Question 1

The formula of palladium(IV)sulfide is __________.

Accepted Answer

A) Pd2S4 
B) PdS4 
C) Pd4S 
D) PdS2 
E) Pd2S2 
A) Pd2S4 
B) PdS4 
C) Pd4S 
D) PdS2 
E) Pd2S2

Question 2

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

Accepted Answer

A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) stays the same, increases 
E) increases, stays the same 
A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) stays the same, increases 
E) increases, stays the same

Question 3

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

Accepted Answer

A) PO43- 
B) SiF4 
C) CF4 
D) SeF4 
E) NF3 
A) PO43- 
B) SiF4 
C) CF4 
D) SeF4 
E) NF3

Question 4

Most transition metals do not form ions with a noble gas configuration.

Accepted Answer

A) True 
 B)False

Question 5

For a given arrangement of ions, the lattice energy decreases as ionic radius __________ and as ionic charge __________.

Accepted Answer

A) decreases, increases 
B) increases, decreases 
C) increases, increases 
D) decreases, decreases 
E) This cannot be predicted. 
A) decreases, increases 
B) increases, decreases 
C) increases, increases 
D) decreases, decreases 
E) This cannot be predicted.

Question 6

Which energy change corresponds to the first ionization energy of potassium?

Accepted Answer

A) 2 
B) 5 
C) 4 
D) 3 
E) 6 
A) 2 
B) 5 
C) 4 
D) 3 
E) 6

Question 7

The central atom in __________ does not violate the octet rule.

Accepted Answer

A) SF4 
B) KrF2 
C) CF4 
D) XeF4 
E) ICl4- 
A) SF4 
B) KrF2 
C) CF4 
D) XeF4 
E) ICl4-

Question 8

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?

Accepted Answer

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

Question 9

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10-30 coulomb-meters; e=1.6 × 10-19 coulombs)

Accepted Answer

A) 1.6 × 10-19 
B) 0.057 
C) 9.1 
D) 1 
E) 0.22 
A) 1.6 × 10-19 
B) 0.057 
C) 9.1 
D) 1 
E) 0.22

Question 10

Bond enthalpy is __________.

Accepted Answer

A) always positive 
B) always negative 
C) sometimes positive, sometimes negative 
D) always zero 
E) unpredictable 
A) always positive 
B) always negative 
C) sometimes positive, sometimes negative 
D) always zero 
E) unpredictable

Question 11

Electropositivity __________ from left to right within a period and __________ from top to bottom within a group.

Accepted Answer

A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) stays the same, increases 
E) increases, stays the same 
A) decreases, increases 
B) increases, increases 
C) increases, decreases 
D) stays the same, increases 
E) increases, stays the same

Question 12

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2?

Accepted Answer

A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. 
B) There aren't enough electrons. 
C) That would result in more than eight electrons around beryllium. 
D) That would result in more than eight electrons around each chlorine atom. 
E) That would result in the formal charges not adding up to zero. 
A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. 
B) There aren't enough electrons. 
C) That would result in more than eight electrons around beryllium. 
D) That would result in more than eight electrons around each chlorine atom. 
E) That would result in the formal charges not adding up to zero.

Question 13

A triple bond consists of __________ pairs of electrons shared between two atoms.

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 6 
A) 1 
B) 2 
C) 3 
D) 4 
E) 6

Question 14

There are __________ paired and __________ unpaired electrons in the Lewis symbol for a chlorine atom.

Accepted Answer

A) 4, 2 
B) 4, 1 
C) 6, 1 
D) 0, 5 
E) 2, 5 
A) 4, 2 
B) 4, 1 
C) 6, 1 
D) 0, 5 
E) 2, 5

Question 15

Using the table of average bond energies below, the △H for the reaction is __________ kJ. C≡O (g)+ 2H2 (g)→ H3C-O-H (g)
Bond: C-O C=O C≡O C-H H-H O-H
D (kJ/mol): 358 799 1072 413 436 463

Accepted Answer

A) +276 
B) -276 
C) +735 
D) -735 
E) -116 
A) +276 
B) -276 
C) +735 
D) -735 
E) -116

Question 16

Of the molecules below, the bond in __________ is the most polar.

Accepted Answer

A) HBr 
B) HI 
C) HCl 
D) HF 
E) H2 
A) HBr 
B) HI 
C) HCl 
D) HF 
E) H2

Question 17

Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br

Accepted Answer

A) O, Se 
B) Sr 
C) Na 
D) Br 
E) Sr, O, Se 
A) O, Se 
B) Sr 
C) Na 
D) Br 
E) Sr, O, Se

Question 18

Write the balanced chemical equation for the reaction for which ΔH˚rxn is the lattice energy for potassium bromide.

Accepted Answer

KBr (s)→ K

Question 19

There can be four equivalent best resonance structures of __________.

Accepted Answer

A) (i) 
B) (ii) 
C) (iii) 
D) (iv) 
E) (v) 
A) (i) 
B) (ii) 
C) (iii) 
D) (iv) 
E) (v)

Question 20

Of the following, __________ cannot accommodate more than an octet of electrons.

Accepted Answer

A) Ni 
B) As 
C) C 
D) V 
E) Y 
A) Ni 
B) As 
C) C 
D) V 
E) Y

Exam 8: Basic Concepts of Chemical Bonding

The formula of palladium(IV)sulfide is __________.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

Most transition metals do not form ions with a noble gas configuration.

For a given arrangement of ions, the lattice energy decreases as ionic radius __________ and as ionic charge __________.

Which energy change corresponds to the first ionization energy of potassium?

The central atom in __________ does not violate the octet rule.

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10-30 coulomb-meters; e=1.6 × 10-19 coulombs)

Bond enthalpy is __________.

Electropositivity __________ from left to right within a period and __________ from top to bottom within a group.

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2?

A triple bond consists of __________ pairs of electrons shared between two atoms.

There are __________ paired and __________ unpaired electrons in the Lewis symbol for a chlorine atom.

Using the table of average bond energies below, the △H for the reaction is __________ kJ. C≡O (g)+ 2H2 (g)→ H3C-O-H (g) Bond: C-O C=O C≡O C-H H-H O-H D (kJ/mol): 358 799 1072 413 436 463

Of the molecules below, the bond in __________ is the most polar.

Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br

Write the balanced chemical equation for the reaction for which ΔH˚rxn is the lattice energy for potassium bromide.

There can be four equivalent best resonance structures of __________.

Of the following, __________ cannot accommodate more than an octet of electrons.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Electronegativity from left to right within a period and from top to bottom within a group.

For a given arrangement of ions, the lattice energy decreases as ionic radius and as ionic charge .

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10^-30 coulomb-meters; e=1.6 × 10^-19 coulombs)

Electropositivity from left to right within a period and from top to bottom within a group.

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl₂?

There are paired and unpaired electrons in the Lewis symbol for a chlorine atom.

Using the table of average bond energies below, the △H for the reaction is __________ kJ. C≡O (g)+ 2H₂ (g)→ H₃C-O-H (g) Bond: C-O C=O C≡O C-H H-H O-H D (kJ/mol): 358 799 1072 413 436 463

Write the balanced chemical equation for the reaction for which ΔH˚_rxn is the lattice energy for potassium bromide.