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ISBN 978 156 198 X
NWADINIGWE, C A
Author 2
Author 3
Title
Inorganic Chemistry: A Guide to IUPAC
Nomenclature (for Schools and Colleges)
Keywords
Description
Inorganic Chemistry: A Guide to IUPAC
Nomenclature (for Schools and Colleges)
Category
Physical Sciences
Publisher
Fourth Dimension Publishers
Publication Date
Signature
1985
INORGANIC CHEMISTRY:
A GUIDE TO IUPAC
NOMENCLATURE
(FOR SCHOOLS
AND COLLEGES)
INORGANIC CHEMISTRY:
A GUIDE TO IUPAC
NOMENCLATURE
(FOR SCHOOLS AND COLLEGES)
INORGANIC CHEMISTRY:
A GUIDE TO IUPAC
NOMENCLATURE
(FOR SCHOOLS AND COLLEGES)
by
C. A. NWADINIGWE
F[3P
FDURTH OIMENS(0N WELISHEAS
First Publsihed 1985 by
Fourth Dimension Publishing Co., Ltd.
64A City Layout,
P.M.B.1164
Enugu, Nigeria
0 1985 by C.A. Nwadinigwe
ISBN 978 156 198 X
CONDITIONS
All rights resenred. No parts of this publication may be reproduced, stored in a
retrieval system, or transmitted in any form or any means, electronic, mechanical,
photocopying, recording, or otherwise without the prior permission of the Publisher.
Photoset and printed in Taiwan, R.O.C.
by At-UNITED INDUSTRIES & SHIPPING INC.
10th FI., Cheng Chung Great Building
No. 12-1, Lane 5, Lin Shen North Road Taipei, Taiwan
CONTENTS
1 NAMES AND SYMBOLS OF THE ELEMENTS .........
2 INDICATlON OF MASS. CHARGE. ETC., ON
A'TOMIC SYMBOLS ...............................................
3 THE USE OF ARABIC NUMBERS. ROMAN
NUMERALS. AND GREEK I'REFIXES ....................
4 OXIDATION NUMBER CONCEPT ..........................
5 NOMENCLATURE WlTH RESPECI' TO IONS .........
(i) cations
................................
(ii) anions ............................................................
.......................
.
6 NOMENCLATURE WITH RESPECT TO ACIDS .......
(i) two element acids .....,.. .................................
................... ................................
.............. ...................................
7 NOMENCLATURE WITH RESPECT TO BASES .......
(i) amphoteric oxides ...........................................
(ii) basic oxides
(iii) hydroxides .....................................................
....................................................
WITH RESPECT TO SALTS .......
(i) simple (anhydrous) Qlts ...................................
(ii) acidic salts .....................................................
( i i i ) basic salts ......................................................
(iv) salts with water of crystallkation ........................
8 NOMENCLATURE
9 DOUBLE SALTS. GUIDELINES FOR FORMULAE
AND NOMENCLATURE
........................
............
..
10 THE HALIDES
OF CARBON. C X , ..........................
1 1 FREE RADICALS
................................................
12 FORMULAE AND NAMES OF COMPOUNDS IN
GENERAL
29
13 FORMULAE AND NAMES OF SOME COMMON
COMPOUNDS ................................. ..................
31
.............................................................
...
APPENDIXES
1. The periodic table of elements
.................................
2 . Oxidation states of elements in the periodic table
..........
3 . Table of elements. symbols. atomic number and relative
atomic masses .......................................................
................................................
5 . Glossary ...............................................................
4 . Answers to questions
37
38
39
42
43
PREFACE
Thc abbreviation IUPAC stands for the International Union of
Pure rind Applied Chemistry, a body charged with the difficult task o f
pronwtmg understanding among chemists all over the world. The
Union has many Commissions under it, each Commission working on
different topics in Chemistry. The Commission on the Nomenclature
of Inorganic Chemistry of the IUPAC was formed in 1921. It drafted
a ~t of rules which was published in 1940. This "1940 Rules" have
been revised and rewritten severally in keeping with the Commission's aim of producing rules which lead to clear and acceptable
names for as many inorganic compounds as possible.
There are two essential requirements for the name of any chemical
compound:
(i)
(ii)
~~
I
I
1
it must be understood by other chemists, and
it must designate the compound unambigously.
To achieve these ends, it is desirable that all chemists should use the
same rules of nomenclature.
ThisA~bookhas become quite necessary as a result of the shift of
emphas~sby the major examining body in West Africa, the West
African Examinations Council, .from the traditional nomenclature to
the IUPAC system. In the absence of any readily available reference
b w k s on the subject, schools, colleges, and private candidates sitting
for ordinary and advanced level examinations in chemistry have had
teething problems adjusting to the new system. Most textbooks in
inorganic chemistry are yet t o be revised to reflectathe new system of
nomenclature.
In the presentation, guidelines for naming the various types of ions
and compounds encountered in 0-and A- level inorganic chemistry
are given, in the hope that such guidelines will enable the user to
name any compound not specifically mentioned in the book. Chemistry teachers will find this approach quite useful. T h e book will also
satisfy the needs of Laboratory Chemical Suppliers, enabling them to
use IUPAC names o n their labels and in their catalogues. University
undergraduate students and other students in institutions of higher
I
learning who take first year inorganic chemistry courses will find the
book a useful companion.
I have consulted introduction to Chemical Nomenclature by R. S.
Cahn and 0.
C. Dermer, fifth edition, Butterworths, London 197'1;
f U P A C Reports, J . Amer. Chem. Soc., 82, 5523 (1960); IUPAC,
Nowrenclature of Inorganic Chemistry, second edition, Definitive
~ h e 1970,
s
Butterworths, London, and I am much indebted to them.
The author wishes to thank Drs. A. Ahmed and F. Nwabue and
Mrs. A . 0. Nwadinigwe, B.Sc., P.G.D,E., who read the work in
typescript and
advised 01
NAMES AND SYMBOLS OF ELEMENTS
There are about 105 known elements. Their names and symbols
form the basis of chemical names and formulae. The periodic table of
clznlcnts found in many chemistry books is also constructed with
these symbols. Such a table is given here in Appedix 1. The
International Union of Pure and Applied Chemistry [TUPAC) has
adopted the names and symbols given in Appendices 1and 3 for these
elements, except for the last two. These two elements, with atomic
numbers 104 and 105, were quite recently dihiovered and so official
names or symbols have not yet been adopted for them. The following
group names should be. noted in the periodic table:
(i) all the group I elements are collectively called the ALKALI
metals,
(ii) all the group V11 clc~~rcntsurc collcctivcly cullcd tile
HALOGENS, and
(iii) all the group 0 elements are collectively called the NOBLE
GASES.
Isaddition, the lUPAC recommends that any new metallic
olcnwnts discovered should be given names ending in -ium. This will
then be consistent with the names of most of the already known
nletals. Examples: aluminium, barium, beryllium, calcium, chromium, lithium, magnesiutn, etc. It also recommends that all new
dements shall have two-letter symbols (like Al, Ba, Be, Ca, etc.) and
that all the isotopes of an element should have the same name but
differentiatedby the mass numbers. Example, the isotopes of oxygen
are named oxygen-16,-oxygen-17, and oxygen-18.
INDICATION OF MAS!!, CHARGE, ETC., ETC.,
ON ATOMIC SYMBOLS
The symbol of an element, when fully and correctly written,
provides the following information about the element:
(i) its isotopic mass number (defined as the sum of the protons and
neutrons in the atomic nucleus),
(ii) its atomic number (defined as the number of protons in the
atomic nucleus or the number of electrons in an electrically
neutral atom),
(iii) the charge on the ion, and
(iv) the number of atoms of thc GICIIICIIL.
