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IGCSE Chemistry EDEXCEL > Summer Assessments 2 > Flashcards

Summer Assessments 2 Flashcards

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1
Q

What are ions

A

charged particles

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2
Q

Why do atoms lose/ gain electrons

A

to form ions as they are trying to get a full outer shell as atoms with a full outer shell are very stable

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3
Q

What are negative ions and when do they form

A

anions

-form when atoms gain electrons

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4
Q

What are positive ions and when do they form

A

cations

-form when atoms lose electrons

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5
Q

What are the charges for metals in Groups 1, 2, 3

A

-lose electrons to form positive ions so:
Group 1 elements form 1+ ions
Group 2 elements form 2+ ions
Group 3 elements form 3+ ions

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6
Q

What are the charges for non-metals in Groups 5, 6, 7

A

-non-metals gain electrons to form negative ions so:
Group 5 elements form 3- ions
Group 6 elements form 2- ions
Group 7 elements form 1- ions

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7
Q

Name 6 ions and there charges that go against the normal

A 
Ag+
Cu2+
Fe2+
Fe3+
Pb2+
Zn2+
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8
Q

Name 6 elements and there charges that go against the normal idea

A

Hydrogen (H+), hydroxide (OH–), ammonium (NH4+), carbonate (CO32–),
nitrate (NO3-)
sulfate (SO42–).

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9
Q

What does ionic bonding involve

A

a metal and a non-metal

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10
Q

Describe ionic bonding in terms of electrostatic attractions

A

Ionic bonding is the electrostatic attraction between oppositely charged ions

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11
Q

Why do compounds with giant ionic lattices have high melting and boiling
points

A

ions are held together in a closely packed 3D lattice arrangement by the attraction between oppositely charged ions

  • the electrostatic attraction between oppositely charged ions is very strong
  • as a result of this a lot of energy is needed to overcome the strong attraction
  • hence why ionic compounds have high melting and boiling point
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12
Q

When can ionic compounds conduct electricity

A
  • conduct
    electricity when molten and in aqueous solution

-can’t conduct electricity when solid

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13
Q

Name the 3 physical properties of ionic compounds

A
  • high melting point
  • high boiling point
  • can conduct electricity when molten or when dissolved in water
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14
Q

What do compounds with ionic bonding always have

A

giant ionic structure

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15
Q

What diagram is used to show the transfer of electrons in ionic bondidng

A

A dot and cross diagram

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16
Q

Describe covalent bonding in terms of electrostatic attractions

A

Covalent bonding is the electrostatic attraction between negatively charged shared electrons

17
Q

What is a covalent bond

A

A shared pair of electrons

18
Q

Why are substances with a simple molecular structure gases or liquids, or
solids with low melting and boiling points

A
  • atoms within a molecule are held together by very strong covalent bonds
  • the molecular forces of attraction between the molecules are very weak
  • therefore the melting and boiling point for simple molecular substances are very low as the molecules are easily separated
19
Q

explain why the melting and boiling points of substances with simple molecular
structures increase, in general, with increasing relative molecular mass

A
  • intermolecular forces are stronger between molecules with high relative molecular mass (Mr) than between smaller molecules
  • as there are more points along larger molecules for intermolecular forces to act between them
  • so more energy is needed to break the forces
  • due to increasing strength of the forces, melting and boiling pints of simple molecular substances increase as the relative molecular mass increases
20
Q

How are giant covalent structures bonded to each other

A

-strong covalent bonds

21
Q

explain why substances with giant covalent structures are solids with high melting and
boiling points

A
  • giant covalent structures bonded to each other by strong covalent bonds
  • there are lots of these bonds so it takes a lot of energy to break them
  • hence why giant covalent structures are solids with high melting and boiling points
22
Q

Do Giant Covalent Structures conduct electricity

A

No- not even when molten

23
Q

Why does diamond have a high melting and boiling point

A
  • diamond is made up of a network of carbon atoms that each form 4 covalent bonds
  • the strong covalent bonds take lots of energy to break, so diamond has a high melting point
24
Q

Why is diamond hard

A

as the strong covalent bonds hold the electrons in a very rigid lattice structure

25
Q

Why doesn’t diamond conduct electricity

A

as it has no free electrons or ions

26
Q

Name the 3 physical properties of diamond

A
  • high melting point
  • its hard
  • doesn’t conduct electricty
27
Q

Why is graphite soft and slippery

A
  • as in graphite each carbon atom only forms three covalent bonds, creating layers of carbon atoms
  • layers are held together weakly by intermolecular forces of attraction so are free to slide over each other
  • this makes graphite soft and slippery
28
Q

Why does graphite have a high melting point

A

As the covalent bonds in layers require lots of energy to break

29
Q

Why does graphite conduct electricity

A

As only three out of each of carbon’s four outer electrons are used in bonds, so each carbon atom has one electron that is delocalised (free) and can move

-hence why graphite conduct electricity

30
Q

Name 2 giant covalent structures

A
  • Graphite

- Diamond

31
Q

Do covalent compounds conduct electricity

A

not usually

32
Q

Are giant covalent structures soluble in water

A

no- insoluble

33
Q

Name a simple molecular substance

A

C60 fullerene

34
Q

Why is C60 fullerene soft

A

The C60 covalent molecules are held together by intermolecular forces and so can slide over each other, hence why C60 fullerene is soft

35
Q

Why is C60 fullerene a poor conductor of electricity

A

Each carbon in C60 fullerene has one delocalised electron

-however, the electrons can’t move between molecules, hence why c60 fullerene is a poor conductor of electricity

36
Q

Name the 3 physical properties of graphite

A
  • soft, slippery
  • high melting point
  • conducts electricity
37
Q

Name the 2 physical properties of C60 fullerene

A
  • soft

- poor conductor of electricity

IGCSE Chemistry EDEXCEL (14 decks)

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