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MODULE 1 > 1.1 General Chemistry > Flashcards

1.1 General Chemistry Flashcards

1
Q

SOLID (shape & volume)

A

Definite *non-compressible

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2
Q

SOLID (Molecular motion)

A

Vibration *2 stones

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3
Q

LIQUID (shape)

A

Indefinite *assumes container shape

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4
Q

LIQUID (volume)

A

Definite

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5
Q

LIQUID (molecular motion)

A

Gliding *ex. water falls

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6
Q

GAS (shape & volume)

A

Indefinite *compressible

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7
Q

GAS (molecular motion)

A

constant random

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8
Q

Plasma/Ionized Gas

A

4th state; most abundant state of matter
• Has p+ and e- (thus, greatly affected by magnetic field)
• Ex. ionized Ne light, Aurora, Stars, Sun

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9
Q

IFA Strength most ↑ or strongest:

A

S > L > G > P

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10
Q

Enthalpy (heat/ reaction energy):

A

P > G > L > S

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11
Q

Melting

A

*aka: Fusion, Liquefaction, Thawing

Solid to Liquid

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12
Q

Freezing

A

Liquid to Solid

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13
Q

Evaporation

A

Liquid to Gass

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14
Q

Condensation

A

Gas to Liquid

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15
Q

Sublimation

A

*moth/naphthalene balls

Solid to Gas

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16
Q

Deposition

A

*dry ice/cardice

Gas to Solid

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17
Q

Recombination

A

*aka: Deionization

Plasma to Gas

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18
Q

Ionization

A

Gas to Plasma

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19
Q

Pure substance

A
  • Element

* Compound

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20
Q

Element

A

simplest form of substance

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21
Q

Compound

A

2 or more chemical united (separated via

chemical means)

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22
Q

Mixture

A
  • Homogeneous

* Heterogeneous

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23
Q

Mixture

A

2 or more substance wherein individual substance identifies are retained (separated via physical means. Alcohol +
Water via distillation)

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24
Q

Homogeneous

A

1 phase; solution *clear colored

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25
Q

Heterogeneous

A

2 phases; suspension, colloid *ex. milk

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26
Q

Extrinsic Property “Dependent”

A

Length, mass/weight, volume, pressure, entropy, enthalpy, electrical resistance

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27
Q

Intrinsic Property “Independent”

A

Density/ SpGr (water = 1g/ml or cc), viscosity (resistance to flow), velocity (m/sec), temperature, color

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28
Q

Law of Conservation of Mass/ Matter

A
  • Antoine Lavoiser

- Mass/ Matter is always constant (neither created nor destroyed)

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29
Q

Law of Definite/Constant Proportions

A
  • Joseph Proust (Proust’s law)
    • Chemical compounds always contain the exact proportion of element in fixed ratio (by mass)
    • Ex. H2O →2H + O, C6H12O6 = CH2O
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30
Q

Law of Multiple Proportion

A 
- John Dalton
• When 2 elements form more than 1 compounds, it can be expressed in a fixed whole number (by mass)
• Ex. CO → 28g/mole, CO2 → 44g/mole
C = 12g/mole
O = 16g/mole
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31
Q

Law of combining weights

A

• Proportions by weight when chemical reaction takes place can be expressed in small integral unit
• Ex. MgO → 40g/mole (100%)
Mg = 24g/mole (60%); O = 16g/mole (40%)

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32
Q

Democritus

A
  • atomos

- “indivisible”

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33
Q

John Dalton

A
  • Billiard ball

- Matter is made up of atoms

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34
Q

Postulates

A
  • Elements are composed of indivisible, indestructible atoms
  • Atoms alike for a given element (isotopes)
  • Atoms of different elements differ in size, mass & other properties (isobars)
  • Compound are formed form 2 or more atoms at different elements
  • Atoms combined in simple numerical ratios to form compounds
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35
Q

