Chem CSET Flashcards
(307 cards)
1
Q
Freon
A
dichlorodifluoromethane
2
Q
isolated system
A
there is no exchange of matter or energy
3
Q
Closed system
A
allows for change in energy but not matter
4
Q
What are the adverse effects of photochemical smog
A
Human health
damage to materials
toxic to plants
atmosphere
5
Q
what substance can be found at the highest point of a fractionating column during fractional distillation of crude oil
A
propane
6
Q
Which molecules require description with resonance structures
A
we can write two are more lewis structures that differ only in the position of electrons.
7
Q
What type of EM spectrum is strong evidence for the big band theory
A
microwave
8
Q
isotopes
A
atoms of the same number of protons but different number of neutrons
Same atomic number
9
Q
atomc mass number
A
number or protons and neutrons
10
Q
Principal quantum number
A
n
energy level or size of an orbital.
larger moving down a group
11
Q
Ground state
A
lowest energy possible
12
Q
Electron energy level
spdf
A
s = 1 -2
p =1-6
d = 1-10
f = 1-14
13
Q
photon
A
electron transition from high to low energy orbital.
the difference in energy released.
weightless particle of electromagnetic radiation
14
Q
types electromagnetic radiation
A
heat light UV light x rays transverse wave
15
Q
atomic spectrum
A
each transition H electrons make correspond to a different amount of energy and different color is released
16
Q
Bohr model
A
a small positive nucleus surrounded by electrons located in a specific energy level
17
Q
electron configuration
A
arrangement of electrons.
1s2
18
Q
Group 1
A
alkali metals
soft
silvery
react violently with water
19
Q
group 17
A
halogens
extremely reactive and poisonous
20
Q
metals
A
shiny
conductive of heat and electricity
malleable
ductile
21
Q
nonmetals
A
brittle,
dull
poor conductors
have low melting and boiling points
22
Q
metalloids
A
has properties of metals and nonmetals
23
Q
when determining molecular mass by osmotic measurement the molar mass will
A
be less
24
Q
atomic radius
A
1/2 the distance between the nuclei of two bonded atoms
increase moving down and left
25
electromagnetic radiation
a form of energy that travels through space
26
ionization energy
the amount of energy required to remove an electron.
| Increases moving up and right.
27
ionized
losing one or more outer electrons
28
electronegative
ability to attract other electrons.
increasing moving up and right.
cannot be measured directly.
has no unit of measurement
29
boiling point
increases then decreases across a period
30
metallic character along the periodic table
increases moving left and down
31
chemical reactivity
substances change chemically
32
photoelectric effect
when electrons are released after light is shone onto a metal
33
maxwell's wave theory of light
brighter (high intensity) light would lead to higher energy electrons
34
quanta
quantities
35
E = hf
h = 6.63 x 10 ^-34
Quantum theory
F= frequency of radiation
36
quantum number
describe a specific aspect of an electron
37
angular/azimuthal momentum quantum number
```
shape of the orbital
l
S= o
p=8
d=88
f = flower
```
38
magnetic quantum number
```
position of the electron
m1
S=0
p= -1 to 1
d = -2 to 2
f = -3 to 3
```
39
spin quantum number
s
spin of the electron determines properties of the atom
+/- 1/2
40
properties of gas
expand to fill container
v of gas = v of container
can be compressed
41
ideal gas
theoretical that follows a set of principles.
KMT
no volume, attractive or repulsive forces
all collisions are elastic
KE is proportional to temperature
42
kinetic molecular theory
model used to explain behavior of matter.
particles are constantly in motion.
KE is related to temperature.
space between particles is related to the state of matter.
phase change happens when temperature changes significantly.
intermolecular forces
43
properties of liquid
fluid and can flow
definite volume but not shape
low compressibility
44
properties of solids
definite volume and shape
little KE
arranged in a packed crystalline structuer.
45
amorphous solid
doesnt have crystalline structure
46
hydrogen bonds
occur between polar molecules that contain an O F N atom covalently bonded to a H atom
47
dipole induced dipole
occur when a polar molecule induces a temporary dipole moment in a neighboring non polar molecule
48
dipole
separation of charges between two covalently bonded atoms.
