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S BLOCK Flashcards

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1
Q

1st Grp. elements(Alkali Metals)

A

lithium , sodium , potassium, rubidium, caesium and francium

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2
Q

2nd Grp. elements(Alkaline earth metals)

A

beryllium, magnesium, calcium, strontium, barium, radium

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3
Q

Half life time of francium

A

21 minutes(longest lived isotope) and radioactive

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4
Q

where are alkaline earth metals found

A

earth crust as meta oxides

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5
Q

where do calcium and magnesium rank in abundance

A
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6
Q

where is radium found

A

igneous rocks

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7
Q

E.C of alkali metals

A

[noble gas] ns1

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8
Q

E.C of alkaline earth metals

A

[noble gas] ns2

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9
Q

which 2 pairs are in diagonal relationship

A

lithium and magnesium ; beryllium and aluminium

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10
Q

diagonal relationship arises due to

A

similar ionic sizes or charge/mass ratio

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11
Q

elements present in bio fluids to maintain ion balance and treat nerve disorders

A

sodium, potassium, calcium and magnesium

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12
Q

ion formed by first grp. elements

A

M+ (most electropositive)

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13
Q

which grp. elements are most electropositive

A

1st

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14
Q

which grp. elements have largest sizes

A

1st

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15
Q

general value of I.E for 1st grp. elements

A

low

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16
Q

trend of atomic radius in grp.1

A

increases top t bottom

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17
Q

trend of I.E in grp.1

A

decreases down the grp.(incr. size outweighs the nuclear charge)

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18
Q

trend of hydration enthalpies in grp. 1

A

decreases top to bottom

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19
Q

physical appearance of grp.1 elements

A

silvery white , soft and light

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20
Q

general value of density in grp.1

A

low

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21
Q

trend of density with exception

A

increases down the group but potassium lighter than sodium

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22
Q

general value of M.P and B.P of grp.1

A

low due to weak metallic bonding

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23
Q

Photoelectric color of li

A

crimson red

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24
Q

Photoelectric color of na

A

yellow

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25
Q

Photoelectric color of k

A

violet

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26
Q

Photoelectric color of rb

A

red violet

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27
Q

Photoelectric color of cs

A

blue

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28
Q

how can alkali metals be detected

A

flame tests

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29
Q

elements used as electrodes in grp.1

A

caesium and potassium

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30
Q

reactivity of alkali metals

A

high due to large size and low I.e

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31
Q

alkali metals + air

A

burn vigorously in oxygen to tarnish by producing oxides

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32
Q

monoxide is formed by which alkali metal

A

lithium

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33
Q

peroxide is formed by which alkali metal

A

sodium

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34
Q

oxides formed by k,rb,cs

A

superoxide

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35
Q

O.S of alakli metals

A

+1

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36
Q

li+n

A

li3n is formed by li exceptional reactivity

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37
Q

where are alkali metals stored due to high reactivity towards water

A

kerosene

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38
Q

alkali metals+ water

A

hydroxide with h2

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39
Q

which alkali metal has the most e- value

A

lithium

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40
Q

which alkali metal has the least e- value

A

sodium

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41
Q

which alkali metal is an exception to their explosive reaction to water

A

lithium due to very low size

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42
Q

alkali metals+h2 9673k)

A

hydrides (M+H-)

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43
Q

alkali metals with halogens

A

ionic halides (M+X-)

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44
Q

which is the only alkali metal that forms a covalent halide

A

lithium

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45
Q

which lithium halide is most covalent

A

lithium iodide

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46
Q

nature if alkali metals in redox rxns.

A

reducing agents

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47
Q

most powerful r.a alkali metal

A

lithium due to high hydration enthaly

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48
Q

least powerful r.a alkali metal

A

sodium

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49
Q

relation between standard reduction potential and r.a

A

inversely proportional

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50
Q

alkali metals + liq. nh3 solns.

A

alkali metals dissolve and turn it into blue color due to ammoniated e-

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51
Q

magnetic nature of alkali metal + ammonia soln.

A

paramagnetic

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52
Q

ammoniated e-+M+

A

amide + h2

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53
Q

in conc. ammonia soln. blue color and paramagnetic changes to

A

bronze color and diamagnetic

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54
Q

use of li

A

with mg to make armor plates
with al to make aircraft parts
with pb to make bearings for motor engines
thermonuclear rxns.
electrochemical cells

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55
Q

use of na

A

with na to make anti knock additives to petrol
liq. coolant in nuclear rxns.

