Question 1

Which of the following is the electron configuration of a sulfide ion?

Accepted Answer

A) [Ne]3s23p4 
B) [Ne] 
C) [Ne]3s23p1 
D) [Ar] 
E) [Ne]3s23p2 
A) [Ne]3s23p4 
B) [Ne] 
C) [Ne]3s23p1 
D) [Ar] 
E) [Ne]3s23p2 D

Question 2

The law of octaves states that every eighth element has similar properties when arranged in order of increasing

Accepted Answer

A) nuclear binding energy. 
B) number of electrons. 
C) number of neutrons. 
D) atomic mass. 
E) atomic number. 
A) nuclear binding energy. 
B) number of electrons. 
C) number of neutrons. 
D) atomic mass. 
E) atomic number. D

Question 3

The successive ionization energies of a certain element are I1 = 589.5 kJ/mol, I2 =1145 kJ/mol, I3= 4900 kJ/mol, I4 = 6500 kJ/mol, and I5 = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is

Accepted Answer

A) K. 
B) Si. 
C) As. 
D) Ca. 
E) S. 
A) K. 
B) Si. 
C) As. 
D) Ca. 
E) S. D

Question 4

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l)$\rarr$ Hg+(g)+ e- is therefore

Accepted Answer

A) 1006 kJ/mol. 
B) greater than 1006 kJ/mol. 
C) less than 1006 kJ/mol. 
D) is equal to the electron affinity of mercury. 
E) is equal to the second ionization energy of mercury. 
A) 1006 kJ/mol. 
B) greater than 1006 kJ/mol. 
C) less than 1006 kJ/mol. 
D) is equal to the electron affinity of mercury. 
E) is equal to the second ionization energy of mercury.

Question 5

The alkali metal elements are found in _______ of the periodic table.

Accepted Answer

A) Group 1A 
B) Group 2A 
C) Group 3A 
D) Period 7 
E) Period 1 
A) Group 1A 
B) Group 2A 
C) Group 3A 
D) Period 7 
E) Period 1

Question 6

For phosphorus atoms, which ionization energy will show an exceptionally large increase over the previous ionization energy?

Accepted Answer

A) 2nd 
B) 3rd 
C) 4th 
D) 5th 
E) 6th 
A) 2nd 
B) 3rd 
C) 4th 
D) 5th 
E) 6th

Question 7

Which of the atoms listed below has the smallest radius?

Accepted Answer

A) Al 
B) P 
C) As 
D) Te 
E) Na 
A) Al 
B) P 
C) As 
D) Te 
E) Na

Question 8

Which of the following ground-state ions has unpaired electrons?

Accepted Answer

A) P3- 
B) V5+ 
C) Mg2+ 
D) Sc2+ 
E) S2+ 
A) P3- 
B) V5+ 
C) Mg2+ 
D) Sc2+ 
E) S2+

Question 9

Which of the following elements behaves chemically similarly to silver?

Accepted Answer

A) nickel 
B) gold 
C) sulfur 
D) chlorine 
E) iron
F)beryllium 
A) nickel 
B) gold 
C) sulfur 
D) chlorine 
E) iron
F)beryllium

Question 10

Which one of the following does not have [Xe] as its electronic configuration?

Accepted Answer

A) Te2- 
B) I- 
C) Cs+ 
D) Ba2+ 
E) Sn4+ 
A) Te2- 
B) I- 
C) Cs+ 
D) Ba2+ 
E) Sn4+

Question 11

Arrange the following ions in order of decreasing ionic radius: Al3+, Mg2+, Na+, O2-. decreasing radius $\rarr$

Accepted Answer

A) Al3+ > Mg2+ > O2- > Na+ 
B) Al3+ > Mg2+ > Na+ > O2- 
C) Na+ > Mg2+ > Al3+ > O2- 
D) O2- > Al3+ > Mg2+ > Na+ 
E) O2- > Na+ > Mg2+ > Al3+ 
A) Al3+ > Mg2+ > O2- > Na+ 
B) Al3+ > Mg2+ > Na+ > O2- 
C) Na+ > Mg2+ > Al3+ > O2- 
D) O2- > Al3+ > Mg2+ > Na+ 
E) O2- > Na+ > Mg2+ > Al3+

Question 12

Which of the following elements has the greatest metallic character?

Accepted Answer

A) Br 
B) F 
C) Ge 
D) Mn 
E) Sc 
A) Br 
B) F 
C) Ge 
D) Mn 
E) Sc

Question 13

In a surprisingly large number of their properties, beryllium resembles aluminum and boron resembles silicon. Such a relationship is called

Accepted Answer

A) amphoterism. 
B) an allotropic relationship. 
C) a diagonal relationship. 
D) the periodic law. 
E) an isoelectronic series. 
A) amphoterism. 
B) an allotropic relationship. 
C) a diagonal relationship. 
D) the periodic law. 
E) an isoelectronic series.

