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Final Flashcards

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0
Q

NCS

A

thiocyanato-N

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1
Q

SCN

A

thiocyanato-S

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2
Q

Harmatite

A

Fe2O3

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3
Q

Fe2O3

A

Harmatite

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4
Q

zinc blende

A

ZnS

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5
Q

ZnS

A

zinc blende

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6
Q

copper pyrites

A

CuFeS2

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7
Q

CuFeS2

A

copper pyrites

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8
Q

Leaching

A

metal extracted from ore by a liquid

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9
Q

Unit Cell Chlorine

A

Face-Centred Cubic

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10
Q

Most abundant element in Earth’s crust

A

Al

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11
Q

Electronegativity

A

ability of an element to attract bonding electrons
- greatest in the upper right
ionic bond: difference > 1.9
covalent bond: 0 - 1.9

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12
Q

Polar

A

0.5 - 1.9

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13
Q

Best Lewis Structure

A

minimize formal charge

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14
Q

Exceptions to Octet Rule

A
  • elements >= 3rd row can hold more
  • less than 8 electrons (B)
  • odd electron species
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15
Q

Resonance Structures

A
  • multiple plausible Lewis structures
  • only move electrons
  • all must be valid
  • actual is a hybrid of all
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16
Q

VSEPR - Valence Shell Electron Pair Repulsion Theory

A
  • shows molecular shape/geometry

- maximize space between electron “group” and central atom

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17
Q

Electron-domain geometry

A
  • shape it is based on
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18
Q

Molecular geometry

A
  • final shape
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19
Q

Molecular Shape and Polarity

A
  • molecular shape can cancel dipoles
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20
Q

Bond order

A 
# of bonds
# bonding e - # anti-bonding e / 2
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21
Q

Bond energy

A

Energy needed to split bonds

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22
Q

Bond Order/Lengths/Energies

A

larger bond order = shorter bond length = larger bond energy

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23
Q

Favourable Transformation

A

Enthalpy is negative

Erxn = Ebreak + Eform

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24
Q

Valence Bond Theory

A
  • overlap of orbitals
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25
Q

Sigma Bond

A

cylindrically around bond axis

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26
Q

Pi Bond

A
  • for multiple bonds

- above and below sigma bond

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27
Q

Hybridization

A
  • # electrons groups bonding = # hybrid orbitals

- only for sigma bonds

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28
Q

Molecular Orbital Theory

A
  • describe all electronic/magnetic features
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29
Q

Anti bonding *

A
  • creates new node
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30
Q

2p sigma and pi orbital switch (MO theory)

A

B, Be, Li, C, N

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31
Q

Key Features of MO Theory

A
  • total number of MO = total number combined AO
  • in phase/bonding = low energy
  • out of phase/anti-bonding = high energy
  • obeys filling rules
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32
Q

Primary Valence

A

bonding between complex and counter ion

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33
Q

Secondary Valence

A

bonding between metal centre and ligands

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34
Q

Ligand

A
  • Lewis base
  • must be able to donate electrons
  • must be negative
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35
Q

H2O

A

Aqua

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36
Q

NH3

A

ammine

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37
Q

CO

A

Carbonyl

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38
Q

NO

A

nitrosyl

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39
Q

F

A

fluoro

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40
Q

Cl

A

chloro

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41
Q

Br

A

bromo

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42
Q

I

A

iodo

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43
Q

O

A

oxo

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44
Q

OH

A

hydroxo

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45
Q

CN

A

cyano

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46
Q

SO4

A

sulfato

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47
Q

S2O3

A

thiosulfato

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48
Q

NO2

A

nitrito-N

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49
Q

ONO

A

nirtrito-O

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50
Q

CH3NH2

A

methylamine

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51
Q

C5H5N

A

pyridine

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52
Q

Chelating Agent

A

polydentante ligand

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53
Q

oxalato

A

bidentate

C2O4

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54
Q

ethylenediamine

A

bidentate

C2H4(NH2)2

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55
Q

ethylenediamminetetraacetato

A

hexadentate (6)

C10H12N2O8

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56
Q

Polydentate in blood

A

porphyrin ring

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57
Q

Name Coordination Compound

A
  • name cation first
  • ligands in alpha order
  • use prefixes on ligands
  • roman numerals for metals
  • add “-ate” to end of metal in anion
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58
Q

