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Chemistry Year 11 Content > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

What is ionic bonding?

A

Ionic bonding involves an attraction between oppositely charged ions.

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2
Q

Where are ionic bonds found?

A

Found in compounds made from metal and non-metals.

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3
Q

What is covalent bonding?

A

Covalent bonding involves 2 atoms sharing one or more pairs of electrons.

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4
Q

Where are covalent bonds found?

A

Found in most non-metal elements and in compounds of non-metals.

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5
Q

What is metallic bonding?

A

Metallic bonding involves an attraction between positively charged ions and negatively charged delocalised electrons.

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6
Q

Where are metallic bonds found?

A

Found in metals and alloys (mixtures of metals and other substances).

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7
Q

How many types of chemical bond are there and name these:

A

3: Covalent, metallic and ionic.

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8
Q

Which type of bonding happens in most non-metal elements?

A

Covalent.

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9
Q

What are ions?

A

Ion are charged particles. They are created when an atom or molecule gains or loses electrons.

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10
Q

How are ions created?

A

Gaining electrons creates a negatively charged ion; losing electrons creates a positively charged ion.

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11
Q

How are positive ions created?

A

Usually created when an atom or molecule loses electrons.

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12
Q

What can positive ions also be called?

A

Cations.

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13
Q

The metals in group 1 and 2 can easily lose..

A

…electrons to become positively charged ions.

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14
Q

How are negative ions created?

A

When an atom or molecule gains electrons.

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15
Q

What are negative ions also called?

A

Anions.

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16
Q

The non-metals in group 7 are most likely to…

A

…gain electrons to fill up their electrons shell and become negatively charged.

17
Q

Ions can be:

A 
Single elements (eg F-) 
A group of element with an overall charge (eg SO42-)
18
Q

How does the nucleus of an atom change when it gains electrons?

A

It doesn’t.

19
Q

Positive ions are usually made when an atom or molecule…

A

loses electrons.

20
Q

What happens when atoms form ions?

A

They try to fill up or empty their outer electron shell.

21
Q

How do group 1 metals form ions?

A

Always lose 1 electron to form positive ions with a charge of +1.

22
Q

How do group 2 metals form ions?

A

Always lose 2 electrons to form doubly positive ions.

23
Q

How do non-metals form ions (groups 6 and 7)?

A

Always gain electrons to form (become) negative ions.

24
Q

How do noble gases (group 0) form ions?

A

Already have a full outer shell so are unreactive and don’t normally form ionic bonds with other elements.

25
Q

Materials with ionic bonds usually…

A

Only conduct electricity when molten/dissolved.

Have high melting points.

26
Q

Sodium is in group 1 and oxygen is in group 6. In the dot-and-cross diagram for sodium oxide, how many sodium ions would there be?

A

2.

27
Q

Through which diagram can we show the transfer of electrons and ions formed?

A

Dot and cross diagrams.

28
Q

What is an ionic compound?

A

When millions of metal atoms transfer their outer electrons to millions of non-metal atoms at the same time, resulting in oppositely charged ions held together in ionic lattices.

29
Q

What is an ionic lattice?

A

Giant structures that are held together by strong electrostatic forces between oppositely charged ions.

30
Q

What are electrostatic forces?

A

Called ionic bonds that extend in all directions within the lattice.

31
Q

What does an empirical formulae help us to do?

A

Helps us to work out the proportion of each ion in a compound and is the simplest ratio of ions possible of an ionic compound.

32
Q

What is the empirical formulae of Ca2+ and F- ions?

A

In order for the charges to balance out and for the overall formula to be neutral, there must be 2 F- ions for each Ca2+ ion.
The empirical formula is CaF2.

33
Q

Facts about ionic lattices…

A

Giant structures.
Held together by electrostatic forces.
Contain negatively charged non-metal ions.
Contain positively charged metal ions.

34
Q

Why are Covalent bonds strong?

A

Because the shared electrons are attracted to the nucleus of both atoms.

35
Q

Covalently bonded substance can be:

A 
Small molecules (water) 
Large molecules (such as polyester and silk) 
Giant covalent structures (diamond)
36
Q

Describe the structure of an metal:

A

Giant structures of regularly arranged electrons. A regular lattice of cations in a ‘sea’ of delocalised electrons.

37
Q

What are delocalised electrons?

A

Not bound to an atom and are free to move around the lattice.

38
Q

Why does delocalisation happen?

A

Metal atoms have a smaller amount of electrons in their outer shells.

Chemistry Year 11 Content (9 decks)

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