NEW
Font size
S
M
L
XL
WorksheetsENV112 (pt2)
Total questions: 25
Worksheet time: 13mins
Name
Class
Date
1.
Which of the following elements has partially filled 3d subshell?
a)
Ti
b)
Sr
c)
Si
d)
Zn
2.
In which of the following reactions does water, H2O behave as a Bronsted base?
a)
4H2O + Cu2+ → [Cu(H2O)4]2+
b)
H2O + CH3NH2 → CH3NH3+ + OH-
c)
H2O + NH3 → NH4+ + OH-
d)
H2O + CH3COOH → H3O+ + CH3COO-
3.
What is the pH of a solution of butanoic acid, C3H7COOH with [H+] = 3.98×10^-4 M?
a)
9.59
b)
3.41
c)
2.41
d)
5.21
4.
Which of the following is not a characteristic property of transition elements?
a)
They form coloured compounds
b)
They show variable oxidation states
c)
They form cations with partially filled d subshell
d)
They dissolve in water to give neutral solutions
5.
The electron configuration of an element is [Ar] ns2 np1. What is the value of n?
a)
2
b)
3
c)
4
d)
5
6.
In a reaction, the limiting reactant is the one that:
a)
has the smaller initial mass
b)
gives the lower yield of product
c)
is left over at the end
d)
has the largest number of atoms in its formula
7.
In the redox reaction: 10Cl- + 2IO3- + 12H+ → 5Cl2 + I2 + 6H2O, the species that gains electrons is
a)
I2
b)
H+
c)
IO3-
d)
Cr
8.
The atom of Bi has a nuclear charge of 83
a)
83+
b)
83-
c)
130-
d)
130+
9.
Comparing pH values of 0.1 M solutions of NaCl, NaOH, and Na2CO3, which is correct?
a)
Na2CO3 = NaCl < NaOH
b)
Na2CO3 < NaCl < NaOH
c)
NaCl < Na2CO3 < NaOH
d)
All have same pH
10.
What type(s) of bond/intermolecular forces can be found in CH3OH?
a)
Covalent and ionic
b)
van der Waals & covalent
c)
Covalent & hydrogen
d)
Covalent only
11.
Which of the following is not a general property of alkaline-earth metals?
a)
They have even numbers of electrons
b)
They are electronegative elements
c)
They are good conductors
d)
They have 2 valence electrons
12.
What is the molecular shape of ZCl3, VSEPR formula AX3E?
a)
Linear
b)
Tetrahedral
c)
Trigonal pyramidal
d)
Trigonal planar
13.
Which compound gives a weakly basic solution in water?
a)
Sodium propionate, C2H5COONa
b)
Nitric acid, HNO3
c)
Sodium bromide, NaBr
d)
Strontium hydroxide, Sr(OH)2
14.
What volume of 1.5 M Pb(NO3)2 contains 0.40 mole of Pb2+?
a)
0.27 dm3
b)
0.27 cm3
c)
0.60 dm3
d)
3.75 cm3
15.
For Ne, HCl, H2O, choose the correct increasing strength of intermolecular forces
a)
H2O<Ne<HCl
b)
Ne<H2O<HCl
c)
Ne<HCl<H2O
d)
HCl<Ne<H2O
16.
The electron configuration of element Z is [Ne]2s2. What are n and l for the valence electrons?
a)
n=2, l=1
b)
n=1, l=0
c)
n=3, l=0
d)
n=2, l=0
17.
What is the molarity of solution prepared by dissolving 21.65 g NH4NO3 in 335.0 cm3 water?
a)
0.09 M
b)
0.81 M
c)
0.01 M
d)
0.18 M
18.
X is a main group element forming XCl3 which dissolves in water as an electrolyte. Which is FALSE?
a)
X is metallic
b)
X can form diatomic molecules X2
c)
X is group IIIA element
d)
XCl3 is ionic
19.
0.01 M CH3COOH titrated with 0.1 M Ba(OH)2. Probable pH at endpoint?
a)
7
b)
5
c)
1
d)
9
20.
0.001 M weak acid HX has [H+] = 3.54×10^-5. Ka = ?
a)
2.82×10^-7
b)
3.54×10^-2
c)
1.25×10^-6
d)
1.25×10^-2
21.
Which is FALSE about H2S?
a)
Molecules can form H-bond
b)
It is a weak acid
c)
S atom oxidation number -2
d)
Boiling point higher than water
22.
Which is TRUE at the endpoint of an acid-base titration?
a)
Sharp pH change
b)
pH=7
c)
Equal moles of acid/base reacted
d)
Solution becomes colourless
23.
Electron configurations of X and Y are 1s2 2s2 2p5 and 1s2 2s2 2p3. Formula of covalent compound?
a)
YX4
b)
X3Y2
c)
YX3
d)
XY3
24.
Volume percent (% v/v) of ethanol: 20.6 cm3 in 0.415 dm3 solution?
a)
0.111
b)
0.0496
c)
0.0201
d)
0.4964
25.
Best indicator for titration between H2SO4 and NH4OH?
a)
Methyl orange (3.2–4.4)
b)
Phenolphthalein (8.2–10.0)
c)
Thymol blue (1.2–2.8)
d)
Bromothymol blue (6.0–7.6)
Reset
