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1.3

periodicity

TermDefinition
all active metals groups 1 and 2
groups 3-6 become more metallic as you go down the group
active non-metals group 7
group 8 noble gases/gases at room temperature
decreases across the table activity of metals and electrical conductivity
melting and boiling points increase to peak at group 4 then decrease
metals tend to be solid at room temp (execpt mercury and bromine)
non-metals tend to be gases or soft solids at room temp
carbon highest melting point of all elements
electronegativity ability of an element to attract electrons from another atom and form a bond
pauling scale used to measure electronegativity (ranges from 0.7-4.0)
non-metals metals ___ are more electronegative than ___
down a group electronegativity decreases
valence electrons are further away from the nucleus why electronegativity decreases down a group
across a period electronegativity increases
because atomic radius decreases across the period so valence shell is closer to nucleus why electronegativity increases across a period
atomic radius the radius size of an atom
across a period atomic radius decreases
more protons in nucleus so stronger attraction which makes it smaller why atomic radius decreases across a period
down a group atomic radius increases
a shell is added each period why atomic radius increases down a group
first ionisation energy the energy required for an atom to lose an electron (measured in kJ/mol)
down a group first ionisation energy decreases
valence electrons are further from nucleus so attraction is weaker why first ionisation energy decreases down a group
across a period first ionisation energy increases
more protons so attraction is stronger why first ionisation energy increases across a period
Created by: hoeshi
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