49
dipole dipole
intermolecular forces between polar molecule.
| positive side of a polar molecule attracts negative or another
50
london dispersion forces
noble gases and non polar molecule
| creates temporary dipoles
51
ion dipole force
force between an ion and dipole molecule
52
intermolecular forces
positive charged poles attracted to the negative charged poles
53
phase change
transition from one state of matter to another
54
sublimination
solid to gas
55
deposition
gas to solid
56
phase diagram
graph of the physical state of a substance and the temperature and pressure of the substance
57
phase equalibium lines
where two phases are in equalibrium
58
triple point
point where the temperature and pressure conditions are right for all three states to exist together at equilibrium
59
critical point
gas and liquid states are identical and the substance is in one phase
60
supercritical fluid
state where the gas and liquid phase of a substance are indistinguishable
61
dipole moment
overall unequal distribution of electrons across the entire molecule
62
non polar molecule
even charge distribution and no dipole moment
63
polar molecule
uneven distribution charge and dipole moment
64
macromolecule
huge molecules made up of smaller subunits called monomers.
65
organic macrmolecules
huge molecules that included C and found in living things
66
inorganic macromolecule
huge molecule not found in living things.
67
C to F
5/9 (F-32)
68
Kelvin scale
absolut scale
K
0 is the absolute lowest
K = C + 273
69
pressure
psi
atm
mmHg
1 atm = 14.7 psi = 760 mmHg
70
daltons law of partial presures
total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each individual gas
Pn + Po = Ptotal
71
diffustion
movement of 1 substance through another
| high to low concentration
72
effustion
gas particles exit through tiny holes in a container
73
graham's law
effusion rate of a gas is inversely proportional to the sqr root of its molecular mass.
used to compare the rate of two different gasses at equilibrium.
speed A / speed B = sqr root (mass B/massA)
74
standard pressure
1 atm = 760 mmHg = 14.7 psi
75
standard temperature
0 C = 273 K
76
Avogadro's number
6. 02 x 10 23 amu = 1 mole
| 1. 2 x 10 ^-7 XRCD
77
mole
you have 6.02 x 10 ^23 of something
78
avogadros law
relationship between the number of particles (n) and the volume of a a gas.
V1/ n1 = V2/ne
79
1 mole of an ideal gas at STP takes up
22.4 L
80
Boyles law
temperature is held constant the pressure of a gas increases as volume decreases
P1(V1) = P2(V2)
81
charles law
if pressure is held constant. as the gas is heated its volume will increase
v1/T1 = V2/T2
T must be Kelvin
82
Gay-lussac's law
volume of a container is held constant as the temperature increase, the pressure inside the container increases
P1/T1 = P2/T2
T must be kelvin
83
ideal gas law
relates the temperature, pressure, number of moles and volume of any gas,
PV = nRT
84
PV = nRT
```
P = pressure
V = volume
n = number of moles
R = .08216 atm/molK
T = Temperature
```
85
solvent
dissolves solutes
86
miscible
liquid dissovles easily in another
87
immiscible
liquid doesnt dissolve easily in another
88
ionic compound
compound held together by ionic bonds
| formed by transfer of electrons
89
polar covalent
atoms held together by valence electrons shared between them
90
nonpolar covalent
valence electrons are shared equally and are no changes in the molecule
91
Molarity
moles of solute / L of solution
| M
92
molality
mole solute / kg solvent
| m
93
mass percentage
percent by mass of the solute in the solution
| {mass solute / mass solution) x 100%
94
concentration
amount of a substance in a given quantity in a solution
M1V1 = M2V2
Stoichiometry given to unknown
95
SOLUBILITY
AMOUNT OF SOLUTE NEEDED TO FORM A SATURATED SOLUTION AT A SPECIFIC TEMPERATURE AND SOLVENT AMOUNT.
96
polarity
unequal sharing of electrons
97
factors that influence the rate of solution
amount of solute already dissolved.
temperature
pressure and nature
98
empirical formula
shows the kind and proportions of atoms in substance in simplest form
99
chemical formula
shorthand of writing a substance by using chemical symbols and number subscripts with the exact numbers of atoms.
100
Determine percent composition of compounds
write formula.
use formula to determine molar mass.
use molar mass to determine mass percentage of each element.
101
determine the empirical formula
1. find percent composition.
2. determine mass composition.
3. determine composition in moles.
4. find smallest whole number ratio of atoms.