T o convey these information, the notation recommended for
writing the symbol of an element X, is:
where the left upper index, a, represents the mass number, the left
lower index, c, represents the atomic number, the right lower index,
d, represents the number of atoms, and the right upper index, b,
represents the ionic charge.
illustrative examples:
:tie
represents an atom of helium of mass number = 4 and
atomic number = 2. It must be noted that in the representawhile d (the
tion :He, b(the ionic charge) is assumed to be 0,
number of atoms) is assumed to be 1. In general, when no
charge is given for b, it is assumed to be 0 charge (neutral)
while in the case of d, if no number is given it is assumed to
be 1.
0
represents a molecule of trioxygen (trivial name = ozone)
containing 3 atoms, each of which has the atomic number = 8 and mass number P: 16. There is no ionic charge,
i.e. the molecule is neutral.
represents a molecule of oxygen (made up of 2 atoms). The
isotopic mass number = 18 while the atomic number = 8.
reprcscnts a molecule of chlorine (made up of 2 atoms). Thc
isotopic mass number = 35 while the atomic numbcr = 17.
represents one atom of sodium whose atomic number = 11
and the ionic charge = + 1.
represents an isotope of sulphur atom. The mass numher = 34, the atomic number = 16, and the io~iiccharge =
'lie following points should be noted.
Ionic charge should be indicated as Xn+and not as X+"
Examples:
~ a ~ not
+ ,~
a
+
~
02-,not 0-'
When a compound is isotopically labelled, the symbol of the
isotope in parenthesis is added to the name of the compound.
Examples:
3 2 ~ is~ phosphorus
~ 3
( 3 2 ~ ) trichloride
H ~ CisI hydrogen chloride ("Cl)
" N H ~is ammonia (I5N).
For allotropes, the systematic names are based on the size
~nolccule.The size is indicated by Greek numerical prelixes.
When the number of atoms is large and unknown. the prefix
"poly" is used. For ring and chain structures prefixes "cyclo"
and "catena" respectivcly are used.
Symbol
H
Trivial name
atomic hydrogen
Systematic name
monohydrogen
0 2
dioxygen
triox ygen
S8
oxygen
o-zone
white phosphorus
(yellow phosphorus)
A-sulphur
s,,
p-sulphur
0 3
p4
tetraphosphorus
cy clooctasulphur or
octasulphur
catenapolysulphur or
polysulphur
Questiurts:
.
:s2-
Explain the difference between lMOzand 02,
and ::S, ?$I
and ::cI,,;ECa and :dCa2+, f H and :H,.
2. If a potassium nuclide has atomic number = 19, mass number = 39 and ionic charge = 1+, represent this atom sy~nbdicully.
1.
THE USE OF ARABIC NUMBERS, ROMAN NUMERALS,
AND GREEK PREFIXES
numeral
Roman numeral
equivalent
I
I1
I11
IV
v
VI
VII
VIl I
IX
X
XI
XI1
Greek numerical
prefix equivalent
mono
di
t rib
tetra
penta
hexa
hepta
octa
nona
deca
undeca
dodeca
The prefix "mono" may generally be omitted. Beyond 12, Greek
p r e f i s s are sometimes replaced by Arabic uumcrals because they
are more readily understood. The Arabic numbers are used when
writing molecular formulae:
to indicate the number of atoms of a particular elemcnt prcscnt
in a molecule. E.g. H 2 0 . Here 2 shows that there are 2
hydrogen atoms in a molccule of water. Similarly ill SO,,
H2S03, and PbSO,, the numbers 2, 3, and 4 show there are
respectively 2, 3, and 4 oxygen atoms in a molecule of SO,,
H z S 0 3 , and PbSO,.
(ii) tb indicate the number of moles of i~ compound. Examples:
2H20, 3S02, 4H2S0.3and 5PbS04 suggest 2, 3,4 and 5 moles
respectively of HzO, SO2, I-12S03 and PbSOJ.
(iii) to indicate the number of times a group which is cnclosrtl
in parenthesis occurs. Examplc: (NI-l,)2S04, Pb(N03)-,,
Fe2(S0,), indicate that the groups N H 4 , NO3, and SO4, occur
2, 2, and 3 timcs respectively in a n~oleculeof (NH4j2SO4,
Pb(N03)?, and Fe2(S04)3.
(iv) to indicate the number of watcr of crystallization and similar
loosely bound muleculcs.
(i)
Exumples:
in
in
in
in
CuS04.5H20,
IIuIIIVLL
w(llL1of crystallization is 5
FeS04 .7H,O,
the number of water of crystallization is 7
MgS0,.7H20,
the number of water of crystallization is 7
Na2C03. 1 0 H 2 0 , the number of water of crystallization is 10
LIIL
The Roman figure is very often used to indicate the oxidation state
oI the key atom in a molecule or.ion especially if that key atom can
have variable oxidation states.
Examples:
FeCI, = iron
FeC13 = iron
FeO = iron
Fe203= iron
(11) chloride
(111) chloride
(11) oxide
(111) oxide
N 2 0 = nitrogen (I) oxide
N O = nitrogen (11) oxide
NO2 = nitrogen (IV) oxide
NO3 = nitrogen (VI) oxide
O n the other hand, the Greek prefix can be encountered in a
number of situation, including:
(i) indicating the number of ligands in parenthesis.
e.g. K4Fe (CN), = potassium hcxacyanoferrate (11)
(ii) indicating the number of oxygen atoms in an anion:
e.g. SO:- = tetraoxosulphate (Vl) ion
SO$- = trioxosulphak (IV) ion
(iii) indicating the number of water of crystallization
e.g. FeS0,.7Hz0 = Iron (11) tetraoxosulphate (VI) heptuhydrate.
THE OXIDATION NUMbER CONCEPT
rile IUPAC nomenclature makes immense use of the crxidation
number of atoms in a molecule. The oxidation number should be
specified for:
,
-- -tals and non-metals that can have variable oxidation states
rnples: CuzO = copper (I) oxide. Here (I) refers to the
3ation number of the copper atom. C O = carbon (11) oxide.
: (11) refers t o the oxidation number of carbon.
key o r central atom in the anion of a salt if that anion
- - ~ a i n smore than one element, e.g. SO:-, tetraoxosulphate
(VI) ion, here (VI) refers to the oxidation state of the sulphur
.om.
le key atom in the anion of an acid if that anion contains more
Ian one element.
\
It is, therefore, quite useful to be able to determine the oxidation
number of any atom in a molecule. We can introduce the concept of
oxidation number by considering these three reactions:
br
(i) Na (s) + 3Fz (s) ---, NaF (s)
(ii) 3Fz (g) + 4F&)
---* F2 (d
(iii) iH2 (d + -9Ch (g)
HCl (g)
ftcaction (i) can be represented as:
-
nuclcuh
(I!!', l 2 N )
nucleus
( W . ION)
':F
nuclcus
(Ill'. 12N)
+
~~uclcu~
(sf', ION)
I I N a ( 1 0 electrons) ,F-(10 electrons)
In the above illustration, the sodium atom is oxidised (by complete
transfer of one electron, the valence electron) to become the sodium
ion. T h e sodium ion has one positive charge (since it now has 10
electrons and 11 protons). Consequently, sodium is said to have an
oxidation number of +l. The fluorine atom which accepts the one
dectron from sodium to complete its octet now has a net -1 charge,
with 9 protons against 10 electrons. Consequently fluorine atom has a
- 1 oxidation number. In t h ~ example,
s
there is a complete transfer of
electron from one atom t o the other because the fluorine atom has a
much greater affinity, a much greater propensity for electrons. O r , t o
use the chemist's language, the fluorine atom is muchlmore electronegative than the d i u m atom.
In the second reaction, i,e. (ii), the two fluorine atoms are of equal
electronegativity and so an electron cannot be transferred from w e
atom to the other. The resulting fluorine molecule is formed by
sharing two electrons equally between the two atoms, resulting in a
nonpolar covalent bond:,
nucleus
(YP, 10N)
nucleus
(W.
