CHEM Exam 02 Practice Problems

[Xe] 6s²

Write the ground state electron configuration for barium using the Noble gas core abbreviation.

1s²2s²2p⁶3s²3p⁶4s²

Write the ground state electron configuration for calcium.

[Ar] 4s²3d⁶

Write the ground state electron configuration for iron using the Noble gas core abbreviation.

1s²2s¹

Write the ground state electron configuration for lithium.

[He] 2s²2p³

Write the ground state electron configuration for nitrogen using the Noble gas core abbreviation.

Zinc

Give the name of the element whose +2 ion has the same number of electrons as Cu⁺.

Vanadium

Give the name of the element whose +3 ion has the same number of electrons as Ti²⁺.

Hydrogen

Give the name of the element whose -1 ion is isoelectronic with He.

Bromine

Give the name of the element whose -1 ion is isoelectronic with Kr.

Oxygen

Give the name of the element whose -2 ion has the same number of 2p electrons as Na⁺.

Sulfur

Give the name of the element whose -2 ion is isoelectronic with Ar.

Tellurium

Give the name of the element whose -2 ion is isoelectronic with Xe.

Nitrogen

Give the name of the element whose -3 ion has the same number of electrons as O²⁻.

B D A C

Given the following valence orbital diagrams, rank these elements in order of increasing atomic size. A: ↑↓ ↑ ↑_ 3s 3p B: ↑↓ ↑↓ ↑↓ ↑ 2s 2p C: ↑↓ _ _ _ 5s 5p D: ↑↓ ↑↓ ↑ ↑ 3s 3p

C A D B

Given the following valence orbital diagrams, rank these elements in order of increasing ionization energy. A: ↑↓ ↑ ↑_ 3s 3p B: ↑↓ ↑↓ ↑↓ ↑ 2s 2p C: ↑↓ _ _ _ 5s 5p D: ↑↓ ↑↓ ↑ ↑ 3s 3p

6

How many electrons can occupy 3 p orbitals?

10

How many electrons can occupy 5 d orbitals?

14

How many electrons can occupy 7 f orbitals?

2

How many electrons can occupy one s orbital?

0.125/0.0625 = 2.00

Hydrogen and oxygen form both water and hydrogen peroxide. The decomposition of a sample of water forms 0.125 g hydrogen to every 1.00 g oxygen. The decomposition of a sample of hydrogen peroxide forms 0.0625 g hydrogen to every 1.00 g oxygen. Show that these results are consistent with the law of multiple proportions.

Cr(PO₄)₂

Write the formula for the following compound: Chromium (VI) phosphate

Co₂O₃

Write the formula for the following compound: Cobalt (III) oxide

Pb₃N₂

Write the formula for the following compound: Lead (II) nitride

LiI

Write the formula for the following compound: Lithium iodide

AgBr

Write the formula for the following compound: Silver bromide

Sn(NO₂)₂

Write the formula for the following compound: Tin (II) Nitrite

C₂Br₄

Write the formulas of the following covalent compound: Dicarbon Tetrabromide

N₂O₃

Write the formulas of the following covalent compound: Dinitrogen Trioxide

SO

Write the formulas of the following covalent compound: Sulfur Monoxide

TeCl₄

Write the formulas of the following covalent compound: Tellurium Tetrachloride

S₄N₂

Write the formulas of the following covalent compound: Tetrasulfur Dinitride

4, 3, 2

A hydrogen atom orbital has n = 5 and ml = -2. What are the possible values of l for this orbital?

1/2, -1/2

A hydrogen atom orbital has n = 5 and ml = -2. What are the possible values of m-sub-l for this orbital?

Cl⁻ P³⁻ Cs⁺ I⁻

Arrange the following in order of increasing ionic radius. P³⁻, Cl⁻, Cs⁺, and I⁻

NaF MgO AlN

Arrange the compounds NaF, MgO, and AlN in order of increasing lattice energy.

Cs K B S

Arrange the elements B, S, Cs, K in order of increasing EA₁.

Sr Cr Ag Br

Arrange the elements Cr, Sr, Br, Ag in order of increasing EA₂.

Si Cu Ca Fr

Arrange the elements Cu, Si, Fr, Ca in order of increasing atomic radius.

Rb Mg P Cl

Arrange the elements Mg, Cl, P, Rb in order of increasing IE₁.

Cs, Na, Al, S, Cl

Arrange the following elements in order of increasing first ionization energy: Na, Cl, Al, S, and Cs.

K⁺ S²⁻ Rb⁺ As³⁻

Arrange the following in order of increasing ionic radius. Rb⁺, As³⁻, K⁺, and S²⁻

Mg²⁺ Na⁺ F⁻ N³⁻

Arrange the following in order of increasing ionic radius. N³⁻, Mg²⁺, F⁻, and Na⁺

Sr²⁺ Br⁻ Ba²⁺ Te²⁻

Arrange the following in order of increasing ionic radius. Te²⁻, Br⁻, Ba²⁺, Sr²⁺

5.252 x 10³

Enter your answer in scientific notation. A hydrogen-like ion is an ion containing only one electron. The energies of the electron in a hydrogen-like ion are given by En = −(2.18 × 10−¹⁸J) Z² (1/n²) where n is the principal quantum number and Z is the atomic number of the element. Calculate the ionization energy (in kJ/mol) of the He+ ion.

1

For a p-shaped Hydrogen orbital where the principle quantum number = 3, what is the angular quantum number?

1

For a p-shaped Hydrogen orbital where the principle quantum number = 4, what is the angular quantum number?

0

For an s-shaped Hydrogen orbital where the principle quantum number = 3, what is the angular quantum number?

¹⁷Ne

In this pair of isotopes shown, indicate which one you would expect to be radioactive: ²⁰Ne or ¹⁷Ne

⁹²Tc

In this pair of isotopes shown, indicate which one you would expect to be radioactive: ⁹⁵Mo or ⁹²Tc

No

Is the following atomic orbital acceptable? 1, 1, 0, −1/2

Yes

Is the following atomic orbital acceptable? 3, 1, 1, 1/2

No

Is the following atomic orbital acceptable? 3, 2, +1, 1

Yes

Is the following atomic orbital acceptable? 3, 2, 0, −1/2

l = 4, 3, 2, 1 m-sub-l= -4, -3, -2, -1, 0, 1, 2, 3, 4

List all the possible subshells and orbitals associated with the principal quantum number n, if n = 5.

O, S, Mg, Na

List the following elements in order from smallest to largest: Na, Mg, O, and S.

Mg²⁺ Na⁺ F⁻ O²⁻ N³⁻

List the following ions in order of increasing ionic radius: O²⁻ Mg²⁺ F⁻ Na⁺ N³⁻

Water

Name the following covalent compound: H₂O

Nitrogen Trichloride

Name the following covalent compound: NCl₃

Phosphorous Dichloride

Name the following covalent compound: PCl₂

Sulfur Tetrachloride

Name the following covalent compound: SCl₄

Selenium Hexafluoride

Name the following covalent compound: SeF₆

Tellurium Trioxide

Name the following covalent compound: TeO₃

Aluminum Cyanide

Name the ionic compound: Al(CN)₃

Beryllium Bicarbonate

Name the ionic compound: Be(HCO₃)₂

Copper (I) Phosphide

Name the ionic compound: Cu₃P

Iron (III) Nitrate

Name the ionic compound: Fe(NO₃)₃

Gallium Arsenide

Name the ionic compound: GaAs

Manganese (III) Sulfite

Name the ionic compound: Mn₂(SO₃)₃

Ammonium Chloride

Name the ionic compound: NH₄Cl

Lead (IV) Sulfate

Name the ionic compound: Pb(SO₄)₂

Tin (IV) Selenide

Name the ionic compound: SnSe₂

Titanium (III) Bromide

Name the ionic compound: TiBr₃

H = 5.43%, O = 19.1%, S = 9.59%, C = 57.5%

Penicillin G, a widely used antibiotic, has the formula C₁₆H₁₈N₂O₄S. Calculate the mass percent of each element in penicillin G.

8.4x10⁹ [J/mol]

Plasma is a state of matter consisting of positive gaseous ions and electrons. In the plasma state, a mercury atom could be stripped of its 80 electrons and therefore would exist as Hg⁸⁰⁺. Use the equation for a hydrogen-like ion Eₙ = -(2.18x10⁻¹⁸[J])Z²(1/n²) to calculate the energy required for the last ionization step, that is, Hg⁷⁹⁺ (g) → Hg⁸⁰⁺ (g) + e⁻. Express your answer in [J/mol].

CsF, Cs₂O₄, Cs₃

Put the following groups in order of increasing lattice energy: Cs₃, Cs₂O₄, CsF

MgI₂ MgCl₂ MgF₂

Put the following groups in order of increasing lattice energy: MgF₂, MgCl₂, MgI₂

Na₂S MgS Al₂S₃

Put the following groups in order of increasing lattice energy: Na₂S, MgS, Al₂S₃

Ti(C₂H₃O₂)₂

Write the formula for the following compound: Titanium (II) acetate

CaCl₂

Select the single best answer. Determine which compound has the larger lattice energy: CaCl₂ or SrCl₂.

15 (5A)

Specify the group in the periodic table in which the following element is found: [Ar]4s²3d¹⁰4p³

8 (8B)

Specify the group in the periodic table in which the following element is found: [Ar]4s²3d⁶

1 (A1)

Specify the group in the periodic table in which the following element is found: [Ar]4s¹

15 (5A)

Specify the group in the periodic table in which the following element is found: [Ne]3s²3p³

²⁰³Tl: 29.52% ²⁰⁵Tl: 70.48%

The atomic masses of ²⁰³Tl and ²⁰⁵Tl are 202.972320 and 204.974401 amu, respectively. Calculate the natural abundances of these two isotopes. To seven significant figures, the average atomic mass of thallium is 204.3833 amu.

V(CO₃)₂

Write the formula for the following compound: Vanadium (IV) carbonate

Yes, they both have the same mass ratio of Chlorine to Sodium.

Two samples of sodium chloride are decomposed into their constituent elements. One sample produces 6.98 g of sodium and 10.7 g of chlorine, and the other sample produces 11.2 g of sodium and 17.3 g of chlorine. Are these results consistent with the law of definite proportions?

Nitrogen

What element is represented by the electron configuration of [Ar]3d⁸4s²?

2

What is the maximum number of electrons that can occupy each of the subshell? 2s

6

What is the maximum number of electrons that can occupy each of the subshell? 3p

14

What is the maximum number of electrons that can occupy each of the subshell? 4f

10

What is the maximum number of electrons that can occupy each of the subshell? 5d

V₂S₅

Write the formula for the following compound: Vanadium (V) sulfide

CI₄

Write the formulas of the following covalent compound: Carbon Tetraiodide

7.5 x 10⁻²² mol silver

Which of the following has a greater mass: 173 atoms of gold or 7.5 x 10⁻²² mol silver?

7.5x10²² mol silver

Which of the following has a greater mass: 173 atoms of gold or 7.5x10²² mol silver?

B

Which of the following would exhibit similar chemical properties? A. 1s22s22p5 and 1s22s22p6 B. 1s22s1 and 1s22s22p63s23p64s1 C. 1s22s22p63s23p64s23d104p6 and 1s22s22p5

Cr(OH)₃

Write the formula for the following compound: Chromium (III) hydroxide

[Xe] 6s²4f¹⁴5d¹⁰6p⁴

Write the ground state electron configuration for polonium using the Noble gas core abbreviation.

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹

Write the ground state electron configuration for rubidium.

[Ne]3s²3p⁶

Write the ground-state electron configuration of Ca²⁺ with the Noble Gas core.

[Ne]3s¹

Write the ground-state electron configuration of Mg⁺ with the Noble Gas core.

1s²2s²2p⁶3s²3p⁶

Write the ground-state electron configurations of the following transition metal ion. Sc³⁺

[Xe]4f¹⁴5d¹⁰

Write the ground-state electron configurations of the following transition metal ion. [Noble gas configuration] Au⁺

[Ar]3d³

Write the ground-state electron configurations of the following transition metal ion. [Noble gas configuration] Cr³⁺

[Ar]3d¹⁰

Write the ground-state electron configurations of the following transition metal ion. [Noble gas configuration] Cu⁺

[Ne]3s²3p²

Write the noble gas configuration for silicon.

[Ar]4s¹3d⁵

Write the noble gas core configuration for Cr.

[Ar]3d⁴

Write the noble gas core configuration for Cr²⁺.

[Ar]3d³

Write the noble gas core configuration for Cr³⁺.

[Ar]4s²3d¹⁰4p²

Write the noble gas core configuration for Ge.

[Ar]4s²3d⁸

Write the noble gas core configuration for Ni.

[Xe]6s²4f¹⁴5d¹⁰6p¹

Write the noble gas core configuration for Tl.

[Xe]6s²4f¹⁴5d⁴

Write the noble gas core configuration for W.

[Ar]4s²3d¹⁰

Write the noble gas core configuration for Zn.