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LC Chemistry > Trends > Flashcards

Trends Flashcards

1
Q

Atomic radius of an atom

A

Half the distance between the nuclei of 2 atoms of the same element that are joined together by a single covalent bond

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2
Q

First ionisation energy

A

Minimum energy required to completely remove the most loosely bound e from a neutral atom in its ground state
Eg NA(g) ->NA+(g) + e

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3
Q

Second ionisation energy

A

Energy required to completely remove an electron from an ion with 1 positive charge in the gaseous state
Eg Ca+ -> Ca+2 (g) + e

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4
Q

Exceptions of first ionisation energy

A

Any sub level that is completely or half filled has extra stability therefore it is harder to remove the electrons leading to a higher ionisation energy

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5
Q

Explain why x has a higher ionisation energy than y

A

Write e configuration of both
Compare e configuration
sublevels that are half filled or full have more stability

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6
Q

Why is second ionisation energy always bigger than the first

A

The e is removed from a positively charged ion
There is a greater attraction between the nucleus and the e being removed
thus more energy is require to move the e-

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7
Q

How does atomic radius differ down a group

A

Increases

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8
Q

Why does atomic radius increase down a group

A

Electrons are going into a new energy level
Increased shielding effect by inner e

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9
Q

How does atomic radius differ across a period

A

Decreases

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10
Q

Why does atomic radius decrease across a period

A

Increase in effective nuclear charge
No increase in shielding

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11
Q

How does first ionisation energy differ down a group

A

Decreases

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12
Q

Why does first ionisation energy decrease down a group

A

Increasing atomic radius
Increased shielding by inner electrons

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13
Q

How does first ionisation energy differ across a period

A

Increases

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14
Q

Why does first ionisation energy increase across a period

A

Increasing effective nuclear charge
Decreasing atomic radius

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15
Q

How does electronegativity differ down a group

A

Decreases

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16
Q

Why does electronegativity decrease down a group

A

Increasing atomic radius
Increased shielding by inner electrons

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17
Q

Why does electronegativity increase across a period

A

Increasing effective nuclear charge
Decreasing atomic radius

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18
Q

How does electronegativity differ across a period

A

Increases

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19
Q

why does x have an exceptionally high first ionisation energy?

A

write e- configuration

sublevels that are half full or full have extra stability
this makes it much harder to remove the most loosely bound e- and it requires much more energy

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20
Q

how do group 1 elements react?

A

by donating 1 e-

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21
Q

how do group 2 elements react

A

by donating 2 e-

22
Q

how does reactivity differ down group 1 and 2

A

it increases

23
Q

is it easier to remove e- when an element is more or less reactive

A

more

24
Q

why does reactivity increase down group 1 of the periodic table

A

increasing atomic radius
increased shielding by inner e-

25
Q

what is produced when a group 1 reacts with O2

A

a metal oxide

26
Q

write the balanced equation of a metal oxide reaction in group 1

A

2(metal) + 1/2 O2 ——->metal2O

27
Q

write the balanced equation of a metal hydroxide reaction in group 1

A

metal + H20 —->(metal)OH + 1/2 H2

28
Q

why are group 1 metals stored in oil

A

to prevent the metals from reacting with oxygen in the air

29
Q

what is formed when a group 1 reacts with water

A

metal hydroxides

30
Q

how do group ones react with water

A

vigorously/ violently
the metal floats on the surface of water
lots of fizzing is observed as H2 gas is produced

as the reactivity increases down the group, potassium is so reactive the hydrogen gas actually ignites and a lilac flame is observed

31
Q

what is formed when group one metals react with HCL

A

metal chloride salt and h gas

32
Q

write the balanced equation of a HCL reaction with group 1

A

metal + HCl –> metalCl + 1/2 H2

33
Q

how does a group 1 react with HCl

A

explosively

34
Q

which group are the most electronegative on the periodic table

A

halogens (group 7/17)

35
Q

how do group 7 react

A

by accepting 1 e- to have a stable outer octet

36
Q

what happens to reactivity down group 7

A

decreases

37
Q

why does reactivity decrease down group 7

A

decreasing electronegativity
increasing atomic radius

38
Q

what is used to show that reactivity decreases down group 7

A

displacement reactions

39
Q

what does displacement mean

A

element is replaced with a more reactive element

40
Q

what is the only element in group 7 that will displace everything in the group and why

A

flourine
has the highest electronegativity value

41
Q

describe the experiment carried out to show that reactivity decreases down group 7

A

bubble chlorine gas through a solution that contains bromide ions. (BrCl)
the Cl is more reactive and takes 1e- from the Br- ion forming a Br atom
2 Br atoms join to form Br2
this is visualised from a colour change of colourless to red

42
Q

what is the colour change shown in the experiment carried out to show that reactivity decreases down group 7

A

colourless to red

43
Q

does boiling point increase or decrease down group 7?

A

increases

44
Q

why does does boiling point increase down group 7

A

as you go down the electron cloud gets larger
thus the van der waals interactions between halogen molecules get stronger
and more energy is needed to overcome the force of attraction

45
Q

what is the appearance of flourine at room temp

A

pale yellow gas

46
Q

what is the appearance of chlorine at room temp

A

greenish-yellow gas

47
Q

what is the appearance of bromine at room temp

A

red-brown liquid

48
Q

what is the appearance of iodine at room temp

A

grey solid

49
Q

what is the balanced equation of the displacement reaction that is carried out to show that reactivity decreases down group 7

A

Cl2 + 2NaBr –> 2NaCl + Br2

50
Q

what is the balanced equation that shows the colour change of the displacement reaction that is carried out to show that reactivity decreases down group 7

A

Cl2 + 2e- –> 2Cl-
2Br- —-> Br2 + 2e-

LC Chemistry (21 decks)

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