Structural Isomers

A
  • coordination
  • ionization
  • linkage
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59
Q

Coordination Isomerism

A
  • switch ligands on a metal centre
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60
Q

Ionization Isomerism

A
  • switch counter ion/ligand
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61
Q

Prefix change CC

A

if prefix in name
prefixes change to
bis, tris, tetrakis

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62
Q

Linkage Isomerism

A
  • donor atom in the ligand is different

- shown in name -O- -N-

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63
Q

Stereoisomers

A

geometric

optical(enantiomers)

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64
Q

Geometric Isomerism

A 
- differ in relative orientation of ligands
cis - similar ligands beside each other
trans - opposite sides
put in front if name
- different properties
- square planar: MA2B2
- octahedral: MA4B2
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65
Q

Optical Isomers

A

Enantiomers

  • non-superimposable mirror images (non-symmetrical)
  • place of attachment of polydentate ligands
  • similar properties
  • acts differently in polarized light
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66
Q

Crystal Field Theory

A
  • model for bonding in transition metals

- d orbitals

67
Q

Octahedral Crystal Field

A

dz^2 dx^2-y^2

dxy dxz dyz

68
Q

Crystal Field Splitting Energy

A
  • determined by metal ion and nature of ligands (spectrochemical series)
69
Q

Spectrochemical Series

A

strong field = large E = low spin

weak field = small E = high spin

70
Q

Tetrahedral Crystal Field

A

dxy dxz dyz

dx^2-y^2 dz^2

71
Q

Square Planar Crystal Field

A

dx^2-y^2
dxy
dz^2
dyz dxz

72
Q

Crystal Field Splitting Diagram

A
  • coordination number
  • shape
  • oxidation state
  • number of d electrons
  • strong or weak field ligands
  • draw energy diagram
73
Q

Colours

A 
higher energy (v)
shorter ¥
lower energy (v)
longer ¥
74
Q

Colour absorbed

A

white light - colour observed

75
Q

Weak Field and Colour

A

low energy = red/yellow absorbed = blue/violet colour

76
Q

Strong Field and Colour

A

strong field = high energy = blue absorbed = yellow/red colour

77
Q

Metallurgy

A
  • separating metal from its ore
78
Q

Ore

A

Purified minerals

79
Q

Gangue

A

Matrix

- impurities within minerals

80
Q

Purification of Ore/Separation

A
  • removal of gangue
    i) Gravity Separation Process/Hydraulic Washing
    ii) Froth Flotation Process
    iii) Cyclonic Winds
81
Q

Gravity Separation Process

A
  • heavy metal oxides (Fe2O3)
  • powdered ore on sloping floor
  • washed by strong current of water
  • lighter impurities washed away
  • heavier ore left
82
Q

Hydraulic Washing

A
  • heavy metal oxides (Fe2O3)
  • powdered ore on sloping floor
  • washed by strong current of water
  • lighter impurities washed away
  • heavier ore left
83
Q

Froth Flotation Process

A
  • light metal sulphides (ZnS, CuFeS2)
  • sulphide are only moistened by oil
  • oxides and gangue particles moistened by water
  • powdered ore mixed with water & pine oil (foaming agent)
  • stirred by compressed air
  • ore sticks to froth and is skimmed off
  • ore concentrated
  • separation by affinity
84
Q

Coordination Number determines

A

shape of complex

octahedral

85
Q

Extraction of Metals

A
  • no universal method
    i) Roasting
    ii) Smelting
    iii) Calcination
    iv) Electrolysis
    v) Leaching
86
Q

Roasting

A
  • heavier metals (Cu, Zn, Fe…)
  • ore converted to metal oxide (oxidation)
  • ore heated below melting point in blast furnace with air
  • volatile impurities (S, As, Sb) are oxidized and escape as gases
  • mass is porous and easily reduced
    ZnCO3(s) > ZnO(s) + CO2(g)
87
Q

