The ionic salt Na2Cl doesn\'t exist. Which of the following statements best expl

Question

The ionic salt Na2Cl doesn't exist. Which of the following statements best explains why?

A. Because Na2 has no charge and therefore would not be attracted electrostatically to the negatively charged Cl- anion.
B. Because the Na+ ion is too large for there to be two of them attached to one Cl- ion.
C. Because chlorine atoms have a relatively high electron affinity, but only for the addition of one electron. Adding two electrons would mean that the 2nd electron must enter the next higher shell at a much higher energy. An anion such as Cl2- is not stable.
D. Because Na2Cl would actually be a polyatomic cation with a +1 charge. It would not be an ionic salt unless another Cl- anion was available, and then it would be properly given as Na2Cl2.


Question 2 of 15
Select the false statement below.

A. The following process is an exothermic process and represents the first ionization energy of an atom A:
A(g) ? A1+(g) + e1-

B. Oxygen has a greater first ionization energy than selenium, and the reason for this is because oxygen has a lesser amount of shielding of outer electrons by inner electrons than does selenium.
C. The first ionization energy of an atom is smaller than the second ionization energy of the same atom.
D. Oxygen has a greater first ionization energy than boron, and the reason for this is because O has a greater effective nuclear charge (Zeff) than B.


Question 3 of 15
Elements with relatively high (highly negative) electron affinities tend to form anions when participating in ionic compound formation.

True
False

Question 4 of 15
A chlorine atom is larger than a silicon atom, and an aluminum atom is larger than a sodium atom.

True
False

Question 5 of 15
A certain main-group element exhibits the following successive ionization energies in kJ/mol:

IE1 = 100; IE2 = 300; IE3 = 700; IE4 = 3100; IE5 = 4200

Select the false statement about this element below.

A. This element has four valence electrons.
B. This element likely ionizes to form a cation when participating in ionic compound formation.
C. The highest-energy electron in an atom of this element resides in a p orbital.
D. This element is likely a metallic element.

Question 6 of 15
Select the false statement below.

A. Generally speaking, the heavier alkaline earth metals can be predicted to exhibit greater shielding of the outer-shell electrons by the inner-shell electrons than lighter alkaline earth metals.
B. Generally speaking, non-metallic elements have greater effective nuclear charge (Zeff) than metallic elements in the same period.
C. Generally speaking, as you go down a group in the periodic table, there is successively less shielding of the outer-shell electrons by the inner-shell electrons.
D. Generally speaking, as you go across a period in the periodic table, the effective nuclear charge (Zeff) increases 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.

Question 7 of 15
Place the following in order of increasing size:

P3-, Cl1-, O2-

A. O2- < P3- < Cl1-
B. P3- < Cl1- < O2-
C. Cl1- < P3- < O2-
D. O2- < Cl1- < P3-

Question 8 of 15
Select the false statement below.

A. The n = 3 shell can accomodate up to 18 electrons in any given atom.
B. There are 3 subshells and 9 orbitals in the n = 3 shell of any given atom.
C. There are 3 electrons with positive spins in any filled p subshell of any given atom.
D. There are only 2 electrons that can have the following quantum numbers in any given atom:
n = 3, l = 1


Question 9 of 15
Select the less metallic element from each pair of elements: K or Ca; Na or Cs; Sn or Sb.

A. Ca; Cs; Sb
B. K; Na; Sn
C. K; Cs; Sn
D. Ca; Na; Sb

Question 10 of 15
Select the false statement below.

A. The copper(I) ion is more paramagnetic than the copper(II) ion.
B. The Sc1+ ion is paramagnetic.
C. The O2-, Mg2+, and Al3+ ions are isoelectronic ions.
D. The Zn2+ ion and the Zn atom both have filled 3d subshells.

Question 11 of 15
Select the false statement below concerning period 4 transition elements.

A. Both the chromium atom and the manganese atom have half-filled d subshells.
B. The zinc atom has 28 inner/core electrons and 2 outer/valence electrons.
C. The vanadium atom has fewer unpaired electrons than the nickel atom.
D. The titanium atom is more paramagnetic than the zinc atom.

Question 12 of 15
Consider the potassium atom and select the false statement below.

A. The potassium atom has 18 inner/core electrons and 1 valence electron.
B. The potassium atom has a filled outer s subshell.
C. The condensed electron configuration of the potassium atom is [Ar]4s1.
D. The potassium atom is paramagnetic.

Question 13 of 15
The photon emitted or absorbed during an electronic transition between n = 2 and n = 4 in a hydrogen atom has a wavelength in the visible portion of the electromagnetic spectrum and an energy that is greater than a similar electronic transition between n = 3 and n = 5 in a hydrogen atom.

True
False

Question 14 of 15
Consider the electronic transition from n = 5 to n = 3 in a hydrogen atom, and select the correct statement from below.

A. A photon of 684 nm wavelength and 2.91x10-19 J energy was emitted from the hydrogen atom during this electronic transition.
B. A photon of 1282 nm wavelength and 1.55x10-19 J energy was emitted from the hydrogen atom during this electronic transition.
C. A photon of 1282 nm wavelength and 1.55x10-19 J energy was absorbed by the hydrogen atom during this electronic transition.
D. A photon of 684 nm wavelength and 2.91x10-19 J energy was absorbed by the hydrogen atom during this electronic transition.

Question 15 of 15
Which of the following statements is false?

A. NaO is more basic in aqueous solution than Al2O3
B. Si has a higher first ionization energy than Al
C. Al exhibits more metallic behavior than Na
D. Si has a greater (more negative) first electron affinity than Al

Explanation / Answer

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