Title | 2021 CHEM Data Book |
---|---|
Course | Introduction to Chemistry |
Institution | Curtin University |
Pages | 8 |
File Size | 493.9 KB |
File Type | |
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CHEMISTRY ATAR COURSE DATA BOOKLET 2021
2021/1618
Chemistry ATAR Course Data Booklet 2021
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 at 25 0C ..........................................................................................8
Copyright © School Curriculum and Standards Authority, 2021 This document – apart from any third party copyright material contained in it – may be freely copied, or communicated on an intranet, for non-commercial purposes in educational institutions, provided that it is not changed and that the School Curriculum and Standards Authority is acknowledged as the copyright owner, and that the Authority’s moral rights are not infringed. Copying or communication for any other purpose can be done only within the terms of the Copyright Act 1968 or with prior written permission of the School Curriculum and Standards Authority. Copying or communication of any third party copyright material can be done only within the terms of the Copyright Act 1968 or with permission of the copyright owners. Any content in this document that has been derived from the Australian Curriculum may be used under the terms of the Creative Commons Attribution 4.0 International (CC BY) licence. This document is valid for teaching and examining until 31 December 2021.
Published by the School Curriculum and Standards Authority of Western Australia 303 Sevenoaks Street CANNINGTON WA 6107
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Periodic table of the elements
[Data source: The International Union of Pure and Applied Chemistry Periodic Table of the Elements (2018)]
Formulae m M = cV V
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
=
pH of a solution
pH
mass molar mass
mass of solute (mg)
mass of solution (kg) = – log10 [H+]
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 STP 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
Insoluble AgCℓ
Most bromides
AgBr
Most iodides
AgI, PbI2
Slightly soluble PbCℓ2 PbBr2
All nitrates
No exceptions
All ethanoates Most sulfates
CaSO4, Ag2SO4
SrSO4, BaSO4, PbSO4
Insoluble in water Insoluble Most hydroxides
Exceptions
Soluble
Slightly soluble
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
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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+
Colour deep green pink
Cu2+ Fe2+ Fe3+ Mn2+ Ni2+
blue pale green pale brown pale pink green
Anion CrO4 2–
Colour yellow
Cr2O72–
orange
–
purple
MnO4
5
α–amino acids Name
Symbol
alanine
Ala
Structure CH3 H2N
arginine
COOH
Arg
NH
H2N asparagine
CH
CH2
CH2
CH2
CH
COOH
NH
Asn
O CH2 H2N
aspartic acid
Asp
Cys
COOH
CH
COOH
CH2
SH
CH
COOH
Gln
O
H2N glutamic acid
Glu H2N
glycine
Gly
histidine
His
NH2
COOH
CH2
H2N glutamine
C
CH
H2N cysteine
C
CH2
CH2
C
CH
COOH
CH2
CH2
CH
COOH
H2N
CH2
NH2
COOH
COOH N
CH2
N H
H2N isoleucine
CH
COOH
CH3
CH
CH2
H2N
CH
COOH
Ile
6
CH3
NH2
α–amino acids Name
Symbol
leucine
Leu
Structure CH3
CH
CH3
CH2 H2N lysine
Lys
CH2
CH2
CH
COOH
H2N methionine
Met
Pro
serine
Ser
threonine
tryptophan
CH2
S
CH3
COOH CH2
H2N proline
CH2
CH
Phe
COOH CH2
CH2 H2N
phenylalanine
CH
CH
COOH
H N
CH2
Thr
COOH
OH
H2N
CH
COOH
CH3
CH
OH
H2N
CH
COOH
Trp
H N CH2 H2N
tyrosine
Tyr
COOH
CH2 H2N
valine
CH
Val
7
CH
OH COOH
CH3
CH
CH3
H2N
CH
COOH
NH2
Standard Reduction Potentials at 25 °C E°(volts)
Half-reaction F2(g) + 2 e–
2 F–(aq)
+ 2.89
H2O2(aq) + 2 H+(aq) + 2 e–
2 H2O(ℓ)
+ 1.76
2–
(aq) + 4 H+(aq) + 2 e–
PbO2(s) + SO4 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 2– 7
+
–
Cr2O (aq) + 14 H (aq) + 6 e O2(g) + 4 H+(aq) + 4 e– –
Br2(ℓ) + 2 e +
–
3+
–
Ag (aq) + e
Fe (aq) + e +
–
O2(g) + 2 H (aq) + 2 e
–
I2(s) + 2 e
PbSO4(s) + 2 H2O(ℓ) + 1.69 + 1.63 Cℓ2(g) + 2 H2O(ℓ) Mn2+(aq) + 4 H2O(ℓ) + 1.51 Au(s) Cℓ –(aq) + H2O(ℓ) 2+
Pb (aq) + 2 H2O(ℓ) –
2 Cℓ (aq)
+ 1.50 + 1.49 + 1.46 + 1.36
3+
2 Cr (aq) + 7 H2O(ℓ) + 1.36 2 H2O(ℓ) – 2 Br (aq)
+ 1.23
Ag(s) Fe2+(aq)
+ 0.80
H2O2(aq) 2 I–(aq)
+ 0.70
+ 1.08 + 0.77 + 0.54
–
–
4 OH (aq)
+ 0.40
2+
–
Cu(s)
+ 0.34
+
–
H2S(aq)
+ 0.17
+
–
H2(g)
0 exactly
2+
–
Pb(s)
– 0.13
2+
–
Sn(s)
– 0.14
2+
–
Ni(s)
– 0.24
2+
–
Co(s)
O2(g) + 2 H2O(ℓ) + 4 e
Cu (aq) + 2 e
S(s)+ 2 H (aq) + 2 e 2 H (aq) + 2 e Pb (aq) + 2 e
Sn (aq) + 2 e
Ni (aq) + 2 e
Co (aq) + 2 e
– 0.28
–
Pb(s) + SO (aq)
– 0.36
2+
–
Cd(s)
– 0.40
+
–
H2C2O4(aq)
– 0.43
2+
–
Fe(s)
– 0.44
3+
–
Cr(s)
– 0.74
2+
–
Zn(s) H2(g) + 2 OH–(aq)
– 0.76
PbSO4(s) + 2 e
Cd (aq) + 2 e 2 CO2(g) + 2 H (aq) + 2 e
Fe (aq) + 2 e
Cr (aq) + 3 e Zn (aq) + 2 e
–
2 H2O(ℓ) + 2 e
2– 4
– 0.83
2+
–
Mn(s)
– 1.18
3+
–
Aℓ(s)
– 1.68
2+
–
Mg(s)
– 2.36
–
Na(s)
– 2.71
2+
–
Ca(s)
– 2.87
2+
–
Sr(s)
– 2.90
2+
–
Ba(s)
– 2.91
–
K(s)
– 2.94
Mn (aq) + 2 e Aℓ (aq) + 3 e Mg (aq) + 2 e +
Na (aq) + e
Ca (aq) + 2 e
Sr (aq) + 2 e Ba (aq) + 2 e +
K (aq) + e
[Data source: Aylward, G.H., & Findlay, T. (2014). SI Chemical Data (7th ed.). Queensland: John Wiley & Sons Australia, Ltd.]
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