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1a03-2016 Tut4 Q-DE.pdf
1a03-2016_Tut4_Q-DE.pdf
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1a03-2016 Tut4 Q-DE.pdf-CHEM 1A03 TUTORIAL #4 Week...
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1a03-2016_Tut4_Q-DE.pdf-CHEM 1A03 TUTORIAL #4 Week of
Page 1
CHEM 1A03
TUTORIAL #4
Week of October 3, 2016
Questions – Unit 5
_____________________________________________________________________
Page 1 of 2
The following problems (1-7) are based on material from Unit 5 and Chapter 10
1.
Arrange the following in terms of increasing electronegativity:
(a)
Mg, N, O, Si,
(b)
F, Se, Sn, Te
2. For the following anions: SO
3
2-
, CO
3
2-
, NO
3
-
, ClO
3
-
, and ClO
2
-
:
a) Draw Lewis structures and resonance forms
b) What are the average bond orders for the central-atom-to-oxygen bonds in these species?
c) What is the average formal charge on the oxygen atoms in each of these species?
d) Indicate whether the species is an exception to the octet rule (i.e. it has more than an octet of
electrons around one of the atoms).
e) Give the VSEPR AX
n
E
m
classes
f) Predict the shapes of the anion.
3. Oxalic acid, (COOH)
2
, has two ionizable hydrogens and contains a carbon-carbon single
bond. When one mole of oxalic acid reacts with one mole of calcium hydroxide,Ca(OH)
2
, the
salt CaC
2
O
4
is formed.
a) Draw adequate Lewis structures to represent the bonding in the oxalate ion, C
2
O
4
2-
.
b) What is the average carbon-oxygen bond order in oxalate ion?
c) What is the average formal charge on each oxygen atom in oxalate ion?
d) Give the shape around each C atom in the oxalate ion.
4. Phosphoric acid, H
3
PO
4
, contains three oxygen-hydrogen single bonds. When one mole of
phosphoric acid reacts with one mole of sodium hydroxide, the salt sodium dihydrogen
phosphate, NaH
2
PO
4
, results.
a) Draw adequate Lewis structures for H
3
PO
4
and H
2
PO
4
-
.
b) Calculate bond orders for all the phosphorus-oxygen bonds of H
3
PO
4
and H
2
PO
4
-
c) Calculate the formal charges on each oxygen atom in H
3
PO
4
and H
2
PO
4
-
.
Page 2
CHEM 1A03
TUTORIAL #4
Week of October 3, 2016
Questions – Unit 5
_____________________________________________________________________
Page 2 of 2
5. A gaseous molecule "X" is made by burning sulfur in air. "X" is converted to "Y" by
reaction with oxygen in the presence of a catalyst. "Y" reacts vigorously with water to produce
"Z" which turns litmus red.
a) Identify "X", "Y", and "Z".
b) Write a balanced equation for each reaction.
c) Draw Lewis diagrams of the molecules "X" and "Y". Determine their AB
n
E
m
VSEPR
classes and name the molecular shapes. Indicate the bond angles, and if they are ideal or less
than ideal. Are the "X" and "Y" molecules polar or non-polar?
d) When 1 mole of "Z" is titrated with 2 moles of NaOH, a soluble salt "W" forms. Write an
appropriate Lewis electron dot structure for the anion of this salt.
6. For the molecules OCS, ICl
3
, IF
5
, PF
3
, and CCl
2
Br
2
:
a) determine the AB
n
E
m
class; name the molecular shape.
b) decide which have dipole moments, and for those that do, decide the direction of the dipole
moment.
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