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56
Q

use of potassium

A

bio fluid
fertilizer
soft soap(KOH)
absorbent of CO

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57
Q

use of cs

A

devising photoelectric cells

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58
Q

li+air

A

li2o mostly and some li2o2

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59
Q

na+air

A

na2o2 mostly and some nao2

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60
Q

trend if stability of oxides

A

increases with incr. in metal ion sizes

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61
Q

alkali metal oxides+water

A

hydroxides

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62
Q

color of oxides and peroxides

A

colorless

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63
Q

color of super oxides

A

yellow and orange

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64
Q

magnetic nature of superoxides

A

paramagnetic

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65
Q

widely used alkali metal oxide as o.a

A

sodium peroxide

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66
Q

alkali metal hydroxides appearance

A

white crystalline solids

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67
Q

most strong bases

A

alkali metal hydroxides

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68
Q

physical nature alkali metal halides

A

high MP and colorless crystalline solids

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69
Q

HX+ appropriate oxide/hydroxide/carbonate

A

alkali metal halides

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70
Q

trend of formation enthalpy of alkali metal halides

A

high negative down the grp. except fluorine

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71
Q

trend of formation of alkali metal halides

A

less negative from MF to MI

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72
Q

trend of MP of halides

A

decreases don the grp.

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73
Q

solubility of alkali metal halides in water

A

high except LiF(very low) and CsI(very high)

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74
Q

licl is soluble in which organic compound

A

pyridine

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75
Q

carbonates of metal oxo acids

A

metal bicarbonates most likely and metal carbonates too

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76
Q

nature of alklai metal oxo acids

A

thermally stable soluble i water

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77
Q

alkali metals + oxo acids

A

salts

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78
Q

trend of stability of alakli metal carbonates

A

increases down the grp.

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79
Q

which alkali metal carbonate is unstable to heating

A

li

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80
Q

reasons for anamolous behaviour of li

A

very small size
high polarizing power which gives rise to high covalent characters

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81
Q

anamolous properties of li

A

hardest
high MP and BP
;east reactive but strongest r.a
mainly forms li2o and li3n with air
deliquescent
crystallizes as hydrates
lithium HCs aren’t available as solids
doesn’t form ethynide with ethyne
lithium nitrate(li3n) heated to give li2o but generally nitrites are formed
lif and li2o are comparitively less water soluble

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82
Q

reason for diagonal relationship with mg

A

similar sizes

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83
Q

diagonal similarities between li and mg

A

harder and lighter
slow rxn. with water
less stable and soluble oxides and hydroxides
nitrates
nitrates heated to give oxides instead of nitrogen
oxides don’t give superoxides
carbonates are decomposed easily on heating to from oxides and co2
halides are soluble in ethane
halides are deliquescent and crystallize to form aq. solns. as hydrates

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84
Q

industrial name of sodium carbonate(na2co3.10h20)

A

washing soda

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85
Q

washing soda is prepared by what process

A

solvay orocess

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86
Q

advantage of sodium hydrogen carbonate that promotes it to undergo solvay process

A

less solubility

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86
Q

by product of solvay process

A

calcium chloride

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87
Q

reactants of solvay process

A

ammonium carbonate, nacl, co2

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88
Q

appearance of washing soda

A

white crystalline solid

89
Q

solubility in water

A

readily soluble

90
Q

type of hydrate formed on heating washing soda

A

monohydrate

91
Q

monohydrate of washing soda above 373 K

A

white powder called soda ash

92
Q

carbonate prt of washing soda + h2o

A

alkaline soln.

93
Q

uses of washing soda

A

softening, laundering, cleaning
manufacture of glass, borax, soap, caustic soda
paper, paint and textile industry
lab reagent in qualitative and quantitative analysis

94
Q

most abundant source of nacl

A

sea water

95
Q

how is salt produced in india

A

evaporating sea water

96
Q

salt produced in india every year

A

50 lakh tons

97
Q

impurities in brine

A

caso4, na2so4, cacl2, mgcl2

98
Q

reactants in prep. of nacl

A

crude nacl, water, hcl (gas)

99
Q

use of nacl

A

table or common salt
prep of na2o, naoh, na2co3

100
Q

industrial name of naoh

A

caustic soda

101
Q

process of prep. of caustic soda

A

elctrolysis

102
Q

reactants used in the prep of naoh

A

brine soln., mercury cathode, carbon anode

103
Q

what is produced at cathode in naoh prep.

A

sodium amalgam(nahg)

104
Q

what is obtained at anode in naoh prep.

