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Chemistry Class 12 > Group 1 Elements > Flashcards

Group 1 Elements Flashcards

1
Q

All group 2 elements are known as alkaline earth metals- true/false

A

False - beryllium is not considered to be and alkaline earth metal

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2
Q

Abundant alkali metals are

A

Sodium and potassium - lithium, rubidium and caesium have lower abundance

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3
Q

Longest lived isotope of Francium

A

Fr 223 [half-life = 21 minutes]

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4
Q

Elements ranked 5th and 6th in abundance in Earth’s crust

A

Calcium and Magnesium respectively [Strontium and Barium have relatively low abundance]

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5
Q

Percentage of igneous rocks which is the element radium

A

10^(-10)%

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6
Q

General electronic configuration of s-block elements

A

[Noble gas] ns1 and [Noble gas] ns2

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7
Q

Igneous rock is formed from

A

Cooled and hardened magma

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8
Q

Diagonal relationship is due to

A

Similarity in ionic sizes and charge/radius ratio of elements

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9
Q

The most electropositive elements are

A

Alkali metals

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10
Q

Ionization enthalpies of alkali metals are

A

Considerably low and decrease down the group

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11
Q

Hydration enthalpy order of group 1 element ions

A

Li+ > Na+ > K+ > Rb+ > Cs+

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12
Q

Lithium salts are never hydrated - true/false

A

False - most lithium salts are hydrated eg. LiCl.2H20

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13
Q

Ionization enthalpy order of group 1 elements

A

Li > Na > K > Rb > Cs> Fr

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14
Q

Metallic radius order of group 1 elements

A

Cs > Rb > K > Na > Li

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15
Q

Ionic radius of group 1 elements

A

Cs > Rb > K > Na > Li

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16
Q

Melting point order of group 1 elements

A

Li > Na > K > Rb > Cs

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17
Q

Boiling point order of group 1 elements

A

Li > Na > K > Rb > Cs

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18
Q

Density order of group 1 elements

A

Cs > Rb > Na > K > Li

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19
Q

Negative SRP value order for group 1 elements

A

Li > Rb > Cs > K > Na

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20
Q

Lithium flame colour

A

Crimson red [670 nm]

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21
Q

Sodium flame colour

A

Yellow [590 nm]

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22
Q

Potassium flame colour

A

Violet [766 nm]

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23
Q

Rubidium flame colour

A

Red violet [780 nm]

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24
Q

Caesium flame colour

A

Blue [455 nm]

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25
Q

Metals used in photoelectric cells

A

Caesium and Potassium

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26
Q

Lithium forms

A

Monoxides [O(2-)]

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27
Q

Sodium forms

A

Peroxides [O2(2-)]

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28
Q

K, Rb, Cs form

A

Super oxides [O2(-)]

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29
Q

Superoxide ion is only stable in the presence of

A

Large cations like K, Rb, Cs

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30
Q

4Li +O2 ———->

A

2 Li2O [oxide]

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31
Q

2Na + O2 ————>

A

Na2O2 [peroxide]

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32
Q

M + O2 [M = K, Rb, Cs] ———————>

A

MO2 [superoxide]

33
Q

Lithium directly reacts with nitrogen to form

A

Lithium nitride Li3N

34
Q

Alkali metals are normally stored in

A

Kerosene oil [Except K]

35
Q

2M + 2H2O [M = alkali metal] —————–>

A

2M+ + 2OH- +H2

36
Q

Reaction of lithium with water when compared to sodium

A

Is less vigorous although Li has most negative SRP value because of small size and very high hydration enthalpy

37
Q

Alkali metals react with hydrogen at temperatures of

A

623 K [Li at 1073 K]

38
Q

All alkali metal hydrides are

A

Ionic solids with high melting points

39
Q

2M + H2 [M = alkali metal] ———————->

A

2MH [M+H-]

40
Q

Nature of halides of alkali metals

A

Ionic in nature except lithium halide which has some covalent character [LiI is most covalent]

41
Q

SEP represents the overall change which includes

A

Sublimation enthalpy + Ionization enthalpy + Hydration enthalpy

42
Q

More negative is the SRP

A

Stronger is the reducing agent [substance itself gets oxidized]