IUN)
Using the electron-dot notation this can be represented as:
'Therefore, in the fluorine molecule one can still picture each atorrl
as consisting of 9 positive charges and 9 negative charges (9 protons
and 9 electrons), giving a net zero charge. T h e oxidation number of
Huorine in F2 is then equal to 0.The same deduction holds for any
free element such as hydrogen in Hz,chlorine in C12, sodium in Na,
oxygen in 02,sulphur in S,, phosphorus in P4,etc.
.
In the third reaction, i.e. reaction (iii), because c h l o r i r is only
slightly more electronegative than hydrogen it does not involve a
complete transfer of electrons from hydrogen to chlorine and it does
not involve an equal sharing of electrons as in (ii). The electrons are
regarded as displaced towards the more electroneyative chlorine
atom, giving rise to a partial covalent bond.
':cl
t ICI
r the purpose of oxidation number calculations, the
ulsplactru c l c ~ ~ l o are
ns
counted with the more electronegative atom.
I n this case the chlorinc atom will appear to have a -1 charge and the
hydrogen atom will appear to have a +1 charge. Thii gives the
oxidation number of hydrogen and chlorine in HCI as +1 and -1
respectively. The deductions are also general for other partial
covalent bonds, namely: the displaced electrons are counted with the
more electronqptive atom.
ridation number then refers to the charge which an atom in
a ~olecu& would hove if the bonding electrons were a s s i p w i arbitrarily lu the more electronegative element.
Rules for w i p i n g oxidation numbers
In principle, electronic ,pictures a s illustrated in (i), (ii) and (iii)
above can be drawn for any molecule and the bonding electrons
assigned arbitrarily to the more electronegative element. However,
deciding oxidation numbers by this approach is quite laborious. In
practice, oxidation numbers are ordinarily obtained in a much easier
way by applying the following operational rules:
1. For free elements, each atom has an oxidation'number of 0,no
matter how complicated the molecule is. Example, fluorine in F2,
iodine in I,, hydrogen in Hz,phosphorus in P,, sulphur in Ss,
sodium in Na, all have oxidation numbers = 0.
2. In ions which contain one atom (monoatomic ions), the oxidation number of the element is equal to the charge on that ion.
+ , CI-, s2-,02-,the oxidation
Example, in ~ e ~~ +e ,~ K+,
numbers of iron, potassium, chlorine, sulphur and oxygen are the
charges on the respective ions, i.e. +2, +3, +1, -1, -2. -2
respectively. Consequently, in the ionic corlrpound NaCI, the
oxidation number of sodium = 1 and the oxidation number of
+
chlorine = - 1.
I t is helpful t o remember that the group I elements of the
periodic table (Appendix 1) from only +1 ions. Their oxidation
number is + 1 in all compounds. The group I1 elements form only
+2 ions and so always have + 2 oxidation numbers in all
compounds.
3. In most compounds containing oxygen, the oxidation number of
the oxygen atom is -2. Example, in H 2 0 , SO2, CaO, etc, the
oxidation number of the oxygen atom is -2. The only exception
to this rule is inperoxides where the oxygen atoms have oxidatio'n
number = -1. i.e., in H 2 0 2 , Na20z and other peroxides, the
oxidation number of the oxygen atom = -1.
4. Hydrogen in its compounds ordinarily has an oxidation number
of + l . Example: in H 2 0 , H2S, HF, H2SO4, etc, the oxidation
nuniber of the hydrogen atom is + l .
The only exception here is in metul hydrides (where hydrogen
is the more electronegative atom). In metal hydrides, tne oxidation number of the hydrogen atom is - 1. i.e., in NaH, CaH2,
ctc, the hydrogen atom has a -1 oxidation number.
5. All oxidation numbers must be consistent with the conservation
of charge. This means that for:
(a) neutral molecules (i.e., molecules without any charges), the
oxidation numbers of all the atoms must add up to zero.
(b) ions which contain more than one atom, the oxidation
number of all the atoms niust be equal to the charge on the
ion. The application of these rules is
illustrated in the examples below:
What is the oxidation number of sulphur in &SO4?
Solution:
+
For H2S0,, knowing that the oxidation number of hydrogen is i
(rule 4), that of oxygen is -2 (rule 3) and that the molecule is neutral,
implying that the sum of all the oxidation numbers must be O (rulc
5a), we have:
IizS04
i.e.
-
2 (-1- 1)
+2
+ [oxid. .no. of
+ [oxid
S ] t J( -2) = O
=O
=+X-2
no. of SJ - X
oxid. no. of S
=
+6
mine the oxidation number of Mn in KMnO,
..,
XMn04, knowing that the oxidation number of potassium =. + I (rule 2), the oxidation number of oxygen = -2 (rule 3),
and that the molecule is neutral, implying that the sum of all the
oxidation numbers must = 0 (rule 5a) we have:
KMnO, = +1
+I
+ [oxid. no. of Mn] + 4(-2)
+ [oxid. no. of Mn] - 8
oxid. no. of Mn
=O
0
=+8= +7
=:
1
Calculate the oxidation number of nitrogen in NO;.
For N O i , knowing that the oxidation number of oxygen = -2
(rule 3), and that the net charge on the ion is -1, implying that the
sum of all the oxidation numbers nlust = - I (rule 5b), we haw..
NO; = [oxid. no. of N]
i.e.
or
+ 3(-2)
[oxid. no. of N] -6
oxid. no. of N
=
=
-1
-1
=-1+6
= +5
Show that the oxidation number of chromium in K,Cr,O,
is 1-6.
For K1Cr2O7. knowing that the oxidation number of poti~ssiu~n
is t 1 (rule 2). that of oxygcu is -2 (rule 3) and that t l ~ cmolcoulc is
ncutrai, i x . , the sum of all the oxidation nunlbers equals 0 (rule 5a).
we have:
K,Cr,O,
i.e
or
=
2(+1)
+2
+ [oxirk
+ [oxid.
no. of ZCr]
no. of ZCr]
oxid. no: of 2Cr
+ 7(-2)
=
O
14
=
O
=
=
+14 - 2
+12
+6
-
from which oxid. no. of Cr =
Questions:
3. Calculate the oxidation number of sulphur in the ion and
compounds below:
(i) so3
(ii) SO:-'
(iii) Na2S203
4.
What is the oxidation number of:
(a) chlorine in each of the following compounds: NaCI,
NaCIO, NaCI0.3, NaCI03?
(b) manganese in each of the following compounds: Nu,MnO,,
M n 0 2 , NaMn04 , Mn,O,, Mn207?
chromium
in the ions CrO;, Cr20;', 00:-,IiCrO, ,
(c)
C ~ O H? ~ +
5. Give the oxidation number of each aton1 in:
(a) As2U3 (b) C a C 2 0 4 (c) PFS (d) NO;
( e ) C r 2 0 ; - (f} 0;
6 . State the oxidation number
(a) Pb in P ~ C I ~ (c) Re in ReO;
( e ) Bi in BiOi(g) M o in (~o,Cl,)''
of:
(b) Sn in Sn2F;
(d) Xe in HXeO;
( f ) N in (NH,OH)+
(h)
in (H~W1204u)6-
7. Calculate the change in oxidation number of the underlined
atoms in the reactants and products of the following equations:
(i) 2K2-Cr,O, (s) + 2 H 2 0 + 3s (s)
3 S o 2 (g) + 4KOH (s) + 2Cr-20,
2KCl (s) + 30.-2 (g)
(ii) 2KClO-, (s)
-
+
8. Consider the q u a t i o n :
2Mn0, (aq)
+ 10 Cl-
(aq)
+ 16H'
-
(aq)
2Mn2+ (aq) + 5Ci2 (g)
+ 3H20
Find the oxidation number of each clement on both sidcs of the
a,...-t.n-
charged species. Two main types are known: cations and
anlorn.
