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Chemistry GCSE > C5-C7 BONDING > Flashcards

C5-C7 BONDING Flashcards

(68 cards)

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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
Dots and crops diagrams
A bonding diagram showing the electrons in the outer shell of each atom with electrons drawn as dots and crosses
26
Hydrogen H2
Two overlapping circles both labelled H one pair in the over lap
27
Hydrogen chloride HCL
Two overlapping circles labelled H and CL one pair in the overlap , 6 electrons around CL
28
Oxygen O2
Two overlapping circles both labelled O two pairs in the overlap 4 electrons around each O
29
Water H2O
Three overlapping circles in a line labelled H, O, H. A pair in each overlap 4 electrons around O
30
Carbon dioxide, CO2
Three overlapping circles in a line labelled O,C,O two pairs in each over lap 4 electrons around each O
31
Methane CH4
Five circles with one in the centre labelled C and 4 labelled H around it a pair in each overlap
32
Valency
The number of covalent bonds an atom can form
33
Valency and groups
Group4=4 (4 electrons needed) Group5=3 (3 electrons needed) Group6=2 (2 electrons needed) Group7=1 (1 electrons needed)
34
Working out molecular formulae
Find the lowest common multiple of the valency of each atom use the number of an atom required to reach the LCM
35
Molecule
A particle made from two or more atoms bonded together
36
Simple molecular structure
A structure made of small molecules in which a few atoms join together to form a small particle
37
Structure of molecular substances
Atoms in a molecule are held together by strong covalent bonds. Neighbouring molecules are held close by weak intermolecular forces
38
Intermolecular force
A weak electrostatic force that holds two neighbouring molecules together
39
Melting point of simple molecular compounds
Low because melting only needs a little energy to break weak intermolecular forces
40
Electrical conductivity of simple molecular compounds
Do not conduct because there are no electrons that are free to move
41
Examples of simple molecular substances
Hydrogen gas, oxygen gas, water, carbon dioxide, methane
42
Giant molecular structure
A structure made of a reappearing patterned of atoms covalently bonded together
43
Melting point of giant molecular compounds
High because melting requires breaking strong covalent bonds
44
Electrical conductivity of simple molecular compounds
Do not conduct (except graphite) because there are no electrons free to move
45
Examples of simple molecular substances
Silicon dioxide (silica), diamond, graphite
46
Polymer
A large molecule made of a small unit repeated many times
47
Monomer
A small molecule that can be joined together many times to form a polymer
48
Allotrope
A different structural form of an element made of the same atoms just bonded together differently
49
Carbons allotrope
Graphite, diamond, graphene, fullerenes
50
Graphite
Structure: stacked sheets of carbon in a honeycomb pattern with delocalised electrons between them Properties: sheets slide apart easily, excellent conductor Uses: lubricants
51
Diamond
Structure: repeating pattern of 4 atoms bonded to 4 others Properties: very strong, excellent conductor Uses: none yet, but potentially many
52
Graphene
Structure: a single layer of atoms in a honeycomb pattern Properties: very strong , excellent conductor Uses: none yet but potentially many
53
Buckminster fullerene
Structure: ball-shaped molecules of C60 Properties: low melting point Uses: none
54
Carbon nanotubes
Structure: cylinders made of carbon bonded in a honey comb pattern Properties: very strong excellent conductors Uses:strong and felixaeble materials, electronics
55
Structure of metals
A lattice of positive metals ions surrounded by a cloud of delocalised electrons
56
Delocalised electrons
Electrons that are not bound to a single atom but more freely around many
57
Metallic bonding
The electrostatic attraction between the lattice of positive metal ions and the cloud of delocalised electrons
58
Electrical conductivity of metals
Metals are good conductors because the electrons are free to move
59
Comparing the conductivity of metals
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
Malleable
When a substance dents when it is hit instead of shattering
61
Malleability of metals
Metals are malleable because the atoms are arranged in regular sheets and these sheets can easily slide over each other when hit
62
Melting point of metals
High because melting them requires breaking the strong force of attraction between the cloud of delocalised electrons
63
Classifying materials
The properties of a material can be used to determine the type of bonding in it
64
Properties of ionic compounds
High melting point, does not conduct electricity, sometimes soluble in water
65
Properties of giant molecular compounds
High melting point, does not conduct electricity (except graphite) insoluble in water
66
Properties of metallic compounds
High melting point , does not conduct electricity, insoluble in water
67
Bonding models
The ideas and drawings that we use to explain the bonding of atoms
68
Problems with bonding models
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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