Question 1

Choose the INCORRECT statement.

Accepted Answer

A) Within a given subshell,each orbital is usually occupied by a single electron before any orbital has two electrons. 
B) When a metallic element unites with a nonmetallic element,electrons are lost by atoms of the metal and gained by atoms of the nonmetals. 
C) The noble gas atoms complete the filling of the p orbitals. 
D) The ionization energy of Ca+ is greater than that for Ca2+. 
E) The radius of Ba2+ is smaller than the radius of Ba+. 
A) Within a given subshell,each orbital is usually occupied by a single electron before any orbital has two electrons. 
B) When a metallic element unites with a nonmetallic element,electrons are lost by atoms of the metal and gained by atoms of the nonmetals. 
C) The noble gas atoms complete the filling of the p orbitals. 
D) The ionization energy of Ca+ is greater than that for Ca2+. 
E) The radius of Ba2+ is smaller than the radius of Ba+.

Question 2

Polarizability decreases with the size of the atom.

Accepted Answer

A) True 
 B)False

Question 3

Which ionization process requires the most energy?

Accepted Answer

A) O(g)→ O+(g)+ e- 
B) O+(g)→ O2+(g)+ e- 
C) F(g)→ F+(g)+ e- 
D) F+(g)→ F2+(g)+ e- 
A) O(g)→ O+(g)+ e- 
B) O+(g)→ O2+(g)+ e- 
C) F(g)→ F+(g)+ e- 
D) F+(g)→ F2+(g)+ e-

Question 4

Which of the following has the most negative electron affinity: Li,Be,N,O,F?

Accepted Answer

A) Li 
B) Be 
C) N 
D) O 
E) F 
A) Li 
B) Be 
C) N 
D) O 
E) F

Question 5

List in order of increasing atomic size: F,Na,K,Mg,Ne.

Accepted Answer

A) K < Mg < Ne < Na < F 
B) Ne < Mg < K < Na < F 
C) Ne < F < Mg < Na < K 
D) Mg < F < Ne < Na < K 
E) K < Na < Mg < F < Ne 
A) K < Mg < Ne < Na < F 
B) Ne < Mg < K < Na < F 
C) Ne < F < Mg < Na < K 
D) Mg < F < Ne < Na < K 
E) K < Na < Mg < F < Ne

Question 6

The first ionization energy for rubidium is +403.0 kJ/mol.How much energy would be required to convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?

Accepted Answer

A) 185 kJ 
B) 80.6 kJ 
C) 68.9 kJ 
D) 40.4 kJ 
E) 34.5 kJ 
A) 185 kJ 
B) 80.6 kJ 
C) 68.9 kJ 
D) 40.4 kJ 
E) 34.5 kJ

Question 7

List in order of increasing ionization potential: O,Mg,Rb,S,Si.

Accepted Answer

A) Si < O < Mg < Rb < S 
B) Si < S < Rb < Mg < O 
C) Mg < O < Rb < S < Si 
D) Rb < Mg < Si < S < O 
E) S < Si < Mg < O < Rb 
A) Si < O < Mg < Rb < S 
B) Si < S < Rb < Mg < O 
C) Mg < O < Rb < S < Si 
D) Rb < Mg < Si < S < O 
E) S < Si < Mg < O < Rb

Question 8

Which of the following species will have the highest ionization energy?

Accepted Answer

A) K+ 
B) Ar 
C) Cl- 
D) S2- 
A) K+ 
B) Ar 
C) Cl- 
D) S2-

Question 9

Which of the following reactions gives a positive value for the electron affinity?

Accepted Answer

A) S-(g)+ e- → S2-(g) 
B) O(g)+ e- → O-(g) 
C) S(g)+ e- → S-(g) 
D) Br(g)+ e- → Br-(g) 
A) S-(g)+ e- → S2-(g) 
B) O(g)+ e- → O-(g) 
C) S(g)+ e- → S-(g) 
D) Br(g)+ e- → Br-(g)

Question 10

Which of the following pairs of elements are classified as metalloids?

Accepted Answer

A) aluminum and silicon 
B) argon and neon 
C) arsenic and germanium 
D) bromine and sulfur 
E) copper and silver 
A) aluminum and silicon 
B) argon and neon 
C) arsenic and germanium 
D) bromine and sulfur 
E) copper and silver

Question 11

Can alkali metal atoms form negative ions in the gaseous state? Explain.