(i)
Cations:
&tions are ions that carry positive charges. In inorganic nornenclaturc the two common types are cations with variable oxidation
numbers and those with fixed oxidation numbers. In earlier nomenclatures, variublc oxidation states were clislinguished by means of
suffixes, -ous and -ic, added to the root of the name of the cation. e.g.
plumbous ....... plumbic
cupprous ....... cuppric
ferrous ....... ferric
The IUPAC recommends that the use of this type of no~~icnclature
may be' retained only for elements exhibiting not more than two
valences. A more favoured no~ncnclatureis that the ionic symbols of
nlonoatonlic cations are named like the correspondirig element,
with%t change or suffix, while thosc with variablo oxidation states
are named by Srock's sysrcrn, that is, they have the appropriate
oxidation numbers written in Ron~iinnun~crals,c~icloscdin parcnthesis, and placed immediately after the nnn'e of the catio~i.
(a) Fixed oxidation state:
Li
lithium ion
Na+ sodium ion
MgZ+ magnesium ion
Ca2' calcium ion
NHZ ammonium
+
(b)
Variable oxidation states:
Fez+ iron (11) ion
Fe"
iron (111) ion
Cu+
copper (I) ion
Cu2+ copper (11) ion
PbC12 lead (11) chloride
Polyutornic cutions:
When a polyatomic cation is formecI trom a monoatomic cation by
the addition of other ions o r neutral atoms or molecules (ligancis),
that polyatomic cation will be regarded as a complex and will be
named according.to the rules'of coordination nomenclature.
'
[A1 (H~o),]'' = the h e m aquoalurninium (111) ion
[CoCI (NN,)~]~
=
the chloropent;~mminecobalt (Ill) ion
Cations from nitrogen buses
The cation formed by adding a proton to ammonia rtrtai~isthe
fan~iliarname ammonium ion. Substituted ammonium ions have
urnmonium as suffixes.
Examples:
NH,)
ammonium ion
HO-i~
hydroxylammoniurn
,
ion
(CH,),NH
(11)
trimethylammonium ion
FROM OTI-IER NITROGEN BASES:
Cations from other nitrogen bases (e.g. pyridine , hydrazine,
aniline) h a i e the ending "-ium" added to the name of the base (if
necessary omitting a final -e o r other vovel in the name of the base).
Examples:
base
Cation
(pyridine)
H+
H2N-NH,
+
(hydrazine) H2N-NH3
C,H,NH,
(aniline)
C,H$H
(pyridinium ion)
(hydrazinium ion)
(anilinium ion)
If a base can give more than one cation, thc appropriate charge is
indicated in the names E.g.
hydrazine
hydrazinium (1 +) ion
hydrazinium ( 2 + ) ion
rr3v 15 a monohydrated proton and the recommended IUPAC
name is oxo~liumion. Derivatives of this parent ion has "oxunium"
occurring in their names.
CH30ki:
methyloxonium ion
(CH,),OH+ dimethyloxoniurn ion
H 3 0 'CIO; oxonium perchlorate
Curions from acids:
When cations are formed by adding protons to acids, their names
are formed by adding the word "acidium" the name of the corresponding anion.
r)
Exurrrplrs:
H2N0,'
H2N0;
CH,COOH+
(ii)
=
=
=
the nitrate acidium ion
the nitrite acidium ion
the acetate acidium ion
Anions:
These arc atoms o r groups of atoms which are negatively
The following guidelines are useful in naming anions:
(a) In general, the names of monatomic anions end in "-ide."
Thus,
HDFC1-
= hydride ion
deuteride ion
= fluroide ion
= chloride ion
Br- = bromide ion
I - = iodide ion
0'- = oxide ion
s'- = sulphide ion
=
= selenide ion
= telluride ion
=
=
=
=
=
=
nitride ion
phosphide ion
arsenide ion
antinionide ion
carbide ion
boride ion
(b)
The names of polyajomic anions consist of the name of the
central atom with the ending "-are".
E.g.,
NO,
[lSb(OH),] (c)
= trioxonitrate (v) ion
=
hexahydroxoantimoncrrp (v) ion
A few polyatomic anions have names ending in "-idc". These
are to be regarded as exceptions to the rule. E.g.
OH - = hydroxide ion
0;peroxide ion
02
hyperoxideion
0,
ozonide ion
S: disulphide ion
1;
triiodidt: ion
HF;
hydrogen
difluor~deion.
(d)
NNH*~
NH;
NHOHN21-Ii
CN-
c;-
azide ion
imide ion
amide ion
hydroxylamide ion
hydrazide ion
cyanidc ion
acetylide ion
Some anions have their names ending in thc letter "o". This
obtains when such anions occur in complex compounds o r when
they are used in combination with other anions in the same
molecule. Under these situations we have,. for example:
02 -
--
OX0
OH-- = hydroxo
CN- = cyano
(e)
The 0 x 0 crniotu: Some anions such as NO3, SO:-. YO:,etc,
retain the tamiliar endings nitrate, sulphate, and phosphate
respectively. However, the oxidation number of the central
atom is specified in Roman nunwrals and the number of oxygen
atoms (0x0 atoms) present indicated by Greek prefixes. The
following examples are illustrative of this new system:
-
= ctioxonitrute (HI) ion
trioxonitrate (V) ion
= trioxosulphate (1V) ion
= tetraoxosulphate (VI) ion
(VI) ion
= tetraoxophosphate (V) ion
= trioxocarbunate (IV) ion
= tetraoxophospliatc
-
= heptaoxodichromate ( V l ) ion
rnonoxochlorate ( I ) ion
rioxochlorate (V) ion
etraoxomanganate (VII) ion
lydrogen tetraoxosulphate (VI) ion
~ydrogentrioxocarbonate (IV) ion
trioxosulphursulpharc ( V I ) ion
(one of [he sulphur arollls I S a ligilnd)
iroxoperoxodisulpha~c(V1) ion
:term pcroxo is uwd for -0-0-Imkayc)
ACIDS
NOMENCLATURE WITH RESPECT TO ACIDS
Arrhenius (1887) defined an acid as e substance that can increase
the concentration of H+ (actually H30+)
ion in aqueous solution.
E.g.9
HCl + H20 ---, H,O+ + C1Bronsted-Lowry defined an acid as a substance that can donate a
proto11 to some other substances.
E-g.,
H2S04
H+ + HSOi
or
H2SO4
2H+ -t- SO:-
=
(i) Two element acids:
From these definitions, an acid has two portions; the catbn part
which is H+ and the anion part (which carries the negative charge).
In naming acids by the IUPAC recommendation, the following
guidelines are helpful: (i) For aclds that contain only two elements,
the general rule applies, namely: the name of two element cornpounds end in "-id&'.
Examples:
HCI = hydrogen chloride acid
HP = hydrogen fluoride acid
HBr = hydrogen bromide acid
I
= hydrogen iodide acid '
(ii) 0 x 0 acids:
For the 0x0 acids, the anion part is named accordingly (as illustrated
-under anions) but the word "acid" is added in place of "ion".
Exumples:
I UPAC name
dioxonitrate (111) acid
zrioxonitrate (V) acid
trioxosulplial
tetraoxosulpl
trioxocarbon
tetraoxophos
tetraoxophos
(iii) Acidic oxides:
Elements on the right of the periodic table do not form simple ionic
oxides. They share electrons with oxygen atoms. Many of these
molecular oxides, such as sulphur (IV) oxide, SO2, an= gases at room
temperature and dissolve in water to give acidic solutions.
Exumples:
SO, (g) + H,O
CO, (g) + HzO
SO, (g) t H 2 0
j)I+
+ HSO;
+ CO$~ ++SO:-
2H'
2
The molecular oxides are, therefore, called acidic oxides or acidic
anhydrides. In their nomenclature by the IUPAC recommendation
the naBes end in "-iden since they are two element compounds. The
oxidation number of the key atom is also given in parenthesis.
