chem 1301 final

R in pv=nrt

.08206 L atm/ mol K

1 Lxatm

101.3 J

5) The law of ________ states that energy that can be neither created or destroyed. A) kinetic energy B) the consecration of energy C) potential energy D) the conservation of energy E) thermochemistry

D

A triple covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs

D

Choose the bond below that is least polar. A) P-F B) C-Br C) C-F D) C-I E) C-Cl

D

Which reaction below represents the first ionization of O? A)O+(g)+e− → O(g) B) O(g) + e− → O−(g) C) O−(g) → O(g) + e− D)O(g) → O+(g)+e− E) O−(g) + e− → O2−(g)

D

Identify the number of valence electrons for Ti. A) 8 B) 7 C) 4 D) 2

2

A cation of +2 indicates that an element has A) lost two electrons. B) lost two protons. C) lost two neutrons. D) gained two electrons. E) gained two protons.

A

Choose the bond below that is the strongest. A) N=O B) N-F C) C-O D) N-C E) N=N

A

Choose the compound below that should have the highest melting point according to the ionic bonding model. A) AlN B) MgO C) NaCl D) CaS E) RbI

A

Choose the diamagnetic species from below. A) Sn2+ B) I C) N D) Cr E) None of the above are diamagnetic.

A

Choose the ground state electron configuration for Ti2+. A) [Ar]3d2 B) [Ar]4s2 C) [Ar]4s23d2 D) [Ar]4s23d4 E) [Ar]3d4

A

Describe the reaction of the noble gases with metals. A) inert B) vigorous C) mild reaction D) forms water E) dissolves

A

Energy that is associated with the motion of an object is called A) kinetic energy B) thermal energy C) potential energy D) chemical energy

A

Give the electron configuration for O. A) 1s22s22p4 B) 1s22p4 C) 1s22s22p3 D) 1s22s22p5 E) 1s22s12p1

A

Halogens can react with each other to form A) covalent bonds. B) ionic bonds. C) salts. D) hydrogen halides. E) metal halides.

A

How many valence electrons do the alkali metals possess? A) 1 B) 2 C) 7 D) 6 E) 8

A

How many valence electrons does an atom of Mg possess? A) 2 B) 1 C) 8 D) 5 E) 3

A

How many valence electrons does an atom of Ti possess? A) 2 B) 4 C) 6 D) 8 E) 0

A

Identify the compound with ionic bonding. A) NaBr B) Na C) H2O D) He E) S

A

Identify the compound with the highest magnitude of lattice energy. A) MgCl2 B) BaCl2 C) SrCl2 D) CsCl2

A

Identify the compound with the smallest dipole moment in the gas phase. A) Cl2 B) ClF C) HF D) LiF

A

Identify the correct values for a 3p sublevel. A) n = 3, l = 1, ml = 0 B) n = 2, l = 1, ml = +2 C) n = 1, l = 0, ml = 0 D) n = 2, l = 0, ml = 0 E) n = 4, l = -1, ml = -2

A

Identify the element that has a ground state electronic configuration of [Kr]5s24d5. A) Tc B) Mn C) Nb D) Ru

A

Identify the most reactive alkali metal with water. A) Cs B) Rb C) K D) Na E) Li

A

Identify the species that has the smallest radius. A) cation B) anion C) neutral D) they are all the same size

A

Identify the substance that conducts electricity. A) NaCl dissolved in water B) solid NaCl C) ethanol D) solid sugar E) sugar dissolved in water.

A

Identify the weakest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) all of the above bonds are the same strength

A

Place the following in order of decreasing dipole moment. I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF A) III > I > II B) II > I > III C) I > III > II D) II > III > I E) I = III > II

A

Place the following in order of decreasing magnitude of lattice energy. K2O Rb2S Li2O A) Li2O > K2O > Rb2S B) Li2O > Rb2S > K2O C) Rb2S > K2O > Li2O D)Rb2S > Li2O > K2O E)K2O > Li2O > Rb2S

A

Place the following in order of increasing Se-X bond angle, where X represents the outer atoms in each molecule. SeO2 SeCl6 SeF2 A) SeCl6 < SeF2 < SeO2 B) SeF2 < SeO2 < SeCl6 C) SeF2 < SeCl6 < SeO2 D) SeO2 < SeF2 < SeCl6 E) SeCl6 < SeO2 < SeF2

A

Place the following in order of increasing radius. Ba2+ Te2− I− A) Ba2+ < I− < Te2− B) I− < Ba2+ < Te2− C) Te2− < I− < Ba2+ D)Ba2+ < Te2− < I− E) I− < Te2− < Ba2+

A

The phosphorus atom in PCl3 would be expected to have a A) partial positive (δ+) charge. B) partial negative (δ-) charge. C) 3+ charge. D) 3- charge.

