Periodicity Flashcards

1
Q

What is Periodicity?

A

A regular periodic variation of properties of elements with atomic number and position in the periodic table

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2
Q

What is the trend for atomic radius across a period?

A

It decreases because as the number of protons increases, the positive charge of the nucleus increases. This means that the electrons are pulled closer to the nucleus, making the atomic radius smaller.

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3
Q

What is the general trend for melting point across Period 3

A

The melting point increases from sodium to silicon, but then generally decrease from silicon to argon.

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4
Q

What is the First ionisation energy?

A

The energy needed to remove one electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions.

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5
Q

What is the trend for first ionisation energy for Period 3?

A

There is a general increase as you go across, because of the increasing attraction between the outer shell electrons and the nucleus, due to the number of protons increasing.

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6
Q

What is the trend in atomic radius for Group 2?

A

Down the group the atomic radii increases, because an increasing number of shells means that the atoms get bigger

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7
Q

What is the general trend in ionisation energies for Group 2?

A

They decrease down the group because:
- Atoms get bigger so the outermost electrons are further from the nucleus
- More electron shells mean shielding increases
So overall attraction to the outer electron decreases.

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8
Q

What is the general trend in melting point for Group 2?

A

It decreases down the group:
- Atoms get bigger so the delocalised electrons are further from the nucleus
- More electron shells meaning shielding increases
Overall attraction to the delocalised electrons decreases, which means the metallic bonding is weaker and requires less energy to break it

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9
Q

What is the trend in reactivity for Group 2?

A

Reactivity increases down the group:

  • Atomic radii increases down group - increased number of shells means atoms get bigger and there is less attraction between the outermost electron and nuclei meaning they are more reactive.
  • They react by losing 2 electrons, forming positive ions - easier to lose electrons = more reactive
  • Shielding increases
  • Lower nuclear attraction to outermost electron
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10
Q

For Group two melting point, why is there a ‘blip’ for magnesium?

A

Its crystal structure (the arrangement of metallic ions) changes.

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11
Q

What is formed from a reaction between water and a metal?

A

A hydroxide is formed.

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12
Q

What is the equation for the reaction between a metal and water?

A

M = metal

- M + 2H2O (l) —-> M(OH)2 (aq) + H2 (g)

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13
Q

What is the equation for the reaction between Magnesium and water vapour?

A
  • Mg (s) + H2O (g) —> MgO (s) + H2 (g)

During this reaction a bright white flame will be observed.

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14
Q

What is the trend with the reaction of water down Group 2?

A
  • The reaction gets more vigorous further down the group.
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15
Q

What observations are made from the reaction between a metal and water?

A
  • Fizzing
  • The metal will dissolve
  • Exothermic - the reaction will feel hot
  • The resulting solution will be alkaline
  • Some precipitate, amount depends on solubility of the hydroxide produced
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16
Q

What is the trend in solubility for the hydroxides?

A

The solubility increases down the group.
Ba(OH)2 is most soluble
Mg(OH)2 is least soluble

17
Q

What is Calcium Hydroxide used for?

A
  • In agriculture to neutralise acidic soil
  • Can be used to test for CO2:
    Ca(OH)2 (aq) + CO2 (g) —> CaCO3 (s) + H2O (l)
18
Q

What is Magnesium Hydroxide used for?

A
  • Used in medicine to treat indigestion - it does this by neutralising stomach acid.
19
Q

What is the trend in solubility for sulfates?

A
  • Solubility decreases down the group.
    MgSO4 most soluble
    BaSO4 least soluble
20
Q

What is Barium sulfate used for?

A
  • It is used in medicine as a barium med - used for x-rays to observe soft tissues like internal organs
  • It is very toxic, but can be used as it is completely insoluble
21
Q

How do we test for sulfate ions?

A
  • Acidified BaCl2 is added to the unknown solution
    (Acidified in HCl as this removes impurities such as carbonate ions - solution will fizz)
  • If sulfate ions are present a white precipitate will form: Ba2+ (aq) + SO42- (aq) –> BaSO4 (s)
22
Q

Why is titanium useful?

A
  • It is abundant
  • It is low density
  • It resists corrosion
    However it must be extracted from its ore.
23
Q

Extraction of Titanium

A
  • Mg is used to extract Ti from its ore (Mg is more reactive than Ti)
  • Main titanium ore TiO2 is converted to TiCl4 by heating to 900 degrees C with carbon in stream of Cl2 (g)
  • TiCl4 is then purified by fractional distillation in an Ar atmosphere, then reduced by Mg in a furnace at 500 degrees C, again under Ar
24
Q

What is the equation for the conversion of TiO2 to TiCl4?

A

TiO2 + 2Cl2 + 2C —> TiCl4 + 2CO

25
Q

What is the equation for the reduction of TiCl4 by Mg?

A

TiCl4 (g) + 2Mg (l) —> Ti (s) + 2MgCl2 (l)

26
Q

Why is Titanium expensive?

A
  • Both purification steps require high temperatures
  • It is a batch process
  • Magnesium is expensive
  • Argon is expensive (maintaining argon atmosphere)