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Day 1: Physical and Chemical Principles > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

1
Q

Dalton’s Atomic Theory (3)

A
  1. elements are composed of tiny indivisible particles called atoms
  2. in a compound, element A mass:element B fixed mass is a whole number/fraction
  3. chemical rxns only involve separation, combination or rearrangement of atoms
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2
Q

Law of Multiple Proportions

A

in a compound, element A mass:element B fixed mass is a whole number/fraction

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3
Q

Law of Conservation of Mass

A

chemical rxns only involve separation, combination or rearrangement of atoms

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4
Q

Law of Definite Proportions

A

a pure compound is made up of elements in the same proportion by mass

  • Proust
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5
Q

Cathode Ray/Geissler Tube

A

Crookes and Geissler

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6
Q

determined ratio of electric charge to mass of electron to be -1.76×10^8 coul/g

A

Joseph John Thomson

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7
Q

determined charge of electron to be -1.60×10^-19

A

Robert Millikan

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8
Q

discovered xrays

A

Wilhelm Roentgen

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9
Q

discovered radioactivity in uranium

A

Becquerel

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10
Q

discovered radioactivity in uranium and polonium

A

Curie

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11
Q

[Who & What]

gold foil experiment

A

Rutherford
1. most of the atom is empty space
2. the positive charge is in the nucleus

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12
Q

discovered neutron

A

Chadwick

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13
Q

quantum number; average distance of electron from nucleus

A

Principal Quantum Number (n)

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14
Q

quantum number; tells shape of orbital

A

Azimuthal/Angular Momentum Quantum Number (l)
0 to n-1

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15
Q

quantum number; describes orientation of orbitals in space

A

Magnetic Quantum Number (ml)
-l to l

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16
Q

quantum number; shows spin of electrons

A

Spin Quantum Number (ms)
+1/2 (CW) or -1/2 (CCW)

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17
Q

[Rule/Principle]

orbitals of an atom must be filled up in increasing energy levels

A

Aufbau Principle

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18
Q

[Rule/Principle]

no two electrons can have the same set of quantum numbers; an orbital must have at most two electrons with opposite spins

A

Pauli’s Exclusion Principle

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19
Q

[Rule/Principle]

the most stable arrangement of electrons in subshells is one with more parallel spins

A

Hund’s Rule of Multiplicity

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20
Q

he arranged elements in triads i.e. Li-Na-K

A

Dobereiner

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21
Q

he arranged elements by atomic mass; found that every 8 elements had similar properties

A

Newlands

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22
Q

they arranged elements according to recurring periodic properties

A

Mendeleev and Meyer

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23
Q

he discovered the relationship bet the elements’ atomic number and frequency of xrays generated from bombarding the element with high-energy electrons

A

Moseley

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24
Q

states that properties of elements are functions of their atomic numbers

A

Modern Periodic Law

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25
Q

average distance between nucleus and valence electron

A

atomic size/radius

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26
Q

energy required to remove an electron from a gaseous atom in its ground state

A

Ionization Energy

lower IE, easier to form cation

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27
Q

change in energy when an electron is accepted by a gaseous atom to form an anion

A

Electron Affinity

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28
Q

measure of ability of an atom to attract a bonding electron

A

Electronegativity

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29
Q

Physical Properties in the Periodic Table

↙️ increasing trend

A

ARM
- Atomic Size
- Reactivity
- Metallic Property

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30
Q

Physical Properties in the Periodic Table

↗️ increasing trend

A

IEEE
- Ionization Energy
- Electron Affinity
- Electronegativity

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31
Q

formation of a bond is due to overlap of two atomic orbitals

A

Valence Bond Theory

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32
Q

a bond is formed when electrons in the bonding molecular orbital is greater than the electrons in the non-bonding molecular orbital

A

Molecular Orbital Theory

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33
Q

[Colligative Properties of Non-Electrolyte Solutions]

Boiling Point Elevation

A

∆T_B = K_B • m

K_B = ebullioscopic constant

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34
Q

[Colligative Properties of Non-Electrolyte Solutions]

