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chemistry Flashcards

1
Q

What is electrolysis?

A

Using electricity to break down electrolytes (e.g sodium, potassium and magnesium) to form elements

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2
Q

At the end of fractional distillation, what should be the result?

A

Each fraction should contain a mix of hydrocarbons that contain a similar number of carbon atoms that have similar MPs and BPs

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3
Q

What are the differences between alkanes and alkenes?

A

Alkanes are saturated single bonded hydrocarbons whereas alkenes are unsaturated double bonded hydrocarbons

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4
Q

In chromatography, how do you calculate the Rf value for each chemical?

A

Distance travelled by the substance / Distance travelled by the solvent

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5
Q

What’s the difference between the results of oxygen and hydrogen?

A

If oxygen is present, it will relight the glowing splint, whereas if hydrogen is present, you will get a squeaky pop from the lit splint

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6
Q

What four factors increases the rate of a reaction?

A

More collisions, increasing the temperature, increasing the concentration/pressure, increasing the surface area

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7
Q

What is one mole of any substance?

A

The amount of that substance that contains an Avogrado number of particles

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8
Q

What’s the difference between the atomic number and the mass number?

A

The atomic number is the number of protons whilst the mass number is the number of protons and neutrons

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9
Q

What formula links mass, molecular mass and moles?

A

Mass= Mr x moles

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10
Q

What is the limiting reactant in a chemical reaction?

A

The reactant that is completely used up because it limits the amounts of products made

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11
Q

What three ways can you measure a rate of reaction?

A

Loss in the mass of reactants, the volume of gas produced, time for a solution to become opaque

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12
Q

What is the disappearance of a cross test?

A

Take a piece of paper and mark a cross, put fraction glass on the top and mix in the reactants. Measure how long it takes for a cloudy mixture to conceal this cross.

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13
Q

What is the collision theory?

A

Chemical reactions only occur when reacting particles collide with each other with sufficient energy (activation energy)

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14
Q

What happens when you increase the pressure of a gas on the rate of reaction?

A

Increases number of gas molecules and increases frequency of collisions and so increases rate of reaction

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15
Q

What is an enzyme?

A

A molecule that acts as a catalyst in a biological system

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16
Q

What’s a reversible reaction?

A

The products can react backwards to product the original reactants

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17
Q

What happens if the temp of a system is increased?

A

Relative amount of products at equilibrium increases for endo and decreases for exo

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18
Q

What is a reaction profile?

A

A graph that shows the relative energies of reactants and products, as well as activation energy of the reaction

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19
Q

What is a battery?

A

Consists of two or more cells that are connected in a series

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20
Q

What are the properties of ionic substances?

A

High MP and BP, do not conduct electricity when solid, do conduct when they are molten or dissolved in water

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21
Q

What are polymers?

A

Large molecules with atoms linked by covalent bonds

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22
Q

What are the properties of the allotrope of carbon- diamond?

A

Four covalent bonds, very hard, high MP, does not conduct electricity

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23
Q

What are the properties of the allotrope of carbon- graphite?

A

Three covalent bonds, layers of hexagonal rings, high MP, layers slide, conduct electricity

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24
Q

What is a fullerene?

A

Hollow shaped molecules thats structure is based on hexagonal rings of carbon atoms

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25
Q

What is an alloy?

A

Mixtures of metals with others elements

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26
Q

What are the main properties of ionic compounds?

A

High MP and BP, can’t conduct electricity when s but can when l, dissolve easily in water

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27
Q

What’s the difference between fractional distillation and simple distillation?

A

Fractional separates liquids with similar BPs and simple separates out a liquid from a solution

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28
Q

What’s the structure of a crystal of sodium chloride?

A

Giant ionic lattice, positive sodium + negative chlorine form closely packed arrangement, strong electrostatic forces of attraction

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29
Q

Properties of diamond?

A

Hard, high MP and BP, lots of energy to break bonds, no delocalised electrons so can’t conduct electricity

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30
Q

What’s the structure of graphite?

A

Each carbon forms 3 covalent bonds, each carbon atom has 1 delocalised electron, creates layers of hexagons

31
Q

What does the concentration measure?

A

How much acid there is in a certain volume of water

32
Q

What’s the pH range for acids?

A

1-6

33
Q

What’s the pH of a neutral solution?

