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inorganic Flashcards

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1
Q

melting point from Na to Al

A

-melting points increase from Na to Al
-because all three are only metallic bonding
-which increases across the period due to higher charge density

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2
Q

melting point at Si

A

-melting point increases significantly at Si
-because it is a macromolecular structure
-which has very strong pure covalent bonds
-that require a lot of energy to break

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3
Q

melting point at p

A

-melting point decreases significantly at p
-because it is only a simple covalent structure
-with only weak Van der Waals

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4
Q

melting point from S to Ar

A

-S has the highest melting point of the non-metal elements
-Cl is next
-Ar has the lowest melting point because it is the smallest (monatomic)
-Van der Waals forces are determined by size

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5
Q

;why does sulfur have slightly higher melting point than phosphorous

A

-Because S is larger than P
-S has 8 atoms whilst P has 4
-thus VDW forces are stronger

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6
Q

Trend in first ionisation energy across period 3

A

-increase across the period
-increased nuclear charge so stronger attraction between the nucleus and electrons
-radius decreased as a result
-no shielding across the period thus does not affect

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7
Q

trend in atomic radius across period 3

A

-decreases across period 3
-because proton is added each time
-so stronger attraction between positive nucleus and negative electrons

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8
Q

Reaction of Al with oxygen

A

burns vigorously with bright white flame
forms 2Al2O3

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9
Q

Reaction of Si with oxygen

A

burns with a bright white flame and white smoke
forms SiO2

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10
Q

Reaction of Na with oxygen

A

burns vigorously with yellow flame
forms 2Na2O

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11
Q

Reaction of Mg with oxygen

A

burns vigorously with a bright white flame
forms 2MgO

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12
Q

Reaction of P with oxygen

A

burns spontaneously with a bright white flame and smoke
forms P4O10

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13
Q

Reaction of S with oxygen

A

burns with a blue flame
forms SO2

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14
Q

Reaction of Na with water

A

2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

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15
Q

Reaction of Mg with water

A

Slow in cold water:
Mg(s) + 2H20(l) → Mg(OH)2(aq) + H2(g)
Vigorous with steam:
Mg(s) + H20(l) → MgO(s) + H2(g)

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16
Q

Reaction of Cl with water

A

dissolves to form chlorine water:
Cl2(aq) + H2O(l) ⇌ HClO(aq) + HCl(aq)

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17
Q

Properties of Na20

A

bonding: ionic
structure: giant ionic lattice
melting point: high

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18
Q

Properties of MgO

A

bonding: ionic/covalent
structure: giant ionic lattice
melting point: high

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19
Q

Why is the melting point higher for Mg than for Na?

A
  • Mg is smaller than Na
  • Mg has a plus 2 charge whilst Na has a plus 1 charge
  • so… stronger attraction between ions in MgO = higher melting point
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20
Q

Properties of Al2O3

A

bonding; ionic/covalent
structure: giant ionic lattice
melting point: high

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21
Q

Properties of SiO2

A

bonding: covalent
structure: giant covalent/ macromolecular
melting point: high

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22
Q

Properties of P4O10

A

bonding: covalent
structure: molecular
melting point: relatively low

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23
Q

properties of SO2 and SO3 and the difference between them

A

bonding: covalent
structure: molecular
melting point: relatively low
difference: SO2 is a gas at room temperature whilst SO3 is a liquid at room temperature

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24
Q

Reaction of NA2O with water
-ions present after reaction
-type of solution
-pH

A

Na+ (aq)
OH− (aq)
strongly alkaline
pH 13-14

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25
Q

Reaction of MgO with water
-ions present after reaction
-type of solution
-pH

A

Mg2+ (aq)
OH- (aq)
moderately alkaline
pH 10

26
Q

Reaction of Al2O3 with water
-ions present after reaction
-type of solution
-pH

A

insoluble
pH 7

27
Q

Reaction of SiO2 with water
-ions present after reaction
-type of solution
-pH

A

insoluble
pH 7

28
Q

Reaction of P4O10 with water
-ions present after reaction
-type of solution
-pH

A

H+ (aq)
H2PO4- (aq)
strongly acidic
pH 0-1

29
Q

Reaction of SO2 with water
-ions present after reaction
-type of solution
-pH

A

H+ (aq)
HSO3- (aq)
weakly acidic
pH 2-3

30
Q

Reaction of SO3 with water
-ions present after reaction
-type of solution
-pH

A

H+ (aq)
HSO4-
strongly acidic
pH 0-1

31
Q

what are the four chemical properties of transition metals

A
  • can form complex ions
  • can form coloured ions
  • variable oxidation states
  • catalytic activity
32
Q