Exumples:
SO,
SO,
NO
N20
sulphur (IV) oxide
sulphur (VI) oxide
nitrogen (11) oxide
nitrogen (I) oxide
NO3
Si02
C02
CO
nitrogen (VI) oxide
silicon (IV) oxide
carbon (1V)'oxide
carbon (11) oxide
However, there are compounds which cannot be named easily and
unambiguously by the above method which is known as the Stock
System. For example, the name nitrogen (IV) oxide describes both
NOz and N204. In such situations the use of Greek numerical
prefixes is preferred:
NO,
N204
P205
P40,,
nitrogen dioxide
dinitrogen tetroxide
diphosphorus pentoxide
tetraphosphorus decoxide
NOMENCUTURE WITH RESPECT TO
BASIC OXlDFS A N D BASES
(i) Amphottric oxides:
It is not possi.ble to classify all known oxides sharply as either acidic
or basic. Some oxides, especially those formed by elements towards
the centre of the periodic table are intermediate in behaviour. They
are able to neutralise both acids and bases. They are known as
amplwteric oyides.
E.g., ZnO
ZnO (s)
ZnO (s)
--
+ 2H+
ZnZ+ +
+ 2 0 ~ - & +H 2 0
HZO
[Zn (OH)$-
However, it is quite straight-forward naming these oxides. Most of
them are compounds with only two different types of atoms. Cunsequently, their names end in "-ide",,
Examples:
ZnO
AI2O3
Sb203
As203
= zinc oxide
= aluminium (111)
= antimony (111) OAIUG
= arsenic (111) oxide
(ii) Basic oxides:
These are also binary compouncIs and so their names end in "-id&'.
10s.
Na,O
LizO
CaO
sodium oxide;
lithium oxide;
calcium oxide;
CuO copper (11) oxidc
MgO magnesium oxide
BaO barium oxide
(iii) Hydroxides:
Hydrogen are three or more element compounds. We will, therefore, expcct their names to end in "-aten. This does not obtain and all
hydroxides, whether basic or ampboteric have their names ending in
.'-ide" like two dement compounds. They nnay be regarded as
exceptions t o therule. N o Roman figures are netcessary except where
the metal atom can exhibit variable oxidation sta tes. The metal or the
more electropositive component is named ti1rst followed by the
"hydroxide" ending.
KOH
potassium hydroxide
Mg(OH)2 magnesium hydroxide
AI(OH), aluminium hydroxide Fe(OH)2 iron (11) hydroxide
Fe(OH)3 iron (111) hydroxide
Ca(OH), calcium hydroxide
Cu(OH), copper (11) hydroxide
NaOH
sodium hydroxide
Zn(OH)* zinc hydroxide
NOMENCLATURE WITH RJISPECT TO SALTS
(i) Simple (anhydrous) salts.
Simple salts are derived from acids by neutralization reactions with
bases:
Base
+ Acid = Salt
+
NaOH + HCI = NaCl
+
Ca(OH)i+ H2S04 = CaS04
N H 4 0 H + HN03 =. NH4NOJ +
water
H20
+ 2H20
H20
The formation of a salt can then be looked upon as the replacement
of the hydrogen ion(s) in the acid by a metal or electropositive group.
In the IUPAC nomenclature, the name of this metal or electropositive group is added to the name of the anion component of the acid
from which it is derived. If the metal can have variable oxidation
numbers, the appropriate one is indicated in Roman numeral enclosed in parenthesis ( ) and placed immediately after the name of
the metal. The oxidation state of the central atom in the anion
portion is also indicated in Roman numerals as the examples below
illustrate:
Kl
NaCl
CaSO,
FcS04
Fe2(S04),
Na2C03
CuSO,
NH4N02
NH,N03
CaC03
PbS03
NaOCl
NaCIOJ
= potassium iodide
= sodium chloride
= calcium tetraoxosulphate (VI)
= iron (11) tetraoxosulphate (VI)
= iron (1li)tetraoxosulphate (VI)
= sodium trioxocarbonate (1V)
= copper (11) tetraoxosulphate (VI)
= ammonium dioxonitrate (111)
= ammonium trioxonitrate (V)
(IV)
(IV)
= sodium monoxochlorate (I)
= calcium trioxocarbonate
= lead (11) trioxosulphate
= sodium trioxochlorate
(V)
It must be noted thqt fractional oxidation ,numbers cannot be
represented in Roman numerals. E.g., the oxidation number of silver
in AgzFis + 4. In naming such compounds withI fracticnnl nv;rl..t;-V ~ I U U L I U I I
numbers, the use of Greek numerical prefixes is pre f a r e d . Thus,
Ag2F is disilver monofluride.
,119.
(ii) Acidic salts:
Their IUPAC names end in "-atew because th ey contam more than
two different atoms per molecule. The metal is 1named first, followed
by the hydrogen, and the anion group is name(d last. The oxidation
number of the key atom in the anion portionI is also indicated in
Roman numerals:
NaHS03 sodium hydrogen trioxosulphate (IV)
NaHSOI sodium hydrogen tetraoxosulphate (VI)
KHC03 ljotassium hydrogen trioxocarbona te (IV)
(iii) Basic d t s :
The cation is named first and then the other combining groups are
named ikalphabetical order.
Mg(0H)CI = magnesium chloride hydroxide (here chloride comes
before hydroxide in keeping with the alphabetical
order rule)
CY~(OH)~CI
= copper (11) chloride trihydroxklc (here again
chloride comes before hydroxide in alphabetical
order)
tiv) SaIts with water of crystcrllization:
In. general, water of crystallization and similar loosely bound molecules are designated by means of Arabic numerals before their
The salt portion is named as explained
formulae e.g., FeS04.7H20.
above for simple salts. This is then followed by a description of the
exact number of molecules of water associated with the salt. Any of
three methods can be used to describe this water of crystallization:
Na,C03. 10 H 2 0 = sodiuh trioxocarbonate (IV) decahydrate
MgSOJ . 7 H 2 0 = magnesium tetraoxosulphate PI)heptahydrate
FeS0, .7HZ0 = iron (11) tetraoxosulphate (VI) heptahydrate
CuS04. 5 H z 0 = copper (11) tetraoxosulphate (VI) pentahydrate
In the above nomenclature "-hydratep' refers to a molecule of water
~k~stallization
while the Greek prefix shows the number of molecules
of such water of crystallization associated with the saIt. Another
acceptable method of expressing the water of crystallization is as
follows:
Na2C03.10HzO = sodium trioxocarbonate (1V)-10-water
MgS04 7H20 = magnesium tetraoxosulphate (V1)-7-water
FeS04.7Hz0 = iron (11) tetraoxosulphate (V1[)-7-water
CuS04.5H20 = copper (11) tetraoxosulphate I(VI)-5-water
-- - - -.
In this method the numbers 10, 7, 7, and 5 indicate the number of
water of crystallization respectively. A third alternative makes use of
a combination of the Greek p r e h and the Latin-derived word
"aquo", such that:
.
a.
Na,CO3. 10H20= sodium decaaquotrioxocarbonate (IV)
MgS04. 7H20 = magnesium heptaaquotetraoxosulphate (VI)
FeS0,. 7H20 = iron (11) heptaaquotetraoxosulphate (VI)
CuS04.5H90 = cooDer (11) ~entaaauotetraoxosulphate(VI)
DOUBLE SALTS: GUIDELINES FO
AND NOMENCLP
(i) in writing the formulae of double sa
placed first and then followed by the anions. 1
in order of inc;easing valence (except hydro1
~tionsare arranged
Exumples:
In KMgF3, the cations are K+ and M ~ ~Ki
+ ,
the formular in increasing order of valenc
valence also explains the order in which the cations appear in:
NH4MgP04.6H20, cations: NH: and ~ g ~ +
(NH4)2Fe (SO,&.6H20, cations: NH; and Fe2+
(ii) When two or more cations have the same valence, they are
arranged in order of decreasing atomic number, with the polyatomic
ions. (e.g. ammonium, NHZ) at the end of the appropriate valence
group.