J.J. Thompson

A
  • Plum Pudding/Raisin bread

- e- in (+) framework

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36
Q

Ernest Rutherford

A
  • discoverer of proton (Nuclear - Gold foil/a-scattering experiment)
  • atom is mostly empty; (+) particles in nucleus
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37
Q

Neil Bohr

A
  • Planetary

- mostly used

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38
Q

Erwin Schrodinger

A
  • Quantum/Mechanical/e- cloud

- Modern atomic Model; estimates the probability of finding an e- in certain position (i.e. at e-cloud/ orbital)

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39
Q

Proton

A
  • (+) ion
    • Atomic number (basis of electronic configuration)
    • Ernest Rutherford
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40
Q

Electrons

A
  • (-) ion
    • negligible weight 1,836x lighter that p+
  • J.J. Thompson
  • R.A. Millikan
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41
Q

J.J. Thompson

A

• Cathode ray tube: e- m/2 ratio

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42
Q

R.A. Millikan

A

Oil drop experiment: measure accurate charge and mass of e-

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43
Q

Neutrons

A
  • no charge
    • Atomic mass (Nucleon) = p+ + n0
    • James Chadwick
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44
Q

Eugene Gold Stein

A

discovered anode rays

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45
Q

Electrochemistry

A

– particle separation based on e-

• Ex: Capillary electrophoresis - separation of compounds based on electrophoretic mobility

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46
Q

ANODE (charge)

A

(+) electrode

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47
Q

ANODE (undergoes:)

A

Oxidation

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48
Q

CATHODE (charge:)

A

(-) electrode

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49
Q

CATHODE (undergoes:)

A

Reduction

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50
Q

RED CAT ELECT IN

A

• REDuction happens in CAThode where ELECTrons get IN

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51
Q

VILEORA

A

• Valence Increase, Loses e-, undergoes Oxidation, Reducing agent

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52
Q

VDGEROA

A

• Valence Decrease, Gains e-, undergoes Reduction, Oxidizing agent (KMnO4-, Na2Cr2O7)

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53
Q

Isotopes

A
  • same p+/atomic number/ element

* differ in atomic mass

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54
Q

Non-isotopes

A

19F, 127I, 31P, etc.

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55
Q

Main isotopes

A

+1: 1H, 12C, 14N, 32S, 35Cl ; +2: 16O, 79Br

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56
Q

Isobars

A
  • same atomic mass

* differ in elements

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57
Q

Isomers

A
  • same molecular formula

* differ in structure

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58
Q

Molecule

A

– aggregate of 2 or more atoms in definite arrangement held together by chemical bonds

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59
Q

Ions

A

– with net (+) or (-) charge

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60
Q

Empirical formula

A

– simplest whole number ratio (might be same with MF). Ex: CH2O vs. C6H12O6

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61
Q

Intermolecular FA/ Van der Waals/ Electrostatic

A
  • Between molecule; weak and short-lived

* Created by “molecule’s polarizability”; exerted when 2 uncharged atoms (n0) approach very closely

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62
Q

H-bonding

A
  • Strongest IFA

- H + S, O, N, X (electronegative atoms)

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63
Q

Keesom orientation (D-D)

A
  • > (next to H-bonding)

- Water-water

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64
Q

Debye Induction (D-ID)

A
  • > (3rd)

- Water-benzene

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65
Q

London Dispersion (ID-ID)

A
  • Weakest IFA

- Aromatics (Benzene-Benzene)

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66
Q

Dipole (D)

A
  • Polar
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67
Q

Induced Dipole (ID)

A
  • Nonpolar
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68
Q

Intramolecular FA

A
  • Within molecule
69
Q

Covalent

A
  • sharing of e-

- Nonmetal + Nonmetal (Glycosidic & Peptide bond)

70
Q

Ionic

A
  • Transfer of e-

- Metal + Nonmetal (NaCl)

71
Q

Glycosidic

A
  • ether bond S─O─S
72
Q

Peptide bond

A

– amide bond AA─peptide─AA bond

73
Q

Covalent Bonding (Lone pair)

