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A - Level Chemistry > Paper 1 > Flashcards

Paper 1 Flashcards

1
Q

Trend in BP down halogens

A

More electrons

Strong LFs

More energy to break IMFs

BP increase

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2
Q

Define 1st ionisation energy

A

Renege required to remove 1 electron form each atom in 1 mol of gaseous atoms of an element to form 1 mole of gaseous 1+ ions.

E.g. Na(g) —> Na+ (g) + e^-

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3
Q

Define periodicity

A

Repeating trend in properties of elements across each period of periodic table

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4
Q

Strongest IMFs

A

LFs —> permanent dipole-dipole —> HBs
—increase in strength—>

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5
Q

How LFs brought about

A

Movement of electrons produce changing dipole

Instantaneous dipole will exist

And induce a dipole on neighbouring molecule

Which further induces dipole on neighbouring molecules and attract 1 another

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6
Q

Acid + metal carbonate

A

Salt + H2O + CO2

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7
Q

Acid + alkali

A

Salt + H2O

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8
Q

Acid + metal oxide/hydroxide

A

Salt + H2O

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9
Q

Ideal gas assumptions

A

No IMFs

Random motion

Elastic collisions

Negligible size

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10
Q

Hydrated salts assumptions

A

All H2O lost - heat to constant mass

No further decomposition

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11
Q

Define hydrated and water of crystallisation

A

H2O molecules are apart of crystalline structure

This water is known as water of crystallisation

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12
Q

Define relative atomic mass

A

Weighted mean mass of an atom of an element relative to 1/12th of mass of an atom of C-12

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13
Q

Define relative isotopic mass

A

Mass of isotope relative to 1/12th of mass of atom of C-12

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14
Q

Define isotope

A

Atoms of same element with different numbers of neutrons and different masses

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15
Q

Shape of p-orbitals

A

Dumb bell

Hold up to 1 or 2 electrons

3 p-orbitals

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16
Q

S-orbital

A

Sphere

Hold 1/2 electrons

17
Q

She’ll number and electrons formula

A

n = shell number

2n^2

18
Q

Define atomic orbital

A

Region around nucelus that can hold up to 2 electrons with OPP spins

19
Q

Acid + metal

A

Salt + hydrogen

20
Q

Define metallic bond

A

Strong electrostatic attraction between positive ions and delocalised electrons

21
Q

Metallic bond properties

A

High electrical conductivity - delocalised electrons carry charge

High MP + BP - strong MB—> strong attraction

Giant metallic lattice

Don’t dissolve

22
Q

Graphene and graphite

A
  • 3 of 4 outer shell e-s used in CB
  • remaining e- released into pool of delocalised e-s shred by all atoms in the structure
    • good electrical conductors
  • giant covalent structures of C
  • planar hexagonal layers
  • bond angle = 120* by electron-pair repulsion

graphene =

  • single layer of graphite
  • hexagonally arranged C atoms linked by strong CBs

graphite =
- parallel layers of hexagonally arranged C atoms
- layers bonded by weak LFs
- 3 of 4 outer shell e-s used in CB
- remaining e- released into pool of delocalised e-s shred by all atoms in the structure

23
Q

what is the bond angle and structure of (carbon) Diamond?

A

tetrahedral arrangement - bond angle = 109.5* because of electron pair repulsion

24
Q

why can’t silicon and carbon (diamond) conduct electricity?

A

in both structures, all 4 outer shell electrons are involved in CB, so none are available for conducting electricity.

25
Q

C & Si

A

group 14 (4) - 4 electrons in their outer shell C (in diamond form) and Si use these 4 electrons to form CBs to other C/Si atoms

26
Q

what is the structure and bonding of B, C and Si?

A

Giant covalent lattice - many billions of atoms are held together by a network of strong covalent bonds

27
Q

Define 2nd ionisation energy

A

He+ (g) —> He2+(g) + e-

Energy required to remove 1 electron from each ion in 1 mol of gaseous 1+ ions of an element to form 1 mole of gaseous 2+ ions.

28
Q

2nd ionisation energy explanation

A

After 1st electron lost, electron pulled closer to nucleus

Nuclear attraction increases + more IE needed to remove 2nd electron

29
Q

Trend in IE down group

A

Atomic radius increases

More inner shell - increased shielding

Nuclear attraction on outer electrons decreases

1st IE decreases

30
Q

Trend in IE across period

A

Nuclear charge increases

Same shell - similar shielding

Nuclear attraction increases

Atomic radius decreases

1st IE increases

31
Q

Trend in reactivity of halogens

A

Atomic radius increases
More inner shells so shielding increases
Less nuclear attraction to capture an electron from another species
Reactivity decreases

32
Q

Disproportionation reaction

A

Redox reaction in which same element is reduced and oxidised

33
Q

Enthalpy change of formation

A

is the enthalpy change that takes place when one mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states.

34
Q

Enthalpy change of combustion

A

enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, with all reactants and products in their standard states.

35
Q

Enthalpy change of neutralisation

A

is the energy change that accompanies the reaction of an acid by a base to
form one mole of H.O(). under standard conditions, with all reactants and products in their standard states.

36
Q

Buffer solution

A

Mixture of weak acid and its conjugate base which minimises changes in pH when small quantities of acid or alkali are added.

37
Q

Define conjugate acid-base pair

A

Contains 2 species that can be interconverted by the transfer of a proton

38
Q

Define a salt

A

The product of a reaction in which the H+ ions from the acid are replaced by metal or ammonium ions.

A - Level Chemistry (11 decks)

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