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Inorganic Chemistry > Group 2 And 7 > Flashcards

Group 2 And 7 Flashcards

(58 cards)

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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

Study These Flashcards
A

-> NaBr + I2 (brown)

25
Br2 + 2NaCl
NVC
26
I2 + 2NaBr
NVC
27
I2 + 2NaCl
NVC
28
Test for halide ions eqn
AgNO3 + NaX -> AgX NaNo3 Ag+ + X- -> AgX
29
AgNO3 + NaF
NVC
30
AgNO3 + NaCl
White ppt
31
AgNO3 + NaBr
Cream ppt
32
AgNO3 + NaI
Yellow ppt
33
Silver halides with dilute ammonia
AgX + 2NH3 -> Ag(NH3) + X- AgCl - soluble AgBr - sparingly AgI - insoluble
34
Silver halides with concentrated ammonia
AgX + 2NH3 -> Ag(NH3) + X- AgBr - soluble AgI - insoluble
35
Why does AgNO3 need to be acidified when testing for halide ions
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
Halide ions as reducing agents Acid base Eqn
NaX + H2SO4 -> NaHSO4 + HX ( misty fumes) 2NaX + H2SO4 -> NaSO4 + 2HX
37
Explain reducing ability of group 7 elements
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
Br- ions as reducing agents Redox
Br- -> Br2 (Brown Gas) H2SO4 -> SO2 (Chocking gas)
39
I- ions as reducing agents Redox
I- -> I2. ( black solid, purple Gas) H2SO4 -> SO2. ( choking gas) H2SO4 -> S. ( yellow solid) H2SO4 -> H2S. ( rotten egg smell)
40
Form of Br2
Brown gas
41
Form of SO2
Choking gas
42
Form of I2
Black solid purple Gas
43
Form of S
Yellow solid
44
Form of H2S
Rotten egg smell
45
Electronegativity of group, 7
Decreases down the group - NO. Principle E levels increases - Weaker attraction between valence e- and nucleus in covalent bond
46
BP of group, 7
Increases down the group - size of atom increases - more VdW forces between molecules to be broken
47
Chlorine and water equation
Cl2 + H2O -> HCl + HClO g. l. Aq. Aq
48
Chlorine water (info)
Disproportionation Universal indicator, paper turns red, then bleached white by HClO
49
Chlorine and water and bright sunlight equation
2Cl2 + 2H2O -> 4HCl + O2 G Chlorine bubbled through water
50
Chlorine with sodium hydroxide equation
Cl2 + 2NaOH -> H2O + NaCl + NaClO Cl2 + 2OH- -> H2O + Cl- + ClO-
51
State of F2
Pale yellow gas
52
State of Cl2
Pale green gas
53
State of Br2
Dark red liquid
54
State of I2
Dark purple solid
55
What do you use carbonate ions to test for? (Na2CO3)
Acids release CO2 H2O Effervescence
56
What do you use sulphate ions to test for? (Na2SO4)
Barium ions White ppt
57
What do you use hydroxide ions to test for? (NaOH)
Magnesium ions White ppt Magnesium hydroxide is insoluble
58
What is the test for ammonium ions?
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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