Question 1

Iodine belongs to the ________ group of the periodic table.

Accepted Answer

A)  alkali metal 
B)  alkaline earth metal 
C)  halogen 
D)  noble gas 
A)  alkali metal 
B)  alkaline earth metal 
C)  halogen 
D)  noble gas C

Question 2

Magnesium tends to lose ________ electron(s) to attain a noble gas configuration.

Accepted Answer

A)  3 
B)  4 
C)  5 
D)  2 
E)  1 
A)  3 
B)  4 
C)  5 
D)  2 
E)  1 D

Question 3

Give the name of the instrument that is used to measure masses of atoms and the percent abundance of isotopes.

Accepted Answer

mass spectrometer

Question 4

Are anions typically larger or smaller than their corresponding atom? Why?

Accepted Answer

Anions are larger than their correspondi

Question 5

Which element has the chemical symbol Ru?

Accepted Answer

A)  rubidium 
B)  ruthenium 
C)  rutherfordium 
D)  rhodium 
A)  rubidium 
B)  ruthenium 
C)  rutherfordium 
D)  rhodium

Question 6

All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?

Accepted Answer

A)  Law of definite proportions 
B)  Law of the conservation of mass 
C)  Law of modern atomic theory 
D)  Law of multiple proportions 
E)  First law of thermodynamics 
A)  Law of definite proportions 
B)  Law of the conservation of mass 
C)  Law of modern atomic theory 
D)  Law of multiple proportions 
E)  First law of thermodynamics

Question 7

Why doesn't a mass spectrum of silver have a peak at 107.9 u?

Accepted Answer

The average atomic mass of sil

Question 8

Carbon has two naturally occurring isotopes, carbon-12 and carbon-13. The more common isotope of carbon is carbon-12 with an abundance of 98.93% while carbon-13 has an atomic mass of 13.00335 u. Calculate the atomic mass of carbon-12 if the atomic mass of carbon is 12.0107 u.

Accepted Answer

A)  13.1 u 
B)  13.0 u 
C)  12.0 u 
D)  12.8 u 
E)  12.4 u 
A)  13.1 u 
B)  13.0 u 
C)  12.0 u 
D)  12.8 u 
E)  12.4 u

Question 9

What mass (in mg) does 2.63 moles of nickel have?

Accepted Answer

A)  44.8 mg 
B)  2.23 × 104 mg 
C)  129 mg 
D)  3.56 × 105 mg 
E)  1.54 × 105 mg 
A)  44.8 mg 
B)  2.23 × 104 mg 
C)  129 mg 
D)  3.56 × 105 mg 
E)  1.54 × 105 mg

Question 10

Identify the largest by size atom or ion of carbon.

Accepted Answer

A)  p+ = 6 n° = 6 e- = 6 
B)  p+ = 6 n° = 7 e- = 6 
C)  p+ = 6 n° = 6 e- = 7 
D)  p+ = 6 n° = 6 e- = 5 
A)  p+ = 6 n° = 6 e- = 6 
B)  p+ = 6 n° = 7 e- = 6 
C)  p+ = 6 n° = 6 e- = 7 
D)  p+ = 6 n° = 6 e- = 5

Question 11

Identify a cation.

Accepted Answer

A)  An atom that has lost (an) electron(s). 
B)  An atom that has gained (an) electron(s). 
C)  An atom that has lost (a) proton(s). 
D)  An atom that has gained (a) proton(s). 
A)  An atom that has lost (an) electron(s). 
B)  An atom that has gained (an) electron(s). 
C)  An atom that has lost (a) proton(s). 
D)  An atom that has gained (a) proton(s).

Question 12

An atom of 31P contains ________ protons.

Accepted Answer

A)  15 
B)  40 
C)  22 
D)  25 
E)  31 
A)  15 
B)  40 
C)  22 
D)  25 
E)  31

Question 13

What species is represented by the following information? p+ = 17 n° = 18 e- = 18

Accepted Answer

A)  Cl 
B)  Cl- 
C)  Ar 
D)  Ar+ 
E)  Kr 
A)  Cl 
B)  Cl- 
C)  Ar 
D)  Ar+ 
E)  Kr

Question 14

If 102.7 g of tin is mixed with 10.9 g of copper to create the alloy pewter, how many moles of metal are present in the pewter?

Accepted Answer

A)  0.9643 mol total 
B)  1.037 mol total 
C)  0.6233 mol total 
D)  1.604 mol total 
E)  0.8675 mol total 
A)  0.9643 mol total 
B)  1.037 mol total 
C)  0.6233 mol total 
D)  1.604 mol total 
E)  0.8675 mol total

Question 15

Which of the following describes a metal?