A

Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-F P-F As-F A)Sb-F > As-F > P-F B) As-F > Sb-F > P-F C) Sb-F > P-F > As-F D)P-F > As-F > Sb-F E)Sb-F > P-F> As-F

A

Which compound has the longest carbon-carbon bond length? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond lengths are the same

A

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat? A) 50.0 g Al, CAl = 0.903 J/g°C B) 50.0 g Cu, CCu = 0.385 J/g°C C) 25.0 g granite, Cgranite = 0.79 J/g°C D) 25.0 g Au, CAu = 0.128 J/g°C E) 25.0 g Ag, CAg = 0.235 J/g°C

A

Which of the following elements can form compounds with an expanded octet? A) Se B) C C) Li D) F E) All of the above elements can form compounds with an expanded octet.

A

Which of the following have their valence electrons in the same shell? A) Li, N, F B) B, Si, As C) N, As, Bi D) He, Ne, F

A

Which of the following ionic compounds would be expected to have the highest lattice energy? A) Li Cl B) Na Cl C) K Cl D) Rb Cl

A

Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiF B) LiCl C) LiBr D) LiI

A

Which of the following is not a standard state? A) for a solid, it is 25°F B) for a liquid, it is 25°C C) for a gas, it is 1 atm D) for a solution, it is 1 M E) for a liquid, it is 1 atm

A

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as gaining heat from the surroundings? A) q = +, w = - B) q = -, w = + C) q = +, w = + D) q = -, w = -

A

Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as losing heat to the surroundings? A) q = -, w = - B) q = +, w = + C) q = -, w = + D) q = +, w = -

A

Which of the following species will have the highest ionization energy? A) K+ B) Ar C) Cl- D) S2-

A

Which of the following statements is TRUE? A) An ionic bond is much stronger than most covalent bonds. B) An ionic bond is formed through the sharing of electrons. C) Ionic compounds at room temperature typically conduct electricity. D) Once dissolved in water, ionic compounds rarely conduct electricity. E) None of the above are true.

A

Which atom in each group (I and II) has the smallest atomic radius? (I) Ba, Hf, At A) Ba; As B) Ba; Bi C) At; As (II) As, Sb, Bi D) At; Bi

C

Which compound has the highest carbon-carbon bond strength? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond strengths are the same

C

Which compound has the shortest carbon-carbon bond length? A) CH3CH3 B) CH2CH2 C) HCCH D) all bond lengths are the same

C

Which element can expand its valence shell to accommodate more than eight electrons? A) N B) O C) Br D) He

C

Which element has the ground-state electron configuration [Xe]6s24f 7? A) Re B) Ir C) Eu D) Gd

C

Which element has the highest first electron affinity? A) Na B) Mg C) O D) Ne

C

Which ion does not have a noble gas configuration in its ground state? A) Sc3+ B) Al3+ C) Ga3+ D) As3-

C

Which ionic compound would be expected to have the highest lattice energy? A) Rb2O B) SrO C) In2O3 D) CO2

C

Which molecule or compound below contains a pure covalent bond? A) Li2CO3 B) SCl6 C) Br2 D) PCl3 E) NaCl

C

Which of the following contains an atom that does not obey the octet rule? A) CsI B) SnO2 C) ClF5 D) ClF

C

Which of the following have the same number of valence electrons? A) Rb, Sb, I B) Ga, Sn, Bi C) As, Sb, Bi D) Ar, Kr, Br

C

Which of the following processes are endothermic? A) K+(g) + I−(g) → KI(s) B) 2 Br(g) → Br2(g) C) Ca(s) → Ca(g) D) 2 Na(s) + O2(g) → Na2O(s)

C

Give the number of core electrons for Cd. A) 44 B) 48 C) 46 D) 45 E) 47

C

Give the number of core electrons for Se. A) 26 B) 30 C) 28 D) 32 E) 34

C

Draw the Lewis structure for SO42−. How many equivalent resonance structures can be drawn? A) 6 B) 2 C) 4 D) 3 E) 8

6

Describe how a neon light works.

A neon sign contains glass tubes filled with neon gas. When an electric current is passed through the tube, the neon atoms absorb some of the energy and re-emits it as light.

A single covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs

B

An element that has the valence electron configuration 6s26p6 belongs to which period and group? A) period 6; group 6A B) period 6; group 8A C) period 7; group 6A D) period 7; group 8A

B

Choose the bond below that is most polar. A) C-N B) C-F C) N-O D) C-C E) Cl-Cl

B

Choose the bond below that is the weakest. A) Na-Br B) Br-Br C) C=N D) Li-I E) C=N

B

Choose the compound below that contains at least one polar covalent bond, but is non polar. A) HCN B) CF4 C) SeBr4 D) ICl3

B

Choose the compound below that should have the highest melting point according to the ionic bonding model. A) SrI2 B) MgF2 C) CaCl2 D) SrF2 E) SrBr2

B

Choose the ground state electron configuration for Zn2+. A) [Ar]4s23d8 B) [Ar]3d10 C) [Ar]4s23d6 D) [Ar] E) [Ar]3d8

B

Choose the paramagnetic species from below. 23 A) Ti4+ B) Se C) Ar D) All of the above are paramagnetic. E) None of the above are paramagnetic.

