Structure 3.1
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Period
Rows across Ptable
Group
Columns on Ptable
What does the period number show
The outer energy level that is occupied by electrons
What do elements in a group have in common?
Their valence electrons, this gives similar chemical properties
Periodicity
Trends in properties of elements across a period and down a group
Trends in properties down a group
Increasing metallic character (G1 elements) decreasing non metallic character (G17 elements)
Oxidation state
A number assigned to an atom to show the number of electrons transferred in forming a bond. The charge that atom would have if it was composed of ions.
Group 1 name
Alkali metals
Group 2 name
Alkali earth metals
Group 17 name
Halogens
Group 18 name
Noble gases
What groups are associated with the s sub-level?
Groups 1 and 2
What groups are associated with the p sub-level?
Groups 13-18
What groups are associated with the d sub-level?
Groups 3-12 (transition metals)
What part of the ptable is the f sub-level associated with?
Lanthanoids and actinoids (2 rows at the bottom)
Metalloids
Under boron and then staircase shape down to Polonium
Atomic radius (r)
Half the distance between neighbouring nuclei. Can be considered as the distance from the nucleus to the outermost electron.
Atomic radius trends across the periods of the ptable.
As the nuclear charge inc so does the electrostatic attraction between the nucleus and the outer electrons resulting in a dec in the atomic radius across a period. Electrons are also being added to the same shell.
Atomic radius trends down the groups of the ptable.
The number of occupied electron levels inc down a group so the atomic radius also increases. Inner shells of electrons also provide additional shielding.
Nuclear charge
Number of protons
Positive ionic radii
Smaller than the atom they are derived from as they have less electrons
Isoelectronic positive ionic radii
Dec in size across a period as the number of electrons remains constant but the nuclear charge inc (electrons are pulled closer to nucleus)
Negative ionic radii
Larger than their parent atom as they have the same number of protons but more electrons.
Isoelectronic negative ionic radii
Decrease in size across a period as the number of electrons is constant but the nuclear charge inc (electrons are pulled closer to the nucleus)