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Chemistry GCSE > C5-C7 BONDING > Flashcards

C5-C7 BONDING Flashcards

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1
Q

Bond

A

An attraction between two atoms that holds them together

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2
Q

Ion

A

An atom that has gained a charge by gaining or losing electrons

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3
Q

Charge

A

Whether an ion is positive or negative

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4
Q

Cation

A

Positive ion formed by losing electrons , formed by metal atoms

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5
Q

Anion

A

Negative ion formed by gaining electrons. Formed by non-metal atoms

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6
Q

Size of charge

A

The number of electrons transferred affects the size of charge : losing two electrons makes a 2+ charge, gaining three electrons makes a 3- charge

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7
Q

How many electrons are gained or lost

A

Metals: however many electrons are in the outer shell

Non-metals: however many electrons are needed to fill the outer shell

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8
Q

Electrostatic force

A

A force attraction between a positive and negative particle

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9
Q

Ionic pound

A

When two oppositely charge ions are held together by an electrostatic force

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10
Q

Forming ionic bonds

A

Electrons are transferred form a metal atom to a non-metal atom to form a positive metal cation and a negative metal anion the oppositely charged ions are attracted to each other

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11
Q

Chemical formula

A

Shows the number of atoms of each element present in one unit of a compound

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12
Q

Writing formulae

A

Each chemical symbol starts with a capital letter

The number of each atom present is shown with a subscript number after the symbol

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13
Q

Determining ionic formulae

A

Ensure the total number of positive and negative chargers balance
Change the number of each ion present by changing the subscript numbers

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14
Q

Compound ions

A

An ion made from two or more atoms that share a charge

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15
Q

Common compound ions

A 
Hydroxide: OH-
Nitrate: NO3
Sulfate: SO42-
Sulfite : SO32-
Carbonate : CO32-
Ammonium: NH4+
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16
Q

Including compound ions in formulae

A

If you need more than one, put brackets around it

E.g. MG(OH)2

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17
Q

Ionic lattice

A

The structure of ionic compounds: a repeating 3D pattern of alternating positive and negative ions

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18
Q

Crystal

A

A piece of material with a regular shape and straight edges formed by the regular pattern of ions in an ionic lattice

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19
Q

Melting point of ionic compounds

A

High because melting needs a lot of energy to break strong ionic bonds

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20
Q

Solubility of ionic compounds

A

Many ionic compounds dissolve in water

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21
Q

Electrical conductivity of ionic compounds

A

Solid: do not conduct because ions can’t move

Liquid (molten or solution): do conduct because ions can move

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22
Q

How ionic compounds conduct electricity

A

When they are in a liquid form the positive cations move to the negative electrode (cathode) and the negative anions move the positive electrode (anode)

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23
Q

Covent bond

A

An electrostatic attraction between two atoms and a share pair of electrons

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24
Q

Double bond

A

A covalent bond involving two shared pairs of electrons

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25
Q

Dots and crops diagrams

A

A bonding diagram showing the electrons in the outer shell of each atom with electrons drawn as dots and crosses

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26
Q

Hydrogen H2

A

Two overlapping circles both labelled H one pair in the over lap

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27
Q

Hydrogen chloride HCL

A

Two overlapping circles labelled H and CL one pair in the overlap , 6 electrons around CL

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28
Q

Oxygen O2

A

Two overlapping circles both labelled O two pairs in the overlap 4 electrons around each O

29
Q

Water H2O

A

Three overlapping circles in a line labelled H, O, H. A pair in each overlap 4 electrons around O

30
Q

Carbon dioxide, CO2

A

Three overlapping circles in a line labelled O,C,O two pairs in each over lap 4 electrons around each O

31
Q

Methane CH4

A

Five circles with one in the centre labelled C and 4 labelled H around it a pair in each overlap

32
Q

Valency

A

The number of covalent bonds an atom can form

33
Q

Valency and groups

A

Group4=4 (4 electrons needed)
Group5=3 (3 electrons needed)
Group6=2 (2 electrons needed)
Group7=1 (1 electrons needed)

