Qualifier
Electron Configuration and the Periodic Table
_________________
Name
Part 1: Vocabulary (1 pt each). Choose the correct letter from the choices on the right column which best match the
definitions below.
1.
An electronic configuration that violates the
Aufbau Principle
K
2.
The amount of energy required to remove an
electron from an atom in the gaseous phase
N
3.
The rule that stipulates electrons fill
degenerate orbitals individually before
pairing up
H
4.
A structure that shows the valence
electrons for a given element
J
5.
The radius of an atom when it either loses
or gains electrons
F
F
A)
B)
C)
D)
E)
F)
G)
H)
I)
J)
K)
L)
M)
N)
Quantum
Electromagnetic Spectrum
Photon
Atomic Emission
Ground State
Excited State
Orbital
Lewis Dot Structure
Atomic Radius
Ionic Radius
Ionization Energy
Electronegativity
Aufbau Principle
Hund’s Rule
Part II: Multiple Choice (1 pt each). Each question must show either a mathematical calculation or process of
elimination explaining why it is not the correct answer for credit.
6.
All the elements in Period 3 have a total of 2 electrons
in the
All atoms in Period 3 have a completely filled 1st and 2nd
energy level, but they do not necessarily have a
completely filled 3 energy level.
a. 2s sublevel – holds 2 electrons – full for each
element
b. 2p sublevel – holds 6 electrons –full for each
element
c. 3s sublevel – holds 2 electrons – NOT full for each
element
d. 3p sublevel – holds 6 electrons – NOT full for each
element
7.
Which two characteristics are associated with metals?
Generally, metals have luster, malleability, ductility,
and are good conductors. Metallic atoms are generally
the largest in the period, have the lowest
electronegativity and ionization energy.
a. Low ionization energy and low electronegativity
b. Low ionization energy and high electronegativity
c. High ionization energy and low electronegativity
d. High ionization energy and high electronegativity
8.
The elements in the periodic table are arranged
byatomic number/number of protons
a. Atomic mass
b. Atomic number
c. Number of electrons
d. Number of neutrons
9.
Which atom has a partially filled d sublevel?Write the
orbrital notation for any element in the d sublevel
a. Mn
c. Clnot in the d sublevel
b. Fnot in the d sublevel
d. Zn
Mn: [Ar] ____
4s
____ ____ ____ ____ ____
3d
Zn: [Ar] ____
4s
____ ____ ____ ____ ____
3d
Manganese is the only element here with any unpaired
electrons in the d subshell
10. Elements that readily gain electrons tend to have
Atoms that gain electrons are nonmetals. Nonmetals
are brittle, dull, substances that do not conduct
electricity or heat. Nonmetal atoms are generally the
smallest in the period, have the highest
electronegativity and ionization energy.
a. High ionization energy and high electronegativity
b. High ionization energy and low electronegativity
c. Low ionization energy and high electronegativity
d. Low ionization energy and low electronegativity
Electron Configuration and the Periodic Table
11. How do the atomic radius and metallic properties of
sodium compare to the atomic radius and metallic
properties of phosphorus? Sodium and phosphorus are
in the same period on the periodic table which means
that the radius of sodium is larger than that of
phosphorus. Since sodium is larger it will naturally lose
electrons more readily making it a more metallic atom.
a. Sodium has a larger atomic radius and is more
metallic
b. Sodium has a larger atomic radius and is less
metallic
c. Sodium has a smaller atomic radius and is more
metallic
d. Sodium has a smaller atomic radius and is less
metallic
12. Quantum numbers [n, l, m, s], are the solutions to the
Schrödinger Wave Equation. The angular momentum
quantum number, l,
Also called the azimuthal quantum number, l, describes
the shape of the orbital.
a. Describes the principle level and the size of the
orbital, n
b. Describes the sub-level and the size of the orbital,
not a quantum number that does both of these
c. Describes the principle level and the shape of the
orbital, n
d. Describes the sub-level and the shape of the
orbital
______________
Name
13. A diatomic element with a high ionization energy would
most likely be
Diatomic elements = 7,7,7 , nonmetals have high
electronegativity, small radius
a. a nonmetal with a high electronegativity
b. a nonmetal with a low electronegativity
c. a metal with a high electronegativity
d. a metal with a low electronegativity
14. Which grouping of circles, when considered in order
from the top to the bottom, best represents the
relative size of the atoms Li, Na, K, and Rb,
respectively?
Radius of atoms increases as you go down a group, so
Li < Na < K <Rb
15. As the elements across Period 2 are considered the
atomic radius is
Across a period – atomic radius decreases, ionization
energy increases, electronegativity increases, nuclear
charge is greater and more effective
a. larger and the nuclear charge is greater
b. larger and the nuclear charge is smaller
c. smaller and the nuclear charge is greater
d. smaller and the nuclear charge is smaller
Part III: Completion
Using the information given in the table below, complete the open blocks [6 pts]
Electron Transition
n = 3 to n = 1
8.
Wavelength Emitted
6.
n = 6 to n = 2
n = 4 to n = 2
10.