B

Describe the reaction of the alkali metals with non-metals. A) inert B) vigorous C) mild reaction D) forms water E) dissolves

B

Energy that is associated with the temperature of an object is called A) kinetic energy B) thermal energy C) potential energy D) chemical energy

B

Identify the compound with metallic bonding. A) NaBr B) Na C) H2O D) He E) S

B

Identify the compound with the lowest magnitude of lattice energy. A) KCl B) KBr C) SrO D) BaO

B

Identify the compound with the smallest percent ionic character. A) HF B) IBr C) HCl D) LiF

B

Of the following elements, which has the highest electronegativity? A) Si B) P C) Ti D) Ge

B

Of the following, which atom has the smallest atomic radius? A) K B) As C) Rb D) Sb

B

Of the following, which element has the highest first ionization energy? A) barium B) lead C) cesium D) thallium

B

Of the following, which element has the highest first ionization energy? A) Al 24 B) Cl C) Na D) P

B

Place the following in order of decreasing magnitude of lattice energy. NaF RbBr KCl A)RbBr > NaF > KCl B) NaF > KCl > RbBr C) KCl > NaF > RbBr D)NaF > RbBr > KCl E)RbBr > KCl > NaF

B

Place the following in order of increasing A-F bond angle, where A represents the central atom in each molecule. PF3 OF2 PF4⁺ A) PF3 < OF2 < PF4⁺ B) OF2 < PF3 < PF4⁺ C) OF2 < PF4⁺ < PF3 D) PF4⁺ < OF2 < PF3 E) PF4⁺ < PF3 < OF2

B

Rank the following molecules in decreasing bond energy. Cl2 Br2 F2 I2 A) I2 > Br2 > Cl2 > F2 B) Cl2 > Br2 > F2 > I2 C) I2 > Cl2 > Br2 > F2 D)Cl2 > I2 > F2 > Br2

B

Use Lewis theory to determine the chemical formula for the compound formed between Al and O. A) Al3O2 B) Al2O3 C) AlO2 D) Al2O E) AlO

B

Using periodic trends, place the following bonds in order of increasing ionic character. Si-P Si-Cl Si-S A) Si-P < Si-Cl < Si-S B) Si-P < Si-S < Si-Cl C) Si-S < Si-Cl < Si-P D) Si-Cl < Si-P < Si-S E) Si-Cl < Si-S < Si-P

B

What is the general valence-electron ground-state electron configuration for neutral alkaline earth metals? A) ns1 B) ns2 C) 1s22s1 D) 1s22s2

B

Which of the following elements can form compounds with an expanded octet? A) O B) Br C) F D) Be E) None of the above can form compounds with an expanded octet.

B

Which of the following processes are endothermic? A) the reaction associated with the lattice energy of LiCl. B) the reaction associated with the ionization energy of potassium. C) the reaction associated with the heat of formation of CaS. D) the formation of F2 from its elements in their standard states. E) None of the above are endothermic.

B

Which of the following processes are exothermic? A) Cl2(g) → 2Cl(g) B) Br(g) + e− → Br−(g) C) Li(s) → Li(g) D) NaF(s) → Na+(g) + F−(g) E) None of the above are exothermic.

B

Define bond energy.

Bond energy is the energy required to break 1 mole of the bond in the gas phase.

A double covalent bond contains ________ of electrons. A) 0 pairs B) 1 pair C) 2 pairs D) 3 pairs E) 4 pairs

C

Choose the bond below that is most polar. A) H-I B) H-Br C) H-F D) H-Cl E) C-H

C

Choose the bond below that is the weakest. A) C≡O B) N≡N C) C-I D) C=O E) K-Br

C

Choose the compound below that contains at least one polar covalent bond, but is non polar. A) GeH2Br2 B) SCl2 C) AsCl5 D) CF2Cl2

C

Choose the compound below that should have the lowest melting point according to the ionic bonding model. A) LiF B) LiCl C) CsI D) KBr E) RbI

C

Choose the ground state electron configuration for Hf2+. A) [Xe]6s2 B) [Xe]6s25d2 C) [Xe]5d2 D) [Xe] E) [Xe]6s25d4

C

Energy that is associated with the position or composition of an object is called A) kinetic energy B) thermal energy C) potential energy D) chemical energy

