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Brown's Chemistry
Advanced Level Inorganic Chemistry Periodic Table
Revision Notes
Part
4. Revising Survey of Period 2 Li to Ne
4.1 Survey of the individual elements of Period 2
A summary of the
physical and chemical characteristics of the elements of period 2,
lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and neon.
For non-A level
students ...
 KS4 Science GCSE/IGCSE
Periodic Table notes links
INORGANIC Part 4
Period 2 survey sub-index : 4.1 Period 2 survey of the
individual elements : 3. lithium : 4. Beryllium
:
5. Boron :
6. Carbon : 7. Nitrogen
:
8. Oxygen :
9. Fluorine
:
10. Neon *
4.2 Period 2
element trends
& explanations of physical properties
*
4.3 Period 2
element trends
in bonding, structure, oxidation state, formulae & reactions
Advanced
Level Inorganic Chemistry Periodic Table Index *
Part 1
Periodic Table history
* Part 2
Electron configurations, spectroscopy,
hydrogen spectrum,
ionisation energies *
Part 3
Period 1 survey H to He *
Part 4
Period 2 survey Li to Ne * Part
5 Period 3 survey Na to Ar *
Part 6
Period 4 survey K to Kr and important trends
down a group *
Part 7
s-block Groups 1/2 Alkali Metals/Alkaline Earth Metals *
Part 8
p-block Groups 3/13 to 0/18 *
Part 9
Group 7/17 The Halogens *
Part 10
3d block elements & Transition Metal Series
*
Part 11
Group & Series data & periodicity plots
Part 4. Survey
of Period
2: Li across to Ne (8 elements, Z = 3
to 10)
4.1 Survey of the individual elements Li, Be, B, C,
N, O, F and Ne
 Z = 3 lithium
Li in Group 1 Alkali Metals
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction of
element with oxygen:
-
Reaction of
oxide with water:
-
Reaction of
oxide or hydroxide with common mineral acids:
-
Li2O behaves as a
basic oxide dissolving to form
the chloride, sulphate and nitrate salt in the relevant dilute acid.
-
The
hydroxide MOH is a strong base and alkali (since a soluble base) and
similarly forms salts.
-
 Li2O(s) + 2HCl(aq)
==> 2LiCl(aq) + H2O(l)
-
Li2O(s) + H2SO4(aq)
==> Li2SO4(aq) + H2O(l)
-
Li2O(s) + 2HNO3(aq)
==> 2LiNO3(aq) + H2O(l)
-
In all cases the
ionic equations are
-
Reaction of
oxide with strong bases/alkalis:
-
Reaction of
element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of
element with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 4 Beryllium
Be in Group 2 Alkaline Earth
Metals
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction of
element with oxygen:
-
Reaction of oxide with
water:
-
Reaction of
oxide with acids:
-
Behaves as a
basic oxide dissolving to form
the chloride, sulphate and nitrate salt in the relevant dilute acid.
-
BeO(s)
+ 2HCl(aq) ==>
BeCl2(aq) + H2O(l)
-
BeO(s)
+ H2SO4(aq) ==>
BeSO4(aq) + H2O(l)
-
BeO(s)
+ 2HNO3(aq) ==>
Be(NO3)2(aq) + H2O(l)
-
In all cases the
ionic equation is: BeO(s) + 2H+(aq)
==> Be2+(aq) + H2O(l)
-
Reaction of
oxide with strong bases/alkalis:
-
The oxide also
behaves as an acidic oxide by dissolving in strong soluble bases
to form beryllate(II) salts.
-
BeO(s)
+ 2NaOH(aq) + H2O(l) ==>
Na2[Be(OH)4](aq)
-
e.g. forming sodium
beryllate(III) with sodium hydroxide.
-
ionic equation:
BeO(s)
+ 2OH-(aq) + H2O(l)
==> [Be(OH)4]2-(aq)
-
Therefore beryllium
oxide is an amphoteric oxide, because of this dual acid-base
behaviour.
