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Inorganic > s-block > Flashcards

s-block Flashcards

1
Q

Write the products of Li with Oxygen gas

A

Li2O

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2
Q

Write the products of Na with Oxygen gas

A

Na2O

Na2O2 (excess oxygen)

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3
Q

Write the products of K with Oxygen gas

A

K2O

K2O2

KO2

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4
Q

Write the products of Rb with Oxygen gas

A

Rb2O

Rb2O2

RbO2

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5
Q

Write the products of Cs with Oxygen gas

A

Cs2O

Cs2O2

CsO2

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6
Q

What’s the only element that reacts with nitrogen gas in first group?

A

Li

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7
Q

Write the reactions of Li with N2 gas

A

Li —> Li3N

Li3N +3H20 —> 3LiOH + NH3

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8
Q

How do 1st group elements react with hydrogen gas?

A

Li –> LiH
Na –> NaH
K –> KH
Cs – CsH
Rb –> RbH

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9
Q

What’s the nature of group 1 hydrides?

A

Ionic

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10
Q

How do group 1 hydrides react w water?

A

They react vigorously

NaH + H2O –> NaOH + H2

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11
Q

Write the reactions of group 1 metals with cold water?

A

Na + H20 —> NaOH + H2

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12
Q

Write the nature of the reactions of group1 metals reacting w cold water

A

Li –> Gently
Na –> Vigorously
K –> Vigorously w/ ignition
Rb/Cs –> Explosively

Na, K, Rb, Cs show exothermic reactions

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13
Q

How do the group 1 oxides react with water?

A

Li2O + H2O –> LiOH
Na2O + H20 –> NaOH
K2O + H2O –> KOH

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14
Q

Explain the variation of the base strength of first group metals down the group

A

increases

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15
Q

What’s the reaction of group 1 peroxides w water?

A

Na2O2 + H2O –> NaOH + H2O2

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16
Q

What’s the reaction of 1st group superoxide w water?

A

KO2 + H2O –> KOH + H202 + O2

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17
Q

Describe the reaction of acids with group 1 metals

A

Forms the salt and hydrogen gas

Na + HCl —> NaCl + H2

Li + H2SO4 –> Na2SO4 + H2

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18
Q

Describe the reactions of group 1 metal hydroxides with CO2

A

NaOH + CO2 –> Na2CO3 + H2O

Na2CO3 + CO2 + H20 –> NaHCO3

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19
Q

Write the products of Be with oxygen gas

A

BeO

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20
Q

Write the products of Mg with oxygen gas

A

MgO

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21
Q

Write the products of Ca with oxygen gas

A

CaO

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22
Q

Write the products of Sr with oxygen gas

A

SrO

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23
Q

Write the products of Ba with oxygen gas

A

BaO

BaO2

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24
Q

Write the reactions of group 2 elements with nitrogen gas

A

M + N2 —> M3N2 (yellow)

M3N2 + H20 –> M(OH)2 + NH3

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25
Q

Which group 2 element doesn’t react with Hydrogen gas?

A

Be

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26
Q

Do all group 2 elements react w hydrogen gas?

A

No. Be doesn’t

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27
Q

Write the products of group 2 metals reacting w hydrogen gas

A

Mg + H2 –> MgH2 ( at high pressure)

Ca + H2 –> CaH2 (at high temp.)

Sr + H2 –> SrH2 (at high temp.)

Ba + H2 –> BaH2 (at high temp.)

Then: CaH2 + H20 –> Ca(OH)2 + 2H2 (not
violent as group 1)

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28
Q

Write the nature of the group 2 metallic hydrides

A

They’re all ionic solids.

Ionic character increases down the group

29
Q

Describe the reactivity of Be with water

A

Be doesn’t react with room temperature water, cold water or hot water

It reacts with steam as:
Be + H2O –> BeO + H2

30
Q

Describe the reactivity of Mg with water

A

Doesn’t react with cold water or room temperature water

Reacts SLOWLY with hot water

Mg + 2H2O —> Mg(OH)2 + H2

Reacts with steam

31
Q

Describe the reactivity of Ca/Sr/Ba with water

A

Readily reacts with water

Ca + H20 –> Ca(OH)2 + H2

Reacts with steam

32
Q

How does reactivity of group 2 metals with water vary?

A

it increases down the group

33
Q

Write reactions of group 2 metals with dilute acids

A

Do not act as oxidizing agents

Mg + HCl –> MgCl + H2

34
Q

Write reactions of group 2 metals with concentrated acids

A

They show oxidizing properties with H2SO4 and HNO2

Mg + H2SO4 –> MgSO4 + SO2 + 2H20

Mg + HNO3 –> Mg(NO3)2 + NO2 + H20

They don’t show oxidizing properties w HCl

Mg + HCl –> MgCl + H2

35
Q

How do group 1 hydroxides decompose?

