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Chem 171 > Focus 8/9 > Flashcards

Focus 8/9 Flashcards

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1
Q

reactions to form hydrogen

A

reforming reaction: CH4 + H2O —-(ni)–> CO + 3H2

shift reaction: CO + H2O —-> CO2 +H2

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2
Q

hydrogen forms (ions and state of matter)

A

H+,H-

transparent gas

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3
Q

what does hydrogen bond with?

A

hydrides with every other element in the periodic table except some rare gases and indium and thallium

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4
Q

Hydrogen with groups 1-2

A

salt-like hydrides

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5
Q

hydrogen with groups 3-12

A

metallic hydrides: black, powdery, electrically conducting solids

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6
Q

hydrogen with groups 13-17

A

molecular hydrides, many of which are gases

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7
Q

hydrogen bond

A

interaction between the H in an H-O- group with some other O atom

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8
Q

what molecules do hydrogen bonds exist for

A

FHF, OHF, NHF, NHO, NHN

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9
Q

what do hydrogen bonds come from?

A

coulomb attraction between partial charges and from weak bonding interactions

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10
Q

why are hydrogen bonds important?

A

ice floats bc of h bonds
h bonds hold dna together
h bonds determine important features of protein structure

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11
Q

how are pure alkali’s made?

A

electrolysis

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12
Q

Downs Process

A

Na+ + Cl- –> Na + 1/2Cl (g)

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13
Q

applications of alkali metals

A

NaHCO3 - baking soda - reacts w weak acid to form CO2 in bread
NaCO3 - washing soda - provides carbonate in solution that precipitates Mg2+
NaNO3,KNO3 - oxidizing agent in black gunpowder, also used in matches

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14
Q

how are pure alkaline earths made?

A

electrolysis of soluble salts

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15
Q

dow process

A

MgCl2 –> Mg2+ + 2Cl- –> Mg(s) + Cl2

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16
Q

beryllium properties

A

both metallic and nonmetallic (does not react with water) properties
unlike the rest of the alkaline earths that form hydrides, halides, hydroxides, etc.

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17
Q

difference between alkalis and alkaline earths in terms of solubility

A

many of the alkaline earth salts are not water soluble

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18
Q

primary uses of alkaline earths

A

Mg(OH)2 milk of magnesia
MgSO4 epsom salts
CaO quicklime, which reacts with water to give Ca(OH)2 slaked lime –> used for agriculture
concrete

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19
Q

boron application

A

production of stiff light fibers that are used in plastics

i.e. aircraft, tennis rackets, golf clubs

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20
Q

boron compounds

A

BF3, BCl3 (boron trihalide) is an industrial catalyst, acts as a lewis acid
NaBH4 (sodium borohydride) is an important reducing agent

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21
Q

where does aluminum come from?

A

bauxite (Al2O3 * xH2O)

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22
Q

what is boron mined as/where does it come from?

A

borax (Na2B4O7 * xH2O)

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23
Q

how do we get pure Al from bauxite?

A

bauxite is electrolyzed in the Hall process

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24
Q

aluminum compounds

A

Al2O3 (alumina) which has several crystal forms: alpha-Al2O3 = corundum, used in sandpaper, gamma-Al2O3 used in chromatography
AlCl3*6H2O used as deodorant and antiperspirant

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25
Q

forms of pure carbon

A 
diamond
graphite (the most stable at room temp)
fullerenes (C60)
carbon nanotubes
soot
activated charcoal
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26
Q

other important inorganic carbon compounds

A

CCl4, CHCl3, CH2Cl2 important solvents
CF4 (refrigerant), CBr4 (fire extinguishing)
SiC (silicon carbride/carborundum) used as an abrasibe

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27
Q

what is silicon made from?

A

from SiO2 in a reaction with graphite in an electric arc furnace

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28
Q

zone refining

A

used to produce ultrapure Si needed for semiconductor manufacturing
electric heater is swept across a cylindrical sample, locally melting the Si. impurities collect in the molten state

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29
Q

forms of silicon

A

pure silicon: diamond structure

amorphous silicon, used in photovoltaics

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30
Q

silicon applications

A

field effect transistors

solar cells

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31
Q

silicon compunds

A

silica (SiO2) used in making glass, ceramics
silica gel (hydrated SiO2) used from chromatography media and as a drying agent
aluminosilicates (replace Si4+ by some amount of Al3+ in silica)
silicones (-O-Si-O-Si-) used as lubricants and for waterproofing

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32
Q

germanium compared to silicon

A

germanium is a sei conductur similar to Si, but much less important
Ge has smaller band gap

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33
Q

how is tin produced?