In KNaC03, the cations K + and Na+ are in the same valence group.
These are, therefore, arranged i,n order of decreasing atomic number.
The atomic number of potassium is 19 while that of sodium is 11.
In TINa(NO&, the cations TIi and Nat--arein the same valence
group and so are arranged in order of decreasing atomic number: TI
(atomic number = 81), Na (atomic number = 11).
(iii) When hydrogen is present as a cation (acidic hydrogen) the
symbol is placed last among the cations.
NaNH4HP0,.4H20. Here NH; is polyatomic and so comes after
Na+ according to guideline (ii). H+ comes last among the cations on
the basis of guideline (iii).
(iv) Anions present in double salts are cited in the following
group order:
1. 1-I2. 0*- and O H - (in that order)
3. o n e element inorganic anions other than H- and 02-.(The
order of appearance is: 0, Si, C, Sb, As, P, N, T e , S e i S , At, I,
Br, CI, F)
4. Inorganic anions containing two or more elements, other than
OH-. (In citing this group of anions, anions with the smallest
number of atoms, are cited first. For two anions with the same
number of atoms, they are cited in order of decreasing i t o mic number of the central atoms).
Exumples:
(v) In naming double salts, the component cations and anions are
named as illustrated for cations and anions in simple saks. However,
the cations present in the formula are named in alphabetical order.
Illustrative examples:
KNaCO,:
potassium sodium trioxocarbonate (IV)
KMgF3:
magnesium potassium fluoride
sodium thallium (1) trioxonitrate (V)
TINa(N03),:
NH4MgP04.6 H 2 0 : ammonium magnesium
tetruoxophuspharc (V) hexahydrate
amnloniurn iron (11) tetraoxusulphate (VI)
(NH,)*Fe(SO,),:
NaNH,HPO, . 4H20: sodium ammonium hydrogen
tetraoxophosphate (V) tetrahydratc
NH4AI(S04)2:
aluminium amn~uniumt ~ t r a ~ x o s u l p h i i (t eV l )
(hexa) sodium chloride tluoride ( b ~ s )
Na6CIF(S04),:
tetraoxosulphate
Ca5F(P04)3:
(penta) calciumfluoride (tris)
tetraoxophosphate
KAI(SO,), . 121-I2D: aluminium potassium bis
[tetraoxosulphatc (VI)] dodecahydrate
THE HALIDES OF CAI
Although these halides of carbon be
organic chemistry and are better discuss1
thcre is need to underscore their IUPA
can be found in inorganic texts as well
rccommcndation, these group of com
carbontetrahalides are to be regarded a>
of halogen atoms per molecule being sp
CF4
CClj
CBr4
CI,
CIiCI
CHBr3
=
=
=
=
,=
=
C:H2C12 =
CHI3
Cb
=
tetruHuoromethane
tetrachloromethane
tetrabrom~methitn~
tetraiodomethane
trichlorornethane
tribron~omethant:
dichioromcthane
triiodomethane
Free radicals are odd electron molecules or atoms. Most ot' then1
are electrically neutral (a few radical ions arc: known). All possess
addit~onproperties and are extremely reactive.
Example:
It is normal to represent the symbol o r formula of it radical with a dot
to signify the add electron. Names of radicals have two components:
the name of the element or group plus the word "radical."
Examples:
F'
CI'
Br'
I'
CH;
fluorine radical
chlorine radical,
bromint: rcldical
iodine radical
methyl radical
FORMULAE AND NAMES 01:COMPO
We can now summarize some of the highli
writing formulae and naming of inorganic c
In writing a chemical formula the ele,
(cation) is written first before the clectron
KCI, nor CIK; NH,NO,, not N 0 3 N H 4 ) .
If the compound contains more than o r
tuent, these are arranged in order of increa
When a binary compound is formed I
constituent which appears earlier in the sc
first. Sequence: B, Si, CjSb, As, P, N, H, TI
F. E.g., NH3, not H,N.
The number of identical atoms o r atomic groups in a formula is
indicated by means of Arabic numerals, placed below and t o the right
of the symbol or symbols in piirenthesis ( ) o r brackets [ ] to which
they refer. E.g., CaCI2, not CaC12; (NM,)2S0,, not 2(NH4)SO,.
However, .water of cryskdlization and similar loosely bound rnolccuks are designated by means of Arabic nunwrals bufore their
formulae. E.g., Na2S0,. 10H20.
? h c charge on thc formula of an ion reprcsuuts tllc arilhnlclic sum
of the oxidation numbers of aH-the con~titucntatoms.
In NH:, sum of oxidation numbers = -3 for N plus +4 for 4(Hj,
giving a net + 1 charge. In SO;-, sum of oxidation numbers = + 6 for
S plus -8 for 4(0) = -2.
The systematic names of compounds ure formed by indicating the
conslit uents and their proportions. The stoichimetric proportion of
the constituents may be expressed in the name of a compound by
means of Greek nurnerical prefixes (mono, di ... ) preceding
without hyphen the names of the elements t o which they refer. E.g.
N,O (dinit rogen oxide), NO2 (nitrogen dioxide). However, the
Stock's system has gained the upper hand. In this system, the
proportions of constituents are indicated indirectly
...
als representing the oxidatidn number or stoichiometric valence of
the element. This is placed in parenthesis immediately following the
name of the atom to which it refers.
Exumples:
N 2 0 nitrogen (I) oxide
NOz nitrogen (IV)oxide
FeClz iron (11) chloride
The name of the electropositive constituent (or that treated as
such) is not modified. Examples CaO (calcium oxide), AgCl (silver
chloride),
I n a compound in which the electronegative constituent is
monoatomic, the name of the compound ends in "-ide).
Examples:
(NH,),S (ammonium sulphide). However, when the electronegative
constituent is polyatomic, the name (with a few exceptions) ends in
"-atew. E.g. NH4N03 ammonium~trioxonitrate(V).
The terms sulphate, nitrate, phosphate, etc., were originally
assigned to anions of particular 0x0 acids. These terms are now used
more generally for any negative group containing sulphur, nitrogen,
phosphorus, etc., respectively, as the central atom, irrespective of its
oxidation state and the number and nature of the ligands.
sodium tetraoxcwulphare (VI)
sodium trioxosulphate (IV)
sodium trioxothicxrulphate (11)
sodium trioxofluorosulphate (VI)
sodium tetraoxophosphute (V)
sodium tetrathiophosphate (V)
sodium hexachlorophosphate (V)
potassium dioxodifluorophosphale (V)
potassium oxodichloroimidophosphate
Names such as sodium sulphate, sodium thiosulphate, etc., can now
be regarded as abbreviations in the above system of nomenclature.
.
