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Chem GCSE > Bonding > Flashcards

Bonding Flashcards

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1
Q

What do ionic compounds contain?

A

A metal and a non-metal.

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2
Q

Charged particles formed from ionic bonding?

A

Ions.

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3
Q

What is a positive ion called?

A

A cation.

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4
Q

What is a negative ion called?

A

An anion.

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5
Q

Ionic bonding definition?

A

The strong electrostatic attraction between positive and negative ions.

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6
Q

What does ‘Electrostatic attraction’ mean?

A

Means that positively charged particles attract negatively charged particles.

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7
Q

What does ‘isoelectronic’ mean?

A

Means ‘have the same number of electrons’

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8
Q

Zinc (Ion) formula?

A

Zn²⁺

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9
Q

Silver (Ion) formula?

A

AG⁺

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10
Q

Hydrogen (Ion) formula?

A

H⁺

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11
Q

Ammonium (Ion) formula?

A

NH₄⁺

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12
Q

Nitrate (Ion) formula?

A

NO₃⁻

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13
Q

Hydroxide (Ion) formula?

A

OH⁻

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14
Q

Carbonate (Ion) formula?

A

CO₃²⁻

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15
Q

Sulfate (Ion) formula?

A

SO₄²⁻

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16
Q

What do all ionic compounds form?

A

They form crystals that consist of lattices of positive and negative ions packed in a regular way. The lattice is held together by the strong electrostatic attractions between the positively and negatively charged ions.

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17
Q

What is a lattice?

A

It is a regular array of particles.

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18
Q

What is a giant ionic lattice?

A

Giant meaning there are no individual molecules. There is no limit to the number of particles present.

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19
Q

Why do ionic compounds have high melting and boiling points?

A

A lot of energy is required to break the strong electrostatic forces of attraction between oppositely charged ions in the giant lattice structure.

20
Q

Why are ionic crystals brittle?

A

Any small distortion of a crystal brings ions with the same charge alongside each other.

21
Q

List physical properties of ionic substances?

A
  • High melting and boiling points.
  • Ionic compounds tend to be crystalline.
  • Ionic crystals tend to be brittle.
  • Tend to be soluble in water.
  • Tend to be insoluble in organic solvents.
22
Q

What does molten mean?

A

Means that the salt has been melted?

23
Q

Why don’t ionic compounds conduct electricity when they are solid?

A

Because the ions are fixed in position and are not free to move around.

24
Q

Why do ionic compounds conduct electricity when they are molten or dissolved in water?

A

Because the ions become free to move around.

25
Q

When do ionic compounds conduct electricity?

A

When they are molten or if they are dissolved in water (aqueous solution).

26
Q

What is a covalent bond?

A

A pair of electrons is shared between two atoms. The atoms are held together by the strong electrostatic attraction between the nuclei of the atoms and the shared pair of electrons.

27
Q

What is a simple molecular structure?

A

A substance which consists of molecules with intermolecular forces of attraction between them.

28
Q

Why do substances with simple molecular structures tend to have low melting and boiling points?

A

Because not much energy is required to break the weak intermolecular forces of attraction between molecules.

29
Q

Physical properties of covalent molecular compounds?

A
  • Low melting and boiling points.
  • Don’t conduct electricity.
  • Tend to be insoluble in water.
  • Often soluble in organic solvents.
30
Q

Why don’t covalent molecular compounds conduct electricity?

A

Because the molecules don’t have an overall electrical charge and electrons are held tightly in the atoms or covalent bonds so not able to move from molecule to molecule.

31
Q

Examples of simple molecular structures?

A
  • H₂O
  • CO₂
  • CH₄
32
Q

Why do substances with giant covalent structures have a very high melting and boiling point?

A

A lot of energy is required to break the very strong covalent bonds which extend throughout the structure.

33
Q

Why doesn’t diamond conduct electricity?

A

All the electrons in the outer shells of the carbon atoms are held tightly in covalent bonds between the atoms. None are free to move around.

34
Q

Why is graphite a soft material?

A

Graphite has a layer structure and the layers slide over each other and can easily be flaked off.

35
Q

Why does graphite conduct electricity?

A

Some electrons are free to move throughout the layers. The movement of these delocalised electrons allows graphite to conduct electricity.

36
Q

What does a metallic structure consist of?

A

It consists of a lattice of positive ions in a sea of delocalised electrons.

37
Q

What is metallic bonding?

A

The electrostatic forces of attraction between each positive ion and the delocalised electrons.

38
Q

What type of structure do metals have?

A

Giant structures.

39
Q

Why do metals conduct electricity?

A

Because the delocalised electrons are free to move throughout the structure?

40
Q

What does malleable mean?

A

‘Can be hammered into different shapes’

41
Q

Why are metals malleable and ductile?

A

When we apply a force to a piece of metal, the layers of positive ions slide over each other.

42
Q

What does ductile mean?

A

‘Can be drawn out into wires’

43
Q

What is an alloy?

A

A mixture of a metal with other metals (or carbon).

44
Q

Why are alloys harder than the individual pure metals from which they are made?

A

The different metals/elements have differently sized atoms. This makes it more difficult for the layers of ions to slide over each other.

45
Q

Examples of common alloys?

A
  • Bronze (mixture of copper and tin)
  • Brass (mixture of copper and zinc)
  • Steel (alloy of iron and carbon)
46
Q

Ethene formula?

A

C₂H₄

47
Q

Ethane formula?

A

C₂H₆

Chem GCSE (6 decks)

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