Primary colours

A

red, green, blue

88
Q

Red & Green

A

yellow

89
Q

Red & Blue

A

Magenta

90
Q

Blue & Green

A

cyan

91
Q

Smelting

A
  • roasting that produces a liquid
  • reduces oxide metal to free metal (reduction)
  • done in blast furnace
    HgS + O2 > Hg(l) + SO2
    ZnO + C > Zn(l) + CO
92
Q

Calcination

A
  • carries out in case of carbonate and hydrated ore
  • ore converted to metal oxide by heating below melting point without air (oxidation)
  • volatile impurities removed as gas
  • mass becomes porous
    CuCO3 (Malachite) • Cu(OH)2 > 2CuO + H2O + CO2
    MCO3 > MO + CO2
    2MS + 3O2 > 2ZnO + 2SO2 (g)
93
Q

ZnCO3

A

Calamine

- calcination

94
Q

Electrolysis (Purification)

A
  • noble metals (Au, Ag, Zn…)

- electrolysis of chloride, oxides or hydroxides

95
Q

Purification of Metals

A

i) Electrolytic Refining

ii) Thermal Method/Carbonyl Method

96
Q

Electrolytic Refining

A
  • noble metals (Cu, Ag, Au, Ni, Zn…)
  • blocks of impure metal at anode
  • thin sheet pure metal at cathode
  • solution of salt of metal as electrolyte (CuSO4)
  • pass current through: pure ions move
  • Cu (2+) > Cu + 2e-
  • impurities dissolve or fall
  • 99.98% pure
97
Q

Thermal Method

A
  • refine metals like Ni and Fe
  • impure metal heated with coke, CO, or H carbonyl is formed and decomposed
    Ni + 4CO > Ni(CO)4 > Ni + 4CO
    first @ 500°C, second @ 1300°C
    ZnO + C > Zn + CO
    ZnC + CO > Zn + CO2
98
Q

CO charge

A

0

99
Q

Carbonyl Method

A
  • refine metals like Ni and Fe
  • impure metal heated with CO, carbonyl is formed and decomposed
    Ni + 4CO > Ni(CO)4 > Ni + 4CO
    first @ 500°C, second @ 1300°C
100
Q

Difference Structural and Stereoisomers

A

structural - have different connectivities

stereoisomers - different spatial arrangements

101
Q

Manufacture steel from … to form… using

A

pig iron (brittle iron with high carbon content)
highly utility iron with controlled carbon content
the Bessemer Process

102
Q

Bessemer Process

A
  • blow cold air (oxygen) through molten pig iron (3-4%) to remove impurities at high pressure in a converter
  • oxidizes impurities
103
Q

Steel

A
  • alloy of carbon and iron
  • 0.15 - 1.50% carbon content with trace impurities (S, Mn, Si, P)
    Fe2O3 + CO2 > 2Fe(l) + CO2(g)
104
Q

Classifications of Steel

A

i) Mild Carbon Steel
- 0.15-0.30%
- low tensile strength
- structural steel
ii) Medium Carbon Steel
- 0.30-0.80%
- balance of ductility and strength
- automobiles
iii) High Carbon Steel
- 0.80-1.50%
- very strong
- high strength wires

105
Q

Iron Triad

l

A
  • Iron (Fe)
  • Cobalt (Co)
  • Nickel (Ni)
  • similar properties
    • 2+ ions
    • ferromagnetic
106
Q

Iron

A
  • 4th most abundant in Earth’s crust
  • hemoglobin (transports oxygen)
    • heme: iron atom in large heterocyclic ring (porphyrin)
    • CO takes place of oxygen
107
Q

Intermolecular Forces

A
  • mutual attraction of unlike charges

- stronger forces = harder to break apart

108
Q

NO3 charge

A

-1

109
Q

Alkali Metals

A
  • very reactive metals
  • soft (softer as move down)
  • low density
  • readily loses electron
  • releases H2 gas in water
    M + H2O > MOH + 1/2H2
  • explosive further down
  • highly reactive with oxygen
    2M(+) + O(2-) > M2O
    - Li
110
Q

charge NO

A

0

111
Q

LiAl(SO3)2

A

Spdoumene

- industrial ceramics, phones, batteries

112
Q

Salt Deposits

A

NaCl
KCl
Na2CO3

113
Q

Pollucite

A

MAl(SiO3)2

114
Q

Peroxide (dioxide)