102
dissolution
dissolving a substance
| like dissolves like
103
calculate frequency
speed of light = frequency x wavelength
104
pure substance
cannot be separated
105
homogeneous mixture
unform throughout
solution
alloy
106
heterogeneous mixture
not uniform throughout
| different components can be seen
107
separating mixtures
```
manually,
dissolving
evaporation
distillation
magnetism
filtration
crystallization
```
108
chromatography
capillary action
109
retention factor
Rf
| distance dye traveled compared to the total distance the solvent traveled
110
conjugate acid
acid forms when a base gains a proton
111
conjugate base
formed when an acid loses protons
112
Acidity Constant
Ka = [H+] [A-] / [HA]
113
calculating pH of a solution
-log[H3O+]
Must be in molarity
logarithmic
114
buffer
solution whose pH will not change much when small amounts of acid or base are added to it.
115
titration
a solution of known properties is used to analyze the properties of an unknown solution
1. balanced equation
2. V1M1/n1 =V2M2/n2
116
equivalence point
the amount of H ions and OH ions are equal and pH = 7
| where titration stops
117
indicator solution
chemical that changes color when a specific pH range
118
Heat transfer
Delta heat = specific heat (m) (delta T)
119
titration curve
graph of PH vs volume of titration added
120
determine the unknown substance concentration
[H+][VH+] = [OH-][VOH-]
1. gather information
2. set up and fill in equation
3. calculate
121
determine pH during titration
1. determine mol of each reactant
2. determine which reactant is in excess
3. calculate pH based on concentration of the excess reactants
122
titrant
solution of known properties
123
pH during weak acid and strong base titration
1. determine number of moles of each reactant
2. determine reactant excess
3. use stoichiometry and Ka/b values to determine acid concentration and pH
1. rice table
b. write equilibrium expression for dissociation of acid.
c. plug and solve
124
Arrhenius equation
```
K = A e ^(-Ea/RT)
A= frequency factor
e = exponential factor
Ea= activation energy J/mol
R = 8.314
```
ln K = -EA/RT + Ln A
125
Arrhenius acid
produce hydrogen ions
126
Arrhenius bases
produces hydroxide ions in water
127
Bronsted Lowry acid
only substance that can donate a proton
128
bronsted lowry base
substance that accepts protons
129
Kw
self ionization of H2O
| [H3O+][OH-] = 1 x 10 -14
130
lewis acid
substance accepts an electron pair to form a covalent bond
131
lewis base
substance donates an elections pair to form a covalent bond
132
lewis acid-base reaction
covalent bond is formed between an electron pair bond donor and acceptor
133
E = mc2
E=energy
m= mass
c = speed of light = 3 x 10 8
134
nuclear binding energy
energy required to separate the nucleus into its individual pieces
135
mass defect
difference in mass between a nucleus and its pieces
| products weight less
136
disintegration energy
energy released during radioactive decay.
1. find the difference of products and reactants
2. multiply 1 u = 1.66 x 10 -27
3. plug into E = mc2
137
radioactive decay
unstable atomic nucleus decays or turns into a more stable nucleus, relating energy in the form of ionizing particles and radiation
138
alpha decay
```
nucleus emits an alpha particle.
one with four less particles
4
2
blocked by paper
cause cancer
```
139
alpha particle
containing two protons and two neutrons
140
beta decay
```
when a neutron turns into a proton and an electron is emitted
0
-1
stopped by wood
penetrate skin
used to date living things
```
141
gamma decay
```
occurs when the nucleus of an atom is very high energy
0
0
contains no mass
stopped by lead
dangerous
```
142
what a change in the chemical structure of a hydrocarbon chain isomers that have a shorter chain are
more volatile
| have a lower boiling point
143
radiocarbon dating
carbon dating
| method used to determine the age of organic material by measuring the radioactivity of its carbon content
144
uranium lead dating
used to find the age of a uranium-containing mineral
145
1 p
| 1
atomic number of a proton is 1
1 = mass number
1 = atomic number
146
nuclear chemistry
field of chemistry that deals with the use of radioactive isotopes and other nuclear reactions
147
nuclear fusion
two or more atoms fuse together to form a single heavier atom
mass and energy is lost
148
nuclear fission
a heavier atom splits into smaller pieces
149
chain reaction
domino effect
| nuclear fission
150
chemical reaction
process where the arrangement of atoms, the way they are connected together, is changed
1. particles must come into contact with one another
2. particles must be lined up correctly
3. particles must collide enough to break their bonds
151
synthesis reaction
joining together of two reactants, to produce a complex product
152
decomposition reaction
chemical reaction in which a single compound breaks down into two or more compounds or atoms
153
single displacement reaction
```
type of chemical reaction where an element reacts with a compound and takes the place of another element in that compound
more reactive replaces a less reactive
1. determine if the reaction will occur
2. determine the products
3. balance the equation
```
154
Double displacement reaction
a chemical reaction where two compounds react and the positive ions and the negative ions of the two reactants switch place forming two new compounds
1. identify individual ions from the reactants and their charges
2. switch the cations and anions
3. balance the equation
155
neutralization reaction
occurs between an acid and a base that forms salt and water
156
gas formation
two compounds react to form a gaseous product
157
synthesis reaction
reactants combine to form a new compound
two elements
two compounds
compound and element
158
aqueous
dissolved in water
159
diatomic molecules
molecules that are composed of two atoms of the same element
| H, N, O, F, Cl, Br, I
160
law of conservation of energy
energy is neither created nor destroyed
161
exothermic reaction
system releases heat and the surroundings heat up
| -
162
endothermic reaction
system gains heat as the surrounding cool down.
