Electromagnetic Spectrum
Electrons Accommodated in Energy
Levels and Sublevels
Electrons Accommodated in Energy
Levels and Sublevels
Quantum Numbers of the First 30 Atomic Orbitals
List in the order of increasing
electronegativity of
I, Br, At, F, Cl
At, I, Br, Cl, F
Identify one trend in this diagram
below.
Identify which trends in this
diagram below.
Which of the following elements is
most electronegative? (choose one)
C, Li, Ti, Zn, B
the one closest to F:
Provide the symbol for the elements
with the following electron
configurations?
a. 1s22s22p63s2
b. 1s22s2
c. 1s22s22p63s23p64s1
d. 1s22s22p63s23p2
Provide the symbol for the elements
with the following electron
configurations?
a. 1s22s22p63s2
b. 1s22s2
c. 1s22s22p63s23p64s1
d. 1s22s22p63s23p2
a. Mg
b. Be
c. K
d. Si
Indicate an element in the same
group as an elements has the
electronic structure:
[Ar]4s23d2
Indicate an element in the same
group as an elements has the
electronic structure:
[Ar]4s23d104p2
Indicate an element in the same
group as an elements has the
electronic structure:
[Ar]4s23d104p2
this is Ge any element in that group
the C group
Which of the following is the correct electron configuration for Ne?
A) 1s1
B) 1s2
C) 1s22s1
D) 1s22s2
E) 1s22s22p1
F) 1s22s22p2
G) 1s22s22p3
H) 1s22s22p4
I) 1s22s22p5
J) 1s22s22p6
Which of the following is the correct electron configuration for Ne?
A) 1s1
B) 1s2
C) 1s22s1
D) 1s22s2
E) 1s22s22p1
F) 1s22s22p2
G) 1s22s22p3
H) 1s22s22p4
I) 1s22s22p5
J) 1s22s22p6
Draw a rectangle (
), this is your periodic table.
On it indicate the direction of increasing ionization,
electron affinity, electronegativity and radii.
Multiple Choice
1. Which of the following relationships is true?
A. Higher-energy light has a higher frequency
than lower-energy light does.
B. Higher-energy light has a longer
wavelength than lower-energy light does.
C. Higher-energy light travels at a faster speed
than lower-energy light does.
D. Higher-frequency light travels at a slower
speed than lower-energy light does.
Multiple Choice
1. Which of the following relationships is true?
A. Higher-energy light has a higher frequency
than lower-energy light does.
B. Higher-energy light has a longer
wavelength than lower-energy light does.
C. Higher-energy light travels at a faster speed
than lower-energy light does.
D. Higher-frequency light travels at a slower
speed than lower-energy light does.
Write out the periodic Law,
Give an elemental example…
Multiple Choice
2. The energy of a photon is greatest for
A. visible light.
B. ultraviolet light.
C. infrared light.
D. X-ray radiation.
Multiple Choice
2. The energy of a photon is greatest for
A. visible light.
B. ultraviolet light.
C. infrared light.
D. X-ray radiation.
Multiple Choice
3. What is the wavelength of radio waves
that have a frequency of 88.5 MHz?
A. 3.4 m
B. 8.9 nm
C. 0.30 m
D. 300 nm
Multiple Choice
3. What is the wavelength of radio waves
that have a frequency of 88.5 MHz?
A. 3.4 m
B. 8.9 nm
C. 0.30 m
D. 300 nm
Multiple Choice
4. Which transition in an excited hydrogen
atom will emit the longest wavelength of
light?
A. E5 to E1
B. E4 to E1
C. E3 to E1
D. E2 to E1
Multiple Choice
4. Which transition in an excited hydrogen
atom will emit the longest wavelength of
light?
A. E5 to E1
B. E4 to E1
C. E3 to E1
D. E2 to E1
Multiple Choice
5. Which of the following quantum numbers is
often designated by the letters s, p, d, and f
instead of by numbers?
A. n
B. l
C. m
D. s
Multiple Choice
5. Which of the following quantum numbers is
often designated by the letters s, p, d, and f
instead of by numbers?
A. n
B. l
C. m
D. s
Multiple Choice
6. Which quantum number is related to the
shape of an orbital?
A. n
B. l
C. m
D. s
Multiple Choice
7. What is the maximum number of unpaired
electrons that can be placed in a 3p
sublevel?
A. 1
B. 2
C. 3
D. 4
Multiple Choice
7. What is the maximum number of unpaired
electrons that can be placed in a 3p
sublevel?