A

from SnO2 by reaction with C

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34
Q

how is lead produced?

A

from PbS (galena) by oxidation, then reaction with C

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35
Q

lead applications

A

past: pipes, glazes, paint
now: x-rays, lead-acid batteries

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36
Q

how is nitrogen produced?

A

liquifying air, followed by fractional distillation

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37
Q

significance/applications of nitrogen

A

essential for life

actively involved in many chemical processes

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38
Q

haber-bosch process

A

industrial process for making ammonia: N2 + 3H2 –>3NH3

used for making fertilizers

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39
Q

nitrogen compounds

A

NH3
NH4NO3 explosive and fertilizer
NaN3 (sodium azide) used in air bags
NO2 (nitrogen dioxide) in smog, NO(nitric oxide) used in biology for signaling, N2O(nitrous oxide) is an anesthetic
HNO3 (nitric acid) is a strong acid used for making fertilizer, HNO2 (nitrous acid) used in making nitrites, HNO (hyponitrous acid)

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40
Q

how is phosphorus produced?

A

from Ca3(PO4)2 by heating with C and sand

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41
Q

stable form of P

A

P4 (white phosphorus), changes into red phosphorus (chains of liked P4 tetrahedra) when heated in the absence of air

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42
Q

phosphorus compounds

A

PH3 (phosphine) poisonous gas
PCl3 and PCL5 used in synthesis of pesticides, oil additives, flame retardants
H3PO4 (phosphoric acid) used in soft drinks, detergents
superphosphate fertilizer is a mixture of CaSO4 and Ca(H2PO4)2

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43
Q

how is arsenic produced?

A

from As2S3

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44
Q

how is antimony produced?

A

from Sb2S3

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45
Q

As application

A

GaAs lasers for CD players

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46
Q

Bi applications

A

metal with properties similar to PB but nontoxic

pepto-bismol

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47
Q

how is oxygen produced?

A

fractional distillation of liquid air

primarily used in steel manufacturing

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48
Q

ozone

A

O3
important in the stratosphere
produced by photodissociation of O2 (O2–>O+O then O+O2–>O3) serving to remove near UV light from solar radiation

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49
Q

pure form of sulfur

A

S8

monoclinic and rhombic forms

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50
Q

sulfur compounds

A

H2S
SO2,SO3
H2SO3, H2SO4 used in production of fertilizer, petrochemicals, dyes, detergents

51
Q

how is fluorine produced?

A

electrolysis of KF

52
Q

compounds of fluorine

A

SF6
UF6 (used for making nuclear reactor fuel)
HF - the only weak acid of the hydrogen halides, used for etching of electronic components in the electronic industry

53
Q

how is chlorine produced?

A

electrolysis of NaCl

54
Q

compounds of chlorine

A

HCl stomach acid
HClO3 perchloric acid (rocket fuel), HClO3 chloric acid, HClO2 chlorous acid, HClO hypochlorous acid (active ingredient in chlorox)

55
Q

how is bromine produced?

A

from chlorine

2Br- + Cl2 –> Br2 + 2Cl-

56
Q

bromine applications

A

synthetic organic chemistry

for making fire retardants

57
Q

bromine compunds

A

HBr

same acids as with Cl

58
Q

how is iodine produced?

A

from chlorine

2I- + Cl2 –> I2 + 2Cl-

59
Q

iodine applications

A

organic chem
essential for life (thyroid)
acts as switch that initiates transcription of ATPase

60
Q

iodine compounds

A

HI

same acids as with Cl

61
Q

electromotive series

A

the ability of an element to be oxidized in a certain way

62
Q

how are rare gases produced? (except He and Rn)

A

fractional distillation of liquid air

63
Q

how is He produced?

A

natural gas wells in texas

64
Q

how is Rn produced?

