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76 Cards in this Set

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Si unit for mass
kg
Si unit for length
m
Si unit for temp
K
Si unit for amount of substance
mol
Si unit for time
s
exponential prefixes

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

10^-1
10^-2
10^-3
10^-6
10^-9
10^-12
giga
mega
kilo
hecto
deka

deci
centi
milli
micro
nano
pico
area
m^2
volume
m^3
density
kg/m^3

g/ml or g/cm^3
speed
m/s
acceleration
m/s^2
force
(kg m)/s^2
pressure
kg/(m s^2)
energy
(kg m^2)/s^2
density = x/x
mass/volume
sig figs

+ -
x /
number right of decmial place (lesser)

number of sig figs (lesser)
323.45

# of sig figs
5
.00661

# of sig figs
3
.0066100

# of sig figs
5
C/F conversion
5/9 ratio
daltons theory of matter
elements made of atoms
element charecterized by mass
compounds form in whole number ratios
compounds=combining elemenents. atoms themselves are unchanged
thompson
cathode rays- determine negative charge on electrons
millikin
oil drop- determine mass of electron
rutherford
scattering experiment, determinded atoms have a dense nucleus
atomic number
# of protons
mass number
number of protons + number neutrons
atomic mass
mass of single atoms
covalent bond
two atoms share electrons
ion
charged atoms
isotopes
differnt mass number (# of neutrons)
1
mono
2
di
3
tri
4
tetra
5
penta
6
hexa
7
hepta
8
octa
products of when a hydrocarbon is burned
water and CO2
weak electrolytes
CH3CO2H

HF
spectrum of light (smallest to largest wavelength)

visible= what range? (~)

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

~10-6, ~10-7
dilution equation
Mi /Vi = Mf/ Vf
molarity=
Moles/L
molality=
moles solute/ kg solvement
strong acids (5)
HClO4
H2SO4
HBr
HCl
HNO3
weak acids (3)
H3PO4
HF
CH3CO2H
Strong bases (4)
NaOH
KOH
Ba(OH)2
CA(OH)2
weak bases (1)
NH3
solubility rules (abbreviations)
see sheet

[C]S[N]

PC, SO
what does an acid base reaction always produce?
water and a salt
color spectrum (abbreviation)

(listed fastest to slowest)
GXU V IMR
energy series for m2 and n2 (names)
lyman
balmer
pashcen
bohr model
uncertain to know where an electron is
pauli exclusion principle
no two electron in an atom can have the same four quantam numbers
quantam numbers

m sub s=
see chart

spin quantam number
ionization energy

def
trend
energy required to remove electron

increase up, right
electron affinities

def
trend
energy released when electron added

increase up, right
atomic radii

def
trend
size or atom

increase left, down

(CHECK ELECTRON # SHIFT)
electronegativity

def
trend
ability to attract an electron

increase up, right
born haber cycle process
turn elements into gases
give appropriate +/- charge
dissasociate if neccesary
-lattice energy to combine
molecular geometry
see handout
1 atm= x mm hg = x pa = x torr
760 mm hg

101325 pa

760 torr
kinetic molecular theory (5)
tiny particles

negligable volume to surrondings

no attraction

elastic collisons

kinetic energy is proportion to K
hydrogen bond
h bonded to O,N, or F and attracted to lone pair of another electronegative atom
colligative property
property that depends on amount of solute disolved rather than the properties of the solvent
how to solve for liquid column height of two differnt liquids
pgh=pgh
lovoiser
davy
arrhenius

contributions to acid/base defs
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-
wavelength
distance between peaks
amplitude
range of distance between peak or trough and the center
frequency
number of wave peaks in a given distance
frequency's unit

the unit is also equal to ?
Hz

S -1
Light equation letter meanings

E
h
c
m
v
lamda
e= energy (J)
h= planks constant
c= speed of light
m= mass
v= frequency
MAKE SURE UNITS CANCEL
MAKE SURE UNITS CANCEL
redox 1/2 reactions

in acid...
determine formal charges

in acid: add H20 and H+ to get balanced 1/2 reactions
dipole dipole
CO2- less electronegative is pulled towards the more electronegative
delta H next to a chemical equation means...
for the reaction as written (number of moles)