c2 Flashcards

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1
Q

name the limitations of the particle model

A
  1. All particles are represented as spheres
  2. Particles are represented solid and unbreakable
  3. We simplify the different forces between particles by calling them all bonds
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2
Q

what happens when when a liquid reaches boiling point

A

particles have enough energy to overcome forces

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3
Q

name the two main types of covalent structures

A
  1. simple molecules
  2. giant covalent structures
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4
Q

describe simple molecules

A
  • low boiling point and melting point
  • molecules held together by weak intermolecular forces
  • covalent bonds between atoms
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5
Q

describe giant covalent structures

A

high boiling point and melting point due to strong covalent bonds which hold the structure together

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6
Q

why does carbon dioxide have a low boiling point

A
  • carbon dioxide is a simple molecule
  • there are weak intermolecular forces
  • therefore a small amount of energy is needed to overcome these forces
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7
Q

why does diamond have a high melting point?

A
  • diamond is a giant covalent structure
  • there are strong covalent bonds between the carbon atoms
  • therefore a large amount of energy is needed to overcome the bonds.
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8
Q

describe the structure of diamond

A

each carbon atom forms four covalent bonds with other carbon atoms

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9
Q

describe the structure of graphite

A

each carbon atom forms three covalent bonds with other carbon atoms forming layers of hexagonal rings

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10
Q

can diamond conduct electricity? why?

A

no

no delocalised electrons

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11
Q

why is graphite soft

A

soft due to weak intermolecular forces between layers of carbon so layers can slide off

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12
Q

can graphite conduct electricity? why?

A

yes

delocalised electrons move between layers carrying charge to conduct electricity

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13
Q

describe the structure of sodium chloride

A

sodium chloride consists of sodium and chloride ions arranged in a giant ionic lattice. the ions are held together by strong electrostatic forces of attraction between positive and negative ions

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14
Q

why do ionic compounds have high melting points?

A

high electrostatic forces of attraction between ions so high amounts of energy needed to overcome these forces

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15
Q

when can ionic compounds conduct electricity

A

ionic compounds can conduct electricity when molten or dissolved because the electrostatic forces are overcome so ions are separated so they are free to move within the structure and carry charge

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16
Q

describe the structure of a metal

A
  • atoms arranged in regular structure
  • positive metal ions
  • with a sea of delocalised electrons
  • strong electrostatic forces of attraction between these hold the structure together
17
Q

why can metals conduct electricity

A

have delocalised electrons which can move through structure and carry current

18
Q

why are metals malleable and ductile

A

layers slide over each other and therefore can form new shapes

19
Q

what is an alloy

A

alloys are mixtures of two or more elements, one of which is a metal

20
Q

why are alloys stronger than pure metals

A
  • they have different sized atoms
  • so layers are distorted
  • can’t cannot slide over eachother as easily