Chapter 9

Question 1

Strength of repulsion between lone pairs and bonding pairs

Answer 1

two lone pairs>one lone pair>double bond>single bond

Question 2

Seesaw shape #of bonding and lone pairs and steric number

Answer 2

lone pairs: 1
Bonding pairs: 4
SN=5

Question 3

T-Shape geometry

Answer 3

SN=5
Bonding pairs: 3
lone pairs: 2

Question 4

Square pyramidal geometry

Answer 4

SN=6
Bonding pairs: 5
Lone pairs: 1

Question 5

Square planar geometry

Answer 5

SN=6
Bonding pairs: 4
Lone pairs: 2

Question 6

Bent(angular geometry)

Answer 6

2 bonding pairs

Question 7

Sigma bond

Answer 7

Covalent bond in which the highest electron density lies between the two atoms along the bond axis

Question 8

Valence bond theory

Answer 8

Made by Linus Pauling, it states that a covalent bond is the overlap of half filled orbitals

Question 9

Hybridization

Answer 9

The mixing if atomic orbitals to generate new sets of orbitals that form covalent bonds with other atoms

Question 10

Shape of sp3 orbitals

Answer 10

tetrahedral

Question 11

Shape of sp2 hybrid

Answer 11

trigonal planar

Question 12

bonds formed by unhybridized p orbitals

Answer 12

double bonds

Question 13

pi bond

Answer 13

A covalent bond in which electron density is great around(not along) the bonding axis

Question 14

Kekulè structure

Answer 14

Shows all bonds but not lone pairs

Question 15

Condensed structure

Answer 15

No bonds, subscripts indicate number of times a subgroup is repeated

Question 16

Carbon skeleton structure

Answer 16

Zigzag lines, no carbon or H shown

Question 17

Delocalization

Answer 17

Spreading of electrons in alternating single and double bonds over 3 or more atoms in a molecule

Question 18

Aromatic compound

Answer 18

Cyclic, planar compound with delocalized pi electrons above and below the plane of the molecule

Question 19

Molecular Orbital Theory

Answer 19

Based mixing atomic orbitals of similar shapes and energies to form molecular orbitals that extend across 2 or more atoms. # of MO=number of atomic orbitals total. MOs represent discrete energy states and orbitals spread out over entire molecule

Question 20

Bonding vs Antibonding orbitals

Answer 20

Bonding: Region of increased electron density between nuclear centers that hold atoms together, lower energy, more stable

Antibonding: Region of electron density that destabilizes the molecule because they do not increase electron density between nuclear centers, less stable

Question 21

Bond order

Answer 21

1/2(bonding e- - antibonding e-)

Question 22

Paramagnetism

Answer 22

Atoms or molecules having unpaired e- are attracted to magnetic fields

Question 23

Diamagnetism

Answer 23

Atoms or molecules having all paired e- are repelled by magnetic fields

Question 24

0 nodes

Answer 24

sigma, bodning

Question 25

1 vertical node

Answer 25

antibonding sigma

Question 26

1 horizontal node

Answer 26

bonding pi

Question 27

2 nodes, 1 horizontal 1 vertical

Answer 27

antibonding pi

Question 28

Trigonal pyramidal

Answer 28

3 Bonding pairs

1 Lone pair