Inorganic Chemistry Flashcards by Therese Gaddi

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

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Law of Multiple Proportions

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

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Law of Conservation of Mass

chemical rxns only involve separation, combination or rearrangement of atoms

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Law of Definite Proportions

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

Proust

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Cathode Ray/Geissler Tube

Crookes and Geissler

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

Joseph John Thomson

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

Robert Millikan

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discovered xrays

Wilhelm Roentgen

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discovered radioactivity in uranium

Becquerel

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discovered radioactivity in uranium and polonium

Curie

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[Who & What]

gold foil experiment

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

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discovered neutron

Chadwick

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quantum number; average distance of electron from nucleus

Principal Quantum Number (n)

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quantum number; tells shape of orbital

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

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quantum number; describes orientation of orbitals in space

Magnetic Quantum Number (ml)
-l to l

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quantum number; shows spin of electrons

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

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[Rule/Principle]

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

Aufbau Principle

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[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

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[Rule/Principle]

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

Hund’s Rule of Multiplicity

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

Dobereiner

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

Newlands

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they arranged elements according to recurring periodic properties

Mendeleev and Meyer

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

Moseley

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states that properties of elements are functions of their atomic numbers

Modern Periodic Law

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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

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)

1. large charges 2. small cation, large anion 3. 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

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

Inorganic Chemistry Flashcards

(96 cards)