A

cl2 gas

105
Q

from which initial product do we get naoh

A

sodium amalgam

106
Q

appearance of naoh

A

white, translucent solid, deliquescent

107
Q

MP of naoh

A

591K

108
Q

MP of nacl

A

1081K

109
Q

nature of naoh

A

strongly alkaline

110
Q

naoh+co2

A

na2co3

111
Q

uses of naoh

A

manufacture of soap paper, artifical silk
petroleum refining
purification of bauxite
mercerising cotton
prep. of pure fats and oil
lab reagent

112
Q

industrial name of sodium hydrogen carbonate(nahco3)

A

baking soda

113
Q

use of sodium bicarbonate

A

mild antiseptic for skin infections
fire extinguishers

114
Q

reactants used in prep. of baking soda

A

na2co3, h2o, co2

115
Q

most abundant metal in our body

A

potassium

116
Q

where are na cells found inside our body

A

outside the cells in interstitial fluids like blood plasma

117
Q

use of na in our body

A

messengers
transport sugar and amino acids
controls flow of water across cell membrane

118
Q

use of potaasium in our body

A

enzyme activator
oxidizes glucose
mesenger

119
Q

pump that operates across cell membranes

A

na-k pump

120
Q

energy consumed by na-k pump

A

1/3rd ATP in resting animal
15Kg in a day in resting human

121
Q

relation between size of grp. 2 and grp.1 elements

A

grp.2 < grp.1 due to incr. in nuclear charge

122
Q

trend of atomic radius in grp.2

A

incr. down the grp.

123
Q

general value of IE in grp.2 elements

A

low

124
Q

trend of IE in grp.2

A

decreases down the gr.

125
Q

relation between IE1 of grp. 2 and grp.1 elements

A

grp.1 < grp. 2

126
Q

relation between IE2 of grp. 2 and grp.1 elements

A

grp.1 > grp. 2

127
Q

trend of hydration enthalpies in grp. 2

A

decreases down the grp.

128
Q

relation between hydration enthalpies of grp. 2 and grp.1 elements

A

grp. 2 > grp.1

129
Q

appearance of alkaline earth metals

A

slivery white, lustrous and relatively soft but harder than alkali metals

130
Q

relation between MP and BP of grp. 2 and grp.1 elements

A

grp. 2 > grp. 1

131
Q

trend of electropositive character in grp.2 elements

A

incr. down the grp.

132
Q

calcium color to flame

A

brick red

133
Q

strontium color to flame

A

crimson

134
Q

barium color to flame

A

apple green

135
Q

alkaline earth metals that don’t release color on de excitation

A

be and mg

136
Q

flame test for which alkaline earth metals is helpful in qualitative and quantitative estimation

A

ca, sr, ba

137
Q

alkaline earth metals conductivity vaue generally

A

high

138
Q

reactivity of alkaline earth metals

A

less than alkali metals

139
Q

alkaline earth metals which are chemically inert to water due to formation of oxide film

A

be and mg

140
Q

be and mg when burnt in air

A

mo and m3n2

141
Q

ca, ba, strontium + air

A

oxide, nitride and also hydroxides

142
Q

alkaline earth metals + x2

A

MX2

143
Q

convenient way to make bef2

A

thermal decomposition of (nh4)2bef4

144
Q

becl2 is prep. from

A

beo

145
Q

alkaline earth metals + h2

A

metal hydrides

146
Q

condition for formation of beh2

A

becl2+lialh4

147
Q

alkaline earth metals + acids

A

h2 is liberated

148
Q

nature of grp. 2 elements in redox rxns.

A

r.a

149
Q

grp. 2 element with least r.a tendency

A

beryllium

150
Q

relation between reducing power of grp.1 and grp. 2

A

grp.1 > grp.2

151
Q

alkaline earth metals + liq. nh3 solns.

A

deep blue black solns. with ammoniated ions

152
Q

uses of be

A

cu-be alloys in high strength springs
windows of x ray tubes

153
Q

uses of mg

A

mg-al alloy in aircraft making
flash powders, bulbs, incedinary bombs
milk of magnesia as antacids
mgco3 as toothpastes

154
Q

uses of ca

A

extradition of metals from oxides

155
Q

which 2 alkaline earth metals are combined used for removing air from vaccum

A

ca and ba

156
Q

use of radium

A

radiotherapy like to treat cancer

157
Q

O>S of grp.2 elements

A

2

158
Q

nature of grp.2 elements compounds

A

ionic but less than alkali metals

159
Q

nature of beo and mgo

A

covalent

160
Q

structure of alkaline earth metals oxide and hydroxide

A

rock salt except beo

161
Q

nature of alkaline earth metal oxides

A

ionic and basic except beo (covalent and amphoteric)

162
Q

trend of solubility , stability and basic character of A.E.Ms

A

incr. down the grp. but less than alkali metals

163
Q

nature of A.E.M halides

A

ionic except beo(covalent)

164
Q

structure of beo

A

chain which forms chloro-bridged dimer that dissociates into linear one at high temperatures

165
Q

Trend of Halide formation in grp.2

A

decreases down the grp.

166
Q

way to dehydrate grp.2 elements

A

heat them(except be and mg - hydrolysis on heating)

167
Q

stability between grp.2 fluorides and chlorides

A

f < cl

168
Q

Water solubility of grp. 2 carbonates

A

insoluble

169
Q

Trend of Water solubility of grp. 2 carbonates

A

decreases down the grp.

