Deck 3: Atoms, Molecules, and Ions

Question 1

Which of the following atoms contains the largest number of neutrons?

A) ${ } _ { 20 } ^ { 42 } \mathrm { Ca }$
B) ${ } _ { 19 } ^ { 39 } \mathrm {~K}$
C) ${ } _ { 17 } ^ { 37 } \mathrm { Cl }$
D) ${ } _ { 19 } ^ { 41 } \mathrm {~K}$
E) ${ } _ { 18 } ^ { 42 } \mathrm { Ar }$

Answer 1

${ } _ { 18 } ^ { 42 } \mathrm { Ar }$

Question 2

How many protons, neutrons, and electrons are present in an atom of iron-59?

A) 26 protons, 33 neutrons, and 59 electrons
B) 26 protons, 33 neutrons, and 33 electrons
C) 26 protons, 33 neutrons, and 26 electrons
D) 59 protons, 26 neutrons, and 59 electrons
E) 59 protons, 26 neutrons, and 26 electrons

Answer 2

26 protons, 33 neutrons, and 26 electrons

Question 3

What is the mass number of an atom of argon with 22 neutrons?

A) 2
B) 18
C) 22
D) 40
E) 44

Answer 3

40

Question 4

A neutral atom of an isotope ²⁰⁰Hg contains _____.

A) 200 neutrons and 280 electrons
B) 80 protons and 200 neutrons
C) 200 protons and 120 electrons
D) 200 protons, 80 neutrons, and 200 electrons
E) 80 protons and 120 neutrons

Question 5

Which of the following atoms contains more protons than neutrons?

A) ${ } _ { 1 } ^ { 1 } \mathrm { H }$
B) ${ } _ { 9 } ^ { 19 } \mathrm {~F}$
C) ${ } _ { 16 } ^ { 34 } \mathrm {~S}$
D) ${ } _ { 12 } ^ { 24 } \mathrm { Mg }$
E) ${ } _ { 2 } ^ { 4 } \mathrm { He }$

Question 6

What is the mass of chlorine-35 relative to carbon-12?

A) 0.657
B) 0.522
C) 1.52
D) 2.92
E) 23

Question 7

Which of the following atoms contains the least protons?

A) ²³²Th
B) ²³¹Pa
C) ²⁴⁵Pu
D) ²³⁸U
E) ²³²Pa

Question 8

Atomic number is equal to the _____ in the nucleus of an atom.

A) number of electrons
B) number of protons
C) number of protons minus the number of neutrons
D) sum of the number of electrons and neutrons
E) sum of the number of neutrons and protons

Question 9

Which of the following elements does 'X' represent in ${ } _ { 28 } ^ { 58 } \mathrm { X }$ ?

A) Ni
B) Zn
C) Rn
D) Ce
E) Pd

Question 10

Which of the following atomic symbols represents an isotope of ${ } ^ { 113 } \mathrm { Cd }$ ?

A) ${ } ^ { 112 } \mathrm { Ag }$
B) ${ } ^ { 114 } \mathrm { In }$
C) ${ } ^ { 113 } \mathrm { In }$
D) ${ } ^ { 114 } \mathrm { Cd }$
E) ${ } ^ { 113 } \mathrm { Ag }$

Question 11

Which of the following is the correct atomic symbol for an element that has 30 neutrons and a mass number of 55?

A) At
B) Zn
C) Co
D) Mn
E) Cs

Question 12

The atomic number of fluorine is _____.

A) 7
B) 9
C) 10
D) 19
E) 13

Question 13

Atoms are made of three subatomic particles. What are these particles and their charges?

A) proton (+1), neutron (0), and electron (−1)
B) proton (−1), neutron (+1), and electron (0)
C) proton (+1), neutron (−1), and electron (0)
D) proton (0), neutron (+1), and electron (−1)
E) proton (−1), neutron (0), and electron (+1)

Question 14

How many protons are there in an atom of scandium-45?

A) 25
B) 66
C) 20
D) 21
E) 24

Question 15

How many neutrons are there in an atom of copper-63 ?

