Chemistry Final

Front 1

Si unit for mass

Back 1

kg

Front 2

Si unit for length

Back 2

m

Front 3

Si unit for temp

Back 3

K

Front 4

Si unit for amount of substance

Back 4

mol

Front 5

Si unit for time

Back 5

s

Front 6

exponential prefixes

10^9
10^6
10^3
10^2
10^1

10^-1
10^-2
10^-3
10^-6
10^-9
10^-12

Back 6

giga
mega
kilo
hecto
deka

deci
centi
milli
micro
nano
pico

Front 7

area

Back 7

m^2

Front 8

volume

Back 8

m^3

Front 9

density

Back 9

kg/m^3

g/ml or g/cm^3

Front 10

speed

Back 10

m/s

Front 11

acceleration

Back 11

m/s^2

Front 12

force

Back 12

(kg m)/s^2

Front 13

pressure

Back 13

kg/(m s^2)

Front 14

energy

Back 14

(kg m^2)/s^2

Front 15

density = x/x

Back 15

mass/volume

Front 16

sig figs

+ -
x /

Back 16

number right of decmial place (lesser)

number of sig figs (lesser)

Front 17

323.45

# of sig figs

Back 17

5

Front 18

.00661

# of sig figs

Back 18

3

Front 19

.0066100

# of sig figs

Back 19

5

Front 20

C/F conversion

Back 20

5/9 ratio

Front 21

daltons theory of matter

Back 21

elements made of atoms
element charecterized by mass
compounds form in whole number ratios
compounds=combining elemenents. atoms themselves are unchanged

Front 22

thompson

Back 22

cathode rays- determine negative charge on electrons

Front 23

millikin

Back 23

oil drop- determine mass of electron

Front 24

rutherford

Back 24

scattering experiment, determinded atoms have a dense nucleus

Front 25

atomic number

Back 25

# of protons

Front 26

mass number

Back 26

number of protons + number neutrons

Front 27

atomic mass

Back 27

mass of single atoms

Front 28

covalent bond

Back 28

two atoms share electrons

Front 29

ion

Back 29

charged atoms

Front 30

isotopes

Back 30

differnt mass number (# of neutrons)

Front 31

1

Back 31

mono

Front 32

2

Back 32

di

Front 33

3

Back 33

tri

Front 34

4

Back 34

tetra

Front 35

5

Back 35

penta

Front 36

6

Back 36

hexa

Front 37

7

Back 37

hepta

Front 38

8

Back 38

octa

Front 39

products of when a hydrocarbon is burned

Back 39

water and CO2

Front 40

weak electrolytes

Back 40

CH3CO2H

HF

Front 41

spectrum of light (smallest to largest wavelength)

visible= what range? (~)

gamma, radio, ultraviolet, visive, x ray, microwave, infared

Back 41

gamma, x ray, ultraviolet, visible, infrared, microwave, radio

~10-6, ~10-7

Front 42

dilution equation

Back 42

Mi /Vi = Mf/ Vf

Front 43

molarity=

Back 43

Moles/L

Front 44

molality=

Back 44

moles solute/ kg solvement

Front 45

strong acids (5)

Back 45

HClO4
H2SO4
HBr
HCl
HNO3

Front 46

weak acids (3)

Back 46

H3PO4
HF
CH3CO2H

Front 47

Strong bases (4)

Back 47

NaOH
KOH
Ba(OH)2
CA(OH)2

Front 48

weak bases (1)

Back 48

NH3

Front 49

solubility rules (abbreviations)

Back 49

see sheet

[C]S[N]

PC, SO

Front 50

what does an acid base reaction always produce?

Back 50

water and a salt

Front 51

color spectrum (abbreviation)

(listed fastest to slowest)

Back 51

GXU V IMR

Front 52

energy series for m2 and n2 (names)

Back 52

lyman
balmer
pashcen

Front 53

bohr model

Back 53

uncertain to know where an electron is

Front 54

pauli exclusion principle

Back 54

no two electron in an atom can have the same four quantam numbers

Front 55

quantam numbers

m sub s=

Back 55

see chart

spin quantam number

Front 56

ionization energy

def
trend

Back 56

energy required to remove electron

increase up, right

Front 57

electron affinities

def
trend

Back 57

energy released when electron added

increase up, right

Front 58

atomic radii

def
trend

Back 58

size or atom

increase left, down

(CHECK ELECTRON # SHIFT)

Front 59

electronegativity

def
trend

Back 59

ability to attract an electron

increase up, right

Front 60

born haber cycle process

Back 60

turn elements into gases
give appropriate +/- charge
dissasociate if neccesary
-lattice energy to combine

Front 61

molecular geometry

Back 61

see handout

Front 62

1 atm= x mm hg = x pa = x torr

Back 62

760 mm hg

101325 pa

760 torr

Front 63

kinetic molecular theory (5)

Back 63

tiny particles

negligable volume to surrondings

no attraction

elastic collisons

kinetic energy is proportion to K

Front 64

hydrogen bond

Back 64

h bonded to O,N, or F and attracted to lone pair of another electronegative atom

Front 65

colligative property

Back 65

property that depends on amount of solute disolved rather than the properties of the solvent

Front 66

how to solve for liquid column height of two differnt liquids

Back 66

pgh=pgh

Front 67

lovoiser
davy
arrhenius

contributions to acid/base defs

Back 67

lavoiser- proposed O is the commonality in acids

davy- acids provide H, not O

arrhenius- acids dissasociate to produce H / bases dissasociate to produce OH-

Front 68

wavelength

Back 68

distance between peaks

Front 69

amplitude

Back 69

range of distance between peak or trough and the center

Front 70

frequency

Back 70

number of wave peaks in a given distance

Front 71

frequency's unit

the unit is also equal to ?

Back 71

Hz

S -1

Front 72

Light equation letter meanings

E
h
c
m
v
lamda

Back 72

e= energy (J)
h= planks constant
c= speed of light
m= mass
v= frequency

Front 73

MAKE SURE UNITS CANCEL

Back 73

MAKE SURE UNITS CANCEL

Front 74

redox 1/2 reactions

in acid...

Back 74

determine formal charges

in acid: add H20 and H+ to get balanced 1/2 reactions

Front 75

dipole dipole

Back 75

CO2- less electronegative is pulled towards the more electronegative

Front 76

delta H next to a chemical equation means...

Back 76

for the reaction as written (number of moles)