CHM113 Chapter 7 MasteringChemistry Homework

Part A
Arrange the following atoms in order of increasing effective nuclear charge experienced by the electrons in the n=3 electron shell: K, Mg, P, Rh, and Ti.
Rank from smallest to largest. To rank items as equivalent, overlap them.

Mg, P, K, Ti, Rh

Part A
Which will experience the greater effective nuclear charge, the electrons in the n=3 shell in Ar or the n=3 shell in Kr?

electrons in the n=3 shell in Kr

Part B
Which will be closer to the nucleus?
– electrons in the n=3 shell in Ar
– electrons in the n=3 shell in Kr

electrons in the n=3 shell in Kr

Part A
Rank the following ions in order of decreasing radius: F−,Cl−,Br−,I−, and At−. Use the periodic table as necessary.
Rank from largest to smallest radius. To rank items as equivalent, overlap them.

At-, I-, Br-, Cl-, F-

Part B
Rank the following items in order of decreasing radius: Na, Na+, and Na−.
Rank from largest to smallest radius. To rank items as equivalent, overlap them.

Na-, Na, Na+

Part C
The following ions contain the same number of electrons. Rank them in order of decreasing ionic radii.
Rank from largest to smallest radius. To rank items as equivalent, overlap them.

Sb3-, Te2-, I-, Cs+. Ba2+, La3+

Part A
I−>I>I+
Match the words in the left column to the appropriate blanks in the sentences on the right.

1. Increase(s) 2. Smaller

Part B
Ca2+>Mg2+>Be2+
Match the words in the left column to the appropriate blanks in the sentences on the right.

1. increase, increase

Part C
Fe>Fe2+>Fe3+
Match the words in the left column to the appropriate blanks in the sentences on the right.

1. farther 2. one orbital 3. reduces

Part A – Predicting Relative Sizes of Atomic Radii
By referring to a periodic table , but not to Figure 7.7, place the following atoms in order of increasing bonding atomic radius: N, O, P, Ge.

O < N < P < Ge

Part A – Bond Lengths in a Molecule
Hypothetical elements X and Y form a molecule XY2, in which both Y atoms are bonded to atom X (and not to one another). The X-X distance in the elemental form of X is 2.04 Å and the Y-Y distance in elemental Y is 1.68 Å. What would you predict for the X-Y distance in the XY2 molecule?

1.86 Å

Part A
For the following set of atoms and ions, arrange the members in order of decreasing size:
Rank items from largest to smallest. To rank items as equivalent, overlap them.

Te2-, Se2-, Se

Part B
For the following set of atoms and ions, arrange the members in order of decreasing size:
Rank items from largest to smallest. To rank items as equivalent, overlap them.

Fe2+, Fe3+, Co3+

Part C
For the following set of atoms and ions, arrange the members in order of decreasing size:
Rank items from largest to smallest. To rank items as equivalent, overlap them.

Ca, Sc3+, Ti4+

Part D
For the following set of atoms and ions, arrange the members in order of decreasing size:
Rank items from largest to smallest. To rank items as equivalent, overlap them.

Cl-, K+, Ca2+

Part A
In terms of d1 and d2, how could you define the bonding atomic radius of atom A?
Express your answer in terms of the variables d1 and d2.

rA = 1/2d1

Part B
In terms of d1 and d2, how could you define the bonding atomic radius of atom X?
Express your answer in terms of the variables d1 and d2.

rX = d2−(d1/2)

Part C
In terms of d1 and d2, what would you predict for the X−X bond length of an X2 molecule?
Express your answer in terms of the variables d1 and d2.

rX−X = 2d2−d1

Part A
What is the ground-state electron configuration of a neutral atom of iron?
Express your answer in condensed form, in order of increasing orbital energy. For example, [He]2s22p2 would be entered as [He]2s^22p^2 .

[Ar]3d^64s^2

Part B
What is the ground-state electron configuration of the oxide ion O2−?
Express your answer in condensed form, in order of increasing orbital energy. For example, [He]2s22p2 should be entered as [He]2s^22p^2 .

[He]2s^22p^6

Part C
Which element has the following configuration: [Xe]6s24f4?
Enter the chemical symbol for the element.