A) 29
B) 2
C) 92
D) 63
E) 34

Question 16

Which of the following is the correct atomic symbol for an element with 17 protons and 18 neutrons?

A) ${ } _ { 17 } ^ { 35 } \mathrm { Ar }$
B) ${ } _ { 17 } ^ { 18 } \mathrm { Ar }$
C) ${ } _ { 17 } ^ { 35 } \mathrm { Cl }$
D) ${ } _ { 18 } ^ { 17 } \mathrm { Ar }$
E) ${ } _ { 17 } ^ { 18 } \mathrm { Cl }$

Question 17

If two different isotopes have the same atomic number, it means that _____.

A) they have the same atomic mass
B) they have the same atomic number
C) they have the same number of protons
D) they have the same number of electrons
E) they have the same number of neutrons

Question 18

An atom that has the same number of neutrons as nickel-59 is _____.

A) ${ } ^ { 58 } \mathrm { Zn }$
B) ${ } ^ { 58 } \mathrm { Co }$
C) ${ } ^ { 57 } \mathrm { Cr }$
D) ${ } ^ { 58 } \mathrm { Mn }$
E) ${ } ^ { 59 } \mathrm { Zn }$

Question 19

Two isotopes of a given element will have the same number of _____, but a different number of _____ in their nucleus.

A) protons; electrons
B) electrons; protons
C) protons; neutrons
D) neutrons; protons
E) electrons; neutrons

Question 20

Arrange the subatomic particles in order of their increasing mass.

A) Electron mass = proton mass = neutron mass
B) Electron mass = neutron mass < proton mass
C) Electron mass = proton mass < neutron mass
D) Electron mass < proton mass < neutron mass
E) Electron mass < proton mass = neutron mass

Question 21

Which of the following elements is present in the fourth period of Group 3A?

A) Sb
B) Ga
C) In
D) Si
E) Tl

Question 22

A sample of an element consists of two isotopes. The percent abundance of one of the isotopes is 75.0%. What is the percent abundance of the other isotope?

A) 62.5%
B) 37.5%
C) 12.5%
D) 75.0%
E) 25.0%

Question 23

Which of the following elements is present in the third period of group 7A?

A) S
B) Cl₂
C) I₂
D) H₂
E) Ar

Question 24

Which of the following groups of periodic table contains only nonmetals?

A) 2A
B) 3A
C) 5A
D) 6A
E) 7A

Question 25

An element consists of three isotopes. The abundance of one isotope is 92.21% and its atomic mass is 27.97693 u. The abundance of the second isotope is 4.70% and its atomic mass is 28.97649 u. The atomic mass of the third isotope is 29.97376 u. What is the atomic weight of the element?

A) 28.09 u
B) 28.98 u
C) 28.96 u
D) 29.87 u
E) 29.07 u

Question 26

Copper has an atomic weight of 63.55 u. If 69.17% of copper exists as ⁶³Cu (62.93960 u), what is the identity and the atomic mass of the other isotope?

A) Cu-64; 63.82 u
B) Cu-64; 64.16 u
C) Cu-65; 64.16 u
D) Cu-65; 64.92 u
E) Cu-66; 65.91 u

Question 27

Silver has two stable isotopes with masses of 106.90509 u and 108.9047 u. The atomic weight of silver is 107.868 u. What is the percent abundance of each isotope?

A) 50.0% ¹⁰⁷Ag and 50.0% ¹⁰⁹Ag
B) 51.8% ¹⁰⁷Ag and 48.2% ¹⁰⁹Ag
C) 55.4% ¹⁰⁷Ag and 44.6% ¹⁰⁹Ag
D) 48.2% ¹⁰⁷Ag and 51.8% ¹⁰⁹Ag
E) 44.6% ¹⁰⁷Ag and 55.4% ¹⁰⁹Ag

Question 28

The masses of isotopes and their abundances are determined experimentally using _____.

A) a mass spectrometer
B) an analytical balance
C) a centrifuge
D) distillation
E) electrolysis

Question 29

The element chlorine has two stable isotopes, chlorine-35 with an atomic mass of 34.97 u and chlorine-37 with an atomic mass of 36.97 u. From the atomic weight found on the periodic table, one can conclude that _____.

