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Chemistry > Higher: C1 - Atomic structure and the periodic table > Flashcards

Higher: C1 - Atomic structure and the periodic table Flashcards

1
Q

Atoms have a radius of about…

A

0.1nm (1x10-10m)

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2
Q

A nanometer is one ___th of a metre.

A

Billonth.

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3
Q

What is one nanometer in standard form?

A

1x10-9m

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4
Q

The nucleus has a radius of ___, which is around 1/___th the radius of an atom.

A

1x10-14m, 1/10,000th

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5
Q

What decides what type of atom an atom is?

A

The number of protons in the nucleus.

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6
Q

How many different elements are there?

A

About 100.

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7
Q

What are isotopes?

A

Different forms of an element which have the same number of protons but different numbers of neutrons.

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8
Q

What is relative atomic mass and why is it used?

A

Because many elements can exist as different isotopes, RAM is used as a mass number. It is an average, taking into account the different masses and their abundances.

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9
Q

What formula is used to calculate the RAM of an element?

A

Ar = sum of (isotope abundance x mass number)

————————————————————

sum of abundances of all isotopes

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10
Q

What is a compound?

A

2 or more different elements, present in fixed proportions, chemically bonded together.

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11
Q

What are mixtures?

A

A substance which consists of 2 or more elements and/or compounds, which can be separated out using physical methods. They are not chemically bonded.

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12
Q

Chromatography is used to separate different dyes within an ink. Explain how a chromatography experiment is set up.

A
  1. Draw a line near the bottom of a sheet of filter paper in pencil (since it’s insoluble).
  2. Add a spot of ink to this line.
  3. Place the sheet in a beaker of solvent (e.g. water - depends on what’s being tested), making sure the ink doesn’t touch the solvent.
  4. Put a lid on the container to stop the solvent evaporating.
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13
Q

Chromatography is used to separate different dyes within an ink. The following method is used to do this:

  1. Draw a line near the bottom of a sheet of filter paper in pencil (since it’s insoluble).
  2. Add a spot of ink to this line.
  3. Place the sheet in a beaker of solvent (e.g. water - depends on what’s being tested), making sure the ink doesn’t touch the solvent.
  4. Put a lid on the container to stop the solvent evaporating.

Explain what will happen during this experiment.

A
  1. The mobile phase (solvent) seeps up the paper, carring the ink with it.
  2. Each dye within the ink moves up the paper at a different rate; the dyes separate out into spots.
  3. If any of the dyes are insoluble, they stay on the stationary phase (pencil line).
  4. When the solvent has nearly reached the top, the paper is taken out and allowed to dry; the result is a chromatogram.
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14
Q

What are the mobile and stationary phases in chromatography?

A

Mobile phase = solvent (bc it moves up the paper).

Stationary phase = paper

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15
Q

How would you separate an insoluble solid from a liquid?

A

Filtration.

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16
Q

How would you separate a soluble salt from a liquid? Give 2 ways.

A
  1. Evaporation: heating the solution, in an evaporating dish, over a bunsen burner. However, this can only be used if the salt doesn’t thermally decompose. If it does:
  2. Crystallisation: gently heating the solution until crystals start to form, then leaving it to cool. More crystals will form, which are filtered out of the solution and left in a warm place to dry.
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17
Q

How would you separate out rock salt (a mixture of salt and sand)?

A
  1. Grind it to make the salt crystals small (so that they dissolve easily).
  2. Put it in water and heat; salt will dissolve but sand won’t.
  3. Filter out the sand.
  4. Evaporate the water from the salt, so that it forms dry crystals.
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18
Q

What is simple distillation used for?

A

Separating out a liquid from a solution.

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19
Q

How does simple distillation separate out a liquid from a solution?

A
  1. Solution is heated.
  2. The part of the solution with the lowest boiling point evaporates first.
  3. The vapour is cooled in a condenser, then collected in a beaker at the end of the condenser.
  4. The rest of the solution remains in the flask.
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20
Q

What is the problem with simple distillation?

A

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

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21
Q

What is fractional distillation used for?

A

Separating out liquids, from a mixture, with close boiling points.

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22
Q

This lab demonstration models the separation of crude oil at a refinery. How does the process work?

A
  1. Heat the mixture in the flask
  2. The liquid with the lowest boiling point evaporates first.
  3. When the thermometer’s temperature reaches the boiling point of this liquid, it reaches the top of the column, condenses, and is collected.
  4. Other liquids may start to evaporate, but will condense part of the way up the column (bc it’s cooler towards the top).
  5. Once the first liquid’s collected, the temperature is raised until the next one reaches the top of the column. Etc.
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23
Q

What was Dalton’s model of the atom?