Freezing Point Depression

A

∆T_F = K_F • m

K_F = cryoscopic constant

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35
Q

[Colligative Properties of Non-Electrolyte Solutions]

Vapor Pressure Lowering

A

∆P = x_solute • P_solvent

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36
Q

[Colligative Properties of Non-Electrolyte Solutions]

Osmotic Pressure (π)

A

π = MRT

M = molarity
R = 0.08206 L-atm/mol-K

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37
Q

K_B of water

A

0.52

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38
Q

K_F of water

A

1.86

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39
Q

Relationship between Kc and Kp

A

Kp = Kc(RT)^∆n

40
Q

[Le Chatelier’s Principle]
Effect of Changing Concentration

A

high concentration to low concentration

41
Q

[Le Chatelier’s Principle]
Effect of Changing Pressure (opposite for Volume)

A

increasing pressure (decreasing volume)

–> system shifts the reaction towards formation of less number of gaseous molecules

42
Q

[Le Chatelier’s Principle]
Effect of Changing Temperature

A

⬆️ temperature favors endothermic reaction
⬇️ temperature favors exothermic reaction

43
Q

[Le Chatelier’s Principle]
Effect of Adding a Catalyst

A

no effect

44
Q

symbol, mass, and charge of

beta particle or electron

A

β or e
mass = 0
charge = -1

45
Q

symbol, mass, and charge of

positron

A

β or e
mass = 0
charge = +1

46
Q

symbol, mass, and charge of

proton or hydrogen nucleus

A

p or H
mass = 1
charge = +1

47
Q

symbol, mass, and charge of

neutron

A

n
mass = 1
charge = 0

48
Q

symbol, mass, and charge of

gamma ray

A

γ
mass = 0
charge = 0

49
Q

symbol, mass, and charge of

alpha particle or helium nucleus

A

α or He
mass = 4
charge = +2

50
Q

number of nuclear disintegrations per second

A

activity [=] Bq

51
Q

rate of disintegration of 1 g of Ra

A

Curie (Ci)

52
Q

Ci to Bq conversion

A

1 Ci = 3.7×10^10 Bq

53
Q

Radiation absorbed dose (rd)
SI unit : Gy (gray)

A

1 rd = 10^-5 J/g tissue
1 Gy = 1 J/kg absorbing material

54
Q

basically a helium nucleus
commonly found during radioactive decay
net result is to increase n:p ratio

A

alpha particle

55
Q

basically an electron; emitted when n:p > zone of stability
- e comes from…
- β comes from…

A

beta particle
- atomic orbital
- nucleus

56
Q

aka high energy proton
by-product of alpha particle decay

A

gamma ray

57
Q

antimatter of electron; emitted when n:p < zone of stability

A

positron

58
Q

usually accomplished by emission of gamma ray; inner orbital electron is captured by the nucleus to increase n:p

A

electron capture

59
Q

a single ___ is rather unstable and will convert itself to a ___ and an ___

A

neutron, proton, electron

60
Q

when a nuclide has __ or more protons, it tends to be unstable and undergo radioactive decay

A

84

61
Q

n:p of stable and unstable nuclides

A

stable: n:p = 1
unstable: n:p > 1

62
Q

arrange nuclides in increasing stability

[# of protons - # of neutrons]

A

even-even > even-odd > odd-even > odd-odd

63
Q

___ emission can lower n:p while ___/___ can increase n:p

A

beta emission
positron emission/electron capture

64
Q

nuclei that contain these magic numbers of protons or neutrons are generally more stable

A

2, 8, 20, 50, 82, 126

65
Q

Binding Energy formula

A

∆E = ∆mc²
∆m = m_products - m_reactants

66
Q

most stable nuclei;

to achieve maximum stability, those with lesser mass # needs to break up (fission) while those with greater mass # needs to combine (fusion)

A

Fe-26

67
Q

in terms of p, n, e

atomic mass (A) = ___
atomic number (Z) = ___
total p, n, e = ___

A

atomic mass (A) = p + n
atomic number (Z) = p = e (if neutral)
total p, n, e = A + Z - charge