170
Q

where only can beo be kept

A

atmosphere of co2

171
Q

Trend of Thermal stability in grp.2

A

incr. down the grp.

172
Q

Trend of Water solubility of grp. 2 sulphates

A

decr. down the grp.

173
Q

Appearance of grp. 2 sulphates

A

white solids

174
Q

Water of crystallization of mg3n2 and be3n2

A

6 and 0

175
Q

grp. 2 nitrates on decomposition give

A

oxides

176
Q

anamolous properties of be

A

largely covalent
easily hydrolysed
maximum CN=4
oxide and hydroxide are amphoteric

177
Q

reason for anamolous properties of be

A

very small size

178
Q

reason for diagonal relationship between be and al

A

same size and similar charge to mass ratio

179
Q

diagonal similarities between be and al

A

not readily attacked by acids
dissolve in water to give beryllate and aluminate ion
chlorides are ridged in vapor phase and strong L.A
string tendency to form complexes

180
Q

calcium oxide is also called as

A

quick lime(CaO)

181
Q

prep. of cao

A

limestone heating

182
Q

appearance of cao

A

white amorphous solid

183
Q

MP of cao

A

2870K

184
Q

addition of limited amount of water to break lump of cao is called

A

slaking of lime

185
Q

quick lime slaked with soda lime gies

A

solid sodalime

186
Q

uses of cao

A

manufacturing cement, na2co3 from naoh and dye stuffs
purification of sugar

187
Q

cheapest from of alkali

A

cao

188
Q

ca(oh)2 is also known as

A

slaked lime(CaCO3)

189
Q

prep. of slaked lime

A

cao=water

190
Q

appearance of slaked lime

A

white amorphous powder

191
Q

Water solubility of slaked lime

A

very less

192
Q

aq. slaked lime is called

A

lime water

193
Q

slaked lime in water is called

A

milk of lime

194
Q

co2 + saked lime

A

milky due to caco3 formation

195
Q

caco3+h2o

A

calcium bicarbonate

196
Q

milk of lime + cl2

A

hypochlorite (a bleaching powder constituent)

197
Q

uses of ca(oh)2

A

prep. of mortar
white wash
disinfectant
tanning industry
prep. of bleaching powder and glass
purification of water

198
Q

caco3 exists in nature as

A

limestone, marble

199
Q

prep. of caco3

A

slaked lime + co2
(or)
na2co3 + cacl2

200
Q

appearance of caco3

A

white fluffy powder

201
Q

Solubility of caco3 in water

A

insoluble

202
Q

caco3 decomposes on heating to from

A

cao + cp2

203
Q

caco3 + dilute acid

A

liberates co2

204
Q

uses of caco3

A

manufacture of cao
building material
marble
along with mgco3 used in metal extraction
manufacture of high quality
paper
antacid
toothpaste
contituent of chewing gum
filler in cosmetics

205
Q

calcium sulphate is also called

A

plaster of paris (pop) (caso4.1/2 h2o)

206
Q

pop is decrystallized at and to

A

above 393 K to caso4 (dead burnt plaster)

207
Q

time taken to form plastic plate with pop in water

A

5 - 15 minutes

208
Q

uses of pop

A

building industry
setting up fractures and sprains
dentistry
ornamental works
getting casts and moulds

209
Q

cement was introduced by

A

Joseph Aspidin(1824)

210
Q

what was the other name of first introduced salt

A

Portland cement

211
Q

composition of cement

A

cao - 50 to 60 %
sio2 - 20 to 25%
al2o3 - 5 to 10%
mgo - 2 to 3%
so3- 1 to 2%

212
Q

ratio of silica and alumina for good cement

A

2.5:4

213
Q

ratio of lime to silicon, aluminium, iron oxides

A

2

214
Q

raw material for cement

A

limestone and clay

215
Q

prep. of cement

A

limestone and clay - cement clinker + 2 to 3% gypsum(caso4.2 h2o)

216
Q

important ingredients of portland cement

A

dicalcium silicate and tricalcium silicate and aluminate

217
Q

hydration of molecules of constituents and their rearrangement to give hard mass of cement

A

setting of cement

218
Q

what is added to slow down the process of setting of cement

A

gypsum

219
Q

uses of cement

A

concrete manufacture and reinforcement
plastering
construction of bridges, dams

220
Q

amount of grp.2 elements in our body

A

mg - 25g
Ca - 1200g

221
Q

uses of mg and ca in our body

A

mg acts as cofactor to enzymes that utilize atp
chlorophyll has mg
99% body ca is in bones and teeth
ca is neuromuscular messenger
ca concentration in blood plasma is around 100 mg/L maintained by 2 hormones calcitonin and parathyroid

inorganic chemistry (1 decks)

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