A

LiOH —> Li2O + H2O
NaOH –> do not decompose
KOH –> do not decompose
RbOH –> do not decompose

36
Q

How do group 2 hydroxides decompose?

A

Be(OH)2 –> BeO + H2O

Mg(OH)2 –> MgO + H2O

Ca(OH)2 –> CaO + H2O

Sr(OH)2 –> SrO + H2O

Ba(OH)2 –> BaO + H20

37
Q

What’s the only group 1 hydroxide that decomposes?

A

LiOH

38
Q

How do group 1 carbonates decompose?

A

Li2CO3 –> Li2O + CO2

Na2CO3 –> do not decompose

K2CO3 –> do not decompose

Rb2CO3 –> do not decompose

Cs2CO3 –> do not decompose

39
Q

What’s the only group 1 carbonate that can decompose?

A

Li2CO3

40
Q

How do group 2 carbonates decompose?

A

BeCO3 –> BeO + CO2

MgCO3 –> MgO + CO2

CaCO3 –> CaO + CO2

SrCO3 –> SrO + CO2

BaCO3 –> BaO + CO2

41
Q

Describe the physical nature of group 1 bicarbonates

A

LiHCO3 –> Aqueous solution

NaHCO3 –> solid

KHCO3 –> solid

RBHCO3 –> solid

42
Q

Describe the decomposition of bicarbonates of group 1

A

LiHCO3 —> Li2CO3 + CO2 + H20

NaHCO3 —> Na2CO3 + CO2 + H20

Li2CO3 is a water insoluble white precipitate

The rest of the carbonates are water soluble solids

43
Q

Describe the physical nature of the carbonates of group 1

A

Li2CO3 is a water insoluble white precipitate

The rest of the carbonates are water soluble solids

44
Q

Describe the physical nature of the carbonates of group 2

A

They are all water insoluble precipitates

45
Q

Describe the decomposition of bicarbonates of group 2

A

Be(HCO3)2 —> BeCO3 + CO2 + H20

46
Q

Describe the physical nature of group 2 bicarbonates

A

They are aqueous solutions

47
Q

Describe the decomposition of group 1 nitrates

A

LiNO3 –> Li2O + NO2 + O2

(reddish brown NO2 evolves)

NaNO3 —> NaNO2 + O2

KNO3 —> KNO3 + O2

RbNO3 —> RBNO3 + O2

48
Q

Describe the decomposition of group 2 nitrates

A

Be(NO3)2 —> BeO + NO2 + O2

49
Q

What are s block elements?

A

elements which fill the last electron to a s-subshell

50
Q

Give alternate names for group I and group II elements

A

Group I –> alkali metals

Group II –> alkali earth metals

51
Q

Metallic character of s block elements

A

H is a non-metal

The rest are metals

52
Q

common electronic configuration of group 1

A

ns1

53
Q

Which group 1 elements do not reach a stable octet?

A

H and Li

54
Q

Valency of group 1

A

always 1

55
Q

Oxidation state of group 1

A

+1 and 0 (H can also have -1)

56
Q

Natural resources containing group 1 metals

A

NaCl - rock salt

Na2B4O7. 10.H2O —> borax (primary standard substance)

KCl - sylvite

KCl. MgCl2. 6H2O - Carnallite

57
Q

metallic character of group 11 elements

A

all are metals

Be is an amphoteric metal

58
Q

valency and oxidation no.

A

+2

59
Q

natural sources containing group II elements

A

CaCO3 - calcite. limestone
MgCO3 - magnesite
CaCO3. MgCO3 - dolomite
KCl. MgCl2. 6H2O - Carnallite
CaSO4. 2H2O - Gypsum
3Ca3(PO4)2. CaF2 - Fluroapatite
3Ca3(PO4)2. CaCl2 - Chlorapatite

60
Q

color of Li with flame test

A

Crimson red

61
Q

color of Na with flame test

A

Yellow

62
Q

color of K with flame test

A

Lilac / violet

63
Q

color of Rb with flame test

A

Red-violet

64
Q

color of Cs with flame test

A

Blue - violet

65
Q

color of Mg with flame test

A

-

66
Q

color of Be with flame test

A

-

67
Q

color of Ca with flame test

A

orange red

68
Q

color of Sr with flame test

A

crimson red

69
Q

color of ba with flame test

A

yellowish green

Inorganic (8 decks)

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