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Inorganic Chemistry > lecture 6 > Flashcards

lecture 6 Flashcards

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1
Q

characteristics of alkali metals

A

dissolved in water giving an alkaline solution.

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2
Q

elements in alkali metals

A

lithium, sodium, potassium, Rubidium, cesium, francium.

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3
Q

what are the most abundant alkali metals.

A

sodium and potassium.

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4
Q

most rate alkali metals.

A

rubidium, lithium, cesium

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5
Q

how is alkali metals are extracted?

A
  • electrolysis of molten halides with something that decreases the degree of fusion.
  • down process.
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6
Q

extracting sodium

A

electrophoretic analysis of the photograph with sodium chloride, calcium chloride.
2 NaCl -> 2 Na + Cl2

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6
Q

extracting sodium

A

electrophoretic analysis of the photograph with sodium chloride, calcium chloride.
2 NaCl -> 2 Na + Cl2

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7
Q

extraction of potassium

A

sodium vapor with molten potassium chloride.

Na + KCl -> K + NaCl

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8
Q

extraction of lithium

A

electrophoretic analysis of a mixture of lithium chloride and potassium chloride.

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9
Q

extraction of rubidium and cesium

A

reduction metal chlorides by calcium

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10
Q

what is the down process.

A

it’s the process to extract sodium.

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11
Q

how does the down process work?

A

molten NaCl is electrolyzed and calcium chloride is added to reduce the temperature.

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12
Q

why does the design of the electrolysis unit matter?

A

because it prevents the sodium and calcium from combining.

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13
Q

why is the metal bonding in alkali metals weak?

A

because of the attraction between delocalized electrons and the metal ion core in crystalline structures.

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14
Q

physical characteristics of alkali metals.

A

low melting point and soft consistancy.

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15
Q

reactivity of alkali metals.

A

highly reactive. and it is a powerful reducing agent,

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16
Q

heat of atomization in alkali metals. as it goes through group.

A

low and decreases as it goes down the group.

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17
Q

what is the heat of atomization?

A

the heat required to turn solid to a single gaseous atom.

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18
Q

ionization energy in alkali metals? as it goes through group?

A

low.

the larger the size, the lower the energy

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19
Q

size of atom in group.

A

decreases considerably when it loses an electron.

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20
Q

lattice energy of alkali metals as it goes through group.

A

decreases

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21
Q

relation between atomic radius and force of attraction?

A

square of atomic radius is inversely proportional to force of attraction.

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22
Q

solubility in alkali metals.

A

water soluble.

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23
Q

why are alkali metals solube?

A

because the attraction between the ion and the polar water molecule.

24
Q

result of mixing water and alkali metal?

A

highly exothermic reaction. (heat of hydration)

25
Q

entropy in alkaline metals.

A

increases as ions disperse into solution.

26
Q

hydration energy in alkali metals.

A

decreases as ionic size increases.

27
Q

normal order of stability vs aqueous ion order of stability

A

normal -> decreases as ionic size increases.

aqueous ion -> increases.

28
Q

flame color of alkali metals.

A

lithium -> red
sodium -> orange
potassium -> lilac

29
Q

how can alkali metal oxides be obtained. chemical equation.

A

with limited air supply but it’s better to prepare it by thermal decomposition of peroxides.
4 Li + O2 -> 2 Li2O

30
Q

example of alkali metal peroxide.

A

2Na + O2 -> Na2O2

31
Q

example of alkali metal super oxide.

A

K + O2 -> KO2

32
Q

use of alkali metal oxide, peroxide and super oxide.

A

KO2 is used in breathing masks

as KO2 reacts with water to make oxygen and KOH which absorbs water.

33
Q

chemical equations for metal oxide and water reacting.

A

1- M2O + H2O -> 2 MOH
2- M2O2 + 2 H2O -> 2 MOH + H2O2
3- 2 MO2 + 2 H2O -> 2 MOH +H2O2 + O2
4- KOH + CO2 -> KHCO3

34
Q

how are alkali metals stored? and why.

A

they submerged in liquid hydrocarbons (oil)

because they react to the weather.

35
Q

reaction: water and alkali metals

A

highly reactive with a strong violent reaction.

releases a high amount of energy that ignites the oxygen around it.

36
Q

alkali metals reacting with acid.

A

violent. (highly reactive)

metals replace the hydrogen acid.

37
Q

alkali metals reacting with acid. chemical equation example.

A

2 Na + 2 HCl -> 2 NaCl + H2

2K + H2SO4 -> K2SO4 + H2

38
Q

alkali metals reacting with oxygen

A

creat metal hydride and ionic compound.

39
Q

alkali metals reacting with oxygen. chemical equation

A

2 Li + H2-> 2LiH

40
Q

alkali metals reacting with halides.

A

direct combination with large negative enthalpy of fusion.

41
Q

alkali metals reacting with halides. chemical equation

A

2Na + Cl2 -> 2 NaCl

42
Q

what is the only alkali metal that reacts with non-metals?

A

lithium only reacts with nitrogen.

43
Q

Lithium reacting with nitrogen chemical equation.

A

6 Li + Cl2 -> 2 Li3N

=> Li3N +3 H20 -> LiOH + NH3

44
Q

what is potassium nitrite used for and why?

A

as explosive because it’s a non-wet material and reacts with oxygen.

45
Q

why can’t sodium nitrate be used for explosives?

A

because it absorbs water.

46
Q

what is sodium hydroxides used for? and why.

A

used in acid equations because it reacts with the acid making salt and water.

47
Q

real world application of sodium hydroxides.

A

soap, paper, fabric, oil purification.

48
Q

potaasium hydride is used for.

A

batteries.

49
Q

example of sodium hydroxide being used in the industry,

A

2 NaCl -[electrolysis]-> 2 NaOH + H2 + Cl2

50
Q

source of sodium carbonate.

A

trons ore which is a mix of sodium bicarbonate and sodium carbonate.

51
Q

sodium carbonate chemical symbol

A

Na2CO3NaHCO32H2O

52
Q

solvay process

A

the process of making sodium carbonate from salt and limestone.

53
Q

chemical equations for solvay process.

A

CaCO3 -[heat]-> CaO +CO2
NH3 + CO2+ H2O + NaCl -> NaHCO3 + NH4Cl
2 NaHCO3 -[heat]-> Na2CO3 + H2O + CO2

54
Q

what is sodium carbonate used for?

A

glass making, paper, soap, ph regulator.

55
Q

lithium is used for?

A

batteries. alloys. medical treatment.

56
Q

sodium bicarbonate used in.

A

baking

57
Q

elemental sodium used in

A

street lights and nuclear reactors.

Inorganic Chemistry (5 decks)

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