DEPARTMENT OF CHEMISTRY, CFS, IIUM
SEMESTER III, 2013/2014
QUIZ 5
CHE 0315
NAME:……………………………………………………..MATRIC NO…..………GROUP:…..…
Answer all questions.
PART 1 [5 marks]
[30 mins]
1. Which of the following will form a metallic bond?
A
H
B
Na
C
C
D
He
B/L1/5(e/g)
1. Which of the following is not a dative covalent compound?
A
BF3NH3
B
NH4+
C
NH3
D
H3O+
C/L1/5(g)
1. Which of the following is an ionic compound?
A
BF3
B
HBr
C
BeCl2
D
MgO
D/L1/5(g)
2. Which of the following is the correct arrangement of increasing bond strength?
A
N-S < N-O < N-F
B
N-F < N-O < N-S
C
N-S < N-F < N-F
D
N-F < N-S < N-O
A/L2/5(h)
2. Which of the following is the correct arrangement of increasing bond strength?
A
P-S < P-O < P-F
B
P-F < P-O < P-S
C
P-S < P-F < N-F
D
P-F < P-S < P-O
A/L2/5(h)
2. Which of the following is the correct arrangement of increasing bond strength?
A
C-S < C-O < C-F
B
C-F < C-O < C-S
C
C-S < C-F < C-F
D
C-F < C-S < C-O
A/L2/5(h)
3. What is the type of bond in C - F?
A
ionic
B
polar covalent
C
non-polar covalent
D
dative covalent
B/L1/5(j)
3. What is the type of bond in C – P?
A
ionic
B
polar covalent
C
non-polar covalent
D
dative covalent
B/L1/5(j)
3. What is the type of bond in H - S?
A
ionic
B
polar covalent
C
non-polar covalent
D
dative covalent
B/L1/5(j)
4. What is the molecular shape for SO42-?
A
seesaw
B
trigonal planar
C
tetrahedral
D
square planar
C/L2/5(q)
4. What is the molecular shape for IF4+?
A
square planar
B
trigonal planar
C
seesaw
D
trigonal pyramidal C/L2/5(q)
4. What is the molecular shape for PF6-?
A
trigonal bipyramidal
B
trigonal planar
C
tetrahedral
D
octahedral
D/L2/5(q)
5.
Which of the compound below is a non-polar compound?
A
XeO3
B
C
SF5Cl
D
CH2O
PF2Cl3
D/L3/5(r)
5. Which of the compound below is a non- polar compound?
A
SOF4
B
SO2Cl2
C
CSe2
D
NO2F
C/L3/5(r)
5. Which of the compound below is a non-polar compound?
A
SOF4
B
NH2Cl
C
SiH4
D
NOCl
C/L3/5(r)
Part II [10 marks]
SET 1
1. Describe the formation of metallic bond by using an appropriate model.
[2]/L1/5(e)
[1] for the diagram OR Each metal atom donates their valence electrons
to form a sea of electron.
A metallic bond is formed by the strong attraction between the positively
charged metal and the delocalized electrons. [1]
2. The Lewis structure of C2H3O2-, is shown below. Describe the hybridization
process of Cb.
C (Ground State)
[2]/L3/5(s)
: [He]
[1]
2s
C (Excited State)
2p
: [He]
2s
C (Hybrid)
2p
: [He]
[1]
sp2
2p
3. The Lewis structure of SCN- is as follow:
(a)
Draw other possible resonance structures of SCN- .
[2]/L1/5(n)
(b)
Choose the best resonance structure. Explain
[2]/L2/5(n)
[1] for the structure
It has smaller formal charges, and the negative formal charge
reside at the more electronegative atom. [1]
4. By using Lewis electron dot symbol, show the formation of ionic bond between
Cs and S.
[2]/L2/5d
SET 2
1. Describe the formation of metallic bond by using an appropriate model.
[2]/L1/5€
[1] for the diagram OR Each metal atom donates their valence electrons
to form a sea of electron.
A metallic bond is formed by the strong attraction between the positively
charged metal and the delocalized electrons. [1]
2. The Lewis structure of CH4N2O2, is shown below. Describe the hybridization
process of C.
b)
Show the hybridization process on C.
[2]/L3/5(s)
C (Ground State) :[He]
[1]
2s
2p
C (Excited State) : [He]
2s
C (Hybrid)
2p
: [He]
[1]
sp2
2p
3. The Lewis structure of N3- is as follow:
N
N
N
(a) Draw other possible resonance structures of N3-.
:N
..
N:
..
N
-
..
N
..
[2]/L1/5(n)
N
..
N
..
(b) Choose the best resonance structure. Explain.
N
-
..
N
..
N
..
N
..
-
N
N
[2]/L2/5(n)
..
:
..
:N
..
N:
..
-
N
N
:
-
..
:
..
N
..
N
..
N
[1] for the structure
It has smaller formal charges compare to another two structure. [1]
:
..
N
..
..
:
..
N
-
:
:N
..
N:
..
N
4. By using Lewis electron dot symbol, show the formation of ionic bond between
Al and F. [2]/L2/5d
SET 3
1. Describe the formation of metallic bond by using an appropriate model.
[2]/L1/5(e)
[1] for the diagram OR Each metal atom donates their valence electrons
to form a sea of electron.
A metallic bond is formed by the strong attraction between the positively
charged metal and the delocalized electrons. [1]
2. The Lewis structure of CH4N2O2, is shown below.
a)
Show the hybridization process on N.
[2]/L3/5(s)
N (Ground State) : [He]
[1]
2s
2p
2s
2p
N (Excited State) : [He]
N (Hybrid)
: [He]
[1]
sp3
3. The Lewis structure of NCO- is as follow:
(a) Draw other possible resonance structures of NCO- .
[2]/L1/5(n)
(b) Choose the best resonance structure. Explain.
[2]/L2/5(n)
[1] for the structure
It has smaller formal charges, and the negative formal charge reside at
the more electronegative atom. [1]
4. By using Lewis electron dot symbol, show the formation of ionic bond between
Sr and O. [2]/L2/5d