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Chemistry M3 > Section 1 > Flashcards

Section 1 Flashcards

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1
Q

First ionisation energy

A

energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms

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2
Q

The lower the ionisation energy the ____

A

easier to form an ion

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3
Q

Ionisation energy

nuclear charge

A

The more protons in the nucleus, the more positive charge there is and the stronger the attraction for the electrons

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4
Q

Ionisation energy

Atomic radius

A

An electron closer will be more strongly attracted

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5
Q

Ionisation energy

shielding

A

The more shielding, the less attraction between outer shell electrons and nucleus

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6
Q

Ionisation energy down the group trend

A

gets smaller because as you go down there are more shells that increases atomic radius and increases shielding

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7
Q

Ionisation energy across a period

A

get larger because there are more protons, higher nuclear charge and small radius

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8
Q

Ionisation energy across period

sometimes vary why?

A

due to electrons being in different types of orbitals

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9
Q

Second ionisation energy

A

energy needed to remove 1 electron from each ion in 1 mole of gaseous +1 ions to form 1 mole of gaseous 2+ ions

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10
Q

graphite structure

A

flat hexagons covalently bonded with three bonds

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11
Q

Graphite structure properties

A

weak forces between layers - sheets can slide
delocalised electrons allow current to flow
insoluble in any solvent - bonds to hard to break
high melting point
low density

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12
Q

diamond properties due to structure

A

high melting point
very hard
wont dissolve in solvent
cant conduct electricity

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13
Q

graphene properties

A

very strong
conducts electricity
transparent and light

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14
Q

metallic bonding

mp and bp

A

the more electrons the stronger the bonds so the higher the mp and bp

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15
Q

metallic bonding

ability to be shaped

A

no ions holding bonds together so ions can slide over each other

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16
Q

metallic bonding

conductivity

A

good thermal conductors

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17
Q

metallic bonding

solubility

A

insoluble because

18
Q

metals across a period

A

bp and mp increase across period because ions have greater charge
increasing number of delocalised electrons
higher charge density

19
Q

simple molecular structures

mp and bp

A

weak induced dipole-dipole forces

20
Q

Group 2

As you go down group 2 __________- decreases and ___________ increases

A

ionisation energy

reactivity

21
Q

Group 2

reaction with water

A

metal hydroxide and hydrogen

22
Q

Group 2

Be reaction with water

A

doesn’t react

23
Q

Group 2

reaction with oxygen

A

solid white oxides

24
Q

Group 2

oxide exception

A

Magnesium
slow reaction - hydroxide insoluble
hydroxides are more soluble down the group so solution gets more alkali

25
Q

Group 2

reaction with dilute acid

A

Hydrogen and metal acid thing

26
Q

Group 2

uses

A

calcium hydroxide to neutralise soil

magnesium hydroxide to neutralise stomach acid

27
Q

`Group 7

F

A

pale yellow

gas

28
Q

Group 7

Cl

A

green

gas

29
Q

Group 7

Br

A

red brown liquid

30
Q

Group 7

I

A

grey

solid

31
Q

Group 7

bp and mp down grouo

A

increase due to stronger induced dipole-dipole as number of electrons increases

32
Q

Group 7

down the group the halogens become less ___

A

oxidising

33
Q

Group 7

iodine water colour

A

brown

34
Q

Disproportionation

A

when a single element is simultaneously oxidised and reduced

35
Q

Disproportionation

making bleach

A

2NaOH + Cl2 -> NaClO + NaCl +H2O

36
Q

Disproportionation

mixing chlorine and water

A

Cl2 + H2O HCl + HClO

chloric acid

37
Q

Disproportionation

chloric acid making chlorate ions

A

HClO + H2O ClO- + H3O+

38
Q

Disproportionation

chlorine alternative

A

Ozone kills bacteria - expensive
UV kills bacteria but inaffective in cloudy water

doesn’t prevent contamination further down the line

39
Q

Tests

suphate

A

barium nitrate solution

white precipitate

40
Q

Tests

halides

A

add nitric acid and silver nitrate solution
c
b
i

41
Q

Tests for ammonia

A

add NaOH
heat
damp litmus paper blue

Chemistry M3 (3 decks)

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