A

Pair of valence electrons that are not shared with another atom in covalent bond

74
Q

Valence shell electron pair repulsion (VSEPR) theory

A

Predicts the geometry of the molecule as well as any bonded and unbonded electron pair

75
Q

Linear (180˚)

A
  • CO2

- Alkynes (Sp)

76
Q

Tetrahedral/bent (109.5˚)

A
  • CCl4 , H2O Alkanes (Sp3)

* 2 bonded pair, 2 unbonded pair

77
Q

Trigonal bipyramid

A
  • PF5
78
Q

Octahedral

A
  • SF5
79
Q

Valence bond theory

A

States that bonds are formed by sharing of electron from overlapping atomic orbitals (covalent)

80
Q

s = spherical

A

(sigma bond – stronger bond formed; headways overlap)

81
Q

p = dumbbell

A

(pi bond – weaker; sideways overlap)

82
Q

Molecular orbital theory

A

• States that bonds are formed from interaction of atomic orbitals from molecular orbitals

83
Q

Bonding

A
  • lower energy (stable)
84
Q

Antibonding

A
  • higher energy (unstable)
85
Q

Synthesis/ Combination/ Direct Union

A

A + B → AB

86
Q

Decomposition/ Analysis

A

AB → A + B

- e.g. Complete & Incomplete combustion

87
Q

Single Displacement

A

AB + X → AX + B

88
Q

Double Displacement/ Metathesis/ Exchange

A

AB + CD → AC + BD

- e.g. Neutralization, Precipitation

89
Q

Metals

A

Li > K > Ba > Ca > Na > Mg > Al > Mn > Zn > Cr > Fe > Cd > Co > Ni > Sn > Pb > H2 > Cu > Ag > Hg > Pt > Au

90
Q

Nonmetals (bases on electronegativity)

A

F > Cl > Br > I

91
Q

Covalent compounds

A
  • CO: Carbon monoxide
  • SiO2: Silicon dioxide
  • N2O: Dinitrogen monoxide
  • CCl4: Carbon tetrachloride
92
Q

Ionic compounds

A

Ex: Pb(NO3)4
• Classical: Plumbic nitrate
• Stock: Lead(IV) nitrate

93
Q

Monovalent

A 
\+1 = Group 1 (H, Li, Na, K ׀ Ag)
\+2 = Group 2 (Be, Mg, Ca, Sr, Ba ׀ Zn, Cd)
-2 = Group 6A (Oxide, Sulfide)
-1 = Group 7A (Fluoride, Chloride, Bromide, Iodide)
94
Q

+1 = Group 1

A

(H, Li, Na, K ׀ Ag)

95
Q

+2 = Group 2

A

(Be, Mg, Ca, Sr, Ba ׀ Zn, Cd)

96
Q

-2 = Group 6A

A

(Oxide, Sulfide)

97
Q

-1 = Group 7A

A

(Fluoride, Chloride, Bromide, Iodide)

98
Q

Multivalent (with variable charges)

A

+1, +2 = Hg, Cu
+1, +3 = Au
+2, +3 = Fe, Co, Ni
+3, +5 = Bi, Sb

99
Q

+1, +2

A

= Hg, Cu

100
Q

+1, +3

A

= Au

101
Q

+2, +3

A

= Fe, Co, Ni

102
Q

+3, +5

A

= Bi, Sb

103
Q

ClO-

A
  • Hypochlorite

- Hypochlorous acid (HClO)

104
Q

ClO2-

A
  • Chlorite

- Chlorous acid (HClO2)

105
Q

ClO3-

A
  • Chlorate

- Chloric acid (HClO3)

106
Q

ClO4-

A
  • Perchlorate

- Perchloric acid (HClO4)

107
Q

NO2-

A
  • Nitrite

- Nitrous acid (HNO2)