Nd

Part A – Periodic Trends in Ionization Energy
Consider the following statements about first ionization energies:
I. Because the effective nuclear charge for Mg is greater than that for Be, the first ionization energy of Mg is greater than that of Be.
II. The first ionization energy of O is less than that of N because in O we must pair electrons in the 2p orbitals.
III. The first ionization energy of Ar is less than that of Ne because a 3p electron in Ar is farther from the nucleus than a 2p electron in Ne.
Which of the statements I, II, and III is or are true?

Statements II and III are true

Part A – Trends in Ionization Energy
The third ionization energy of bromine is the energy required for which of the following processes?

Br2+(g) → Br3+(g) + e−

Part A
Co2+
Use the buttons at the top of the tool to add orbitals in order of increasing energy, starting at the bottom with the lowest energy orbitals. Click within an orbital to add electrons.

3d -||- -||- -|- -|- 3p -||- -||- -||- 3s -||- 2p -||- -||- -||- 2s -||- 1s -||- [Ar]3d^7

Part B
Sn2+
Use the buttons at the top of the tool to add orbitals in order of increasing energy, starting at the bottom with the lowest energy orbitals. Click within an orbital to add electrons.

4d -||- -||- -||- -||- -||- 5s -||- 4p -||- -||- -||- 3d -||- -||- -||- -||- -||- 4s -||- 3p -||- -||- -||- 3s -||- 2p -||- -||- -||- 2s -||- 1s -||- [Kr]5s^2 4d^10

Part C
Zr4+
Use the buttons at the top of the tool to add orbitals in order of increasing energy, starting at the bottom with the lowest energy orbitals. Click within an orbital to add electrons.

4p -||- -||- -||- 3d -||- -||- -||- -||- -||- 4s -||- 3p -||- -||- -||- 3s -||- 2p -||- -||- -||- 2s -||- 1s -||- [Ar]3d^10 4s^2 4p^6

Part D
Ag+
Use the buttons at the top of the tool to add orbitals in order of increasing energy, starting at the bottom with the lowest energy orbitals. Click within an orbital to add electrons.

4d -||- -||- -||- -||- -||- 4p -||- -||- -||- 3d -||- -||- -||- -||- -||- 4s -||- 3p -||- -||- -||- 3s -||- 2p -||- -||- -||- 2s -||- 1s -||- [Kr]4d^10

Part E
S2−
Use the buttons at the top of the tool to add orbitals in order of increasing energy, starting at the bottom with the lowest energy orbitals. Click within an orbital to add electrons.

3p -||- -||- -||- 3s -||- 2p -||- -||- -||- 2s -||- 1s -||- [Ne]3s^2 3p^6

Part F
Determine which ions have noble-gas configurations.
Check all that apply.

Zr4+ S2−

Part A
Select the atoms whose ions have an electron configuration of nd6 (n = 3, 4, 5 …). For example, the 2+ ion for V ends the electron configuration with 3d 3.
Check all that apply.

Co Pt Ru

Part A
What is the relationship between the ionization energy of an anion with a -1 charge, such as F−, and the electron affinity of the neutral atom, F?
Express your answer in terms of EF, which represents the electron affinity of the neutral atom, F.

I1F− = −EF

Part A
In the group 3 to group 12 elements, which subshell is filled up going across the rows?

d subshell

Part B
A sample of soil from a newly discovered cave is analyzed by a team of explorers. They find an element that is a good conductor of electricity. It also forms a chloride in the form XCl2 and an oxide in the form XO. The element is a liquid at room temperature. What is the identity of this element?
Express your answer using a chemical symbol.

Hg

Part A
Arrange the following oxides in order of increasing acidity.
Rank from least acidic to most acidic. To rank items as equivalent, overlap them.

CaO, Al2O3, SiO2, CO2, P2O5, SO3

Part A
barium oxide with water
Express your answer as a chemical equation. Identify all of the phases in your answer.

BaO(s)+H2O(l)→Ba(OH)2(aq)

Part B
sulfur trioxide with water
Express your answer as a chemical equation. Identify all of the phases in your answer.

SO3(g)+H2O(l)→H2SO4(aq)

Part A
Predict the products of the following reaction:

MgCl2+K⇌
The equation may not be correctly balanced.
Express your answer as a chemical formula. If no reaction occurs, enter noreaction.

MgCl2+K⇌ KCl+Mg