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Chemistry OCR B Alevel > Elements of Life > Flashcards

Elements of Life Flashcards

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1
Q

How did the structure of the atom develop over time?

A

First was plum pudding model

Disproved by Geiger marsden

Bohr model - protons, neutrons and electrons

Evidence for shells - ionisation enthalpies and spectra

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2
Q

What reaction conditions are needed for fusion reaction?

A

High temperature and pressure

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3
Q

How do covalent bonds work?

A

There is a balance between repulsive forces between the nuclei and there is attractive forces between the nuclei and electrons

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4
Q

What is the bond angle of a tetrahedral molecule?

A

109.5

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5
Q

What is the bond angle of a pyramidal molecule with a lone pair?

A

107

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6
Q

What is the bond angle of a bent molecule with two lone pairs?

A

104.5

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7
Q

How do giant ionic compounds work?

A

Overall attraction in a lattice made of attraction beteeen I one of different charge shd repulsion of ions of the same charge

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8
Q

Explain the Trend in meltibg points in period 2 and 3

A

In period 2 meltibg point increases until carbon/silicon (increased delocalised electrons in metallics structure) then drops suddenly and decreases as molecules have less atoms so weaker intermolecular bonds

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9
Q

Negative ions with -1 charge

A

Nitrate no3

Hydroxide

Hydrogencarbonate

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10
Q

Ions with -2 charge

A

Sulphate

Carbonate

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11
Q

Ions with + charge

A

Ammonium

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12
Q

Ions with +2 charge

A

Copper

Zinc

Iron (ii)

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13
Q

Ion with +3 charge

A

Iron 3

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14
Q

What happens and what is the trend when group 2 metals react with water?

A

Form metal hydroxides and hydrgen

Increasing reactivity down group as outer electrons are more easily lost

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15
Q

What hapens when group 2 metals react with oxygen?

A

For metal oxides

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16
Q

What is the trend in thermal stability of group 2 carbonates?

A

Increased stability down group

The ions have lower charge density so less distortion

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17
Q

What is the trend in solubility of group 2 hydroxides?

A

Increase in solubility down the group

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18
Q

What is the trend in solubility of group 2 carbonates?

A

Decreases down group

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19
Q

Define ionisation ebthalpy?

A

The entgalpy needed to remove the 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous ions

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20
Q

What is the trend in ionisation enthalpues and why?

A

Increase across the period
And decreases down group

Atomic radius decreases

Nuclear charge Increases

Electron shielding

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21
Q

Solubility of nitrates?

A

Soluble

22
Q

Sulfates are soluble except?

A

Barium

Calcium

Lead

23
Q

Solubility of carbonates?

A

Insoluble except lithium potassium sodium and ammonium

24
Q

Solubility of hydroxides?

A

Insoluble expect lithium sodium potassium strontium calcium barium and ammonium

25
Q

Test for calcium?

A

White precipitate with sodium hydroxide

26
Q

Test for copper?

A

Blue precipitate with sodium hydroxide

27
Q

Test for iron (ii)?

A

Green precipitate with sodium hydroxides

28
Q

Test for iron (iii)?

A

Brown precipitate with sodium hydroxide

29
Q

Test for aluminium?

A

White dissolvable precipitate with sodium hydroxide

30
Q

Test for carbonates?

A

HCl forms co2 so turns lime water cloudy

31
Q

Test for sulfates?

A

Barium chloride

Forms a white precipitate

32
Q

Test for ammonia

A

Litmus paper

Red- blue

33
Q

Test for halides?

A

Add silver nitrate

White

Cream

Yellow

34
Q

What happens when you add group 2 oxides and hydroxides to water?

A

They form alkaline solutions

Oxides form stronger alkalines down the group

35
Q

Group 2 hydroxides/oxides and acids?

A

Neutralisation

36
Q

What is the order of the electromagnetic spectrum?

A

Infrared visible ultraviolet

37
Q

What is the melting point, solubility in water and conductivity like for giant ionic?

A

High melting point

Most soluble except: ba, ca, pb ag sulphate
Ag+ pb halides
Carbonates
Hydroxides (except g1 and nh4)

Conduct when in solution of molten

38
Q

What is the melting point, solubility in water and conductivity of giant metallic structures?

A

High melting point

Insoluble in water, some react

Conductive when solid or liquid

39
Q

What is the melting point, solubility in water and conductivity I’d giant covalent ?

A

Very high melting point

Insoluble

Unconductive - except graphite

40
Q

What is the melting point, solubility in water and conductivity of simple covalent?

A

Low melting point

Insoluble unless the have polar group

Inconductive

41
Q

What is an acid?

A

Has the ability to transfer H+

42
Q

What is a base?

A

Has ability to accept H+ ions

43
Q

What is an alkali?

A

Base that dissolved in water to produce hydroxide ions

44
Q

What do solid and dashed wedges mean?

A

Solid wedges coming out of plane of paper, dashed are going behind

45
Q

Define activation energy

A

The minimum energy needed in a collision to cause a reaction

46
Q

What is meant by the term mole?

A

The amount of substance that has the same number of particles as there are atoms in 12g of carbon 12

47
Q

What is an salt?

A

A compound where a H+ in an acid has been replaced by a metal ion

48
Q

What is relative isotopic mass?

A

The mass of the atom compared to 1/12 th of the mass of carbon 12

49
Q

describe the appearance and origin of the emission spectrum of the sun and explain how the lines can be used to identify elements

A 
Appearance and origin
• atoms absorb energy
• electrons move up energy levels
• energy levels quantised
• (electrons) drop back down
• emit light
• ∆E = hv
• give coloured lines

How lines can be used
• atoms of each element have their own specific
energy levels
• thus different gaps
• thus different frequency lines
• frequencies of lines can be checked against a
database

50
Q

what is charge density?

A

the ratio of charge on an ion to its volume

Chemistry OCR B Alevel (14 decks)

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