Accepted Answer

A) No,an electron cannot be added. 
B) No,only a liquid can be ionized. 
C) Yes,an electron can be added to a Li half-filled 2s orbital. 
D) Yes,an electron can be removed from a Li half-filled 2s orbital. 
E) No,the 2s orbital is completely filled. 
A) No,an electron cannot be added. 
B) No,only a liquid can be ionized. 
C) Yes,an electron can be added to a Li half-filled 2s orbital. 
D) Yes,an electron can be removed from a Li half-filled 2s orbital. 
E) No,the 2s orbital is completely filled.

Question 12

Which of the following could never be isoelectronic species?

Accepted Answer

A) anions of two different elements 
B) cations of two different elements 
C) an anion and a cation 
D) an anion and an atom 
E) atoms of two different elements 
A) anions of two different elements 
B) cations of two different elements 
C) an anion and a cation 
D) an anion and an atom 
E) atoms of two different elements

Question 13

The ion represented as  Ti4+ has:

Accepted Answer

A) 22 electrons 
B) 48 neutrons 
C) 26 protons 
D) 4 3d electrons 
E) 0 4s electrons 
A) 22 electrons 
B) 48 neutrons 
C) 26 protons 
D) 4 3d electrons 
E) 0 4s electrons

Question 14

Which of the following has the smallest value of the first ionization energy: Ar,Cs,N,Cu,Rb?

Accepted Answer

A) Ar 
B) Cs 
C) N 
D) Cu 
E) Rb 
A) Ar 
B) Cs 
C) N 
D) Cu 
E) Rb

Question 15

The energy difference between atomic cesium and its most stable ion,in the gaseous state,is referred to as ________.

Accepted Answer

A) atomic energy 
B) electron affinity 
C) entropy of vaporization 
D) ionization energy 
E) magnetic moment 
A) atomic energy 
B) electron affinity 
C) entropy of vaporization 
D) ionization energy 
E) magnetic moment

Question 16

What is the general valence electronic configuration (where n = principal quantum number)that best describes the halogens as a group?

Accepted Answer

A) ns1np6  
B) ns2np4  
C) ns2np5  
D) ns2np6  
E) ns2np3  
A) ns1np6  
B) ns2np4  
C) ns2np5  
D) ns2np6  
E) ns2np3

Question 17

List in order of increasing number of unpaired electrons: N,Na,Si,Cr,Ar.

Accepted Answer

A) Cr < Si < Na < N < Ar 
B) Ar < Cr < N < Na < Si 
C) Ar < Cr < Si < Na < N 
D) N < Na < Cr < Si < Ar 
E) Ar < Na < Si < N < Cr 
A) Cr < Si < Na < N < Ar 
B) Ar < Cr < N < Na < Si 
C) Ar < Cr < Si < Na < N 
D) N < Na < Cr < Si < Ar 
E) Ar < Na < Si < N < Cr

Question 18

The transition elements refer to what group of elements?

Accepted Answer

A) s-block elements 
B) d-block elements 
C) actinides 
D) lanthanides 
E) p-block elements 
A) s-block elements 
B) d-block elements 
C) actinides 
D) lanthanides 
E) p-block elements

Question 19

Of the following,which atom has the largest atomic radius?

Accepted Answer

A) Rb 
B) I 
C) Cs 
D) At 
A) Rb 
B) I 
C) Cs 
D) At

Question 20

Which 1+ ion is isoelectronic with S2-?

Accepted Answer

Exam 9: The Periodic Table and Some Atomic Properties

Choose the INCORRECT statement.

Polarizability decreases with the size of the atom.

Which ionization process requires the most energy?

Which of the following has the most negative electron affinity: Li,Be,N,O,F?

List in order of increasing atomic size: F,Na,K,Mg,Ne.

The first ionization energy for rubidium is +403.0 kJ/mol.How much energy would be required to convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?

List in order of increasing ionization potential: O,Mg,Rb,S,Si.

Which of the following species will have the highest ionization energy?

Which of the following reactions gives a positive value for the electron affinity?

Which of the following pairs of elements are classified as metalloids?

Can alkali metal atoms form negative ions in the gaseous state? Explain.

Which of the following could never be isoelectronic species?

The ion represented as Ti4+ has:

Which of the following has the smallest value of the first ionization energy: Ar,Cs,N,Cu,Rb?

The energy difference between atomic cesium and its most stable ion,in the gaseous state,is referred to as ________.

What is the general valence electronic configuration (where n = principal quantum number)that best describes the halogens as a group?

List in order of increasing number of unpaired electrons: N,Na,Si,Cr,Ar.

The transition elements refer to what group of elements?

Of the following,which atom has the largest atomic radius?

Which 1+ ion is isoelectronic with S2-?

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

The ion represented as Ti⁴⁺ has:

Which 1+ ion is isoelectronic with S^2-?