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CHEMISTRY
ATAR COURSE
DATA BOOKLET
2016
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© School Curriculum and Standards Authority, 2016
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This document is valid for teaching and examining until 31 December 2016.
2016/29197
Chemistry ATAR Course Data Booklet 2016
Table of contents
Periodic table of the elements........................................................................................................ 3
Formulae........................................................................................................................................ 4
Units............................................................................................................................................... 4
Constants....................................................................................................................................... 4
Solubility rules for ionic solids in water........................................................................................... 4
Colours of selected substances..................................................................................................... 5
α-amino acids........................................................................................................................... 6 – 7
Standard reduction potentials......................................................................................................... 8
2
Periodic table
[Data source: The International Union of Pure and Applied Chemistry Periodic Table of the Elements (2016)]
3
Formulae
m
=
M
cV
V
mass
molar mass
Number of moles
n
=
Number of moles of solute
n
=
Number of moles of a gas at STP
n
Ideal gas law
PV
= 22.71
= nRT
Parts per million
ppm
= mass of solution (kg)
pH of a solution
pH
+
= - log [H ]
mass of solute (mg)
Units
Volumes are given in the units of litres (L), or millilitres (mL)
Temperatures are given in the units of degrees Celsius (°C) or kelvin (K)
It may be assumed that 0.0 °C = 273.15 K
Energy changes are given in kilojoules (kJ)
Pressures are given in kilopascals (kPa)
Solution concentrations are given in the units moles per litre (mol L-1),
grams per litre (g L-1) or parts per million (ppm)
Constants
Universal gas constant, R = 8.314 J K-1 mol-1
Avogadro constant, N = 6.022×1023 mol-1
Volume of 1.00 mol of an ideal gas at 0.0 °C and 100.0 kPa is 22.71 L
S.T.P. is 0.0 °C and 100.0 kPa
Equilibrium constant for water at 25 °C, Kw = 1.00×10–14
Solubility rules for ionic solids in water
Soluble in water
Exceptions
Soluble
Most chlorides
Most bromides
Most iodides
Slightly soluble
PbCℓ2
PbBr2
Insoluble
AgCℓ
AgBr
AgI, PbI2
All nitrates
No exceptions
All ethanoates
Most sulfates
CaSO4, Ag2SO4
SrSO4, BaSO4, PbSO4
Insoluble in water
Insoluble
Exceptions
Soluble
Slightly soluble
Most hydroxides
NaOH, KOH, Ba(OH)2
NH4OH*, AgOH**
Ca(OH)2, Sr(OH)2
Most carbonates
Na2CO3, K2CO3, (NH4)2CO3
Most phosphates
Na3PO4, K3PO4, (NH4)3PO4
Most sulfides
Na2S, K2S, (NH4)2S
*
** NH3 dissolves in water to form both NH3 (aq) and NH4+(aq)/OH–(aq)
Ag+(aq) reacts with OH–(aq) to form insoluble Ag2O
Soluble = more than 0.1 mole dissolves per litre
Slightly soluble = between 0.01 and 0.1 mole dissolves per litre
Insoluble = less than 0.01 mole dissolves per litre
4
Colours of selected substances
In general, ionic solids have the same colour as that of any coloured ion they contain. Two colourless ions
in general produce a white solid. Selected exceptions to these two basic rules are noted below.
Ionic Solid
copper(II) carbonate
copper(II) chloride
copper(II) oxide
copper(II) sulfide
lead(II) iodide
lead(II) sulfide
manganese(IV) oxide
silver carbonate
silver iodide
silver oxide
silver sulfide
Colour
green
green
black
black
yellow
grey
black
yellow
pale yellow
brown
black
Other coloured substances
Most gases and liquids are colourless, and most metals are silvery or grey. Selected exceptions to these
basic rules are noted below.
