Chapter 2

Question 1

what is a molecule

Answer 1

consist of multiple molecules (like or unlike) bonded together

Question 2

1 mole (Avogadro’s number)

Answer 2

6.022 x 10^23

Question 3

octet rule

Answer 3

each atom will act in such a way to obtain 8 electrons in its valence shell

Question 4

2 main intramolecular forces

Answer 4

ionic and covalent bonds

Question 5

ionic bonds

Answer 5

strong chemical bonds that hold together ions electrons are completely transferred from the cation to the anion metals tend to form ionic bonds with non metals

Question 6

covalent bonds

Answer 6

involves the sharing of an electron pair between 2 atoms

Question 7

non polar covalent bonds

Answer 7

form between atoms that have very similar or identical electronegativity values

Question 8

polar covalent bonds

Answer 8

form between atoms where the more electronegative atom will attract the shared electrons more strongly making it partially negative while the other atom will be partially positive (dipole moment)

Question 9

coordinate covalent bond

Answer 9

(dative bond) forms when the shared electrons are derived from a lone pair on only one of the bonded atoms

Question 10

bond order

Answer 10

describes the number of bonds between 2 atoms

Question 11

single bond

Answer 11

sigma bond

Question 12

double bond

Answer 12

1 sigma and 1 pi bond

Question 13

triple bond

Answer 13

1 sigma and 2 pi bonds

Question 14

bond length

Answer 14

single is longest, triple is shortest

Question 15

bond energy

Answer 15

takes more energy to break triple bond than double than single

Question 16

metallic bonding

Answer 16

when metal atoms are joined together and electrons become delocalized “sea of electrons” = conduct heat and electricity

Question 17

intermolecular forces

Answer 17

attractive forces between molecules that are notably weaker than intramolecular bonds

Question 18

intramolecular vs intermolecular forces

Answer 18

Intramolecular forces are the forces that hold atoms together within a molecule. Intermolecular forces are forces that exist between molecules.

Question 19

London-dispersion forces (VDW)

Answer 19

weakest intermolecular force The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.

Question 20

dipole-dipole interactions

Answer 20

Dipole -dipole interactions occur when the partial charges formed within one molecule are attracted to an opposite partial charge in a nearby molecule. Polar molecules align so that the positive end of one molecule interacts with the negative end of another molecule. (stable dipoles already exist)

Question 21

hydrogen bonds

Answer 21

hydrogen bonding occurs when a hydrogen atom attached to a nitrogen, oxygen, or fluorine atom is attracted to the lone pair of a nitrogen, oxygen or fluorine atom on another molecule

Question 22

ion-dipole forces

Answer 22

occur between ions and molecules with a dipole

Question 23

ionic interactions

Answer 23

occur between 2 molecules with a full charge

Question 24

2 regions of electron density

Answer 24

sp

Question 25

3 regions of electron density

Answer 25

sp2

Question 26

4 regions of electron density

Answer 26

sp3

Question 27

Linear

Answer 27

electron rich regions: 2

bonded atoms: 2

lone pairs: 0

bond angle: 180 degrees

Question 28

trigonal planar

Answer 28

electron rich regions: 3

bonded atoms: 3

lone pairs: 0

bond angle: 120 degrees

Question 29

tetrahedral

Answer 29

electron rich regions: 4

bonded atoms: 4

lone pairs: 0

bond angle: 109.5 degrees

Question 30

trigonal pyramidal

Answer 30

electron rich regions: 4

bonded atoms: 3

lone pairs: 1

bond angle: 107 degrees

Question 31

bent

Answer 31

electron rich regions: 4

bonded atoms: 2

lone pairs: 2

bond angle: 104.5 dergees

Question 32

trigonal bipyramidal

Answer 32

electron rich regions: 5

bonded atoms: 5

lone pairs: 0

bond angle: 90, 120, 180

Question 33

octahedral

Answer 33

electron rich regions: 6

bonded atoms: 6

lone pairs: 0

bond angle: 90, 180 degrees