Honors Chemistry
Chapter 7-8 Take-home Quiz
Name ____________________________________
Period _____ Date ____________
1)_____ Place the following types of electromagnetic radiation in order of decreasing energy.
ultraviolet light
radio waves
microwaves
A) radio waves > microwaves > ultraviolet light
B) ultraviolet light > microwaves > radio waves
C) radio waves > ultraviolet light > microwaves
D) ultraviolet light > radio waves > microwaves
E) microwaves > radio waves > ultraviolet light
2)_____ How many photons are contained in a burst of yellow light (589 nm) from a sodium
lamp that contains 609 kJ of energy?
A) 3.37 × 1019 photons
D) 4.03 × 1028 photons
30
B) 3.06 × 10 photons
E) 2.48 × 1025 photons
C) 1.80 × 1024 photons
3)_____ Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106
m/s.
A) 1.99 × 10-10 m
D) 5.52 × 10-9 m
-10
B) 5.03 × 10
m
E) 2.76 × 10-9 m
C) 1.81 × 10-10 m
4)_____ Choose the transition (in a hydrogen atom) below that represents the absorption of
the shortest wavelength photon.
A) n = 1 to n = 2
D) n = 6 to n = 3
B) n = 2 to n = 3
E) n = 3 to n = 1
C) n = 4 to n = 5
5)_____ What are the possible orbitals for n = 3?
A) s, p, d
B) s, p, d, f
C) s
D) s, p
E) p, d, f
6)_____ Which of the following statements is TRUE?
A) We can sometimes know the exact location and speed of an electron at the same
time.
B) All orbitals in a given atom are roughly the same size.
C) Since electrons have mass, we must always consider them to have particle
properties and never wavelike properties.
D) Atoms are roughly spherical because when all of the different shaped orbitals are
overlapped, they take on a spherical shape.
E) All of the above are true.
7)______ No two electrons can have the same four quantum numbers is known as the
a. Pauli exclusion principle
c. Aufbau principle
b. Hund's rule
d. Heisenberg uncertainty principle
8)______ Only two electrons, with opposing spins, are allowed in each orbital is known as the
a. Pauli exclusion principle
c. Aufbau principle
b. Hund's rule
d. Heisenberg uncertainty principle
9)______ When filling degenerate orbitals, electrons fill them singly first, with parallel spins is
known as
a. Pauli exclusion principle
b. Hund's rule
c. Aufbau principle
d. Heisenberg uncertainty principle
10)______ Choose the orbital diagram that represents the ground state of N.
A)
C)
B)
D)
E)
11)______ Give the set of four quantum numbers that could represent the last electron added
(using the Aufbau principle) to the Cl atom.
1
2
1
b. n = 3, l = 0, ml = 1, ms = 2
1
c. n = 3, l = 2, ml =1 , ms = +
2
a.
n = 3, l = 1, ml = 1, ms = +
1
2
1
e. n = 3, l =2 , ml = 1, ms = 2
d. n = 2, l = 1, ml = 1, ms = -
12)______ Which of the following statements is TRUE?
A) An orbital that penetrates into the region occupied by core electrons is less shielded
from nuclear charge than an orbital that does not penetrate and therefore has a lower
energy.
B) An orbital that penetrates into the region occupied by core electrons is more shielded
from nuclear charge than an orbital that does not penetrate and therefore has a lower
energy.
C) It is possible for two electrons in the same atom to have identical values for all four
quantum numbers.
D) Two electrons in the same orbital can have the same spin.
E) None of the above are true.
13)______ Give the number of core electrons for O.
A) 0
B) 1
C) 2
D) 3
E) 4
14)______ How many valence electrons do the alkali earth metals possess?
A) 1
D) 6
B) 2
E) 8
C) 7
15)______ The complete electron configuration of gallium, element 31, is __________.
A) 1s22s22p103s21s22s22p103s2 3p104s23d3
B) 1s22s22p63s23p63d104s24p1
C) 1s42s42p63s43p64s43d3
D) 1s42s42p103s43p9
E) 1s42s42p83s43p84s3
16)______ The condensed electron configuration of silicon, element 14, is __________.
A) [He]2s42p6
D) [He]2s4
B) [Ne]2p10
E) [He]2s62p2
2
2
C) [Ne]3s 3p
17)______ What is the general valence-electron ground-state electron configuration for neutral
alkaline earth metals?
A) ns1
C) 1s22s1
B) ns2
D) 1s22s2
18)______ Place the following elements in order of increasing atomic radius.
P Ba Cl
A) Ba < P < Cl
D) Cl < Ba < P
B) P < Cl < Ba
E) Ba < Cl < P
C) Cl < P < Ba
19)______ What period 3 element having the following ionization energies (all in kJ/mol)?
IE1 = 1012IE2 = 1900
IE3= 2910
IE4= 4960
IE5= 6270
IE6 = 22,200
A) Si
D) Cl
B) S
E) Mg
C) P
20)______ Choose the paramagnetic species from below.
a. Ca
d. Zn
2+
3+
b. O
e. Nb
2+
c. Cd
21)______ Which ionization process requires the most energy?
a. W(g) → W+(g) + ec. W2+(g) → W 3+(g) + eb. W+(g) → W 2+(g) + ed. W3+(g) → W 4+(g) + e-
22)______
Calculate the energy change associated with the transition from n=4 to n=1 in the
hydrogen atom.
23)______
Determine the end (final) value of n in a hydrogen atom transition, if the electron
starts in n = 4 and the atom emits a photon of light with a wavelength of 486 nm.
24)______
Why does the size of the transition elements stay roughly the same as you move
across a period?
25)______
Define paramagnetic.
26)______
Below is a list of successive ionization energies (in kJ/mol) for a period 3
element. Identify the element and explain how you came to that conclusion.
IE2 = 2250
IE3 = 3360 IE4= 4560 IE5= 7010 IE6= 8500
IE7 = 27,100
27)______
Why is the first ionization energy of sulfur smaller than the first ionization energy
of phosphorus?
28)______
Define electron affinity.