energy is absorbed
(+)
vaporization
163
enthalpy change
amount of energy as heat that is lost or gained by a system
| Delta H = (sum of enthalpies of products) - (sum of enthalpies of reactants)
164
reaction rate
change in concentration of reactants or products over time
1. number of particles
2. temperature
3. pressure
4. catalyst
5. size
165
reaction rate of disappearance
-delta(element) / time
166
reaction rate of appearance
delta(element) / time
167
effective collision
1. molecules collide with enough energy to break bonds.
| 2. collide with a favorable orientation
168
activation energy
minimum amount of energy it takes to start a chemical reaction
169
activated complex
unstable state what is between the reactants and the products in a chemical reaction
170
collision theory
helps scientists make predictions about how fast chemical reactions occur
related to the number of successful collisions.
only for gases
171
chemical equilibrium
when the rate of the forward reaction equals the rate of the reverse reaction and the concentrations of the products and reactants are unchanged
172
Equilibrium constant
K = [Cx x Dy] / [An x Bm]
| only gas and aqueous elements
173
lechatelier's principle
any change in a substance on one side of the equation in concentration, temperature or pressure results in an equilibrium shift to oppose the change until a new equilibrium is reached
174
increase in concentration of reactants will make the reaction shift
right
175
an exothermic reaction the reactants have an increased temperature the reaction will shift
left
176
if there is an increase of pressure on the reactants then the reaction will shift
right
177
reaction quotient
```
Q = [C]c [D]d / [A]a [B]b
determines the direction in which the reaction is moving
Q>K right
Q=K equilibrium
Q < K left
```
178
Gibbs free energy
G = H - TS
H= enthalpy
S= entropy
predicts whether a chemical reaction will occur spontaneously
the energy available to do work in chemical reactions.
chemical is measure in reference to another chemical state that is assigned a gibbs free energy of 1
179
spontaneous reactions
happen without the need of any input of energy
180
gibbs free energy and spontaneous reactions
delta G = Gf -Gi = Delta H - T(delta S)
181
Entropy
S
particles spread out more
THird law of thermodynamics
182
covalent bonds
atoms share elections
| strongest
183
ionic bond
electrons are transferred between atoms of opposite charge
184
electron sea model
metallic bonding where electrons float free in a sea of electrons around metal atoms
185
metallic bonding
chemical bonding that takes place from the attraction of metal atoms and the surrounding sea of electrons
186
structural formula
shows the location of atoms relative to one another.
1. determine type and number of atoms.
