Chemistry Final Review

Front 1

Chemical bond

Back 1

Force that holds two atoms together

Front 2

Bond dissociation energy

Back 2

Energy required to break a bopnd

Front 3

Types of electrons does bonding require the behavior of?

Back 3

Valence electrons (outermost s+p levels)

Front 4

Ionic Bonding

delta X > 1.7

Back 4

Involves mixture of (usually) metal and nonmetal

Nonmentals alomst at full valance, therefore want to pull e-

Highest- Fluorine
Lowest- Francium/Cesium

Make a large group of ions...resulting crystal is very sturdy and strong (electrostatic attractions holding it together)

Front 5

Electronegativity

Back 5

Tendancy of bonded atoms to pull electrons toward itself

Front 6

Lewis dot diagrams

Back 6

Diagrams used to represent element in question w/ its correct number of electrons

Front 7

Covalent Bonding

delta x < .5 or 50

Back 7

Generally occurs w/ two nonmetals

E- on one atom will start to be attracted to nucleus(proton) of other, v.e- lowers energy (attracted forces tend to lower energy of a system)

Potential energy goes up when nuclei gets too close together forming repulsion

chemical potential energy stored in bond

difference between 0 and lowest energy point ...but because difference in small to 0, don't take e- from eachother

Front 8

Polar Covalent Bonding

Back 8

Mixture of an ionic bond and covalent bond

Bond is a covalent bond (due to difference in X), but is one in which the electrons are unequally shared

drawing different for covalent bonds

Front 9

Drawing covalent bonds

Back 9

1. write skeleton structure of the mlcl
2. find total v. e-, including any charges present
3. connect atomos w/ a single bond (a line which stands for 2e-)
4. fill up octets of outside atom w/ remaining e-
5. a) any extra e- go on center atom, even if has octet
b) if run out of e-; meed to multiple bond

Front 10

VSEPR

Back 10

Can find shape of the ion/mlcl formed

shape tells us to dictate how mlcl/ion interacts with other stuff

Front 11

Coordination number

Back 11

Sum of the # of atomos attached and # of nonbinding (lone) pairs of electros on the atom

Tells # orbitals need, which tells you # of old orbitals you used up

V = Valence
S = Shell
E = Electron
P = Pair
R = Repulsion

Front 12

All atoms positioning themselves to be as far apart as possible

Back 12

Because surrounded by e- density and lone pairs of e- around a central atom

minimize the repulsion forces between regions of e- density and lone pairs e- more repulsive than atoms (more pushing power)

Front 13

Coord. # : 2
Lone Pairs : 0

Back 13

Electron Geo. = linear
Molecular Geo. = linear
(180 degrees)
Ex: BeF2

Front 14

Coord. # : 3
Lone Pairs : 0

Back 14

Electron Geo. = trig. planar
Molecular Geo. = trig. planar
(120 degrees)
Ex: BF3

Front 15

Coord. # : 3
Lone Pairs : 1

Back 15

Electron Geo. = trig. planar
Molecular Geo. = v-shaped/bnt
( <120 degrees)
Ex: BF2 -

Front 16

Coord. # : 4
Lone Pairs: 0

Back 16

Electron Geo. = tetrahedral
Molecular Geo. = tetrahedral
(109.5 degrees)
Ex: CF4

Front 17

Coord. # : 4
Lone Pairs: 1

Back 17

Electron Geo. = tetrahedral
Molecular Geo.=trig. pyramid.
(<109.5 degrees)
Ex: CF3-

Front 18

Coord. # : 4
Lone Pairs: 2

Back 18

Electron Geo. = tetrahedral
Molecular Geo. = v-shaped/bnt
(<109.5 degrees)
Ex: CF2 2-

Front 19

Coord. # : 5
Lone Pairs: 0

Back 19

Electron Geo. = trig. bipyram
Molecular Geo.= trig. bipyram
(120 + 90 degrees)
Ex: SbF5

Front 20

Coord. # : 5
Lone Pairs: 1

Back 20

Electron Geo. = trig. bipyram
Molecular Geo. = see-saw
(<120,<90 degrees)
Ex: SbF4 -

Front 21

Coord. # : 5
Lone Pairs: 2

Back 21

Electron Geo. = trig. bipyram
Molecular Geo. = t-shaped
(<90 degrees)
Ex: SbF3 2-

Front 22

Coord. # : 5
Lone Pairs: 3

Back 22

Electron Geo. = trig. bipyram
Molecular Geo. = linear
(180 degrees)
Ex: SbF2 3-

Front 23

Coord. # : 6
Lone Pairs: 0

Back 23

Electron Geo. = octahedral
Molecular Geo. = octahedral
(90 degrees)
Ex: TeF6

Front 24

Coord. # : 6
Lone Pairs: 1

Back 24

Electron Geo. = octahedral
Molecular Geo. = sq. pyramid.
( degrees)
Ex: TeF5 -

Front 25

Coord. # : 6
Lone Pairs: 2

Back 25

Electron Geo. = octahedral
Molecular Geo. = sq. planar
(<90 degrees)
Ex: Tef4 2-

Front 26

Hybridization

Back 26

Behavior of an atom that's involved in bonding

When they bond, often create new orbitals specifically for bonding (covalent)

Each coordination # has corresponding hybrid., which produces own unique shape

Certain kind of symmetry- sigma (sigma bond). formed by p orbital having pi symm. so any multpile bonds are called pi bonds.

Front 27

Coord # 2

Back 27

Hybrid: sp
Shape: linear

Front 28

Coord # 3

Back 28

Hybrid: sp2
Shape: trigonal planar

Front 29

Coord # 4

Back 29

Hybrid: sp3
Shape: tetrahedral

Front 30

Coord # 5

Back 30

Hybrid: sp3d
Shape: trigonal bipyramidal