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INDIAN SCHOOL MUSCAT
THE p-BLOCK ELEMENTS
1.
2.
3.
4.
5.
6.
Complete the following and balance
j. Pb (NO3)2 --673K
+
a. IO3 + I + H 
k. XeF4 + H2O 
b. KBrO3 + KBr + H2SO4 
l. XeF4 + SbF5 
c. Pu + O2F2 
m. XeF6 + KF 
d. CaF2 + H2SO4 
n. I2 + N2H4 
e. CaBr2 + H2SO4 
o. P4 + KOH + H2O 
f. Cl2 + Ba(OH)2 
p. Ca3P2 + H2O 
g. U + ClF3 
q. Pb3O4 + HNO3 
h. XeO3 + OH 
r. SiO2 + HF 
i. Acid K2Cr2O7 + Fe2+ 
s. SO2 + NaC lO3(acid) 
Give the oxidation number of the element highlighted.
a) Ca3P2; Na3PO4; POF3; H3PO3; PCl3
Give equations for the manufacture of
a) aluminium from bauxite b) tin from cassiterite c) phosphorous from rock phosphate
d) sulphur from natural gas e) lead from galena f) sulphuric acid from sulphur
g) fluorine from antimony pentafluoride h) iodinefrom sodium iodate i)bleaching powder
j) bromine from sea water
Draw the structures of XeF2, XeF4, XeF6, XeO3, XeOF4, Cl2O, Cl2O7, IF7, SF4, PCl5(s),
orthophosphoric acid, metaphosphoric acid, pyrophosphoric acid, phosphorous acid,
peroxydisulphuric acid, iodine pentafluoride, peroxomonosulphuric acid, P4O6; P4O10; ClO4SO32Explain why
i. Bond energy of F2 is lower than that of Cl2.
ii. C and Si are mainly tetravalent while Ge, Sn and Pb show bivalency.
iii. Carbon exhibits catenation while Silicon does not.
iv. CO2 is a gas at room temperature while SiO2 is a high melting solid.
v. Elemental Silicon does not form graphite like structure.
vi. Electron affinity of fluorine is less than that of chlorine.
vii. Fluorine is the most reactive among halogens.
viii. H2S is gas while water is liquid at room temperature.
ix. H3PO3 is diprotic.
x. HF has a higher boiling point than HCl.
xi. HI is a stronger acid than HCl.
xii. Inter-halogen compounds are more reactive than the related molecular halogens.
xiii. Maximum covalence of nitrogen is four.
xiv. Nitrogen is a diatomic molecule while Phosphorous is tetra atomic.
xv. Noble gases exhibit low chemical reactivity.
xvi. Noble gases form compounds with oxygen and fluorine only.
xvii. PbX2 is more stable when compared to PbX4.
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xviii. SF6 is known while SH6 is not.
xix. SiCl4 is easily hydrolysed while CCl4 cannot be hydrolysed.
xx. The +2 oxidation state of Pb is more stable than the +2 oxidation state of Sn.
xxi. Sulphur at elevated temperatures exhibit paramagnetism.
xxii. Unlike phosphorous, nitrogen has no tendency for catenation.
xxiii. Pentavalent bismuth is a strong oxidising agent.
xxiv. Bonds in PF5 are not equivalent.
xxv. Atomic size of Ga is smaller than that of Al
xxvi. AlCl3 dimerises
xxvii. Al does not react with nitric acid.
xxviii. SiCl62- does not exist.
xxix. Most stable oxidation state of Tl is +1
xxx. Electro negativity of lead is more than that of tin.
7. Name a compound in which chlorine displays ‘+7’ oxidation number.
8. How can you prepare the following and give one use of each.
a) pure silicon b) LiAlH4 c) SnO2 d) S2Cl2 e) SF6 f) Cl2 g) NH4ClO4 h) silicone
9. Which compound led to the discovery of noble gas compounds?
10. Which of the xenon fluorides molecule is isoelectronic with IF5? Draw its structure.
11. Arrange the following according to the property mentioned. Give reason.
a. F2, Cl2, Br2, I2 (decreasing BDE)
b. H2S, H2O, H2Se, H2Te (decreasing thermal stability)
c. HF, HCl, HBr, HI (increasing acidity)
d. HF, HCl, HBr, HCl (increasing stability)
e. NH3, PH3, AsH3, SbH3 (decreasing basic nature)
f. HOCl, HOClO, HOClO2, HOClO3 ( decreasing acidity)
g. H2S, H2O, H2Se, H2Te ( increasing boiling point)
h. NH3, PH3, AsH3, SbH3 (increasing boiling point)
i. HOCl, HOBr, HOI ( increasing acid character)
12. How are XeO3 and XeOF4 prepared?
13. Name the molecular geometry of XeOF6, XeO3, and SF4.
14. What are interhalogen compounds? How are they prepared? Why are they more reactive
than molecular halogens?
15. Give a method of preparation of XeF6. Discuss its hydrolysis.
16. Compare bond angles in a) NH3 and PH3 b] H2S and H2O
17. Why should binary compounds of oxygen & fluorine be called oxygen fluorides & not
fluorine oxides?
18. Calculate the volume of 0.1M NaOH solution required to neutralise a solution prepared by
dissolving 1.1g of P4O10 in water.
19. Calculate the mass of HI formed by the reaction of 62g of red P with iodine in presence of
water.
20. Explain disproportionation reaction by giving an example.
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