108
Q

NO3-

A
  • Nitrate

- Nitric acid (HNO3)

109
Q

SO3^2-

A
  • Sulfite

- Sulfite Sulfurous acid (H2SO3)

110
Q

SO4^2-

A
  • Sulfate

- Sulfuric acid (H2SO4)

111
Q

PO4^3-

A
  • Phosphate

- Phosphoric acid (H3PO4)

112
Q

HCO3-

A

Bicarbonate (Hydrogen carbonate)

113
Q

HSO3-

A

Bisulfite

114
Q

HSO4-

A

Bisulfate

115
Q

HPO4^-2

A

Biphosphate

116
Q

H2PO4^-1

A

Dihydrogen phosphate

117
Q

Aufbau Principle

A
  • Atoms may be built by progressive filling of energy of main energy sub level (i.e., levels of lower energy levels are occupied first)
  • s=2, p=6, d=10, f=14
118
Q

Principal Quantum Number (n = 1 to 7)

A
  • main energy level; size of orbital (electron cloud), distance of e- from nucleus
  • Ex. O2 = 1s2. 2s2. 2p4 (n=2)
119
Q

Azimuthal/ Angular Momentum (ℓ = 0 to 3)

A
  • Angular momentum & shape of orbital; subshell

* Ex. O2 = ℓ = 1

120
Q

ℓ = 0 ─ s :

A

sharp (spherical shape)

121
Q

ℓ = 1 ─ p :

A

principle (dumbbell shape)

122
Q

ℓ = 2 ─ d :

A

diffuse (clover leaf)

123
Q

ℓ = 3 ─ f :

A

fundamental

124
Q

Magnetic Quantum Number (mℓ = -ℓ, 0, +ℓ)

A
  • Orientation of orbital in space

* Ex. O2 = mℓ = -1, 0, +1

125
Q

Magnetic Spin (ms = + ½ , - ½ )

A 
• Magnetic moment/ Rotation
Spin
↑ = Incomplete; clockwise + ½
↑↓ = Complete; counterclockwise = - ½
• Ex. Oxygen = ms= + ½
126
Q

Diagmagnetism

A

– no unpaired e-

127
Q

Paramagnetism

A

– at least 1 unpaired e-

128
Q

• No 2 e- will have same set of quantum number (“exclusive”

A

Pauli’s exclusion theory

129
Q

• Impossible to predict/ accurately determine the particle’s velocity (position & momentum)

A

Heisenberg’s uncertainty theory

130
Q
  • Orbitals are filled up singly before pairing up

* Most stable arrangement of e- in subshells is the one with greatest no. of parallel spins.

A

Hund’s rule

131
Q

P₁𝑽₁ = 𝑷₂𝑽₂ 𝑜𝑟 𝑷 ∝
1/𝑣
• Temperature (in K)

A

Boyle’s/Mariotte

132
Q

𝑻₁𝑽₁ = 𝑻₂𝑽₂
𝑜𝑟 𝑽 ∝ �
• Pressure (in atm)

A

Charles

133
Q

𝑷₁𝑻₁ = 𝑷₂𝑻₂
𝑜𝑟 𝑷 ∝ 𝑻
• Volume (in L)

A

Gay-Lussac’s

134
Q 
𝑷₁𝑽₁
𝑻₁
= 
𝑷₂𝑽₂
𝑻₂
A

Combined

135
Q

𝑷𝑽 = 𝒏𝑹𝑻

A

Ideal

136
Q

• Equal volumes of different gases have same no. of moles at
STP
𝑽₁𝒏₁ = 𝑽₂𝒏₂
𝑜𝑟 𝑽 ∝ 𝒏 𝑜𝑟 𝑽/𝒏 = k

A

Avogadro’s

137
Q

• Total pressure in a mixture (non-interacting gases) is equal to the sum of the partial pressures of each gas. 𝑃𝑡 = 𝑃1 + 𝑃2 + 𝑃3

