LONGER ANSWERS PAPER 1 Flashcards

1
Q

Explain why the reactivity of elements changes going down Group 1.

A
  • reactivity increases
  • as outer electron is further from the nucleus
  • there is less attraction between the nucleus and the outer electron
  • so the atom loses an electron more easily
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2
Q

Explain why alloys are harder than pure metals

A
  • in an alloy the atoms are of different sizes
  • so the layers of atoms are distorted
  • so in an alloy the layers slide over each other less easily
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3
Q

Explain the trend in boiling points of the halogens as you go down the group

A
  • boiling point increases down the group
  • because the size of the molecule increases
  • so the intermolecular forces increase in strength
  • so more energy is needed to overcome the intermolecular forces
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4
Q

Explain why the reactivity of the halogens decreases going down the group.

A
  • going down the group the outer electrons become further from the nucleus
  • so the nucleus has less attraction for the outer electrons
  • so an electron is gained less easily
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5
Q

Explain why ammonia has a low boiling point.

A
  • ammonia has small molecules / a simple molecular structure
  • ammonia has weak intermolecular forces
    -so little energy is needed to overcome the intermolecular forces
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6
Q

Explain why hydrogen chloride is a gas at room temperature

A
  • hydrogen chloride is made of small molecules / is simple molecular structure
  • so hydrogen chloride has weak intermolecular forces
  • intermolecular forces require little energy to overcome
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7
Q

Explain why this alloy is harder than the pure metal

A
  • the atoms / particles / ions are different sizes
  • so there are no layers to slide
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8
Q

Potassium forms an ionic compound with sulfur.
Describe what happens when two atoms of potassium react with one atom of sulfur. Potassium has 1 electron and sulfur has 6.

A
  • electrons transferred from potassium to sulfur
  • two potassium atoms each lose one electron, forming K 1+ ions
  • sulfur atoms gain 2 electrons forming S 2− ions
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9
Q

Explain why graphite is:
* a good electrical conductor
* soft and slippery.

A
  • bonds are covalent
  • giant / macromolecular structure
  • three(covalent bonds per carbon atom
  • so one electron per carbon atom is delocalised, they can move through the structure carrying charge
  • so graphite conducts electricity
  • layered structure of hexagonal rings
  • with weak intermolecular forces between layers
  • so the layers can slide over each other
  • so graphite is soft and slippery
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10
Q

Suggest why it is cheaper to use nanoparticles of silver rather than coarse particles of silver

A
  • nano particles have a larger surface area to volume ratio
  • so less can be used for the same effect
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11
Q

Explain why diamond is hard.

A
  • it is a giant structure
  • that has strong covalent bonds
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12
Q

Explain why thermosetting polymers are better than thermosoftening polymers for saucepan handles.

A
  • thermosetting polymers do not melt when heated
  • due to cross-links between chains
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