Deck 2: Atoms, Ions, and Compounds

Question 1

A atom has __________ protons, __________ neutrons, and __________ electrons.

A) 17, 18, 19
B) 17, 20, 17
C) 17, 17, 20
D) 17, 18, 17
E) 18, 17, 18

Answer 1

17, 18, 17

Question 2

Rutherford, Geiger, and Marsden's experiment demonstrated that the volume of the nucleus is roughly what fraction of the volume occupied by the electrons?

A) 1/10
B) 1/100
C) 1/1,000
D) 1/10,000
E) 1/100,000

Answer 2

1/10,000

Question 3

What is the correct symbol for a neutron?

A)
B)
C)
D)
E)

Answer 3

Question 4

Who discovered electrons?

A) Robert Boyle
B) Robert Millikan
C) Joseph John Thomson
D) John Dalton
E) Albert Einstein

Question 5

In the atoms in the Rutherford-Geiger-Marsden experiment, the  particles were repelled by __________

A) electrons.
B) protons.
C) neutrons.
D) nuclei.
E) gravity.

Question 6

Which one of the following experiments provided evidence that atoms contained small massive nuclei with positive charges?

A) Bunsen and Kirchoff's flame test
B) Fraunhofer lines
C) the Rutherford-Geiger-Marsden experiment
D) Thomson's experiments with cathode ray tubes
E) Millikan's oil-drop experiment

Question 7

Which particle diagram is the best representation for a atom?

A)
B)
C)
D)

Question 8

In the Rutherford-Geiger-Marsden experiment,  particles were projected at a thin film of __________

A) gold.
B) silver.
C) platinum.
D) sodium.
E) aluminum.

Question 9

Protons and neutrons are examples of __________

A) nuclei.
B) nuclides.
C) nucleons.
D) isotopes.
E) charged particles.

Question 10

Which statement best describes isotopes?

A) They have the same atomic mass.
B) They have the same total number of protons and neutrons.
C) They have the same number of neutrons but a different number of protons.
D) They have the same number of protons but a different number of neutrons.
E) They have very different chemical reactivity.

Question 11

Who was the first scientist to determine the charge of an electron?

A) Robert Boyle
B) Robert Millikan
C) Joseph John Thomson
D) John Dalton
E) Albert Einstein

Question 12

What is the correct symbol for an electron?

A)
B)
C)
D)
E)

Question 13

The average atomic mass of calcium is 40.078 amu. Which is the most abundant isotope of calcium?

A)"⁴⁰Ca"
B)"⁴²Ca"
C)"⁴³Ca"
D)"⁴⁴Ca"
E)"⁴⁸Ca"

Question 14

What is the correct symbol for a proton?

A)
B)
C)
D)
E)

Question 15

If an atom had a radius of 100 m, it would be approximately the size of a football stadium. On this scale, what would be the radius of the atomic nucleus since the radius of the nucleus is approximately 10,000 times smaller than the radius of an atom?

A) 1 mm, like a very dull pencil point
B) 1 cm, like a dime
C) 10 cm, like your longest finger
D) 10 m, like a red blood cell
E) 100 pm, like a real atom

Question 16

A ion has __________ protons, __________ neutrons, and __________ electrons.

A) 8, 10, 8
B) 8, 10, 10
C) 8, 8, 10
D) 8, 8, 8
E) 8, 16, 8

Question 17

What is the correct symbol for an  particle?

A)
B)
C)
D)
E)

Question 18

The ⁴He nucleus is an example of __________

A) a nuclide.
B) an element.
C) a proton.
D) a neutron.
E) a nucleon.

Question 19

Which particle-level diagram is the best representation of a ion?

A)
B)
C)
D)

Question 20

When cosmic rays strike atoms in the upper atmosphere, energetic neutrons are produced. These neutrons collide with nitrogen-14 atoms, producing carbon-14 atoms and hydrogen atoms. Which diagram represents the carbon-14 product?

A)
B)
C)
D)

Question 21

Elements in group 17 (VIIA) are called __________

A) alkali metals.
B) pnictogens.
C) alkaline earth metal.
D) halogens.
E) chalcogens.

Question 22

Cobalt is best described as a __________

A) metalloid.
B) transition metal.
C) chalcogen.
D) noble gas.
E) nonmetal.

Question 23

Sodium is best described as a __________

A) metalloid.
B) metal.
C) transition metal.
D) noble gas.
E) nonmetal.

Question 24

For each of the elements below, there are only two naturally occurring isotopes. Using information in your periodic table, identify the pair in which the heavier isotope is the more abundant one.

A)"⁶³Cu" and ⁶⁵Cu
B)"⁸⁵Rb" and ⁸⁷Rb
C)"¹⁰B" and ¹¹B
D)"⁷⁹Br" and ⁸¹Br
E)"¹⁴N" and ¹⁵N

Question 25

He is the symbol for __________

A) hydrogen.
B) hafnium.
C) mercury.
D) helium.
E) holmium.

