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 valence electrons are farther from the nucleus.
Question 19 (3 points)
Arrange these from biggest to smallest
Question 19 options:123noble gas123cation123anion
Question 20 (1 point)
Which of these statements describes one of the exceptions to the ionization energy trend? 
Question 20 options:
group 5A has a lower ionization energy than group 6A because group 5A has a half-filled p subshell, which is aless stable confirmation than group 6A, in  which the p subshell is neither half full nor completely full.
group 5A has a higher ionization energy than group 6A because group 5A has a half-filled p subshell, which is aless stable confirmation than group 6A, in which which the p subshell is neither half full nor completely full.
group 5A has a higher ionization energy than group 6A because group 5A has a half-filled p subshell, which is a more stable confirmation than group 6A, in which the p subshell is neither half full nor completely full.
group 5A has a lower ionization energy than group 6A because group 5A has a half-filled p subshell, which is a more stable confirmation than group 6A, in which the p subshell is neither half full nor completely full.
Question 21 (1 point)
The ionization energy__________________
Question 21 options:
is the energy it takes to remove an electron from an atom and is a positive number
is the energy it takes to add an electron to an atom and is a negative number.
is the energy it takes to add an electron to an atom and is a positive number.
is the energy it takes to remove an electron from an atom and is a negative number.
Question 22 (1 point)
Which element has the electron configuration
1s22s22p63s23p64s23d103p65s24d105p66s24f145d106p67s25f146d7
Question 22 options:
Ds #110
Ra #88
Tr #77
Hs #108
Mt #109
Question 23 (1 point)
What is the electron configuration of carbon?
Question 23 options:
1s22s12p3
1s22s4
1s22s22p2
1s22p4
Question 24 (1 point)
When writing the noble gas configuration for Ts (#117), which noble gas do you use?
Question 24 options:
Og
Xe
Ne
Kr
Rn
He
Ar
Question 25 (3 points)
Match the families to the blocks on the periodic table.
Question 25 options:1234
inner transition metals
1234
lanthanides
1234
alkaline earth metals
1234
alkali metals
1234
nonmetals
1234
halogens
1234
transition metals
1234
semimetals
1234
noble gases
1234
actinides
1.
s-block
2.
p-block
3.
d-block
4.
f-block
Question 26 (1 point)
The noble gas configuration for Aluminum ion is ?
Question 26 options:
Kr
Ar
Ne
Og
Rn
He
Xe
Question 27 (1 point)
When writing electron box diagrams, which of these is false?
Question 27 options:
Electrons in the same subshell can have parallel spins
Electrons in the same orbital can have parallel spins
Question 28 (1 point)
The electron affinity__________________
Question 28 options:
is the energy it takes to remove an electron from an atom and is a positive number
is the energy it takes to add an electron to an atom and is a positive number.
is the energy it takes to add an electron to an atom and is a negative number.
is the energy it takes to remove an electron from an atom and is a negative number.
Question 29 (1 point)
Atomic radii are determined by
Question 29 options:
the number of valence electrons; they repel each other and increase the ionic radius.
the electronegativity; more electronegative atoms attract more electrons and therefore are greater in size.
Zeff: the higher nuclear charge pulls the electrons closer to the nucleus to decrease the size of the atom.
Question 30 (1 point)
Which of these is not isoelectronic with the others?
Question 30 options:
Na+
S2-
Mg2+
Ar
Cr2+
Question 31 (1 point)
What is the electron configuration for Calcium ION?
Question 31 options:
[Ar]4s1
[Ar]
[Ar]4s23d2
[Ar]4s2
Question 32 (1 point)
What is the electron configuration for Fe2+ ion?
Question 32 options:
 [Ar]4s23d4
[Ar] 3d6
[Ar]
[Ar]3d10
[Ar]4s23d6
Question 33 (1 point)
Electronegativity is 
Question 33 options:
the ability to donate electrons to another atom
the ability to donate protons to another atom
the ability to attract protons to oneself
the ability to attract electrons to oneself
Question 34 (1 point)
Which of these is diamagnetic?
Question 34 options:
Se
Si
Cl
Ar
Question 35 (1 point)
Which element has an electron configuration of 1s22s22p63s23p64s23d103p65s24d4 
Question 35 options:
W
Mo
Ba
Cr
Sr
Question 36 (1 point)
Which of these have ions with noble-gas configurations?
Question 36 options:
actinides
main group elements
lanthanides
transition metals
Question 37 (1 point)
Zeff increases accross a period (for the main group elements) because
Question 37 options:
the nuclear charge decreases with the number of protons in the atoms, but the number of shielding electrons inreases.
the nuclear charge increases with the number of protons in the atoms, but the number of shielding electrons inreases.
the nuclear charge decreases with the atomic number, but the number of shielding electrons stays the same.
the nuclear charge increases with the atomic number, but the number of shielding electrons stays the same.
Question 38 (1 point)
Which is true about Zeff
Question 38 options:
it is the nuclear charge minus the total charge of the rest of the electrons in the atom  
it is the nuclear charge minus the total charge of the rest of the electrons that penetrate the nucleus of the atom
it is the nuclear charge minus the total charge of the electrons in lower energy shells 
it is the nuclear charge minus the total charge of the electrons in higher energy shells
Question 39 (1 point)
Using the trend for EA (not the exceptions), select the element that has the highest electron affinity)
Question 39 options:
F
N
O
Ar
Question 40 (1 point)
Which of these decreases in magnitude as you go right on the periodic table?
Question 40 options:
atomic radius
electronegativity
electron affinity
ionization energy

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