43
Q

Alkali metals dissolve in liquid ammonia to give

A

Deep blue conducting solutions

44
Q

M+ + (x+y)NH3(l) —————>

A

[M(NH3)x]+ + [e(NH3)y]-

45
Q

Colour of solution of alkali metal in ammonia is due to

A

Ammoniated electrons [Solutions are paramagnetic]

46
Q

Solutions of alkali metals and ammonia, on standing, give off

A

Hydrogen, resulting in the formation of amide

47
Q

M+ + e- + NH3 —————————>

A

MNH2 + 1/2H2

48
Q

In concentrated solution of alkali metal in ammonia

A

Blue colour changes to bronze colour and solution becomes diamagnetic

49
Q

Lithium + lead

A

White metal

50
Q

Armour plates are made using

51
Q

Colour of oxides, peroxides and superoxides of alkali metals

A 
Oxides = colourless (pure)
Peroxides = colourless
Superoxides = yellow/orange and paramagnetic
52
Q

Order of enthalpy of formation of alkali metal fluorides (negative)

A

LiF > NaF > KF > RbF > CsF

53
Q

Order of enthalpy of formation of alkali metal chlorides, bromides and iodides (negative)

A

CsX > RbX > KX > NaX > LiX

54
Q

Order of enthalpy of formation of alkali metal halide (negative)

A

MF > MCl > MBr > MI

55
Q

Order of melting and boiling points of alkali metal fluorides

A

MF > MCl > MBr > MI

56
Q

LiF has (solubility)

A

Low solubility due to high lattice enthalpy

57
Q

CsF has (solubility)

A

Low solubility due to low hydration enthalpy of constituent ions

58
Q

Halides of lithium are also soluble in

A

Ethanol, acetone, ethylacetate [LiCl is soluble in pyridine]

59
Q

Stability of alkali metal carbonates and bicarbonates

A

Increases down the group with electropositive character

60
Q

LiHCO3 exists as a solid - true/false

61
Q

Hardest alkali metal

62
Q

Lithium + ethyne

A

Ethynide is not formed unlike other alkali metals

63
Q

Lithium nitrate when heated gives

A

Li2O, unlike MNO2, which all other alkali metals give

64
Q

Washing soda

A

Na2CO3.10H20

65
Q

Washing soda is prepared by

A

Solvay process

66
Q

Solvay process

A

2NH3 + H2O + CO2 ————>(NH4)2CO3
(NH4)2CO3 + H2O + CO2 ————->2NH4HCO3
NH4HCO3 + NaCl —————>NH4Cl + NaHCO3
2NaHCO3 ——————–>Na2CO3 + CO2 + H2O

2NH4Cl + Ca(OH)2 —————->2NH3 + CaCl2 + H20

67
Q

Potassium Carbonate cannot be manufactured by solvay process because

A

KHCO3 is too soluble to be precipitated out by addition of NH4HCO3

68
Q

Na2CO3.10H2O at 375 K ——————>

A

Na2CO3.H2O

69
Q

Na2CO3.H2O above 373K —————–>

A

Na2CO3 + H2O (soda ash - white powder)

70
Q

Sea water contains salt % of

A

2.7 - 2.9% by mass

71
Q

Weight of salt produced annually in India by solar evaporation

A

50 lakh tonnes

72
Q

NaOH is produced commercially by

A

Electrolysis of NaCl in Castner-Kellner cell

73
Q

Brine solution is electrolysed in Castner-Kellner cell using

A

Mercury cathode and carbon anode

74
Q

Na-amalgam + H2O —————->

A

NaOH + Hg + 1/2H2

75
Q

NaHCO3 is used as

A

Mild antiseptic and in fire extinguishers

76
Q

Weight of metals present in 70 Kg man

A

90g of Na, 170g of K, 5g of Fe, 0.06g of Cu

77
Q

Most abundant cations within cell fluid

78
Q

More than 1/3rd ATP in a resting animal is consumed by

A

Sodium-potassium pump

79
Q

Sodium potassium pump in human consumes

A

15 Kg per 24 hrs in resting human

Chemistry Class 12 (2 decks)

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