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CHEM 219 MODULE 1 PROBLEM SET QUESTIONS WITH ANSWERS 100% CORRECT
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CHEM 219 MODULE 1 PROBLEM SET QUESTIONS WITH ANSWERS 100% CORRECT
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Name: Score:39 Multiple choice questions
Term 1 of 39
The structural formula:
Has what molecular formula?
Each contributing individual resonance structure contributes characteristics to the
overall hybrid structure of the compound. The hybrid "averages" bond lengths and formal
charges by delocalizing them among atoms that share them in each contributing
individual resonance structure.
(c) C7H14
a) Super-Condensed
b) Condensed
c) Bond-line
d) Dash
Two (or more) different chemical compounds with the same molecular formula but
different connectivity between the atoms in their structural formulae.
,Term 2 of 39
The compound carbon monoxide has the following structural formula:
What is the formal charge on the carbon and the oxygen? Show your calculation. What is the
overall charge on the molecule?
a) Branched
b) Linear (continuous)
c) Cyclic
Carbon = 4-(2+3) = -1
Oxygen = 6-(2+3) = +1
Overall = FC Carbon + FC Oxygen = [-1 + (+1)] = 0
Both compounds have a MF of C3H6O - same MF.
Compound "a" has a 3-carbon chain with a C=O in the middle. No H atom
connected to C of C=O.
Compound "b" has a 3-carbon chain with a C=O at the end. There is an H
attached to the C of the C=O.
(b)
,Term 3 of 39
On a piece of scratch paper, write out the Lewis Dot Diagram for each of the indicated
elements and determine the following for each:
a) The number of Lone Pairs the atom possesses in its valence shell.b) The number of Unpaired
Electrons the atom possesses in its valence shell.c) The number of bonds the atom will form.
Oxygen
Carbon
Hydrogen
Nitrogen
Oxygen: 1 lone pair, 1 single bond, 1 double bond, +1 formal charge.
Carbon (1): 0 lone pair, 2 single bond, 1 double bond, 0 formal charge.
Carbon (II): 1 lone pair, 3 single bond, 0 double bond, -1 formal charge.
S orbitals are spherical (single lobe), while P orbitals are dumbbell-shaped (two lobes).
Oxygen - a) 2 b) 2 c) 2
Carbon - a) 0 b) 4 c) 4
Hydrogen- a) 0 b) 1 c) 1
Nitrogen - a) 1 b) 3 c) 3
***Bond that occurs when atoms are shared unequally.
- electronegativity diff: Between 0.4 and 1.8
Term 4 of 39
Major contributor
When an atom is more stable when bonded to another atom
Ideal arrangement/structure
Arrangement/structure does not match or correlate with correct atoms/electrons in an
element.
Less ideal arrangement/structure
, Term 5 of 39
Describe how individual resonance structures impact the true structure of a molecule or
polyatomic ion.
End-on overlap of atomic orbitals leads to the formation of sigma (single) covalent
bonds. Sideways overlap of P orbitals leads to the formation of pi (multiple) covalent
bonds.
Each contributing individual resonance structure contributes characteristics to the
overall hybrid structure of the compound. The hybrid "averages" bond lengths and formal
charges by delocalizing them among atoms that share them in each contributing
individual resonance structure.
Atoms form bonds by overlapping individual atomic orbitals from each atom to produce
molecular (bonding) orbitals.
S orbitals are spherical (single lobe), while P orbitals are dumbbell-shaped (two lobes).
Term 6 of 39
Ionic bond
***the complete transfer of one or more valence electrons from one atom to another
- electronegativity diff > 1.8 (large)
***Bond that occurs when atoms are shared unequally.
- electronegativity diff: Between 0.4 and 1.8
Two or more structural formula of a molecule with identical arrangements of atoms BUT
different arrangements of electrons
The process or preference of an element to link/bond with another atom of the same
element.
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