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Inorganic Chemistry > Group 2 And 7 > Flashcards

Group 2 And 7 Flashcards

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1
Q

Atomic radius - 2

A

Increases
-NO. Principal energy levels increases
- Shielding increases
- less attraction between Valence e- and nucleus

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2
Q

First IE down group 2

A

Decreases
- NO. Principal E levels increases
- shielding increases
- weaker attraction between valence e- and nucleus

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3
Q

Melting point down group 2

A

Decreases
- size of ion increases
- weaker electrostatic forces of attraction between positive ions and delocalised e-

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4
Q

Group 2 + water reactivity down group

A

-More reactive down group
-atomic radius increases
- shielding increases
- reactivity increases

More vigorous, warmer, more ppt

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5
Q

Group 2 + water eqn

A

X + H2O -> X(OH)2 +H2

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6
Q

Mg with steam

A

Mg + H2O -> MgO + H2
s. g. s. g

White solid white flame

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7
Q

Solubility of group 2 hydroxides (not explanation)

A

Mg - very sparingly white ppt
Ca - sparingly White ppt
Sr - slightly
Ba - soluble

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8
Q

Group 2 hydroxides pH

A

Mg 8-9
Ca 10-11
Sr 11-12
Ba 13-14
More OH- ions in solution

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9
Q

Test for Mg 2+ ions in solution

A

(Sodium) hydroxide + solution with Mg2+
- white ppt of Mg(OH)2
MgCl2 + 2NaOH-> Mg(OH)2 + 2NaCl
Aq. Aq. S. Aq

Mg2+ + 2OH- -> Mg(OH)2
Aq. Aq. S

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10
Q

Test for OH- ions in solution (group 2)

A

Magnesium (chloride) solution + solution with OH-
White ppt of Mg(OH)2

MgCl2 + 2NaOH-> Mg(OH)2 + 2NaCl
Aq. Aq. S. Aq

Mg2+ + 2OH- -> Mg(OH)2
Aq. Aq. S

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11
Q

Test for Ba2+ ions in solution

A

Sulphuric acid + barium ions
White ppt

H2SO4 + BaCl2 -> BaSO4 + 2HCl
Aq. Aq. S. Aq

SO4 ²- + Ba2+ -> BaSO4
Aq. Aq. S

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12
Q

Test for SO4 ²- ions in solutions

A

ACIDIFIED barium (chloride) + sulfate ions

Na2SO4 + BaCl2 -> BaSO4 + 2NaCl
Aq. Aq. S. Aq

SO4 ²- + Ba2+ -> BaSO4
Aq. Aq. S

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13
Q

Why does barium chloride have to be acidified in a sulphate ion test

A

With HCl or HNO3
- Remove carbonate ions that would give false positive
2H+ + CO3 ²- -> CO2 + H2O

BaCO3 formed

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14
Q

Uses of Mg(OH)2

A

Neutralises, excess stomach acid
CaCO3 not used as produces CO2

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15
Q

Ca(OH)3 uses

A

Neutralises acidic soils

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16
Q

CaO & CaCO3 uses

A

Fluegas desulphurisation
Neutralises SO2
CaO + SO2 -> CaSO3

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17
Q

BaSO4 uses

A

CT scans/x-rays
Barium meal, damaged areas of digestive tract seen
Insoluble

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18
Q

BaCl2 uses

A

Test for sulphate in solutions
Ba²- + SO4²- -> BaSO4

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19
Q

Uses of Mg

A

Extraction of titanium

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20
Q

Process of titanium extraction

A

Rutile ore high temp
TiO2 + 2Cl2 + 2C -> TiCl4 + 2CO
S. G. S. G. G

Magnesium used as reducing agent heated, atmosphere of argon (inert)
TiCl4 + 2Mg -> Ti 2MgCl2

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21
Q

Halogens as oxidising agents

A

Down group, less oxidising
-Size increases
-more shielding
-Gain electrons, less readily
-weaker attraction from nucleus

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22
Q

Cl2 + 2NaBr

A

-> 2NaCl + Br2 (yellow)

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23
Q

Cl2 + 2NaI

A

-> 2NaCl + I2 (brown)

