the periodic table on the inside cover of this book to write the element's atomic number.
a. $\mathrm{Ni}$
b. copper
c. Se
d. cadmium
e. $S$
f. silicon
g. $\mathrm{V}$
h. xenon

Dr. Satish Ingale

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Problem 36

For each of the following elements, use the periodic table on the inside cover of this book to write the element's atomic number.
a. Ge
b. zinc
c. Cr
d. tungsten
e. Sr
f. cobalt
g. Be
h. lithium

Dr. Satish Ingale

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Problem 37

Write the atomic symbol $\left(\frac{A}{Z} X\right)$ for each of the isotopes described below.
a. $Z=8,$ number of neutrons $=9$
b. the isotope of chlorine in which $A=37$
c. $Z=27, A=60$
d. number of protons $=26,$ number of neutrons $=$ 31
e. the isotope of I with a mass number of 131
f. $Z=3,$ number of neutrons $=4$

Dr. Satish Ingale

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Problem 38

Write the atomic symbol $\frac{A}{Z} \mathrm{X}$ for each of the isotopes described below.
a. number of protons $=27,$ number of neutrons $=$ 31
b. the isotope of boron with mass number 10
c. $Z=12, A=23$
d. atomic number $53,$ number of neutrons $=79$
e. $Z=9,$ number of neutrons $=10$
f. number of protons $=29,$ mass number 65

Dr. Satish Ingale

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Problem 39

How many protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, how many electrons are present?

Dr. Satish Ingale

Dr. Satish Ingale

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Problem 40

How many protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, how many electrons are present?

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Problem 41

Complete the following table.

Bryan Lynn

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Problem 42

Complete the following table.

Bryan Lynn

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Problem 43

On the basis of what property are the elements arranged in order on the periodic table? Why?

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Problem 44

In which direction on the periodic table, horizontal or vertical, are elements with similar chemical properties aligned? What are families of elements with similar chemical properties called?

Cole Hogan

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Problem 45

List the characteristic physical properties that distinguish the metallic elements from the nonmetallic elements.

Natalie Britton

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Problem 46

Where are the metallic elements found on the periodic table? Are there more metallic elements or nonmetallic elements?

Cole Hogan

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Problem 47

Most, but not all, metallic elements are solids under ordinary laboratory conditions. Which metallic elements are not solids?

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Problem 48

List five nonmetallic elements that exist as gaseous substances under ordinary conditions. Do any metallic elements ordinarily occur as gases?

Lottie Adams

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Problem 49

Under ordinary conditions, only a few pure elements occur as liquids. Give an example of a metallic and a nonmetallic element that ordinarily occur as liquids.

Natalie Britton

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Problem 50

What is a metalloid? Where are the metalloids found on the periodic table?

Lottie Adams

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Problem 51

Write the number and name (if any) of the group (family) to which each of the following elements belongs.
a. cesium
b. Ra
c. Rn
d. chlorine
e. strontium
f. $\mathrm{Xe}$
g. $\mathrm{Rb}$

Dr. Satish Ingale

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Problem 52

Write the number and name (if any) of the group (family) to which each of the following elements belongs.
a. $K$
b. aluminum
c. He
d. silicon
e. sulfur
f. Kr
g. selenium

Dr. Satish Ingale

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Problem 53

For each of the following elements, use the tables on the inside cover of this book to give the chemical symbol, atomic number, and group number of each element, and to specify whether each element is a metal, nonmetal, or metalloid.
a. strontium
b. iodine
c. silicon
d. cesium
e. sulfur

Courtney R

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Problem 54

For each of the following elements, use the tables on the inside cover of this book to give the chemical symbol, atomic number, and group number of each element, and to specify whether the element is a metal, nonmetal, or metalloid.
a. lithium
b. arsenic
c. radon
d. radium
e. germanium

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Problem 55

Most substances are composed of__________rather than elemental substances.

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Problem 56

Are most of the chemical elements found in nature in the elemental form or combined in compounds? Why?

Lottie Adams

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Problem 57

The noble gas present in relatively large concentrations in the atmosphere is ____________.

