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Chemistry > Periodic Table > Flashcards

Periodic Table Flashcards

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0
Q

Periodicity

A

Number of shells

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1
Q

Group

A

Outer shell electron

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2
Q

Group 1 name

A

Alkali metals

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3
Q

Group 2 name

A

Alkali earth metals

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4
Q

Group 7

A

Halogens

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5
Q

Group 8 other name

A

Noble gasses

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6
Q

5 metal properties

A 
Conducts electricity
Metal oxides are bases
Shiny
High mp/bp
Malleable
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7
Q

5 non-metal properties

A 
Don't conduct electricity 
Non-metal oxides are acidic
Dull
Low mp/bp
Not malleable
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8
Q

3 properties of noble gases

A

Inert
Colourless
Monatomic gases

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9
Q

Uses of Nobel gases

A

Helium used in balloons as denser than air
Neon used in advertising signs as glows when electricity is passed through it
Argon used in builds as very unreactive even at high temp so won’t react with the thin metal filament like O2 would
Krypton used in lasers

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10
Q

Properties of alkali metals (6)

A 
Shiny
Conduct electricity
Soft
Low mp/bp
Low density
React with water
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11
Q

Lithium + water = (and observations)

A

Lithium hydroxide + hydrogen

Float, move, fizz

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12
Q

Sodium + water = (and observations)

A

Sodium hydroxide + hydrogen

Float, move, fizz, melt

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13
Q

Potassium + water = (and observations)

A

Potassium hydroxide + hydrogen

Float, move, lilac flame, violent reaction, fizz

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14
Q

Water + alkali metals turns universal indicator…

A

Purple (alkali)

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15
Q

Rubidium + water = (and observations)

A

Rubidium hydroxide + hydrogen
Sinks as denser than water
Immediately reacts with a violent exposition

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16
Q

Caesium + water = (and observations)

A

Caesium hydroxide + hydrogen

Explodes shattering container

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17
Q

Ions group 1 forms

A

1+

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18
Q

Explaining trend in group 1 reactivity

A

Reactivity increases as you go down the group
As you go down the group:
Number of shells increase
Outer electrons further from nucleus
Less strongly attracted
Therefore atom can give up its electrons more easily

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19
Q

What happens to melting point as you go down group 1

A

Melting point decreases

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20
Q

Fluorine state, colour, use

A

Gas
Colourless / pale yellow
F– used in toothpaste

21
Q

Chlorine state, colour, use

A

Gas, pale green, disinfectant

22
Q

Bromine state, colour, use

A

Liquid, red/brown, water purification

23
Q

Iodine state, colour, use

A

Solid, silver/black, anti-septic

24
Q

Astatine state, colour, use

A

Solid, black, radioactive isotope

25
Q

Halogen ending, halide ending

A

ine, ide

26
Q

Chlorine water aqueous layer

A

Colourless

27
Q

Bromine water aqueous layer

A

Orange

28
Q

Iodine water colour of aqueous layer

A

Red/brown

29
Q

Explaining reactivity in group 7

A

Reactivity decreases as you go down the group
As you go down the group:
Number of shells increase
Outer shell electrons further from nucleus
This means they are less strongly attracted to the nucleus
Therefore it is more difficult to attract the extra electron into its outer shell

30
Q

As you go down group 7

A

Mp increases

Density increases

31
Q

How to determine percentage of oxygen in air

A

Passing air in syringe over hot copper turnings

Starting volume - final volume
———————————– x 100
Starting volume

32
Q

Making and collecting oxygen

A

Hydrogen peroxide—————-> water + oxygen
Catalyst

H2O2.

33
Q

Catalyst in making oxygen

A

Manganese 4 oxide

34
Q

Percentage of nitrogen in air

A

78%

35
Q

Percentage of oxygen in air

A

21%

36
Q

Percentage of argon in air

A

Almost 1%

37
Q

Percentage of carbon dioxide in air

A

0.04%

38
Q

Magnesium burnt in oxygen

A

Bright white light
White solid
pH 10

39
Q

Carbon burnt in oxygen

A

Orange flame and sparks
Colourless gas
pH5

40
Q

Soulful burnt in oxygen

A

Melted then burned with a blue flame
Colourless gas
pH1

41
Q

Metal oxides are…

A

Bases

42
Q

Non-metal oxides are…

A

Acids

43
Q

Preparation of carbon dioxide

A

Metal carbonate + acid

CaCO3 + HCl —> CO2 + H2O + CaCl2

44
Q

How to collect CO2

A

Over water

45
Q

Uses of CO2

A

Fizzy drinks

Fire extinguisher

46
Q

Use of oxygen

A

O2 cylinders

47
Q

Preparation of hydrogen

A

Metal + acid

Mg + 2HCl —> MgCl2 + H2

48
Q

Uses of hydrogen

A

Balloons

Fuel

49
Q

Metal acid——>

A

Metal salt + hydrogen

50
Q

Rust equation

A

Fe2O3•XH2O

51
Q

3 ways to prevent rusting

A

Barrier method
Alloying
Sacrificial protection with a more reactive metal

Chemistry (23 decks)

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