A

Atoms were solid, indivisible spheres. Each element was made of a different type of sphere.

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24
Q

What was Thomson’s model of the atom?

A

He discovered electrons which could be removed from atoms, disproving Dalton’s theory of indivisibility.

Thomson suggested atoms were spheres of positive charge, with negative electrons scattered throughout (plum pudding model).

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25
Q

What was Rutherford’s model of the atom?

A

Positively charged nucleus, surrounded by a cloud of negative electrons. This was the first nuclear model of the atom.

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26
Q

What discovery did Bohr make? How was he proven right?

A

Electrons orbit the nucleus in fixed positions, called energy levels.

His theoretical calculations agreed with experimental data.

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27
Q

What discovery was made after electron orbits?

A

Experiments showed that the nucleus’ positive charge was subdivided between a group of particles, called protons.

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28
Q

What discovery did Chadwick make? Why did this make sense?

A

He proved the existence of neutrons in the nucleus. This explained the imbalance between the atomic and mass numbers.

29
Q

Who theorised that atoms were solid, indivisible spheres?

A

Dalton.

30
Q

Who theorised the plum pudding model?

A

Thomson.

31
Q

Whose discoveries led to the nuclear model of the atom?

A

Rutherford.

32
Q

Who calculated that electrons had fixed orbits?

A

Bohr.

33
Q

Who discovered neutrons?

A

Chadwick.

34
Q

How was Rutherford’s alpha scattering experiment conducted?

A

Scientists in Rutherford’s lab fired a beam of alpha particles at a thin sheet of gold foil.

35
Q

In Rutherford’s alpha scattering experiment, what did the scientists expect to happen and why?

A

From the plum pudding model, they expected particles to pass straight through the gold foil, or only be slightly deflected.

36
Q

What were the results of Rutherford’s alpha scattering experiment? Why wasn’t this as expected?

A

The majority of the alpha particles went straight through the gold sheet. However, some were deflected more than expected and a few were deflected right back the way they came. The plum pudding model couldn’t explain this.

37
Q

In Rutherford’s alpha scattering experiment, a few alpha particles were deflected back. What did the scientists deduce from this?

A

They realised that most of the atom’s mass was concentrated in a central nucleus, which must also have a positive charge, since it repelled the positive alpha particles.

38
Q

In Rutherford’s alpha scattering experiment, most of the alpha particles passed straight through. What did the scientists deduce from this?

A

They realised that most of the atom is just empty space, and that the nucleus is very small relative to this space.

39
Q

What was deduced from the results of Rutherford’s alpha scattering experiment?

A
  1. Because a few alpha particles were deflected back, they realised that most of the atom’s mass was concentrated in a central nucleus, which must also have a positive charge, since it repelled the positive alpha particles.
  2. Because most of the alpha particles passed straight through, they realised that most of the atom is just empty space, and that the nucleus is very small relative to this space.
40
Q

How were elements organised in the early periodic table, and what was the problem with this?

A
  1. Elements were organised according to their relative atomic masses.
  2. The table wasn’t complete, and some elements were placed in the wrong group because the ordering didn’t take into account their properties.
41
Q

How was Mendeleev’s periodic table different to - and better than - the early versions of the periodic table?

A
  1. He organised elements mainly in order of atomic mass, but also taking into account their properties.
  2. The discovery of isotopes showed he was right to do this.
  3. He left gaps which predicted the existence of undiscovered elements, allowing him to predict their properties.
  4. The discovery of certain elements that fit this pattern confirmed his ideas, for example, he left a gap for an element with similar properties to aluminium. Gallium was discovered, and it showed these properties.
42
Q

How many elements are there?

A

About 100.

43
Q

How are elements organised in the modern periodic table?

A
  1. Elements are laid out in order of increasing proton number, meaning there are repeating patterns of properties.
  2. Metals on left; non-metals top right.
  3. Elements with similar properties form columns: groups. Group no. = no. electrons on outer shell.
  4. The rows are periods; the period number shows how many electron shells an element has.
44
Q

Give 4 properties of metals.

A
  1. Strong
  2. Malleable and ductile
  3. Good conductors of heat and electricity
  4. High melting and boiling points: almost always solids at room temp. (exception is mercury)
45
Q

Non-metals form a variety of different structures, sohave a wide range of chemical properties. Give 5 typical properties of non-metals.

A
  1. Dull-looking
  2. Brittle
  3. Lower density than that of metals
  4. Bad conductors of electricity
  5. Not always solids at room temp. / lower melting points than metals
46
Q

Transition metals are found in the middle of the periodic table. Give 7 properties of transition metals.

A
  1. Good conductors of electricity + heat
  2. Strong
  3. Dense
  4. Shiny
  5. Can form more than one ion
  6. Colourful
  7. Transition metal compounds often make good catalysts
47
Q

What are group 1 elements known as?

