periodic trends Flashcards

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1
Q

atomic radius

A

distance of an atom from its nucleus to the outermost electron

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2
Q

atomic radius across a period

A

From left to right across a period the net attraction force of the nucleus to each electron increases as the number of protons in the nucleus increases.

a greater force of attraction means a smaller distance between the nucleus and valance electrons and a smaller atomic radius.

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3
Q

atomic radius down a group

A

from top to bottom down a group the number of energy levels increases.
more energy levels result in a larger atomic radius

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4
Q

ionisation energy

A

amount of energy required to remove one electron from a single atom in the gaseous phase

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5
Q

ionisation proportionality

A

inversely proportional to atomic radius

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6
Q

ionisation energy across a period

A

from left to right across a period the net. attraction force of the nucleus to each electron increases as the number of protons in the nucleus increases.
A strong force of attraction means a smaller distance between the nucleus + valence electron and a smaller atomic radius.
A strong force of attraction means that more energy is required to overcome force to remove one electron

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7
Q

ionisation energy down a group

A

from top to bottom down a group the number of energy levels increases (increasing atomic radius).
valence electrons are increasingly shielded from the positive nucleus by core electrons .
This results in a weaker force of attraction on each electron means that less energy is required to overcome
a weak force of attraction means that less energy is required to overcome forces to remove electrons

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8
Q

electron affinity

A

the amount of energy liberated when an electron is added to a single atom in the gaseous phase

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9
Q

electron affinity across a period

A

from left to right across a period the number of protons in the nucleus increases.
The attraction for an electron increases.
More energy is released when an electron is added

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10
Q

electron affinity down a group

A

from top to bottom down a group the number of energy levels increases (increasing atomic radius).
More energy levels means more electron shielding of positive nucleus .
The attraction for an electron decreases .
Less energy is released when an electron is added

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11
Q

electronegativity

A

the ability of an atom to attract bonding pairs of electrons

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12
Q

density

A

mass per unit volume
mass/volume
non metals are less dense than metals

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13
Q

density across a period

A

from left to right across a group density increases
atomic radius decreases
atomic mass increases

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14
Q

density down a group

A

from top to bottom down a group density increases
atomic radius increases
atomic mass increases substantially

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15
Q

melting point

A

the temperature at which a solid changes phase to a liquid

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16
Q

boiling point

A

the temperature at which a liquid changes phase to a gas

17
Q

melting and boiling point trends

A

metals group 1-14 (left to right) increases
non metals group 15-18(left to right) very low
metals group 1 +2 (top to bottom) decreases
non metals group 17+18 (top to bottom) increases

18
Q

properties of group 1

A

alkali metals
most reactive - have single valance e- which is easily lost
found in compounds
soft and light grey
react w cold water

19
Q

properties of group 2

A

alkaline earth metals
reactive - 2 valance e-
react w cold water,light grey,soft,good conductors (except Be)

20
Q

properties of group 17

A

halogens
very reactive
form salts
7 valence e-
found in compounds
low melting points

21
Q

properties of group 18

A

nobles gases
unreactive
gases at room temperature