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Chemistry GCSE > 1- Principles Of Chemistry > Flashcards

1- Principles Of Chemistry Flashcards

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1
Q

Define solvent

A

Liquid the solute is dissolved into

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2
Q

Define Solute

A

The substance being dissolved

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3
Q

Crystallisation

A

Pour solution in evaporating dish, heat gently

Evaporate the water, solution +concentrated

When crystals appear remove from heat

Filter and dry

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4
Q

Equation for solubility

A

= (mass of solid/ Mass of water removed) x100

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5
Q

Simple distillation

A

Liquid from solution

Heat until substance with lowest boiling point evaporates

Cooled condensed collected

Boiling points must be very different

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6
Q

Fractional distillation

A

Use a flask and fractionating column

Heat, as they evaporate at diff temperatures

They rise as they evaporate to top

Use cold water as a condenser

Continue for all stages

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7
Q

Chromatography

A

Draw baseline in pencil

Add spots and place in solvent (eg water) (makes sure solvent is below base line)

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8
Q

Equation for Rf value (ratio of distances travelled)

A

Distance traveled by solute/ distance travelled by solvent

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9
Q

Define isotope

A

Form of the same element with a different number of NEUTRONS

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10
Q

Find Ar from isotopes

A

Turn each percentage into decimal

Multiply by mass number (changed number)

Add together

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11
Q

Groups are…. (V/h)

A

Vertical

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12
Q

What do elements of the same group have in common?

A

Same number of electrons on outershell

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13
Q

Moles, mass, Mr equation

A

Moles= mass/Mr

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14
Q

Calculate reacting masses ( Pg 23 CGP)

A

Write balanced equation

Work out Mr (of what ur interested in)

Calculate number of moles

Look at the ratio of moles

Calculate the mass (of the moles of the substance)

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15
Q

Empirical formula

A

Elements
Mass
Moles
Ratio

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16
Q

Ionic -electrostatic static attractions

A

Oppositely charged ions are strongly attracted to each other

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17
Q

Giant Ionic Lattice

A

Strong electrostatic attractions, strongly packed

Need large amount of energy to overcome (/break) these attractions

Don’t conduct as solids, only melted or dissolved (in water)

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18
Q

Covalent- electrostatic attractions

A

Strong attraction between the shared electron and the positive nuclei

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19
Q

Why are simple molecular structures liquids or gases, or solids with low boiling points?

A

They have weak intermolecular forces, which need little energy to overcome (/break) them

20
Q

Giant covalent structures

A

No charged ions

Lots of strong bonds

More energy needed to overcome (/break) the bonds

Don’t conduct (-graphite)

Usually insoluble

21
Q

Diamond

A

Each C has four bonds

Strong bonds

Rigid lattice structure (hard)

Doesn’t conduct (no free electrons or ions)

22
Q

Graphite

A

Each C has 3 bonds

Creates layers held weakly by intermolecular forces

High melting point (covalent bonds in layers)

Conducts (one delocalised electron)

23
Q

C60 Fullerene

A

Held weakly by intermolecular forces (can slide, is soft)

One delocalised electron but cannot move between molecules and so is A POOR CONDUCTOR

24
Q

Is group 1 acid or alkali?

A

Alkali

25
Q

Reaction- lithium and water

A

Fizzes steadily, becomes smaller until all reacted

Least reactive

26
Q

Reactions- sodium and water

A

Forms a ball, fizzes more rapidly, quickly becomes smaller until disappears

2nd most/ least reactive

27
Q

Potassium

A

Forms a ball (melts) quickly, fizzes, possibly burns (with a lilac flame), (and sometimes reacts with an explosion)

28
Q

Chlorine at room temperature

A

Atomic number,17

Colour- green

State- gas

Boiling point- -34

29
Q

Bromine at room temp

A

Atomic number-36

Colour- red brown

State- liquid

Boiling point - 59C

30
Q

Iodine at room temp

A

Atomic number- 53

Colour- dark grey

State- solid

Boiling point- 185C

31
Q

What’s a displacement reaction?

A

A more reactive element displaces ( or pushes out) a less reactive element

(Can be used to find out what is more/ less reactive)
Eg chlorine water + potassium iodide forms potassium chloride (chlorine is more reactive)

32
Q

What are the four main gases, and their percentages, in air?

A

78% nitrogen

21% oxygen

> 1% argon

0.04% carbon dioxide

33
Q

Combustion of magnesium

A

Burns with a bright white flame

Forms white powder / magnesium oxide

Slightly alkaline when dissolved in water

34
Q

Combustion of hydrogen

A

Orange/ yellow flame

Water vapour as only product

35
Q

Combustion of sulphur

A

Pale blue flame

Produces sulphur dioxide

Acidic when dissolved in water

36
Q

Thermal decomposition of metal carbonates

A

Produces CO2 and a metal oxide

Substance broken down when heated

Use copper (II) carbonate and a delivery tube

37
Q

Acid + metal goes to…

A

Salt + hydrogen

38
Q

Metal + water goes to…

A

Metal hydroxide + hydrogen

39
Q

A sacrificial method of preventing rust

A

Coat with Zinc ( which is more reactive)

Called galvanising

40
Q

Define oxidising agent

A

The substance that is reduced (oxidises other substance)

41
Q

Define reducing agent

A

The substance that is oxidised (reduces the other substance)

42
Q

Indicators- litmus paper

A

Red in acid

Blue in alkaline

Purple in neutral

43
Q

Indicators- phenolphthalein

A

Colourless in acid

Pink in alkaline

44
Q

Indicators- Methyl orange

A

Red in acid

Yellow in alkaline

45
Q

Acids in solutions are a source of…

A

Hydrogen ions

46
Q

Alkalis in solutions are a source of…

A

Hydroxide ions

Chemistry GCSE (8 decks)

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