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Chemistry > S Block Elements > Flashcards

S Block Elements Flashcards

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1
Q

Group1 elements trends

A

Alikaline metals
They are soft metals having a low density
Highly reactive metals and reactivity incrrases down the group.

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2
Q

Reactions with oxygen

Group 1 metals

A

Generally forms the metal oxide
Na produces peroxides with excess oxygen
K, Rb, Cs produces superoxides with excess oxygen

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3
Q

Reactions with air

Group 1 metals

A

With nitogen Li gives Li3N, K,Na does not react with N2

When K is burnt in air, KO2 is produced as the main product while peroxides and oxides are also formed.

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4
Q

Na2O(s) + H2O(l)

A

2NaOH(aq)

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5
Q

Li3N(s) + 3H2O(l)

A

3LiOH(aq) + NH3(g)

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6
Q

2NaOH(aq) + CO2(g)

A

Na2CO3(aq) + H2O(l)

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7
Q

2Na(s) + H2(g)

A

2NaH(s)

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8
Q

NaH(s) + H2O(l)

A

NaOH(aq) + H2(g)

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9
Q

2Li(s) + dil. 2HNO3(aq)

A

2LiNO3(aq) + H2(g)

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10
Q

2Na(s) + dil. H2SO4(aq)

A

Na2SO4(aq) + H2(g)

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11
Q

4LiNO3(s)

A

2Li2O(s) + 4NO2(g) + O2(g)

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12
Q

2KNO3(s)

A

2KNO2(s) + O2(g)

General reaction for all other group 1 metal nitrates except Li(diagonal relationship with Mg)

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13
Q

Li2CO3(s)

A

Li2O(s) + CO2(g)
Less stable and gets decomposed easily.
Other group 1 carbonates are stable and they will melt before getting decomposed.

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14
Q

2NaHCO3(s)

A

Na2CO3(s) + H2O(g) + CO2(g)

General reaction for group 1 metals.

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15
Q

Solubility of Group 1 salts

A

All Group 1 salts are soluble in water except some lithium salts such as LiF, Li2CO3 and
Li3PO4. All these salts are white solids unless the salt anion is a coloured ion.
Solubility of Group 1 halides increase down the group

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16
Q

Flame test- Lithium

A

– Crimson red

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17
Q

Flame test- Sodium

A

Yellow

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18
Q

Flame test- Rubidium

A

Red-violet

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19
Q

Flame test- Caesium

A

Blue-violet

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20
Q

Flame test- Potassium

A

Lilac

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21
Q

Group 2 elements trends

A

They are known as alkaline earth metals. They are less reactive than Group 1 metals due to its valence shell ns2
electron configuration.
Group 2 metal oxides produce basic oxides except for BeO which shows amphoteric properties.

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22
Q

Reaction with water

Group 2 metals

A

Beryllium does not react with water, but it reacts with steam. The reaction of magnesium
with water at room temperature is negligible. However, magnesium reacts slowly with
hot water. Calcium, strontium and barium react readily with cold water.
Ca(s) + 2H2O(l)———-> Ca(OH)2(aq) + H2(g)

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23
Q

Ca(s) + H2(g)

A

CaH2(s)

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24
Q

CaH2(s) + 2H2O(l)

A

Ca(OH)2(aq) + 2H2(g)

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25
Q

3Mg (s) + N2(g)

A

Mg3N2(s)

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26
Q

Mg3N2(s) + 6H2O(l)

A

3Mg(OH)2(aq) + 2NH3(g)

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27
Q

2Mg(NO3)2(s)

A

2MgO(s) + 4NO2(g) + O2(g)
Behaves similar to LiNO3
All nitrates are soluble in water.

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28
Q

MCO3

A

MO + CO2
Thermal stability of group 2 metals increases down the group.
When going down the group the polarizing power of the cation decrease resulting in a less polarized anion.
Less the polarization of the anion more the thermal stability.

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29
Q

Ca(HCO3)2(aq)

A

CaCO3(s) + CO2(g) + H2O(l)

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30
Q

Flame test- Calcium

A

Orange-red

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31
Q

Flame test- Strontium

A

Crimson red

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32
Q

Flame test- Barium

A

Yellowish green

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33
Q

Colors of carbonates formed by group 2 metals

A

All formed carbonates are white.

34
Q

Solubility of Group 2 nitrates

A

All group 2 nitrates are soluble in water.

35
Q

Solubility of Group1 salts

A

All salts of group1 are soluble except some Li salts such as PO42-, F, CO32-

36
Q

Solubility of group 2 carbonates and phosphates

A

All are insoluble

37
Q

Solubility of group 2 hydroxides

A 
From Mg to Ba solubility increases
Mg - IS
Ca - SS
Sr - SS
Ba - aq
38
Q

Solubility of group 2 Sulfates

A 
From Mg - Ba solubility decreases
Mg - aq
Ca - SS
Sr  - IS
Ba -  IS
39
Q

Solubility of group 2 Sulfites

A

Except Mg all others are insoluble while Mg is sparingly soluble

40
Q

Solubility of group 2 chromates

A

Mg, Ca - aq

Sr, Ba - IS

41
Q

Solubility of group 2 oxalates

A

Mg, Ba - SS

Ca, Sr - IS

42
Q

Which has largest ionic radii in water?