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24
Q

Br2 + 2NaI

A

-> NaBr + I2 (brown)

25
Q

Br2 + 2NaCl

A

NVC

26
Q

I2 + 2NaBr

A

NVC

27
Q

I2 + 2NaCl

A

NVC

28
Q

Test for halide ions eqn

A

AgNO3 + NaX -> AgX NaNo3

Ag+ + X- -> AgX

29
Q

AgNO3 + NaF

A

NVC

30
Q

AgNO3 + NaCl

A

White ppt

31
Q

AgNO3 + NaBr

A

Cream ppt

32
Q

AgNO3 + NaI

A

Yellow ppt

33
Q

Silver halides with dilute ammonia

A

AgX + 2NH3 -> Ag(NH3) + X-

AgCl - soluble
AgBr - sparingly
AgI - insoluble

34
Q

Silver halides with concentrated ammonia

A

AgX + 2NH3 -> Ag(NH3) + X-

AgBr - soluble
AgI - insoluble

35
Q

Why does AgNO3 need to be acidified when testing for halide ions

A

To remove hydroxide and carbonate ions, which would form ppt with Ag+

Add dilute nitric acid
2HNO3+Na2CO3 ->2NaNO3+CO2+H2O

Cant use HCl, has Cl

36
Q

Halide ions as reducing agents
Acid base
Eqn

A

NaX + H2SO4 -> NaHSO4 + HX ( misty fumes)

2NaX + H2SO4 -> NaSO4 + 2HX

37
Q

Explain reducing ability of group 7 elements

A

Increases down the group
- Size of ion increases
-Shielding increases
-Outer e- further away from nucleus
-So less attraction
- ions lose e- more readily

38
Q

Br- ions as reducing agents
Redox

A

Br- -> Br2 (Brown Gas)

H2SO4 -> SO2 (Chocking gas)

39
Q

I- ions as reducing agents
Redox

A

I- -> I2. ( black solid, purple Gas)
H2SO4 -> SO2. ( choking gas)
H2SO4 -> S. ( yellow solid)
H2SO4 -> H2S. ( rotten egg smell)

40
Q

Form of Br2

A

Brown gas

41
Q

Form of SO2

A

Choking gas

42
Q

Form of I2

A

Black solid purple Gas

43
Q

Form of S

A

Yellow solid

44
Q

Form of H2S

A

Rotten egg smell

45
Q

Electronegativity of group, 7

A

Decreases down the group
- NO. Principle E levels increases
- Weaker attraction between valence e- and nucleus in covalent bond

46
Q

BP of group, 7

A

Increases down the group
- size of atom increases
- more VdW forces between molecules to be broken

47
Q

Chlorine and water equation

A

Cl2 + H2O -> HCl + HClO
g. l. Aq. Aq

48
Q

Chlorine water (info)

A

Disproportionation
Universal indicator, paper turns red, then bleached white by HClO

49
Q

Chlorine and water and bright sunlight equation

A

2Cl2 + 2H2O -> 4HCl + O2
G

Chlorine bubbled through water

50
Q

Chlorine with sodium hydroxide equation

A

Cl2 + 2NaOH -> H2O + NaCl + NaClO

Cl2 + 2OH- -> H2O + Cl- + ClO-

51
Q

State of F2

A

Pale yellow gas

52
Q

State of Cl2

A

Pale green gas

53
Q

State of Br2

A

Dark red liquid

54
Q

State of I2

A

Dark purple solid

55
Q

What do you use carbonate ions to test for? (Na2CO3)

A

Acids
release CO2 H2O
Effervescence

56
Q

What do you use sulphate ions to test for? (Na2SO4)

A

Barium ions
White ppt

57
Q

What do you use hydroxide ions to test for? (NaOH)

A

Magnesium ions
White ppt
Magnesium hydroxide is insoluble

58
Q

What is the test for ammonium ions?

A

Ammonium containing salt, heated with aqueous sodium hydroxide

Produces ammonia, gas
Turns moist litmus paper blue

(NH4)+ + OH- -> NH3 +H2O

Inorganic Chemistry (1 decks)

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