Chemistry 130 (Review Worksheet #2)
Answer
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1. The ground state electron configuration for element X is 1s 2s 2p 3s 3p . The
compound that X will form with magnesium is
a. MgX
b. MgX2
c. Mg3X2
d. Mg2X3
2. The Pauli Exclusion principle states that
a. No two electrons can have an identical set of four quantum
numbers
b. We always add electrons to the lowest energy orbital
c. We half fill degenerate orbitals before pairing electrons
d. The number of protons is unique to each element
3. The properties of four consecutive elements in the periodic table
(abbreviated Ea, Eb, Ec, and Ed) are listed below (IE=ionization energy,
EN=electronegativity)
Ea
Eb
Ec
Ed
IE (kJ/mol)
780
1060
1005
1255
Radius (pm)
132
128
127
99
EN
1.8
2.1
2.5
3.0
Which of the following sets of elements best fits the properties of Ea, Eb,
Ec, and Ed (in this order)?
a. Mg, Al, Si, P
b. Al, Si, P, S
c. Si, P, S, Cl
d. P, S, Cl, Ar
4. The most reactive elements are found in which locations of the periodic
table?
a. Upper left and upper right
b. Lower left and upper right
c. Upper left and lower right
d. Lower left and lower right
5. Which of the following elements has the smallest atomic radius?
a. Br
b. Ba
c. Be
d. B
6. What is the most likely formula for aluminum oxide?
a. AlO
b. Al2O
c. AlO3
d. Al2O3
7. Which of the following elements has the lowest first ionization energy?
a. Xe
b. Cs
c. Ca
d. Al
8. Which series of species has the same electron configuration?
a. K+, Na+, Ar
b. Sr2+, Br-, Kr
c. B3+, Be2+, O2d. O2-, S2-, Se29. Which of the following has the highest fifth ionization energy?
a. Al
b. Si
c. P
d. S
10. In general, does the first ionization energy increase or decrease across a row? Circle your
choice.
Increase
Decrease
a) The first ionization energy of As is 947 kJ/mol; the first ionization energy of Se is 941
kJ/mol. Do these values agree or disagree with your answer above? Rationalize these
values.
b) Do you expect K or Ca to have a second ionization energy? Briefly explain your answer.
11.) Provide the name/formula for each of the compounds given below.
a) Mg3(PO4)2
h) iron (III) sulfate
b) Ni(OH)2
i) xenon tetrafluoride
c) Pb(CO3)2
j) ammonium nitrate
d) I2O5
k) barium chlorite
e) potassium perchlorate
l) Ca(OH)2
f) zinc nitrate
m) KMnO4
g) tetraphosphorus trisulfide
o) Co2(SO4)3
12.) Provide the correct symbol for the species described below. The given electron
configuration may be in the ground or an excited state.
i) [Ar]4s24p4
ii) [Ne]3s23p5
iii) The -3 ion that is isoelectronic with Ne
13.) Write the ground state electron configuration (using the noble gas shorthand) for each of the
following atoms or ions.
Bi
How many unpaired electrons (if any) does Ni have?
Ti2+
14.) Which of the following electron configurations (for atoms) correspond to an excited state?
Identify the atoms in all cases and write the ground-state electron configuration where
appropriate.
a) 1s22s23p1
b) [Ar]4s23d54p1
15.)
a.) What is the wavelength of the emitted radiation for the 43 transition in a hydrogen atom?
b.) What is the total energy (in KJ) emitted by the 43 transition in a mole of hydrogen atoms?
16.) Which of the following atoms/ions has the smallest radius? Circle each choice.
a. Br- or Kr
b. Be2+ or Mg2+
c. Na+ or Na
d. O or O-
17.) Put the following in order of decreasing atomic radius: S, Mg, Cl, Al
18.) Match the quantum number with the feature it describes
i. n
a. electron spin
ii. ms
b. orbital orientation
iii. ℓ
c. orbital shape
iv. m ℓ
d. orbital size
19.) Define the term “effective nuclear charge” and explain how it relates to the periodic trend
for atomic radius.
20.) The first four ionization energies of an element are approximately 738 kJ/mol, 1450 kJ/mol,
7.7×103 kJ/mol, and 1.1×104 kJ/mol. To which periodic group does this element belong? Explain
your reasoning.
21.) Identify the orbitals below. Also, state the number and type of nodes present
i)
ii)
iii)
Name:
Name:
Name:
Nodes:
Nodes:
Nodes:
http://webphysics.davidson.edu/physletprob/ch10_modern/radial.html