A

The alkali metals.

These are: lithium, sodium, potassium, rubidium, caesium and francium.

48
Q

Give 3 properties of alkali metals.

A
  1. Soft
  2. Low density (lithium, sodium + potassium less dense than water)
  3. Very reactive (only 1 electron in outer shell; easily lost)
  4. Only ever form ionic compounds (1+ ions)
49
Q

What are the trends in properties of alkali metals as you go down the group?

A
  1. Increasing reactivity
  2. Decreasing melting + boiling points
  3. Increasing relative atomic mass
50
Q

Alkali metals only ever form ionic compounds. What are these compounds usually like?

A

White solids that dissolve in water to form colourless solutions.

51
Q

Explain why sodium is more reactive than lithium.

A
  1. Sodium is further down group 1 than lithium.
  2. Group 1 ions lose one electron to become stable.
  3. Sodium’s outer electron is further from the nucleus that lithium’s.
  4. So the electrostatic attraction between the electron and nucleus is weaker.
  5. So the electron is more easily released.
  6. So sodium is more reactive.
52
Q

Compare the reactions of lithium and potassium with water. Describe what would be observed in each reaction and explain the similarities and differences. (6)

A

A vigorous reaction would be observed with both metals.

The reaction with potassium would be more vigorous as it is more reactive than lithium. This is because the outer electron of potassium is further from its nucleus and therefore more easily lost.

Both metals would float, as they are less dense than water.

Both metals will fizz, producing bubbles of hydrogen gas.

The reaction with potassium would produce more hydrogen bubbles, as potassium is more reactive.

The reaction with potassium would release more energy, to the extent that the potassium and hydrogen could ignite.

53
Q

Compare the properties of transition and alkali metals.

A
  1. Alkali metals are much more reactive.
  2. Transition metals are stronger, denser and harder.
  3. Alkali metals have much lower boiling points.
54
Q

How do alkali metals react with water?

A
  1. They react vigorously to produce hydrogen gas and metal hydroxides.
  2. The violence of reactivity (and energy released from the reaction) increases as you go down the group.
55
Q

How do alkali metals react with chlorine?

A
  1. When heated in chlorine gas, they form white metal chloride salts.
  2. The reaction gets more vigorous as you go down the group.
56
Q

How do alkali metals react with oxygen?

A

They react with oxygen to form metal oxides (which is why they tarnish in the air), different types of oxide forming depending on the metal:

Lithium → lithium oxide.

Sodium → mixture of sodium oxide and sodium peroxide

Potassium → mixture of potassium peroxide and potassium superoxide

57
Q

What are group 7 elements known as?

A

The halogens.

58
Q

What are the trends in properties of the halogens as you go down the group?

A
  1. Decreasing reactivity
  2. Increasing melting + boiling points
  3. Increasing relative atomic masses
59
Q

Give 3 properties of the halogens.

A
  1. Form diatomic molecules
  2. Bond ionically w/ metals
  3. Bond covalently to form simple molecular compounds
  4. A more reactive halogen will displace a less reactive one from an aqueous solution of its salt
  5. They decrease in reactivity as you go down the table
60
Q

What is the colour and state of fluorine at room temperature? Give 2 of its properties.

A

Yellow gas.

Very reactive and poisonous.

61
Q

What is the colour and state of chlorine at room temperature? Give 3 of its properties.

A

Green gas.

Fairly reactive, poisonous, dense.

62
Q

What is the colour and state of bromine at room temperature? Give 3 of its properties.

A

Red-brown liquid.

Poisonous, dense, volatile.

63
Q

What is the colour and state of iodine at room temperature? What does its gas look like?

A

Dark grey, crystalline solid.

Purple gas.

64
Q

A chemist places a glass lid over a beaker containing aqueous iodine. She places an ice cube on top of the lid and then gently heats the solution. Predict and explain her observations.

A

A purple vapour will form over the solution as the iodine evaporates.

Purple/grey crystals will form on the lid as the iodine deposits/crystallises/solidifies.

65
Q

What are the group 0 elements known as?

A

The noble gases.

66
Q

Give 4 properties of noble gases.

A
  1. Inert
  2. Non-flammable (bc of above)
  3. Exist as monatomic gases
  4. All colourless gases at room temperature
67
Q

Why are the noble gases inert?

A

They have full outer shells which are energetically stable. They therefore don’t need to react to gain or lose electrons to become stable.

68
Q

What are the trends in properties of the noble gases as you go down the group?

A
  1. Increasing boiling points (greater no. electrons in each element leads to greater intermolecular forces
  2. Increasing relative atomic mass

Chemistry (6 decks)

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