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GCSE Edexcel Separate Chemistry > SC5 Ionic Bonding > Flashcards

SC5 Ionic Bonding Flashcards

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1
Q

Define ‘bonds’

A

Forces of attraction that hold atoms together

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2
Q

Define ion

A

An atom or a group of atoms with a positive or negative charge

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3
Q

How do ions form?

A

When atoms gain or lose electrons in their outermost shell

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4
Q

What kind of ions do metals form?

A

Cations: positively charged, because they tend to lose electrons

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5
Q

What kind of ions do non-metals form?

A

Anions: negatively charged, because they tend to gain electrons

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6
Q

Explain the what dot and cross diagrams are

A
  • models the transfer of electrons between two atoms
  • one atom will have electrons represented by dots
  • and the other will have electrons represented by a cross
  • the non-metal will gain electrons, which will be different to the shapes used to represent its own electrons
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7
Q

Describe the limitations in dot and cross diagrams.

A

Doesn’t show the three-dimensional shape of the molecule.

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8
Q

Why do ionic bonds occur?

A

So that atoms can gain a full outer shell

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9
Q

What is an ionic lattice?

A

The regular arrangement of ions in an ionic substance

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10
Q

How do we work out the number of electrons in an ionic substance?

A
  • Work out how many electrons a neutral atom would have (same as the proton number)
  • Work out how many electrons have been lost or gained
  • -ve means electrons have been gained
  • +ve means electrons have been lost
  • Calculate the number of ions in an atom plus electrons gained or minus electrons lost
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11
Q

How will elements in group 1 form ions?

A

They will lose the electron in their outermost shell and form 1+ ions

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12
Q

How will elements in group 2 form ions?

A

They will lose the two electrons in their outermost shell and form 2+ ions

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13
Q

How will elements in group 6 form ions?

A

They will gain two electrons in their outermost shell and form 2- ions

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14
Q

Why is the ionic lattice formed in ionic substances?

A

Ions attract each other and form a regular pattern with oppositely charged ions next to each other

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15
Q

What are ionic bonds?

A

Strong electrostatic forces between oppositely charged ions, which spread in all directions within an ionic lattice

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16
Q

Describe some properties of ionic compounds

A
  • high melting and boiling points
  • can conduct electricity when molten
17
Q

What are the two conditions that a substance has to meet for it to be able to conduct electricity?

A
  • must contain charged particles
  • particles must be able to move freely
18
Q

Why do ionic substances have high melting and boiling points?

A
  • electrostatic forces of attraction between oppositely charged ions are strong
  • a lot of energy is required to overtake these bonds in order to separate and melt the lattice structure
  • therefore requiring high temperatures
19
Q

Why can ionic substances only conduct electricity when molten?

A

The ions are free to move and carry charge

20
Q

When are the endings -ate and -ide used?

A

Used for the negatively charged ions in the compound

21
Q

What does the ending -ate mean a compound contains?

A

3 elements, one of which is oxygen

22
Q

What does the ending -ide mean a compound contains?

A

2 elements, one of which is a non-metal

23
Q

Name some examples of compounds ending in -ide

A
  • sodium chloride
  • magnesium oxide
  • calcium sulphide
  • potassium iodide
  • ions sulfide
24
Q

Name some examples of compounds ending in -ate

A
  • magnesium carbonate
  • sodium nitrate
  • copper sulphate
  • potassium iodate
  • iron sulphate
25
Q

Why don’t ionic compounds conduct electricity as a solid?

A

The charged particles (ions) are unable to move around and therefore wouldn’t be able to carry the charge

26
Q

What is the ionic formula of oxygen?

A

O ^2-

27
Q

What is the ionic formula of hydroxide?

A

OH^1-

28
Q

What is the ionic formula of nitrate?

A

N03^1-

29
Q

What is the ionic formula of carbonate?

A

CO3^2-

30
Q

What is the ionic formula of sulphate?

A

SO4^2-

31
Q

How do you deduce the charges of ionic compounds?

A

Balance the charges of both the ionic compounds involved to make the overall charge 0.

32
Q

What is the ionic formula of ammonium?

A

NH+4

33
Q

What is the ionic formula of calcium?

A

Ca2+

34
Q

What is the ionic formula of sodium?

A

NA+

35
Q

What is the ionic formula of lead?

A

Pb2+

GCSE Edexcel Separate Chemistry (23 decks)

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