A

found in the ground as a result of radioactive processes

65
Q

rare gases applications

A

He - cyrogenics, blimps, He-Ne lasers
Ne,Kr,Xe - lighting
Ar - welding in inert atmospheres

66
Q

colloid

A

particles (1nm to 1 um) suspended in a solvent
the particles are smaller than the wavelength of light, so you cant see them with a microscope and the material appears uniform
brownian motion
particles may be charged, so that electrostatic repulsion keeps them from aggregating

67
Q

brownian motion

A

particles in a colloid are in constant motion, which keeps them from settling out

68
Q

sol colloid

A

solid in gas (smoke), aerosol
liquid in gas (fog), aerosol
solid in liquid (paint)

69
Q

emulsion colloid

A

liquid in liquid (milk, mayonnaise)

70
Q

gel

A

solid in liquid that typically has solid texture (jello)

71
Q

foam

A

gas in liquid

72
Q

solid dispersion

A

solid in solid (stained glass windows)

73
Q

solid emulsion

A

liquid in solid (ice cream)

74
Q

solid foam

A

gas in solid (insulation)

75
Q

why are transition metals in a given row similar in chemical and physical properties

A

either d or f orbitals are filled while there are occupied s orbitals in a valence shall having a higher principal quantum number

76
Q

atomic radii trends for transition metals

A

radii of first row of d block are mostly the same, but there’s a general contraction for the first few (due to increasing nuclear charge), followed by a slight expansion (due to too many electrons)

77
Q

radii of row 1 vs. row 2 transition metals

A

row 2 radii are systematically larger due to increased principal quantum number

78
Q

radii of row 2 vs. row 3 transition metals

A

about the same

79
Q

why are atomic radii of row 2 and row 3 about the same for transition metals?

A

lanthanide contraction

80
Q

lanthanide contraction

A

contraction of the atomic radii going across the lanthanides
happens because:
inner shell of electrons of row 3 transition metals are so close to the nucleus that relativistic effects are important. this makes electrons heavier, so they are located closer to the nucleus
1s electrons travel super fast, and when they travel that fast the electrons act heavier because of relativity

81
Q

oxidation number trends for transition metals

A

most transition metals have multiple oxidation numbers

number of oxidation numbers goes up and down throughout the row

82
Q

ligands

A

atoms or molecules bonded to central metal ion in a complex ion (“the other stuff”)
usually nonmetal
lewis bases (molecules and ions that possess a lone pair of electrons)

83
Q

complex ion

A

polyatomic ion composed of a transition metal to which other atoms or groups (called ligands) are bonded through coordinate covalent bonds
all complex ions are Lewis adducts

84
Q

shapes of coordination complexes

A

depends on how many ligands there are (usually connected to the oxidation number)
depends on hybridization of orbitals in the metal atom
common examples: octahedral, tetrahedral, square planar

85
Q

shape of elements in 3rd row of d block and elements in f block with more than 6 ligands

A

square antiprism structure

dodecahedral structure

86
Q

polydentate ligands

A

ex: ethylene diammine

87
Q

chelate formation

A

bidentate ligand forms a ring with the metal atom as one member

88
Q

stereo isomers

A

arise when atoms are permuted in a complex but all the bonds are the same
possibilities: geometrical isomers and optical isomers

89
Q

geometrical isomers

A

arise when the molecule is superimposable on its mirror image

90
Q

optical isomers

A

compounds that are mirror images

they rotate circular polarized light in opposite directions

91
Q

crystal field theory

A

imagine that ligands are simple point charges located at the vertices of the octahedron (or other shape) that defines the symmetry of the complex
this creates an electric field that interacts with the metal atom, splitting the d-orbitals
splitting creates low lying excited states that determine colors of the complexes
(size of the splitting depends on the ligand)

92
Q

problem with crystal field theory

A

it doesnt describe the actual bonding between the metal d-orbitals and the ligand orbitals
because of this: it cant describe why the CO ligand is a strong field ligand, but Cl- is a weak field ligand

93
Q

ligand field theory

A

MO theory as applied to transition metal complexes, using the valence electrons on the metal and ligands