What are the two exceptions- they are not transition metals

A

Scandium and Zinc

33
Q

Why are variable oxidation states possible

A

3d and 4s sublevels are very close in energy thus the electron can be lost from either

34
Q

Shapes of complex ions: LINEAR

A
  • coordination number of 2
  • 180 degrees
35
Q

Shape of complex ions: TETRAHEDRAL

A
  • coordination number of 4
  • 109.5 degrees
  • most common with 4
36
Q

Shape of complex ions: SQUARE PLANAR

A
  • coordination number of 4
  • 90 degrees
37
Q

Shape of complex ions: OCTAHEDRAL

A
  • coordination number of 6
  • 90 degrees
38
Q

What are all the trends going down group 2?

A
  • atomic radius increases
  • shielding increases
  • reactivity increases
  • ionisation energy decreases
  • melting point decreases
  • solubility of hydroxides increases
  • solubility of sulphates decreases
39
Q

what is the general equation for group 2 metals reacting with water

A

metal + 2water —-> metal(OH)2 + H2

40
Q

what happens when magnesium reacts with water

A

two reactions:
1. with cold water- much slower
Mg + 2H2O —-> Mg(OH)2 + H2
2. with steam- much faster
Mg + H2O —-> MgO + H2

41
Q

what is the other exception in the reaction with water

A

Beryllium
Be + H2O —-> BeO + H2

42
Q

when are group 2 metals used in medicine

A
  1. Mg(OH)2. is the least soluble hydroxide so is used as an antacid as it can neutralise stomach acids without dissolving into the bloodstream
  2. BaSO4. Is the least soluble sulphate so is used as a barium cookie as a medical tracer. If dissolved into the bloodstream it would be toxic however its insolubility prevents this.
43
Q

when are group 2 metals used in agriculture and industry

A
  1. Mg(OH)2 is the least soluble hydroxide so is used in agriculture to neutralise acidic soils
  2. Magnesium can also be used in the extraction of titanium via a displacement reaction.
    TiCl4 + 2Mg —-> 2MgCl2 + Ti
44
Q

what is the equation for the reduction of vanadium from yellow to blue

A

Write out

45
Q

what is the equation for the reduction of vanadium from blue to green

A

write out

46
Q

What is the original aqueous solution for Copper(ll) both colour and equation

A

blue solution
write out

47
Q

what is the colour and equation of copper (ll) after addition of NaOH

A

blue ppt
write out

48
Q

what is the colour and equation of copper (ll) after addition of excess NaOH

A

no further change

49
Q

What is the colour and equation of copper (ll) after addition of NH3

A

blue ppt
write out

50
Q

What is the colour and equation of copper (ll) after addition of excess NH3

A

deep blue solution
write out

51
Q

What is the colour and solution of copper (ll) after addition of Na2CO3

A

green-blue ppt
write out

52
Q

what is the equation that happens when excess NH3 is added to copper(ll) hexaqua complex

A

Cu(H2O)4(OH)2 + 4NH3 —> [Cu(H2O)2(NH3)4]2+ + 2H2O + 2OH-

53
Q

What is the equation that happens when NaOH is added to copper(ll) haxaqua complex

A

[Cu(H2O)6]2+ + 2NaOH —> Cu(H2O)4(OH)2 + 2H2O

54
Q

what is the equation that happens when NH3 is added to copper(ll) haxaqua complex

A

[Cu(H2O)6]2+ + 2NH3 —> Cu(H2O)4(OH)2 + 2NH4+

55
Q

What is the equation that happens when Na2CO3 is added to copper(ll) hexaqua complex

A

[Cu(H2O)6]2+ + CO3 2- —> CuCO3 + 6H2O

56
Q

What is the original aqueous solution for Iron(ll) both colour and equation

A

green solution
[Fe(H2O)6]2+

57
Q

what is the colour and equation of iron (ll) after addition of NaOH

A

green ppt
Fe(H2O)4(OH)2
[Fe(H2O)6] + 2NaOH —> Fe(H2O)4(OH)2 + 2H2O

58
Q

what is the colour and equation of iron (ll) after addition of excess NaOH

A

no further change

59
Q

what is the colour and equation of iron (ll) after addition of NH3

A

green ppt
Fe(H2O)4(OH)2
[Fe(H2O)6] + 2NH3 —> Fe(H2O)4(OH)2

60
Q

what is the colour and equation of iron (ll) after addition of excess NH3

A

no further change

61
Q

What is the colour and equation of iron(ll) after addition of Na2CO3

A

green ppt
FeCO3
[Fe(H2O)6] + CO3 2- —> FeCO3

62
Q
A

chemistry (3 decks)

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