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GCSE Chemistry for OCR Gateway (Grade 9-1) > Revision Guide > Flashcards

Revision Guide Flashcards

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1
Q

What does the ‘mass’ number tell us?

A

The total number of protons and neutrons in the nucleus of an atom.

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2
Q

What does the ‘atomic’ number tell us?

What two things can be determined from it?

A

The number of protons in the nucleus of an atom.

a) The position of the element in the periodic table.
b) What the chemical element is, because the number is unique.

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3
Q

What can you determine from the ‘period’?

What can you determine from the ‘group’?

Elements within the same group have … ?

A

The number of full shells of electrons.

The number of electrons in the outer shell (valence electrons).

Similar chemical properties

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4
Q

What is the name of the bonding that occurs between ‘Cations’ and ‘Anions’?

What type of elements, does it happen between?

A

Ionic Bonding.

Metals and Non-Metals.

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5
Q

Cations can be found in what groups on the periodic table?

What type of element are they?

A

Group 1 and 2

Metals

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6
Q

Anions can be found in what groups on the periodic table?

What type of element are they?

A

Group 6 and 7

Non-Metals

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7
Q

Why do cations become more reactive, the more electron shells they have?

A

The distance of the electrons from the nucleus increases meaning it is easier for them to be removed.

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8
Q

A full outer shell is also known as?

A

Stable electronic structure.

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9
Q

What type of force is present with Ionic Bonds?

A

Electrostatic

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10
Q

What type of structure do Ionic Compounds form?

A

Giant Ionic Lattice

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11
Q

The strong attraction between ions results in what two properties, and why?

A

High melting and boiling points because it takes a large amount of energy to overcome the strong attraction.

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12
Q

What property changes when an ionic compound is dissolved or melted and why?

A

Electrical conductivity. The ions separate and are free to move. This allows them to carry an electric charge.

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13
Q

Covalent Bonds form when _____ elements combine together. They do this by _____ _____ ______ _____ to achieve a _____ _____ _____ .

A

non-metal / sharing pairs of electrons / full outter shell

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14
Q

What are fullerenes?

Describe their shape.

A

Large carbon molecules

Molecules shaped like hollow balls or tubes.

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15
Q

Two characteristics of Nanoparticles.

A

1) High surface area to volume ratio.
2) They can modify the properties of materials.

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16
Q

What is the reaction called when a monomer becomes a polymer?

What does it usually need to occur?

A

Polymerisation

High pressure and a catalyst

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17
Q

What determines the properties of a plastic?

A

Intermolecular forces between the polymer chains.

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18
Q

What type of structure do Metals have?

A

Crystal

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19
Q

Name the start and end markings on the stationary phase.

A

Point of origin or baseline / Solvent front

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20
Q

How do you reveal a colourless spot?

A

Use a locating agent (reagent).

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21
Q

What is an Rf value and how do you calculate it?

A

Rf = The ratio between the distance travelled by the dissolved substance (the solute) / and the distance travelled by the solvent.

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22
Q

What is the time it takes for a chemical to travel through the tube called?

A

Retention time.

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23
Q

What is an isotope?

A

A different form of the same element which has a different number of neutrons.

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24
Q

Simple molecular structures formed with covalent bonds, for example _____ and _____ . They have _____ _____ and _____ _____ .

A

Carbon Dioxide / Water / high melting / boiling points

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25
Q

What is the characteristic of an element?

A

All the atoms are the same.

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26
Q

Define the term ‘compounds’.

A

Two or more different elements, chemically combined in a fixed proportion.

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27
Q

Compounds usually have ______ ______ ______ to the elements that they are made from.

A

totally different properties

28
Q

What is a mixture?

A

Different elements or compounds, not chemically combined together.

29
Q

What are molecules?

A

A molecule has any elements chemically joined.

Molecules can be created from elements and compounds.

30
Q

What bonds do elements in group 7 form with each other and why?

