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chemistry (paper one) > ionic bonding (topic 2) > Flashcards

ionic bonding (topic 2) Flashcards

1
Q

(4)

A
  • one sodium atom loses one electron
  • chlorine gain one electron
  • sodium ion has an electron configuration of 2,8
  • chloride ion has an electron configuration 2,8,8
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2
Q

explain why ionic compounds are usually solid at room temperature (2)

A
  • strong electrostatic forces
  • which require a lot of energy to overcome
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3
Q

electronic configuration of Na is 2,8,1

A
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4
Q

give the formula of sodium oxide

A
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5
Q

draw a dot and cross diagram to show how magnesium and chlorine form magnesium chloride

A
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6
Q

name the type of bonding in magnesium chloride

A

ionic

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7
Q

chem formula of sodium fluoride

A

NaF

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8
Q

describe the structure of a sodium fluoride crystal (2)

A
  • the sodium and fluoride ions are arranged in a regular giant ionic lattice
  • there are very strong electrostatic forces of attraction between the ions, acting in all directions
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9
Q

explain why solid sodium fluoride cannot conduct electricity

A
  • solid sodium fluoride does not have any delocalised electrons
  • the sodium and fluoride ions are unable to move
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10
Q
A
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11
Q

describe what happens to its electrons when a calcium atom forms a calcium ion, state the charge on the calcium ion formed (4)

A
  • two electrons
  • are lost by the calcium atom
  • to get a full outer shell
  • calcium ions are 2+
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12
Q

describe what happens to its electrons when an oxygen atom forms an oxygen ion, state the charge on the oxygen ion formed (3)

A
  • two electrons
  • are gained by the oxygen atom
  • to get a full outer shell
  • oxygen ions are 2-
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13
Q

why do ionic compounds have high melting points (2)

A
  • they are held together by many strong forces
  • a lot of energy is required to break these forces
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14
Q

Na = 2,81
S = 2,86

A
  • one outer shell electron from each sodium atom
  • is transferred to the sulfur atom
  • the sulfur atom gains two electrons
  • each sodium atom becomes a sodium ion, Na+
  • the sulfur atom becomes a sulfide ion, S2-
  • both atoms achieve a full outer shell configuration
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15
Q
A
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16
Q

(3)

A
  • B
  • there are two potassium ions for each sulfide ion in K2S
  • in A there are 14 large spheres and 13 smaller ones, giving a ratio of 1:1
  • in B there are 14 large spheres and 8 smaller ones, giving a ratio of 2:1
17
Q

the ball and stick model is not a true representation of the structure of potassium sulfide, give one reason why (1)

A

there are no gaps between the potassium and sulfide ions

18
Q
A

it has a high melting point

19
Q
A
20
Q

which ion is represented by the (-) charge, and which ion is represented by the (+) charge in sodium chloride (1)

A

sodium is represented by the + charge chloride is represented by the - charge

21
Q

give two limitations of a two-dimensional diagram like the one above

A
  • it is not to scale
  • it gives no information about the forces of attraction between the ions
  • it does not show where the ions are located on the other layers
22
Q

write the electron configuration of an atom of aluminium and an atom of fluorine

A

aluminium: 2,8,3
fluorine: 2,7

23
Q

draw a ‘dot and cross’ diagram to show how aluminium and fluorine form aluminium fluoride:
aluminium: 2,8,3
fluorine: 2,7

A
24
Q

give one limitation of ‘dot and cross’ diagrams

A
  • it does not show how the ions are arranged in space
  • it does not show the ions in an ionic lattice
25
Q

what is an ion (1)

A

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

26
Q

(4)

A
  • metal atoms lose electrons
  • neutral metal atoms become positively charged ions
  • non-metal atoms gain electrons
  • neutral non-metal atoms become negatively charged ions
27
Q
A
  • NaCl contains Na+ and Cl- ions
  • MgO contains Mg2+ and O2- ions
  • the strength of ionic bonds depends on the charge on the ions
  • ionic bonds between Mg2+ and O2- ions are stronger than those between Na+ and Cl- ions
  • more energy is needed to overcome the forces between Mg2+ and O2- ions
28
Q
A
29
Q

describe how giant ionic lattices are held together (3)

A
  • held together by strong electrostatic forces of attraction
  • acting in all directions
  • between oppositely charged ions
30
Q

explain why ionic compounds have high melting and boiling points (2)

A
  • large amount of energy required
  • to break the many strong bonds in the giant ionic lattice

chemistry (paper one) (24 decks)

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