C

Give the set of four quantum numbers that could represent the electron gained to form the Br ION from the Br atom. A) n = 4, l = 1, ml = 1, ms = +1/2 B) n = 4, l = 0, ml = -1, ms = +1/2 C) n = 4, l = 1, ml = 1, ms = -1/2 D) n = 3, l = 2, ml = 1, ms = +1/2 E) n = 5, l = 1, ml =-1, ms = -1/2

C

Given w = 0, an endothermic reaction has the following. A) +ΔH and -ΔE B) - ΔH and +ΔE C) + ΔH and +ΔE D) - ΔH and -ΔE

C

How many of the following elements can form compounds with an expanded octet? I O Br Xe A) 2 B) 0 C) 3 D) 1 E) 4

C

How many of the following species are paramagnetic? Sc3+ Cl− Ba2+ Se A) 0 B) 2 C) 1 D) 4 E) 3

C

Identify an ionic bond. A) Electrons are pooled. B) Electrons are shared. C) Electrons are transferred. D) Protons are gained. E) Electrons are lost.

C

Identify the compound with covalent bonding. A) NaBr B) Na C) H2O D) He E) S

C

Identify the number of bonding pairs and lone pairs of electrons in water. A) 1 bonding pair and 1 lone pair B) 1 bonding pair and 2 lone pairs C) 2 bonding pairs and 2 lone pairs D) 2 bonding pairs and 1 lone pair E) 3 bonding pairs and 2 lone pairs

C

Identify the number of valence electrons in Cl-1. A) 6 B) 7 C) 8 D) 5 E) 4

C

Identify the shortest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) all of the above bonds are the same length

C

Identify the strongest bond. A) single covalent bond B) double covalent bond C) triple covalent bond D) all of the above bonds are the same strength

C

Of the following elements, which has the lowest electronegativity? A) Sr B) I C) Ba D) At

C

Of the following, which atom has the largest atomic radius? A) Rb B) I C) Cs D) At

C

Of the following, which element has the highest first ionization energy? A) beryllium B) boron C) carbon D) lithium

C

Place the following in order of decreasing A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N2O NCl3 NO2⁻ A) NCl3 > NO2⁻ > N2O B) NO2⁻ > N2O > NCl3 C) N2O > NO2⁻ > NCl3 D) NCl3 > N2O > NO2⁻ E) N2O > NCl3 > NO2⁻

C

Place the following in order of decreasing bond length. H-F H-I H-Br A)H-F > H-Br > H-I B) H-I > H-F > H-Br C) H-I > H-Br > H-F D)H-Br > H-F > H-I E)H-F > H-I >H-Br

C

Place the following in order of decreasing metallic character. CONF A)O > N > F > C B) F > O > N > C C) C > N > O > F D)F > N > O > C E) N > C > O > F

C

Place the following in order of increasing magnitude of lattice energy. CaO MgO SrS A)MgO < CaO < SrS B) SrS < MgO < CaO C) SrS < CaO < MgO D)CaO < MgO < SrS E)CaO < SrS < MgO

C

The compound ClF contains A) ionic bonds. B) nonpolar covalent bonds. C) polar covalent bonds with partial negative charges on the F atoms. D) polar covalent bonds with partial negative charges on the Cl atoms.

C

The electronegativity is 2.1 for H and 1.9 for Pb. Based on these electronegativities PbH4 would be expected to A) be ionic and contain H- ions. B) be ionic and contain H+ ions. C) have polar covalent bonds with a partial negative charges on the H atoms. D) have polar covalent bonds with a partial positive charges on the H atoms.

C

Which of the following reactions is associated with the lattice energy of Li2O (ΔH°latt)? A) Li2O(s) → 2 Li+(g) + O2−(g) B) 2 Li+(aq) + O2−(aq) → Li2O(s) C) 2 Li+(g) + O2−(g) → Li2O(s) D) Li2O(s) → 2 Li+(aq) + O2−(aq) E) 2 Li(s) + O2(g) → Li2O(s)

C

Which of the following represents the change in electronic configuration that is associated with the first ionization energy of strontium? A) [Kr]5s15p1 → [Kr]5s1 + e- B) [Kr]5s2 → [Kr]5s15p1 C) [Kr]5s2 → [Kr]5s1 + e- D) [Kr]5s2 + e- → [Kr]5s25p1

C

Which of the following statements is TRUE? A) The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in the set. B) A bond order of 0 represents a stable chemical bond. C) When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals. D) Electrons placed in antibonding orbitals stabilize the ion/molecule. E) All of the above are true.