-
Reaction of
element with chlorine:
-
Reaction of chloride
with water:
-
Reaction of
element with water:
-
Other comments:
-
Beryllium shows
considerable anomalous behaviour compared to the rest of Group 2
(Mg to Ra) e.g. the covalent chloride and the amphoteric oxide. It
also has a maximum co-ordination number of 4, e.g. in the tetra-aqa
beryllium(II) ion and the beryllate(II) ion shown above. This applies to all the period 2
elements, but for period 3 e.g. magnesium, the maximum co-ordination number is 6.
-
Links to other pages
on site:
Z = 5
Boron B in Group 3/13
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction of element with oxygen:
-
Reaction of
oxide with water:
-
Reaction of
oxide with acids:
-
Reaction of
oxide with strong bases/alkalis:
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 6 Carbon C
in Group 4/14
-
The
structure of the element:
-
Non-metal existing as
three allotropes covalently bonded. Diamond (tetrahedral bond
network) and graphite (layers of connected hexagonal rings) have
giant covalent structures Cn where n is an extremely
large number, and a series of large molecules (3rd allotrope) called fullerenes
e.g. C60.
-
Bonding
details and diagrams of the allotropes of carbon.
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Gp4; e.c. 2,4 or 1s22s22p2; (can
be +2,
but usually +4) e.g.
-
(+2) CO, (+4) CO2 and CCl4 etc.
-
Reaction of element with oxygen:
-
Reaction of
carbon dioxide with water:
-
Quite soluble to form
a weakly acid solution of pH 4-5. So called carbonic acid, H2CO3,
does not really exist, but the dissolved carbon dioxide reacts
with water to form hydrogen/oxonium ions and hydrogencarbonate
ions. The equilibrium is very much on the left - hence the fizz in
'fizzy drinks'!
-
Reaction of
oxide with acids:
-
Reaction of
oxide with bases/alkalis:
-
It is a weakly
acidic oxide dissolving sodium hydroxide solution to form sodium
carbonate.
-
CO2(g) + 2NaOH(aq)
==> Na2CO3(aq) + H2O(l)
-
ionic equation:
CO2(g) + 2OH-(aq) ==> CO32-(aq)
+ H2O(l)
-
With excess of
carbon dioxide, sodium hydrogencarbonate is formed.
-
CO2(g) + Na2CO3(aq)
+ H2O(l) ==> 2NaHCO3(aq)
-
ionic equation:
CO2(g) + CO32-(aq)
+ H2O(l) ==> 2HCO3-(aq)
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 7 Nitrogen
N in Group 5/15
-
The structure of the
element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Gp5; e.c. 2.5 or 1s22s22p3;
Variety of oxidation states from -3 to +5 e.g.
-
NH3
(-3), N2O (+1), NO (+2), NCl3 (+3), NO2
(+4) and N2O5 and HNO3 (+5).
-
Reaction of element with oxygen:
-
At high temperatures
e.g. in car engines, nitrogen(II) oxide (nitrogen monoxide)
is formed.
-
and the nitrogen(II)
oxide rapidly reacts in air to form nitrogen(IV) oxide (nitrogen
dioxide).
-
The theoretical highest oxide
is N2O5 nitrogen(V) oxide (nitrogen
pentoxide) and does exist.
-
Reaction of
oxides with water:
-
Nitrogen(IV) oxide
dissolves to form an acidic solution of weak nitrous acid and
strong nitric acid.
-
NO and N2O are
neutral oxides but nitrogen(V) oxide is strongly acidic and
dissolves to form nitric acid.
-
Reaction of
oxides with acids:
-
Reaction of
oxides with bases/alkalis:
-
Nitrogen(IV) oxide
or nitrogen dioxide forms sodium nitrite and sodium nitrate with sodium
hydroxide solution.
