Ch. 9 Chemical Bonding II

Question 1

Electrons act as _____. Either bonding or lone pairs.

Answer 1

Domains

Question 2

Electron domain geometries and molecular structures are determined by _____ the distance between electron domains and thereby minimizing repulsion between them.

Answer 2

Maximizing

Question 3

Two electron domains is linear and has a bond angle of?

Answer 3

180

Question 4

Three electron domains is trigonal planar and has a bond angle of?

Answer 4

120

Question 5

Four electron domains is tetrahedral and has a bond angle of?

Answer 5

109.5

Question 6

Five electron domains is trigonal bipyramidal and has a bond angle of?

Answer 6

120

90

Question 7

6 electron domains is octahedral and has a bond angle of?

Answer 7

90

Question 8

The bond angle between bonding domains decreases as he number of lone pairs ______.

Answer 8

Increases

Question 9

The lone pairs reside closer to the central atom and push the adjacent bonds ______ ______.

Answer 9

Closer together

Question 10

In a trigonal biopyramidal the lone pairs prefer the ____ position to the axial position.

Answer 10

Equatorial

Question 11

This is the property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative.

Answer 11

Dipole moment

Question 12

A dipole moment is represented by an arrow also known as a ____.

Answer 12

Vector

Question 13

A vector points to the negative charge center with the tail of the arrow indicating the ____ center of the charge.

Answer 13

Positive

Question 14

Dipole moment points toward the more ______ atom.

Answer 14

Electronegative

Question 15

Covalent bonds are described using the atomic orbitals of valence electrons. Atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on the other. Each overlapping atomic orbital
Must contain a single unpaired electron and have opposite spin.

Answer 15

Valence bond theory

Question 16

Single bonds are also called ____ bonds.

Answer 16

Sigma

Question 17

A covalent bond in which two atoms share 3 pairs of electrons is indicated with a ____ dash.

Answer 17

Triple

Question 18

Triple bonds are comprised of one ____ and 2 ____ bonds overlapping of two pairs of p orbitals)

Answer 18

Sigma

Pie

Question 19

A covalent bond in which two atoms share two pairs of electrons is indicated by a ____ dash.

Answer 19

Double

Question 20

Double bonds are comprised of one _____ and one _____ bond (overlap of 2 p orbitals)

Answer 20

Sigma

Pie

Question 21

What is the hybridization required for 2 electron domains?

Answer 21

sp

Question 22

What is the hybridization required for 3 electron domains?

Answer 22

sp2

Question 23

What is the hybridization required for 4 electron domains?

Answer 23

sp3

Question 24

What is the hybridization required for 5 electron domains?

Answer 24

dsp3

Question 25

What is the hybridization required for 6 electron domains?

Answer 25

d2sp3

Question 26

Species that contain one or more unpaired electrons and that are attracted by magnetic fields are?

Answer 26

Paramagnetic

Question 27

Species in which all the electrons are paired and repelled by magnetic fields are?

Answer 27

Diamagnetic

Question 28

Diamagnetism is a much ____ effect.

Answer 28

weaker

Question 29

Paramagnetic and diamagnetic properties are the result of a molecules _____ _____.

Answer 29

Electron Configuration

Question 30

Atomic orbitals combine t form new orbitals that are the "property" of the entire molecule not just the property of the atoms forming bonds. Shared electrons reside in molecular orbits. This is what theory?

Answer 30

Molecular Orbital theory

Question 31

This is is the number of chemical bonds between a pair of atoms.

Answer 31

Bond Order

Question 32

The value of the bond order is a qualitative measure of a molecules ____.

Answer 32

Stability

Question 33

A molecule with a positive bond order is ____. | A molecule with a zero or negative bond order is ____.

Answer 33

Stable | Not Stable

Question 34

Lower- energy orbitals fill first is what principle?

Answer 34

Aufbau Principle

Question 35

Each orbital can accommodate a maximum of 2 electrons with opposite spins is which principle?

Answer 35

Pauli Exclusion Principle

Question 36

Electrons are placed in separate degenerate orbitals before they are paired up is which rule?

Answer 36

Hund's Rule

Question 37

What is the equation for determining bond order?

Answer 37

bond order = # of electrons in bonding orbitals- #of electrons in anti bonding molecular orbitals Divided by 2

Question 38

Antibonding molecular orbitals are identified by what?

Answer 38

*