Ap Chemistry

Front 1

How to find the energy of the electron of Hydrogen atom?

Back 1

E = (-2.178x10^-18)/ n^2 Joules

n is the shell (principal quantum number)

Front 2

How to find the amount of electromagnetic radiation released when electrons jump to lower energy levels?

Back 2

ΔE = hv = hc/λ

λ= wavelength of the radiation (0.0000001m = 100nm)
h= 6.63x10^-34 joule-sec
v= frequency of radiation
c= 3.00x10^8 m/sec (speed of light)

Front 3

How to find the wavelength related to the momentum of teh particle?

Back 3

λ= h/mv

Front 4

Relationships to the Periodic Table

Back 4

EN (attract electron)to the right and up
Atomic Radius to the left and down
IN (remove electron)to the right and up

Front 5

Couloumb's Law

Back 5

((-q)(+q))/r^2
q = magnitude of charges

Front 6

Trigonal Planar (degree/ hybridization)

Back 6

120/ sp2

Front 7

Tetrahedral (degree)
-Pyramidal
-Angular Bent

Back 7

109.5
107
104.5

Front 8

Trigonal bipyramidal

Back 8

90, 120

Front 9

How many significant figures does this number have?
1200.000

Back 9

7 sig figs

Front 10

moles in comparison to gases

Back 10

mole = PV/RT (R = 0.0821 L-atm/mol-K)

Front 11

moles under STP (volume

Back 11

liters/(22.4 L/mol)

Front 12

at STP what is the temperature, the pressure in mmHg and liters occupied by 1 mol of gas?

Back 12

273K or 0 C
760 mmHg
22.4 liters

Front 13

What is the total kinetic energy of a gas sample?

Back 13

KE =3/2nRT (8.31 joules/mol-K)

Front 14

What is the average kinetic energy of a single gas molecule?

Back 14

KE =1/2mv^2
m = kg mass of the molecule
v= speed of the molecule( meters/sec)
KE is measured in joules

Front 15

What is the gas constant for PV=nRT

Back 15

0.0821 L-atm/mol-K

Front 16

Dalton's Law of Partial Pressure

Back 16

Pa= Ptotal)(Xa)
Xa = moles of gas A/ total moles of gas
Ptotal = Pa+Pb+Pc....

Front 17

Density of gas

Back 17

D = m/v

Front 18

Van der Waals Equation for Nonideal conditions

Back 18

nRT = (P + n^2a/v^2)(v − nb)
R = 0.0821 L-atm/mol-K

Front 19

Graham's Law (average speed of a gas molecule at a given temperature)

Back 19

average speed of a gas molecule = square root of 3kT/m = square root of 3RT/M

m= mass of gas in kg
M= molecular weight of gas in kg/mol
k = 1.38x10^-23 joule/K
R= 8.31

Front 20

Graham's Law for the rate of effusion

Back 20

the square root of (m1 / m2) = r2 / r1

m= molecular weight

Front 21

What is enthalpy change

Back 21

ΔH= ΣΔH products - ΣΔH reactants
when bonds are formed, energy is released
when bonds are broken, energy is absorbed

Front 22

What is heat capacity?

Back 22

Cp= ΔH/ΔT

Front 23

What is specific heat?

Back 23

Specific heat is the amount of heat required to raise the termperature of one gram of a substance one degree Celsius
q=mcΔT

Front 24

What is entropy?

Back 24

The measure of the randomness of system

Front 25

What is Gibbs free energy change?

Back 25

if ΔG is negative, the reation is spontaneous
if ΔG is 0, equilibrium is reached

Front 26

The relationship of spontaneity, enthalpy and entropy?

Back 26

ΔG= ΔH - TΔS (T in K)

Front 27

How to find the free energy change?

Back 27

ΔG = ΔG° + RTlnQ

Front 28

How to find the standard free energy change under equilibrium?

Back 28

ΔG° = - RTlnK
k is equilibrium constant

Front 29

Hwo do you find the boiling point elecation when a solute is added to a solution?

Back 29

ΔT = ikbm
i= Van't Hoff factor
kb the boiling point constant for the solvent
m- molality

Front 30

How can you calculate the molality?

Back 30

kg of solvent/ moles

Front 31

How do you find the freezing point depression?

Back 31

ΔT= ikfm

i the van't hoff factor
kg= the freezing point deprresiong constant for the solvent
m= molality

Front 32

How do we observe the decrease in vapor pressure when solute is added to a solution?

Back 32

P =XP°
P=vapor pressure of the solution
P°= vapor pressure of the pure solvent
X = the mole fraction of the solvent

Front 33

How can we calculate the osmotic pressure in atm?

Back 33

λ= MRTi

Front 34

How do we find the partial pressure constant using atmospheres as units?

Back 34

Kp = Kc(RT)^Δn

Front 35

Observe the equation:
N2 +3H2 <--> 2NH3 ΔH°=-92.6kJ
what happens when the volume is increased?

Back 35

the reaction procceds to the reverse reaction
(increase V, more moles)

Front 36

Could you please possibly tell me what are the strong acids?

Back 36

HCl, HBR, HI, HNO3, HClO4, H2SO4

Front 37

Could you please tell me which are the important strong bases that I would need to know?

Back 37

LiOH, NaOH, KOH, Ba(OH)2, Sr(OH)2

Front 38

tell me about the Henderson-Hasselbalch Equation

Back 38

pH= pKa + log[A-]/[HA]

pOH = pKb + log [HB+]/[B]

Front 39

In a strong acid and strong base titration, what is the major relationship between pH and pKa @ half-equivalence point?

Back 39

they are equal

Front 40

First Order Rate Law

Back 40

ln[A]tln[A]o = -kt

Front 41

Half Life of first order

Back 41

ln2/k

Front 42

second order rate law

Back 42

1/[A]t - 1/[A]o = kt

Front 43

half life of second order

Back 43

1/k[A]o

Front 44

find relationship between voltage and spontaneity

Back 44

ΔG°= -nFE°

E°= standard reaction potential

Front 45

Find the relationship between voltage and equilibrium

Back 45

E° = RT/nFlnK

Front 46

Find cell potential under nonstandard conditions when not under equilibrium

Back 46

Ecell= E°cell - (RT/nF)lnQ

R = 8.31

Front 47

Find the current

Back 47

I = q/t (charge over time)