Trends in the periodic table

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Covalent Radius
a measure of the size of atom, half the distance between the nuclei of two covalently bonded atoms
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Going across a period, covalent radius....
decreases
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Going down a period, covalent radius....
increases
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covalent radius, decreases Going across a period because of
increasing nuclear charge
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covalent radius, increases Going down a period because of
the number of filled electron shells increase, (shielding effect)
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electronegativity
is a measure of attraction for electrons in a covalent bond
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the higher the electronegativity
the stronger attraction for the electrons
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Going down a period, electronegativity....
decreases
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Going across a period, electronegativity....
increases
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electronegativity,decreases Going down a period because of
the number of filled electron shells increase, screening effect which means that electrons are less strongly attracted to the atom
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electronegativity,increases Going across a period because of
increase in nuclear charge causes the atom to attract to bonded electrons more strongly
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ionisation energy
the energy required to move one mole of electrons from one mole of gaseous atoms
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going down a group, ionisation energy ..
decreases
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going across a group, ionisation energy ..
increases
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going down a group, ionisation energy decreases because..
an electron is being removed from the layer of electrons which is furthest from the nucleus
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going across a group, ionisation energy increases because..
the nuclear charge is increasing, the outermost electrons are therefore more strongly held .
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Other cards in this set

Card 2

Front

decreases

Back

Going across a period, covalent radius....

Card 3

Front

increases

Back

Preview of the back of card 3

Card 4

Front

increasing nuclear charge

Back

Preview of the back of card 4

Card 5

Front

the number of filled electron shells increase, (shielding effect)

Back

Preview of the back of card 5
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