A

with Na

2Na(+) + O2 (2-) > Na2O2

115
Q

Superoxide

A

with K, Rb, Cs

K(+) + O2(-) > KO2

116
Q

Alkaline Metals Applications

A 
Closed Breathing Apparatus
   4KO2 + 2H2O > 4KOH + 3O2
Fireworks/Flame Test
High Power Density Batteries
Brain Neurons
- send/receive with Na+ and K+
Salt
Manic Depression Medecine
117
Q

Alkaline Earth Metals

A
  • readily loses 2 electrons
  • forms Basic Oxides
    MO + H2O > M(OH)2
    M(OH)2 > M(2+) + 2(OH)(-)
  • commonly compounded with Al, SO*, CO3, SiF6 (silicates)
  • less reactive than alkali metals
  • found as minerals
  • more reactive as size increases
    Be/Mg does not react in cold water
    Ca/Sr/Ba reacts with cold water
    M + 2H2O > M(OH)2 + H2
118
Q

Ionic Characteristics of Alkaline Earth Metals

A

Be behaves as a covalent molecule (electronegative)

MgX2, CaX2, SrX2, BaX2 acts as salts

119
Q

Beryl

A

BeO•Al2O3 6SO2

120
Q

Emerald

A

Be3Al2(SiO3)6

121
Q

Limestone

A

CaCO3

  • slightly soluble in acidic water
  • stalactites and stalacmites
122
Q

Diagonal Relationships

A
  • similar characteristics (size,…)
    Li & Mg
    B & Si
    C & P
123
Q

Hard Water

A
  • water with high levels of Ca & Mg salts
    Type I: Temporary Hardness
    Type II: Permanent Hardness
124
Q

Hard Water Problems

A 
Bad Taste
Scaling & Spotting on Wet Surfaces
Cloudy Ice Cubes
Laxative Effect
Accumulation of "mineral fur" around faucet outlet
Boiler Scale
    Ca(2+) + 2HCO3(-) > Ca(2+) + CO3(2-)
Kills soap
- hydrophillic ends that normally removes grease joins with hard water to form a precipitate
125
Q

Type I: Temporary Hardness

A
  • caused by the presence of Calcium and Bicarbonate (HCO3-)
  • removed by boiling
    • forms carbonate from bicarbonate and precipitates calcium carbonate out of solution
      2HCO3(-) > CO3(2-) + CO2
  • add lime
    CaHCO3 + CaOH > 2CaCO3 + 2H2O
126
Q

Type II: Permanent Hardness

A
  • cannot be removed by boiling
  • caused by a presence of CaSO4 and MgSO4 and or CaCl2 and MgCl2 in water (more soluble with heat)
  • removed using water softener or exchange column
    CaSO4 + NaCO3 > CaCO3 + NaSO4
127
Q

Applications of Alkaline Earth Metal Mg

A
  • lighter cars > fuel economy
  • obtained by electrolysis: Dow Process
    MgCl2 > Mg + Cl2
  • solve rust with Fe/Si/Mg alloy
128
Q

Applications of Alkaline Earth Metal Ca

A

Cement
- binder: substance which sets and hardens independently
CaCO3 (limestone) >(heat) CO2 + CaO (quicklime)
CaO + SiO2(sand) >(water & CO2) CaCO3 + SiO3

Humans (1kg)

  • bones: CaPO4H
  • teeth (apatite): Ca5(PO4)3OH
    • cavities: Ca5(PO4)3OH + H(+) > H2O + Ca(2+) + HPO4(2-)
    • fluoride: Ca5(PO4)3OH + F(-) > Ca5(PO4)3F
129
Q

Intermolecular Forces depend on… and determine…

A
  • charge
  • distance (size)
  • molecule’s structure
  • state (solid/liquid/gas)
  • boiling/melting point
130
Q

Larger charge =

A

Stronger attraction

131
Q

Longer distance =

A

Weaker attraction

132
Q

n-Alkane

A

CH3 - (CH2)n - CH3

133
Q

Intermolecular forces are ____ than intramolecular forces

A

smaller

134
Q

London Dispersion Forces

A
  • in all bonds
  • created by instantaneous dipoles
  • increase with shape and size/mass
  • weak
135
Q