Question 14

Which of the following make an isoelectronic pair: Cl- , O2-, F, Ca2+, Fe3+?

Accepted Answer

A) Ca2+ and Fe3+ 
B) O2-  and F 
C) F and Cl- 
D) Cl-  and Ca2+ 
E) None of the above. 
A) Ca2+ and Fe3+ 
B) O2-  and F 
C) F and Cl- 
D) Cl-  and Ca2+ 
E) None of the above.

Question 15

Which of the following elements has the greatest electron affinity (largest positive value)?

Accepted Answer

A) Mg 
B) Al 
C) Si 
D) P 
E) S 
A) Mg 
B) Al 
C) Si 
D) P 
E) S

Question 16

Which of the atoms listed below has the largest radius?

Accepted Answer

A) Cl 
B) I 
C) P 
D) Sb 
E) Se 
A) Cl 
B) I 
C) P 
D) Sb 
E) Se

Question 17

Electron affinity is always a positive quantity.

Accepted Answer

A) True 
 B)False

Question 18

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

Accepted Answer

A) nuclear binding energy. 
B) number of neutrons. 
C) atomic mass. 
D) atomic number. 
E) atomic size. 
A) nuclear binding energy. 
B) number of neutrons. 
C) atomic mass. 
D) atomic number. 
E) atomic size.

Question 19

Consider the following reaction: 3Li + Z $\rarr$ Li3Z. What is the formula for the compound if we substitute magnesium for lithium?

Accepted Answer

A) MgZ 
B) Mg2Z 
C) MgZ2 
D) Mg3Z 
E) Mg3Z2 
A) MgZ 
B) Mg2Z 
C) MgZ2 
D) Mg3Z 
E) Mg3Z2

Question 20

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

Accepted Answer

A) X has a larger electron affinity than Y does. 
B) X has a larger effective nuclear charge than Y does. 
C) X has greater metallic character than Y does. 
D) X has a larger first ionization energy than Y does. 
E) X is a poorer conductor of electricity than Y when in the solid state. 
A) X has a larger electron affinity than Y does. 
B) X has a larger effective nuclear charge than Y does. 
C) X has greater metallic character than Y does. 
D) X has a larger first ionization energy than Y does. 
E) X is a poorer conductor of electricity than Y when in the solid state.

Exam 8: The Periodic Table

Which of the following is the electron configuration of a sulfide ion?

The law of octaves states that every eighth element has similar properties when arranged in order of increasing

The successive ionization energies of a certain element are I1 = 589.5 kJ/mol, I2 =1145 kJ/mol, I3= 4900 kJ/mol, I4 = 6500 kJ/mol, and I5 = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) →\rarr→ Hg+(g)+ e- is therefore

The alkali metal elements are found in _______ of the periodic table.

For phosphorus atoms, which ionization energy will show an exceptionally large increase over the previous ionization energy?

Which of the atoms listed below has the smallest radius?

Which of the following ground-state ions has unpaired electrons?

Which of the following elements behaves chemically similarly to silver?

Which one of the following does not have [Xe] as its electronic configuration?

Arrange the following ions in order of decreasing ionic radius: Al3+, Mg2+, Na+, O2-. decreasing radius →\rarr→

Which of the following elements has the greatest metallic character?

In a surprisingly large number of their properties, beryllium resembles aluminum and boron resembles silicon. Such a relationship is called

Which of the following make an isoelectronic pair: Cl- , O2-, F, Ca2+, Fe3+?

Which of the following elements has the greatest electron affinity (largest positive value)?

Which of the atoms listed below has the largest radius?

Electron affinity is always a positive quantity.

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

Consider the following reaction: 3Li + Z →\rarr→ Li3Z. What is the formula for the compound if we substitute magnesium for lithium?

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

The successive ionization energies of a certain element are I₁= 589.5 kJ/mol, I₂=1145 kJ/mol, I₃= 4900 kJ/mol, I₄ = 6500 kJ/mol, and I₅ = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) $\rarr$ Hg⁺(g)+ e^- is therefore

Arrange the following ions in order of decreasing ionic radius: Al³⁺, Mg²⁺, Na⁺, O^2-. decreasing radius $\rarr$

Which of the following make an isoelectronic pair: Cl^-, O^2-, F, Ca²⁺, Fe³⁺?

Consider the following reaction: 3Li + Z $\rarr$ Li₃Z. What is the formula for the compound if we substitute magnesium for lithium?