C

Energy that is associated with the relative positions of electrons and nuclei in atoms and molecules is called A) kinetic energy B) thermal energy C) potential energy D) chemical energy

D

For ΔEsys to always be -, what must be true? A) q = w B) +q > -w C) +w > -q D) -w > +q

D

Give the set of four quantum numbers that could represent the electron lost to form the K ION from the K atom. A) n = 3, l = 1, ml = 1, ms = -1/2 B) n = 4, l = 0, ml = 0, ms = -1/2 C) n = 4, l = 4, ml = 0, ms = -1/2 D) n = 4, l = 0, ml = 0, ms = +1/2 E) n = 3, l = 0, ml = -1, ms = -1/2

D

How many electrons are in the outermost shell of the Ga3+ ion in its ground state? A) 2 B) 3 C) 6 D) 18

D

How many of the following elements can form compounds with an expanded octet? P Kr Xe B A) 0 B) 1 C) 2 D) 3 E) 4

D

How many of the following species are diamagnetic? Fr Zr2+ Al3+ Hg2+ A) 1 B) 3 C) 0 D) 2 E) 4

D

Identify the bond with the highest bond energy. A) Si=O B) N=N C) C=C D) C=N E) O=O

D

Identify the compound with the highest percent ionic character. A) HF B) IBr C) HCl D) LiF

D

Identify the compound with the largest dipole moment in the gas phase. A) Cl2 B) ClF C) HF D) LiF

D

List the following compounds in decreasing electronegativity difference. F2 HF KF A)KF > F2 > HF B) F2 > HF > KF C) HF > KF > F2 D)KF > HF > F2

D

Place the following elements in order of decreasing atomic radius. Xe Rb Ar A) Ar > Xe > Rb B) Xe > Rb > Ar C) Ar > Rb > Xe D) Rb > Xe > Ar E) Rb > Ar > Xe

D

Place the following elements in order of increasing electronegativity. Na Rb P A)P < Na < Rb B) Na < P < Rb C) Rb < P < Na D) Rb < Na < P E)P < Rb < Na

D

Place the following in order of decreasing A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS2 CF4 SCl2 A) CS2 = SCl2 > CF4 B) SCl2 > CF4 > CS2 C) CF4 > CS2 > SCl2 D) CS2 > CF4 > SCl2 E) CF4 > CS2 = SCl2

D

Place the following in order of increasing bond length. C-F C-S C-Cl A)C-S < C-Cl < C-F B) C-Cl < C-F < C-S C) C-F < C-S < C-Cl D)C-F < C-Cl < C-S E)C-S < C-F < C-Cl

D

Place the following in order of increasing bond length. NO2− NO3− NO A)NO < NO2− < NO3− B) NO2− < NO3− < NO C) NO3− < NO < NO2− D)NO < NO3− < NO2− E)NO3− < NO2− < NO

D

The iodine atom in I2 would be expected to have a A) charge of 1-. B) partial charge δ-. C) partial charge δ+. D) charge of 0.

D

Which ionization process requires the most energy? A) W(g) → W+(g) + e- B) W+(g) → W2+(g) + e- C) W2+(g) → W3+(g) + e- D) W3+(g) → W4+(g) + e- Answer: D

D

Which ionization process requires the most energy? A) O(g) → O+(g) + e- B) O+(g) → O2+(g) + e- C) F(g) → F+(g) + e- D) F+(g) → F2+(g) + e-

D

Which molecule or compound below contains a polar covalent bond? A) C2H4 B) ZnS C) LiI D) NCl3 E) AgI

D

Which of the following processes are exothermic? A) the second ionization energy of Mg B) the sublimation of Li C) the breaking the bond of I2 D) the formation of NaBr from its constituent elements in their standard state E) None of the above are exothermic

D

Which of the following reactions is associated with the lattice energy of CaS (ΔH°latt)? A) Ca(s) + S(s) → CaS(s) B) CaS(s) → Ca(s) + S(s) C) Ca2+(aq) + S2−(aq) → CaS(s) D) Ca2+(g) + S2−(g) → CaS(s) E) CaS(s) → Ca2+(aq) + S2−(aq)

D

Define dipole moment.

Dipole moment is the measured quantitative value associated with the separation of the partial positive and negative charges found within a molecule.

Choose the bond below that is the strongest. A) C-F B) C=O C) C-I D) I-I E) C≡N

E

Choose the paramagnetic species from below. A) Ca B) O2− C) Zn2+ D) Cd E) Nb3+

E

Give the number of core electrons for Cl-. A) 22 B) 30 C) 17 D) 12 E) 10

E

Give the number of valence electrons for Cl. A) 8 B) 6 C) 5 D) 3 E) 7

E

Give the set of four quantum numbers that could represent the electron lost to form the Rb ION from the Rb atom. A) n = 6, l = 0, ml = -1 ms = -1/2 B) n = 4, l = 1, ml = 1, ms = +1/2 C) n = 5, l = 0, ml = 0, ms = -1/2 D) n = 4, l = 1, ml = 0, ms = -1/2 E) n = 5, l = 0, ml = 0, ms = +1/2

