Question 1

How many s-sp2 sigma bonds are in the following compound?

Accepted Answer

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

Question 2

What is the approximate bond angle around sulfur atom in Cl2CO?

Accepted Answer

A)  900 
B)  109.50 
C)  1050 
D)  1200 
E)  1800 
A)  900 
B)  109.50 
C)  1050 
D)  1200 
E)  1800

Question 3

What is the approximate bond angle around the indicated carbon atom?

Accepted Answer

A)  600 
B)  900 
C)  109.50 
D)  1200 
E)  1800 
A)  600 
B)  900 
C)  109.50 
D)  1200 
E)  1800

Question 4

Which of the following compounds have both polar covalent and ionic bonds?

Accepted Answer

A)  NH4Br 
B)  H2O2 
C)  HCN 
D)  H2S 
E)  None of these. 
A)  NH4Br 
B)  H2O2 
C)  HCN 
D)  H2S 
E)  None of these.

Question 5

Destructive interference of waves results in_______.

Accepted Answer

A)  a wave with smaller amplitude 
B)  a wave with larger amplitude 
C)  cancellation of both waves 
D)  formation of a node 
E)  Both C and D 
A)  a wave with smaller amplitude 
B)  a wave with larger amplitude 
C)  cancellation of both waves 
D)  formation of a node 
E)  Both C and D

Question 6

What is the correct Lewis structure for nitric acid, HNO3, including the formal charges?

Accepted Answer

A)  I 
B)  II 
C)  III 
D)  IV 
E)  None of these 
A)  I 
B)  II 
C)  III 
D)  IV 
E)  None of these

Question 7

What is the hybridization state and molecular geometry around the sulfur atom in SO3?

Accepted Answer

A)  sp2, tetrahedral 
B)  sp2, trigonal planar 
C)  sp3, tetrahedral 
D)  sp3, trigonal pyramidal 
E)  sp2, trigonal pyramidal 
A)  sp2, tetrahedral 
B)  sp2, trigonal planar 
C)  sp3, tetrahedral 
D)  sp3, trigonal pyramidal 
E)  sp2, trigonal pyramidal

Question 8

Which of the intermolecular forces listed below is generally considered the strongest?

Accepted Answer

A)  London dispersion forces 
B)  fleeting dipole-dipole interactions 
C)  dipole-dipole interactions 
D)  hydrogen bonding 
E)  the vital force 
A)  London dispersion forces 
B)  fleeting dipole-dipole interactions 
C)  dipole-dipole interactions 
D)  hydrogen bonding 
E)  the vital force

Question 9

What is the correct Lewis dot structure for C?

Accepted Answer

A)  I 
B)  II 
C)  III 
D)  IV 
E)  V 
A)  I 
B)  II 
C)  III 
D)  IV 
E)  V

Question 10

The sigma bond that is part of C=C in the following compound results from the overlap of which orbitals?

Accepted Answer

A)  sp-sp2 
B)  sp-sp3 
C)  sp2-sp2 
D)  sp2-sp3 
E)  sp3-sp2 
A)  sp-sp2 
B)  sp-sp3 
C)  sp2-sp2 
D)  sp2-sp3 
E)  sp3-sp2

Question 11

Draw the Lewis structure for NH2CN including formal charges, if any?

Accepted Answer

Question 12

Which of the following compounds have bent molecular geometry?

Accepted Answer

A)  I 
B)  II 
C)  III 
D)  IV 
E)  I and IV 
A)  I 
B)  II 
C)  III 
D)  IV 
E)  I and IV

Question 13

Which of the following structures have a formal charge on at least one atom?

Accepted Answer

A)  I 
B)  II 
C)  III 
D)  IV 
E)  None of these 
A)  I 
B)  II 
C)  III 
D)  IV 
E)  None of these

Question 14

Interaction of the following two atomic orbitals results in what kind of molecular orbital, in the orientation shown?

Accepted Answer

pi antibon

Question 15

Which compound does not have a linear molecular geometry?

Accepted Answer

A)  CO2 
B)  H2O 
C)  BeCl2 
D)  HCN 
E)  C2H2 
A)  CO2 
B)  H2O 
C)  BeCl2 
D)  HCN 
E)  C2H2

Question 16

Rank the following compounds in decreasing order of boiling point.