A

7

34
Q

What’s the pH of an alkali solution?

A

7-14

35
Q

What ion in an aqueous solution causes acidity?

A

H+

36
Q

What ion in an aqueous solution causes alkalinity?

A

OH-

37
Q

What is a decomposition reaction?

A

A single compound breaks down into 2+ elements or new compounds

38
Q

What is a neutralisation reaction?

A

When an acid and alkali react

39
Q

What’s the difference between a reduction and an oxidation reaction?

A

Reduction is where oxygen is lost and electrons are gained whereas oxidation is where oxygen is gained and electrons are lost

40
Q

What salt is produced when the acid used is hydrochloric acid?

A

A chloride

41
Q

What is the salt produced when the acid used is sulfuric acid?

A

A sulfate

42
Q

What is an indicator?

A

Something you can add to a solution to tell you if something is acidic or alkali

43
Q

What colour will a solution turn if it’s acidic?

A

Red

44
Q

What colour will a solution turn if it’s alkali?

A

Purple

45
Q

What does JJ Thompsons plum pudding model show?

A

A positive sphere with negative particles randomly arranged insides

46
Q

What is the difference between a compound and a mixture?

A

A compound is two or more different atoms that are chemically combined whereas in a mixture they are not chemically combined

47
Q

What is an ionic bond a covalent bond and a metallic bond?

A

Ionic involves a metal and a non metal sharing electrons, a covalent involves two non metals and a metallic involves two metals

48
Q

What is the simple distillation method?

A

1) solution heated & part that has lowest BP evaporates first
2) Vapour is coded, condensed and collected
3) Rest of solution is left behind in the flask

49
Q

Features of transition metals?

A

1) Form more than 1 ion
2) Often coloured
3) Make good catalysts

50
Q

What happens if metals are higher than carbon?

A

They must be extracted by electrolysis

51
Q

What is an isotope?

A

Same element, different number of neutrons (different mass number)

52
Q

What holds polymer molecules together?

A

Weak intermolecular forces

53
Q

What element can make inert electrodes?

A

Carbon

54
Q

What’s the test to identify hydrogen?

A

Place burning splint at end of test tube and if it’s present it will burn and there will be a squeaky pop sound

55
Q

What’s the test to identify oxygen?

A

Place glowing splint inside test tube, if present then the splint will relight

56
Q

What’s the test to identify oxygen?

A

Place glowing splint inside test tube, if present then the splint will relight

57
Q

What’s the test to identify carbon dioxide?

A

Lime water is mixed and if it’s present the limewater will go cloudy

58
Q

What’s the test to identify chlorine?

A

Damp litmus paper, if it’s present it will become bleached and turn white

59
Q

What are bases?

A

Chemicals which can neutralise acids and produce a salt and water and if it’s soluble in water it’s an alkali

60
Q

What do salts contain?

A

Positive ion which comes from the base or alkali and a negative ion which comes from the acid

61
Q

When acids react with a metal carbonate what do they make?

A

Salt, water and carbon dioxide

62
Q

What are strong acids?

A

They fully ionise in aqueous solutions

63
Q

What is meant by the concentration of acids?

A

Amount of acid molecules in a given volume of solution

64
Q

What is the reactivity series starting with most reactive?

A

Potassium, sodium, lithium, calcium, magnesium, carbon,zinc, iron, hydrogen, copper

65
Q

Examples of exothermic reactions?

A

Combustion, oxidation reactions and neutralisation

66
Q

Example of an endothermic reaction?

A

Thermal decomposition

67
Q

Do breaking bonds release or require energy?

A

Requires energy

68
Q

Is breaking bonds exothermic or endothermic?

A

Endothermic

69
Q

What is meant by the term bond energy?

A

Amount of energy required to break one mole of a particular covalent bond

70
Q

What is the charge in an ionic compound?

A

The charges on the ions have to cancel out to leave an overall charge of zero

71
Q

Equation to calculate overall energy change of a reaction?

A

Energy of bonds broken- energy of bonds formed

72
Q

What are transition metals?

A

Share same properties as metals but these metals can create ions of diff charges and form different coloured solutions

73
Q

What are fullerenes?

A

An allotrope of carbon that molecules are connected by single or double bonds

74
Q

What is an indicator solution?

A

A chemical dye that changes colour depending on the pH it’s mixed with

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