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Chemistry > C2 - Bonding, Structure and Properties of Matter > Flashcards

C2 - Bonding, Structure and Properties of Matter Flashcards

1
Q

Where are OH⁻ ions found

A

In alkalis

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2
Q

Charge of non-metal ions

A

Negative

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3
Q

Where are H⁺ ions found

A

Acids

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4
Q

Why can’t ions with negative charges form ionic bonds with each other

A

They repel

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5
Q

Structure of simple covalent molecules

A
  • Strong covalent bonds between atoms
  • Weak forces holding the molecules together
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6
Q

3 giant covalent structures

A

Diamond

Graphite

Silicon dioxide

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7
Q

How many bonds per carbon in diamond

A

4

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8
Q

Why don’t most covalent structures conduct electricity

A

There are no electrons/ions/charged particles free to move

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9
Q

Melting points of ionic substances

A

High

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10
Q

Structure of giant ionic lattice

A

3D network of alternating positive and negative ions held together by electrostatic forces of attraction

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11
Q

What substances ionic bond

A

Metals with Non-metals

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12
Q

What substances covalent bond

A

Non-metals

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13
Q

Structure of metals

A

Positive metal ions in a sea of delocalised electrons

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14
Q

How does graphite conduct electricity

A

Each carbon has 3 bonds so one electron is delocalised to move through the graphite and carry a charge

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15
Q

Graphene

A

Single layer of graphite

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16
Q

Fullerene

A

Molecules of carbon shaped like hollow balls

17
Q

Why can graphite act as a lubricant

A

Layers are free to slide over each other as the forces holding them together are weak

18
Q

Why do ionic compounds not conduct electricity when solid

A

Ions are not free to move and carry charge/they don’t have delocalised electrons to carry a charge

19
Q

Structure formed when metals and non-metals react together

A

Giant ionic lattice

20
Q

How are ions attracted to each other

A

Electrostatic force of attraction

21
Q

Will NaCl (s) conduct electricity

A

No

22
Q

Word ending for 3 or more elements combining with 1 being oxygen

A

-ate

23
Q

Chemical formula of methane

A

CH₄

24
Q

Why are pure metals soft

A

Layers are free to slide over each other

25
Q

Why do ionic compounds have high melting points

A
  • strong bonds
  • takes lots of energy to overcome them
26
Q

What attracts covalent bonds

A

Electrostatic forces

27
Q

Properties of simple molecular substances

A
  • held together by strong covalent bonds
  • weak intermolecular forces
  • low melting/boiling points
  • don’t conduct electricity
28
Q

What happens as molecules get larger

A
  • strength of intermolecular forces increase
  • melting/boiling points increase
29
Q

Properties of giant covalent structures

A
  • strong covalent bonds
  • high melting/boiling points
  • don’t conduct electricity
30
Q

Allotrope

A

Different structural form of same element in same physical state

31
Q

Properties of graphite

A
  • sheets of carbon atoms arranged in hexagons
  • no covalent bonds between layers
  • soft/slippery
  • high melting point
  • conducts electricity
32
Q

Properties of fullerene

A
  • large surface area
  • nanotubes can conduct electricity and heat
33
Q

Properties of non-metals

A
  • strong electrostatic forces of attraction
  • high melting/boiling points
34
Q

Structure of solids

A
  • strong forces of attraction
  • particles held close together in fixed positions in lattice arrangements
  • vibrate in fixed positions
  • expand slightly when heated
35
Q

Structure of liquids

A
  • weak forces of attraction
  • randomly arranged and free to move past each other
  • definite volume but no definite shape
  • particles move faster when heated
  • particles constantly moving
36
Q

Aqueous

A

Dissolved in water

37
Q

Structure of gases

A
  • weak forces of attraction
  • no definite shape or volume
  • particles constantly moving in random motion
  • expand when heated or pressure increases

Chemistry (5 decks)

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