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GCSE Chemistry > Topic 1c- Bonding (Paper 1 + 2) > Flashcards

Topic 1c- Bonding (Paper 1 + 2) Flashcards

1
Q

What is the relative mass of an electron?

A

1/1840

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2
Q

What is the relative mass of a proton?

A

1

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3
Q

What is the relative mass of a neutron?

A

1

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4
Q

What is the relative charge of an electron?

A

-1

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5
Q

What is the relative charge of a neutron?

A

0

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6
Q

What is the relative charge of a proton?

A

+1

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7
Q

What are isotopes?

A

Isotopes are atoms of the same element that have a different number of neutrons and therefore also a different mass number.

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8
Q

What is relative atomic mass?

A

The relative atomic mass is the weighted average mass of an atom of an element compared to 1/12 the mass of a Carbon atom (12).

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9
Q

How many electrons are in each shell (up to 3rd)?

A

2,8,18 (but behaves like 8)

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10
Q

What holds together a substance that is ionically bonded?

A

Positive and negative ions are held together by electrostatic forces of attraction in a giant lattice structure.

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11
Q

What holds together a substance that is ionically bonded?

A

Positive and negative ions are held together by electrostatic forces of attraction in a giant lattice structure.

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12
Q

What are properties of ionic substances?

A

High melting and boiling points.
Hard but brittle.
Generally soluble in water.
Don’t conduct electricity in a solid state.
Do conduct electricity as liquids i.e. when molten or dissolved in water.

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13
Q

What are ions?

A

Ions are charged particles.

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14
Q

What substances form covalent bonds?

A

Two or more non-metals.

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15
Q

What substances form ionic bonds?

A

A metal and a non-metal.

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16
Q

What substances form metallic bonds?

A

Two or more metals.

17
Q

What are simple covalent substances?

A

Composed of separate molecules bonded strongly together by covalent bonds. (e.g. H20, CH4, O2…)

18
Q

What are giant covalent substances?

A

Giant covalent substances contain millions of atoms bonded together by many strong covalent bonds to form a giant molecule or macromolecule. (e.g. diamond and graphite.)

19
Q

Why are the melting and boiling points of covalent substances low?

A

Only need to overcome weak intermolecular forces that need little energy.

20
Q

Why are simple covalent substances poor conductors?

A

No ions or free electrons present.

21
Q

Why do simple covalent substances have poor solubility in water?

A

No charged particles present to be attracted to water molecules.

22
Q

What are the physical properties of simple covalent substances?

A

Low melting and boiling points.
Poor electrical conductivity.
Poor solubility in water.

23
Q

What are the physical properties of metallically bonded compounds?

A

High melting and boiling points.
Malleable and ductile.
Good conductors of electricity.
Good conductors of heat.

24
Q

Why do metallically bonded substances have high melting and boiling points?

A

Lots of energy is needed to overcome the forces of attraction between the positive ions and delocalised electrons.

25
Q

Why are metallically bonded substances malleable and ductile?

A

Layers of ions can slide over each other when force is applied.

26
Q

Why are metallically bonded substances malleable and ductile?

A

Layers of ions can slide over each jother when force is applied.

27
Q

Why are metallically bonded substances good conductors of electricity?

A

The electrons in the sea of delocalised electrons are free to move and can flow when a potential difference is applied.

28
Q

Why are metallically bonded substances good conductors of electricity?

A

The electrons in the sea of delocalised electrons are free to move and can flow when a potential difference is applied.

29
Q

Why are metallically bonded substances good conductors of electricity?

A

The electrons in the sea of delocalised electrons are free to move and can flow when a potential difference is applied.

29
Q

Why are metallically bonded substances good conductors of electricity?

A

The electrons in the sea of delocalised electrons are free to move and can flow when a potential difference is applied.

30
Q

Why are metallically bonded substances good conductors of heat?

A

The delocalised electrons gain kinetic energy when heated and move faster through the material transferring heat.

31
Q

What is an alloy?

A

Mixtures of metals where the metals are metallically bonded in a giant metal lattice.

32
Q

Why are alloys not regarded as compounds?

A
  1. The metals can be separated by physical methods.
  2. There is no fixed ratio for an alloy, unlike atoms in a compound.
33
Q

Why are alloys generally tougher and less malleable than pure metals?

A

The foreign metal atoms prevent the layers of metal atoms from sliding over each other, therefore they are stronger.

GCSE Chemistry (26 decks)

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