E

Identify the states of the halogens at room temperature. A) Fluorine, chlorine, bromine, and iodine are solids. B) Fluorine, chlorine, and bromine are solids, and iodine is a solid. C) Fluorine and iodine are solids, chlorine and bromine are gases. D) Fluorine is a gas, chlorine and bromine are liquids, and iodine is a solid. E) Fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

E

Place the following elements in order of decreasing electronegativity. S F Se A)Se > S > F B) F > Se > S C) Se > F > S D)S >F > Se E)F > S > Se

E

Place the following in order of decreasing XO bond length, where "X" represents the central atom in each of the following compounds or ions. SiO32− CO2 CO32− A) CO2 > SiO32− > CO32− B) CO2 > CO32− > SiO32− C) CO32− > CO2 > SiO32− D) CO32− > SiO32− > CO2 E) SiO32− > CO32− > CO2

E

Place the following in order of increasing A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H2O H3O⁺ A) H2O = H3O⁺ < HCN B) H3O⁺ < H2O < HCN C) HCN < H3O⁺ < H2O D) H2O < HCN < H3O⁺ E) H2O < H3O⁺ < HCN

E

Place the following in order of increasing dipole moment. I. BCl3 II. BIF2 III. BClF2 A) I < II = III B) II < III < I C) I < II < III D) II < I < III E) I < III < II

E

Two aqueous solutions are both at room temperature and are then mixed in a coffee cup calorimeter. The reaction causes the temperature of the resulting solution to fall below room temperature. Which of the following statements is TRUE? A) The products have a lower potential energy than the reactants. B) This type of experiment will provide data to calculate ΔErxn. C) The reaction is exothermic. D) Energy is leaving the system during reaction. E) None of the above statements are true.

E

Using periodic trends, place the following bonds in order of increasing ionic character. S-Cl Se-Cl O-Cl A) Se-Cl < S-Cl < O-Cl B) S-Cl < Se-Cl < O-Cl C) O-Cl < Se-Cl < S-Cl D) Se-Cl < O-Cl < S-Cl E) O-Cl < S-Cl < Se-Cl

E

Which molecule or compound below contains an ionic bond? A) CO2 B) C2Br4 C) SiF4 D) OCl2 E) NH4NO3

E

Which of the following reactions is associated with the lattice energy of RbI (ΔH°latt)? 3 A) Rb(s) + I2(g) → RbI(s) B) RbI(s) → Rb+(g) + I−(g) C) RbI(s) → Rb(s) + I2(g) D) RbI(s) → Rb+(aq) + I−(aq) E) Rb+(g) + I−(g) → RbI(s)

E

Which of the following statements is TRUE? A) A covalent bond is formed through the transfer of electrons from one atom to another. B) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." C) It is not possible for two atoms to share more than two electrons. D) Single bonds are shorter than double bonds. E) A covalent bond has a lower potential energy than the two separate atoms

E

Which of the following statements is TRUE? A) State functions do not depend on the path taken to arrive at a particular state. B) DErxn can be determined using constant volume calorimetry. C) Energy is neither created nor destroyed, excluding nuclear reactions. D) ΔHrxn can be determined using constant pressure calorimetry. E) All of the above are true.

E

Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? A) 10.0 g Cu, CCu = 0.385 J/g°C B) 10.0 g H2O, CH2O = 4.18 J/g°C C) 10.0 g ethanol, Cethanol = 2.42 J/g°C D) 10.0 g Al, CAl = 0.903 J/g°C E) 10.0 g Pb, CPb= 0.128 J/g°C

E

How many orbitals are contained in the n = 2 level? Give the l and ml values of each of them.

Four: the 2s and three 2p orbitals. 2s, l = 0, ml = 0; 2p, l = 1, ml = -1 and l = 1, ml = 0 and l =1, ml = +1.

List the noble gas that has the highest ionization energy.

He

Using Lewis structures and formal charge, which of the following ions is most stable? OCN− ONC− NOC−

OCN-

Q

Q=MCdeltaT M in kg T can be in Celsius

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?

The energies of atoms are quantized. When an electron moves from one energy level to another during emission, a specific wavelength of light (with specific energy) is emitted. The electrons are not allowed "in between" quantized energy levels and thus only specific lines are observed.

