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A-Level Chemistry > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

What is the first ionisation energy?

A

The energy required to remove one mole of electrons from one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

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2
Q

What is the first ionisation of Mg?

A

Mg(g) ——> Mg+ (g) + e-

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3
Q

What is the second ionisation of Mg?

A

Mg+(g) ——> Mg2+ (g) + e-

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4
Q

What is shielding?

A

When inner electrons screen the outer electrons from the pull from the nucleus

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5
Q

What is nuclear charge?

A

The positive charge on the nucleus

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6
Q

What is atomic radius?

A

Radius of an atom. We measure atomic radius by measuring the distance between two nuclei of touching atoms and halving the distance

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7
Q

What happens to the shielding across period 3?

A

Stays the same

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8
Q

What happens to the nuclear charge across period 3?

A

Increases

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9
Q

What does a stronger nuclear charge mean?

A

The closer the electrons are pulled to the nucleus

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10
Q

What happens to the atomic radius across period 3 and why?

A

Decreases as electrons pulled closer to nucleus

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11
Q

What is the general trend of first ionisation energy across period 3?

A

Increases

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12
Q

Why does the first ionisation energy increase across period 3?

A

Nuclear charge increases
Attraction of electrons increase
Atomic radius decreases
Takes more energy to remove 1st e-

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13
Q

Why is there a dip in the trend between Mg and Al in period 3?

A

Mg has full sub shell stability (3s)
Al has one electron in higher sub shell
So easier to remove as further from nucleus
Al= lower 1st IE

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14
Q

Why is there a dip in the trend between P and S in period 3?

A 
P has half sub shell stability (3p)
S has 3p containing a pair of electrons
Pair of electrons repel each other 
So one of these electrons easier to remove 
S= lower 1st IE
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15
Q

What is the general trend of 1st IE down group 2?

A

Decreases

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16
Q

Why does the first ionisation energy decrease down group 2?

A

More inner shell electrons as you go down group
So shielding increases
Atomic radius increases so electrons further away
Nuclear attraction decreases
So easy to remove first electron

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17
Q

How do you draw metal diagram?

A

At least 6 cations
Sea of delocalised electrons
Cations in fixed position
Each cation has a positive charge

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18
Q

What are the properties of metals?

A 
Electrical conductivity
High melting + boiling point
Solubility
Good thermal conductor
Malleable
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19
Q

Why do metals conduct in solid and liquid?

A

Because delocalised electrons can move freely within the lattice

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20
Q

Why do metals have high melting + boiling point?

A

Strong electrostatic attraction between metal ion + delocalised electron
So needs lots of energy to break

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21
Q

Do metals dissolve in solvents?

A

NO

22
Q

Why are metals good thermal conductors?

A

Because when heated e- gain KE so move faster

Movement transfers gained energy throughout metal

23
Q

Why are metals malleable?

A

Because no bonding between ions therefore layers can slide

24
Q

What are alloys?

A

Mixture of two or more metals

25
Q

What do alloys do?

A

They dissort the layers so they can’t slide therefore making the metal harder

26
Q

What are the giant covalent structures?

A

Diamond
Graphite
Fullerenes
Graphene

27
Q

What is the structure of diamond?

A

Giant covalent
Lattice
Made of carbon
Each carbon is bonded to 4 other carbons

28
Q

What are the properties of diamond?

A

Hard - giant covalent structure + lots of strong bonds
Doesn’t conduct - no e-
High melting point - strong covalent bonds = needs lots of energy to break

29
Q

What is the structure of graphite?

A 
Made of carbon
Hexagonal structure
Strong covalent bonds
Parallel layers
Weak intermolecular forces between layers
Each carbon bonded to 3 carbons 
e-
30
Q

What are the properties of graphite?

A

Soft/slippery - layers slide as weak forces between
Conduct - e-
High melting point

31
Q

Why does graphite have a high melting point?

A

Giant structure with lots of strong covalent bonds between atoms so need lots of energy to break bonds

32
Q

What are fullerenes?

A

Cage like structures

33
Q

What are examples of fullerenes?

A

Nanotubes

Buckminster fullerenes

34
Q

What is an allotrope?

A

Different physical forms of an element

35
Q

What is the structure of graphene?

A

One layer of graphite
Sheet of carbons joined together in hexagons
One atom thick = 2D compound

36
Q

What are the properties of graphene?

A

Conducts - e-
Strong - delocalised electrons strengthen covalent bonds
Transparent + light - single layer

37
Q

What is graphene used in?

A

Touchscreens
High-speed electronics
Aircraft technology

38
Q

What is the general trend of melting point across period 3?

A

Increases to Si then decreases afterwards

39
Q

Why does the melting point increase (across period 3) from Na to Al?

A

Charge on metal ion increases
So no. of e- increases
So strength increases
So more energy needed to break bonds

40
Q

Why does Si have the highest melting point in period 3?

A

Have to break lots of covalent bonds
Requires lots of energy
Giant covalent structure

41
Q

Why does the melting point (after Si) decrease across period 3?

A

Non-metals
So exist as simple molecules with weak London forces between molecules
So need little energy to break

42
Q

Why does S have an elevated melting point in comparison to the other non-metals in period 3?

A

Has more electrons since it has more molecules
As exists as S8
So more London forces
So more energy needed to break bonds

43
Q

What does P exist as?

A

P4

44
Q

What does S exist as?

A

S8

45
Q

What does Cl exist as?

A

Cl2

46
Q

What does Ar exist as?

A

Ar since it is monoatomic

47
Q

Why is diamond a poor electrical conductor?

A

Outer electrons are in localised covalent bonds

48
Q

Why is graphene a better conductor than graphite?

A

No layers to slow down electrons

49
Q

From a successive ionisation energies graph how can you work out which group it is from?

A

Count how many electrons are removed before the first big jump

50
Q

From a successive ionisation energies graph how can you work out the electronic structure of the element?

A

Working from right to left count how many points there are before each jump to find out how many electrons there is in each shell

A-Level Chemistry (26 decks)

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