Radiation Type
Color
103 nm
7.
UV
None
410 nm
9.
Visible
violet
486 nm
visible
11.
blue
Electron Configuration and the Periodic Table
______________
Name
16. How many unpaired electrons in each of the following elements? Write the orbital notation correctly labeling the orbitals
containing the electrons. Use lines or boxes for each orbital and arrows for the electrons.
[2 each]
a. N 3
b. K1
Orbital Notation:
Orbital Notation:
[He] ____
2s
____ ____ ____
2p
[Ar] ____
4s
17. In the space below, write the following notations for Fe.
a. Write the noble gas configuration.[2]
[Ar]4s23d6
b.
Write the orbital notation for the electrons past the noble gas. Include the correct subshell in the boxes and use
arrows to represent electrons. [2]
c.
[Ar ]___
4s
___ ___ ___ ___ ___
3d
Part IV: Free Response Questions:All questions must be answered in complete sentences to receive credit.
18. Explain, in terms of electrons, why the radius of a nitride ion is larger than the radius of a nitrogen atom. Show the
electron configuration of each species. [2]
N 1s22s22p3, 7 protons, 7 electrons
N-31s22s22p6, 7 protons, 10 electrons
Nitride is larger than nitrogen because it has 3
extra electrons that repel each other in the outer
shell.
19. A sample of a potassium-containing compound is heated in the flame of a Bunsen burner until the atoms are in the excited
state. The color of the flame appears pink.
a. Explain the pink color of the flame in terms of both subatomic particles and energy states. [1]
Atoms of potassium become excited when they are heated in a flame. The electrons of potassium absorb energy and
move to a higher energy level (the excited form) and when they release the energy the electron falls back to the n=2
energy level, where visible light is produced. A photon is released as the electron relaxes with a wavelength that
corresponds to the visible spectrum, specifically pink light.
20. In the space below, answer the following questions for arsenic
a. Write an electron configuration for an atom of arsenic in an excited state. [1]
Ground state:
1s22s22p63s23p64s23d104p3
Excited state: 1s22s22p63s23p64s23d104p26s1
Note: there is more than one possible configuration for the excited state, the configuration can be different, but the
quantity of electrons must be the same
b.
Explain, in terms of atomic structure and electron configuration, how arsenic reacts. [1]
Arsenic reacts by gaining three valence electrons to completely its 4p orbitals and achieves the noble gas configuration
of krypton.
Electron Configuration and the Periodic Table
______________
Name
21. The latest element to have a claim of discovery, with six atoms having been detected by a joint Russia-US collaboration at
Dubna, Moscow Olbast, Russia, in 2009-2010, is Unuseptium. The temporary name for this element is assigned until the
discovery is acknowledged by the IUPAC. Ununseptiums symbol is Uus. Scientist created this element by fusing Calcium-48
and Berkelium-249. The new element has the following electron configuration 2-8-18-32-32-18-7.
a. State the group and period this element is in. [1]
Element #117 – 117 electrons & 117 protons
Group 17, Period 7
b.
Draw the Lewis electron-dot diagram for the atom. [1]
Uus – 7 valence electrons = 7 dots
Ask for this in class
c.
List two other elements with similar properties as this element. [2]
F, Cl, Br, I, At
22. State the trend in first ionization energy for the
elements in the table as the atomicnumber increases.
[1]
The first ionization energies in the table decrease as
the atomic number increases.
23. Explain, in terms of atomic structure, why this trend
occurs. [1]
This trend occurs because orbital size increases as you
go down a group.
24. Explain, in terms of atomic structure, why cesium is
more reactive than lithium. [1]
Cesium is more reactive than lithium because it has
lower ionization energy. Ionization Energy is a measure
of metal reactivity. Less energy is required to remove
an electron from cesium than lithium.
Electron Configuration and the Periodic Table
______________
Name
Honors Only
1.
2.
Bohr’s model of the atom was able to accurately
explain:the energy for spectral lines for each atom
a. Why spectral lines appear when atoms are
heated.
b. The energies of the spectral lines for each
element.Best answer of the two
c. Why electrons travel in circular orbits around
the nucleus.False, this is not true
d. all of the above answers is correct.If c is
false, d is false
Which of the following is true of the distance of an
electron from the nucleus of a 1H atom?Heisenberg’s
Uncertainty Principle states that you can either know
the location or the energy of an electron, we know the
energy.
a. It is 1 amu.
b. It remains constant over time.
c. Its distance at any given time can only be
predicted by looking at a“wave function”.
d. It is impossible to say where an electron will
be at any given time.
3.
The magnetic quantum number of an orbital defines:
m, defines the orientation of the orbital
a. The energy level of the orbitaln
b. The shape of the orbitall
c. The spatial orientation of the orbital
d. The spin of the electrons in the orbitals
4.
For which of the following atoms does the electron in
the outermost occupied orbital have thequantum
numbers n = 3 and l = 1?3p
a. N 2p
b. S3p
c. Mg 3s
d. Cs 6s
e. Ge4p
5.
