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Chemistry GCSE > Bonding > Flashcards

Bonding Flashcards

1
Q

What does ionic bonding occur in?

A
  • metals and non-metals
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2
Q

Describe ionic bonding

A
  • metal ion loses electrons to form a full outer shell
  • becomes positve (state charge here) ion
  • non-metal ion gains electrons, forms full outer shell
  • becomes negative (insert charge) ion
  • strong electrostatic forces of attraction between opposite charges bond them together
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3
Q

Describe the structure of an ionic compound

A
  • giant ionic lattices
  • regular structure
  • strong electrostatic forces of attraction between oppositely charged ions
  • forces act in all directions
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4
Q

What are the properties of ionic compounds?

A
  • high melting and boiling point : the lattice structure and the strong electrostatic forces between the ions require a lot of thermal energy to break
  • Crystalline : this reflects the regular arrangement of teh ions
  • brittle : small distortions in the crystal bring ions with the same charge together and similar charges repel each other, breaking the crystal apart
  • soluble in water : the slightly negative oxygen in the water attracts the positive ions while the slightly oxygen hydrogen in the water attracts negative ions, pulling the crystal apart
  • do not conduct when solid : the ions cannot move when the ionic compound is solid there cannot carry any charge and cannot conduct electricity
  • conduct when molten/ in solution : the ions are free to move when molten or dissolved and will carry the charge and conduct electricity
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5
Q

What does covalent bonding occur in?

A
  • between non metals
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6
Q

Describe covalent bonding

A
  • pairs of electrons shared between atoms
  • gives full outer shells
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6
Q

What are the three types of molecule that can be formed by covalently bonded substances?

A
  • small molecules
  • very large molecules
  • giant covalent structures
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7
Q

What are the properties of small molecules?

A
  • low melting and boiling points
  • usually gases or liquids at room temp
  • weak intermolecular forces (much weaker than covalent bonds)
  • larger molecules = stronger intermolecular forces = higher boiling/ melting points
  • do not conduct electricity (no electric charge)
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8
Q

What are the properties of very large molecules?

A
  • high melting and boiling points
  • solids at room temp.
  • strong intermolecular forces between polymer molecules
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9
Q

What are large molecules?

A
  • polymers made by joining many monomers together
  • atoms in polymer molecules linked to other atoms by strong covalent monds

polymers have very large molecules

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10
Q

What are the properties of giant covalent structures?

A
  • solids with very high melting points
  • all atoms linked to other atoms by strong covalent bonds
  • these bonds must be overcome to melt or boil these substances
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11
Q

What are the properties of graphite?

A
  • high melting point
  • conducts electricity
  • slippery (weak intermolecular forces, layers slide over each other)
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12
Q

Describe graphite

A
  • each carbon has 3 covalent bonds to other carbon atoms
  • weak intermolecular forces between layers
  • layers can slide over each other
  • one delocalised electron per atom
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13
Q

Describe diamond

A
  • each carbon atom covalently bonded to 4 other carbon atoms
  • no delocalised electrons
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14
Q

What are the properties of diamond?

A
  • very hard
  • high melting point (high energy breaking covalent bonds)
  • doesn’t conduct electricity)
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15
Q

Describe graphene and its properties

A
  • single layer of graphite
  • conducts electricity (delocalised electrons) used for electronics
  • strong covalent bonds used for composites
16
Q

Describe metallic bonding

A
  • electrostatic force of attraction between positively charged centres of metal atoms and delocalised electrons
  • electrons can move through structure
  • metals = giant structures of atoms arranged in a regular pattern
17
Q

What are the properties of metals?

A
  • high melting and boiling points (giant structure of strong metallic bonding)
  • can be bent or shaped- pure metals = atoms arranged in layers, can slide over each other
  • good electrical conductors - delocalised electrons carry electrical charge through structure of metal
  • good thermal conductors - energy transferred by delocalised electrons
18
Q

What are the properties of alloys?

A
  • harder than pure metals- distorted layer structure
  • harder to slide over each other
19
Q

What are fullerenes?

A
  • molecules of carbon atoms with hollow shapes
  • based on rings of carbon atoms (5-7)
20
Q

What is C60?

A
  • spherical shape
  • buckminsterfullerene
21
Q

What are nano tubes?

A
  • cylindrical fullerenes
  • high length to diameter ratio
22
Q

What are fullerenes used for?

A
  • nanotechnology
  • electronics
  • lubricants (particles can roll)
23
Q

How large are nanoparticles?

A

1-100nm

a few hundred atoms

24
Q

How big are fine particles?

A

PM2.5
diameter 100-2500nm

25
Q

How big are coarse particles?

dust

A

PM 10
10 000 nm

26
Q

What is the rule of SA to volume ratio?

A
  • side decreases by factor of 10
  • SA to volume ratio increases by fator of 19
27
Q

Why do nanoparticles have different properties from the same materials in bulk?

A
  • because of their high surface area to volume ratio
  • smaller quantities needed to be effective than normal particle size
28
Q

What are the risks of using nanoparticles?

A
  • can enter human body (breathing, cuts, ingested)
  • might carry toxic substances into cells
  • catalyse damaging reactions

unsure of long term effects

29
Q

What are nanoparticles used for?

A
  • electronics (high length to diameter ratio, smaller components)
  • cosmetics (small size = absorbed into skin better, absorbs UV light)
  • deodorants (high SA to volume ratio)
  • medicines (small size penetrates cell walls, high length to diameter ratio)
  • catalysts (high SA to volume ratio)
30
Q

What are the disadvantages of using a ball and stick model?

A
  • doesn’t show electrons
  • appears large gaps between atoms
31
Q

What are the disadvantages of using dot and cross diagrams?

A
  • 2D
  • don’t show bond angles

Chemistry GCSE (17 decks)

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