VAHS
M
This is 60% of what is on the final exam.
1.
What ideas did each of the four men below contribute to atomic theory? [pictured from left to right in each row: Schrodinger, , Heisenberg de Broglie Bohr]
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V
2.
Next to each, write how many total electrons it has. Then write how many valence e- it has.
F N B
V
5+
F
-
N
3-
B
3+

4.
On these diagrams, only consider the five lowest permitted orbits/energy levels in a hydrogen atom, and that the amount of jump between levels is correlated to the energy ofthe photon that is absorbed or emitted.
An electron is currently in energy level 3, as shown at right.
Clearly circle your answers below.
(a) Which electron movement starting from energy level 3 would emit the lowest-energy photon?
3 →5
3 →4
3 →2
3→ 1
5.
Which electron movement starting from energy level 3 would absorb the highest-energy photon?
3 →5
3 →4
3 →2
3 →1
6.
Write the full electron configuration (1s22s2, etc) for each of the following elements:
7.
Potassium (19 total electrons)
8.
The most common ion of potassium (20 total electrons)
9.
Krypton (36 total electrons)
10.
Write the noble gas abbreviation for neutral bromine (35 total electrons
11.
Write the boxes and arrows notation to show the electron orbitals of titanium
Remember what the n, l, m, s numbers stand for: n- number:
Lowest the n number can be is 1. n can be any positive integer.
L= number
L is a follower. It depends on what number n is. The lowest L can be is 0.
The highest L can be is n-1.
L can be any integer in between 0 and n-1 m- number m depends on L.
The lowest m can be is –L.
The highest m can be is +Lj.
M can be any integer in between -L and +L s-number s is either +1/2 or -1/2.
An up arrow in a diagram is s=+ ½.
A down arrow is s= -1/2
12.
For 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 2 a.
how many electrons are in each energy level? b.
what element is this?
13.
How many e- are in the valence shell of

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 1
14.
Draw the electron dot diagram for 1s 2 2s 2 2p 6 3s 1
15.
Draw a “tree” diagram to show all of the quantum numbers[n,L,m,s] for n = 5 L=2. How many electrons in an atom can have quantum numbers that start with n = 5 L= 2?
16.
How many electrons in an atom can have quantum numbers that start n=9 L=1? (optional: draw little tree if it helps)
17.
Circle the electron from each pair which has the lowest energy OR write "degenerate" after the pair.
[5, 3, 0, +½] OR [4, 1, 0, -½]
[3, 1, 0, -½] OR [3, 2, 0, -½]
[4, 3, 0, -½] OR [4, 3, -1, -½]
The following refer to the [ n, L, m, s ] numbers for the solutions to the Schrodinger Equation:
18.
The letter ______ represents the shape of the 90% probability orbital
19.
The letter ______ represents the spin, up and down
20.
The letter ______ represents the orientation of the orbital (y, x, z axis for the p orbital but something more complex than that for the d and f orbitals)
21.
The letter ______ represents the energy and the average distance of the electron from the nucleus
Answer the following questions by looking at the appropriate pages in your black book.
Principal Quantum Number (pp. 117-118)

What are the first 5 values of n
(the principal quantum
number)?

What is the formula for finding how many electrons a level can hold?
 how many electrons can level
 n=6 hold?
Energy Sublevels and Orbitals (pp. 119-120)
 what is a sublevel and what letter is its quantum number symbol?
 how can you calculate how many sublevels a given level should have?
 how many pairs of electrons can be held in the s, the p, the d, and the f sublevels?
Shape of the Charge Cloud (p. 121)
 what is the charge of the
 nucleus? of the electrons? what factors push, repel, and shield the electrons?

(pp. 122-123)
 in the case where L=3, what values can m have?
 what are the only two values that the last quantum number, s, can have?
22. Assume that there is a substance in each of these containers and the manometer is open to the atmosphere. The ambient (room) pressure is 441 inches of water. c. What is the vapor pressure, in units of “inches of water” for Liquid 1? _______ d. What is the vapor pressure, in units of “inches of water” for Liquid 2? _______ e.
What is the vapor pressure, in units of “inches of water” for Liquid 3? _______ f. If they are all at the same temperature, which liquid has the strongest intermolecular forces?
At 20
At