A) both isotopes have the same percent natural abundance
B) there is an isotope of nitrogen with an atomic mass of 35.45 u
C) chlorine-35 has the highest percent natural abundance
D) chlorine-37 has the highest percent natural abundance
E) there is an isotope of nitrogen with an atomic mass of 37.95 u

Question 30

A certain element consists of two stable isotopes. The first has a mass of 14.0031 amu and a percent natural abundance of 99.63%. The second has a mass of 15.001 amu and a percent natural abundance of 0.37%. What is the atomic weight of the element?

A) 13.95 amu
B) 14.00 amu
C) 14.01 amu
D) 14.50 amu
E) 19.50 amu

Question 31

The elements in groups 1A-8A are known as the _____.

A) main group elements
B) transition metals
C) halogens
D) metalloids or semimetals
E) noble gases

Question 32

Lithium has two naturally occurring isotopes, ⁶Li and ⁷Li. The atomic weight of lithium is 6.941. Which of the following statements concerning the relative abundance of each isotope is correct?

A) The abundance of ⁷Li is greater than ⁶Li.
B) The abundance of ⁷Li is less than ⁶Li.
C) The abundance of ⁶Li is equal to the abundance of ⁷Li.
D) Not enough data is provided to determine the correct answer.
E) Based on the atomic mass, only ⁷Li occurs naturally.

Question 33

Which of the following elements is present in fourth period of group 3?

A) Flourine
B) Chlorine
C) Barium
D) Argon
E) Sodium

Question 34

Which of the following statements is true concerning ${ } ^ { 16 } \mathrm { O }$ and ${ } ^ { 17 } \mathrm { O }$ ?

A) They have the same number of neutrons.
B) They are isotopes.
C) They have the same relative atomic mass.
D) They have the same mass number.
E) They have different chemical properties.

Question 35

Naturally occurring element X exists in three isotopic forms: X-28 (27.979 u, 90.64% abundance), X-29 (28.976 u, 4.00% abundance), and X-30 (29.974 u, 5.36% abundance). Calculate the atomic weight of X.

A) 29.64 u
B) 28.13 u
C) 28.99 u
D) 29.83 u
E) 27.15 u

Question 36

Rubidium has two naturally occurring isotopes. The atomic weight of Rb is 85.4678 u. If 72.15% of Rb is found as Rb-85 (84.9117 u), what is the mass of the other isotope?

A) 0.56 u
B) 85.68 u
C) 86.68 u
D) 86.02 u
E) 83.47 u

Question 37

The mass spectrum of an element with two naturally occurring isotopes is shown below. What is the best estimate of the element's (average) atomic weight?

A) 10 amu
B) 11 amu
C) 10.8 amu
D) 10.2 amu
E) 10.5 amu

Question 38

What is the common name of the group that has an element with 38 protons in its nucleus?

A) Transition metals
B) Halogens
C) Noble gases
D) Alkaline earth metals
E) Alkali metals

Question 39

Which of the following elements belongs to the alkaline earth metals series?

A) Barium
B) Potassium
C) phosphorus
D) Bromine
E) Argon

Question 40

Which of the following statements is not true about the element vanadium?

A) It is a metal.
B) It has chemical and physical properties most similar to krypton.
C) It is in period 4.
D) It has chemical and physical properties most similar to silver.
E) It is in group 5B.

Question 41

Which of the following sets of ions is present in calcium hydrogen phosphate, CaHPO₄?

A) Ca²⁺ and PO₄^3-
B) Ca²⁺ and HPO₄^2-
C) Ca⁺ and HPO₄^-
D) Ca³⁺ and HPO₄^3-
E) Ca²⁺, H⁺, P^3-, and O^2-

Question 42

What is the charge on the sodium ion in Na₃P?

A) 3-
B) 1-
C) 0
D) 1+
E) 3+

Question 43

The formula of acetic acid, CH₃CO₂H, is an example of a(n) _____.