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Problem 58

Why are the elements of Group 8 referred to as the noble or inert gas elements?

Lottie Adams

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Problem 59

Molecules of nitrogen gas and oxygen gas are said to be __________ ,which means they consist of pairs of atoms.

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Problem 60

Give three examples of gaseous elements that exist as diatomic molecules. Give three examples of gaseous elements that exist as monatomic species.

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Problem 61

A simple way to generate elemental hydrogen gas is to pass ________ through water.

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Problem 62

If sodium chloride (table salt) is melted and then subjected to an electric current, elemental ___________ gas is produced, along with sodium metal.

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Problem 63

Most of the elements are solids at room temperature. Give three examples of elements that are liquids at room temperature, and three examples of elements that are gases at room temperature.

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Problem 64

The two most common elemental forms of carbon are graphite and ______________.

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Problem 65

An isolated atom has a net charge of__________.

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Problem 66

How are ions produced from an atom? Does the formation of a simple ion involve changes to the atom's nucleus?

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Problem 67

A simple ion with a $3+$ charge (for example, $\mathrm{Al}^{3+}$ ) A simple ion with a $3+$ charge (for example, $\mathrm{Al}^{3+}$ ) _________ electrons.

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Problem 68

An ion that contains more protons than electrons will be (positively/negatively) charged.

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Problem 69

Positive ions are called __________, whereas negative ions are called _________.

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Problem 70

Simple negative ions formed from single atoms are given names that end in ____________.

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Problem 71

Based on their location in the periodic table, give the symbols for three elements that would be expected to form positive ions in their reactions.

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Problem 72

The tendency to gain electrons is a fundamental property of the __________ elements.

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Problem 73

How many electrons are contained in each of the following ions?
a. $\mathrm{Fe}^{2+}$
b. $C a^{2+}$
c. $C O^{2+}$
d. $C O^{3+}$
e. $S^{2-}$
f. $C I^{-}$
g. $\mathrm{Cr}^{3+}$
h. $\mathrm{K}^{+}$

Dr. Satish Ingale

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Problem 74

Consider the following ions. For the positive ions listed, predict the formula of the simplest compound that would be expected to be formed between the given ion and the sulfide ion, $S^{2-}$. For the negative ions listed, predict the formula of the simplest compound that would be expected to be formed between the given ion and the aluminum ion, $\mathrm{Al}^{3+}$.
a. $\mathrm{Fe}^{3+}$
b. $\mathrm{Fe}^{2+}$
c. $\mathrm{O}^{2-}$
d. $I^{-}$
e. $R b^{+}$
f. $P^{3-}$
g. $\mathrm{Mn}^{2+}$
h. $S n^{4+}$

Dr. Satish Ingale

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Problem 75

For the following processes that show the formation of ions, use the periodic table to indicate the number of electrons and protons present in both the ion and the neutral atom from which the ion is made.a. $\mathrm{Ca} \rightarrow \mathrm{Ca}^{2+}+2 \mathrm{e}^{-}$
b. $P+3 e^{-} \rightarrow P^{3-}$
c. $\mathrm{Br}+\mathrm{e}^{-} \rightarrow \mathrm{Br}^{-}$
d. $\mathrm{Fe} \rightarrow \mathrm{Fe}^{3+}+3 \mathrm{e}^{-}$
e. $A l \rightarrow A l^{3+}+3 e^{-}$
f. $\mathrm{N}+3 \mathrm{e}^{-} \rightarrow \mathrm{N}^{3-}$

Dr. Satish Ingale

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Problem 76

For the following processes that show the formation of ions, fill in the number of electrons that must be lost or gained to complete the process.
a. $\mathrm{Co} \rightarrow \mathrm{Co}^{2+}+$ _________$-e$
b. $N+$__________ $\mathrm{e}^{-} \rightarrow \mathrm{N}^{3-}$
c. $\operatorname{Sn} \rightarrow \operatorname{Sn}^{2+}+$________$e^{-}$.
d. $\operatorname{sn} \rightarrow \operatorname{sn}^{4+}+$_________$e^{-}$.
e. $R b \rightarrow R b^{+}+$_______$e^{-}$.
e. $R b \rightarrow R b^{+}+$________$e^{-}$.
f. $S+$ __________ $\mathrm{e}^{-} \rightarrow \mathrm{S}^{2-}$

