Topic 4 Structures Flashcards Preview

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Flashcards in Topic 4 Structures Deck (27):
1

Give 4 properties of Giant Ionic Lattices?

Crystalline
High Melting and Boiling Point
Conducts electricity when liquid, molten or dissolved in water
Soluble in water

2

Why do Giant Ionic Lattices have such high melting and boiling points?

The ionic bonds are very strong, and bond breaking is an endothermic reaction therefore lots of heat/energy is required to break these bonds

3

Why do Giant Ionic Lattices conduct electricity when molten, liquid or dissolved in water?

The attractions between the ions are overcome, allowing ions to move freely and carry current

4

Give 4 properties of Simple Covalent structures?

Low melting and boiling point
Don't conduct electricity
Not soluble in water
Soft when solid

5

Why do Simple Covalent structures have low melting and boiling points?

The Van Der Waal forces between the simple covalent molecules are very weak, meaning very little heat/energy is required to depart the molecules

6

Why don't Simple Covalent Molecules conduct electricity?

There are no free electrons and molecules don't have any charges

7

Give 3 examples of Simple Covalent Structures?

Chlorine
Carbon Dioxide
Water

8

What is an allotrope?

Different form of same element in same physical state

9

Give 2 allotropes that are Giant Covalent Molecules?

Diamond
Graphite

10

Give 4 properties of Diamond?

Very high melting and boiling point
Doesn't conduct electricity
Insoluble in water
Extremely hard solid

11

Give 4 properties of Graphite?

Very high melting and boiling point
Conducts electricity
Insoluble in water
Slippery soft solid

12

Why doesn't diamond conduct electricity?

No free electrons or ions to carry charge

13

Why does Diamond have such high melting and boiling point?

The carbon atoms in diamond are held together by very strong covalent bonds

14

Why does Graphite conduct electricity?

There are delocalised electrons between the layers of graphite so current can be carried by these electrons

15

Why is Graphite so soft and slippery?

Th weak Van Der Waal Forces between the layers of Graphite allow the layers to slide over each other

16

Why does Graohite have such a high melting and boiling point?

Although the Van Der Waal forces between the layers are very weak, the string covalent bonds in the hexagonal layers are extremely difficult to break

17

Give one use of Diamond?

Diamond can be used for cutting tools, such as glass cutters or drill bits

18

Give one use of Graphite?

Graphite can be used as a lubricant, as the layers are able to slide over each other making it very soft and slippery. This lubricant can be used on machinery

19

Give 5 properties of Metallic Structures?

High Melting Point and Boiling Point
Dense and Strong
Conducts heat and electricity
Malleable
Ductile

20

Why do Meatllic Structures conduct electricity?

The delocalised electrons can move freely and can carry current

21

Why do Metallic Structures have such high melting and boiling points?

The strong bond between positive metal ions and negative delocalised electrons is very hard to break, although in some metals can be
relatively weak, such as in Potassium or Sodium

22

Why are Metallic Structures Malleable and Ductile?

The layers can slide over each other when force is applied, also delocalised electrons move between the metal ions and hold together the structure when bent or stretched

23

Give 2 uses of Aluminium?

Overhead electrical wiring
Alloys for aircraft

24

Give 4 uses of copper?

Electrical wiring
Plumbing
Brass
Coinage

25

Give 2 uses of iron?

Bridges
Structures

26

Give 2 uses of Magnesium?

Flares
High strength alloys in aircraft

27

Name 2 examples of Giant Ionic Lattices?

Sodium Chloride
Magnesium Oxide