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Bonding, Structure and Properties of Matter > Bonding structure and properties of matter > Flashcards

Bonding structure and properties of matter Flashcards

1
Q

group 1 and 2 elements are most likley to form ions

A
  • metals
  • lose electrons
  • form positive ions
  • cations
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2
Q

group 6 and 7 are most likely to form ions

A
  • non-metals
  • gain electrons
  • form negative ions
  • anions
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3
Q

describe the ionic compound’s structure: the giant ionic lattice

A
  • ions form closely packed regular lattice arrangement
  • strong electrostatic forces of attraction
  • between oppositely charged ions
  • in all directions of lattice
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4
Q

ionic compounds all have similiar properties

A
  • high melting/boiling points
  • solid: can’t conduct electricity
  • soluble
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5
Q

why do ionic compounds have high melting/boiling points?

A
  • many strong bonds between ions
  • lots of energy needed to overcome
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6
Q

why do solid ionic compounds not conduct electricity?

A
  • ions held in place
  • melted: ions free to move carry current
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7
Q

what happens when ionic compounds dissolve in water?

A
  • ions seperate
  • free to move
  • carry electric current
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8
Q

what are simple molecular substances?

A
  • made up of molecules containing few atoms
  • joined by covalent bonds
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9
Q

what are the properties of the simple molecular substances?

A
  • atoms within molecules very strong covalent bonds
  • low melting/boiling points
  • gases/liquid at room temp
  • don’t conduct electricity
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10
Q

although simple molecular structures have very strong covalent bonds…

A

the forces of attraction between these molecules are very weak

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11
Q

why do simple molecular structures have low melting/boiling points?

A
  • only need to break feeble intermolecular forces
  • molecules easily parted
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12
Q

what happens when a molecular substance gets bigger?

A
  • strength intermolecular forces increase
  • more energy to break
  • melting/boiling point increase
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13
Q

why do molecular compounds not conduct electricity?

A
  • aren’t charged
  • no free electrons/ions
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14
Q

what are polymers?

A
  • long chains
  • repeating small units
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15
Q

atoms in a polymer are joined by…

A

strong covalent bonds

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16
Q

why are polymers solid at room temp?

A
  • intermolecular forces between molecules larger
  • more energy needed to break them
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17
Q

why do polymers have low boiling points?

A
  • intermolecular forces weaker than ionic or covalent bonds
  • lower boiling point than ionic or giant molecular compounds
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18
Q

what are macromolecules?

A
  • giant ocvalent structure
  • atom strongly covalent bond
  • very high melting/boiling point
  • don’t conduct electricity: no charged particles
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19
Q

describe the macromolecule of diamond

A
  • each carbon atom forms 4 covalent bonds
  • very rigid giant covalent structure
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20
Q

decribe the macromolecule of graphite

A
  • each carbon atom forms 3 covalent bonds
  • create hexagon layers
  • each carbon atom has one delocalised electron
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21
Q

decribe the macromolecule of silicon dioxide

A
  • sand made of silica
  • each grain one giant structure of silicon and oxygen
22
Q

what are the properties of a diamond?

A
  • giant covalent structure makes it really hard
  • very high melting point: strong covalent bonds lots energy to break
  • doesn’t conduct electricity: no free electrons/ions
23
Q

how does graphite containing sheets of hexagons make it ideal as lubricating material?

A
  • soft and slippery
  • no covalent bonds between layers
  • held weakly, free to move over eachother
24
Q

why does graphite have a high melting point?

A
  • lots energy to break
  • covalent bonds in layer
25
Q

why can graphite conduct electricity and thermal energy?

A
  • 3/4 outer electrons used in bonds
  • one free electron can move
26
Q

what is graphene?

A
  • sheet of carbon atoms joined in hexagons
  • one atom thick
  • two-dimensional compound
27
Q

what are the properties of graphene?

A
  • strong: network of covalent bonds
  • light: add to composite materials improve strength without added weight
  • conduct electricity through whole structure
28
Q

what are fullerenes?

A
  • molecules of carbon
  • shaped close tubes/hollow balls
29
Q

how are carbon atoms arranged in fullerenes?

A
  • mainly hexagons
  • pentagons
  • heptagons
30
Q

how can fullerenes be used to deliver a drug into the body?

A

-structure cages other molecules

31
Q

why can fullerenes make great industrial catalysts?

A

-large surface area

32
Q

what is the buckminsterfullerene?

A
  • first discovered
  • molecular formula C60
  • hollow sphere
33
Q

what is metalic bonding?

A
  • delocalised electrons in outer shell of metal atom
  • strong froces of electrostatic attraction
  • between positive metal ions and shared negative electrons
34
Q

why are most metals solid at room temp?

A
  • strong electrostatic forces of attraction
  • lots energy to break
  • very high melting/boiling point
35
Q

why are most metals malleable?

A

-layers of atoms slide over eachother

36
Q

what are alloys?

A
  • mixture of two or more metals
  • different sized atoms
  • distorted layers
  • pure metals too soft
37
Q

how are alloys harder than pure metals?

A
  • different element shave different sized atoms
  • new metal atoms ditort layers of metal atoms
  • more difficult to slide over eachother
38
Q

the state of something at a certain temp depends on…

A

how strong forces of attraction are between particles of material

39
Q

how strong froces of attraction are depends on…

A
  • material
  • temp
  • pressure
40
Q

explain the particle theory of a solid

A
  1. strong forces of attraction between particles, holds close together in fixed position to from lattice arangement
  2. definite shape and volume
  3. vibrate about their positions
41
Q

explain the particle theory of a liquid

A
  1. weak forces of attraction between particles, randomly arranged, move past eachother, stick together
  2. definite volume, don’t keep definite shape
  3. constantly move in random motion
42
Q

explain the particle theory of a gas

A
  1. very weak forces of attraction, free to move, far apart
  2. don’t keep definite shape or volume
  3. move constantly in random motion
43
Q

solid melted to liquid

A
  • particles gain more energy
  • vibrate more: weakens forces
  • melting point: enough energy to break free
44
Q

liquid boiled to gas

A
  • particles gain more energy
  • more faster: weakens and breaks bonds
  • boiling point: enough energy to break bonds
45
Q

gas condensed to liquid

A
  • cools: particles no longer have enough energy overcome forces
  • bonds form
  • boiling point: many bonds form gas to liquid
46
Q

liquid freezed to solid

A
  • cools: particles have less energy
  • not enough energy to overcome forces: more bonds form
  • melting point: so many bonds form liquid to solid
47
Q

what are coarse particles (PM10)?

A
  • dust
  • diameter: 2.5x10-6m and 1x10-5m
48
Q

what are fine particles (PM2.5)?

A

-diameter: 1x10-7m and 2.5x10-6m

49
Q

how can you calculate the surface area to volume ratio?

A

surface area/volume

50
Q

how is electricity conducted in a metal?

A
  • giant ionic lattice
  • made up of positive ions
  • with free electrons
  • moves to carry charge
51
Q

why is alloys used in dental braces?

A

-turn back into original shape

52
Q

why are instrumental methods used to detect impurities on metals?

A
  • accurate
  • small samples

Bonding, Structure and Properties of Matter (11 decks)

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