1.
At what temperature does water have a vapor pressure of 110kPa? ___________
2.
Find the boiling point of each liquid in  C.
Propanone ________ ethanol_________
water________ ethanoic acid________
3.
Find the vapor pressure of the 4 liquids listed above at 75  C.
Propanone ________ ethanol_________
water________ ethanoic acid________
4.
Using Tuesday’s lesson, In each pair of compounds, circle the one , which will boil at the highest temperature: a.
C
2
H
6
versus C
4
H
10 b.
Chlorine liquid versus fluorine liquid c.
CH
4
versus H
2
O
5.
In each pair of compounds, circle the one that, at equal temperature, will have the highest vapor pressure. d.
Helium versus xenon e.
Chlorine liquid versus fluorine liquid f.
CH
4
versus H
2
O
6.
During which segment is the substance changing from solid to liquid but its temperature is not changing?
B to C C to D
7.
During which segment is the heat being absorbed but the substance is staying in the same phase (solid or liquid or gas are all
“phases”)?
B to C C to D
8.
9.
10.
Carbon monoxide, a poisonous gas, has a formula of CO. What mass of carbon monoxide occupies a volume of
0.445 L at STP? [First solve for n. Then convert moles of CO into grams of CO.]

11.
What pressure is exerted by 0.693 moles of oxygen in a 7.55 L vessel at 18°C?
12.
A gas filled weather balloon with a volume of 80.0 L is released at sea level at 102.0 kPa pressure and 27.0°C.
The balloon expands to final volume of 835.0L at maximum altitude, where the temperature is 0.00°C. What will be the pressure at this time?
13.
A gas filled weather balloon contains 33.0 L of air at 10.0°C at a pressure of 745. Torr. How many moles of gas are in the balloon?
14.
Examine this phase diagram. a.
When this substance is compressed, starting at 0.611 kPa and 0°C it changes from _____ to ______. b.
Which is denser for this substance i.
Solid ii.
Liquid iii.
Solid and liquid have equal density.
15.
In a closed system, a liquid and its vapor can reach equilibrium. At that point, which is possible: a.
there are equal numbers of vapor and liquid particles and the rate of change from liquid to vapor equals the rate of change from vapor to liquid b.
there are unequal numbers of vapor and liquid particles and the rate of change from liquid to vapor does not equal the rate of change from vapor to liquid c.
neither of these is possible
16.
What is the relationship between the freezing point and melting point of a pure substance?

17.
Examine this phase diagram. a.
When this substance is compressed starting at 40 kPa and 130°C it changes from _____ to ______. b.
Which is denser for this substance i.
Solid ii.
Liquid iii.
Solid and liquid have equal density.
18.
Indicate whether each relationship is direct (linear) or inverse. a.
__________ boiling point and intermolecular forces b.
__________ boiling point and ambient atmospheric pressure c.
__________ vapor pressure of a liquid and temperature of that liquid d.
__________ volume of a gas and pressure of a gas, if temperature is constant e.
__________ pressure of a gas and temperature of a gas, if volume is constant
1.
If you save your birthday balloon in a refrigerator at your house at -25.0 °C and its volume is 2.11 L, what will be the new volume if you take the balloon out of your refrigerator and let it warm up to +25.0 °C (assume constant pressure)?
19.
Region of positive particles
20.
Region of negative particles
21.
Region of neutral particles
22.
Region where particles weigh 1 amu each
23.
Region where particles weigh about
1
2000
amu each (almost zero)
24.
If this is a neutral atom it should have
_____ e- and _____P+
25.
According to the periodic table this is probably the element _____________
26.
This element, on earth, comes in a mix of isotopes with an average mass of
______________.
27.
This particular atom shown in the picture, if it had 40 neutrons, would have a weight of ________ amu
Label this by drawing arrows from the terms to the left.
The following questions all refer to single atoms, not doubles or molecules.
28.
Which has a greater radius? B or F
29.
Which has a greater radius phosphorous or nitrogen?
30.
Which is more difficult ot steal one electron from, sulfur or chlorine?
31.
Which is more difficult to steal one electron from, sodium or lithium?
32.
Which requires more energy to add an electron to, aluminum or boron?
33.
N ame two elements that should act similarly to sulfur.
34.
What charge is the most likely charge if neutral sulfur changes to form an ion?
35.
Which has a greater radius, Mg or Mg 2+ ?
36.
Which has a greater radius, N or N 3?