Question 26

Silicon is best described as a __________

A) metalloid.
B) metal.
C) transition metal.
D) noble gas.
E) nonmetal.

Question 27

Elements in group 18 (VIIIA) are called __________

A) alkali metals.
B) noble gases.
C) alkaline earth metals.
D) halogens.
E) chalcogens.

Question 28

A hypothetical element has two stable isotopes: one isotope has a mass of 106.9051 amu with an abundance of 48.183%, the other isotope has a mass of 108.9048 amu with an abundance of 51.825%. What is the average atomic mass of this element?

A) 107.980 amu
B) 107.970 amu
C) 107.960 amu
D) 107.950 amu
E) 107.940 amu

Question 29

The average atomic mass of zinc is 65.39 amu. Given the data in the following table, what is the natural abundance of ⁶⁶Zn? Isotope
Mass (amu)
Natural Abundance (%)⁶⁴Zn
63)9291
48)89⁶⁶Zn
65)9260
?⁶⁷Zn
66)9271
4)11⁶⁸Zn
67)9249
18)56⁷⁰Zn
69)9253
0)62

A) 27.81%
B) 0.2781%
C) 50.00%
D) 2.781%
E) 28.71%

Question 30

Zinc has five naturally occurring isotopes with an average mass of 65.39 amu. Three isotopes, in roughly equal amounts, account for 95% of zinc. Which isotope is most abundant?

A)"⁶⁴Zn", 63.9291 amu
B)"⁶⁶Zn", 65.9260 amu
C)"⁶⁷Zn", 66.9271 amu
D)"⁶⁸Zn", 67.9249 amu
E)"⁷⁰Zn", 69.9253 amu

Question 31

Which of the following is an alkali metal?

A) K
B) Mg
C) Al
D) Cu
E) Ca

Question 32

For each of the elements below, there are only two naturally occurring isotopes. Using information in your periodic table, identify the pair in which the lighter isotope is the more abundant one.

A)"⁶Li" and ⁷Li
B)"⁷⁹Br" and ⁸¹Br
C)"¹⁰B" and ¹¹B
D)"¹⁹¹Ir" and ¹⁹³Ir
E)"⁵⁰V" and ⁵¹V

Question 33

What is the symbol for sulfur?

A) Si
B) Sc
C) Su
D) S
E) Sf

Question 34

The average atomic mass of lithium is 6.941 amu. Lithium has two naturally occurring isotopes, ⁶Li (7.52%) and ⁷Li (92.48%). The mass of ⁶Li is 6.0151 amu. What is the mass of ⁷Li?

A) 7.016 amu
B) 0.926 amu
C) 6.001 amu
D) 7.000 amu
E) 6.941 amu

Question 35

An unknown element is found to contain isotopes with the following masses and natural abundances: 38.9637 amu (93.08%), 39.9640 amu (0.012%), and 40.9618 amu (6.91%). Using these data, identify the element.

A) S
B) Cl
C) Ar
D) K
E) Ca

Question 36

Elements 21 through 30 are known as __________

A) alkaline earths.
B) chalcogens.
C) halides.
D) transition metals.
E) rare earths.

Question 37

Enriched weapons-grade uranium consists of 80% uranium-235 (235.044 amu) and 20% uranium-238 (238.051 amu). What is the average atomic mass of weapons grade uranium assuming the percentages are exact?

A) 235.044 amu
B) 236.547 amu
C) 238.051 amu
D) 235.645 amu
E) 235.754 amu

Question 38

Calcium is an example of __________

A) an alkali metal.
B) a transition metal.
C) an alkaline earth metal.
D) a halogen.
E) a chalcogen.

Question 39

Oxygen is best described as a __________

A) metalloid.
B) metal.
C) transition metal.
D) noble gas.
E) nonmetal.

Question 40

What is the symbol for magnesium?

A) M
B) Mg
C) Mn
D) Mo
E) Ma

Question 41

Based on its position in the periodic table, which atom would you predict to form a compound with one chlorine atom?

A) boron
B) aluminum
C) lithium
D) calcium
E) carbon

Question 42

Which one of the following statements is not consistent with Dalton's atomic theory of matter?

A) Atoms of one element can be converted into atoms of another element.
B) Each element is composed of atoms that are identical in size, mass, and chemical properties.
C) Compounds are formed from different atoms in simple whole number ratios.
D) Atoms of different elements can combine in several different proportions to make different compounds.
E) Matter is discrete, as proposed by Democritus.

Question 43

Identify the binary compound that has ionic bonding.

A) H₂O
B) NO
C) LiF
D) CH₄

Question 44

Which one of the following is an anion?

