Equations Flashcards

1
Q

Plank’s frequency relation

A

E = h(f or nu)

E=energy
h= Plank’s constant (6.63 x 10^-34 Js)
f=frequency

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2
Q

What equation is similar to Plank’s frequency relation?

A

c/v=wavelength x frequency (v or nu)

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3
Q

When would Plank’s frequency relation be used?

A

To calculate energy or frequency

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4
Q

Angular momentum equation

A

L=nh/2(pi)

n=principal quantum number
h=Plank’s constant

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5
Q

Plank’s constant

A

6.63 x 10^-34 Js

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6
Q

When would angular momentum of an electron around a hydrogen be used?

A

Quantized by higher principle number, higher momentum

Larger principle quantum numbers have higher momentum

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7
Q

Energy of an electron equation

A

E=-RH/n^2

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8
Q

When would the energy of an electron be important?

A

Energy of electron is directly proportional to the principle quantum number
Because of negative sign, larger number gets closer to zero, larger

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9
Q

Rydberg unit of energy

A

2.18 x 10^-18 J/electron

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10
Q

Avagadro’s number

A

6.02 x 10^23
Measure of things - usually measures a number of atoms within a mass number
1 mol=6.02 x 10^23 atoms= # amu
The units of a mol

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11
Q

Electromagnetic energy of a photon equation

A

E=hc/(wavelength) or

-RH[1/n^2-1/n^2]

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12
Q

Speed of light (c)

A

3 x 10^8 m/s

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13
Q

Max number of electrons in a shell

A

2n^2

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14
Q

Values of l

A
Subshell
0=s
1=p
2=d
3=f
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15
Q

Max number of electrons in a subshell

A

4l + 2

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16
Q

Max value of l

A

0 to n-1

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17
Q

ml

A

Orbital within subshell

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18
Q

Max electrons in a orbital

A

2e

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19
Q

Values of ml/orbitals per l

A

any l has 2l +1 values of ml

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20
Q

Orbitals/ml per principle number

A

n^2

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21
Q

Values of ms

A

+1/2, -1/2

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22
Q

How to determine which subshell is lower

A

n +1

If same, lower n will fill first

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23
Q

Values of ml

A

between -l and +l

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24
Q

Percent composition

A

All of them= 1

Each one’s mass number amount= given atomic weight

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25
1 amt =
760 Torr = 760 mmHg = 101.325 kPa
26
STP
273 K 1 atm For gas law calculations
27
Standard conditions
298 K 1 M For entropy, enthalpy, Gibb's free energy, and electromotive forces
28
Ideal gas law
PV=nRT
29
R
Ideal gas constant 8.21 x 10^-2 Latm/molK or 8.314 J/molK
30
How much does 1 mol of ideal gas occupy?
22.4 L
31
Density equation
=m/V = PM/RT
32
Combined gas law
PV1/T1 = PV2/T2
33
When would the combined gas law be used?
When the moles stay constant, but need to find the other factor
34
How to find density from combined gas law?
Substitue V1= 22.4 L and use STP to compare to current | Then divide mass/new volume
35
How to find molar mass from combined gas law?
Used combined gas to find V at STP Divide weight by newfound liter amount Multiply g/L by ideal gas volume = g/mol Density at STP x volume of one mol
36
Avagadro's principle
n/V=k n1/V1=n2/V2 k is a constant
37
Gibb's free energy equation
Delta G= Delta H- TDelta(S)
38
Percent by mass
mass of solute/mass of solution x 100
39
Mole fraction
mol of A/mol of all species
40
Molarity
mol solute/L solution
41
p value=
m-0.n
42
Ka
[H3O=]{A-]/[HA]
43
Kb
[B+][OH-]/[BOH]
44
Faraday's constant
10^5 C/mol e-
45
Electrodeposition equation
mol M=It/nF n=oxidation state
46
Boyle's Law
PV=k | PV=PV
47
Charles's Law
V/T=k | V/T=V/T
48
Gay-Lussac's Law
P/T=k | P1/T1=P2/T2
49
Dalton's Law of Partial Pressures
Ptotal=PA + PB +PC ...
50
Partial pressure equation
PA=XA(PT) | XA=mol of gas A/total moles of gas
51
Vapor pressure
``` [A]= kH x Pa [A]1/P1=[A]2/P2= kH ``` [A]=concentration kH=Henry's constant PA=partial pressure of A
52
Average kinetic energy of a gas
KE=1/2mv^2=(3/2)kBT kB=Boltzmann constant
53
Boltzmann constant (kB)
1.38 x 10^-23 J/KT
54
Root-mean-square speed (u rms)
u rms= Square root (3RT/M) R=ideal gas constant M=molar mass in kg/mol
55
R (Ideal gas constant)
8.314 J/Kmol
56
Graham's law
r1/r2=Square root(M2/M1) Ex. A gas that has a molar mass 4x of another, it will travel half as fast
57
Van der Waals Equation of State
(P +n^2a/V^2)(V-nb)=nRT ab=constants for each gas
58
a constant
Corrects for attractive forces (smaller for smaller less polarizable molecules and largest for polar moleucles)
59
b constant
Corrects for volume of molecules due to size
60
Standard electromotive force (emf)
E(cell)=E(red,cathode)-E(red,anode)
61
Do you multiply cell potentials when coming up with net reactions?
No
62
Delta G and emf
Delta G= -nFEcell n=mols of electrons exchanged F=Faraday constant Ecell=standard emf
63
Deviation from normal cell emf
Ecell=E(cell standard) - RT/nF (lnQ) Q=reaction quotient
64
Simplified deviation from normal cell emf
E cell=E(cell standard) -0.0592/n(logQ)
65
Reaction quotient
Q=[C]^c[D]^d/[A]^a[B]^b Lower case is number in front
66
Delta G equation
-RTlnKeq
67
Change in Free energy of electrochemical cell with varying concentration
Delta G= Delta G(standard) + RTlnQ
68
Rate law
k[A]^x[B]^y
69
Arrhenius equation
k=Ae^-Ea/RT
70
Radioactive decay
[A]t=[A]e^-kt
71
Concentration of Solution after dilution
MV=MV
72
Normality
mols solute/kg solvent
73
Boiling point depression expression
Delta(T)=iKbm i=van't Hoff factor=number of particles in which a compound dissociates (NaCl=2) Kb=proportionality constant of the solvent m=molality Temperature in Kelvin
74
Density of water
1g/mL
75
Freezing point depression
Delta T f=iKfm i=van t'Hoff Kf=proportionality constant m=molality Temperature in Kelvin