WorksheetsCh. 7 Atomic Structure and Periodicity
Total questions: 60
Worksheet time: 1hrs 14mins
P, Cs, Co, Sr
Which of the following properties are inversely proportional to one another, i.e., which choice represents a pair where as one value increases, the other value decreases? (Assume other variables to be constant).
Sheilding and number of occupied electron shells
Effective nuclear charge and number of protons
First ionization energy and number of occupied shells Atomic number and number of protons
Atomic number and number of protons
For which of the following elements would the most common ion be expected to have a larger radius than that of its corresponding atom?
Cl
Na
Cu
Sr
Which of the following is the most likely value for X (the ionic radius of Be2+) in the table?
60 pm
89 pm
105 pm
110 pm
Which statement best explains the general trend in atomic radii that is observed when crossing a period from left to right?
Electrons enter the same quantum shell, experience no extra shielding, and the number of protons increase
Electrons enter the same quantum shell, experience extra shielding, and the number of protons increase
Electrons enter a different quantum shell, experience no extra shielding, and the number of protons increase
Electrons enter the same quantum shell, experience extra shielding, and the number of protons decrease
Order the following species from smallest to largest radius. Li+, Be2+, Cs+, K+
Li+ < Be2+ < K+ < Cs+
Be2+ < Li+ < K+ < Cs+
K+ < Li+ < Be2+ < Cs+
Cs+ < K+ < Li+ < Be2+
Which of the statements given below is a direct consequence of the fact that first ionization decreases when comparing an element high in a group with an element lower in the same group?
Sodium metal reacts violently with water
Lithium is a more reactive metal than potassium metal
Calcium is a less reactive metal than potassium metal
Rubidium metal is a more reactive metal than sodium metal
Which element will the most likely ion of sulfur be isoelectronic with?
Ne
Ar
Cl
P
Which electron transition would release the greatest amount of energy?
From n = 1 to n = 4
From n = 1 to n = 2
From n = 5 to n = 4
From n = 2 to n = 1
(i) [Kr] 5s1
(ii) [Ne] 3s2 3p5
(iii) [Ar] 4s2 3d10 4p4
(iv) [Ne] 3s2 3p6
The only way to increase the number of photoelectrons emitted is by increasing the _________ of the light
Intensity
Wavelength
Frequency
Energy
The energy of photoelectrons emitted from a metal surface can be increased by
using light of higher frequency.
using light of longer wavelength.
using light of higher intensity.
using monochromatic, polarized light.
Neon lighting is one application using concepts from emission spectroscopy. Which of the following best describes how the emission process works in neon lighting?
Ultraviolet light excites the neon gas to produce emitted white light.
Energy excites the neon gas to an excited state. The relaxation to ground state causes light to be emitted.
Neon gas reacts with oxygen in the air, which causes the emission of light.
none of the above.
Peaks A, B, and C represent the binding energies of electrons in which subshells of neon?
1s, 2s, 2p
2p, 2s, 1s
1s, 1s, 1s
2s, 2p, 2p
Which of the following statements best accounts for peak A being to the left of peaks B and C?
The electron configuration of neon is 1s2 2s2 2p6.
Neon has 8 electrons located in its valence shell.
Core electrons of an atom experience a much higher effective nuclear charge than valence electrons
Peaks B and C show first ionization energies in neon, whereas peak A shows the second ionization energy of neon
Which of the following statements best accounts for peak C being three time the height of peak B?
The intensity of the photoelectron signal at a given energy is a measure of the number of electrons in that energy level.
Electrons represented by peak B have approximately triple the binding energy than those represented by peak C
In a photoelectron spectrum, as binding energy increases the relative number of electrons decreases.
The height of peaks in a photoelectron spectrum does not have any relation to the structure of the atom
If the binding energy of an electron is between 0 - 10 eV, it can be assumed that the electron originated in:
an s orbital
a p orbital
a core electron
a valence orbital
What is the identity of element Z?
Boron
Carbon
Neon
Magnesium
The frequency of violet light is 7.5x1014 Hz. What is its wavelength?
4.0x10-7 m
4.0x107 m
2.25x1023m
2.25x1023 Hz
If an AM radio station broadcasts at
9.95 x 105 Hz, what is the wavelength of this radiation?
6.59 x 10-28 m
1.01 x 10-6 m
3.32 x 10-3 m
302 m
The frequency of light is 7.14 x 1014 Hz. What is the energy?
4.73 x 10-19 J
1.20 x 10-48 J
1.13 x 10-17 J
4.97 x 10-49 J
Calculate the energy of light with a frequency of 5.10 x 1014 Hz.
3.38 x 10-19 J
5.88 x 10-7 J
9.62 x 1012 J
1.04 x 10-13 J
What is the frequency of ultraviolet light with a wavelength of 1.24 x 10-7 m?
2.42 x 1015 Hz
8.22 x 10-34 Hz
3.00 x 108 Hz
1.04 x 1013 Hz
Newton’s prism experiments showed that white sunlight is made up of
the full electromagnetic spectrum.
only blue light.
all the colors of the visible spectrum.
only the longest wavelengths.
Light in the form of a particle that has discrete amount of energy is called a
Charm
Photon
Exciton
Muon
Any given orbital may hold a maximum of __ electrons
2
8
18
32
The first energy level to have d-orbitals is:
1
2
3
4
What is untrue about f orbitals?
first found at energy level 4
when all f orbitals of a given energy level are full, they may contain up to 14 electrons
there are 5 different orientations, or axes
each f orbital may hold an electron with a +1/2 spin and a -1/2 spin
This shape is that of a/n:
s orbital
p orbital
d orbital
f orbital
What is the correct representation for an orbital which has an "n" value of 4 and an "l" value of 2?
4d
4s
4f
4p
What quantum number describes the energy level of an orbital?
l
m
s
n
Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?
2, 1, 0, -½
2, 0, 0, -½
3, 1, 1, +½
3, 0, 0, +½
Which set of Quantum numbers is not allowed?
(3,1,1,-1/2)
(2,1,-2,+1/2)
(4,2,-1,-1/2)
Identify the subshell in which electrons with the following quantum numbers are found:
n = 3, l = 2
3s
3p
3d
Ionization energy is...
the energy required to add an electron to a specific atom
how much energy it takes to remove an electron from an atom in the gas phase
the energy required to shield the outer electrons from the nucleus
a measure of the ability of an atom to attract electrons in the gas phase
What is the noble gas electron configuration for the Sulfur atom?
[Ar] 3p4
[He] 3s23p4
[Ne] 3s23p4
[Na] 3s23p4
Which of the following ions do not have this electron configuration?
O2-
F-
Na+
Be2+
The sulfate anion is a complex anion with the formula [SO4]2-. What is the likely charge on the sulfur ion within the sulfate anion complex?
2+
3+
4+
6+
