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chemestry > C2 New Version > Flashcards

C2 New Version Flashcards

1
Q

Why do metal have high melting point

A

Because lots of heat energy is needed to overcome strong electrostatic attraction between many positive ions and negative electrons

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2
Q

Why do non metals have a low melting point

A

It does not take a lot of heat to overcome the weak attraction

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3
Q

What is metallic bonding

A

A strong electrostatic attraction between positive ions and negative delocalised electrons

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4
Q

Ionic bonding

A

A non metals and metals loses or gains electrons to obtain a full outer shell

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5
Q

Covalent

A

When two or more non metals share electrons to obtain a full outer shell

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6
Q

Metals are malleable

A

Because the layers of ions can slide past

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7
Q

Metals are good conductors

A

Because free elections carry charge

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8
Q

Alloys are harder

A

Because different sizes makes the layers distorted and Cannot slide past each other

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9
Q

Alloys have high melting points because

A

Lots of energy is needed to overcome the strong electrostatic attraction between the positive ions and negative electrons

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10
Q

Alloys are good conductors

A

Because free elections can move and carry charge

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11
Q

Ionic compound have a high melting point

A

Because lots of energy is needed to overcome the strong electrostatic attraction between the positive ions and negative ions

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12
Q

Describe ionic bond

A

Electron transfers from metal to non metal to have full outer shell

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13
Q

Why do small covalent structures have a low boiling point

A

Little bit energy is needed to overcome weak intermolecular forces

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14
Q

Why are Small covalent properties soft

A

Weak intermolecular forces

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15
Q

Why do small covalent particles have poor electrical conductors

A

Because molecules are neutral

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16
Q

Why do diamonds have high melting boiling points

A

Needs lots of energy to overcome strong covalent

17
Q

Why are diamonds very hard

A

Giant structure of strong covalent bonds so layers cannot slide

18
Q

Why do diamonds not conduct electricity

A

No delocalised electrons the Carry charge

19
Q

Why do diamonds have a crystal structure

A

4 covalent bonds to each atom in tetrahedral structure

20
Q

Why does graphite have a high melting and a boiling point

A

Needs a lot of energy to overcome strong covalent bonds

21
Q

Why is graphite soft

A

Layers of atoms can slide past each other because of weak intermolecular forces

22
Q

Why is graphite a good electrical conductor

A

Because of delocalised electrons can move and carry charge

23
Q

Why does graphite rub off into paper

A

3 covalent bonds to each atom in hexagonal layers

24
Q

Why does silicone have a crystal structure

A

Covalent bonds in tetrahedral structure

25
Q

Why does silicone have a high melting and boiling point

A

Lots of energy needed to overcome strong covalent bonds

26
Q

Why is silicone very hard

A

Layers are distorted and can’t slide past each other

27
Q

Why is silicone a poor conductor

A

No delocalised elections are free and can carry charge

28
Q

What are the properties of metal

A

Malleable/ductile,good conductors
High melting points

29
Q

What are the properties of alloys

A

High melting point. Harder. Good conductors

30
Q

What are the properties of ionic compounds

A

High melting points Brittle. Do not conduct electricity when solid. Do conduct electricity when liquid

31
Q

What are the properties of covalent bonds

A

Lower melting boiling point Soft Poor electrical conductor

32
Q

What are the properties of diamonds

A

High melting and boiling points does not conduct electricity hard crystal structures

33
Q

What are the properties of graphite

A

Soft high melting and boiling points points good electrical conductor layers will rub of paper

34
Q

What are the properties of silicon oxide

A

Crystal structure high melting and boiling point hard poor electrical conductors

chemestry (4 decks)

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