Substance
copper(s)
gold(s)
nitrogen dioxide(g)
sulfur(s)
Colour
salmon pink
yellow
brown
yellow
Coloured halogens
Halogen
F2(g)
Cℓ2(g)
Br2(ℓ)
I2(g)
Colour of free element
yellow
greenish-yellow
red
purple
Halogen
Cℓ2(aq)
Br2(aq)
I2(aq)
Colour of halogen in aqueous solution
pale yellow
orange
brown
Halogen
Br2
Colour of halogen in organic solvent
red
I2
purple
Coloured ions in aqueous solution
Cation
Cr3+
Co2+
Cu2+
Fe2+
Fe3+
Mn2+
Ni2+
Colour
deep green
pink
blue
pale green
pale brown
pale pink
green
Anion
CrO42–
Colour
yellow
Cr2O72–
MnO4–
orange
purple
5
α–amino acids
Name
Symbol
alanine
Ala
Structure
CH3
H 2N
arginine
COOH
Arg
NH
H 2N
asparagine
CH
CH2
CH2
CH
COOH
CH2
NH
Asn
O
CH2
H 2N
aspartic acid
Asp
Cys
COOH
CH
COOH
CH2
SH
CH
COOH
Gln
O
CH2
H2 N
glutamic acid
H 2N
Gly
histidine
His
CH2
CH
Glu
glycine
NH2
COOH
CH2
H 2N
glutamine
C
CH
H2N
cysteine
C
CH2
CH2
CH
COOH
H 2N
NH2
COOH
CH2
COOH
COOH
N
CH2
H 2N
isoleucine
C
Ile
CH
N
H
COOH
CH3
CH
CH2
H2N
CH
COOH
6
CH3
NH2
α–amino acids
Name
Symbol
leucine
Leu
Structure
CH3
CH
CH3
CH2
H 2N
lysine
Lys
H2N
methionine
CH2
CH2
CH
COOH
Met
H2N
phenylalanine
CH
CH2
CH
COOH
serine
Ser
threonine
tryptophan
CH2
S
CH3
CH2
H2N
Pro
CH2
CH2
Phe
proline
COOH
CH
H
N
CH2
Thr
COOH
COOH
OH
H2N
CH
COOH
CH3
CH
OH
H 2N
CH
COOH
H
N
Trp
CH2
H 2N
tyrosine
Tyr
COOH
CH2
H2 N
valine
CH
Val
7
CH
OH
COOH
CH3
CH
CH3
H 2N
CH
COOH
NH2
Standard Reduction Potentials at 25 °C
Half-reaction
F2(g) + 2 e
H2O2(aq) + 2 H (aq) + 2 e
+
PbO2(s) + SO4 (aq) + 4 H (aq) + 2 e
2–
+
2 F (aq)
+ 2.89
–
2 H2O(ℓ)
+ 1.76
–
2 HCℓO(aq) + 2 H+(aq) + 2 e–
MnO4–(aq) + 8 H+(aq) + 5 e–
Au3+(aq) + 3 e–
HCℓO(aq) + H (aq) + 2 e
–
PbO2(s) + 4 H (aq) + 2 e
–
+
+
Cℓ2(g) + 2 e
Cr2O7 (aq) + 14 H (aq) + 6 e
2–
+
O2(g) + 4 H (aq) + 4 e
+
E°(volts)
–
–
PbSO4(s) + 2 H2O(ℓ) + 1.69
Cℓ2(g) + 2 H2O(ℓ)
+ 1.63
Mn2+(aq) + 4 H2O(ℓ) + 1.51
Au(s)
+ 1.50
Cℓ (aq) + H2O(ℓ)
+ 1.49
–
Pb (aq) + 2 H2O(ℓ)
2+
+ 1.46
–
2 Cℓ (aq)
–
2 Cr (aq) + 7 H2O(ℓ) + 1.36
–
+ 1.36
–
3+
2 H2O(ℓ)
+ 1.23
–
–
2 Br (aq)
+ 1.08
Ag (aq) + e
–
Ag(s)
+ 0.80
Fe (aq) + e
–
Fe (aq)
+ 0.77
O2(g) + 2 H (aq) + 2 e
–
H2O2(aq)
+ 0.70
Br2(ℓ) + 2 e
+
3+
+
I2(s) + 2 e
2+
2 I (aq)
+ 0.54
–
4 OH (aq)
+ 0.40
Cu (aq) + 2 e
–
Cu(s)
+ 0.34
S(s)+ 2 H (aq) + 2 e
–
+ 0.17
2 H (aq) + 2 e
H2S(aq)
–
Pb (aq) + 2 e
–
Pb(s)
– 0.13
Sn (aq) + 2 e
–
Sn(s)
– 0.14
Ni (aq) + 2 e
–
Ni(s)
– 0.24
Co (aq) + 2 e
–
Co(s)
–
O2(g) + 2 H2O(ℓ) + 4 e
2+
+
+
2+
2+
2+
2+
PbSO4(s) + 2 e
–
–
–
H2(g)
0 exactly
– 0.28
Pb(s) + SO4 (aq)
2–
– 0.36
Cd (aq) + 2 e
–
Cd(s)
– 0.40
2 CO2(g) + 2 H (aq) + 2 e
–
– 0.43
Fe2+(aq) + 2 e–
H2C2O4(aq)
Fe(s)
– 0.44
Cr (aq) + 3 e
–
Cr(s)
– 0.74
Zn (aq) + 2 e
–
Zn(s)
2+
+
3+
2+
2 H2O(ℓ) + 2 e
–
Mn 2+(aq) + 2 e–
– 0.76
H2(g) + 2 OH (aq)
–
– 0.83
Mn(s)
– 1.18
Aℓ (aq) + 3 e
–
Aℓ(s)
– 1.68
Mg (aq) + 2 e
–
Mg(s)
– 2.36
Na (aq) + e
–
Na(s)
– 2.71
Ca2+(aq) + 2 e–
Ca(s)
– 2.87
Sr (aq) + 2 e
–
Sr(s)
– 2.90
Ba (aq) + 2 e
–
Ba(s)
– 2.91
K (aq) + e
–
K(s)
– 2.94
3+
2+
+
2+
2+
+
[Data source: Aylward, G.H., & Findlay, T. (2008). SI Chemical Data (6th ed.). Queensland: John Wiley & Sons Australia, Ltd.]
8