Ap Chemistry Mid Term Part 2

Front 1

Avogadro's number

Back 1

6.022 X 10 (23)

Front 2

Volume

Back 2

22.4
Mol ---> Liters
Liters ---> mols

Front 3

Limiting reagent

Back 3

You take the smaller/ smallest of the two moles and use mols---> grams to figure this out

Front 4

Percent yield

Back 4

Actual yield/ theoretical yield X 100

Front 5

Precipitation reaction

Back 5

Figuring out if something is a gas of aqueous solution in a double replacement reaction

Front 6

Net ionic reaction

Back 6

The two ions that make and solid compound

Front 7

Acid

Back 7

Donates an H+ ion

Front 8

Base

Back 8

Donates an OH- ion

Front 9

Salt

Back 9

Cation of the base
Anion of the acid

Front 10

Redox

Back 10

OILRIG
•The oxidation state of an atom in a free element is zero
•The oxidation state of a monatomic ion is equal to its charge
•the sum of the oxidation states of all the atoms in:
- a neutral molecule or formula unit is zero
- an ion is equal to the charge of the ion
•In compounds, metals have positive oxidation charges
- group one elements have +1
- group two elements have +2
•In their compounds, non metals are assigned oxidation states
- hydrogen +1
- oxygen -2
- group 7 -1
- group 6 -2
- group 5 -3

Front 11

q= mC/\T

Back 11

Specific heat capacity

Front 12

Frequency

Back 12

How many times a wave crosses a point

Front 13

Amplitude

Back 13

Length of the crest to the line

Front 14

Wavelength

Back 14

Crest to crest

Front 15

Wavelength and frequency

Back 15

What two things are indirectly proportional

Front 16

Red

Back 16

Lowest frequency
Highest wavelength

Front 17

Violet

Back 17

Highest frequency
Lowest wavelength

Front 18

C= frequency X wavelength

Back 18

Speed of light
C= 3.00 x 10 (8) m/s

Front 19

Red

Back 19

LiCl (2)

Front 20

Blue

Back 20

CuCl(2)

Front 21

Orange- Red

Back 21

CaCl(2)

Front 22

Yellow

Back 22

NaCl

Front 23

Purple

Back 23

KCl

Front 24

N

Back 24

Principle energy level

Front 25

L

Back 25

Angular momentum number
S orbital shape (one circle)
P orbital shape (bow tie)
D orbital shape (clover)
F orbital shape (8 rings)
L=N-1

Front 26

M(l)

Back 26

Magnetic quantum number
-l ~ l

Front 27

M(s)

Back 27

Magnetic spin
+, -

Front 28

Autobahn

Back 28

Fill one orbital in at a time

Front 29

Hunds

Back 29

Lowest energy level to the highest energy level

Front 30

Pauli exclusion

Back 30

2 electrons per orbital

Front 31

Atomic size and ion size

Back 31

-----> decreases
|
|
V increases

Front 32

Ionization energy

Back 32

Energy it takes to move an electron
-----> increases
|
|
V Decreases

Front 33

Electro negativity

Back 33

The ability of an atom to draw electrons to itself

Front 34

Ionic compound

Back 34

Transfers electrons one metal
Dissolves in water and conducts electricity

Front 35

Molecular

Back 35

Shares electrons
Low melting and boiling point

Front 36

Resonance structure

Back 36

Lewis structure written in two or more ways

Front 37

VSEPR

Back 37

Valence shall electron pair repulsion
To be the most stable, you have to keep the electrons away from each other

Front 38

Linear

Back 38

Two atoms bonded to an atom

Front 39

Trigonal planer

Back 39

Three atoms bonded to an atom

Front 40

Tetrahedral

Back 40

4 atoms bonded to an atom

Front 41

Trigonal planer

Back 41

5 atoms bonded to an atom

Front 42

Octandril

Back 42

6 atoms bonded to an atom

Front 43

Bent

Back 43

The presence of lone pairs repels the bonding pairs downward