Download GROUP QUIZ UNIT 04 NAMES I. Fill in the charts (1 point per blank

GROUP QUIZ UNIT 04
NAMES
________________________________ ________________________________
________________________________ _______________________________
I. Fill in the charts (1 point per blank).
Energy level (4 lowest)
# sublevels
Sublevel
# orbitals
# orbitals
1. _____
15. ______
29. ______
2. _____
16. ______
30. ______
3. _____
17. ______
31.
4. _____
18. ______
5. _____
19. ______
6. _____
20. ______
7. _____
21. ______
8. _____
22. ______
9. _____
23. ______
10. _____
24. ______
11. ______
25. ______
12. ______
26. ______
13. ______
27. ______
14. ______
28. ______
32.
33.
Maximum # e-s
# electrons
NAME: __________________________________
Group Quiz Unit 4
I. Fill in the charts (1 point per blank).
Energy level (4 lowest)
# sublevels
Sublevel
Maximum # e-s
# orbitals
# orbitals
# electrons
II. Choose the best answer to each question (2 points each).
____1. If the third main energy level contains 15 electrons, how many more could it possible hold?
a. 0
b. 1
c. 3
d.
17
____2. At n = 1, the total number of electrons that could be found is
a. 1.
b. 2.
c.
18.
6.
d.
____3. If the four principal quantum numbers for the last electron of an element is n=4, l=2, m=-1, and ms= -1/2, what is the element?
a. Zr
b. Co
c. Rh
d. Se
____4. A three-dimensional region around a nucleus in which a particular electron may be found is called a(n)
a. spectral line.
b. electron path.
c. orbital.
d. orbit.
____5. An orbital that would never exist according to the quantum description of the atom is
a. 3d.
b. 8s.
c. 6d.
____6.
a.
b.
c.
d.
d.
3f.
An orbital may be defined as
the most stable state of an atom.
the circular path followed by an electron around the nucleus.
the positively charged central part of an atom.
a highly probable location of an electron within the atom.
____7. The letter designations for the first four sublevels with the number of electrons available for each sublevel are
a. s:1, p:3, d:10, and f:14.
b. s:1, p:3, d:5, and f:7.
c. s:2, p:6, d:10, and f:14.
d. s:1, p:6, d:10, f:4.
____8. How many half-filled orbitals are there in a bromine atom?
a. 1
b. 2
c.
3
d.
4
____9. What is the electron configuration for neon?
a. 1s22s22p43s2
b. 1s21p62s2
1s22s22p6
d.
1s22p63s2
5p
d.
5s
c.
____10. The atomic sublevel with the next highest energy after 4p is
a. 4d
b. 4f
c.
____11. The Lewis-dot configurations of all noble gases beginning with neon would show how many dots around
element’s symbol?
a. 1
b. 2
c. 8
d. 10
____12. The element with the electron configuration 1s22s22p63s23p2 is
a. Mg
b. C
c. S
d.
the
Si
____13. The Lewis-dot notation for an element in the third period is represented by a symbol surrounded by three dots. The electron
configuration for this element is
a. 1s22s22p63s23p1.
b. 1s22s22p63s13p2.
c. 1s22s22p53s23p2.
d. 1s22s22p63s2.
____14. The Lewis-dot notation for fluorine would show
a. 9 dots around the symbol.
b. 1 dot around the symbol.
c. 7 dots around the symbol.
d. 8 dots around the symbol.
____15 How many electrons are needed to fill the third main energy level if it already contains 8 electrons.
a. 0
b. 8
c. 10
d. 22
____16. Complete the electron-configuration notation for bromine: 1s22s22p6
a. 3s23p64s24p5
b. 3s23p64s24p54d10
c. 2d103s23p64s24p5
d.
3s23p64s23d104p5
____17. The major difference between a 1s orbital and a 2s orbital is that
a. the 2s orbital can hold more electrons.
b. the 2s orbital has a slightly different shape.
c. the 2s orbital is at a higher energy level.
d. the 1s orbital can have only one electron.
____18. The maximum number of electrons that can occupy any single orbital at any energy level is
a. two, if they have opposite spins.
b. two, if they have the same spin.
c. one.
d. no more than eight.
____19. The electron configuration for the element with atomic number 11 is
a. 1s22s22p63s1.
b. 2s22p23p6.
c. 1s22s22p43s3.
d.
1s22s22p22p62d1.
____20. The total number of orbitals that can exist at the second main energy level is
a. 2.
b. 3.
c. 4.
d.
8.
d.
4
____21. In the correct Lewis dot notation for sulfur, the symbol S is surrounded by
a. three pairs of dots.
b. two pairs of dots and two single dots.
c. four single dots.
d. two pairs of dots.
____22. How many sublevels are there in the second principal energy level?
a. 1
b. 2
c. 3
____23. What shapes of orbitals are in the third principal energy level?
a. s only
b. s and p only
c. s, p, and d only
d.
s, p, d and f
____24. What is the maximum number of d orbitals in one energy level?
a. 1
b. 3
c. 5
d.
7
____25. What is the maximum number of electrons in the second principle energy level?
a. 2
b. 8
c. 18
d.
32
d.
4f
____26.
a.
b.
c.
d.
The formula 2n2 represents ___.
the number of orbitals in a sublevel
the maximum number of electrons that can occupy an energy level
the number of sublevels in any energy level.
None of the above.
____27. Which of the following sublevels has the lowest energy?
a. 3d
b. 4s
c.
4p
____28.
a.
b.
c.
d.
If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
one electron in each orbital
two electrons in one orbital, one in another, none in the third
three in one orbital, one in the other two
cannot be predicted, determined by random chance
____29. How many unpaired electrons are there in a sulfur atom?
a. 0
b. 1
c.
2
____30. What is the number of electrons in the outermost energy level of an oxygen atom?
a. 2
b. 4
c. 6
d.
3
d.
8
III. Problems:
Write the electron configurations using shorthand notation (2 points) and draw orbital spin diagrams for the following
elements (2 points):
31. arsenic
e- config:
Spin diagram:
32. barium
e- config:
Spin diagram:
Give the four quantum numbers for the following boxed electron. (1 point for each quantum number)
33.
1s
2s
2p