1.
Write electronic configuration of an element having
atomic number 13.
2.
State an example of an endothermic reaction.
3.
Why do we store silver chloride in dark
coloured bottles? Explain in brief.
4.
“A
solution of potassium chloride when mixed
with silver nitrate solution, an insoluble white substance is formed”.
a.
Translate
the above statement into a chemical
equation.
b.
State
two types for this reaction.
5.
Write the chemical
name and formula of common salt. State how
sodium hydroxide is prepared using
this salt.
6.
Draw
a labelled schematic diagram to show the electrolysis of water. Why is the amount of gas collected in one of the test tubes in this activity double of the amount collected in the other
?
7.
Five
solutions A, B, C, D and E when tested
with universal indicator showed pH as 4, 1, 11, 7 and 9 respectively. Which
solution is (a) neutral (b)
strongly alkaline (c) strongly acidic
(d) weakly acidic and (e) weakly alkaline. Arrange the pH in
increasing order of H—ion concentration.
8.
What
happens when chlorine is passed over
dry slaked time? Write chemical
equation of the reaction involved.
Mention three properties of the
product.
9.
How is charcoal different from coal
How is it prepared? State two
criteria for considering charcoal
a letter fuel than wood for domestic purposes.
10.
State the
reason why
(i) carbon
is not used to reduce the
oxides of sodium or aluminium.
(ii) an iron strip dipped in a blue copper sulphate solution
turns the blue solution pale green.
(iii) metals
replace hydrogen from acids
whereas non-metals do not.
(iv) calcium
does not occur
free in nature.
(v) zinc is used in the galvanisation of iron and
not the copper.
OR
(a)
list
two differences between calcinator
and roasting.
(b) An element ‘X burns in oxygen to form
an electrovalent compond XO.
State the compounds you
expect will form
if the element X is made to combine with (i) chlorine and (ii) sulphur. Mention the Chemical formula and nature of bond present in each case.
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