A

Li

43
Q

Basicity of s block elements depends on

A

Depends on the electropositivity of the elements
Higher the electropositivity higher the basic character
Lower the ionization energy higher the electropositivity

44
Q

Ionic radii in water of s block elements

A

Smaller the cationic radius larger the ionic radii in water

45
Q

Reactivity with hydrogen

A

Lower the difference between the anionic radius and the cationic radius higher will be the stability
Elements tends to from stable compounds so that the reactivity increases.

46
Q

Metallic nature

A

Metallic character depends onthe ability of an element to lose its outer valence electrons.
Across a period from left to right metallic nature decreases while down the group it increases.

47
Q

Basic nature of hydroxides

A

Lower the bond strength higher will be the basic nature

48
Q

Thermal stability

A

Thermal stability increases down the group.
When going down the group the polarizing power of the cation decrease resulting in a less polarized anion.
Less the polarization of the anion more the thermal stability.

49
Q

Solubility depends on

A

Solubility depends on the radii difference between the anion and cation
Higher the difference higher the solubility

50
Q

Melting points of s and p block elements

A

Boiling points of metals increases from left to right as the metallic bond strength increases due to the decrease in cationic radius.
14th group elements like carbon and silicon will have the highest melting points due to the formation of covalent bond network structures.
From 15th to 16th group boiling point increases and from 17th to 18th group boiling point decreases

51
Q

Na2O(s)-Nature, oxidation no and bonding type

A

Strongly basic
+1
Ionic

52
Q

MgO(s)-Nature, oxidation no and bonding type

A

Basic
+2
Ionic

53
Q

Al2O3(s)-Nature, oxidation no and bonding type

A

Amphoteric
+3
Ionic

54
Q

SiO2(s)-Nature, oxidation no and bonding type

A

Very weakly acidic
+4
Covalent bond network

55
Q

P4O10(s)-Nature, oxidation no and bonding type

A

Weakly acidic
+5
Covalent

56
Q

SO3(g)-Nature, oxidation no and bonding type

A

Acidic
+6
Covalent

57
Q

Cl2O7(l)-Nature, oxidation no and bonding type

A

Strong acid
+7
Covalent

58
Q

SiO2(s) + 2NaOH(aq)

A

Na2SiO3(aq) + H2O

59
Q

P4O10(s) + 6H2O(l)

A

4H3PO4(aq)

60
Q

SO3(g) + H2O(l)

A

H2SO4(aq)

61
Q

Cl2O7 (l) + H2O(l)

A

2HClO4(aq)

62
Q

P4O10(s) + 12NaOH(aq)

A

4Na3PO4(aq) + 6H2O(l)

63
Q

SO3(g) + 2NaOH(aq)

A

Na2SO4(aq) + H2O(l)

64
Q

Cl2O7 (l) + 2NaOH

A

2NaClO4(aq) + H2O(l)

65
Q

H2S(g) + H2O(l)

A

HS ̶ (aq) + H3O+(aq)

66
Q

HCl(g) + H2O(l)

A

Cl ̶ (aq) + H3O+(aq)

67
Q

NaH(s)-Nature, oxidation no and bonding type

A

Strongly basic
+1
Ionic

68
Q

MgH2(s)-Nature, oxidation no and bonding type

A

Weakly basic
+2
Ionic

69
Q

AlH3(s)-Nature, oxidation no and bonding type

A

Amphoteric
+3
Network covalent

70
Q

SiH4(g)-Nature, oxidation no and bonding type

A

Very weakly acidic
-4
Covalent

71
Q

PH3(g)-Nature, oxidation no and bonding type

A

Neutral
-3
Covalent

72
Q

HCl(g)-Nature, oxidation no and bonding type

A

Very strongly acidic
-1
Covalent

73
Q

H2S(g)-Nature, oxidation no and bonding type

A

Weakly acidic
-2
Covalent

74
Q

SiCl4(l) + 2H2O(l)

A

SiO2(s) + 4HCl(aq)

75
Q

PCl5(g) + 4H2O(l)

A

H3PO4(aq) + 5HCl(aq)

76
Q

2SCl2(g) + 3H2O(l)

A

H2SO3(aq) + S(s) + 4HCl(aq)

77
Q

NaCl(s)-Nature, oxidation no and bonding type

A

Neutral
+1
Ionic

78
Q

MgCl2(s)-Nature, oxidation no and bonding type

A

Very weakly acidic
+2
Ionic

79
Q

AlCl3(s)-Nature, oxidation no and bonding type

A

Acidic
+3
Covalent

80
Q

SiCl4(l)-Nature, oxidation no and bonding type

A

Acidic
+4
Covalent

81
Q

PCl5(g)-Nature, oxidation no and bonding type

A

Acidic
+5
Covalent

82
Q

SCl2(g)-Nature, oxidation no and bonding type

A

Acidic
+2
Covalent

Chemistry (15 decks)

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