Exam # 3 Spring 2000
Chemistry 111
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1. What is the partial pressure of He(g) in a vessel containing
a mixture of 1.00 mol He(g), 2.00 mol Ne(g), and 3.00 mol Ar(g)
with a total pressure of 12.0 atm?

First add all the moles of gas to get 6.00 mol.  Next determine
the fraction of the moles which are He.

1.00
----  = 1/6
6.00

Last multiply the total pressure times the fraction which is He:

1/6 x 12 = 2 atm

2. Which of the following ideal gases has the highest kinetic
energy at 200 K?

All gases have the SAME kinetic energy at the same temperature.

3. Which of the following ideal gases has the highest average
particle speed at 200 K?

The energy is a function of mass and velocity.  Since the
energies are the same (Question 2), the velocities must be
inversely proportional to the mass.  The heavier mass moves
slower while the lightest mass moves the fastest.

4. According to the Kinetic Theory of Gases:

The average kinetic energy of a gas is actually determined by
the temperature but one can extend this to recognize that IF a
gas have an average kinetic energy of a specific value THEN it
must be at a certain temperature.  (Reverse logic)

5. Gases will deviate from the ideal gas law as:

"more" correct.

As temperature moves to either extreme the behavior of gases
deviates from ideal.  Thus as temperature increases gas behavior
deviates and as temperature decreases gas behavior deviates.
When a gas condenses to a liquid, the particles can no longer
behave as gases, the "more" correct answer was D, the gas
approaches condensation to the liquid state.

6. The electron configuration for a P atom is:

P is in the 3rd level and in the p sublevel section of the
periodic table.  P has ALL preceding electron configuration
through Ne and 3s2 3p3 beyond Ne so:

[Ne]3s23p3

7. Light traveling at a wavelength of 557.7 nm is of a green
color.  What is the frequency of this light?

The fact it is green is irrelevant to the calculation.  The same
equation serves for calculating all combinations of frequency
and wavelength.

c = ln

c = 2.998 x 108 m/s

n = c/l

Plug in the values:

n = (2.998 x 108 m/s /557.7 nm

Convert nm to meters by substituting the power of ten for which
the "n" stands:

n = (2.998 x 108/557.7 x 10-9 m

Finish the math:

n = 5.38 x 1014 Hz

Remember Hz means 1/s

8. The frequency of light emitted when an electron moves from n=3
to n=2 is 4.570 x 1014 Hz.  What is the wavelength of
this light?

As above use:

c = ln

c = 2.998 x 108 m/s

This time solve the equation for l:

l = c/n

Substitute the numbers:

l = 2.998 x 108 m/s /4.570 x 1014 Hz

Complete the math:

l = 6.560 x 10-7 m

Recall wavelengths are expressed in nanometers (nm) so adjust the
decimal point and power of ten to get a nano- (10-9

l = 656.0 x 10-9 m

l = 656.0 nm

9. There are four sublevel types associated with electron
orbitals or elements in the current preiodic table.  They are:

D) s, p, d, f

10. Electrons require a certain amount of energy in order to
maintain their motion and position orbiting the nucleus of an
atom.  Since the energy for each level and sublevel is a fixed
amount chemists state the energy is:

A) quantized

11. Which of the following is not an allowed set of quantum
numbers?

n  l  ml  ms

A) 7  0  0  1/2

Perfectly good because 7 is a maximum level, l must be from 0
to n-1 which it is, ml must range from l down to -l
and spin must be either +1/2 or -1/2.

B) 3  1  4  -1/2

BAD!  ml is NOT l to -l

C) 1  0  0  1/2

Perfectly good because 1 is a level, l must be from 0
to n-1 which it is, ml must range from l down to -l
and spin must be either +1/2 or -1/2.

D) 7  6  5  -1/2

Perfectly good because 7 is a maximum level, l must be from 0
to n-1 which it is, ml must range from l down to -l
and spin must be either +1/2 or -1/2.  While we have no elements
that meet this set of numbers, the values follow all the rules
and we may one day find an element with these quantum numbers.

12. What quantum numbers describe a 4s subshell?

Quick and easy

n is the level number so it must be  4

l describes the subshell and s is 0

13. What element has the lowest first ionization energy?

Again, quick and easy.

The lowest ionization energies are with those elements that
lose elections the easiest (or have the lowest
electronegativity).  Look at the periodic table and figure which
element is furthest to the left and farthest down.  Or
alternatively, see which of the given elements has the lowest
electronegativity on the table.

14. Which of the following quantum numbers violates the Pauli
Exclusion Principle?

The principle is that no two electrons in a single atom can
have the same set of quantum numbers.  Perfectly logical since
quantum numbers are used to specify which electron is being
observed so if two in one atom have the same number, the entire
method would fail.

15. How many unpaired electrons does an oxygen atom have?

Use Hund's rule for filling:

There are 2 "s" electrons which are paired and 2 "p"
electrons which are unpaired.

16. Which element has the following orbital diagram beyond Ar?

4s                 3d                      4p
(��)       (��)(��)(��)(��)(��)        (� )(� )(� )

This element is in the 4th level and has passed the 3d level
(it's full).  It has 3 electrons in the p sublevel of the 4th
level so it must be:

C) As

17. Moving from top to bottom in a group in the periodic table

D) increases

More levels means a larger atom.

18. The most electronegative atoms have ________________
attraction for electrons in chemical bonds.

A) the strongest

The way to figure out this question was to read the above
sentence and fill in each choice as you read it.  They were all
worded so they would read correctly.