A. 1
B. 2
C. 3
D. 4
Multiple Choice
8. What is the maximum number of
electrons that can occupy a 3s orbital?
A. 1
B. 2
C. 6
D. 10
Multiple Choice
8. What is the maximum number of
electrons that can occupy a 3s orbital?
A. 1
B. 2
C. 6
D. 10
Multiple Choice
9. Which element has the noble-gas
notation [Kr]5s24d2?
A. Se
B. Sr
C. Zr
D. Mo
Multiple Choice
9. Which element has the noble-gas
notation [Kr]5s24d2?
A. Se
B. Sr
C. Zr
D. Mo
Short Answer
10. When a calcium salt is heated in a flame, a photon of
light with an energy of 3.2 × 10−19 J is emitted. On the
basis of this fact and the table below, what color
would be expected for the calcium flame?
Frequency, s–1
7.1 × 1014
6.4 × 1014
5.7 × 1014
Wavelength, nm
422
469
526
Color
violet
blue
green
Frequency, s–1
5.2 × 1014
4.8 × 1014
4.3 × 1014
Wavelength, nm
577
625
698
Color
yellow
orange
red
Short Answer
10. When a calcium salt is heated in a flame,
a photon of light with an energy of 3.2 ×
10−19 J is emitted. What color would be
expected for the calcium flame?
Answer: The color will be orange.
Converting energy into frequency gives
4.8 × 1014, which corresponds to the
frequency of orange light.
Short Answer
11. The electron configuration of sulfur
is 1s22s22p63s23p4. Write the orbital
notation for sulfur.
Short Answer
11. The electron configuration of sulfur
is 1s22s22p63s23p4. Write the orbital
notation for sulfur.
Answer:
       
1s
2s
2p
3s
3p

Extended Response
12. Explain the reason for the hydrogen
line-emission spectrum.
Extended Response
12. Explain the reason for the hydrogen lineemission spectrum.
Answer: Electrons in atoms can occupy
orbitals of only specific energies. When an
atom is excited, the electron is no longer
in the ground state. When the electron
returns to a lower energy level, light is
emitted. Because only specific energies
are allowed, certain wavelengths of light
are emitted, giving rise to the individual
lines in the spectrum.
Extended Response
13. When blue light shines on potassium
metal in a photocell, electrons are
emitted. But when yellow light shines
on the metal, no current is observed.
Explain.
Multiple Choice
1. In the modern periodic table, elements are
arranged according to
A.
decreasing atomic mass.
B.
Mendeleev’s original model.
C.
increasing atomic number.
D.
when they were discovered.
Multiple Choice
1. In the modern periodic table, elements are
arranged according to
A.
decreasing atomic mass.
B.
Mendeleev’s original model.
C.
increasing atomic number.
D.
when they were discovered.
Multiple Choice
2. Group 17 elements, the halogens, are the most
reactive of the nonmetal elements because they
A. require only one electron to fill their outer
energy level.
B. have the highest ionization energies.
C. have the largest atomic radii.
D. are the farthest to the right in the periodic table.
Multiple Choice
2. Group 17 elements, the halogens, are the most
reactive of the nonmetal elements because they
A.
require only one electron to fill their outer
energy level.
table.
B.
have the highest ionization energies.
C.
have the largest atomic radii.
D.
are the farthest to the right in the periodic
Multiple Choice
3. The periodic law states that
A.
B.
C.
D.
the chemical properties of elements can be
grouped according to periodicity.
the properties of the elements are functions of
atomic mass.
all elements in the same group have the same
number of valence electrons.
all elements with the same number of occupied
energy levels must be in the same group.
Multiple Choice
3. The periodic law states that
A.
the chemical properties of elements
can be
grouped according to periodicity.
B.
the properties of the elements are
functions of
atomic mass.
C.
all elements in the same group have
the same number of valence electrons.
D.
all elements with the same number of
occupied energy levels must be in the same
group.
Multiple Choice
4. As you move left to right across Period 3
from Mg to Cl, the energy needed to remove
an electron from an atom
A.
generally increases.
B.
generally decreases.
C.
does not change.
D.
varies unpredictably.
Multiple Choice
4. As you move left to right across Period 3
from Mg to Cl, the energy needed to remove
an electron from an atom
A.
generally increases.
B.
generally decreases.
C.
does not change.
D.
varies unpredictably.
Multiple Choice
5. Which of the following elements has the
highest electronegativity?
A.
oxygen.
B.
hydrogen.
C.
fluorine.
D.
carbon.
Multiple Choice
5. Which of the following elements has the
highest electronegativity?