-
2NO2(g) + 2NaOH(aq)
==> NaNO2(aq) + NaNO3(aq)
+ H2O(l)
-
ionic equation: 2NO2(g) + 2OH-(aq)
==> NO2-(aq) + NO3-(aq)
+ H2O(l)
-
As well as being a
neutralisation reaction, it is also a redox reaction, the oxidation
states of oxygen (-2) and hydrogen (+1) do not change BUT the
oxidation state of nitrogen changes from two at (+4) to one at (+3) and
one at (+5). The simultaneous change of an element into an lower and
upper oxidation sate is sometimes called disproportionation.
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 8 Oxygen O in Group 6/16
-
The structure of the
element:
-
Non-metal existing as
diatomic molecule, O2, with a double covalent
bond.
-
It has two
allotropes: 'normal oxygen' O2 (dioxygen above) and the
highly unstable and reactive gas ozone, O3 (trioxygen).
-
Physical properties
of the element:
-
Group, electron configuration
(and oxidation states):
-
Gp6; e.c. 2,6 or 1s22s22p4; Normally
(-2) e.g. H2O, CO2 etc. but can have
other ox. states ...
-
e.g. H2O2 (-1), F2O
(+2).
-
Reaction of element with oxygen:
-
Reaction of
oxide with water, acids
or bases/alkalis: Not applicable.
-
Reaction of element with chlorine:
-
Reaction of
chloride with water:
-
Reaction of element with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 9 Fluorine
F in Group 7/17 The Halogens
-
The structure of the
element:
-
Physical properties:
-
Group, electron
configuration (and oxidation states):
-
Gp7 Halogen; e.c. 2,7
or 1s22s22p5; (only
-1) e.g. HF, ClF, F2O (O is +2!)
-
An extremely
reactive element and readily combines with almost every other
element.
-
Reaction of element
with oxygen:
-
Reaction of
oxide with water:
-
Reaction of
oxide with acids:
-
Reaction of
oxide with bases/alkalis:
-
Reaction of element
with chlorine:
-
Can combine directly
or indirectly to form ClF, ClF3, ClF5 and
ClF7.
-
e.g. Cl2(g)
+ F2(g) ==> 2ClF(g)
-
Reaction of
chloride with water:
-
Reaction of element
with water:
-
Other comments:
-
Links to other pages
on site:
 Z = 10 Neon
Ne in Group 0/18 The Noble Gases
-
The
structure of the element:
-
Physical properties:
-
Group, electron configuration
(and oxidation states):
-
Reaction with anything:
-
Other comments:
-
Links to other pages
on site:
WHAT NEXT?
See also 5.1
Period 3 survey of elements,
5.2 Period 3 element trends
& explanations of physical properties,
5.3
Period 3 element trends in bonding, structure, oxidation
state, formulae & reactions, 6.1 Survey of
Period 4 elements, 6.2 Period 4 element trends in physical properties, 6.3
Period 4 element trends in bonding, formulae and
oxidation state and
6.4
Important element trends down a Group
INORGANIC Part 4
Period 2 survey sub-index : 4.1 Period 2 survey of the
individual elements : 3. lithium : 4. Beryllium
:
5. Boron :
6. Carbon : 7. Nitrogen
:
8. Oxygen :
9. Fluorine
:
10. Neon *
4.2 Period 2
element trends
& explanations of physical properties
*
4.3 Period 2
element trends
in bonding, structure, oxidation state, formulae & reactions
Advanced
Level Inorganic Chemistry Periodic Table Index *
Part 1
Periodic Table history
* Part 2
Electron configurations, spectroscopy,
hydrogen spectrum,
ionisation energies *
Part 3
Period 1 survey H to He *
Part 4
Period 2 survey Li to Ne * Part
5 Period 3 survey Na to Ar *
Part 6
Period 4 survey K to Kr and important trends
down a group *
Part 7
s-block Groups 1/2 Alkali Metals/Alkaline Earth Metals *
Part 8
p-block Groups 3/13 to 0/18 *
Part 9
Group 7/17 The Halogens *
Part 10
3d block elements & Transition Metal Series
*
Part 11
Group & Series data & periodicity plots
  
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Be(OH)2(s) + 2HCl(aq) 
N.
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