37.
When it forms an ion, calcium becomes ( + / - ) and its radius (increases
/ decreases )
38.
When it forms an ion, bromine becomes ( + / - ) and its radius (increases
/ decreases )
39.
When it forms an ion, xenon becomes _______ and its radius _____________
40.
Hydrogen gas can be formed by reacting octane in gasoline, C
8
H
18
, with steam, to produce carbon monoxide and hydrogen gas. The balanced reaction for this is
C
8
H
18
+ 8 H
2
O --> 8CO 17H
2 c.
41.
Write the electronegativity number next to each atom. a.
This atom has _____ covalent bonds b.
Of these, ______ are polar covalent bonds c.
And _____ are nonpolar covalent bonds
42.
At standard temperature and pressure, what volume of hydrogen gas can be produced if 100.0 grams of octane react completely? (correct answer 1pt, showing correct work 2pts)
Write the electronegativity number next to each atom. a.
This atom has _____ covalent bonds b.
Of these, ______ are polar covalent bonds
And _____ are nonpolar covalent bonds
Write arrows next to each bond to show which end of the bond the electrons go more towards
Does this molecule have a negative end and positive end that are opposite to each other?
(yes/no)
If you answered “yes”, draw a hollow arrow which shows which end the negative electrons are mostly going towards.
This molecule is
(polar / nonpolar )
Write arrows next to each bond to show which end of the bond the electrons go more towards
Does this molecule have a negative end and positive end that are opposite to each other?
(yes/no)
If you answered “yes”, draw a hollow arrow which shows which end the negative electrons are mostly going towards.
This molecule is
(polar / nonpolar )
43. At STP, circle the gas in each pair that will diffuse most rapidly: a. CO
2
vs CH
4 b. NO
2
vs nitrogen gas c. xenon vs neon
In each case, for underlined characteristic, compare the two particles by writing <, =, or > in the blank. radius: radius: electronegativity: velocity at STP: neutral iron a Ca 2+ ion _______ selenium nitrogen gas
_______
_______
_______ neutral titanium a neutral Ca atom oxygen neon gas number of electrons in the outermost level: number of electrons in the outermost level: neutral phosphorous atom a neutral oxygen atom
_______
_______ neutral nitrogen atom the most common ion of oxygen

stability of the electrons
stability of the electrons number of atoms: mass number of protons: number of electrons ionization energy:
1s
2
2s
2
2p
6
3s
2
_______ a mole of xenon
2.00 moles of helium at STP
_______
_______
_______ an oxygen ion _______ potassium ion _______ oxygen _______
1s
2
2s
2
2p
6
22.4 liters of xenon at STP
30.0 liters of helium at STP a neutral oxygen atom chlorine ion nitrogen
44. What is the molecular mass of a gas if 6.91 g of it occupy 4.38 L at 1.10 atm and 0.00 degrees C?
45. Hydrogen gas collected over water at 60.0 deg C fills a 4.50 L vessel. The manometer indicates that the inside of the vessel has a total pressure of 758 mmHg. a. What is the pressure of just the gas, after you subtract out the pressure of the water vapor? b. What volume would the dry hydrogen gas occupy at STP?
Consider Substance A, chlorine and substance B, CO
2
For A draw the Lewis Dot structure Name the shape
(from notes)
Draw a cartoon of the shape. Write the electronegativity numbers. Add arrows to show polarity .
This molecule is (polar / nonpolar)
For B draw the Lewis Dot structure Name the shape
(from notes)
Draw a cartoon of the shape. Write the electronegativity numbers. Add arrows to show polarity .
This molecule is (polar / nonpolar)
Circle one of these sentences:

Next to each, write either IONIC BOND or
METALLIC BOND.
2
3
2
These sentences are all false!
Replace each BOLD WORD to make the
sentence true.
1.
The three types of bonds are metallic bonds,
GOOBER BONDS, and ionic bonds.
2.
Ionic bonds form when a metal is brought close to A METAL.
Most atoms become stable when their valence shell has SEVEN electrons.
Draw the Lewis dot symbol for each of these, including charge, and square brackets:
 The ion of oxygen
 The ion of magnesium

A neutral atom of xenon
 Ionic bonded magnesium oxide

Ionic bonded potassium iodide
2
2
1.
Draw the electron dot symbol 2.
Draw the electron dot symbol the
ION of oxygen