94
Q

advantages of ligand field theory

A

we can calculate the splittings
results are more realistic than with crystal field theory, showing the difference between a strong field and weak field ligand
allows one to describe more subtle interactions, such as those involving the pi orbitals on the ligands with the metal d orbitals

95
Q

Sc

A

similar chemistry to Al with +3 oxidation #
not useful as a metal because it reacts with water
used as an alloy to strengthen Al

96
Q

Ti

A

+4 oxidation # is dominant in compounds
used in aircraft (lightweight)
TiO2 (rutile) is white paint, also important semicondictor, and as a photocatalyst (splitting water)
BaTiO3 is piezoelectric (distorts shape when charged)

97
Q

V

A

+5 oxidation #
used as an alloy in steel
V2O5 is an oxidant used as a catalyst in H2SO4 production

98
Q

Cr

A

+3,+6 oxidation numbers
red color of ruby in Al2O3
+3 state: essential for life –> required for insulin to work
available in foods and dietary supplements
+6: carcinogenic when airborne
metal used in steel and for plating
CrO2 is ferromagnetic material used in tapes
Na2Cr2O7 is an oxidizing agent

99
Q

Mn

A 
\+2,+4,+7 oxidation numbers
responsible for color of amethyst
used as strengthening alloy in steel
MnO2 is component in standard dry cell batteries
KMnO4 is an oxidizing agent
100
Q

Fe

A

+2,+3 oxidation numbers
5.6% of earth’s crust
in the body, mostly as hemoglobin
used in steel, magnets

101
Q

Co

A

+2,+3 oxidation numbers
in vitamin B12
used in steel
magnets

102
Q

what elements are in magnets

A

Fe, Ni, Co, Al

103
Q

Ni

A

+2,+3 oxidation numbers
alloy in steel
nickels are 75% Cu bc Ni is relatively rare

104
Q

Cu

A

+1,+2 oxidation numbers
0.0007% of earth’s crust
Cu used for oxygen transport in some animals
used in bronze, pennies

105
Q

Zn

A 
\+2 oxidation number
0.007% of earth's crust
present in many enzymes
galvanized metal is zinc coated
used in batteries
106
Q

how steel is made

A

reduction of iron ore (Fe2O3 and FeO) to Fe by CO

CO is produced by burning coke

107
Q

why is limestone added when making steel

A

to convert impurities (silicates, aluminosilicates) into a molten mixture called slag that can be removed

108
Q

pig iron

A

iron made in a blast furnace

it has high carbon content, which makes the iron brittle

109
Q

what manganese does to steel

A

a little: increases strength and hardness, lowers ductility

a lot: increases wear resistance

110
Q

what nickel does to steel

A

a little: increases strength and shock resistance

a lot: increases corrosion resistance and hardness

111
Q

what chromium does to steel

A

a little: increases hardness and wear resistance

a lot: increases corrosion resistance

112
Q

vanadium

A

increases hardness

113
Q

tungsten

A

increases hardness, especially at high temperatures

114
Q

iron in biology

A

hemoglobin, myoglobin (oxygen transport)

115
Q

cobalt in bio

A 
vitamin B12 (pernicious anemia)
this compound contains the only C-Co bond in biology
116
Q

Nickel in bio

A

urease, hydrogenase

117
Q

Copper in bio

A

oxygen transport in octopus (hemocyanin)

118
Q

zinc in bio

A 
carbonic anhydrase (hydrolyze CO2 to make HCO3-)
carboxypeptidase (hydrolyzes peptides in digestion)
alcohol dehydrogenase (converts alcohol to aldehyde)
119
Q

molybdenum in bio

A

nitogenase is a Fe/Mo protein (nitrogen fixation)
this is a part of the nitrogenase compex that also includes reductase (an Fe protein)

The overall reaction in nitrogenase is:
N2 +8e- +16ATP+16H2O→2NH3 +H2 +16ADP+16Pi +8H+
where ATP = adenosine triphosphate, ADP=adenosine diphosphate
Pi = phosphate

120
Q

platinum in biology

A

cis-platin, used in treating cancer

121
Q

C2O4

A

Oxalate

122
Q

gadolinium

A

magnetic resonance contrast agent

123
Q

bidentate ligands

A

Ethylenediamine

oxalate

Chem 171 (2 decks)

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