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Chem Module 3 > The periodic table 3.1 > Flashcards

The periodic table 3.1 Flashcards

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1
Q

How are elements arranged in the modern periodic table?

A

In order of increasing atomic number

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2
Q

What is periodicity?

A

The repeating patterns of physical and chemical properties across a period

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3
Q

What leads to periodicity?

A

That all elements in a period have the same number of electron shells

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4
Q

What is an orbital?

A

A region around the nucleus that can hold up to 2 electrons with opposite spin

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5
Q

What is a shell?

A

A group of orbitals in the same energy level (energy level)

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6
Q

What is a sub shell?

A

A group of the same type of atomic orbital within a shell

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7
Q

When does ionisation happen?

A

when atoms gain or lose electrons

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8
Q

What is the first ionisation energy?

A

The energy required to remove one electron from each atom in 1 mole of a gaseous element to form 1 mole of gaseous 1+ ions

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9
Q

What is second ionisation energy?

A

The energy required to remove one electron from each atom ion in 1 mole of gaseous 1+ ions of an element to form 1 mole of gaseous 2+ ions

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10
Q

What are the rules for writing out first ionisations?

A
  • write a gas symbol next to an element even if it is not a gas
  • write the ion as positive even if it may be of a different charge
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11
Q

What are the factors affecting the first ionisation energy

A
  • atomic radius
  • nuclear charge
  • electron shielding
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12
Q

How does first ionisation energy change as you move across a period?

A

It increases overall

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13
Q

How does atomic radius change as you move across a period?

A

It decreases

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14
Q

How does nuclear charge change as you move across a period?

A

It increases

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15
Q

How does electron sheilding change as you move across a period?

A

It remains constant

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16
Q

What effect does atomic radius have on first ionisation energy across a period?

A

It increases it

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17
Q

What effect does nuclear charge have on first ionisation energy across a period?

A

It increases it

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18
Q

What effect does electron shielding have on first ionisation energy across a period?

A

It has no effect

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19
Q

Is more or less energy needed in sucessive ionisations?

A

More energy is needed

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20
Q

Why is there a decrease in the ionisation energies between the group 2 and 13 elements?

A

Group 13 have the outer electron in a P orbital and group 2 have it in a S orbital, P orbitals have higher energy so are further away from the nucleus and are easier to remove

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21
Q

Why is there a decrease in the ionisation energies between the group 15 and 16 elements?

A

In groups 13, 14 and 15 each P orbitals contain 1 electron and they begin to get spin paired in group 16, they experience more repulsion and makes them easier to remove

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22
Q

Why is there a sharp decrease in ionisation energy between the end of one period and the start of another?

A

With the addition of a new shell it increases the distance of that shell from the nucleus and increases the electron shielding

23
Q

What happenes to the ionisation energies as you move down a group?

A

It decreases

24
Q

Why does ionisation energy decrease as you move down a group?

A
  • number of shells increases
  • shielding increases
  • atomic radius increases
    (nuclear charge has no effect)
25
Q

What are the characteristics of metallic bonding?

A
  • cations are in fixed positions
  • delocalised electrons between ions
  • electrostatic attraction between ions and delocalised electrons produces the bond
26
Q

What structure do metals form?

A

Giant metal lattice structures

27
Q

What are the properties of giant mettalic lattices?

A
  • high melting and boiling points
  • good electrical conductivity
  • malleability and ductility
28
Q

Why do metals have a high melting and boiling point?

A

The atrraction between the positive ions and negative freemoving electrons is very strong and a lot of energy is needed to overcome the mettalic bonds which results in a high temperature

29
Q

Why do metals have good electrical conductivity?

A

The delocalised electrons are free moving and they can carry charge even in a solid state resulting in electrical conductivity

30
Q

Why are metals malleable and ductile?

A

Since the electrons are free to move the structure has a degree of ‘give’ which allows atoms to slide past eachother

31
Q

What does ductile mean?

A

Can be drawn out or streched

31
Q

What does malleable mean?

A

Can be hammered into different shapes

32
Q

What happens to the boiling point as you move across the period with metals?

A

The boiling point increases

33
Q

What is charge density?

A

The ratio of ions’ charge to its size

34
Q

How does the number of free electrons affect the strength of the force?

A

The more free electrons per cation the stronger the forces of attraction

35
Q

What structure does silicon have?

A

Macromolecular structure

36
Q

What does a recation between a group 2 metal and water create?

A

Metal hydroxide + hydrogen

37
Q

How does solubility change as you move down group 2?

A

It increases

38
Q

How does the boiling point change as you move down the halogen group?

A

It increases

39
Q

Which does boiling point increase as you move down the halogen group?

A

Since they have extra shells of electrons which leads to more stronger london forces between molecules

40
Q

How does reactivity change as you move down group 7?

A

It decreases

41
Q

Why does reactivity decrease down group 7?

A
  • atomic radius increases
  • electron shielding increases
  • the ability to gaon an electron in the P subshell to form an ion decreases
42
Q

What colour do the halogens form in water?

A
  • Cl2 = pale green
  • Br2 = orange
  • I2 = brown
43
Q

What colour do halogens form in a non polar solvent (cyclohexane)?

A
  • Cl2 = pale green
  • Br2 = orange
  • I2 = violet
44
Q

What is a disproportionation reaction?

A

A reaction in which the same element is both oxidised and reduced

45
Q

How do you test for carbonate ions (CO3 -2)?

A
  • add a dilute strong acid to the solution
  • Collect any gas formed and pass it through limewater
46
Q

What is a positive result for a carbonate ion test?

A
  • colourless gass produces
  • gas turns limewater cloudy
47
Q

How do you test for sulfate ions (SO4 -2)?

A
  • add dilute hydrochloric acid and barium chloride to the solution
48
Q

What is a positive result for a sulfate ion test?

A
  • white precipitate of barium sulfate is produced
49
Q

How do you test for halide ions (Cl, Br, I)?

A
  • dissolve solution in water
  • add aqueous solution of silver nitrate
  • note the colour of precipitate formed
  • add aqueous ammonia if colour is hard to tell
  • note solubility of the precipitate in ammonia
50
Q

What is a positive result for a halide ion test?

A
  • silver chloride - white precipitate + soluble in dilute ammonia
  • silver bromide - cream precipitate + soluble in conc. ammonia
  • silver iodide - yellow precipitate + insoluble in ammonia
51
Q

How do you test for ammonium ions (NH4+)?

A
  • add sodium hydroxide solution to the solution
  • warm gently
  • test any gas produced with red litmus paper
52
Q

What is a positive result for an ammonium ion test?

A
  • ammonia gas will turn litmus paper blue
  • ammonia gas has a distinctive smell

Chem Module 3 (3 decks)

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