19. How many valence electrons does a Selenium (Se) atom have?

Check the group number, if greater than 10 cover the 1 (subtract
10) and that's the number of valence electrons.

20. What would the Lewis structure of a boron (B) atom look like?

First see what group B is in.  It is the 13th so subtract 10 an B
has 3 electrons.  So the Lewis structure would be:

.
B)  .B.

21. Which of the following Lewis structures is(are) correct?

+
|      H      |
|      |      |
i) NH4+                           |  H - N - H  |
|      |      |
|      H      |

Looks OK from here.

..   ..  ..
ii) CS2                          :S - C - S:
..   ..   ..

Octets look good BUT count the total number of electrons.
There are 8 on each S and 4 on C for a total of 20 BUT 2 S
and 1 C only have 16 so this is wrong.

..       ..
iii) PF3                          :F - P - F:
..   |   ..
:F:
..

P does not have a complete octet.

iv) SF2                           ..  . .  ..
:F - S - F:
..  . .  ..

Every atom has a complete octet and there are exactly the
right number of total electrons.

22. Which is a correct Lewis structure for OCN- ion?

A) carbon has 5 bonds, can't happen

B) carbon only has 4 electrons, doesn't meet octet rule.

C) Meets octet rule BUT carbon has picked up electrons from
somewhere.  Carbon only has 4 electrons so something is
wrong.

D) Perfect. Octet rule met.  Proper number of electrons.  No
electron shift.

23. An atom has the Lewis structure:
2-
|     :O:     |
| ..  | |  .. |
| :O - X - O: |
| ..       .. |
|             |

What is a possible element for X?

A) F only forms single bonds cause it only needs one
electron.  If it was F, then there are not enough total
electrons

B) B has only 3 electrons to share. So it will only form 3
bonds and there are more total electrons than could be
with B.

C) C fits just right since it forms 4 bonds and the total

D) N likes 3 or 5 bonds and the total number of electrons
is not right.

24.  What is the molecular shape of NF3?

..  . .  ..
:F - N - F:
..   |   ..
:F:
..

Since there are only three attached atoms, one might want to
call this a planar molecule.  BUT, the extra electrons repel the
others.  The electron shape would be predicted to be tetrahedral
since there are four pairs of electrons on the central atom.  It
cannot fit in the tetrahedral shape because a tetrahedron by
definition must have all angles equal.  This molecule is
therefore:

D) triangular (trigonal) pyramid

25. Which of the following is linear?

A) Extra electrons on the central atom repel the others and
cause this molecule to be bent.

B) Same as A.

C) Same as A.

D) This is the only one where all bonds to the central atom
are the same and there are no extra electrons to repel.

26. Which of the following has a tetrahedral molecule shape?

A) Nope, not equal angles to the bonds because the repulsive
forces only match on three of the bonds

B) Nope, not equal angles since there are two bonded atoms
and two unbonded pairs.

C) OK, we hit paydirt.  Four matched bonds with four matched
atoms.  Can't do any better than this.

D) See above.

27. What is the molecular shape of phosgene, CCl2O?

First a note, phosgene is a toxic gas used in World War I to
poison the troops.

Next, look at the probable structure.  C is the most likely
central atom because Cl only gets one bond and O only gets two.
S forms 4 bonds.

Cl
\
C = O
/
Cl

Double bonds behave as single bonds in structures so this is an
AX3 with no extra electrons on the central atom so the

A) triangular planar

28. The structure of phosphate, PO4, ion
is:
3-
|     :O:     |
| ..   |   .. |
| :O - P - O: |
| ..   |   .. |
|     :O:     |
|             |

The O-P-O bond angle is closest to:

In order to answer this one, the testtaker had to first get out
of the "paper" mode and look at the 3-dimensional structure.  I
admit this one was a bit harder than other and when one is
testing it is not always easy to think clearly.  The O-P-O on the
question line affected some who chose D) 180. Had the question
line shown   O    these same folks would have chosen A) 90.
|
P-O

The correct answer is due to the fact that this is a tetrahedral
molecule which has bond angles of B) 109.

29. The bond angle in SF2 is closest to:

..  . .  ..
:F - S - F:
..  . .  ..

Since there are extra electrons on the central atom we know this
is not linear, not 180.  Since there are two extra pairs, we should also
know this is not a planar molecule, so not 120.  That leaves 90
and 109 for answers.  The closest shape this molecule approaches
is that of a tetrahedron, based on electron shape.  SO the angle
is probably closest to 109.

30. Which molecule has a bond angle closes to 120?

A) SO2  Look at Lewis structure.

. .
S
//    \ ..
:O        O:
..        ..

Sure looks like a triangular planar molecule to me.  And
triangular planar molecules have 120 degree angles.

B) SF2  from previous question we know this one is
109.

C) CO2  from class discussion and from problem 25
we know this is linear (180)

D) PF3  Now this is a possible but we already have
one answer.  In order to check we must draw the Lewis
structure.
..  . .  ..
:F - P - F:
..   |   ..
:F:
..

To form an octet, P, the central atom, MUST have an extra
pair of electrons so the molecule is not planar and thus the
angles are not 120.  Also note P is under N in the periodic
table which means it behaves similarly to N and we known N
compounds are triangular pyramid, i.e the extra electrons
bend the molecule from the planar shape but not enough to be
a tetrahedral.

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