A) condensed formula
B) empirical formula
C) structural formula
D) ionic compound formula
E) elemental formula

Question 44

Which of the following is the correct formula for cobalt(III) bromide?

A) CoBr
B) CoBr₃
C) Co₂Br₃
D) Co₃Br₂
E) Co₃Br

Question 45

Which of the following atoms of elements is most likely to form a 2+ ion?

A) Scandium
B) Calcium
C) Aluminum
D) Oxygen
E) Fluorine

Question 46

Which of the following formulas is not correct?

A) AlPO₄
B) KClO₄
C) CaS
D) Na(NO₃)₂
E) Na₂HPO₄

Question 47

Which of the following is the correct formula for an ionic compound that contains barium ions and carbonate ions?

A) BaCO₃
B) Ba(HCO₃)₂
C) Ba₂CO₃
D) Ba₂C
E) Ba(CO₃)₂

Question 48

C₂H₂F₄ is the formula for two possible molecules. C₂H₂F₄ is an example of a(n) _____.

A) structural formula
B) empirical formula
C) condensed formula
D) spatial formula
E) molecular formula

Question 49

The correct name for Cd²⁺ is _____.

A) monocadmium ion
B) cadmium(II) ion
C) cadmium(2) ion
D) cadmium(I) ion
E) cadmium

Question 50

Which of the following elements is not a metalloid?

A) Boron
B) Selenium
C) Germanium
D) Arsenic
E) Silicon

Question 51

Which of the following atoms of elements is most likely to form a 2- ion?

A) Potassium
B) Magnesium
C) Phosphorus
D) Bromine
E) Sulfur

Question 52

Which of the following is the correct formula for calcium nitrate?

A) CaN
B) Ca₃N₂
C) CaNO₂
D) Ca₃(NO₃)₂
E) Ca(NO₃)₂

Question 53

The formula for aluminum fluoride is _____.

A) AlF₃
B) AlF
C) Al₂F
D) AlF₄
E) AlF₂

Question 54

Which of the following sets of ions is present in sodium sulfate, Na₂SO₄?

A) Na⁺, S²⁻, and O²⁻
B) Na⁺, S²⁺, and O²⁻
C) Na⁺ and SO₄²⁻
D) Na⁺, S²⁻, and O²⁺
E) Na⁺ and SO₄−

Question 55

Which of the following is the correct formula for manganese(III) sulfate?

A) MnSO₄
B) Mn₂SO₄
C) Mn₃(SO₄)₂
D) Mn₂(SO₄)₃
E) Mn(SO₄)₂

Question 56

Which of the following is the correct formula for potassium dihydrogen phosphate?

A) KH₂PO₄
B) K₂HPO₄
C) K₂H₂PO₄
D) K₃H₂PO₄
E) KH₂P

Question 57

The chemical formula for chromium(III) sulfate is _____.

A) CrSO₄
B) Cr(SO₄)₃
C) Cr₂(SO₄)₃
D) Cr₂SO₄
E) Cr₃(SO₄)₂

Question 58

Scandium(III) sulfite is an ionic compound formed from Sc³⁺ and SO₃^2-. What is the correct way to represent the formula?

A) ScSO₃⁺
B) Sc(SO₃)₂^-
C) Sc³⁺SO₃^2-
D) Sc₂(SO₃)₃
E) Sc₅(SO₃)₈

Question 59

For a nonmetal in Group 6A of the periodic table, the most common monatomic ion will have a charge of _____.

A) 3-
B) 2-
C) 1-
D) 1+
E) 2+

Question 60

What charge is likely possible on a monatomic silver cation?

A) 2-
B) 1-
C) 1+
D) 2+
E) 3+

Question 61

The correct name for the compound P₂F₄ is _____.

A) diphosphorus tetrafluoride
B) phosphorus fluoride
C) diphosphide tetrafluoride
D) diphosphorus tetrafluorine
E) phosphorus tetrafluorine

Question 62

A 0.0050 g sample of boron contains _____ boron atoms.

A) 4.6 × 10^-4
B) 7.7 × 10^-28
C) 2.8 × 10²⁰
D) 3.1 × 10²¹
E) 3.3 × 10²²

Question 63

Which of the following is the correct name for the compound Ca(CH3CO2)2?

