Summary AQA A Level chemistry 3.2.2 Group 2 Alkaline Earth Metals
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Course
Unit 3.2.2 - Group 2, the alkaline earth metals
Institution
AQA
5 page document which follows the AQA specification closely with detailed notes and easy to understand language while still covering the key information you need to know about Group 2 alkaline Earth Metals. I talk about the physical properties (including trends in ionisation energies, atomic radius...
The periodic table elements according proton number
.
arranges to
·
·
All elements along a
period have the same number of electron shells
. All elements
down a
group
:
same no .
of outer electrons
.
Elements are classified
S-block groups 142 d-block transition metals
: :
into blocks that show
3 to 0 f-block :
radioactive elements
p-block groups
:
configuration
:
electron
Macromolecular
(giant covalent) atomic
-
giant metallic
metals
↑ semical
molscar ·
non-metals noble
group D
gas
-
S block P block
noble gas
havegiant P4
- One r
"C
C2
- unreactive
Na
Mg Al si p s Ar
metals , so : lose
electrons to
! --
form ionic
-- ↓
compounds has some
metallic
2
form ionic compounds or share
foure's in outer
properties either accept es to
shell : forms 4
their outer shell es to form covalent compounds.
covalent bonds
-
ATOMIC RADIUS
Along a period :
atomic radius decreases
. The increased nuclear charge (for
the same no of shells) increases the attraction from the nucleus and pulls
the outer shell electrons closer to the nucleus
.
NISATION
ENERGY
Along a
period
:
isnisation energy increases
. As the atomic radius decreases
and nuclear charge increases ,
the attraction between the nucleus outer
shell electrons increases and :· the electrons are held more strongly
. This
means that more energy is required to remove the outer electron & ionise
the atom
.
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