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Chemistry Stuff Flashcards

0
Q

Displacement of metals from their salts

A

Any metal will displace another below it in the reactivity series from a solution of one of its salts

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1
Q

Hydrogen displacement

A

Can be displaced from an aqueous solutions
The solution is an acid

Metals above hydrogen in the reactivity series can displace hydrogen gas from dilute hydrochloric/ sulfuric acid

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2
Q

Salts of metals

A

Chlorides, nitrates, sulfates

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3
Q

Chlorides

A

Soluble on waer except silver chloride and led (iii) chloride

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4
Q

Nitrates

A

Soluble in water

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5
Q

Sulfates

A

Soluble in water

except barium sulfate, calcium sulfate and lead (ii) sulfate

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6
Q

Reduction

A

Oxygen removed from a metal oxide

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7
Q

Reducing agent

A

A substance that carries out the reduction

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8
Q

Reduction of a metal oxide

A

Heating the metal oxide with a more reactive metal

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9
Q

Carbon in reduction

A

Can reduce some metal oxides into metals

Carbon becomes carbon dioxide

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10
Q

Combustion of hydrogen

A

Hydrogen burns when heated in air or oxygen

Forms water

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11
Q

Test for hydrogen

A

Put a lighted splint at the mouth of a test tube, a squeaky pop will be heard if hydrogen is present

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12
Q

Test for water

A

Add the liquid to anhydrous copper (ii) sulfate
The white powder will turn blue if pure water is present
Copper (ii) sulfate formed

Boils at 100C freezes at 0C

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13
Q

Sacrificial protection of iron

A

Zinc is more reactive than iron

Even if the iron is scratched the iron is still protected because the zinc reacted and corrodes instead of the iron.

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14
Q

Galvanised iron

A

Iron coated in zinc

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15
Q

Preventing steel and iron rusting

A

Can be prevented by preventing contact with water and oxygen

Can be done by orating in: grease, oil, paint, plastic, a less reactive metal

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16
Q

Problems of coating to prevent rusting

A

Once the coating is scratched/washed away the iron is once again exposed to water and oxygen and will rust

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17
Q

Rusting of iron

A

Iron+ water+ oxygen

Iron —> iron (iii) due to loss of electrons

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18
Q

Speeding up rusting

A

By having electrolytes in the water

19
Q

More reactive the hydrogen metals

A

React with both: dilute hydrochloric acid and dilute sulfuric acid
Form a salt and hydrogen

20
Q

magnesium+ HCl / H2SO4

A

Bubbles
Disappears
Mixture gets hot
Colourless solution formed

21
Q

Aluminium+ HCl / H2SO4

A

Bubbles when heated
Disappears
Colourless
Solution formed

22
Q

Zinc+ HCl / H2SO4

A

Bubbles
Disappears
Colourless solution formed

23
Q

Iron+ HCl / H2SO4

A

Bubbles
Disappears
Pale green solution formed

24
Q

Presence of carbon dioxide

A

Limewater turns milky

25
Q

Carbon dioxide absorbs

26
Q

Acid rain

A

Rain with a below 6 PH
leaches vital vitamin out of the soil- kills trees
Lowers the PH of lakes so that fish can’t live in it
Weathers building made of; limestone, marble, iron

27
Q

Laboratory preparation of carbon dioxide

A

Metal carbonate + an acid = carbon dioxide

Calcium carbonate most often used

28
Q

Laboratory preparation of oxygen

A

Hydrogen peroxide decomposes slowly and forms water and oxygen

Decomposition sped up by adding the catalyst solid manganese dioxide

29
Q

Finding oxygen using iron

A

Place wet iron fillings at the end of a burette
Water rises up the burette
Due to iron reacting with air

Percentage of oxygen =
( volume of oxygen used/volume of air at start ) x 100

30
Q

Finding oxygen - copper

A

Aparratus with 100cm^3 of air
Heat copper at one end of the silica tube
Pass air over the copper
Keep heating fresh copper
Stop heating when gas in the servings stops decreasing
Final volume of air left should be 79cm^3
21cm^3 has reacted

31
Q

Nitrogen in air

32
Q

Oxygen in air

33
Q

Argon in air

34
Q

Carbon in air

35
Q

Group 7

A

Halogens
Non-metals
Poisonous
React with metals and form salts

36
Q

Three halogens

A

Chlorine
Bromine
Iodine

37
Q

Chlorine room temperature

38
Q

Bromine room temperature

A

Liquid

Red-brown

39
Q

Iodine room temperature

A

Solid

Black

40
Q

Group number

A

Number of electrons in outer shell

41
Q

Same group

A

Same chemical properties

42
Q

Periodic group left to right

A

Increasing atomic number

Periods

43
Q

Top to bottom

A

The more shells

Groups

44
Q

Group 1

A 
More reactive the further down you go
Very reactive metals
Stored under oil so they can't react with water/oxygen 
Alkali metals
React with water form alkaline solutions
45
Q

Group 1 characteristics

A 
Good conductors
Very soft
Low melting/ boiling points
Low densities
Shiny surface (dull after reacting with oxygen)
Burnt in air/oxygen
Form white, solid oxides
46
Q

Group 8/0

A

Noble gases
Chemically unreactive
Neither lose or gain electrons easily

Chemistry (10 decks)

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