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WorksheetsENV112 (pt1)
Total questions: 25
Worksheet time: 13mins
Name
Class
Date
1.
The systematic name for Cr2(SO4)3 is
a)
chromium (II) sulphate
b)
chromium (II) sulphite
c)
chromium (III) sulphate
d)
chromium (III) sulphide
2.
For the equation: xKN03 → yK2O + yN2 + 5O2, to be balanced, the coefficients x and y must be:
a)
x=2, y=4
b)
x=4, y=2
c)
x=2, y=1
d)
x=4, y=3
3.
An element M has the electron configuration of 1s2 2s2 2p5. M is probably a
a)
a halogen
b)
a transition metal
c)
an alkali metal
d)
an alkaline-earth metal
4.
What is the relative molecular mass of an acid H3X if 0.025 mole of the acid weighs 2.45 g?
a)
49
b)
9.8
c)
98
d)
147
5.
What volume of 5.00 M HBr is needed to prepare 250 cm3 of 0.11 M solution?
a)
0.0055 dm3
b)
5.0 cm3
c)
10.0 cm3
d)
0.012 dm3
6.
What is the principal quantum number n for the energy level which can accommodate a maximum of 32 electrons?
a)
n=2
b)
n=3
c)
n=4
d)
n=5
7.
The oxidation number of S in the formula Na2S2O3 is
a)
-2
b)
3
c)
4
d)
2
8.
How many single covalent bonds are present in the molecule HCOOH?
a)
4
b)
3
c)
5
d)
2
9.
Which of the following molecules is polar?
a)
BCl3
b)
CCl4
c)
HCl
d)
CO2
10.
What is the relative molecular mass of [Cd(NH3)4Cl2]NO3?
a)
315
b)
277.5
c)
253
d)
313
11.
A solution of 100 cm3 of 0.05 M H2SO4 contains:
a)
0.005 mole of H+
b)
0.01 mole of H+
c)
0.2 g of H+
d)
0.02 mole of H+
12.
Which of the following changes represents an oxidation half-reaction?
a)
Cu2+ → Cu
b)
Cl- → Cl2
c)
Cr2O7^2- → Cr3+
d)
CH3COOH → CH3CH2OH
13.
The electron configuration of sulphur (atomic number = 16) is
a)
1s2 2s2 2p6 3s2 3p4
b)
1s2 2s2 2p6 3s2 3p2
c)
1s2 2s2 2p6 3s2
d)
1s2 2s2 2p6 3s2 3p5
14.
What is the percentage composition by mass of FeCl3?
a)
34.46% Fe, 65.54% Cl
b)
44.27% Fe, 55.73% Cl
c)
28.33% Fe, 71.67% Cl
d)
56.46% Fe, 43.54% Cl
15.
In the reaction: 2NaBr + F2 → 2NaF + Br2, the reducing agent is
a)
Br2
b)
F2
c)
NaF
d)
NaBr
16.
The conjugate base of the Bronsted acid HS- is:
a)
OH-
b)
H2S
c)
H+
d)
S2-
17.
Which of the following statements is not true for the Group VIA elements in the Periodic Table?
a)
They form both ionic and covalent compounds
b)
They form anions of the type A2-
c)
They have the general valence-shell electron configuration ns2 np6
d)
They are nonmetals
18.
Consider the reaction: 3O2 + 4X → 2X2O3. How many moles of O2 are needed to produce 1.0 g of X2O3, if the molar mass of X2O3 is w?
a)
3l/(2w)
b)
1/(2w)
c)
4/(3w)
d)
3w/2
19.
A buffer solution can be prepared by mixing ammonium chloride with an aqueous solution of
a)
ammonium nitrate
b)
sodium hydroxide
c)
ammonium hydroxide
d)
ethanoic acid
20.
The electron configuration of an element Y is [Ne] 3s2 3p2. It has a mass number of 28. Atom Y contains
a)
14 p, 14 n, 4 v.e
b)
14 p, 14 n, 2 v.e
c)
14 p, 18 n, 4 v.e
d)
28 p, 14 n, 14 v.e
21.
What are the formulas of the cation and anion present in Pb(H2PO4)2?
a)
Pb2+ and PO4^3-
b)
Pb2+, H+, and PO4^3-
c)
Pb2+ and (H2PO4)-
d)
Pb+ and (H2PO4)2-
22.
What is the empirical formula for the compound: C4H9COOC3H7?
a)
C8H18O2
b)
C4H8O
c)
C7H14O2
d)
(CH3)4O2
23.
Which of the following species is not the product of reduction of SO3?
a)
H2S
b)
S
c)
SO2
d)
SO4^2-
24.
Which of the following bromide compounds is distinctly ionic?
a)
CBr4
b)
RbBr
c)
HBr
d)
BBr3
25.
The Ka value for HCOOH is 2.09×10^-4. What is the pKa value?
a)
3.68
b)
3.2
c)
4.01
d)
10.32
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