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GCSE Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is an ionic bond?

A

An electrostatic force holding oppositely charged atoms together, between at least one metal and non metal (unless involving hydrogen)

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2
Q

What is transferred in an ionic bond?

A

Electrons

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3
Q

What is the result of an ionic bond in terms of electrons?

A

Atoms having full outer shells of electrons

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4
Q

Do ions have high or low melting and boiling points? Why?

A

High melting points because they have strong electrostatic bonds that require lots of energy to break

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5
Q

What are intermolecular forces?

A

The forces holding separate atoms, compounds or molecules together

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6
Q

What are intramolecular forces?

A

The forces holding atoms that make up a molecule or compound together

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7
Q

What are ionic, covalent and metallic bonds examples of?

A

Intermolecular bonds

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8
Q

When can ions conduct electricity? Why?

A

Ions only conduct electricity when they are not solid, since the ions can move more.

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9
Q

Are ionic compounds soluble in water?

A

Yes

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10
Q

What is a covalent bond?

A

The electrostatic force between a positive nucleus and a bonding pair of electrons

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11
Q

What is the valence shell?

A

The outer shell

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12
Q

What happens to electrons in a covalent bond?

A

They are shared between atoms to form full outer shells

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13
Q

Do simple covalent compounds have high or low melting and boiling points? Why?

A

Low melting points because they have weak intermolecular forces that require little energy to break

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14
Q

Do covalent compounds dissolve in water?

A

No

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15
Q

What is diamond made from?

A

Carbon

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16
Q

What is graphite made from?

A

Carbon

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17
Q

What is buckminsterfullerene made from?

A

Carbon

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18
Q

Do diamonds conduct electricity? Why?

A

No since it has no delocalised electrons

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19
Q

Does graphite conduct electricity? Why?

A

Yes, since it has delocalised (free) electrons

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20
Q

Does buckminsterfullerene conduct electricity? Why?

A

Yes, since it has delocalised (free) electrons

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21
Q

Do diamonds have high or low melting and boiling points? Why?

A

High, since it has strong covalent bonds which require lots of energy to break

22
Q

Describe the structure of a diamond

A

Tetrahedral structure

23
Q

How is graphite arranged?

A

In layers

24
Q

How many other atoms does each atom bond to in graphite?

A

3

25
Q

How many other atoms does each atom bond to in diamonds?

A

4

26
Q

Does graphite have high or low melting and boiling points? Why?

A

High, since it has strong covalent bonds which require lots of energy to break

27
Q

Does buckminsterfullerene have high or low melting and boiling points? Why?

A

Low, since it has weak covalent bonds which require little energy to break compared to other giant covalent structures, but high compared to other compounds

28
Q

Are diamonds hard or soft?

A

Very hard

29
Q

Is graphite hard of soft?

A

Soft

30
Q

Is buckminsterfullerene hard or soft?

A

Very hard

31
Q

Diamond, graphite and buckminsterfullerene are examples of…

A

Giant covalent compounds

32
Q

Name some properties of metals

A
  • Sonorous
  • Shiny
  • Dense
  • Good conductors of heat and electricity
  • Malleable
  • Hard
33
Q

What is a metallic bond?

A

The electrostatic force between positive metal ions and their delocalised electrons

34
Q

In metallic bonding, how are metal ions arranged?

A

In layers that can slide over each other

35
Q

Which of these metal chlorides are insoluble in water?

A) copper chloride
B) lead chloride
C) magnesium chloride
D) potassium chloride

A

B) lead chloride

36
Q

Do metallic compounds have high or low melting and boiling points? Why?

A

High melting points because they have strong electrostatic bonds that require lots of energy to break

37
Q

What is the total number of atoms in Al(NO3)3

A

13

38
Q

Do simple covalent compounds conduct electricity? Why?

A

No, because they have nothing to carry an electrical charge

39
Q

Name 3 giant covalent compounds

A
  • Diamond
  • Graphite
  • Buckminsterfullerine
40
Q

What are diamonds, graphite and buckminsterfullerene examples of?

A

Giant covalent compounds

41
Q

What ions do group 1 elements form?

A

+1

42
Q

What ions do group 2 elements form?

A

+2

43
Q

What ions do group 0 elements form?

A

They do not form ions

44
Q

What ions do group 7 elements form?

A

-1

45
Q

What ions do group 6 elements form?

A

-2

46
Q

Name the 7 diatomic elements

A
  • Hydrogen
  • Oxygen
  • Nitrogen
  • Fluorine
  • Bromine
  • Iodine
  • Chlorine
47
Q

How are electrons arranged in a metallic bond?

A

A sea of electrons surrounding the positive metal ions

48
Q

Do metallic compounds conduct electricity? Why?

A

Yes, since it has delocalised electrons

49
Q

Are covalent compounds soluble in water?

A

No

50
Q

Are metallic compounds soluble in water?

A

No

51
Q

What structure to all ionic compounds form?

A

A giant ionic lattice

52
Q

What structure do all metallic compounds form?

A

Giant metallic lattices

GCSE Chemistry (16 decks)

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