34
Q

Working out molecular formulae

A

Find the lowest common multiple of the valency of each atom use the number of an atom required to reach the LCM

35
Q

Molecule

A

A particle made from two or more atoms bonded together

36
Q

Simple molecular structure

A

A structure made of small molecules in which a few atoms join together to form a small particle

37
Q

Structure of molecular substances

A

Atoms in a molecule are held together by strong covalent bonds. Neighbouring molecules are held close by weak intermolecular forces

38
Q

Intermolecular force

A

A weak electrostatic force that holds two neighbouring molecules together

39
Q

Melting point of simple molecular compounds

A

Low because melting only needs a little energy to break weak intermolecular forces

40
Q

Electrical conductivity of simple molecular compounds

A

Do not conduct because there are no electrons that are free to move

41
Q

Examples of simple molecular substances

A

Hydrogen gas, oxygen gas, water, carbon dioxide, methane

42
Q

Giant molecular structure

A

A structure made of a reappearing patterned of atoms covalently bonded together

43
Q

Melting point of giant molecular compounds

A

High because melting requires breaking strong covalent bonds

44
Q

Electrical conductivity of simple molecular compounds

A

Do not conduct (except graphite) because there are no electrons free to move

45
Q

Examples of simple molecular substances

A

Silicon dioxide (silica), diamond, graphite

46
Q

Polymer

A

A large molecule made of a small unit repeated many times

47
Q

Monomer

A

A small molecule that can be joined together many times to form a polymer

48
Q

Allotrope

A

A different structural form of an element made of the same atoms just bonded together differently

49
Q

Carbons allotrope

A

Graphite, diamond, graphene, fullerenes

50
Q

Graphite

A

Structure: stacked sheets of carbon in a honeycomb pattern with delocalised electrons between them

Properties: sheets slide apart easily, excellent conductor

Uses: lubricants

51
Q

Diamond

A

Structure: repeating pattern of 4 atoms bonded to 4 others

Properties: very strong, excellent conductor

Uses: none yet, but potentially many

52
Q

Graphene

A

Structure: a single layer of atoms in a honeycomb pattern

Properties: very strong , excellent conductor

Uses: none yet but potentially many

53
Q

Buckminster fullerene

A

Structure: ball-shaped molecules of C60

Properties: low melting point

Uses: none

54
Q

Carbon nanotubes

A

Structure: cylinders made of carbon bonded in a honey comb pattern

Properties: very strong excellent conductors

Uses:strong and felixaeble materials, electronics

55
Q

Structure of metals

A

A lattice of positive metals ions surrounded by a cloud of delocalised electrons

56
Q

Delocalised electrons

A

Electrons that are not bound to a single atom but more freely around many

57
Q

Metallic bonding

A

The electrostatic attraction between the lattice of positive metal ions and the cloud of delocalised electrons

58
Q

Electrical conductivity of metals

A

Metals are good conductors because the electrons are free to move

59
Q

Comparing the conductivity of metals

A

Metals with more electrons in the outer shell such as AL are better conductors than those with fewer such as LI because there are more delocalised electrons that are able to move

60
Q

Malleable

A

When a substance dents when it is hit instead of shattering

61
Q

Malleability of metals

A

Metals are malleable because the atoms are arranged in regular sheets and these sheets can easily slide over each other when hit

62
Q

Melting point of metals

A

High because melting them requires breaking the strong force of attraction between the cloud of delocalised electrons

63
Q

Classifying materials

A

The properties of a material can be used to determine the type of bonding in it

64
Q

Properties of ionic compounds

A

High melting point, does not conduct electricity, sometimes soluble in water

65
Q

Properties of giant molecular compounds

A

High melting point, does not conduct electricity (except graphite) insoluble in water

66
Q

Properties of metallic compounds

A

High melting point , does not conduct electricity, insoluble in water

67
Q

Bonding models

A

The ideas and drawings that we use to explain the bonding of atoms

68
Q

Problems with bonding models

A

Dot and cross diagrams make electrons seem different, they are not
Atoms appear stationary the are actually vibrating
Atoms don’t appear to be touching when they actually are

Chemistry GCSE (8 decks)

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