Inorganic Chemistry Flashcards
Dalton’s Atomic Theory (3)
- elements are composed of tiny indivisible particles called atoms
- in a compound, element A mass:element B fixed mass is a whole number/fraction
- chemical rxns only involve separation, combination or rearrangement of atoms
Law of Multiple Proportions
in a compound, element A mass:element B fixed mass is a whole number/fraction
Law of Conservation of Mass
chemical rxns only involve separation, combination or rearrangement of atoms
Law of Definite Proportions
a pure compound is made up of elements in the same proportion by mass
- Proust
Cathode Ray/Geissler Tube
Crookes and Geissler
determined ratio of electric charge to mass of electron to be -1.76×10^8 coul/g
Joseph John Thomson
determined charge of electron to be -1.60×10^-19
Robert Millikan
discovered xrays
Wilhelm Roentgen
discovered radioactivity in uranium
Becquerel
discovered radioactivity in uranium and polonium
Curie
[Who & What]
gold foil experiment
Rutherford
1. most of the atom is empty space
2. the positive charge is in the nucleus
discovered neutron
Chadwick
quantum number; average distance of electron from nucleus
Principal Quantum Number (n)
quantum number; tells shape of orbital
Azimuthal/Angular Momentum Quantum Number (l)
0 to n-1
quantum number; describes orientation of orbitals in space
Magnetic Quantum Number (ml)
-l to l
quantum number; shows spin of electrons
Spin Quantum Number (ms)
+1/2 (CW) or -1/2 (CCW)
[Rule/Principle]
orbitals of an atom must be filled up in increasing energy levels
Aufbau Principle
[Rule/Principle]
no two electrons can have the same set of quantum numbers; an orbital must have at most two electrons with opposite spins
Pauli’s Exclusion Principle
[Rule/Principle]
the most stable arrangement of electrons in subshells is one with more parallel spins
Hund’s Rule of Multiplicity
he arranged elements in triads i.e. Li-Na-K
Dobereiner
he arranged elements by atomic mass; found that every 8 elements had similar properties
Newlands
they arranged elements according to recurring periodic properties
Mendeleev and Meyer
he discovered the relationship bet the elements’ atomic number and frequency of xrays generated from bombarding the element with high-energy electrons
Moseley
states that properties of elements are functions of their atomic numbers
Modern Periodic Law
average distance between nucleus and valence electron
atomic size/radius
energy required to remove an electron from a gaseous atom in its ground state
Ionization Energy
lower IE, easier to form cation
change in energy when an electron is accepted by a gaseous atom to form an anion
Electron Affinity
measure of ability of an atom to attract a bonding electron
Electronegativity
Physical Properties in the Periodic Table
↙️ increasing trend
ARM
- Atomic Size
- Reactivity
- Metallic Property
Physical Properties in the Periodic Table
↗️ increasing trend
IEEE
- Ionization Energy
- Electron Affinity
- Electronegativity
formation of a bond is due to overlap of two atomic orbitals
Valence Bond Theory
a bond is formed when electrons in the bonding molecular orbital is greater than the electrons in the non-bonding molecular orbital
Molecular Orbital Theory
[Colligative Properties of Non-Electrolyte Solutions]
Boiling Point Elevation
∆T_B = K_B • m
K_B = ebullioscopic constant
[Colligative Properties of Non-Electrolyte Solutions]
Freezing Point Depression
∆T_F = K_F • m
K_F = cryoscopic constant
[Colligative Properties of Non-Electrolyte Solutions]
Vapor Pressure Lowering
∆P = x_solute • P_solvent
[Colligative Properties of Non-Electrolyte Solutions]
Osmotic Pressure (π)
π = MRT
M = molarity
R = 0.08206 L-atm/mol-K
K_B of water
0.52
K_F of water
1.86
Relationship between Kc and Kp
Kp = Kc(RT)^∆n
[Le Chatelier’s Principle]
Effect of Changing Concentration
high concentration to low concentration
[Le Chatelier’s Principle]
Effect of Changing Pressure (opposite for Volume)
increasing pressure (decreasing volume)
–> system shifts the reaction towards formation of less number of gaseous molecules
[Le Chatelier’s Principle]
Effect of Changing Temperature
⬆️ temperature favors endothermic reaction
⬇️ temperature favors exothermic reaction
[Le Chatelier’s Principle]
Effect of Adding a Catalyst
no effect
symbol, mass, and charge of
beta particle or electron
β or e
mass = 0
charge = -1
symbol, mass, and charge of
positron
β or e
mass = 0
charge = +1
