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Chemistry > C1 - Atomic Structure and the Periodic Table > Flashcards

C1 - Atomic Structure and the Periodic Table Flashcards

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1
Q

How big is an atom?

A

1 X 10^-10

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2
Q

State five facts about the nucleus.

A

1) It’s in the middle of the atom.
2) It contains protons and neutrons.
3) The nucleus has a radius of 1 X 10^-14 (1/10,000 of the radius of an atom).
4) It has a positive charge (because of the protons).
5) Almost all of the mass of an atom is found in the nucleus.

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3
Q

What is the mass, charge and position of protons, neutrons and electrons?

A

Protons - 1g, +1, nucleus.
Neutrons - 1g, 0, nucleus.
Electrons - 0 or negligible, -1, energy levels.

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4
Q

How do you calculate the amount of neutrons in an atom?

A

Subtract the atomic number from the mass number.

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5
Q

What is an element?

A

A substance made up of the same atoms.

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6
Q

Elements consist of atoms with the same?

A

Atomic number.

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7
Q

What is an isotope?

A

They have the same number of protons, but a different number of neutrons. This means that they have the same atomic number but different mass numbers.

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8
Q

How do you calculate relative atomic mass?

A

Sum of (isotope abundance X isotope mass number)
———————————————————
Sum of abundances of all the isotopes

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9
Q

What is a compound?

A

Substances made up of two or more elements and are held together by chemical bonds.

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10
Q

What does a compound which is formed from a metal and non metal consist of?

A

Positive and negative ions which have a strong electrostatic force of attraction between each other.

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11
Q

What do chemical equations show?

A

Chemical changes.

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12
Q

What is a mixture?

A

A group of substances that aren’t chemically bonded together.

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13
Q

What is chromatography used for?

A

Separating different dyes in an ink.

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14
Q

Describe the chromatography practical.

A

1) Draw a base line near the bottom of a sheet of chromatography paper. This must be done in pencil so it doesn’t dissolve in the solvent.
2) Add a spot of ink to the base line and place the sheet in a beaker of solvent (such as water).
3) Make sure the base line doesn’t touch the solvent so the ink doesn’t dissolve into it.
4) Place a lid on top of the container to stop the solvent evaporating.
5) The solvent should then seep up the paper, carrying ink with it.
6) If a dye is insoluble, it will stay on the base line. This is because the more soluble the dye, the further up the paper it moves.
7) When the solvent has nearly reached the top of the paper, take the paper out and leave it to dry.
8) The end result is called a chromatogram.

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15
Q

What does filtration separate?

A

Insoluble solids from liquids.

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16
Q

Describe filtration.

A

1) Fold the filter paper into a cone shape.
2) Place the filter paper into a funnel.
3) Place the funnel into a beaker.
4) Pour the mixture into the funnel.
5) The insoluble solid wouldn’t flow down the tube, so it is separated from the liquid.

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17
Q

Describe how to separate soluble solids.

A

1) Pour the solution into an evaporating dish.
2) Slowly heat the solution until crystals start to form.
3) Heat the solution or allow the solution to dry off until all you have left is dry crystals.

18
Q

What is simple distillation used for?

A

To separate solutions.

19
Q

Describe simple distillation.

A

1) The solution is slowly heated. The part of the solution that has the lowest boiling point will evaporate first.
2) The vapour then travels through a condenser where it cools, condenses and is collected.
3) The rest of the solution would remain in the flask.

20
Q

What is the problem with simple distillation?

A

You can only use it to separate solutions with very different boiling points.

21
Q

What is fractional distillation used for?

A

Separate mixtures of liquids with similar boiling points.

22
Q

Describe fractional distillation.

A

1) Pour your mixture into a flask and stick a fractionating column on top. Then heat the flask.
2) The liquids will have different boiling points, so they will evaporate at different temperatures.
3) The liquid with the lowest boiling point evaporates first. When the temperature reaches this point, the liquid will reach the top of the column.
4) Liquids with higher boiling points may also begin to evaporate, but the column is cooler towards the top so they will only get part of the way up before condensing and going back to the bottom of the flask.
5) When the first liquid has been collected, raise the temperature until the next one reaches the the top.

23
Q

How did John Dalton describe atoms?

A

Atoms were solid spheres and different spheres made up the different elements.

24
Q

Who created the plum pudding model and what is it?

A
  • JJ Thomson
  • The atom was described as a ball of positive charge with negative electrons embedded in it.
25
Q

Who conducted the alpha scattering experiment and what was it?

A
  • Ernest Rutherford.
  • Positive alpha particles were fired at an extremely thin sheet of gold.
26
Q

What discoveries were made about the atom after the alpha scattering experiment?

A
  • Most atoms went straight through the the gold sheet, so it showed that atoms were made up of mostly empty space.
  • Some particles were deflected, so there was a positive mass in the atom.
  • One particle deflected backwards, so the positive mass was very, very small.
27
Q

What did Niels Bohr discover?

A

Energy levels. Electrons orbited the nucleus in these fixed shells that were a fixed distance away from the nucleus.

28
Q

How were protons and neutrons discovered?

A
  • Further experiments by Rutherford showed that the nucleus could be divided into smaller particles. These were called protons.
  • James Chadwick carried out experiments to prove the existence of neutral particles, known as neutrons.
29
Q

How were elements arranged before?

A

1) Physical and chemical properties.
2) Atomic Weight.

30
Q

How did Mendeleev arrange elements?

A

1) He left gaps. This allowed him to predict the properties of undiscovered elements such as Gallium.
2) He arranged them both in order of atomic weight and properties, so he swapped a few elements when arranging them.

31
Q

Where are metals and non-metals found on the periodic table?

A

Metals are found on the right whereas non-metals are found on the left.

32
Q

What are the properties of metals and non-metals?

A

Metals:
- Strong
- Malleable
- Conductors of heat and electricity
- High melting and boiling points
- Lustrous
- Higher density

Non-metals:
- Weak
- Brittle
- Don’t conduct heat and electricity
- Dull
- Lower density

33
Q

What are the special properties of transitional metals?

A
  • Have more than one ion.
  • Often make coloured compounds.
  • Make good catalysts.
34
Q

What are Group 1 metals known as?

A

Alkali metals.

35
Q

Why are Group 1 metals very reactive?

A

They only have one electron in their outer shell.

36
Q

What are the trends for Group 1 elements as you move down the group?

A

1) Reactivity increases because the outer electron is more easily lost because the electrostatic force of attraction between the nucleus and electron decreases.
2) Lower melting and boiling points.
3) Higher relative atomic mass.

37
Q

How do group 1 metals react with water?

A
  • Vigorously
  • Produce hydrogen gas
  • Potassium —> flame
38
Q

What are the differences between alkali metals and transitional metals?

A
  • More reactive.
  • Less dense.
  • Weaker.
  • Soft.
  • Lower boiling/melting points.
39
Q

What is the trend in Group 7 elements as you move down the group?

A
  • Less reactive.
  • Higher melting and boiling points.
  • Higher relative atomic mass.
40
Q

Why are Group 0 elements inert?

A

They have a stable electronic configuration, so they don’t have to react.

41
Q

What is the trend in Group 0 as you move down the group?

A

Boiling points increase because there are more electrons so there are stronger intermolecular forces which require more energy to overcome.

Chemistry (10 decks)

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