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A-level Chemistry Paper 1- Periodic Table and Energy > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

what is periodicity?

A

The repeating pattern of properties of elements across different periods in the periodic table

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2
Q

How are elements arranged in?

A

order of atomic number

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3
Q

How do the elements in period 2 resemble closely to the elements in period 3?

A

In terms of that repeating chemical behaviour and physical properties, the elements in groups have similar chemical properties

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4
Q

what do elements in the same period have?

A

A similar electron core

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5
Q

what is the first ionisation energy?

A

The energy required to move one mole of electrons from one mole of gasesous atoms

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6
Q

What is ionisation?

A

-The removal of an electron from an atom to make a positive ion

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7
Q

what happens when an electron is removed?

A

The atom has been ionised

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8
Q

what is generally called the ionisation energy?

A

Energy needed to remove electrons from the atom

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9
Q

Why is ionisation an endothermic process?

A

because energy is needed to overcome the electrostatic force of attraction between the negative electron and the positive nucleus

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10
Q

What are the factors influencing the magnitude of ionisation energy?
(attraction)

A

-nuclear charge
-distance of electrons from nucleus (atomic/ionic radius
-shielding effect

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11
Q

What does more protons mean for nuclear charge?

A

the greater the nuclear charge

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12
Q

when is nuclear attraction reduced?

A

With increasing distance (the further, the electron is from the nucleus the easier it is to remove)

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13
Q

How does the shielding affect work?

A

-inner the shell electrons repel outer of shell electrons
-this repelling effect, reduces the attraction experience by the outer electrons from the nucleus
-Electrons in inner shell shield outer electrons from the attractive force of the nucleus

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14
Q

what happens to ionisation across a period? (NcArss)

A

-nuclear charge in increases
-outer electron in the same sub shell (atomic radius decreases)
-shielding the same
-Nuclear attraction increases
-Therefore electron requires more energy to remove
-So ionisation energy increases across the period

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15
Q

What happens to ionisation energy down the group?

A

-nuclear charge increases (outweighed by changes in shielding and shells)
-outer electron in new shell (atomic radius increases)
-Shielding increase
-Nuclear attraction decreases
-therefore electron requires less energy to remove
-So ionisation energy decreases down a group

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16
Q

what does electron repulsion mean?

A

Electron is easier to remove

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17
Q

What can electronic configurations of elements be predicted from?

A

successive ionisation energies

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18
Q

what do successive ionisation energy provide?

A

Evidence for different energy levels

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19
Q

how many ionisation energies does an element have?

A

it has as many ionisation energies as it has electrons

20
Q

Why does the ionisation energy increase each time an electron is removed?

A

-as an electron is removed nuclear attraction increases as there are more protons than electrons (the proton:electron ratio increases)

21
Q

Why is the third ionisation energy much greater than the second in mg?

A

-there is a massive change because the third electron is removed from a lower shell

22
Q

why are the third to tenth successive ionisation energies of similar order (in magnesium)?

A

-this is because they are all removed from the same shell so similar amount of energy needed
-they all experience similar shielding from the nucleus

23
Q

why is there a large difference in value between the 10th and 11th ionisation energy? (in magnesium)

A

-because the 11th electron is on a different shell (removed from the fist main energy shell)

24
Q

what happens to metallic character as we go from left right?

A

It decreases

25
Q

What structure do all metals have?

A

giant metallic lattice structure

26
Q

What is the definition of metallic bond?

A

The strong electrostatic attraction between cations (positive ions) and delocalised electrons.

27
Q

what are the electrons in the outer shell of a metal?

A

-The electrons are delocalised to give positive metal centres (cations)

28
Q

what metal ions does Na form?

A

Na+

29
Q

what metal ions does mg form?

A

mg2+ ions

30
Q

what is the arrangement of a giant metallic lattice structure?

A

-fixed metal cations are surrounded by mobile, delocalised electrons

31
Q

What do the mobile delocalised electrons mean?

A

metals can conduct as both solids and liquids

32
Q

What do the strong metallic bonds in metals mean?

A

-High temperatures are needed to provide a large amount of energy needed to overcome the electrostatic attraction between the cations and electrons

33
Q

What do metals tend to have?

A

high melting and boiling points

34
Q

what are giant covalent lattices is held together?

A

The are held together by a network of strong covalent bonds

35
Q

what does strong covalent bonds need to overcome them?

A

A large amount of energy

36
Q

what do giant covalent materials have?

A

-High melting and boiling points

37
Q

why are covalent materials insoluble in most solvents?

A

-The covalent bonds are too strong to be broken by interactions with solvent molecules

38
Q

why can most covalent structures not conduct electricity?

A

all the outer shell electrons are involved in covalent bonding

39
Q

why can graphite and graphene conduct electricity?

A

They have mobile electrons

40
Q

What is the melting/boiling point of particular element dependent on?

A

The bonding present in the structure of the element

41
Q

Why do metals have high melting points?

A

Because they contain metallic bonding

42
Q

why do non-metals with giant covalent structures (like silicon) have high melting points?

A

they have high melting points because the covalent bonds are strong and require large amounts of energy to break

43
Q

why do simple covalent molecules (like phosphorus and chlorine) have low melting and boiling points?

A

-because they are held together by intermolecular forces, which are weaker and require less energy to overcome

44
Q

why do metals conduct electricity?

A

because their giant structures contain delocalised electrons which are mobile

45
Q

What does metallic character increase?

A

-Conductivity to a maximum in group 3

46
Q

when does metallic character increase?

A

Down the group

47
Q

why do elements be on the silicon show no conduction?

A

-all electrons are involved in bonding and are not mobile

A-level Chemistry Paper 1- Periodic Table and Energy (7 decks)

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