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Chemistry Paper 1 > practice questions > Flashcards

practice questions Flashcards

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1
Q

what shape is buckminsterfullerene molecule?

A

spherical

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2
Q

give one use of a fullerene

A
  • drug delivery (around the body)
  • lubricants
  • catalysts
  • anti-oxidants
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3
Q

why does propanone have a low boiling point?

A

the intermolecular forces are weak

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4
Q

explain why graphite is a good electrical conductor; soft and slippery

A
  • in graphite, each carbon atom is covalently bonded to three other carbon atoms
  • this leaves one free electron per each carbon atom
  • these form a sea of delocalised electrons which can move around the structure and carry the charge
  • so graphite conducts electricity
  • layered structure of hexagonal rings
  • there are no covalent bonds between the layers
  • so they can slide over each other, so graphite is soft and slippery
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5
Q

give the meaning of isotopes

A

atoms with the same number of protons but different number of neutrons

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6
Q

give two reasons why the discovery of gallium helped Mendeleev’s periodic table to become accepted

A
  • gallium fitted in a gap that Mendeleev had left
  • gallium’s properties were predicted correctly by Mendeleev
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7
Q

give two observations you could make when a small piece of potassium is added to water

A
  • lilac flame
  • effervescence
  • potassium melts
  • potassium becomes smaller
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8
Q

explain why the reactivity of elements changes going down group 1

A
  • going down the group, reactivity increases
  • this is because the size of the atom increases going down the group
  • and the shielding effect increases
  • this means that the attraction between the positively charged nucleus and negatively electron is weaker
  • so it is easier for atoms to lose an electron going down the group
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9
Q

why is oxygen described as being reduced in the reaction between sodium and oxygen?

A

oxygen gains electrons

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10
Q

explain why sodium oxide has a high melting point

A
  • giant structure
  • with strong electrostatic forces of attraction between oppositely charged ions
  • so large amounts of energy are needed to break the bonds
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11
Q

name the salt produced by the neutralisation of hydrochloric acid with potassium hydroxide

A

potassium chloride

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12
Q

explain why alloys are harder than pure metals

A
  • the atoms are different sizes
  • so the layers are distorted
  • and slide over each other less easily than in pure metals
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13
Q

what are the differences between covalent and ionic bonding?

A
  • in covalent electrons are shared, in ionic electrons are transferred
  • in covalent there are intermolecular forces, in ionic there are electrostatic forces of attraction
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14
Q

what did Niels Bohr discover?

A

electrons exist in shells and orbit the nucleus at specific distances

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15
Q

what is the order of discovery of the sub-atomic particles?

A

electrons, protons, neutrons

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16
Q

what is the relative mass of a proton?

A

1

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17
Q

what is the relative mass of a neutron?

A

1

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18
Q

what is the relative mass of an electron?

A

very small, close to 0

19
Q

what is a compound?

A

different atoms chemically bonded in a fixed ratio

20
Q

explain why argon does not react with tungsten

A
  • argon is unreactive
  • because it has a full outer shell of electrons
21
Q

why does iodine have a higher boiling point than chlorine?

A

the forces between iodine molecules are stronger

22
Q

why does potassium iodide solution conduct electricity?

A

it contains ions which can move

23
Q

what are the products of electrolysing potassium iodide solution?

A

cathode: hydrogen
anode: iodine

24
Q

what are the physical properties of transition elements?

A
  • high melting points
  • high densities
  • strong
  • hard
25
Q

what are the chemical properties of transition elements?

A
  • used as catalysts
  • form ions with different charges
  • form colourless compounds
  • low reactivity, react slowly with water
26
Q

what are the physical properties of group 1 elements?

A
  • low melting points
  • low densities
  • soft
27
Q

what are the chemical properties of group 1 elements?

A
  • only from ions with 1+ charge
  • very reactive
  • form white/colourless compounds
28
Q

what is meant by a strong acid?

A
  • completely ionises
  • when dissolved in water
29
Q

explain how a covalent bond holds two atoms together

A
  • electrostatic force of attraction between shared pair of negatively charged electrons
  • and both positively charged nuclei
30
Q

what is a compound?

A

two or more elements that are chemically bonded together

31
Q

what is the main differences between metals and non-metals?

A
  • metals conduct electricity, whereas, non-metals are generally electrical insulators
  • metals also have higher boiling and melting points
  • metals are ductile and malleable whereas non-metals are brittle
32
Q

what does ductile mean?

A

can be drawn out into wires

33
Q

what does malleable mean?

A

can be hammered into shapes without smashing it

34
Q

what is the name of the elements in Group 0 of the periodic table?

A

noble gases

35
Q

describe three other differences between the plum pudding model and the nuclear model of the atom

A

in the nuclear model:
- the positive charge is all in the nucleus
- the mass is all concentrated in the nucleus
- the electrons and the nucleus are separated
- the atom is mostly empty space

36
Q

describe the change that Bohr made to the nuclear model

A
  • electrons orbit the nucleus
  • at specific distances from the nucleus
37
Q

why did Mendeleev reverse the order of some pairs of elements?

A

so their properties matched the rest of the group

38
Q

which sub-atomic particle has the lowest mass?

A

electron

39
Q

describe how the process of distillation shown in figure 2 produces pure water from salt solution

A
  • salt solution is heated
  • solution evaporates
  • the vapour condenses inside the condenser
  • pure water is collected inside the beaker
40
Q

define mass number

A

the sum of protons and neutrons

41
Q

why is the mass number different in the two isotopes?

A

different numbers of neutrons

42
Q

explain how evidence from the alpha scattering experiment led to a change in the model of the atom from the plum pudding model

A
  • most alpha particles passed straight through the foil
  • so the mass of the atom is concentrated in the nucleus//most empty space
  • some alpha particles were deflected
  • so the atom has a positively charged nucleus
43
Q

explain how Chadwick’s work led to a better understanding of isotopes

A
  • Chadwick proved the existence of the neutron
  • which was necessary because isotopes have the same number of protons
  • but different number of neutrons
44
Q

explain why sodium oxide has a high melting point

A
  • sodium oxide is arranged in a giant ionic lattice
  • strong electrostatic forces of attraction between oppositely charged ions
  • requires a lot of energy to overcome these bonds

Chemistry Paper 1 (9 decks)

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