CHEM QUIZ
How many elements cannot have a noble gas configuration?
Question 1 options:
0
1
2
3
Question 2 (1 point)
Which of these describes sheilding?
Question 2 options:
core electrons shield valence electrons from the positive charge of the nucleus so that the valence electrons experience a charge less than the total nuclear charge.
core electrons shield valence electrons from the nucleus, but the valence electrons experience the total nuclear charge.
valence electrons shield core electrons from the positive charge of the nucleus so that the core electrons experience a charge less than the total nuclear charge.
valence electrons shield core electrons from the nucleus, but the valence electrons experience the total nuclear charge.
Question 3 (1 point)
The properties of an element are determined by (choose the best answer).
Question 3 options:
number of neutrons
number of protons
number of electrons
its valence electron configuration
number of valence electrons
Question 4 (1 point)
For increasing metallic character, make two arrows pointing toward _________on the periodic table
Question 4 options:
Fr
F
Question 5 (1 point)
When determining the electron configuration for an ion, which of these electrons should always be removed first?
Question 5 options:
the last electrons you listed
the highest energy electrons
electrons in the outermost (valence) shell -with the highest n value
Question 6 (1 point)
Which of these has the highest first ionization energy?
Question 6 options:
B
N
O
F
C
He
Question 7 (1 point)
When writing the noble gas configuration for Gd (#64) which noble gas do you use?
Question 7 options:
Og
Xe
Kr
He
Ne
Rn
Ar
Question 8 (1 point)
When writing the noble gas configuration for Aluminum, which noble gas do you use?
Question 8 options:
He
Ar
Xe
Kr
Rn
Ne
Og
Question 9 (1 point)
According to Coulomb’s law, the attraction between a proton and an electron in an atom ____________with increasing_____________
Question 9 options:
decreases; their sizes
increases; distance between their centers
decreases; their charges
decreases; distance between their centers
decreases; their sizes
Question 10 (1 point)
Each element has multiple ionization energies. The first ionization energy is the energy required to pull off one electron. The second ionization energy is the energy required to remove one more electron after that, and so on. If you look at a list of ionization energies, for any element, you find a big jump______________________
Question 10 options:
between the first and second ionization
the ionization energy after the resulting ion has a noble gas configuration because a noble gas configuration is already stable
between the second and third ionization
Question 11 (1 point)
What is the electron configuration for bromide ion?
Question 11 options:
[Ar]4s23d104p6
[Ar]4s23d104p7
[Kr]
[Ar]
Question 12 (1 point)
Which of these decreases in magnitude as you go across a period on the periodic table?
Question 12 options:
Zeff
ionization energy
electron affinity
atomic radius
electronegativity
Question 13 (1 point)
Which of these statement describes one of the exceptions to the ionization energy trend?
Question 13 options:
column 2A has a lower ionization energy than column 3A because s electrons are farther from the nucleus, and therefore harder to remove than p electrons.
column 2A has a lower ionization energy than column 3A because s electrons are closer to the nucleus, and therefore harder to remove than p electrons.
column 2A has a higher ionization energy than column 3A because s electrons are farther from the nucleus, and therefore harder to remove than p electrons.
column 2A has a higher ionization energy than column 3A because s electrons are closer to the nucleus, and therefore harder to remove than p electrons.
Question 14 (1 point)
The driving force for elements form ions (whether positive or negative) is
Question 14 options:
to obtain a noble gas configuration
to become charged instead of neutral
To release energy
Question 15 (1 point)
Valence electrons are always all except
Question 15 options:
electrons in the outermost shell
electrons of the highest energy
s electrons in the shell with the highest number n
p electrons in the shell with the highest number n
Question 16 (1 point)
Which of these is not isoelectronic with the others?
Question 16 options:
Cl-
Na+
S2-
Ar
Br-
Mg2+
Question 17 (1 point)
Calculate Zeff for a lithium ion. You may want to draw one so that you can identify the core electrons and the valence electrons.
Question 17 options:
+3
+2
0
-1
+4
+1
Question 18 (1 point)
Which of these describes penetration?
Question 18 options:
The wavefunction of an electron from a higher energy orbital overlaps the wavefunction of a lower energy orbital.
The wavefunction of an electron from a lower energy orbital overlaps the wavefunction of a higher energy orbital.
Electrons attract each other such that valence electrons are closer to the nucleus.
Electrons repel each other such that val