68
Q

photoelectric effect/energy of a photon formula

A

E = hv = KE + Φ

h = Planck’s constant, J/s
v = frequency, 1/s
Φ = work function (multiply w/ charge of e^- in J/eV)

69
Q

relationship between c, v, λ

A

c = vλ

c or c_0 = speed of light in vacuum, m/s
λ = wavelength, m

70
Q

what is wave number

A

1/λ

71
Q

KE of electron formula

A

KE = 1/2 * m_e * v^2

72
Q

Bohr’s Theory and Hydrogen Atom formula

A

E_n = -R_H * (1/n^2)

R_H = Rydberg constant, 1/m
n = hydrogen level

72
Q

Bohr’s Theory and Hydrogen Atom formula

A

E_n = -R_H * (1/n^2)

R_H = Rydberg constant, 1/m
n = hydrogen level

73
Q

Hydrogen Spectral Series

A

n = 1 Lyman: UV
n = 2 Balmer: UV-Vis
n = 3 Paschen: IR
n = 4 Brackett: IR

74
Q

Physical Properties in the Periodic Table

↘️ increasing trend

A

Effective Nuclear Charge

75
Q

formula for no. of lone pairs in VSEPR Model

A

Lone Pair = 1/2 [valence_cat + charge_molec + (charge_anion)(n_anion)]

76
Q

VSEPR Model BP, LP, Shape (7)

A

BP LP Shape
2 1 Bent
2 2 Bent
3 1 Trigonal Pyramidal
3 2 Trigonal Square
4 1 Square
4 2 Square Planar
5 1 Square Pyramidal

77
Q

Hydrogen bonding

A

H bonded with N, O, F

78
Q

Formula for solving vapor pressure of a solvent over a solution

A

Raoult’s Law

P_soln = x_solv * P0_solv

79
Q

∆S (solution) ___ ∆S (pure solvent)

A

∆S (solution) > ∆S (pure solvent)
Solutions are more disordered than a pure solvent

80
Q

van’t Hoff factor (i)

A

for electrolytic solutions
∆T_b = i * K_b * m
∆T_f = i * K_f * m
π = iMRT

i = 1 for organic and non-electrolytic solutions

81
Q

degree of dissociation (α)

A

α = (i - 1) / (v - 1)

v = max no. of particles

82
Q

if repulsion > attraction, the nucleus ________

A

disintegrates, emitting particles and/or radiation

83
Q

if repulsion < attraction, the nucleus ________

A

is stable

84
Q

the principal factor that determines stability

A

neutron-to-proton ratio (n:p)

85
Q

All isotopes of ____ and ____ are radioactive

A

technetium and promethium

86
Q

Binding energies per nucleon are greatest for elements in the _______

A

iron, cobalt, and nickel region

87
Q

rate of decay at time t

A

rate = kN

k = rate constant
N = no. of radioactive nuclei present at time t

88
Q

half-life of radioactive decay

A

t_1/2 = ln 2 / k

89
Q

radioactive decay formula

A

N = N_0 * e^-k(t)

*N = naiwan, not emitted

90
Q

formula for Kb and Kf when not given

A

Kb = MRT^2 / ∆H_vap
Kf = MRT^2 / ∆H_fusion

91
Q

Fajan’s Rule (3)

A
  1. large charges
  2. small cation, large anion
  3. pseudo-octet
92
Q

[Metals Reactivity Series]
Highly Reactive Elements

A

Cs Fr Rb

K Na Li Ba Ra

Sr Ca

93
Q

[Metals Reactivity Series]
Moderately Reactive Elements

A

Mg Al Ti Mn Zn

Cr Fe Cd Co Ni

Sn Pb

(H)

94
Q

[Metals Reactivity Series]
Least Reactive Elements

A

Sb Bi Cu W

Hg Ag Au Pt

95
Q

Binding Energy per Nucleon

A
  1. ∆m = amu×(1.66×10-²⁷) - (#p×mp + #n×mn)
  2. ∆E = ∆mc² in J/nucleus
  3. Divide by atomic mass
  4. Convert 1 meV = 1.6×10-¹³

Day 1: Physical and Chemical Principles (2 decks)

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