Question 1

The radii of ions are always smaller than the radii of the corresponding atoms of the same element.

Accepted Answer

A) True 
 B)False

Question 2

Which of the elements listed below has the highest first ionization energy?

Accepted Answer

A) C 
B) Ge 
C) P 
D) O 
E) Se 
A) C 
B) Ge 
C) P 
D) O 
E) Se

Question 3

Why is the Mg2+ ion smaller than F-, even though they are isoelectronic?

Accepted Answer

Mg²⁺ has a h

Question 4

Arrange the following ions in order of increasing ionic radius: K+, P3- , S2-, Cl-. increasing radius $\rarr$

Accepted Answer

A) K+ - 2- 3- 
B) K+ 3- 2- - 
C) P3- 2- - + 
D) Cl- 2- 3- + 
E) Cl- 2- + 3- 
A) K+ - 2- 3- 
B) K+ 3- 2- - 
C) P3- 2- - + 
D) Cl- 2- 3- + 
E) Cl- 2- + 3-

Question 5

Which element will display an unusually large jump in ionization energy values between I3 and I4, its third and fourth ionization energies?

Accepted Answer

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

Question 6

The general electron configuration for atoms of all elements in Group 5A is

Accepted Answer

A) ns2np6 
B) ns2np5 
C) ns2np4 
D) ns2np3 
E) ns2np1 
A) ns2np6 
B) ns2np5 
C) ns2np4 
D) ns2np3 
E) ns2np1

Question 7

The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s)$\rarr$ Na+(g)+ e- is therefore

Accepted Answer

A) 495.9 kJ/mol. 
B) less than 495.9 kJ/mol. 
C) greater than 495.9 kJ/mol. 
D) is equal to the electron affinity of sodium. 
E) is equal to the second ionization energy of sodium. 
A) 495.9 kJ/mol. 
B) less than 495.9 kJ/mol. 
C) greater than 495.9 kJ/mol. 
D) is equal to the electron affinity of sodium. 
E) is equal to the second ionization energy of sodium.

Question 8

The sulfide ion, S2-,  is isoelectronic with which one of the following?

Accepted Answer

A) O2- 
B) F- 
C) Na+ 
D) Al3+ 
E) K+ 
A) O2- 
B) F- 
C) Na+ 
D) Al3+ 
E) K+

Question 9

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

Question 10

Consider the following reaction 2A + 3F2 $\rarr$2AF3.What is the formula for the reaction product if we substitute sulfur for fluorine?

Accepted Answer

A) A2S3 
B) A3S2 
C) AS3 
D) A3S 
E) AS 
A) A2S3 
B) A3S2 
C) AS3 
D) A3S 
E) AS

Question 11

Write the ground-state electron configuration for O2-.

Accepted Answer

Question 12

Amphoteric oxides exhibit both acidic and basic properties.

Accepted Answer

A) True 
 B)False

Question 13

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

Accepted Answer

A) Se2- 
B) Br- 
C) Rb+ 
D) Y3+ 
E) Zn2+ 
A) Se2- 
B) Br- 
C) Rb+ 
D) Y3+ 
E) Zn2+

Question 14

Electron affinity is always a positive quantity.

Accepted Answer

A) True 
 B)False

Question 15

Which of the following elements has the greatest metallic character?

Accepted Answer

A) Ca 
B) Mg 
C) Ba 
D) As 
E) Se 
A) Ca 
B) Mg 
C) Ba 
D) As 
E) Se

Question 16

Write the ground-state electron configuration for S2-.

Accepted Answer

Question 17

Given the following melting point data, what is a reasonable estimate of the melting point of potassium.

Accepted Answer

The answer of Given the following melting point data, what...

Question 18

Write the ground-state electron configuration for Mg2+.

Accepted Answer

Question 19

Which of the elements listed below has the smallest first ionization energy?

Accepted Answer

A) C 
B) Ge 
C) P 
D) O 
E) Se 
A) C 
B) Ge 
C) P 
D) O 
E) Se

Question 20

What is the charge on the stable ion formed by selenium?

Accepted Answer

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

Exam 8: Periodic Relationships Among the Elements

The radii of ions are always smaller than the radii of the corresponding atoms of the same element.

Which of the elements listed below has the highest first ionization energy?

Why is the Mg2+ ion smaller than F-, even though they are isoelectronic?

Arrange the following ions in order of increasing ionic radius: K+, P3- , S2-, Cl-. increasing radius →\rarr→

Which element will display an unusually large jump in ionization energy values between I3 and I4, its third and fourth ionization energies?

The general electron configuration for atoms of all elements in Group 5A is

The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s) →\rarr→ Na+(g)+ e- is therefore

The sulfide ion, S2-, is isoelectronic with which one of the following?

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

Consider the following reaction 2A + 3F2 →\rarr→ 2AF3.What is the formula for the reaction product if we substitute sulfur for fluorine?

Write the ground-state electron configuration for O2-.

Amphoteric oxides exhibit both acidic and basic properties.

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

Electron affinity is always a positive quantity.

Which of the following elements has the greatest metallic character?

Write the ground-state electron configuration for S2-.

Given the following melting point data, what is a reasonable estimate of the melting point of potassium.

Write the ground-state electron configuration for Mg2+.

Which of the elements listed below has the smallest first ionization energy?

What is the charge on the stable ion formed by selenium?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Why is the Mg²⁺ ion smaller than F^-, even though they are isoelectronic?

Arrange the following ions in order of increasing ionic radius: K⁺, P^3-, S^2-, Cl^-. increasing radius $\rarr$

Which element will display an unusually large jump in ionization energy values between I₃ and I₄, its third and fourth ionization energies?

The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s) $\rarr$ Na⁺(g)+ e^- is therefore

The sulfide ion, S^2-, is isoelectronic with which one of the following?

Consider the following reaction 2A + 3F₂ $\rarr$ 2AF₃.What is the formula for the reaction product if we substitute sulfur for fluorine?

Write the ground-state electron configuration for O^2-.

Write the ground-state electron configuration for S^2-.

Write the ground-state electron configuration for Mg²⁺.