Accepted Answer

A)  III > I > IV > II 
B)  II > IV > III > I 
C)  III > I > II > IV 
D)  IV > II > I > III 
E)  I > III > II > IV 
A)  III > I > IV > II 
B)  II > IV > III > I 
C)  III > I > II > IV 
D)  IV > II > I > III 
E)  I > III > II > IV

Question 17

How are electrons distributed in the molecular orbitals, when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?

Accepted Answer

A)  two electrons in the bonding molecular orbital 
B)  one electron in the bonding molecular orbital, one electron in the non-bonding molecular orbital 
C)  one electron in the bonding molecular orbital, one electron in the antibonding molecular orbital 
D)  two electrons in the antibonding molecular orbital 
E)  two electrons in the non-bonding molecular orbital 
A)  two electrons in the bonding molecular orbital 
B)  one electron in the bonding molecular orbital, one electron in the non-bonding molecular orbital 
C)  one electron in the bonding molecular orbital, one electron in the antibonding molecular orbital 
D)  two electrons in the antibonding molecular orbital 
E)  two electrons in the non-bonding molecular orbital

Question 18

Which of the following compounds has no dipole moment?

Accepted Answer

A)  CH4 
B)  NH3 
C)  HF 
D)  HCl 
E)  HBr 
A)  CH4 
B)  NH3 
C)  HF 
D)  HCl 
E)  HBr

Question 19

Which intermolecular force is generally considered the weakest?

Accepted Answer

A)  ion-dipole interactions 
B)  London dispersion forces 
C)  dipole-dipole interactions 
D)  hydrogen bonding 
E)  covalent bonding 
A)  ion-dipole interactions 
B)  London dispersion forces 
C)  dipole-dipole interactions 
D)  hydrogen bonding 
E)  covalent bonding

Question 20

Ar, K+, and Cl- have equal numbers of electrons, and are considered isoelectronic. Provide the ground state electron configuration for them.

Accepted Answer

Exam 1: A Review of General Chemistry: Electrons, Bonds, and Molecular Properties

How many s-sp2 sigma bonds are in the following compound?

What is the approximate bond angle around sulfur atom in Cl2CO?

What is the approximate bond angle around the indicated carbon atom?

Which of the following compounds have both polar covalent and ionic bonds?

Destructive interference of waves results in_______.

What is the correct Lewis structure for nitric acid, HNO3, including the formal charges?

What is the hybridization state and molecular geometry around the sulfur atom in SO3?

Which of the intermolecular forces listed below is generally considered the strongest?

What is the correct Lewis dot structure for C?

The sigma bond that is part of C=C in the following compound results from the overlap of which orbitals?

Draw the Lewis structure for NH2CN including formal charges, if any?

Which of the following compounds have bent molecular geometry?

Which of the following structures have a formal charge on at least one atom?

Interaction of the following two atomic orbitals results in what kind of molecular orbital, in the orientation shown?

Which compound does not have a linear molecular geometry?

Rank the following compounds in decreasing order of boiling point.

How are electrons distributed in the molecular orbitals, when the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule?

Which of the following compounds has no dipole moment?

Which intermolecular force is generally considered the weakest?

Ar, K+, and Cl- have equal numbers of electrons, and are considered isoelectronic. Provide the ground state electron configuration for them.

Molecular Representations

Acids and Bases

Alkanes and Cycloalkanes

Stereoisomerism

Chemical Reactivity and Mechanisms

Alkyl Halides: Nucleophilic Substitution and Elimination Reactions

Addition Reactions of Alkenes

Alkynes

Radical Reactions

Synthesis

Alcohols and Phenols

Ethers and Epoxides; Thiols and Sulfides

Infrared Spectroscopy and Mass Spectrometry

Nuclear Magnetic Resonance Spectroscopy

Conjugated Pi Systems and Pericyclic Reactions

Aromatic Compounds

Aromatic Substitution Reactions

Aldehydes and Ketones

Carboxylic Acids and Their Derivatives

Alpha Carbon Chemistry: Enols and Enolates

Amines

Introduction to Organometallic Compounds

Carbohydrates

Amino Acids, Peptides, and Proteins

Lipids

Synthetic Polymers

Filters

How many s-sp² sigma bonds are in the following compound?

What is the approximate bond angle around sulfur atom in Cl₂CO?

What is the correct Lewis structure for nitric acid, HNO₃, including the formal charges?

What is the hybridization state and molecular geometry around the sulfur atom in SO₃?

Draw the Lewis structure for NH₂CN including formal charges, if any?

Ar, K⁺, and Cl^- have equal numbers of electrons, and are considered isoelectronic. Provide the ground state electron configuration for them.