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Chemistry > Structure and bonding > Flashcards

Structure and bonding Flashcards

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1
Q

Properties of giant covalent molecules

A
  • very high melting and boiling points
  • hard and strong (graphite is soft and slippery)
  • insoluble in water
  • electrical insulators
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2
Q

Properties of graphite nanotubes

A
  • high tensile strength (can be stretched without breaking)
  • good conductors
  • high melting and boiling points
  • strong
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3
Q

Properties of buckminster fullerenes

A
  • high melting points
  • strong
  • good conductors
  • good lubricants - layers can slide on top of one another due to weak intermolecular forces in between layers
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4
Q

Properties of graphenes

A
  • high melting and boiling points - many covalent bonds are strong and needs lots of energy to break
  • good conductors of heat and electricity - each carbon atom has a free delocalised electron which can move about and carry a charge
  • very strong
  • transparent
  • flexible
  • high resistance
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5
Q

Uses of fullerenes

A
  • pharmaceutical delivery
  • lubricants
  • catalysts
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6
Q

Bronze info

A
  • made of copper and tin
  • good conductor
  • high strength
  • corrosion resistant
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7
Q

Brass info

A
  • made of copper and zinc
  • malleable
  • tarnish resistance
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8
Q

Steel info

A
  • made of iron and carbon
  • high strength
  • low cost
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9
Q

What makes graphite slippery

A

its arranged in layers with weak intermolecular forces in between which allow is to slide on top one another

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10
Q

Properties of transition metals

A
  • hard and strong
  • high melting points
  • high densities
  • less reactive then alkali metals
  • conductors
  • form colored compounds
  • can form ions with different charges
  • used as catalysts
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11
Q

How many bonds does graphite have

A

3 covalent bonds

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12
Q

Why do most giant covalent structures not conduct electricity

A

all electrons are locked up in covalent bonds - no free electrons to carry a charge through the structure

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13
Q

Why are metals good conductors of heat and electricity

A

consist of delocalised electrons that are free to move and carry a current

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14
Q

How are metals ductile/malleable

A
  • layers of metal ions can slide over each other
  • closely packed layers (regular arrangement)
  • makes them relatively soft
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15
Q

Uses of nanoparticles

A
  • catalysts
  • sunscreens
  • deodorants
  • delivering drugs around the body
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16
Q

How many bonds does a diamond have

A

4 strong covalent bonds

17
Q

Why do metals have high melting and boiling points

A

strong electrostatic forces/metallic bonds - require lots of energy to break

18
Q

Properties of gases

A
  • can be compressed
  • fill the container
  • volume can change
  • least dense
  • particles move quickly and randomly
19
Q

How do allows make metals harder and stronger

A

Alloys have differently sized atoms - disrupts the layers/regular structure, making it harder for them to slide on top of eachother

20
Q

Sizes on nanoparticles, fine particles and coarse particles

A

nano: 1nm-100nm
fine: 100nm-2500nm
coarse: 2500nm-10µm

21
Q

What is metallic bonding

A

a bond in metals

22
Q

How is graphite soft

A

layers can slide due to weak intermolecular forces

23
Q

What happens when an ionic lattice is heated

A
  • particles vibrate vigorously
  • overcome strong electrostatic forces
24
Q

How are atoms arranged in a metal

A
  • giant lattice structures
  • regular pattern
  • electrons in the outer shell of each atom are delocalised
  • lattice of positive ions
25
Q

Disadvantages of nanoparticles

A
  • need more research
  • could be absorbed into our bodies and enter our cells
  • no one knows the potential long term effects
  • easily released into the environment
26
Q

What do nanotubes look like

A
  • tubes of hexagonal rings of carbon
  • sheets of graphite rolled up
27
Q

What are alloys

A

mixtures of two or more elements where one is a metal

28
Q

What is diamond and graphite made of

A

carbon

29
Q

What makes graphite slippery

A
  • arranged in layers
  • no covalent bonds between the layers so they can slide
30
Q

Why don’t most giant covalent structures conduct electricity

A
  • all electrons are locked up in bonds - no free electrons to carry a charge through the structure
31
Q
A

Chemistry (12 decks)

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