Which of the following atoms has a half-filled p-orbital
in its ground state?
a. B p1
b. C p2
c. Pp3
d. Sp4
e. Tep4
6.
Which of the following orbitals cannot exist?
Calculate the l values for each n value below
a. 3dfor n = 3, l = 2,1,0 (s, p, d)
b. 4f for n = 4, l = 3,2,1,0 (s, p, d, f)
c. 2s for n = 2, l = 0 (s)
d. 5d for n = 5, l = 4,3,2,1,0 (s, p, d, f, g)
e. 2dfor n = 2, l = 1,0 (s, p)
7.
One of the outermost electrons in aArgon atom in the
ground state can be described by which of the
following sets of four quantum numbers?
3p6, n = 3, l = 1
a. 3, 0, 0, -½
b. 3, 1, -1, -½
c. 2, 1, 0, ½
d. 3, 0, 1, -½
e. 2, 1, -1, ½
8.
Which of the following sets of quantum numbers (n, l,
ml, ms) are disallowed for an electron inan atom?
n values must be whole numbers, l must be n-1, m values
are –l through +l, and spin values are either – ½ or + ½
a. 4, 2, 0, ½
b. 3, 3, -3, -½
Three answers – oops!
c. 2, 0, +1, ½
d. 4, 3, 0, ½
e. 3, 2, -2, -1
9.
In which of the following groups are all the species
isoelectronic?Same number of electrons
a. Mg+, Na, Ne
11, 11, 10
b. Br-, Rb+, Sr2+
36, 36, 36
v
c. K, Ca+, Cl19, 19, 18
d. Be2+, He, Li+2+
2, 2, 1
e. Ba2+, Rn, I54, 86, 54
10. One of the outermost electrons in a strontium atomin
the ground state can be described by which of the
following sets of four quantum numbers? (2 points)
Sr has 2 valence electrons in 5s2
a. 5, 2, 0, ½
5d3
b. 5, 1, 1, ½
5p3
c. 5, 1, 0, ½
5p2
d. 5, 0, 1, ½
Doesn’t exist
e. 5, 0, 0, ½
5s1
Electron Configuration and the Periodic Table
______________
Name
For each of the following questions show all work where necessary and use complete sentences in your explanations.
11. Give the four quantum numbers which describe the circled electrons (n,l,ml,ms) [2 each]
a.
K
↑
4s
↑n = 4, l = 0, m = 0, s = + ½
4p
b.
U
↑↓
7s
↑
↑
↑ ↑
5f
n = 5, l = 3, m = -2, s = + ½
12. A certain violet light has a wavelength of 413 nm. What is the frequency of the light? What is the energy of the light? [2]
c=ν ν=c/
c= 3.0x108 m/s
= 413 nm = 413x10-9m
c = 3.0 x 108 m/s = 7.26 x 1014 s-1
413 x 10-9m
E=hν
E=?
h= 6.626x10-34 Js
ν= 7.26 x 1014 s-1
E = (6.626 x 10-34Js)(7.2 x 1014 s-1) = 4.81 x 10-19 J
13. If an electron transitions from n=5 to n=2, how much energy does the photon released carry? [2]
DUPLICATE FROM PROBLEMS WORKED IN CLASS – OOPS!!
According to the Bohr Model of Hydrogren a transition from n=5 to n=2 will release a photon with a
wavelength of 434nm. This can be found using your reference pages and can be used to calculate the
frequency or energy of a photon.
E=hc/
E=?
h= 6.626x10-34 Js
c= 3.0x108 m/s
= 434 nm = 434x10-9m
E = (6.626 x 10-34Js)(3.0 x 108 m/s) = 4.58 x 10-19 J
434 x 10-9 m
14. Using orbital notation and stability arguments explain why tin and lead form both +2 and +4 ions. [2]
Both tin and lead have the valence configuration s2p2 and have a relatively unstable configuration with a full s subshell and a
partially filled p subshell. When the two atoms form the +2 ion they lose the 2 p electrons leaving the ion with a more stable
configuration (full s subshell) than the atom. The atoms then lose the remaining 2 s valence electrons when they form the
+4 ion and have a full energy level. This configuration is the most stable.
15. Explain the why the anomalies between group 15 and group 16 become less pronounced as you go down the periodic table. [2]
The difference between the orbitals is less pronounced as you increase the atomic radius of the atoms in group 15 and 16 so
the energy difference between the two configurations decreases.
Electron Configuration and the Periodic Table
______________
Name
16. Of the four trends which trend is best to predict metallic and non-metallic reactivity? Why? [2]
Ionization energy predicts metallic reactivity because it describes the loss of electrons.
Electron affinity predicts non-metallic reactivity because it describes the gaining of electrons.
17. Silver (Ag) is an exception in nomenclature because as a transition metal, it only forms one cation, Ag +1. Using orbital
notation and stability arguments, explain why silver doesn’t want to form Ag +2 as well. [2]
Silver does not want to form Ag+2 because its configuration is [Kr] 5s14d10, when it loses the first electron it has a full
energy level.