symbol, mass, and charge of
proton or hydrogen nucleus
p or H
mass = 1
charge = +1
symbol, mass, and charge of
neutron
n
mass = 1
charge = 0
symbol, mass, and charge of
gamma ray
γ
mass = 0
charge = 0
symbol, mass, and charge of
alpha particle or helium nucleus
α or He
mass = 4
charge = +2
number of nuclear disintegrations per second
activity [=] Bq
rate of disintegration of 1 g of Ra
Curie (Ci)
Ci to Bq conversion
1 Ci = 3.7×10^10 Bq
Radiation absorbed dose (rd)
SI unit : Gy (gray)
1 rd = 10^-5 J/g tissue
1 Gy = 1 J/kg absorbing material
basically a helium nucleus
commonly found during radioactive decay
net result is to increase n:p ratio
alpha particle
basically an electron; emitted when n:p > zone of stability
- e comes from…
- β comes from…
beta particle
- atomic orbital
- nucleus
aka high energy proton
by-product of alpha particle decay
gamma ray
antimatter of electron; emitted when n:p < zone of stability
positron
usually accomplished by emission of gamma ray; inner orbital electron is captured by the nucleus to increase n:p
electron capture
a single ___ is rather unstable and will convert itself to a ___ and an ___
neutron, proton, electron
when a nuclide has __ or more protons, it tends to be unstable and undergo radioactive decay
84
n:p of stable and unstable nuclides
stable: n:p = 1
unstable: n:p > 1
arrange nuclides in increasing stability
[# of protons - # of neutrons]
even-even > even-odd > odd-even > odd-odd
___ emission can lower n:p while ___/___ can increase n:p
beta emission
positron emission/electron capture
nuclei that contain these magic numbers of protons or neutrons are generally more stable
2, 8, 20, 50, 82, 126
Binding Energy formula
∆E = ∆mc²
∆m = m_products - m_reactants
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)
Fe-26
in terms of p, n, e
atomic mass (A) = ___
atomic number (Z) = ___
total p, n, e = ___
atomic mass (A) = p + n
atomic number (Z) = p = e (if neutral)
total p, n, e = A + Z - charge
photoelectric effect/energy of a photon formula
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)
relationship between c, v, λ
c = vλ
c or c_0 = speed of light in vacuum, m/s
λ = wavelength, m
what is wave number
1/λ
KE of electron formula
KE = 1/2 * m_e * v^2
Bohr’s Theory and Hydrogen Atom formula
E_n = -R_H * (1/n^2)
R_H = Rydberg constant, 1/m
n = hydrogen level
Bohr’s Theory and Hydrogen Atom formula
E_n = -R_H * (1/n^2)
R_H = Rydberg constant, 1/m
n = hydrogen level
Hydrogen Spectral Series
n = 1 Lyman: UV
n = 2 Balmer: UV-Vis
n = 3 Paschen: IR
n = 4 Brackett: IR
Physical Properties in the Periodic Table
↘️ increasing trend
Effective Nuclear Charge
formula for no. of lone pairs in VSEPR Model
Lone Pair = 1/2 [valence_cat + charge_molec + (charge_anion)(n_anion)]
VSEPR Model BP, LP, Shape (7)
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
Hydrogen bonding
H bonded with N, O, F
Formula for solving vapor pressure of a solvent over a solution
Raoult’s Law
P_soln = x_solv * P0_solv
∆S (solution) ___ ∆S (pure solvent)
∆S (solution) > ∆S (pure solvent)
Solutions are more disordered than a pure solvent
van’t Hoff factor (i)
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
degree of dissociation (α)
α = (i - 1) / (v - 1)
v = max no. of particles
if repulsion > attraction, the nucleus ________
disintegrates, emitting particles and/or radiation
if repulsion < attraction, the nucleus ________
is stable
the principal factor that determines stability
neutron-to-proton ratio (n:p)
All isotopes of ____ and ____ are radioactive
technetium and promethium
Binding energies per nucleon are greatest for elements in the _______
iron, cobalt, and nickel region
rate of decay at time t
rate = kN
k = rate constant
N = no. of radioactive nuclei present at time t
half-life of radioactive decay
t_1/2 = ln 2 / k
radioactive decay formula
N = N_0 * e^-k(t)
*N = naiwan, not emitted
formula for Kb and Kf when not given
Kb = MRT^2 / ∆H_vap
Kf = MRT^2 / ∆H_fusion
Fajan’s Rule (3)
- large charges
- small cation, large anion
- pseudo-octet
[Metals Reactivity Series]
Highly Reactive Elements
Cs Fr Rb
K Na Li Ba Ra
Sr Ca
[Metals Reactivity Series]
Moderately Reactive Elements
Mg Al Ti Mn Zn
Cr Fe Cd Co Ni
Sn Pb
(H)
[Metals Reactivity Series]
Least Reactive Elements
Sb Bi Cu W
Hg Ag Au Pt
Binding Energy per Nucleon
- ∆m = amu×(1.66×10-²⁷) - (#p×mp + #n×mn)
- ∆E = ∆mc² in J/nucleus
- Divide by atomic mass
- Convert 1 meV = 1.6×10-¹³
