Types Of Substance Flashcards

1
Q

What structure do ionic compounds have?

A

Giant ionic lattice. Ions form a closely packed regular lattice which strong electrostatic forces of attraction between oppositely charged charged ions.

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2
Q

What are the properties of ionic compounds?

A

High melting + boiling point due to strong attraction. Don’t conduct electricity unless melted as ions can’t move. Dissolve easily in water and can carry electric current in solution as ions separate.

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3
Q

What is the structure of substances containing covalent bonds?

A

Have simple molecular structures + atoms within the molecules are held together by very strong covalent bonds but the forces of attraction between these molecules are very weak

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4
Q

What are the properties of simple molecular substances?

A

Low melting + boiling points as only need to break the intermolecular forces not covalent bonds. Don’t conduct electricity as no free electrons or ions. Some are soluble /aren’t in water

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5
Q

What are the properties of giant covalent structures?

A

All atoms are bonded to each other by strong covalent bonds. High MP + BP. Generally don’t contain charged particles so don’t conduct electricity. Aren’t soluble in water.

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6
Q

What is the structure of metallic compounds?

A

Giant structure, delocalised electrons in outer shell of metal atoms. Strong forces of electrostatic attraction between positive metal ions + negative electrons.

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7
Q

What are the properties of metals?

A

Most compounds with metallic bonds have high BP/MP. Shiny solids. Aren’t soluble in water. Layers of atoms slide over each other so they’re malleable. Good conductors of electricity + heat due to delocalised electrons.

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8
Q

What are some examples of carbon based giant covalent structures?

A

Diamond, graphite, graphene.

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9
Q

What is the structure of diamond?

A

Strong covalent bonds hold the atoms in a rigid lattice structure making diamond really hard - used to strengthen cutting tools. Doesn’t conduct electricity as no free electrons or ions

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10
Q

What is the structure of graphite?

A

Layers of carbon atoms arranged in hexagons. Free to move over each other so it’s a good lubricating material. Conducts electricity. High MP

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11
Q

Why is graphite used to make electrodes?

A

Only 3 out of carbons 4 outer electrons are used in bonds so each carbon atom has 1 delocalised electrons to carry charge.

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12
Q

Why is graphite a good lubricant?

A

Because there’s no covalent bonds between the layers so they’re slippery.

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13
Q

What are fullerenes?

A

Molecules of carbon shaped like closed tubes or hollow balls.

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14
Q

What are some properties of graphene?

A

Conduct electricity, tensile strength so can strengthen materials without adding much weight.

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15
Q

Properties of fullerenes

A

Huge surface area so could help make industrial catalysts

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16
Q

What is C60?

A

A fullerene that forms a hollow sphere make up of 20 hexagons + 12 pentagons. Stable molecule that forms soft brownish/black crystals.

17
Q

What are polymers?

A

Molecules made up of long chains of covalently bonded carbon atoms eg polyethene.

18
Q

What are the differences between metals + non metals properties?

A

metals are shiny solids which have high MP, high density and are good conductors of electricity but most non-metals have low BP and are poor conductors of electricity

19
Q

What are the limitations of 2D models?

A

Don’t show shape of substance + don’t show sizes of the atoms

20
Q

What are the limitations of dot and cross diagrams?

A

Don’t show size of atoms/ions or how they’re arranged

21
Q

What are the limitations of 3D models?

A

Only show the outer layer of arrangement of ions on the substance

22
Q

What are the limitations of ball + stick models?

A

Make it look like there’s big gaps between atoms. Don’t show correct scales of atoms or ions.