Draw the Lewis structure for CO32- including any valid resonance structures. Which of the following statements is TRUE? A) The CO32- ion contains one C—O single bond and two C=O double bonds. B) The CO32- ion contains two C—O single bonds and one C=O double bond. C) The CO32- ion contains three C—O double bonds. D) The CO32- ion contains two C—O single bonds and one C≡O triple bond. E) None of the above are true.

b

Draw the Lewis structure for NO2− including any valid resonance structures. Which of the following statements is TRUE? A) The nitrite ion contains one N—O single bond and one N=O double bond. B) The nitrite ion contains two N—O bonds that are equivalent to 1 C) The nitrite ion contains two N=O double bonds. D) The nitrite ion contains two N—O single bonds. E) None of the above are true.

b

Identify the compound with atoms that have an incomplete octet. A) ICl5 B) CO2 C) BF3 D) Cl2 E) CO

c

Which statement is FALSE? A) An exothermic reaction gives heat off heat to the surroundings. B) Enthalpy is the sum of a system's internal energy and the product of pressure and volume. C) ΔErxn is a measure of heat. D) ΔHrxn is the heat of reaction. E) Endothermic has a positive ΔH.

c

Which of the following resonance structures for OCN− will contribute most to the correct structure of OCN−? A) O(2 lone pairs)=C=N (2 lone pairs) B) O(1 lone pair) ≡C—N(3 lone pairs) C) O(1 lone pair)=C(2 lp) N(1 lone pair) D) O(3 lone pairs)—C≡N(with 1 lone pair) E) They all contribute equally to the correct structure of OCN−.

d

heat

mass x specific heat x change in temperature

Give an example of a p orbital.

px, py, or pz

C

specific heat capacity

Heat capacity

the quantity of heat required to change a system's temperature by 1 degree C J/degree C

molar heat capacity

the quantity of heat required to raise the temp of 1 mole of a substance by 1 degree C

specific heat capacity

to quantity of heat required to raise the temperature of 1 gram of a substance by 1°C J/g degree C

Give the ground state electron configuration for Br−. A) [Ar]4s23d104p6 B) [Ar]4s23d104p5 C) [Ar]4s24p6 D) [Ar]4s24d104p6 E) [Ar]4s23d104p4

A

Give the ground state electron configuration for Se. A) [Ar]4s23d104p4 B) [Ar]4s24d104p4 C) [Ar]4s23d104p6 D) [Ar]4s23d10 E) [Ar]3d104p4

A

Give the number of valence electrons for Si. A) 4 B) 2 C) 28 D) 12 E) 26

A

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Cl atom. A) n = 3, l = 1, ml = 1, ms = +1/2 B) n = 3, l = 0, ml = 1, ms = -1/2 C) n = 3, l = 2, ml =1, ms = +1/2 D) n = 2, l = 1, ml = 1, ms = -1/2 E) n = 3, l =1, ml = 1, ms =-1/2

A

How many different values of ml are possible in the 5f sublevel? A) 1 B) 7 C) 4 D) 6 E) 2

B

How many unpaired electrons are present in the ground state As atom? A) 0 B) 3 C) 1 D) 2 E) 4

B

How many valence electrons do the alkali earth metals possess? A) 1 B) 2 C) 7 D) 6 E) 8

B

How many valence electrons does an atom of As have? A) 3 B) 5 C) 8 D) 4 E) 6

B

In which orbital below would an electron (on average) be farthest from the nucleus? A) 1s B) 4f C) 3s D) 3d E) 2p

B

Place the following in order of increasing IE1. N F As A)N < As < F B) As < N < F C) F < N < As D)As < F < N E)F < As < N

B

Place the following in order of increasing metallic character. Rb Cs K Na A)K < Cs < Na < Rb B) Na < K < Rb < Cs C) Cs < Rb < K < Na D)K < Cs < Rb < Na E)Na < Rb < Cs < K

B

Place the following in order of increasing radius. Br− Na+ Rb+ A)Br− < Rb+ < Na+ B) Na+ < Rb+ < Br− C) Rb+ < Br− < Na+ D)Br− < Na+ < Rb+ E)Rb+ < Na+ < Br−

B

The complete electron configuration of gallium, element 31, is ________. A) 1s22s22p103s23p104s23d3 B) 1s22s22p63s23p63d104s24p1 C) 1s42s42p63s43p64s43d3 D) 1s22s42p103s43p9 E) 1s22s42p83s43p84s3

B

What are the possible values of l if n = 6? A) 6 B) 0, 1, 2, 3, 4, or 5 C) -4, -3, -2, -1, 0, +1, +2, +3, or +4 D) -5, -4, -3, -2, -1, 0, +1, +2, +3, +4, or +5

B

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as A) Pauli exclusion principle B) Hund's rule C) Aufbau principle D) Heisenberg uncertainty principle

B

Which reaction below represents the second electron affinity of S? A)S(g)+e− → S−(g) B) S−(g) + e− → S2−(g) C) S(g) → S+(g) + e− D) S−(g) → S(g) + e− E) S2−(g) → S−(g) + e−

B

Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error? A) n = 2, l = 1, ml = +1 B) n = 4, l = 2, ml =0 C) n = 3, l =3, ml = -2 D) n = 1, l = 0, ml =0 E) n = 3, l = 0, ml =0

C

For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy? A) 2s → 3p B) 2p → 6d C) 6p → 4s D) 7f → 5d

