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Theoretical
Physical Chemistry Revision
Notes
The shapes of Molecules and Ions
and bond angles
related to their Electronic Structure
Part 2 Some other molecules and ions of carbon,
nitrogen, sulfur and chlorine and other elements in the same group i.e.
in groups 14, 15, 16 and 17
[Author
©
Dr
WP Brown PhD: Doc
Brown's advanced level inorganic chemistry exam revision notes suitable
for students of UK AQA, Edexcel, OCR, Salters, WJEC, CCEA & IB advanced
level chemistry courses & US K12 grades 11-12 and AP honors chemistry courses:
shapes and bond angles of
selected oxide molecules
and oxyanions of
carbon, nitrogen, sulfur and chlorine
[page updated Mar 9th 2026 *]
SHAPES OF MOLECULES INDEX:
two other separate pages
Introduction - theory - lots of inorganic
molecule/ion examples
shapes and bond
angles of organic molecules
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All by structure
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Introduction
Molecule shapes, dot and cross
diagrams, bond angles for selected molecules and ions of nitrogen,
sulfur and chlorine using the valence-shell electron-pair repulsion
model (VSEPR) and the dot and cross (ox) diagrams are presented in
'Lewis style' The 'scribbles' will be replaced by
neat diagrams eventually!
A
description, explanation, shapes
and bond angles of the carbonate ion, nitrate(III) ion (nitrite ion),
nitrate(V) ion (nitrate ion), nitrogen(IV) oxide (nitrogen dioxide),
nitronium ion, sulfur(IV) oxide (sulfur dioxide), sulfur(VI) oxide
(sulfur dioxide), sulfate(IV) ion (sulfate ion), sulfur(VI) ion
(sulfate ion), chlorate(III) ion, ClO2- (chlorite ion), chlorate(V) ion, ClO3- (chlorate ion)
and the chlorate(VII) ion, ClO4- (perchlorate
ion) are all described and discussed.
Carbon
in Group
4/14
- Carbonate ion,
CO32- is trigonal planar in shape with a O-C-O
bond angle of 120o because of three groups of bonding
electrons and no lone pairs of electrons.
- The shape is deduced below
using dot and cross diagrams and VSEPR theory and illustrated below.
- Note that all the C-O bonds are identical due
to delocalisation of some of the electrons (σ
sigma and π pi bonding)
valence bond dot and cross diagram for the carbonate
ion
2.
Nitrogen
in Group 5/15
- Nitrogen(IV)
oxide, NO2 (nitrogen dioxide) is bent shaped
(angular), O-N-O bond angle ~120o because of two
bonding groups of bonding electrons and a single lone electron in
the same plane as the bonding pairs of electrons.
- The nitrate(III) ion,
NO2- (nitrite
ion) is bent shaped (angular), O-N-O bond angle ~120o
due to two groups of bonding electrons and one lone pair of
electrons.
- The nitrate(V) ion, NO3- (nitrate ion)
is trigonal planar, O-N-O bond angle 120o due to three
bonding groups of electrons and no lone pairs of electrons.
- The nitronium ion, NO2+,
is linear, O-N-O bond angle of 180o because there are two
groups of bonding electrons and no lone pairs of electrons (you
easily see this from the NO2 neutral molecule diagram
below).
- The shapes are deduced below
using dot and cross diagrams and VSEPR theory and illustrated below.
valence bond dot and cross diagrams for nitrogen
oxides and nitrogen oxyanions
Note that all the N-O bonds within the
molecule or ion are identical due to delocalisation of some of the
electrons (σ sigma and π
pi bonding)
Sulfur
in Group 6/16
- Sulfur(IV)
oxide, SO2 (sulfur dioxide/sulfur dioxide)
molecule is a bent shape (angular), O-S-O bond angle ~120o
due to two groups of bonding electrons and one non-bonding lone pair
of electrons.
- The sulfate(IV) ion/sulfate(IV) ion,
SO32- (sulfite ion/sulfite
ion) is a trigonal pyramid shape, O-S-O bond angle ~109o
due to three groups of bonding electrons and one lone pair of
electrons.
- Sulfur(VI) oxide/sulfur(VI) oxide, SO3 (sulfur
trioxide/sulfur trioxide),
is a trigonal planar shape, O-S-O
bond angle of 120o due to three bonding groups of
electrons and no lone pairs of electrons.
- Sulfate(VI) ion/sulfate(VI)
ion, SO42- (sulfate ion/sulfate ion)
is tetrahedral in shape, O-S-O bond angle of 109.5o. due to
four groups of bonding electrons and no lone pairs of electrons.
- The shapes are deduced below
using dot and cross diagrams and VSEPR theory and illustrated below.
The valence bond dot and cross diagrams for sulfur
oxides and sulfur oxyanions.
Note the delocalisation is the more
realistic distribution of electron charge.
Theoretically you can substitute Se or Te
for S in group 6/16.
Note that all the S-O bonds within the
molecule or ion are identical due to delocalisation of some of the
electrons (σ sigma and π
pi bonding)
Chlorine
in Group 7/17
- Consider three oxyanions of the
halogens in their
+3,
+5
and +7
oxidation states (oxygen is in its
-2 oxidation
states)..
-
The chlorate(III) ion,
ClO2- (chlorite ion), is bent shaped (angular), O-Cl-O bond angle ~109o because of two
groups of bonding electrons and two lone pairs of electrons.
-
The
chlorate(V) ion,
ClO3- (chlorate ion),
is a trigonal pyramid shape, O-Cl-O bond angle ~109o
because of three groups of bonding electrons and one lone pair of
electrons.
- The chlorate(VII) ion,
ClO4- (perchlorate
ion), is a tetrahedral shape, O-Cl-O bond angle 109.5o
due to four groups of bonding electrons and no lone pairs of
electrons.
- The shapes are deduced below
using dot and cross diagrams and VSEPR theory and illustrated below.
- In most cases you can write
similar formulae and oxyanion structures for bromine and iodine ions
in their oxidation states of +3, +5 and +7.
The valence bond dot and cross diagrams for selected
chlorate ions.
Note the delocalisation is the more
realistic distribution of electron charge.
Theoretically you can substitute Br or I
for Cl in Group 7/17.
Note that all the Cl-O bonds within the
molecule or ion are identical due to delocalisation of some of the
electrons (σ sigma and π
pi bonding)
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Revision notes for GCE Advanced
Subsidiary Level AS Advanced Level A2 IB
Revise AQA GCE Chemistry OCR GCE Chemistry Edexcel GCE Chemistry Salters
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Explaining the importance of
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