FORMULAE AND IUPAC NAMES OF SOME COMMON
COMPOUNDS AND IONS
Formula
Name
AgCl
AgN03
ALC3
silver chloride
silver trioxonitrate (V)
aluminium carbide
aluminium (111) oxide
arsenic (111) oxide
barium (11) oxide
barium (11) peroxide
barium tetraoxosulphate (VI)
bismuth (111) chloride oxide
bromide ion
calcium dicarbide
calcium dichloride
calcium trioxocarbonate (1V)
calcium hydrogen trioxwarbonatc (Icalcium oxide
calcium hydroxide
calcium tetraoxosulphate (VI)
tetrabromomethane
tetrachioromethane
tetrafluoromethane
trichloromethane
tribromomethane
dichloromethane
tetraiodomethane
carbon (11) oxide
carbon (IV) oxide
trioxocarbonate (IV) ion
chromium (11) oxide
chromium (111) oxide
chrdmium (VI) oxide
chromium (111) sulphide
A1203
As203
BaO
Ba02
BaSO,
BiOCl
BrCaC2
CaCll
CaC03
Ca (H C03)2
CaO
#"(OW2
CaSO,
CBr4
CCI,
CF4
CHC13
CHBr-,
CH2C12
Cl4
CO
COz
co: CrO
(3203
CrOJ
(32%
CrSO,,
-'
copper (TI) chloride
dicopper (11) frioxocarbonate (IV)
dihydroxide
copper (11) oxide
copper (1) oxide
tetraarnine copper (11) dichloride
copper (11) hydroxide
copper (11) chloride trihydroxide
copper (11) tetraoxosulphate (VI)
capper (11) tetraoxosulphate (VI)
pentahydrate
iron (If) chloride
iron (111) chloride
iron (11) oxide
iron (111) oxide
triiron tetraoxide
iron (11) hydroxide
iron (111) hydroxide
iron (IS) s u l ~
iron (11) tetr
e (v1)
e (VI) heptahydrate
iron (11) tetr
iron (111) tetraoxosulpnate (V1)
hydrogen bromide acid
hydrogen chloride acid
mercury (I) chloride
mercury (11) chloride
hydrogen fluoride acid
hydrogen iodide acid
trioxonitrate (1V) acid
trioxonitrate (V) acid
tetraoxophosphate (V) acid
tetraoxosulphate (IV) acid
tetraoxosulphate (VI) acid
iodine (I) chloride
iodine (V) oxide
aluminium potassium bis
[tetraoxosulphate,(VI)] dodecahydrate
potassium bromide
potassium heptaoxodichromate (VI)
potassium monoxchlorate (I)
potassium trioxochlora te (V)
potassium hexac:yanoferrate (11)
potassium hexac:yanoferrate (111)
potassium iodidcrn
potassium tetrac~xomanganate(VII)
potassium tetracyanonicollate (0)
potassium oxide
potassium tetrac~xosulphate(VI)
magnesium chloride
magnesium oxidle
magnesium h y droxide
~
magnesium chlaride hydroxide
magnesium tetrlioxosulphate (VI)
magnesium tetriioxosulphate (VI)
heptahydrate
manganese (I I) chloride
manganese (11) oxide
manganese (IV) oxide
manganese (111) oxide
trimanganese tetraoxide
manganese (11) tetraoxosulphate (Vl)
sodium hexafluoroalumnate (111)
sodium chloride
sodium monoxchlorate (I)
sodium trioxochlorate (V)
sodium trioxocarbonate (IV)
sodium hydride
sodium hydrogen trioxocarbonate (IV)
sodium dihydrogen tetraoxophosphate (V)
sodium hydrogen trioxosulphate (IV)
sodium hydrogen tetraoxosulphate (VI)
dioxonitrate (111) ion
srioxonitrate (V) ion
sodium hydroxide
sodium trioxosuiphate (IV)
sodium tetraoxosulphate (IV)
ammonium ion
ammonia solution
amrnooium dioxonitrate (111)
ammonium trioxonitrate (V)
aluminium ammonium tetraoxosulphate (VI)
w
NaCl
NaClO
NLICIO~
Ni12C03
NaH
NaliC03
NaH,IJ04
NallSO,
NaHSO,
NO;
N 0,
NaOI-I
Na2S03
Na2S04
NH:
NHIOH
N H4NO2
NH4N03
NI 14AI(S04)2
(NH4)2Fe(S04)2
N2O
NO
NO2
N204
IY2@
amnfonium iron (II) tetraoxosulphate (Vl)
nitrogen (I) oxide
nitrogen (11) oxide
nitrogen (IV) oxide
dinitrogen tetraoxide
nitrogen (V) oxide
nitroeen (VI\ oxide
NO,
NiO
Ni02
Ni(OH)*
nicl
nicl
nickel (11) hydrOXld&
PbCl,
PbCI3
le
le
PbCIS
PO:poi-
le
terraoxopnospnarc ( vl) ion
tetraoxophosphate (V) ion
tetraphosphorus dccaoxidt
lead (11)I bxide
lead (IV') oxide
trilead trmaoxide
lead (11)I sulphide- lead (11) tnoxosulphate (N)
lead (11) tetraoxosulphate (VI)
lead (11) trioxonitrate (V)
phosphorus (UI) chloride
phosphorus (V) chloride
antimony (111) oxide
silican (IV)oxide
sulph~ u r(IV) oxide
sulphbur (VI) oxide
trioxosulpnare (I v ) Ion
tetraoxosulphate (V1) ion
zinc 1oxide
zinc chloride
zinc tetraoxosulphate (V 1)
P4O10
PbO
PbOz
bO4
PbS
PbS03
PbS04
Pb(NW2
PC13
PCIS
Sb203
Si02
SO2
SO3
so: so;ZnO
ZnCI,
ZnSOJ
a
rn
A
I,.,\
!-
1
bxochlorate (I) ion
trioxochlorate (V) ion
tetraoxochlorate (VII) ion
trioxocarbonate (IV)ion
heptaoxod
I L I ~ I U I I I ~ C C\; v I) ion
hydrogen Itrioxocarbonate (IV) ion
tetraoxom;angiinate (Vl) ion
tetraoxom;anganate, (VlI) ion
dioxonitraite (111) i on
trioxonitra te (V) ic>n
trioxosulpilate (IV:
I ion
tetraoxmu lphate (1f1) ion
thiosulpha~
te ion or
tfioxosuIp~
~ursulphi
3te (IV) ion
tetrathiona~ t eor
hexaoxodhrulphurd!isulphare (V) ion
persulphatie or
hexaoxope roxodisu lphate (VI) ion
Basic Salts
,...-.
BiOCl
Mg(0H)CI
PbzCOdOH)2
bismuth (I,,,
ide oxide
magnesium chloridle hvdroxide
dilcad (11) trioxocarbok (IV) diL-+"---:-'-
W o u b l e Salts
Fe(NH&(SO,)
,.6 H 2 0 diammonium iron (11) bis
KAI (SO&. 12H20
[tetraoxosuIphate (VI)]-bexahyc
aluminium potassium bis
[tetraoxosulphate (VI)]-dodecal
Complex Ioru
diamminesilver (I) ion
tetrahydridoalurninate (111) ion
tetrahydroxodiaquaalurninate (111) ion
tetrahydridoborate (111) ion
diammine copper (I) ion
tetraamminecopper (11) ion
hexacyanoferrate (11) ion
hexacytlnoferrate (UI)ion
oxonium ion or
hydronium ion or
hydroxonium ion
ammonium ion
tetraammine zinc (11) ion
9. Give the chemical formulae of the following compounds:
(i) sulphur (11) chloride
(ii) bromine (111) fluoride
(iii) manganese (IV) oxide
(iv) mercury (11) chloride
( v ) niolybdc~~um
(VI) oxidc
(vi) dinitrogen tetroxide
(vii) diphosphorus pel-- ' '
(viii) dichloromethane
10. The following names have been submitted by students for the
compounds and ions indicated. Each is wrong in at Icilst orie
respect. Indicate what is wrong in each case:
(i) MnFJ
manganic fluoride
(ii) F e S 0 4 .'lh& iron (111) tetraoxosulphate (VI)
pentahydrate
(iii) NO,
trioxonitrate (111) ion
(iv) NaCIQ3
sodium oxochlorate (1)
(v) SO$tsioxosulphate (IV) ion
THE PERIODIC TABLE OF ELEMENTS
a
1I.i
!
4
6.841
9.U1218
I1
19,
Na
u.esw7
JV.lHll
Rb
85.4671
55
8
He
10.111
Mg
tr.31~~
4I.lMJ
38
U.VS59
Sr
87.152 1.9059
56
7
22
5B
23
47.W
50.9414
411
V
6B
78
24
.25
Cr
5I.M
OB
26
27
2E
511.70
Mn
Fe
Co
Y.Y.7WI
55.847
5A.9332
I
Se
Br
7H.'&
79.WM
SO
51
52
53
5.
