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Chemistry > C2 - Bonding, Structure, and The Properties of Matter > Flashcards

C2 - Bonding, Structure, and The Properties of Matter Flashcards

1
Q

What is Ionic Bonding?

A

The electrostatic attraction between positive and negative ions.

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2
Q

How are ionic compounds held together?

A

Held together in a giant lattice.
Regular structure that extends in all directions in a substance.
Electrostatic attraction between positive and negative ions holds the structure together.

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3
Q

State properties of Ionic Substances.

A

High melting and boiling points.
Do not conduct electricity when solid.
Conduct when molten or dissolved in water.

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4
Q

What is important when working out a formula of an Ionic Compound?

A

They are electrically neutral, because positive and negative charges balance each other.

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5
Q

How are Ionic Compounds formed? Explain in terms of MgO case. (4 Marks)

A

Reaction of a metal with a non-metal.
Metal gives away its outer shell electrons to non-metal.
Mg is in Group 2, so has 2 available outer shell electrons.
O is in Group 6, so can accept 2 electrons to get a full outer shell configuration.
Mg becomes Mg^2+ and O becomes O^2-.

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6
Q

What is a Covalent Bond?

A

A shared pair of electrons between two atoms.

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7
Q

Describe the structure and properties of simple molecular covalent substances.

A

Do not conduct electricity.
Small molecules.
Weak intermolecular forces, therefore:
Low melting and boiling points.

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8
Q

What are Polymers?

A

Very large molecules with atoms linked by covalent bonds.

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9
Q

What are thermosoftening polymers?

A

They melt/soften when heated. There are no bonds between polymer chains. Weak intermolecular forces ensure that the structure is solid at room temperature.

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10
Q

What are giant covalent substances?

A

Solids, atoms covalently bonded together in a giant lattice.
High melting and boiling points - strong covalent bonds.
Mostly don’t conduct electricity.

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11
Q

Give example of Giant Covalent Substances.

A

Diamond
Graphite
Silicon dioxide

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12
Q

Describe and explain the properties of Diamond.

A

Four, strong covalent bonds for each carbon atom
Very hard
Very high melting/boiling points
Insulator

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13
Q

Describe and explain the properties of Graphite.

A

Three covalent bonds for each carbon atom
Layers of hexagonal rings
High melting point
Layers free to slide as weak intermolecular forces between layers
Conducts thermal and electricity.

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14
Q

Describe and explain the properties of Fullerenes.

A

Hollow shaped molecules
Based on hexagonal rings but may have 5/7 carbon rings
Has spherical shape, simple molecular structure (Buckminsterfullerene)

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15
Q

Describe and explain the properties of Nanotubes.

A

Cylindrical fullerene with high length to diameter ratio
High tensile strength
Conductivity

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16
Q

What is Graphene?

A

A single layer of graphene.

17
Q

What is Metallic Bonding?

A

Forces of attraction between delocalised electrons and nuclei of metal ions.

18
Q

What are Alloys?

A

Mixtures of metal with other elements, usually metals.

19
Q

What are Alloys harder than pure metals?

A

Different sizes of atoms distorts the layers, so they can’t slide over each other, therefore alloys are harder than pure metals.

20
Q

What are the limitations of the simple model?

A

There are no forces between spenders and atoms, molecules, and ions are solid sphere - this is not true.

21
Q

What does the amount of energy needed to change state from solid to liquid or liquid to gas depend on?

A

The strength of the forces between the particles of the substance. The nature of the particles involved depends on the type of bonding and the structure of the substance.

22
Q

A pure substance will melt or boil at…?

A

A fixed temperature.
A mixture will melt over a range of temperature.

23
Q

What are the 3 states of matter?

A

Solid
Liquid
Gas

24
Q

State 4 uses of Nanoparticles.

A

Medicine
Electronics
Deodorants
Sun creams

25
Q

What are fine and coarse particles?

A

Fine particles: 100-2500nm diameter.
Coarse particles: 2500-10^5nm diameter.

26
Q

Why do Nanoparticles have different properties to those for the same materials in bulk?

A

High surface area to volume ratio.

Chemistry (2 decks)

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