A) Na⁺
B) CO₂
C) Cl^-
D) Na
E) O₃

Question 45

When 10.0 g of sulfur is combined with 10.0 g of oxygen, 20.0 g of sulfur dioxide is formed. What mass of oxygen would be required to convert 10.0 g of sulfur into sulfur trioxide?

A) 5.0 g
B) 10 g
C) 15 g
D) 30 g
E) 20 g

Question 46

Dalton's law of multiple proportions deals with __________

A) the proportions of reacting chemicals that maximize the reaction rate.
B) the total number of different compounds that can be made from two elements.
C) the volumes of two elements that can combine to form two or more compounds.
D) the masses of two elements that can combine to form two or more compounds.
E) reactions that involve multiple steps.

Question 47

The sixth period of the periodic table contains __________ elements.

A) 18
B) 32
C) 24
D) 16
E) 8

Question 48

What is the correct formula for the compound formed between sodium and iodine based on their positions in the periodic table?

A) Na₂I
B) NaI₂
C) NaI
D) Na₂I₂
E) Na₃I

Question 49

Which one of the following is a molecular compound? Molecular compounds also are known as covalent compounds.

A) Na₂O
B) CaO
C) FeO
D) CCl₄
E) Fe₂O₃

Question 50

Based on its position in the periodic table, which atom would you predict to form a compound with two bromine atoms?

A) sodium
B) aluminum
C) lithium
D) calcium
E) carbon

Question 51

Which contains more carbon by mass, 1 g of CO₂ or 1 g of CO?

A) CO₂
B) CO
C) Both contain the same mass of carbon.
D) Both contain the same mass of carbon, but different masses of oxygen.

Question 52

Which one of the following is an ionic compound?

A) SO₂
B) ClO₂
C) H₂O
D) TiO₂
E) CO₂

Question 53

Dalton's law of multiple proportions can be applied to __________

A) H₂O and CO₂.
B) CO and NO.
C) PF₃ and PF₅.
D) SO₂ and CO.
E) O₂ and O₃.

Question 54

Which one of the following is a cation?

A) NO₃^-
B) SO₂
C) Ca²⁺
D) Na
E) O₂

Question 55

Which would produce the larger mass of carbon dioxide, CO₂, when combined with oxygen: 1 g of pure carbon or 1 g of pure octane (C₈H₁₄)? Assume that all the carbon is converted to carbon dioxide in both cases.

A) C
B) C₈H₁₄
C) They would produce the same mass of CO₂.
D) It depends on the densities of the carbon and octane.

Question 56

Which of the following is most likely to exhibit covalent bonding?

A) NaF
B) CaCl₂
C) Cs₂O
D) CO₂
E) NaCl

Question 57

Iron can form two sulfides: FeS and Fe₂S₃. Use Dalton's law of multiple proportions to predict the ratio of the two masses of sulfur that combine with 100 g of iron in each case to form these compounds.

A) 1:1
B) 1:3
C) 1:2
D) 2:3
E) 3:4

Question 58

Nitrogen and oxygen combine to form several different nitrogen oxides. In one case, 8.4 g of nitrogen reacted completely with 4.8 g of oxygen. In another case, 4.2 g of nitrogen reacted with 9.6 g of oxygen. Which pair of nitrogen oxides is consistent with these data?

A) NO and N₂O
B) NO and NO₂
C) N₂O and N₂O₅
D) NO and N₂O₄
E) N₂O and N₂O₄

Question 59

Which has more mass: a lump of coal (assumed to be 100% carbon) or the carbon dioxide gas formed from burning the lump of coal?

A) The lump of coal because it is a solid.
B) The lump of coal because gases have little mass.
C) The carbon dioxide gas because it occupies a much larger volume.
D) The carbon dioxide gas because it includes oxygen that was added from the air.
E) Both weigh the same because mass is conserved.

Question 60

Which has more mass, 1 g of CO₂ gas or 1 g of CO gas?

A) CO
B) CO₂
C) Both have the same mass.
D) It depends on the density of these gases.
E) It depends on the volume of these gases.

Question 61

Manganese(IV) oxide is a brown insoluble solid often found as a product of reactions of potassium permanganate. What is the formula of manganese(IV) oxide?

A) Mn₄O
B) MnO₄
C) Mn(IV)O
D) MnO₂
E) Mn₂O₂

Question 62

Zinc oxide is found in ointments for the skin. What formula best describes this compound, which has Zn as a doubly charged cation?

A) ZnO
B) Zn₂O
C) ZnO₂
D) Zn₂O₂
E) Zn₂O₃

Question 63

According to the Big Bang theory, which statement about the origin of the elements is not correct?

