Exam 1 Flashcards
Molecules
nonmetal elements that bond
Ionic
metal +nonmetal that bond NH4 is a metal when at the beginning
Chemical change
you make a new chemical (EX acid plus base)
physical change
Nothing chemically changes (EX: heat)
INTensive property
INDependent of sample size
EXTensive property
More stuff EXTends the property. bigger sample size changes property
Chromatography
seperating inks SEPERATES BASED ON POLARITY.
distillation
boiling methanol SEPERATE TWO LIQUIDS VIA BOILING POINT
filtration
coffee filter SOLID FROM LIQUID
kinetic energy
energy of motion (temp)
Potential energy
ability to store energy that can become kinetic energy (heat)
volumetric glassware
very accurate/ calibrated glassware ex graduated cylinder.
Density equation
D = Mass g/volume mL
1 mL = 1 ???
cm^3
1.0 + 1.2298887 in sig figs
2.2
(1.0 +1.0085749)/ 2.000989 in sig figs
1
JJ Thompsom Cathode Ray
showed that there were charged particles comming out of atoms (electrons)
Millikan’s Oil drop
found out what charge were for electrons via the rate that the drops fell
Rutherfords gold foil
shot alpha particles through gold foil and showed that solids weren’t really that solid (most fly through). Proved existence of nucleus
Rutherford’s atom model
had a nucleus and a charged space around it filled with electrons.
JJ Thomson’s model
plum pudding model, basically soup of charges.
mass spectrometer
shows how heavy things are using magnets (counts up atoms)
molecular formula
ACTUAL amount of atoms in molecule
empirical formula
RATIO of atoms in molecule
7 Diatomic molecules
H2, N2, O2, F2, Cl2, Br2, I2,
NOTE NOT FOR ELEMENTAL
Eth-
2 carbons
Meth-
1 carbon
Prop-
3 carbons
But-
4 carbons
cyclo-
all carbons bounded in a circle
OH functional group
Alchohol, adds -ol ex: methane to methanol
combustion rxn
Fuel + 02 = CO2 + H2O
avogandros number
6.022 x 10^23 amu
empirical formula from mass percent
percentage x mass / atomic mass/ smallest amount of moles =empirical formula
percent yield
actual yield/ theoretical yield x 100
scaleen factor
gets from empirical to molecular
Metric system is GI-ME-KI or GMK
10^9 10^6 10^3
deci (d)
10^-1
Centi (c)
10^-2
Milli (m)
10^-3
Micro (u?)
10^-6
Nano (n)
10^-9
Pico (p)
10^-12
Femto (f)
10^-15
how many times must we convert m^3 to cm^3?
3
Kinetic energy equation
KE = 1/2 mv^2
Discrete element
Diatomic element thing H2
ite replaced with _____ in acids
ous
ate replaced with ____ in acids
ic
5 carbons
penta
6 carbons
Hexa
7 carbons
hepta
8 carbons
octa
9 carbons
nona
10 carbons
deca
formula units
amu’s
isomers
molecules with the same molecular formula, but different structural appearances.
PO4 name and charge
phosphate 3-
C2O4 name and charge
Oxalate 2-
CO3 name and charge
Carbonate 2-
Dichromate formula and charge
C2O7 2-
SO4 name and charge
Sulfate 2-
SO3 name and charge
Sulfite 2-
IMP for mass spectrometer questions….
Remember diatomics or discrete elements