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GCSE Chemistry AQA > C2 Bonding, structure and the properties of matter > Flashcards

C2 Bonding, structure and the properties of matter Flashcards

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1
Q

What are the three types of chemical bonds?

A

The three types of chemical bonds are ionic bonds, covalent bonds and metallic bonds.

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2
Q

Where do ionic bonds form?

A

Ionic bonds form between metals and non-metals.

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3
Q

Where do covalent bonds form?

A

Covalent bonds form between non-metal atoms.

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4
Q

Where do metallic bonds form?

A

Metallic bonds form in mettalic elements and alloys.

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5
Q

What are the particles involved with ionic bonding?

A

For ionic bonding the particles are oppositely charged ions.

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6
Q

What are the particles involved with covalent bonding?

A

For covalent bonding the particles are atoms which share pairs of electrons.

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7
Q

What are the particles involved with metallic bonding?

A

For metallic bonding the particles are atoms which share delocalised electrons.

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8
Q

Ionic bonding involves the transfer of what?

A

Ionic Bonding involves the transfer of electrons.

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9
Q

Do metals lose or gain electrons?

A

Metals lose electrons.

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10
Q

Do non metals lose or gain electrons?

A

Non metals gain electrons.

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11
Q

What is the charge of a metal ion?

A

The charge of a metal ion is positive.

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12
Q

What is the charge of a non-metal ion?

A

The charge of a non-metal ion is negative.

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13
Q

Draw a dot and cross diagram showing the formation of NaCl. Include electronic configurations.

A
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14
Q

What is an ionic compound and how are ions held together?

A

An ionic compound is a giant structure of ions. Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions.

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15
Q

What is a giant ionic lattice?

A

A giant ionic lattice is made up of oppositely charged ions held togther by electrostaic forces acting in all directions. This is called ionic bonding.

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16
Q

What does the picture of the giant ionic lattice of sodium chloride look like?

A
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17
Q

What are covalent bonds?

A

When atoms share pairs of electrons, they form covalent bonds. These bonds between atoms are strong.

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18
Q

What different diagrams can covalent structures be represented by?

A
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19
Q

Draw dot and cross diagrams for the molecules of hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia and methane.

A
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20
Q

What is metallic bonding?

A

Metals consist of giant structures of positive metal cations arranged in a regular pattern. The cations are surrounded by delocalised electrons. The attractions between of delocalised electrons and positive cations gives rise to strong metallic bonds.

21
Q

What does metallic bonding look like?

A
22
Q

What are the three states of matter?

A

The three states of matter are solid, liquid and gas.

23
Q

What determines the melting and boiling point of substances?

A

The melting and boiling points of substances are determined by the forces between the particles. This depends upon the structure and bonding within the substance.

24
Q

List the state symbols used in chemical equations.

A
  • Solid (s)
  • Liquid (l)
  • Gas (g)
  • Aquesous (aq)

Aqueaous measn the substance is dissolved in water.

25
Q

Why do ionic compounds have high melting points?

A

Ionic compounds have high melting points and high boiling points because of the large amounts of energy needed to break the many strong bonds.

26
Q

Why do ionic compunds conduct electricity when molten or dissolved, but not when solid?

A

When melted or dissolved in water, ionic compounds conduct electricity because the ions are free to move and so charge can flow.

27
Q

Describe some of the physical properties of small molecules.

A

Small molecules are usually gases or
liquids that have relatively low melting points and boiling points.

28
Q

Describe the the strength of the intermolecular forces between small molecules.

A

Small molecules have only weak forces between the molecules (intermolecular forces). It is these intermolecular forces that are overcome, not the covalent bonds, when the substance melts or
boils.

29
Q

What is the pattern in melting and boiling points as molecule size gets bigger?

A

The intermolecular forces increase with the size of the molecules, so larger molecules have higher melting and boiling points.

30
Q

Do small covalent molecules conduct electricity?

A

No, small covalent molecules do not conduct electricity as there is no overall charge or spare ions or electrons to carry a charge.

31
Q

Polymers have very strong covalent bonds between atoms, true or false?

A

TRUE! Atoms in polymers are held in palce by strong covalent bonds.

32
Q

Describe what a monomer looks like.

A

A monomer is an unsaturated compound with a double bond.

33
Q

What does a polymer look like?

A
34
Q

Explain why polymer molecules are solids at room temperature.

A

Polymer molecules are solid at room temperature because they have relatively strong intermolecular forces between polymer chains.

35
Q

Giant covalent structures are solids with high melting points. Expalin why.

A

Giant covalent compounds are solids with high metling points because the atoms are held together by strong covalent bonds that require large amounts of energy to break them.

36
Q

Give three examples of giant covalent structures.

A

Three examples of giant covalent structures are diamond, graphite and silicon dioxide.

37
Q

Metals have stong metallic bonding which makes them have high melting and boiling points. Explain why.

A

Strong metallic bonds are held together by strong forces of attraction between positive metal cations and delocalised electrons. They need lots of energy to be broken.

38
Q

Why do metals conduct electricity.

A

Metals conduct electricity because delocalised electrons are free to carry the electrical charge.

39
Q

Pure metals can be bent or drawn into wires. What are the names given to these properties?

A

Metals that can be bent are called malleable. Metals that can be drawn into wires are called ductile.

40
Q

How are pure metals made harder?

A

Pure metals are made harder by combining them with other metals to make alloys.

41
Q

Describe the bonding in diamond and some of its properties.

A

In diamond, each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, so diamond is very hard, has a very high melting point and does not conduct electricity.

42
Q

Describe the bonding in graphite.

A

In graphite, each carbon atom forms three covalent bonds with three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between the layers. In graphite, one electron from each carbon atom is delocalised.

43
Q

Describe the properties of graphite in relation to its structure.

A

Graphite is soft and slippery becuase of the weak intermolecular forces between layers. The delocalised electrons allow graphite to carry an electrical charge so it conducts electricity.

44
Q

Describe the structure of graphene and give one use of this material.

A

Graphene is made up of a single layer of graphite. It can be used in electrical circuits.

45
Q

Describe fullerenes and give a named example.

A

Fullerenes are molecules of carbon atoms with hollow shapes. The structure of fullerenes is based on hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms. The first fullerene to be discovered was buckminsterfullerene (C60) which has a spherical shape.

46
Q

What are carbon nanotubes and why are they useful?

A

Carbon nanotubes are cylindrical fullerenes with very high length to diameter ratios. Their properties make them useful for nanotechnology, electronics and materials.

47
Q

What do the allotropes of carbon look like?

A
48
Q
A

GCSE Chemistry AQA (11 decks)

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