IIJ.l$2
Ilb.bY
121.75
127.W
lb.W+5
Irl.30
81
82
83
X4
85
At
Hn
Gu , Ge
69.72
9S.M
98.YUbZ
101.07
l%2.9WS
106.4
107.4WI
77
78
79
132.9(%4
IJ7..U
138.W55
178.49
IOO.llJ7Y
1113.m
186.287
1Bt.L
192.22
39.619
As
7,n
b5.33
73
Yf
J.~..Jz)
74.V116
Cu
9Z.W
Ir
At-
72.59
2 8 . 0 ~ 30.9737~ JZJM
63.544
72
0s
IH
Cl
32
91.22
Re
D.17V
31
Rh
W
34
17
w.carsr
Ru
l'a
13
S
10.WKIY
30
Tc
Hf
f
!h
2B
Mo
*La
IS.%
29
Nb
Ba
I.I.Ulf67
1B
Zr
Cs
IZ.UII
10
Au
112.40
4;
TI
Ph
Ili
R,
HJ.
86
APPENDIX 2:
OXI9ATION STATES OF ELEMKNTS 1N THE PERIODIC
TABLE. WHERE A N ELEMENT CAN HAVE MORE THAN ONE
0XIL)ATION STATES, THE MOST COVMON O N K 1s GIVEN IN
BOLD TYPE.
Groups
APPENDIX 3:
TADLE OF ELEMENTS, SYMBOLS, A'TOMIC NUMBER A N D
RELATIVE ATOMIC MASSES. THE ArTOMlC MASSES AWE
BASED ON CAHBO?Y-12.
Symbol
Actinium
Alun~inum
Americium
Antimony
Argon
Arsenic
Astatine
Hariunr
Lferkellum
Beryllium
Bisniuth
Boron
Bromine
Cadmium
Calcium
Cali&rnium
Carbon
Cerium
Cesium
Chlorine
Chromium
Cobalt
Copper
Curium
Dysprosium
Einsteinium
Erbium
Europium
Fermium
Fluorine
Francium
Gadolinium
Gallium
Germanium
Gold
Hatnium
Ac
Al
Am
Sb
Ar
As
At
Ba
Bk
Be
Bi
U
Br
a
Ca
Cf
C
Ce
Cs
CI
cr
eo
Cu
Cm
DY
Es
E;
Ell
bm
F
Fr
Gd
Gn
Ge
Au
HI
No.
Atomic Muss
12271
P433'
121.75
137.34
208.980 J
10.81
79.w
112.40
40.08
W I
12.01 1
140.12
132.ws4
35,453
51.996
58.9332
63.546
r2471
162.50
12541
167.26
151.96
12571
18.99840
P I
157.25
69.72
72.59
196.966 5
178.49
1 lelium
Holmium
1-1ydrogen
Indium
Iodine
Iridium
Iron
Krypton
Lanthanum
Lawrencium
I-cad
Lithium
1.11terium
Mitgncsium
hlangancse
Mendelevium
Mercury
Molybdenum
Neodymium
Neon
Neptunium
Nickel
Niobium
N~trogen
Nobelium
Osmiuni
Oxygen
I'~ilIidi~i~~
Phosphorus
Platinum
Plutonium
Poionium
Potassium
Praseodymium
Promethium
Protactinium
Kadium
Radon
Rhenium
Rhodium
Rubidium
IWhenium
Samarium
Scandium
Selenium
Silicon
Silver
Sodium
Strontium
Sulfur
Tantalum
Technetium
Tellurium
Terbium
Thallium
Tl~oriun~
Thulium
Tin
Titanium
Tungsten
Uranium
Vanadium
Xenon
Ytterbium
Yitriunl
Zinc
Zirconium
e
'A value given in brackets denotes the mass number of the
isotope.
11.
Give
(i)
(ii)
(iii)
(iv)
systematic names for the following
KCaPO,
NaHC03
NO
CrC03
(v) Ag2F
APPENDIX 4:
ANSWERS TO NUMERICAL QUESTIONS
2. :;K+
3. (i) t 6
(ii) 4-6
(iii) +2
4. (a) - 1 , + I , +3, and +7 respectively.
(b) +6, +4, +7, +2:; and 7 respcctivcly.
(c) +3, +6$, +6, -t6, and $3 rcspectively.
5. (a) +3, -2
(b) +2, t 3 , -2
(c) $ 5 , - 1
(d) +3, -2
(e) +6, -2
(f) -?
6. (a) +4
(e) + 3
(f) -1
(b) +2
(d + 2
(c) +7
(d) I-6
(h) + 6
7. (i) chromium changed oxidation number from +6 to + 3
(ii) oxygen changed oxidation number from -2 to O
8.
Oxid. No. of Reactants
Oxid. No. of Products
+7
Mn
0
-2
C1
-1
+2
-2
O
H
+1
-t 1
(i) SOCI,
(ii) BF,3
(iv)
I-IgCI,
(iii) h1110,
(v) hlo0.3
(vi) N,O,
(vii!) CH2CI2
(vii) P 2 0 5
10. The correct names are:
(i) manganese (IV) fluoride ,
(VI) hcptahydra~e
(ii) iron (11) te~raoxosulpha~e
(iii) trioxonitrate (V) ion
(IV)
sodium trioxochlornte (V)
( v ) t ~ . i ~ ~ o s u l p h i(1V)
i t e ion
11. (i) cdcium potassium tetraoxophosphate ( V ,
(ii) sodium hydrogen trioxocarhonate (1V)
( i i i ) nitrogcn (11) oxide
(iv) chromium (!I) triost)carbonrttc (IV)
(v) disilver rno~wfluoridt:
9.
1
APPENDlX 5:
GLOSSARY
i d :
a substance which on being diswlved in water
produces a solution in which the hydrogen ion
concentration is greater than 1 W 7 ~Exam.
ples: H2S04, H N 0 3 , HCI, H2C03.
allotropy:
the property which some elements possess of
existing in different forms with different properties. The chief differences are' usually found
in the physical properties, though there are
sometimes differences in the chemical propeities as well. The different forms of the element are called allotropes, or allotrcrpic
modifications. Example: O2 and 03.
am&~tericoxide:
an oxide which can function both as a basic
oxide and as an acidic oxide, depending on
reaction conditions. Examples: ZnO, A1203.
anion:
an ion that is negatively charged. Examples:
C1-, SO:-, NO;.
atomic number:
the number of protons in the atomic nucleus,
and hence the number of unit positive charges
on the nucleus. It also represents the nuniber
of extranuclear electrons in an atom.
base:
a substance which on being dissolved in water
produces solution in which hydroxide ion concentration is gredter than 10-'M. fianlples:
NaOH, KOH, NH3.
cation:
an ion that is positively charged. Eramples:
Li+,Ca2+, AP+,
electronegativity:
a measwe of the tendency of an atom to attract
shared electrons.
electropositive
refen to elements whose atoms tend to lose
elements:
elections easily. Examples: Li, Na, K,Ca, Mg.
ion :
a charged species; an entity chrryinp either
positive or negative charge. Fsanrples: CI- ,
SO:-, NHZ, Ca2+
different kinds of atoms of the same element.
They have the same atomic number (and consequently they have t h e same arrangemnt of
extranuclear electrons and hence the same
chemical properties). They differ solely in having different mass numbers on account of.
having different numbers of neutrons on the
nucleus. Example: the three isotopes of oxygen
are: '20,
I@,
'@
isotopes:
ligand:
neutralization:
a species bonded to the central atom in a
complex ion. Examples: H 2 0 in [ A I ( H ~ o ) ~ J ~ + ,
OH in [Zn(OH),I2-
a term used to describe the reaction between
an acid and a base t o give a neutral (sah)
solution.
nonpolar bond:
a chemicat bond in which there are no positive
and negative ends; mainly found in homonuclear diatomic molecules such as CI,, 0 2 ,H2.
periodic table:
an arrangement of the elements into rows and
columns such that elements with similar properties occur in the same column.
I
I
I
I
I