Accepted Answer

A)  poor conductor of heat 
B)  good conductor of electricity 
C)  tends to gain electrons 
D)  forms ionic compounds with group 18 elements 
E)  found on the upper right corner of the periodic table 
A)  poor conductor of heat 
B)  good conductor of electricity 
C)  tends to gain electrons 
D)  forms ionic compounds with group 18 elements 
E)  found on the upper right corner of the periodic table

Question 16

In which of the following sets do all species have the same number of electrons?

Accepted Answer

A)  F-, Ne, Mg2+ 
B)  Ge, Se2-, Br- 
C)  K+, Rb+, Cs+ 
D)  Br, Br-, Br+ 
A)  F-, Ne, Mg2+ 
B)  Ge, Se2-, Br- 
C)  K+, Rb+, Cs+ 
D)  Br, Br-, Br+

Question 17

The mass number of an atom of 67Ga is ________.

Accepted Answer

A)  31 
B)  76 
C)  36 
D)  67 
E)  70 
A)  31 
B)  76 
C)  36 
D)  67 
E)  70

Question 18

Which of the following statements about subatomic particles is TRUE?

Accepted Answer

A)  A neutral atom contains the same number of protons and electrons. 
B)  Protons have about the same mass as electrons. 
C)  Electrons make up most of the mass of an atom. 
D)  Protons and neutrons have opposite, but equal in magnitude, charges. 
E)  Neutrons and electrons are found in the nucleus of an atom. 
A)  A neutral atom contains the same number of protons and electrons. 
B)  Protons have about the same mass as electrons. 
C)  Electrons make up most of the mass of an atom. 
D)  Protons and neutrons have opposite, but equal in magnitude, charges. 
E)  Neutrons and electrons are found in the nucleus of an atom.

Question 19

Which of the following statements about isotopes is TRUE?

Accepted Answer

A)  Isotopes of the same element differ only in the number of electrons they contain. 
B)  An isotope of an atom with a larger number of neutrons is larger than an isotope of the same atom that contains fewer neutrons. 
C)  Isotopes of the same element have the same mass. 
D)  Isotopes of the same element don't usually have the same properties. 
E)  Some elements have three or more naturally occurring isotopes. 
A)  Isotopes of the same element differ only in the number of electrons they contain. 
B)  An isotope of an atom with a larger number of neutrons is larger than an isotope of the same atom that contains fewer neutrons. 
C)  Isotopes of the same element have the same mass. 
D)  Isotopes of the same element don't usually have the same properties. 
E)  Some elements have three or more naturally occurring isotopes.

Question 20

Argon belongs to the ________ group of the periodic table.

Accepted Answer

A)  alkali metal 
B)  alkaline earth metal 
C)  halogen 
D)  noble gas 
A)  alkali metal 
B)  alkaline earth metal 
C)  halogen 
D)  noble gas

Exam 2: Atoms and Elements

Iodine belongs to the ________ group of the periodic table.

Magnesium tends to lose ________ electron(s) to attain a noble gas configuration.

Give the name of the instrument that is used to measure masses of atoms and the percent abundance of isotopes.

Are anions typically larger or smaller than their corresponding atom? Why?

Which element has the chemical symbol Ru?

All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?

Why doesn't a mass spectrum of silver have a peak at 107.9 u?

Carbon has two naturally occurring isotopes, carbon-12 and carbon-13. The more common isotope of carbon is carbon-12 with an abundance of 98.93% while carbon-13 has an atomic mass of 13.00335 u. Calculate the atomic mass of carbon-12 if the atomic mass of carbon is 12.0107 u.

What mass (in mg) does 2.63 moles of nickel have?

Identify the largest by size atom or ion of carbon.

Identify a cation.

An atom of 31P contains ________ protons.

What species is represented by the following information? p+ = 17 n° = 18 e- = 18

If 102.7 g of tin is mixed with 10.9 g of copper to create the alloy pewter, how many moles of metal are present in the pewter?

Which of the following describes a metal?

In which of the following sets do all species have the same number of electrons?

The mass number of an atom of 67Ga is ________.

Which of the following statements about subatomic particles is TRUE?

Which of the following statements about isotopes is TRUE?

Argon belongs to the ________ group of the periodic table.

Units of Measurement for Physical and Chemical Change

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

An atom of ³¹P contains ________ protons.

What species is represented by the following information? p⁺ = 17 n° = 18 e^- = 18

The mass number of an atom of ⁶⁷Ga is ________.