Question 1 of 15 (worth 2 points) The NaCl2 ionic salt does not exist. Which of

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Question 1 of 15 (worth 2 points)
The NaCl2 ionic salt does not exist. Which of the following statements best explains why?

A. Because the formation of Na2+ is an unfavorable process due to the great amount of energy required to remove the 2nd electron from the Na atom (the 2nd electron would have to be removed from the core electrons of the Na atom).
B. Because Cl2 has no charge and therefore would not be attracted electrostatically to the positively charged Na2+ cation.
C. Because NaCl2 is actually a polyatomic ion with a -1 charge, and not an ionic salt. In the presence of another Na+ ion, the Na2Cl2 salt would form.
D. Because the Cl- anion is too large for there to be two of them attached to one Na+ ion.
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Question 2 of 15 (worth 2 points)
Select the false statement below.

A. Fluorine has a greater first ionization energy than iodine, and the reason for this is because fluorine has a greater amount of shielding of outer electrons by inner electrons than does iodine.
B. The following process is an endothermic process and represents the first ionization energy of an atom A:
A(g) ? A1+(g) + e1-

C. Phosphorus has a greater first ionization energy than magnesium, and the reason for this is because P has a greater effective nuclear charge (Zeff) than Mg.
D. The first ionization energy of an atom is smaller than the second ionization energy of the same atom.
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Question 3 of 15 (worth 2 points)
The following process represents the first electron affinity of an atom A:

A(g) ? A1+(g) + e1-

True
False
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Question 4 of 15 (worth 2 points)
Generally speaking, most nonmetal atoms are smaller than most metal atoms.

True
False
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Question 5 of 15 (worth 2 points)
A certain main-group element exhibits the following successive ionization energies in kJ/mol:

IE1 = 100; IE2 = 1200; IE3 = 2300; IE4 = 3100; IE5 = 4200

Select the false statement about this element below.

A. If this element is given a symbol of "J", it would form an ionic compound with sulfur as J2S.
B. This element is typically found uncombined in nature (that is, it is not usually found in compounds, but rather as a free element).
C. This is likely a Group 1A element.
D. If this element was in period 2 of the periodic table, it would be lithium.
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Question 6 of 15 (worth 2 points)
Select the false statement below.

A. Generally speaking, as you go down a group in the periodic table, there is successively greater shielding of the outer-shell electrons by the inner-shell electrons.
B. Generally speaking, non-metallic elements have greater effective nuclear charge (Zeff) than metallic elements in the same period.
C. Generally speaking, the heavier alkali metals can be predicted to exhibit greater shielding of the outer-shell electrons by the inner-shell electrons than lighter alkali metals.
D. Generally speaking, as you go across a period in the periodic table, the effective nuclear charge (Zeff) decreases because each successive element contains more protons in the nucleus than the previous element and the outer electrons are all in the same shell as you go across a period.
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Question 7 of 15 (worth 2 points)
Place the following in order of increasing size:

O2-, F1-, Li1+

A. F1- < O2- < Li1+
B. F1- < Li1+ < O2-
C. Li1+ < O2- < F1-
D. Li1+ < F1- < O2-
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Question 8 of 15 (worth 2 points)
Select the false statement below.

A. The n = 4 shell of any given atom can accomodate up to 16 electrons.
B. In any given atom, the l = 2 subshell can accomodate up to 5 electrons that have negative spins (ms =

Explanation / Answer

B. Because Cl2 has no charge and therefore would not be attracted electrostatically to the positively charged Na2+ cation.

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