Dr. Satish Ingale

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Problem 77

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form.
a. 53
b. 38
c. 55
d. 88
e. 9
f. 13

Cole Hogan

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Problem 78

On the basis of its location in the periodic table, indicate what simple ion each of the following elements is most likely to form.
a. $\mathrm{T} 1(Z=81)$
b. Se $(Z=34)$
c. Ba $(Z=56)$
d. As $(Z=33)$
e. Fr $(Z=87)$
f. $\operatorname{Cs}(Z=55)$

Nicole Smina

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Problem 79

List some properties of a substance that would lead you to believe it consists of ions. How do these properties differ from those of nonionic compounds?

Natalie Britton

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Problem 80

Why does a solution of sodium chloride in water conduct an electric current, whereas a solution of sugar in water does not?

Lottie Adams

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Problem 81

Why does an ionic compound conduct an electric current when the compound is melted but not when it is in the solid state?

Natalie Britton

Natalie Britton

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Problem 82

Why must the total number of positive charges in an ionic compound equal the total number of negative charges?

Lottie Adams

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Problem 83

For the following pairs of ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simplest compound that the ions are most likely to form.
a. $\mathrm{Fe}^{3+}$ and $\mathrm{P}^{3-}$
b. $\mathrm{Fe}^{3+}$ and $\mathrm{S}^{2-}$
c. $\mathrm{Fe}^{3+}$ and $\mathrm{Cl}^{-}$
d. $\mathrm{Mg}^{2+}$ and $\mathrm{Cl}^{-}$
e. $\mathrm{Mg}^{2+}$ and $\mathrm{O}^{2-}$
f. $\mathrm{Mg}^{2+}$ and $\mathrm{N}^{3-}$
g. $\mathrm{Na}^{+}$ and $\mathrm{P}^{3-}$
h. $\mathrm{Na}^{+}$ and $\mathrm{S}^{2-}$

Cole Hogan

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Problem 84

For the following pairs of ions, use the concept that a chemical compound must have a net charge of zero to predict the simplest compound that the ions are most likely to form.
a. $\mathrm{Co}^{2+}$ and $\mathrm{O}^{2-}$
b. $C o^{3+}$ and $S^{2-}$
c. $A l^{3+}$ and $C l^{-}$
d. $\mathrm{Ba}^{2+}$ and $\mathrm{N}^{3-}$
e. $C a^{2+}$ and $C^{4-}$
f. $K^{+}$ and $N^{3-}$

Dr. Satish Ingale

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Problem 85

For each of the following elements, give the chemical symbol and atomic number.
a. astatine
b. xenon
c. radium
d. strontium
e. lead
f. selenium
g. argon
h. cesium

Dr. Satish Ingale

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Problem 86

Give the group number (if any) in the periodic table for the elements listed in problem $85 .$ If the group has a family name, give that name.

Lottie Adams

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Problem 87

List the names, symbols, and atomic numbers of the top four elements in Groups $1,2,6,$ and 7.

Lottie Adams

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Problem 88

List the names, symbols, and atomic numbers of the top four elements in Groups $3,5,$ and 8.

Dr. Satish Ingale

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Problem 89

What is the difference between the atomic number and the mass number of an element? Can atoms of two different elements have the same atomic number? Could they have the same mass number? Why or why not?

Natalie Britton

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Problem 90

Which subatomic particles contribute most to the atom's mass? Which subatomic particles determine the atom's chemical properties?

Lottie Adams

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Problem 91

Is it possible for the same two elements to form more than one compound? Is this consistent with Dalton's atomic theory? Give an example.

Natalie Britton

Natalie Britton

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Problem 92

Carbohydrates, a class of compounds containing the elements carbon, hydrogen, and oxygen, were originally thought to contain one water molecule $\left(\mathrm{H}_{2} \mathrm{O}\right)$ for each carbon atom present. The carbohydrate glucose contains six carbon atoms. Write a general formula showing the relative numbers of each type of atom present in glucose.