A) Calcium(II) carbonate
B) Calcium carbonate
C) Calcium acetate
D) Acetic calcide
E) Calcium carbonide

Question 64

Which of the following is the correct name for the compound CCl₄?

A) Carbon chlorine
B) Tetracarbon chloride
C) Carbon tetrachloride
D) Carbon(IV) chloride
E) Tetrachlorocarbide

Question 65

Calculate the number of moles in 0.48 g of Cu.

A) 0.033 mol
B) 0.48 mol
C) 31 mol
D) 7.6 × 10−³ mol
E) 1.3 × 10² mol

Question 66

What is the approximate mass of 0.71 mol Na?

A) 1.2 × 10^-24 g
B) 12 g
C) 16 g
D) 0.031 g
E) 32 g

Question 67

The molar mass of platinum is 195.08 g/mol. What is the mass of 1.00 × 10² Pt atoms?

A) 8.51 × 10^-25 g
B) 3.24 × 10^-24 g
C) 1.67 × 10^-22 g
D) 3.24 × 10^-22 g
E) 3.24 × 10^-20 g

Question 68

What is the symbol for an ion of an element that has 12 protons and 10 electrons?

A) Mg²⁺
B) Mg^2-
C) Ne²⁺
D) Ne^2-
E) Ti²⁺

Question 69

What is the formula for the compound that is formed of ammonium and bromide ions?

A) NH₃Br
B) NH₄Br
C) NH₃Br₂
D) NH₄Br₂
E) (NH₄)₂Br

Question 70

What mass of aluminum contains the same number of atoms as 3.0 g of lead?

A) 23 g
B) 0.014 g
C) 3.0 g
D) 0.39 g
E) 0.11 g

Question 71

Which of the following ionic compounds has the highest melting point?

A) KBr
B) MgO
C) RbI
D) CaBr₂
E) CsCl

Question 72

Which of the following is the correct molar mass of sodium sulfate?

A) 55.06 g/mol
B) 119.1 g/mol
C) 78.05 g/mol
D) 142.0 g/mol
E) 110.0 g/mol

Question 73

Which of the following is the correct name for the compound SrCl2?

A) Strontium dichloride
B) Strontium dichlorine
C) Strontium(III) dichloride
D) Strontium chloride
E) Iodine strontide

Question 74

A 0.4272 g sample of an element contains 2.241 × 10²¹ atoms. What is the symbol of the element?

A) In
B) Cs
C) Sb
D) Xe
E) Te

Question 75

You have 2.50 g of each of the following elements: Ca, Cu, Cs, C, and Cr. Which sample contains the largest number of atoms?

A) Ca
B) Cu
C) Cs
D) C
E) Cr

Question 76

Which of the following is the correct name for the compound NH₄NO₃?

A) Ammonia hydrogen nitrate
B) Ammonia hydrogen nitride
C) Ammonium nitric acid
D) Ammonium nitrate
E) Ammonium nitride

Question 77

A nail is coated with a 0.053 cm thick layer of zinc. The surface area of the nail is 8.59 cm². The density of zinc is 7.13 g/cm³. How many zinc atoms are used in the coating?

A) 5.9 × 10²⁰ atoms
B) 3.0 × 10²² atoms
C) 3.8 × 10²² atoms
D) 2.0 × 10²⁴ atoms
E) 1.3 × 10²⁶ atoms

Question 78

Which of the following is the common name for the compound PH₃?

A) Laughing gas
B) Hydrazine
C) Nitroglycerin
D) Ammonia
E) Phosphine

Question 79

Which of the following is the correct molar mass of calcium chloride hexahydrate?

A) 75.53 g/mol
B) 111.0 g/mol
C) 117.0 g/mol
D) 183.6 g/mol
E) 219.1 g/mol

Question 80

What is the molecular mass of cyclononane, C₉H₁₈?

A) 13.02 g/mol
B) 1963.92 g/mol
C) 109.11 g/mol
D) 126.24 g/mol
E) 30.15 g/mol