2. write lewis dot structure for each
3. connect the atoms by electron pair bonds
187
polyatomic ion lewis dot structure
1. sum the number of valence electrons from each atom
2. make a skeleton structure by connecting atoms with single bonds
3. determine the remaining electrons
4. place remaining electrons to satisfy octet
5. double bonds if needed
188
VSEPR theory
shape of the molecule is related to the organization of the central atom's valence electrons
189
molecular geometry
linear
trigonal planar
tetrahedral
bent
trigonal pyramidal
1. find lewis dot structure of the molecule
2. locate of central atom, count the number of electron domains
3. identity the number of nonbonding and bonding domains
4. compare to chart
190
molar mass
the sum of the total mass in grams of all the atoms that make up a mole of a particular molecule
grams / mole
191
finding molar mass of a compound
1. find the atomic masses of each element
2. count how many atoms there are for each element
3. find molar mass
192
calculating number of grams using molar mass
number of moles x molar mass
193
stoichiometry
study of chemical quantities consumed or produced in a chemical reaction
194
mole ratio
ratio of moles of one substance to the moles of another substance in a balanced equation
195
mole to mole calculation
moles of given (moles desired/ moles given ratio) =moles desiered
196
moles to mass calculations
moles A (mole ration of B / A) (molar mass B) = mass B
197
mass to moles calculations
mass A (1 / molar mass A)(mole ration B /A) = moles B
198
mass to mass calculation
mass A (1/molar mass A)(mole ration B/A)(mass B/1) = mass B
199
molar volume
at STP one more of any gas will fill t 22.4 liters
200
stoichiometry of gases
1. balance the equation
2. find the moles of the reactants
3. use mole ration to find products made
4. convert to desired units
201
limiting reactant
used up first
202
excess reactant
substance that is in excess
203
finding the limiting reactant
1. layout givens
2. change mass to moles
3. multiply a reactant with the mole ratio
204
determine the amount of product made from the limiting reactant
limiting reactant (mole ration product / limiting reactant)(molar mass product)
205
theoretical yield
maximum amount of product that can be made from the amount of reactant
1. changes to moles
2. mole ratio product /reactant
3. change product to mass
206
percent yield
actual yield / theoretical yield (100%)
207
oxidation number
number assigned to atoms in molecules to show the general distribution of electrons
1. if electrons are shared, they belong to the more electronegative atom
2. pure elements = 0
3. a binary compound the more electronegative element receive oxidation number equal to the negative charge it would have if it were an anion. the less electronegative element receives an oxidation number if it were a cation
4. fluorine = -1
5. oxygen = - 2 except H2O -1, OF2 is + 2
6. Hydrogen = +1 or -1 when combined with metals
7. the sum in neutral compound is 0
8. sum of polyatomic ions is equal to the charge on the ion
9. monatomic ion is equal to the charge of the ion
208
oxidizing agent
substance that causes the oxidation in another substance
209
reducing agent
substance that causes another substance to reduce
loses electrons
BIH3 is the strongest
increase down a group
210
balancing a redox reaction
1. write unbalanced equation in ionic form excluding spectator ions.
2. give each atom an oxidation number
3. write and balance the half reactions
4. balance oxygen by adding water
5. balance hydrogen by adding hydronium
6. make electrons equal and combine the half reactions q
211
oxidation reaction
reactions that takes an electron
212
when an element is reduced it
gains electrons
213
single bonds
type of covalent bond formed from the sharing of two electrons between two atoms
214
double bonds
type of covalent bond where four electrons are shared between two atoms
215
triple bond
type of covalent bond where six electrons are shared between two atoms
216
functional group
an atom or group of atoms that is responsible for a particular chemical property of an organic compound
217
alcohol
contains one or more hydroxyl groups
R - OH
Higher boiling point due to H bonds between molecules
218
hydrocarbon
compound made of only carbon and hydrogen
219
alkyl halide
compound with a halogen atom
takes place of one or more hydrogens in a hydrocarbon
R-X
220
ketone
the carbon of a carbonyl group share bonds with two other carbons
R - CO -R
221
aldehyde
carbon of the carbonyl group share a bond with at least one hydrogen
R - CHO
222
ether
oxygen is bonded to two carbons
| R - O - R
223
carboxylic acid
carboxyl group
| R - COOH
224
hydroxyl group
OH
225
amine group
NH4
| R - N
226
carbonyl group
C=O
227
carboxylic acid
OH-C=O
228
ester group
OR - C =O
229
polymerization
product is produced with repeating units
230
addition reaction
two molecules combine together
231
cracking
breaking up of big hydrocarbons into smaller pieces
232
redox reaction
where a reduction and oxidation occur
233
esterification reaction
alcohol combines with carboxylic acid to form an ester and water
234
fermentation
process of turning a sugar into alcohols, gases or acids
235
saturated hydrocarbons
have as many hydrogen atoms as possible attached to every carbon
236
aliphatic hydrocarbons
compounds of hydrogen and carbon that do not contain benzene rings
237
alkanes
linear
| compounds that are made of varying numbers of carbon atoms that are all saturated with hydrogen atoms
238
cycloalkanes
alkane that contain a carbon ring
239
alkenes
have at least one double bond between carbon atoms
| Eth--
240
alkynes
have at least one triple bond between carbon atoms
241
alkenynes
have both double and triple bonds
242
arenes
aromatic hydrocarbons
| have at least one benzene ring
243
benzene ring
a ring of 6 carbon atoms with three double bonds
244
aromatic compound
any compound with a benzene ring
245
isomers
different forms of the same compound.
| functional group is placed at a different location.
