Quantum Numbers and Periodic Table Test Review
1) Identify which waves move contain more energy. More energy means lower wavelength (or just closer to gamma)
A. Blue light or red?
B. orange or violet
C. x-ray or yellow
D. infrared or indigo
2) In a hydrogen atom rank the following jumps of an excited electron form highest energy photon released to lowest
energy photon released.
A. 3rd energy level to 1st energy level 103 nm
B. 6th energy level to the 3rd energy level 1094 nm
C. 2nd energy level to the 1st energy level 122 nm
D. 4th energy level to the 2nd energy level 486 nm
So, the highest energy goes with A. Then C, D, and lowest energy is B.
4) Without looking at your notes, write down the Periodic and Group Trends for:
a. Ionization Energy – Increases up and to the right (highest for noble gases)
b.
Atomic Radius – increases down and to the left (biggest is Fr)
c.
Electronegativity – increases up and to the right (highest for halogens)
d. Activity or Reactivity – for nonmetals, highest is F. for metals, highest is Fr
5) How many energy levels exist in an atom? 7
6) How many sublevel exist in an atom? 4 (s, p, d, f)
7) For the “f” sublevel, how many orbitals exist? 7 orbitals (14 electrons)
8) For the “d” sublevel, how many orbitals exist? 5 orbitals (10 electrons)
9) How many electrons can live in the “s” sublevel? 2 electrons (1 orbital)
10) How many electrons can live in the “p” sublevel? 6 electrons (3 orbitals)
11) Determine how many electrons total can live on the 3rd energy level. 18 electrons (s, p, and d electrons)
12) Determine how many electrons total can live on the 4th energy level. 32 electrons (s, p, d, and f electrons)
13) Determine the higher energy orbital in each of the following pairs. Figure out based on which you’d get to last if
doing electron configuration
A. 3d or 4s
B. 4d or 4f
C. 6d or 7s
D. 5p or 4f
14) Write the orbital notation for: For this, make sure you draw each of the orbitals, even if they are empty. Put up
arrows in the entire sublevel before coming back and doubling up at all.
A. Fe
B. Br
C. Al
D. N
15) How many half filled orbitals exist for Al? 1
16) How many empty orbitals exist for Al? 2
17) What is the highest occupied energy in Br? 4p
18) What is the electron configuration for
A. Sr 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
B. Sc 1s2 2s2 2p6 3s2 3p6 4s2 3d1
D. P 1s2 2s2 2p6 3s2 3p3
19) How many valence electrons do the following have?
A. Cu 2
B. P 5
C. Ar 8
D. Br 7
20) Draw the Lewis dot structure for the elements in # 20.
21) Determine the element represented below
E. Al 3
C. Cl 1s2 2s2 2p6 3s2 3p5
A.
Sc 1s22s22p63s23p64s23d1
D.
Cs [Xe]6s1
B. B 1s22s22p1
C. Tc [Kr]5s24d5
E. Os [Xe] 6s24f145d6
22) How many valence electrons do the following elements have?
a. Rn 8
b. Ra 2
c.Xe 8
d.K 1
e.Hg 2
f. As 5
23) Write the lewis dot structures for the following elements: Just put dots for valence electrons around the symbol.
Should never have more than 8. Start at the top and go clockwise with one, then go around a second time and double
up.
a. Cs
b. I
c. Sn
d. Po
e.Ca
f. Zn
24) Name an element for each of the following: You just need to know groups and periods. You don’t need to know
what elements are used for…
a. a halogen used in pool maintenance Cl
g. an actinide metal ending in f8 curium
b. a member of Group 15 in Period 3 P
h. a lanthanide metal ending in f3 Pr
c. an element that has 3 valence electrons Anything in Boron group i. 3 transition metals found in jewelry Au, Ag, Pt
d. a noble gas with the smallest radius He
j. 2 metalloids in Period 4 There are lots: Fe, Mn, Co, Sc, …
e. an alkali metal that is the MOST reactive Fr
k. oxygen group element needed for combustion O
f. an alkaline earth metal important in bone health Ca
l. an inner transition metal used in nuclear plants U
25) Name an element for each of the following:
a. the element in Group 2 and Period 5
Sr
b. The element in Group 18 and Period 4 Kr
c. an element with a -3 oxidation number in Period 3 P
d. an element with a +2 oxidation number in Period 5 Sr
e. an element with a +1 oxidation number in period 4 K
f. the element whose e- config. ends with 5p1 In
g. the element whose e- config. ends with 7s2
Ra
h. the elements whose e- config. ends with 4d4 Mo
i. the element whose e- config. ends with 3d1
Sc
j. the element whose e- config. ends with 5d8 Pt
k. an element that has the valence of s2p4
O Group
l. an element that has a valence of s2p1 boron group
26) Within each of the following groups, state which is the larger:
a. Li and Be
b. F and Ne
c. Rb and Y
d. Au and Ag
e. Br and I and Cl
27) Within each of the following groups, state which has the largest ionization energy:
a. Li and Be
b. F and Ne
c. C and O
d. B and Al
e. K and Na
f. N and Na
28) Within each of the following groups, state which has the greatest electronegativity:
a. Li and Be
b. F and Fr
c.F and Ne
e. Hg and Zr
f. Xe and I
g. Cs and K
d. C and O
29) Identify the following:
[Kr] 5s2 4d3
Nb
[Ne] 3s2 3p5
Cl
[Xe] 6s1 Cs
30) Write Noble Gas configurations for:
Mn [Ar] 4s2 3d5
Te [Kr] 5s2 4d10 5p4
31) Rank the following from least to most active (within each set)):
a.
Mg, Al, Ba
Al -> Mg -> Ba
c. Si, P, S, O Si -> P -> S -> O
b. Br, Ar, I, Ne Ar and Ne -> I -> Br
Ra [Rn] 7s2