Chem eoc Flashcards
The two types of substances
element and compound
classify Cl2 as either a substance or mixture, and what type
A substance: element
classify H2O as either a substance or mixture, and what type
A substance: compound
The two types of mixtures
homogeneous and heterogeneous
classify Sugar water (C2H12O6+H2O) as either a substance or mixture, and what type
homogeneous mixture
classify Cookie dough ice cream as either a substance or mixture, and what type
heterogeneous mixture
color property=chemical or physical?
physical property
density property=chemical or physical?
physicalf
flammability property =chemical or physical?
chemical
solubility property=chemical or physical?
physical
reaction property (reacts w/..)=chemical or physical?
chemical
sour taste property=chemical or physical?
physical
melting point property==chemical or physical?
physical
luster property=chemical or physical?
physical
odor property=chemical or physical?
physical
rusting property=chemical or physical?
chemical
king henry drank bubbly dark chocolate milk
king henry danced badly during christmas morning
ya
Atlantic rule
if the 0 is AFTER the decimal point, it should be accounted for in sig. figs
Pacific rule
if the 0 is PREVIOUS (before) the decimal point, it should NOT BE ACCOUNTED FOR
how many sig digs. in 8040
3
how many sig digs in 0.020
2
how many sig digs in 6,051.00
6
calculate the percent error given
experimental value: 1.24 g
accepted value: 1.30g
(1.30g-1.24g)/1.30g
times 100
=4.62%
IMPORTANT: bigger value goes first always
how to calculate density? d=
d=m/v
how to calculate mass? m=
m=dv
how to calculate volume? v=
v=m/d
what goes on top in the triangle
m
plum pudding model guy
Jj thomson
cathode ray guy
jj thomson
charge and mass of electron guy
robert millikan
oil drop experiment guy
robert millikan
first atomic theory guy from experiment
dalton
electron clouds guy
niels bohr
uncertainty principle guy
heisenberg
top number in atomic structure is what?
the mass number
bottom number in atomic structure is what?
the atomic number
isotope name example
element-number (Cs-133)
what does the 133 in Cs-133 stand for?
the mass number
How to calculate average atomic mass
(mass number)(percent abundance)+(mass number2)(percent abundance2) etc
group name for 1a elements
alkali metals
group name for 2a elements
alkali earth metals
group name for 7a elements
halogens
group name for 8a elements
noble gases
group name for 3-12 elements (or 3d elements in the electron configuration)
transition metals
highest electronegativity
Fluorine
highest ionization energy
Helium
highest atomic radius
Francium
Negative ion=
gains electrons
Positive ion=
loses electrons
ammonium polyatomic formula
NH4+
acetate polyatomic formula
C2H3O2-
hydroxide polyatomic formula
OH-
phosphate polyatomic ion formula
PO43-
sulfate polyatomic ion formula
SO42-
Carbonate polyatomic ion formula
CO3^2
Nitrate polyatomic ion formula
NO3-
Cation=
Pawsitively charged
Anion
negatively charged
covalent bonds=
nonmetal+nonmetal
ionic bonds=
metal+nonmetal
If the polyatomic ion ends in ate then you change the acid formula ending to…
ic acid
if the polyatomic ion ends in ite then you change the acid formula ending to…
ous acid
if the polyatomic ion ends in ide then you change the acid formula prefix and ending to…
hydro….ic
H2SO4- formula acid name
Sulfuric acid
one more than -ate polyatomic=
add per prefix (ex: ClO4- is perchlorate)
one less than -ate polyatomic=
add -ite (ex: ClO2- is chlorite)
two less than -ate polyatomic=
add hypo and -ite (ex: ClO- is hypochlorite)
remove oxygen from -ate polyatomic
add -ide (Cl- is chloride)
H2SO3 acid name
sulfurous acid
H2S acid name
hydrosulfuric acid
HClO4 acid name
perchloric acid
HCLO acid name
hypochlorous acid
HCl acid name
hydrochloric acid
HNO3
Nitric acid
HNO2 acid name
Nitrous acid
Standard number for particles
6.022*10^23 particles
how to find percentage composition
divide mass of element by total mass of compound for each element, then multiply by 100.
how to find empirical formula of a compound, given percentage compositions
turn the percent into grams, then solve for moles. then divide by smallest number of moles for whole number. if the number is not close to a whole number (ex:2.5) then multiply by a whole number for each to have all numbers be whole. Then those numbers will signify how many of each element is in the compound
Molecular formula given empirical formula compound and molecular weight.
divide the molecular weight by the mass of the empirical formula compound. then multiply that whole number by the subscript numbers indicating how much of each element there is in a compound given.
ex: CHO *2= C2H2O2
temperature increase shift
shifts to the side that doesn’t state the heat energy.
if one element is removed, shifts to what side?
shifts to the side where the element is removed.
if one element is added, shifts to what side?
shifts to the opposite side of the elemtn added.
if pressure decreases, shifts to what side?
the side with less moles
reducing agent in a redox reaction does what with electrons:
gains electrons
oxidizing agent in a redox reaction does what with electrons:
loses electrons
strength of solid Intermolecular forces
are strong
strength of gas intermolecular forces
are weak
ideal gas law equation
PV=nRT
boyle’s law
P1V1=P2V2
endothermic reactions do what wtih energy
gain energy
exothermic reactions do what with energy
release energy
where is the activation energy located in potential energy curves?
the arrow on the side from the activated complex to the dotted line signifying the reactants
STP of gas’ volume
22.41 L
STP of temperature
273.15 K or 0 degrees Celsius
STP of pressure
1 atm
Charle’s law
V1T2=V2T1
Gay lussac’s law
P1T2=P2T1
Combined gas law
P1V1T2=P2V2T1
Molarity formula=
moles/volume(L)
Molarity by dilution formula
M1V1=M2V2
in what direction do excited electrons move in the Bohr Model
to a higher ring.
elements in the same group have…
similar properties
C of water
4.184 J/g*C
formula to find energy from a wavelength
E=hc/wavelength
h in wavelength/energy formulas=
6.62610^-34 Jg
Relationship between frequency and wavelength
inverse:
high frequency=short wavelength
example of a high frequency form of energy
gamma rays
example of a long wavelength form of energy
Radio waves