246
carbohydrates
sugars
| contain ether, hydroxyl groups
247
polysaccharide
large sugar
248
when counting carbons in a carbohydrate
1. find carbon attached to 2 oxygen atoms
| 2. then count carbons it is attached to
249
monosaccharide
single sugar
250
disaccharide
sugar molecule containing two monosaccharides
251
glycosidic linkage
bond between sugars
252
lipids
biological molecules that are insoluble in water but soluble in nonpolar solvents
253
saturated fats
triglycerides that have no double bonds in their carboxylic acid chains
254
unsaturated fats
triglycerides that have double bonds in their carboxylic acid chains
255
trans fats
synthetic
| triglycerides that have trans double bonds in their carboxylic acid chains
256
peptide body
covalent bond that holds amino acids together
| carbonyl and amino nitrogen group
257
enzymes
proteins that enable chemical reactions in our bodies
| decrease activation barrier
258
the amount of kinetic energy of an object is dependent on
mass
| speed
259
Kinetic energy
KE = 1/2 mas (velocity)sqr
260
energy transformation
process of changing energy from one form to another
261
chemical energy
from chemical reaction
262
heat energy
from thermal reactions
263
electrical energy
from charged particles
264
gravitational potential energy
energy stored by an object because of its location above the ground
265
elastic potential energy
energy stored by an object that can be stretched or compressed
266
nuclear energy
energy stored in the nucleus of an atom
fission
fusion
267
internal energy of the system
total kinetic energy of the particles and the potential energy of the particles
268
potential energy is measured by
the phase of an object
269
1 food calories =
1,000 calories
| 4.184 J
270
heat of fusion
heat energy/mass
| Hf = m/q
271
heat of vaporization
amount of energy required to turn a liquid into a gas at its boiling point
Hv = q/m
272
hess's law
measure enthalpy change of a chemical reaction
adding or subtracting chemical reactions with the same products or reactants.
what ever happens to one side you must do to the other
273
thermochecmical equations
shows the enthalpy change going from reactants to products
274
calorie
amount of energy required to raise the temperature of one gram of water by 1 C
275
specific heat capacity
```
amount of energy required to change the temperature of one gram of a substance by 1 C
Q = sm deltaT
Q= energy
s= specific heat capacity
T = Celcius
```
S = q/m delta T
276
heating and cooling curves
line graph that shows the phase changes a given substance undergoes with increasing or decreasing temperature
277
bond enthalpy
energy needed to break a particular bond in a gaseous compound
kJ/mol
278
bond enthalpy values
value of energy required to break a particular chemical bond at 298K (25 C)
279
radiation
transmission of energy from a body in the form of waves or particles
280
nonionizing radiation
encompasses the electromagnetic spectrum from low energy ultraviolet light
nuclear fusion
281
ionization radiation
higher frequencies of the electromagnetic spectrum
nuclear fission
radioactive decay
282
Electronegativity
increased up and right
283
During titration of adding acid to a base, a few drops of acid are added into the solution after the endpoint. How will this affect calculations for the concentration of the base?
It will make the calculations too high. Making the base look stronger than it is.
284
Few drops of water left in a buret that is used to titrate a base into an acid. Will the small amount of water have any effect on the determined value for the concentration of the acid?
Yes, because the water will dilute the base, creating an error.
285
Calculating pOH
pH =-log [H]
pOH = 14 -pH
Must be molarity
286
pKa
-logKa
287
Find pKb from pKa
14 - pKa
288
to find concentration from pH
10 ^ concentration
289
parts per million
(g solute / g solution) x 10^6
290
Erg =
visible waves
291
Magnetic moment
sqrt (n(n+2))
| n= unpared eletrons
292
Density
g/cm3
293
What gas is mostly responsible for the greenhouse effect
carbon dioxide
294
calculate percentage error
actual - measured / acual ) x 100
295
How do energies of similar bonds compare
consistent
296
x rays are in the wavelength range of
.01 - 10 nm
297
Bohr's atomic model
```
mvr = nh/2pi
N = number of orbits
```
298
Coulombs law
ionization energy increases proportionally with the atomic number
299
Faraday
1 mole of electrons
300
How does dialysis work
allows the electrolytes to pass through and not solution particles
301
types of statistical series
```
Spatial
conditional
times
qualitative
quantitative
```
302
calculate the molecular mass from vapor pressure
2 (vapor density)
303
Solubility of alkaline earth metal hydroxides/ oxides
increase down a group
304
solubility of alkaline earth metal sulfates
increase up a group
305
Amu of an electron
1/2000
306
accuracy
how close a measurement is to the true value
307
precision
how close repeated measurements are to each other
