Summary notes for CIE IGCSE Biology Topic 9: The Periodic Table
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Course
Chemistry
Institution
GCSE
Complete revision notes for Topic 9 of the CIE IGCSE Chemistry course: The Periodic Table. Explanations with diagrams for every specification point. These notes are written for candidates taking the Extended paper.
Describe the Periodic Table as a method of classifying elements and its use to predict
properties of elements
Elements are arranged on the periodic table in order of increasing atomic number, where
each element has one proton more than the element preceding it.
Groups
Vertical columns
Shows the number of valence electrons an element has
Periods
Horizontal rows
Shows the number of electron shells that an element has
Only hydrogen and helium are in period 1
Because there are patterns in the way the elements are arranged on the periodic table,
there are also patterns and trends in the chemical behaviour of the elements
Example: reactivity of alkali metals + water
In this way the periodic table can be used to predict how a particular element will behave.
9.2 Periodic trends
The metallic character of an element is determined by its tendency to lose its valence
electrons (more metallic) as opposed to filling the remaining gaps in its valence shell (more
non-metallic).
, Describe the change from metallic to non-metallic character across a period
The metallic character of the elements decreases along a period.
There is a middle section of the periodic table where elements display properties of both
metals and non-metals. These are referred to as metalloids or semi-metals.
Describe and explain the relationship between group number, number of outer-shell
electrons and metallic/non-metallic character
The metallic character of the elements increases down a group.
Property Metals Non-metals
Electron arrangement 1-3 valence electrons 4-7 valence electrons
(although more in periods 5
and 6)
Bonding Metallic (loss of valence Covalent (sharing of valence
electrons) electrons)
Electrical conductivity Good conductors Poor conductors
Type of oxide Basic (a few are amphoteric) Acidic (a few are neutral)
Reaction with acids Many react with acids Do not react with acids
Physical characteristics Malleable Brittle
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