A

Dalton’s Law of Partial Pressures

138
Q

• Rate of effusion (diffusion) and speed gas are inversely proportional to the square root of their density providing the temperature and pressure are same for 2 gases

A

Graham’s

139
Q

Rate at which 2 gases mix

A

Diffusion

140
Q

Rate at which gas escapes through a pinhole vaccume

A

Effusion

141
Q

• Diffusion rate (flux) of liquid or gas is directly proportional to the concentration gradient (ftom high concentration to low
concentration)

A

Fick’s 1st Law

142
Q

𝑷𝒓𝒆𝒔𝒔𝒖𝒓𝒆 ∝ 𝑺𝒐𝒍𝒖𝒃𝒊𝒍𝒊𝒕𝒚

• Decrease temperature, Increase Pressure (i.e., sealed container), more CO2 is dissolved in water.

A

Henry’s Law of Gas Solubility

143
Q

Solute + Solvent

A

Solution

144
Q

• Study of energy conversion/transformation in the universe

A

Thermodynamics

145
Q

Allows exchange of energy and matter

A

Open System

146
Q

Allows exchange of energy but not matter

A

Closed System

147
Q

Does not allow exchange of both energy and matte

A

Isolated System “Adiabatic Walls”

148
Q
  • Independent (depends only on initial & final states of system)
  • Ex. Enthalpy (H), Internal energy (U), Gibb’s Free Energy (G), Entropy (S)
A

State Function

149
Q
  • Dependent

* Work and Heat

A

Non-state Function

150
Q

• If two systems are in thermal equilibrium respectively with a third system, they must be in thermal equilibrium with each
other

A

Zeroth Law

151
Q

• Energy is neither created nor destroyed but can be transformed from one form to another

A

1ST LAW: Law of conservation of Energy

152
Q

∆H is independent of reaction/steps that occurred (only the initial and final steps is the basis)

A

Hess’ Law

153
Q

∆H = (+) → heat is absorbed;

A

COLD (endothermic)

154
Q

∆H = (-) → heat is released;

A

HOT (exothermic)

155
Q
  • No way but UP

* For an isolated system, Total entropy can never decrease over time

A

2ND LAW: Law of Entropy

156
Q

Measure of system’s thermal energy per unit temperature; degree of disorderliness or randomness

A

Entropy (∆S)

157
Q
  • If an object reaches absolute zero temperature (0 K = -273.15 = -459.67 °)
  • Entropy of perfect, solid, crystalline substance is zero at absolute 0 temperature
A

3RD LAW

158
Q
  • Thermodynamic state function that combines enthalpy and entropy
  • ∆G = ∆H ‒ T∆S
A

Gibb’s free energy (∆G)

159
Q

• Study of reaction rates and reaction mechanism

A

Chemical Kinetics

160
Q
  • Change in concentration of a reactant or product concentration with time
  • aA + bB → cC + dD
A

Reaction Rate (M/s)

161
Q

• Expresses relationship of the rate of reaction to the rate constant (K) and concentration of reactants raised to some
power
• aA + bB → cC + dD

A

Rate Law

162
Q

• rate of chemical reaction is proportional to the number of collisions per time

A

Collision Theory

163
Q

• (Formation of Intermediate Complex) - rate depends on Ea required to form intermediate state (where new bonds are
formed and old bonds are broken)

A

Transition Theory

164
Q

= ↑ reactivity ↑ reaction rate (faster)

A

Nature of Reactants

165
Q

= ↑ concentration ↑ reaction rate

A

Concentration of Reactants (except Zero order)

166
Q

= ↑ reaction rate

A

Catalyst

167
Q

= ↑ SA ↓ particle size ↑ reaction rate ↓ reaction time

A

Surface Area

168
Q 
= ↑ Temp ↑ KE ↑ mobility of molecules ↑ collision ↑ reaction rate; 
Arrhenius Equation (T, Ea, RR)
A

Temperature

MODULE 1 (2 decks)

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