LJ

Lena Jake

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Problem 93

When iron rusts in moist air, the product is typically a mixture of two iron-oxygen compounds. In one compound, there is an equal number of iron and oxygen atoms. In the other compound, there are three oxygen atoms for every two iron atoms. Write the formulas for the two iron oxides.

Natalie Britton

Natalie Britton

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Problem 94

How many protons and neutrons are contained in the nucleus of each of the following atoms? For an atom of the element, how many electrons are present?
a. $\quad \frac{63}{29} \mathrm{Cu}$
b. $\frac{80}{35}$ Bi
c. $_{12}^{24} \mathrm{Mg}$

Dr. Satish Ingale

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Problem 95

Though the common isotope of aluminum has a mass number of $27,$ isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of $24,25,26,28,29,$ and $30 .$ How many neutrons are present in each of these isotopes? Why are they all considered aluminum atoms, even though they differ greatly in mass? Write the atomic symbol for each isotope.

Natalie Britton

Natalie Britton

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Problem 96

The principal goal of alchemists was to convert cheaper, more common metals into gold. Considering that gold had no particular practical uses (for example, it was too soft to be used for weapons), why do you think early civilizations placed such emphasis on the value of gold?

Lottie Adams

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Problem 97

How did Robert Boyle define an element?

Natalie Britton

Natalie Britton

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Problem 98

Give the chemical symbol for each of the following elements.
a. iodine
b. silicon
c. tungsten
d. iron
e. copper
f. cobalt

Dr. Satish Ingale

Dr. Satish Ingale

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Problem 99

Give the chemical symbol for each of the following elements.
a. calcium
b. potassium
c. cesium
d. lead
e. platinum
f. gold

Dr. Satish Ingale

Dr. Satish Ingale

Numerade Educator

Problem 100

Give the chemical symbol for each of the following elements.
a. bromine
b. bismuth
c. mercury
d. vanadium
e. fluorine
f. calcium

Dr. Satish Ingale

Dr. Satish Ingale

Numerade Educator

Problem 101

Give the chemical symbol for each of the following elements.
a. silver
b. aluminum
c. cadmium
d. antimony
e. tin
f. arsenic

Dr. Satish Ingale

Dr. Satish Ingale

Numerade Educator

Problem 102

For each of the following chemical symbols, give the name of the corresponding element.
a. Os
b. $\mathrm{zr}$
c. Rb
d. $R n$
e. $U$
f. Mn
g. $\mathrm{Ni}$
h. Br

Dr. Satish Ingale

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Problem 103

For each of the following chemical symbols, give the name of the corresponding element.
a. Te
b. $\mathrm{Pd}$
c. $\mathrm{Zn}$
d. $\mathrm{Si}$
e. $\mathrm{Cs}$
f. $\mathrm{Bi}$
g. F
h. $\mathrm{Ti}$

Lottie Adams

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Problem 104

Write the simplest formula for each of the following substances, listing the elements in the order given.
a. a molecule containing one carbon atom and two oxygen atoms.
b. a compound containing one aluminum atom for every three chlorine atoms.
c. perchloric acid, which contains one hydrogen atom, one chlorine atom, and four oxygen atoms.
d. a molecule containing one sulfur atom and six chlorine atoms.

Lottie Adams

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Problem 105

For each of the following atomic numbers, write the name and chemical symbol of the corresponding element. (Refer to Figure 4.11.)
a. 7
b. 10
c. 11
d. 28
e. 22
f. 18
g. 36
h. 54

Lottie Adams

Numerade Educator

Problem 106

Write the atomic symbol $(^{A}_{z} X)$ for each of the isotopes described below.
a. $Z=6,$ number of neutrons $=7$.
b. the isotope of carbon with a mass number of 13.
c. $Z=6, A=13$
d. $Z=19, A=44$
e. the isotope of calcium with a mass number of 41
f. the isotope with 19 protons and 16 neutrons

Dr. Satish Ingale

Dr. Satish Ingale

Numerade Educator