A

Colavent bonds, They sharing electrons to achieve a full outer shell.

31
Q

Group 1 metals are also know as?

A

Alkali metals

32
Q

What are four properties of Group 1 elements?

A

Soft, can be cut with a knife.

Relatively low melting points

React rapidly with Oxygen, Chlorine and Water

Form +1 ions

33
Q

What are four properties of transition elements?

A

Hard and strong

High melting points

High density

Can form ions with different charges

34
Q

What is it called when a metal gains oxygen?

A

Oxidation

35
Q

The reactivity of a metal depends ….

A

… on its ability to lose electrons and form a positive ion.

36
Q

What do you get when reacting a metal with water?

A

Metal hydroxide (alkali) and Hydrogen gas

37
Q
A
38
Q

A more reactive element will _____ _____ a _____ _____ element from its _____ .

Also known as a _____ _____ .

A

more reactive / push out / less reactive / compound

displacement reaction

39
Q

What do bases produce when neutralising an acid?

A

Salt and water

40
Q

Bases that are soluble in water are called?

What do they produce when in aqueous solution?

A

Alkalis

Hydroxide ions (OH-)

41
Q

What is the equation for neutralisation?

A
42
Q

Name three acids and the salts they produce.

A

Hydrochloric - Chloride

Sulfuric - Sulfate

Nitric - Nitrate

43
Q

When acids react with metal carbonates, what is produced?

A

Salt, water and Carbon Dioxide

44
Q

Strong acids _____ _____ in aqueous solutions.

A

fully ionise

45
Q

Name three weak acids.

A

Carbonic

Ethanoic

Citric

46
Q

What is a titration used for?

A

To work out the concentration of a quantity of acid or alkali.

47
Q

What are group 7 elements also known as?

A

Halogens

48
Q

List three points acount halides

A

One atom of a halogen.

Can only exist in compounds (other wise they would pair up and become halogens)

They are ions

49
Q

In electrolysis, if the aqueous solution contains a halide, what is produced at the anode?

A

The compound has been separated, and the halides form covalent bonds to become halogens.

50
Q

Breaking chemical bonds is ______

Making chemical bonds is ______

A

Endothermic

Exothermic

51
Q

What is relative atomic mass?

A

The average of the mass numbers of different isotopes.

Weighted for the abundance of each isotope.

52
Q

What is relative formula mass?

A

All the relative masses of the elements in a compound, added together.

53
Q

The relative atomic mass, in grams, is equal to _____ ?

A

1 mole

e.g. Carbon has a relative atomic mass of 12. In 12g of carbon there is 1 mole.

54
Q

What is the equation to calculate ‘number of moles’?

A
55
Q

What is the equation to calculate the ‘mass of a number of moles’?

A
56
Q

Electrons in a shell are found in regions called what?

A

Atomic orbitals

57
Q

What are the letters given to the atomic orbitals?

A

S, P, D, F

58
Q

Define ‘subshell’

A

All the orbitals of the same type in the same shell. e.g. 2P, 3D

59
Q

Group 2 metals are also known as?

A

Alkaline Earth Metals

60
Q

Adding a Group 1 metal to water produces what type of base?

A

Alkali

61
Q

Adding a Group 2 metal to water produces what type of base?

A

Alkaline

62
Q

What are two types of endothermic reactions?

A

Thermal decomposition

Electrolysis

63
Q

What are three types of exothermic reactions?

A

Neutralisation

Combustion

Oxidation

64
Q

Endothermic reactions _____ _____ energy from the surroundings.

A

take in

65
Q

Reactions can only occur when particles _____ _____ _____ _____

The minimum amount of energy that particles must have to react is called _____ _____ .

A

collide with each other

activation energy

66
Q

The loss and gain of electrons is known as?

A

Oxidation Is the Loss of electrons

Reduction Is the Gain of electrons

GCSE Chemistry for OCR Gateway (Grade 9-1) (1 decks)

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