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Chemistry > 3.1 Introduction to chemistry > Flashcards

3.1 Introduction to chemistry Flashcards

(51 cards)

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1
Q

Name of compounds containing 1 metal, 1 non metal

A

Metal, Non-metal ide
e.g. FeS = Iron sulfide

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2
Q

Name of compounds containing 1 metal and 2 non metals

A

Metal, Non-metal that isn’t oxygen, Change end of non-metal to ate
e.g. MgSO4 = magnesium sulphate

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3
Q

Diatomic molecules

A

Bromine
Oxygen
Chlorine
Iodine
Hydrogen
Nitrogen
Fluorine
(Astatine)

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4
Q

Observations to make when describing substances in practical work

A
  • solid/liquid/gas
  • coloured/colourless
  • crystalline/powdered (for solids)
  • clear/cloudy (for liquids)
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5
Q

Observations to make when describing changes in practical work

A
  • fizzing?
  • has a solid appeared/disappeared
  • colour change
  • unusual sounds/smells
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6
Q

pH scale

A

pH less than 7 = acidic
pH is 7 = neutral
pH greater than 7 = alkaline

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7
Q

Methyl orange colours

A

Acid - red
Neutral - yellow
Alkaline - yellow

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8
Q

Phenolphthalein colours

A

Acid - colourless
Neutral - colourless
Alkaline - pink

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9
Q

red litmus colours

A

Acid - red
Neutral - red
Alkaline - blue

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10
Q

blue litmus colours

A

Acid - red
Neutral - blue
Alkaline - blue

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11
Q

universal indicator

A

pH 0-14
ROYGBIV

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12
Q

Evidence of particles (diffusion)

A

Diffusion is when particles spread out from high to low concentrations

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13
Q

3 states of matter

A

solid, liquid, gas

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14
Q

particle arrangement of a solid

A

close
ordered
vibrate around fixed positions

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15
Q

particle arrangement of a liquid

A

close
random
move freely past each other

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16
Q

particle arrangement of a gas

A

far apart
random
move completely freely

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17
Q

changes of state

A

solid –> liquid = melting
liquid –> gas = vaporizing
gas –> solid = deposition
solid –> gas = sublimation
gas –> liquid = condensing
liquid –> solid = freezing

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18
Q

test to show diffusion of gases

A

ammonium chloride tube

two gases (ammonia and hydrogen chloride) diffuse from the ends of a sealed tube
where they meet the compound ammonium chloride forms as a white smoke
this shows while molecule is heavier as it will diffuse slower

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19
Q

Element definition

A

a substance containing only one type of atom

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20
Q

Compound definition

A

a substance containing more than one type of atom, chemically bound together

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21
Q

Pure substance

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A

All particles are the same

22
Q

Mixture

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A

Made up of more than one substance, not chemically bound

23
Q

Chemical test for water

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A

Anhydrous copper (II) sulphate turns form white to blue
Tells you water is present but not its purity

24
Q

Physical tests for water

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A

Melting point = 0 degrees C
Boiling point = 100 degrees C
pure water will melt and boil at exactly these points

25
What can elements be categorised into
metal and non-metal
26
Metal properties
Left-hand side of the periodic table high MP/BP electrical conductors malleable shiny form alkaline oxides
27
Non metal properties
Right-hand side of the periodic table low MP/BP electrical insulators brittle dull form acidic oxides
28
Element combustion
when an element reacts with oxygen to form an oxide element + oxygen --> element oxide
29
Combustion of magnesium
Magnesium + oxygen -> magnesium oxide Observation: bright white light and white powder formed
30
Combustion of sulphur
Sulphur + oxygen --> sulphur dioxide Observations: blue flame
31
Combustion of hydrogen
Hydrogen + oxygen --> water Observations: squeaky pop
32
Dissolving oxides
Metal + oxygen --> metal oxide Metal oxide + water --> alkaline solution Non-metal + oxygen --> non-metal oxide Non-metal oxide + water --> acidic solution
33
How to determine if an unknown element was a metal or non-metal
1. combust it in oxygen 2. dissolve the oxide formed 3. check the pH of the solution with an indicator
34
Making compounds
Compounds can often be formed by heating their elements together e.g. zinc + sulphur --> zinc sulphide
35
Properties of compounds
the properties of compounds are usually totally different from the properties of the elements the compound is made from
36
Types of chemical bonding
2 metals = metallic 2 non - metals = covalent 1 of each = ionic
37
composition of the air
Nitrogen - 78% Oxygen - 21% Argon - 0.96% Carbon dioxide - 0.04%
38
How do we measure the percentage of oxygen in the air
React oxygen with another element, often a metal The air gradually decreases in volume until all of the oxygen has been added to the element Results - take the decrease in volume, divide it by the initial volume of air, then times by 100 (should decrease by 21%) If it doesn't it is usually because: the metal was not heated for long enough for all of the oxygen to react or there was a leak in the apparatus
39
solute definition
the substance which is going to be dissolved
40
solvent definition
the liquid which is going to do the dissolving
41
solution definition
the resulting mixture of solute dissolved in solvent
42
saturated definition
a solution in which no more solute can be dissolved
43
suspension definition
a solid floating in a liquid because it cannot dissolve
44
soluble definition
a substance which can be dissolved
45
insoluble definition
a substance which cannot be dissolved
46
unit for measuring solubility
g per 100g of solvent
47
solubility curves
above the line - insoluble :/ on the line - saturated below the line - soluble :) x axis - temperature (degrees c) y axis - solubility (g/100g)
48
thermal decomposition
when heat energy is used to break down a substance Metal carbonates thermally decompose to form metal oxides and carbon dioxide Carbon dioxide is denser than air, so is collected by downward delivery (sinks to the bottom of a test tube)
49
Copper carbonate thermal decomposition colour change
Green —> black
50
How can carbon dioxide be collected after thermal decomposition
Downward delivery (Sinks to the bottom of a tube and stays there until you want to use it) Works because it is more dense than air
51
Chromatography method
1. Draw a line in pencil 2. Put a spot of ink on the line 3. Pour some solvent in the beaker 4. Place paper in the beaker so spots are above solvent 5. Leave until solvent has risen up the paper

Chemistry (13 decks)

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