A.
oxygen.
B.
hydrogen.
C.
fluorine.
D.
carbon.
Multiple Choice
6. The noble gases have
A.
high ionization energies.
B.
high electron affinities.
C.
large atomic radii.
D.
a tendency to form both cations and anions.
Multiple Choice
6. The noble gases have
A.
high ionization energies.
B.
high electron affinities.
C.
large atomic radii.
D.
a tendency to form both cations and
anions.
Multiple Choice
7. Which electron configuration is not correct?
A.
O2– [He]2s22p6
B.
Mg2+ [He]2s22p6
C.
V3+ [Ar]3d2
D.
Al3+ [Ar]2s22p6
Multiple Choice
7. Which electron configuration is not correct?
A.
O2– [He]2s22p6
B.
Mg2+ [He]2s22p6
C.
V3+ [Ar]3d2
D.
Al3+ [Ar]2s22p6
Multiple Choice
8. Which two elements are more likely to have
the same charge on their ions?
A.
Se and As
B.
Sn and Si
C.
Ca and Rb
D.
I and Xe
Multiple Choice
8. Which two elements are more likely to have
the same charge on their ions?
A.
Se and As
B.
Sn and Si
C.
Ca and Rb
D.
I and Xe
Multiple Choice
9. Which list ranks the elements Sr, Te, Kr, Ru,
and Cs in order of increasing electron affinity?
A.
Sr < Te < Ru < Cs < Kr
B.
Te < Ru < Sr < Cs < Kr
C.
Cs < Sr < Ru < Te < Kr
D.
Kr < Cs < Sr < Ru < Te
Multiple Choice
9. Which list ranks the elements Sr, Te, Kr, Ru,
and Cs in order of increasing electron affinity?
A.
Sr < Te < Ru < Cs < Kr
B.
Te < Ru < Sr < Cs < Kr
C.
Cs < Sr < Ru < Te < Kr
D.
Kr < Cs < Sr < Ru < Te
Short Answer
10. The second ionization energies for the elements S–Ti are listed
in a scrambled order below. Assign the correct IE2 value to
each element (Hint: S has IE2 = 2251 kJ/mol, and Ti has IE2 =
1310 kJ/mol.) Explain your reasoning.
IE2 values (kJ/mol): 2666, 2297, 3051, 1235, 2251, 1310, and
1145
Short Answer
10. The second ionization energies for the elements S–Ti are listed
in a scrambled order below. Assign the correct IE2 value to
each element (Hint: S has IE2 = 2251 kJ/mol, and Ti has IE2 =
1310 kJ/mol.) Explain your reasoning.
IE2 values (kJ/mol): 2666, 2297, 3051, 1235, 2251, 1310, and
1145
Answer: S: 2551 kJ/mol; Cl: 2297 kJ/mol;
Ar: 2666 kJ/mol; K: 3051 kJ/mol; Ca: 1145 kJ/mol; Sc: 1235
kJ/mol; Ti: 1310 kJ/mol. For the second ionization, the general
trend is for increasing IE2 across the period in Groups 218 with
Group 1 having the highest IE2. IE2 decreases going down a
group.
Short Answer
11. What group most commonly forms 2–
ions? Explain your reasoning.
Short Answer
11. What group most commonly forms 2–
ions? Explain your reasoning.
Answer: Group 16 most commonly forms 2–
ions, because these elements require only
two more electrons to fill their shell (obtain a
noble-gas configuration).
Extended Response
12. An ordered list of atomic radii for 14 consecutive elements is
shown below. Without using the graph in your book, make a graph
of these atomic radii versus the element’s atomic number. Explain
your reasoning.
Atomic radii (pm): 75, 73, 72, 71, 186, 160, 143, 118, 110, 103,
100, 98, 227, and 197.
Extended Response
12. An ordered list of atomic radii for 14 consecutive elements is
shown below. Without using the graph in your book, make a graph
of these atomic radii versus the element’s atomic number. Explain
your reasoning.
Atomic radii (pm): 75, 73, 72, 71, 186, 160, 143, 118, 110, 103,
100, 98, 227, and 197.
Answer: There are eight numbers between the first and second
minimum; therefore, these eight elements must either be the
second or third period. There are four numbers before the first
maximum; hence, these four numbers must be elements in the
second row because the first row contains only two elements (H
and He). Therefore, the eight elements must be in the third period.
The first atomic radius listed must correspond to atomic number 7,
which is N. (continued on next slide)
Extended Response
12. Answer, continued: Your graph should
look like
the following: