How many orbitals would you expect for a system with the following set of quantum numbers?

	a. 1
	b. 3
	c. 5
	d. 7

.

What is the designation for the subshell with the following set of quantum numbers?

	a. 5d
	b. 6f
	c. 6p
	d. The subshell does not exist.

.

The following set of quantum numbers

	a. is representative of a transition metal.
	b. is not allowed.
	c. is representative of a p-block element.
	d. is representative of an element with two valence electrons.

.

One of the p-orbitals of an unknown element is half filled. Assuming that Hund's rule is upheld, which of the following elements could not be the unknown element?

	a. xenon
	b. silicon
	c. gallium
	d. iodine

.

Which of these compounds has a nonzero dipole moment?

	a. boron trifluoride
	b. water
	c. carbon dioxide
	d. methane

.

The configuration for cadmium has 48 electrons. How many electrons occupy the 3d orbital?

	a. 2
	b. 6
	c. 10
	d. 14

.

How many electrons are in the outermost energy shell for promethium (element 61)?

	a. 2
	b. 4
	c. 8
	d. 12

.

The element represented by this orbital diagram is

	a. lithium.
	b. carbon.
	c. silicon.
	d. nitrogen.

.

The element represented by this orbital diagram is

	a. chlorine.
	b. argon.
	c. neon.
	d. boron.

.

In the experimentally observed Z_eff values for the 2p elements, we find that the increase in the Z_eff for a 2p electron is slightly smaller between N and O (ΔZ_eff ≈ 0.62) than between C and N (ΔZ_eff ≈ 0.69). Which of the following is not a reason for the differences in the ΔZ_eff values?

	a. Moving from C to N adds an electron to an occupied orbital.
	b. The Zeff value for oxygen is raised due to additional shielding from fluorine.
	c. Moving from N to O pairs two electrons in a single orbital.
	d. The Zeff value decreases with an increase in electron repulsion.

.

Which element has the largest ionization energy?

	a. fluorine
	b. chlorine
	c. bromine
	d. iodine

.

Which element has the smallest atomic radius?

	a. indium
	b. gallium
	c. boron
	d. aluminum

.

For which of these systems does the metal have a d⁰ electron configuration?

	a. RuNH33+
	b. MnO4-
	c. CuNO3
	d. Zn(ClO4)2

.

Which element has the lowest electron affinity?

	a. argon
	b. chlorine
	c. xenon
	d. bromine

.

The 4th ionization energy of aluminum is approximately 154 eV. From which orbital is the electron being removed?

	a. 2p
	b. 2s
	c. 3p
	d. 3s

.

For the nitrite ion structure below, what is the formal charge on the nitrogen atom?

	a. 1+
	b. 1-
	c. 2+
	d. There is no charge on the nitrogen.

.

The Lewis dot structure for a sulfate ion gives sulfur a formal charge of zero with six bonds. Based on the structure and the Lewis dot theory, which of the following statements about the sulfur atom is false?

	a. The sulfur disobeys the octet rule.
	b. Sulfur has more valence electrons than oxygen.
	c. Sulfur has a greater number of electron shells than oxygen.
	d. Sulfur is less electronegative than oxygen.

.

The AX₃E structure notation best describes which molecule?

	a. H2O
	b. SF4
	c. NH3
	d. XeF4

.

What is the molecular geometry of BCl₃?

	a. square planar
	b. octahedral
	c. tetrahedral
	d. trigonal planar

.

What is the bond order for the Be₂ molecule?

	a. 0
	b. 1
	c. 2
	d. 3

.

According to molecular orbital theory, which molecule is the most stable?

	a. N2
	b. C2
	c. B2
	d. Be2

.

The crystal field splitting diagram shown here represents a _________ complex.

	a. high-spin iron(II)
	b. low-spin iron(II)
	c. high-spin iron(III)
	d. low-spin iron(III)

.

The reaction between hexaamminechromium(III) perchlorate and an excess amount of _________ would definitely lead to the following crystal field splitting diagram.

	a. water
	b. oxalic acid
	c. ammonia
	d. hydrobromic acid

.

Which orbital would you expect to be the LUMO for a O₂^2- peroxide ion?

	a. 2pσ
	b. 2pπ
	c. 2pσ*
	d. 2pπ*

.

The crystal field splitting diagram shown here represents

	a. [Co(NH3)6]3-.
	b. [NiCl6]4-.
	c. [Ni(NH3)6]2+.
	d. [CoF6]3-.

.

The crystal field splitting diagram shown here represents

	a. paramagnetic [FeCl6]3+.
	b. paramagnetic [Fe(CN)6]3+.
	c. diamagnetic [Co(NH3)6]3+.
	d. diamagnetic [CoF6]2+.

.

The chemical formula for potassium hexacyanorhodium(III) is

	a. K3[Rh(CN)6].
	b. Na2[Rh(CN)6].
	c. Na2[Rh(NH3)6].
	d. K[Rh(CN)6].

.

The proper name for the Na[PtCl₃(NH₃)] complex is

	a. amminetrichloroplatinate(II) ion.
	b. sodium amminetrichloroplatinate(II).
	c. sodium amminetrichloroplatinate(IV).
	d. potassium amminetrichloroplatinate(II).

.

Which complex would you expect to be blue in an aqueous solution?

	a. [Ni(CO)6]3+
	b. [Ru(bipy)3]2+
	c. [FeCl6]3+
	d. [Co(CN)6]3-

.

What geometry would you expect [Pt(CN)₄]^2- complex to have?

	a. trigonal bipyrimidal
	b. tetragonal
	c. tetrahedral
	d. square planar

.

A rhombohedral crystal system has which characteristics?

	a. a ≠ b ≠ c, α = β = γ = 90°
	b. a = b = c, α = β = γ ≠ 90°
	c. a = b = c, α = β = γ = 90°
	d. a ≠ b ≠ c, α = β = γ ≠ 90°

.

The complex M_XL_Y has the crystal coordinate system seen below. Of the 14 Bravais lattices, to which could M_XL_Y belong?

	a. base-centered orthorhombic
	b. face-centered cubic
	c. body-centered orthorhombic
	d. base-centered monoclinic

.

How many spheres/atoms are contained in a face-centered cubic unit cell?

	a. 2
	b. 4
	c. 6
	d. 8

.

Which of the following statements concerning amorphous solids is false?

	a. Unlike crystalline solids, amorphous solids lack a repeating unit cell, leading to a random organization of atoms.
	b. Unlike crystalline solids, amorphous solids tend to lose structural organization as their lattices extend.
	c. Amorphous solids are said to behave as supercooled liquids, leading to an ease in transitioning between physical states.
	d. The formation of amorphous solids is aided by the rapid cooling of a molten compound.

.

Which of the following is not a characteristic of covalent solids?

	a. high melting point
	b. low electrical conductivity
	c. high level of hardness
	d. high water solubility

.

How many complete flourine atoms are present in a single unit cell of flourite (CaF₂)?

	a. 4
	b. 6
	c. 8
	d. 14

.

How many spheres/atoms are contained in a simple cubic unit cell?

	a. 0
	b. 1
	c. 2
	d. 4

.

Which halogen would form a binary rubidium compound (RbX) with the longest bond length?

	a. fluorine
	b. chlorine
	c. bromine
	d. iodine

.

Which ion has the smallest radius?

	a. selenium
	b. tellurium
	c. oxygen
	d. sulfur

.

Which of the following statements about the 14 Bravais unit cells is incorrect?

	a. The unit cell is the simplest repeating unit in the crystal lattice.
	b. Opposing faces of a unit cell are parallel.
	c. Each unit cell edge is equivalent in length.
	d. Each unit cell edge connects equivalent points/atoms.

.

Using the table below, determine the crystal lattice energy of KBr.

	a. -604 kJ/mol
	b. -660 kJ/mol
	c. -740 kJ/mol
	d. -819 kJ/mol

.

Cesium and sodium are Group 1 metals, but the coordination number of cesium in the CsCl unit cell is 8, whereas the coordination number of sodium in the NaCl unit cell is 6. What allows cesium to have a larger coordination number?

	a. Sodium has a larger ionic radius than cesium, allowing for less anion attraction.
	b. Due to its size, cesium makes more contact with adjacent anions than sodium does.
	c. The NaCl radius ratio is greater than that of CsCl, forcing anions farther from the metal cation.
	d. Chlorine is too electronegative to be completely compatible with sodium.

.

How many complete NaCl molecules are found in the rock salt unit cell?

	a. 1
	b. 4
	c. 8
	d. 12

.

The coordination numbers of Ca²⁺ and F^- in flourite are _________, respectively.

	a. 2 and 4
	b. 4 and 2
	c. 4 and 4
	d. 6 and 4

.

A body-centered cubic crystal system is best represented in the unit cell of which crystalline solid?

	a. perovskite
	b. NaCl
	c. rutile
	d. CsCl

.

In a close-packed system, what percentage of the unit cell is occupied by holes?

	a. 14
	b. 26
	c. 74
	d. 86

.

In a hexagonal close-packed system, the metal atom caps are arranged in an _________ pattern.

	a. ABC
	b. AAA
	c. ABB
	d. ABA

.

For a face-centered cubic crystal system MX, the metal M is located at the coordinates (1/2, 1/2, 1/2). What would you expect the metal's coordination number to be?

	a. 4
	b. 6
	c. 8
	d. 12

.

A Madelung constant value near 2.4 would likely represent which compound?

	a. barium selenide
	b. beryllium oxide
	c. titanium(II) oxide
	d. strontium chloride

.

Tetrahedral holes have a coordination number of

	a. 4.
	b. 6.
	c. 8.
	d. 12.

.

How many octahedral holes would you expect to find in a closed-packed crystal containing 8 atoms?

	a. 4
	b. 6
	c. 8
	d. 12

.

How many tetrahedral holes would you expect to find in a close-packed crystal containing 6 atoms?

	a. 4
	b. 6
	c. 8
	d. 12

.

What is the size of an octahedral hole in a cubic close-packed system with a radius of 1.5 Ä?

	a. 0.310 Ä
	b. 0.414 Ä
	c. 0.621 Ä
	d. 0.932 Ä

.

What is the size of a tetrahedral hole in a cubic close-packed system with a radius of 1.2 Ä?

	a. 0.23 Ä
	b. 0.27 Ä
	c. 0.40 Ä
	d. 0.54 Ä

.

The MX compound has a radius ratio of 0.51. The metal ion M has the crystal lattice coordinates shown below. Which of the following statements about the MX compound is false?

	a. There are at least three M spheres within the lattice.
	b. The lattice is body centered.
	c. The lattice is close-packed cubic.
	d. The system is hexacoordinate.

.

A body-centered cubic unit cell has a coordination number of

	a. 4.
	b. 6.
	c. 8.
	d. 10.

.

Steel—a solid solution consisting of carbon atoms seated in the holes of an iron atom structure—is an example of a(n)

	a. pure metal.
	b. alkali metal.
	c. substitutional alloy.
	d. interstitial alloy.

.

Brass—a solid solution consisting of zinc and copper atoms—can be considered a(n) _________ and a(n) _________.

	a. substitutional alloy, interstitial alloy
	b. intermetallic alloy, interstitial alloy
	c. substitutional alloy, intermetallic alloy
	d. pure metal, intermetallic alloy

.

Raising the temperature of a metal serves to

	a. ease electron flow over band gaps.
	b. slow down the activity of the atom, promoting a gradual increase in conductivity.
	c. impede conductivity due to increased atom vibration.
	d. allow the metal to behave as a superconductor.

.

Which of the following statements about superconductors is true?

	a. Superconductors are perfectly paramagnetic.
	b. Most superconductors require low temperatures to be efficient.
	c. Superconductors exhibit high resistance to electron flow.
	d. Superconductors exhibit large energy gaps between the valence and conductor bands.

.

The LUMO of a semiconductor

	a. has a limited number of electrons present.
	b. is often separated from the HOMO by an unsurmountable energy gap.
	c. serves as a dopant to the valence band.
	d. serves to provide electrons to the valence band.

.

Glass and quartz are examples of

	a. conductors.
	b. semiconductors.
	c. insulators.
	d. superconductors.

.

For n-type semiconductors,

	a. conduction band electrons outnumber valence band holes.
	b. electron flow is halted due to dopant impurities.
	c. an equal number of valence band holes and conductor band electrons exist, making dopants unnecessary.
	d. doping is facilitated by halides.

.

The doping of silicon with which element would likely form an p-type semiconductor?

	a. phosphorus
	b. boron
	c. antimony
	d. carbon

.

Which of the following statements about semiconductors is true?

	a. Intrinsic superconductors require a dopant to conduct electricity.
	b. Semiconductors have no energy gap between the valence and conductor bands.
	c. Semiconductors increase in conductivity with increasing temperatures.
	d. Intrinsic semiconductors are more efficient than extrinsic semiconductors.

.

For potassium metal, the 4p band represents the _________ and the _________.

	a. LUMO, antibonding orbital
	b. LUMO, bonding orbital
	c. HOMO, nonbonding orbital
	d. HOMO, antibonding orbital

.

At low temperatures, semiconductors and insulators differ only in

	a. valence band composition, with semiconductors and insulators having half- and fully filled HOMOs, respectively.
	b. electron placement, with electrons occupying the conductance bands of semiconductors but not of insulators.
	c. resistivity, with semiconductors being less conductive than insulators with increasing temperatures.
	d. band gap size, with insulator band gaps being greater in energy than those of semiconductors.

.

A material that is able to maintain zero electrical resistance at temperatures near 30K° is considered a(n)

	a. intrinsic semiconductor.
	b. high-temperature superconductor.
	c. low-temperature superconductor.
	d. extrinsic semiconductor.

.

Which system below represents an n-type semiconductor?

	a. I
	b. II
	c. I and II
	d. none of the above

.

4s-4p band overlap allows calcium to behave as a conductor. How many energy levels are present in the conduction band?

	a. 2
	b. 6
	c. 8
	d. 14

.

Which system below represents an intrinsic semiconductor?

	a. I
	b. II
	c. I and II
	d. none of the above

.

Nuclear magnetic resonance (NMR) spectroscopy makes use of liquid helium in order to generate large magnetic fields. The metals involved in creating these fields are behaving as

	a. intrinsic semiconductors.
	b. high-temperature superconductors.
	c. low-temperature superconductors.
	d. extrinsic semiconductors.

.

For which Lewis base would you expect Cu⁺ to have the greatest affinity?

	a. I-
	b. Br-
	c. Cl-
	d. F-

.

Under acidic aqueous conditions, the permanganate ion dissociates and forms Mn²⁺ and 4 mol of water. How many electrons are transferred in this reaction?

	a. 0
	b. 2
	c. 5
	d. 7

.

As the oxidation number of a Lewis acid becomes larger (such as Co²⁺ to Co³⁺), what happens to its hard/soft acid/base character?

	a. The Lewis acid becomes softer.
	b. The Lewis acid becomes harder.
	c. No change is observed.
	d. The Lewis acid behaves as a base.

.

The pOH of the conjugate base of an unknown acid is 4.17. What is the [H+] concentration of the unknown acid?

	a. 2.27 x 10-12
	b. 1.48 x 10-10
	c. 6.76 x 10-5
	d. 4.66 x 10-2

.

In a sulfur-based Lewis base, as the oxidation number of sulfur increases (such as SO₃^2- to SO₄^2-), what happens to its Lewis base character?

	a. No change is observed.
	b. The Lewis base becomes harder.
	c. The Lewis base becomes softer.
	d. The Lewis base behaves as an acid.

.

At room temperature, which hydrogen halide has the lowest boiling point?

	a. HI
	b. HF
	c. HCl
	d. HBr

.

The addition of 4.5x molar excess of aminodimethylsulfoxide (ADMSO) to an ethanolic solution of CuCl₂ leads to the formation of Cu(ADMSO)₄. What is the makeup of the metal-ligand bond?

	a. C-O
	b. C-C
	c. C-S
	d. C-N

.

For the reaction of mercury(II) chloride and ammonia, which product is a conjugate Lewis base?

	a. NH3
	b. HgCl2
	c. Hg(NH3)2
	d. Cl-

.

For the reaction below, the hydrogen phosphate ion behaves as a(n)

	a. acid.
	b. base.
	c. chelator
	d. catalyst.

.

For the reaction below, water behaves as a(n)

	a. acid.
	b. base.
	c. both A and B
	d. none of the above

.

For the pair of reactions below, which compounds are represented by X, Y, and Z, respectively?

	a. FeSO43, 3Ag2SO4, 3Pt(SCN)4
	b. Fe2(SO4)3, 6Ag2SO4, 3Pt(SCN)4
	c. Fe2(SO4)3, 6Ag2SO4, 3Pt(SCN)2
	d. Fe2(SO4)3, 3Ag2SO4, 3Pt(SCN)4

.

For which Lewis acid would you expect CO to have the least affinity?

	a. Ag+
	b. Ru3+
	c. Be2+
	d. Zn2+

.

For which Lewis acid would you expect H₂O to have the greatest affinity?

	a. Pt4+
	b. Cd2+
	c. Ni2+
	d. Fe3+

.

Which of the following hydrogen halides has the smallest bond enthalpy?

	a. HI
	b. HF
	c. HBr
	d. HCl

.

The combustion of methane gas forms _________ and water.

	a. oxalic acid
	b. carbon monoxide
	c. carbon suboxide
	d. carbon dioxide

.

The reaction of a Group I metal hydroxide with excess nitric acid leads to a series of solid metal nitrates. Of the following, which would you expect to have the lowest boiling point?

	a. RbNO3
	b. LiNO3
	c. NaNO3
	d. KNO3

.

Which Group 3 element has the highest melting point?

	a. aluminum
	b. boron
	c. indium
	d. gallium

.

Which diatomic system has the largest bond enthalpy?

	a. PbO
	b. SiO
	c. CO
	d. GeO

.

Nitrogen and phosphorus are Group 5 elements, but nitrogen forms only three bonds, while phosphorus can form up to five. What accounts for the ability of phosphorus to form more bonds?

	a. Phosphorus has an additional electron shell.
	b. Phosphorus has two more valence electrons than nitrogen.
	c. Phosphorus is more electronegative than nitrogen.
	d. Nitrogen has three unpaired electrons in its ground state.

.

Which Group 6 element has the largest atomic radius?

	a. oxygen
	b. sulfur
	c. selenium
	d. tellurium

.

The molecular formula for chlorous acid is

	a. HClO.
	b. HClO2.
	c. HClO3.
	d. HClO4.

.

Which of the following halogens is a solid at room temperature?

	a. bromine
	b. chlorine
	c. iodine
	d. fluorine

.

While not to the same extent as Group I metals, Group II metals are quite reactive with water. Each metal has a different level of reactivity with water, but they ultimately follow a well-observed reactivity trend. What is an explanation for the trend observed in water reactivity when moving down from beryllium to barium?

	a. The electronegativity increases with additional electron shells.
	b. The electrons of the larger metals are farther from the nucleus and easier to remove.
	c. The smaller metals have a greater attraction to the lone pairs on the H2O oxygens.
	d. The presence of d-orbital electrons in the larger metals allows for decreased water reactivity.

.

In the product for the reaction below, what is the oxidation state of phosphorus?

	a. 2+
	b. 3+
	c. 3-
	d. 5+

.

For the reaction below, X could represent which element?

	a. calcium
	b. rubidium
	c. indium
	d. silicon

.

For the reaction below, element X is a _________ element.

	a. Group 2
	b. Group 3
	c. Group 4
	d. Group 5

.

For the reaction below, X could represent which element?

	a. strontium
	b. potassium
	c. magnesium
	d. gallium

.

For the reaction below, element X is a _________ element.

	a. Group 1
	b. Group 2
	c. Group 5
	d. Group 7

.