A) Initially, energy was transformed into electrons and other elementary particles.
B) As the universe cooled, neutrons and protons were formed.
C) Collisions of neutrons and protons produced deuterons, which then led to the formation of alpha particles.
D) The nuclides of the elements then were formed by nuclear reactions in the interior of stars.
E) These nuclear reactions all require the addition of energy to form the elements.

Question 64

Radium often is found in uranium ores and can be separated from solutions by precipitation as radium sulfate. What is the formula for radium sulfate?

A) RnSO₄
B) RaSO₄
C) Rn₂SO₃
D) Ra₂SO₄
E) Ra(SO₄)₂

Question 65

Sodium nitrite, which is used in meat processing, has been implicated as a possible health hazard because it can react with amines present in meat to form trace quantities of carcinogenic nitrosamines. What is the formula of sodium nitrite?

A) SNO
B) NaNO₂
C) NaNO₃
D) Na₂NO₄
E) Na₂NO₂

Question 66

Two neutrons were walking down the street. One said, "Wait a minute…I think I lost a __________!" The other one asked, "Are you sure?" The first replied, "Yes, I'm positive!"

A) positron
B) "" particle
C) "" ray
D) neutrino

Question 67

Buffer solutions that maintain certain levels of pH or acidity are widely used in biochemical experiments. One common buffer system uses sodium dihydrogenphosphate and sodium monohydrogenphosphate. What are the formulas of these two compounds?

A) Na(HPO₄) and Na(HPO₄)₂
B) NaH₂PO₄ and Na₂HPO₄
C) Na₂H₂PO₄ and NaHPO₄
D) NaPO₄ and NaHPO₄

Question 68

What is the empirical formula for benzene, C₆H₆?

A) CH
B) C₆H₆
C) C₂H₂
D) CH₃
E) C₆H

Question 69

The emission of a  particle is associated with the __________

A) conversion of a neutron to a proton.
B) conversion of a proton to a neutron.
C) increase in mass number.
D) decrease in mass number.
E) the formation of an isotope.

Question 70

TiO₂ is a white oxide used in paints. What is the proper name for TiO₂?

A) titanium oxide
B) titanium(IV) oxide
C) titanic acid
D) titanium oxoate
E) titanium dioxide

Question 71

What is the proper name for Co(ClO₄)₃?

A) cobalt trichlorate
B) cobalt chlorate
C) cobaltous chlorate
D) cobalt(III) perchlorate
E) cobalt(III) chlorate

Question 72

Which one of the formula-name combinations is not correct?

A) sulfur monoxide: SO
B) sulfur dioxide: SO₂
C) sulfur trioxide: SO₃
D) disulfur oxide: S₂O
E) heptasulfur oxide: S₆O

Question 73

A high-energy particle with a negative charge is called a __________ particle?

A) ""
B) ""
C) ""
D) neutron
E) positron

Question 74

What is the correct name for FeCl₃?

A) iron(III) chloride
B) iron trichloride
C) ferrum trichloride
D) ferric trichloride
E) iron chloride

Question 75

What is the formula for sodium bromide?

A) SBr
B) NaBr
C) Na₂Br
D) NaBrO
E) NaBr₂

Question 76

Active metals often form a protective oxide surface film that prevents further reaction of the metal with oxygen in the air. Which one of the following formulas for the metal oxide is not correct?

A) Al₂O₃ is aluminum(III) oxide.
B) Fe₂O₃ is iron(III) oxide.
C) Na₂O is sodium oxide.
D) MgO₂ is magnesium oxide.
E) FeO is iron(II) oxide.

Question 77

The Murrah Federal Building in Oklahoma City was destroyed on April 19, 1995, killing 168 people by a simple, but powerful, bomb made from 4800 lb of ammonium nitrate. What is the formula for ammonium nitrate?

A) Am(NO₃)₂
B) Am(NO₃)
C) NH₄NO₃
D) NH₄(NO₃)₂
E) (NH₄)₂NO₃

Question 78

Aqua regia is a mixture of hydrochloric acid and nitric acid that is capable of dissolving gold. What are the formulas of these acids?

A) HClO, HNO₄
B) HClO₄, HNO₃
C) HCl, HNO₂
D) HCl, HNO₃
E) HCl, HNO

Question 79

Which stellar nuclear reaction is not correctly written?

A)
B)
C)
D)
E)

Question 80

Name the following oxides of nitrogen in this sequence: NO, N₂O, NO₂, N₂O₄.

A) nitrogen monoxide, dinitrogen oxide, nitrogen dioxide, dinitrogen tetroxide
B) nitrox, dinitrox, nitridiox, dinitritriox
C) mononitrogen monoxide, dinitrogen monoxide, mononitrogen dioxide, dinitrogen tetraoxide
D) nitrogen oxide, nitrogen(II) oxide, nitrogen oxide(II), nitrogen(II) oxide(IV)
E) nitric oxide, nitrous oxide, nitrogen dioxide, nitrogen tetraoxide