Polarizability

A
  • large atoms are more polarizable because there is more space to move
136
Q

Dipole-Dipole Force

A
  • caused by permanent NET dipole
  • stronger than dispersion forces (except in large molecules)
  • weaker than ionic/covalent bonds
137
Q

Solubility

A

like dissolves like

138
Q

Hydrogen Bonding

A
  • H bonded to N, O, F
  • highly electronegative
  • lone pair of electrons
  • strongest of the three
  • directional bond
  • weaker than covalent/ionic bonds
  • Water/DNA/Kevlar
139
Q

Molecules of similar nature have stronger forces when they are

A

larger

140
Q

More surface area = _____ forces

A

stronger

141
Q

Simple Cubic Unit Cell

A
  • identical ions at all 8 corners
  • total 1 ion per cell
    Coordination Number: 6
142
Q

Body Centred Cubic Unit Cell

A
  • identical ions at all 8 corners and 1 in the middle
  • total 2 ions per cell
    Coordination Number: 8
143
Q

Face Centred Cubic Unit Cell

A
  • identical ions at all 8 corners and 6 on the faces
  • total 4 ions per cell
    Coordination Number: 12
  • cubic closest packed
144
Q

Lattice Energy

A

more negative = stronger ionic bond

145
Q

Network Solids

A
  • non-molecular solid of covalent bonds
    quartz - SiO2
  • non-molecular solid
146
Q

Allotropes of Carbon

A 
diamond
- 4 e- used, insulator
graphite
- 3 e- used, conductor
fullerenes
- carbon-cage molecular (C60)
nanotubes
- 3 e- used, rolled-up graphene sheet, conductive, strongest
147
Q

Ionic Solids

A
  • non-molecular solids held together by ionic bonds

- highly organized lattice made of unit cells

148
Q

Ion-Dipole Attraction

A
  • in mixture/solution/liquid
  • ions attracted to dipole in polar molecule
  • stronger than hydrogen bonding
149
Q

Coordination Number in a Unit Cell

A
  • number of oppositely charged ions an ion is in contact with
  • high coordination number = stronger attractive forces
150
Q

Classify Crystalline Solids

A 
I. Molecular Solids
II. Ionic Solids
III. Atomic Solids
- non-bonding: held by dispersion
- metallic: held by metallic bonds
- network covalent: held by covalent bonds
151
Q

Molecular Solids

A
  • composed of molecules
  • held together by dispersion forces, dipole-dipole and H bonds
  • low melting point
152
Q

Ionic Solids

A
  • composed of ions
  • held together by ions charges
    • non-directional
  • higher coordination number = more stable solid
    • depends on size of ions
  • fairly high boiling point
  • non-conductors as solids
  • good conductor as liquids
  • soluble in polar liquids (water)
153
Q

Metallic Atomic Solids

A
  • strength depends on size and charge of cations
  • always in closed-packed arrangements
  • always cations
  • hardness varies
  • melting point varies
  • ductile/malleable
  • great conductor
154
Q

Network Covalent Non-Bonding Atomic Solids

A
  • noble gases in solid form
  • held by very weak dispersion forces
  • closed packed structure
155
Q

Network Covalent Solids

A
  • held by covalent bond
  • no closed packed arrangement (bonds are directional)
  • very high melting point
  • very hard
  • non-conductors
156
Q

chiral

A

optical isomer

157
Q

Cyclonic Winds

A
  • upwards airstream brings lighter particles up and leaves the heavier ore
  • separation by density
158
Q

Flux

A

added to react with non-volatile gangue to create low melting waste product that is easy to separate

159
Q

Slag

A

waste liquid separated from molten metal by density

SiO2(gangue) + CaCO3(flux) > CO2(g) + CaSiO3(slag)

160
Q

Zone Refining

A
  • move rod of material past a heated coil

- impurities concentrate in molten zoe

161
Q

Hydrometallurgy

A
  • use aqueous solution to extract metal from its mineral
162
Q

Manufacture Glass

A

Na2CO3

163
Q

Alkaline Earth Metals

A

form peroxides

Ba + O2 > BaO2

164
Q

Alkaline Metals: Thermal Decomposition of Carbonates

A

MCO3 > MO + CO2

CHEM 110 (2 decks)

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