C3 Structure And Bonding Flashcards

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1
Q

What is ionic bonding

A

Ionic compounds are held together by strong forces of attraction between their oppositely charged ions

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2
Q

How are electrons transferred between a magnesium atom and oxygen atom

A

The magnesium atom has 2 electrons on its outermost shell which it wants to lose but oxygen has 6 and wants to gain 2 so the magnesium’s electrons go to the oxygen atom

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3
Q

What ions do group 1 form

A

1+

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4
Q

What ions do group 2 form

A

2+

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5
Q

What ions do group 3 form

A

3+

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6
Q

What ions do group 4 form

A

Do not form ions

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7
Q

What ions do group 5 form

A

3-

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8
Q

What ions do group 6 form

A

2-

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9
Q

What ions do group 7 form

A

1-

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10
Q

What ions do group 0 form

A

Never form ions in compounds

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11
Q

Why do ionic compounds have high melting points

A

The ionic bonds are very strong and operate in all directions which hold a giant ionic lattice together meaning it takes a lot of energy to break them

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12
Q

What are ionic compounds at room temperature

A

Solids

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13
Q

When and why will ionic compounds conduct electricity

A

When molten or dissolved in water. This is because their ions can then become mobile and can carry charge through the liquid

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14
Q

Why are convalent bonds formed

A

Atoms of non-metals share pairs of electrons with each other

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15
Q

Why do atoms convalently bond with other atoms

A

To gain more stability, which is gained by forming a full electron shell

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16
Q

How do the pairs of electrons in convalent bonding bond the atoms together

A

Electrostatic attraction between electrons and positive nuclei on either side of the pair of electrons

17
Q

Why do convalent compounds have low boiling and melting points

A

They have strong convalent bonds yet the intermolecular forces between molecules are weak therefore meaning it doesn’t require much energy to seperate.

18
Q

Do simple molecules conduct electricity

A

No as they have no overall charge meaning they cannot carry electrical charge.

19
Q

What are polymers

A

A substance or material which are made up of many small reactive molecules that bond to each other to form long chains

20
Q

Properties of giant convalent structures

A

-They have very high melting and boiling points.
-They are insoluble in water
-Apart from graphite, they are hard and don’t conduct electricity.

21
Q

What are giant convalent structures

A

Huge networks of atoms held together by convalent bonds

22
Q

Why can graphite conduct electricity

A

Graphite’s layers are arranged in hexagons, each carbon atom forms three strong convalent bonds. Carbon atoms have 4 electrons in the outer shell meaning there is one spare on each atom in graphite. These delocalised electrons move freely across the layers and allow graphite to conduct electricity

23
Q

Why is graphite used for pencils

A

As there are no convalent bonds between the layers only weak intermolecular forces the layers can slide over each other easily which can transfer on to paper.

24
Q

What are fullerenes

A

Large cage like structures and tubes, based on hexagonal rings of carbon atoms

25
Q

What are fullerenes used for

A

A transport mechanism for drugs to specific sites in the body

26
Q

Difference between graphene and graphite

A

Graphene is a single layer of graphite so it is one atom think

27
Q

Properties of graphene

A

-excellent electrical conductivity
-incredibly strong for there mass
-very low density

28
Q

How are metal atoms structured

A

Closely packed together and arranged in regular layers.

29
Q

What is metallic bonding

A

The electrostatic attraction between positive metal ions and delocalised electrons

30
Q

What is an alloy

A

A mixture of metals