C

Give the complete electronic configuration for Mn. A) 1s22s22p63s23p64s24d5 B) 1s22s22p63s23p64s13d6 C) 1s22s22p63s23p64s23d5 D) 1s22s22p63s23p64s24p5

C

Give the ground state electron configuration for Rb+. A) [Ar]4s24p6 B) [Kr]5s1 C) [Ar]4s23d104p6 D) [Kr]5s2 E) [Kr]5s24d2

C

Give the ground state electron configuration for Sr. A) [Kr]5s24d2 B) [Kr]5s24d105p2 C) [Kr]5s2 D) [Kr]5s25d105p2 E) [Kr]5s24d10

C

How many of the following elements have 1 unpaired electron in the ground state? B Al O F A) 1 B) 2 C) 3 D) 4

C

How many unpaired electrons are present in the ground state Kr atom? A) 1 B) 2 C) 0 D) 3 E) 5

C

Identify a characteristic of halogens. A) powerful reducing agents B) forms water in reactions C) powerful oxidizing agents D) absorbs water in reactions E) inert

C

Identify the element that has a ground state electronic configuration of [Ar]4s23d104p1. A) Al B) In C) Ga D) B

C

Only two electrons, with opposing spins, are allowed in each orbital is known as the A) Pauli exclusion principle B) Hund's rule C) Aufbau principle D) Heisenberg uncertainty principle

C

Place the following elements in order of increasing atomic radius. P Ba Cl A) Ba < P < Cl B) P < Cl < Ba C) Cl < P < Ba D) Cl < Ba < P E) Ba < Cl < P

C

Place the following in order of decreasing radius. Te2− F− O2− A)F− > O2− > Te2− B)F− > Te2− > O2− C) Te2− > O2− > F− D)Te2− > F− > O2− E) O2−>F−>Te2−

C

Place the following in order of increasing IE1. N F As A)N < As < F B) As < N < F C) F < N < As D)As < F < N E)F < As < N

C

The U.S. Food and Drug Administration recommends the ingestion of recommended doses of ________ in the event of a nuclear emergency. A) sodium bromide B) sodiuim chloride C) potassium iodide D) potassium bromide E) sodium iodide

C

The condensed electron configuration of silicon, element 14, is ________. A) [He]2s42p6 B) [Ne]2p10 C) [Ne]3s23p2 D) [He]2s4 E) [He]2s62p2

C

The element that corresponds to the electron configuration 1s22s22p63s23p64s13d5 is ________. A) titanium B) vanadium C) chromium D) manganese E) iron

C

The element that corresponds to the electron configuration 1s22s22p63s23p64s23d3 is ________. A) scandium B) manganese C) vanadium D) iron E) cobalt

C

What period 3 element having the following ionization energies (all in kJ/mol)? IE1 = 1012 IE2 = 1900 IE3= 2910 IE4= 4960 IE5= 6270 IE6 = 22,200 A) Si B) S C) P D) Cl E) Mg

C

Why don't we observe the wavelength of everyday macroscopic objects?

Due to the large mass of macroscopic objects, the deBroglie wavelength is extremely small. The wavelength is so small that it is impossible to detect compared to the size of the object.

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 4, l = 4, ml =0 B) n = 3, l = 2, ml =+3 C) n = 4, l = 0, ml =-1 D) n = 3, l = 1, ml = -2 E) n = 5, l = 3, ml =-3

E

Give the ground state electron configuration for Cd. A) [Kr]5s25d10 B) [Kr]5s24d105p2 C) [Kr]4d10 D) [Kr]5s24d8 E) [Kr]5s24d10

E

Give the ground state electron configuration for the ion of Ba. A) [Kr]5s25p6 B) [Kr]5s24d105p66s26p2 C) [Kr]5s24d105p66s1 D) [Kr]5s24d105p66s2 E) [Kr]5s24d105p6

E

Give the number of valence electrons for Se. A) 0 B) 8 C) 2 D) 4 E) 6

E

How many unpaired electrons are there in the ground state of Cl? A) 5 B) 4 C) 3 D) 2 E) 1

E

How many valence electrons do the halogens possess? A) 5 B) 6 C) 2 D) 1 E) 7

E

How many valence electrons do the noble gases possess? A) 1 B) 2 C) 7 D) 6 E) 8

E

Identify the correct values for a 4f sublevel. A) n = 3, l = 1, ml = 0 B) n = 2, l = 1, ml = 2 C) n = 1, l = 0, ml = 0 D) n = 2, l = 0, ml = 0 E) n = 4, l = 3, ml = -2

E

Identify the species that has the smallest radius. A) N-5 B) N-2 C) N0 D) N+1 E) N+3

E

Place the following in order of decreasing metallic character. P As K A)P > As > K B) As > P > K C) K > P > As D)As > K > P E)K > As > P

E

Place the following in order of increasing atomic radius. As O Br A) As < Br < O B) O < As < Br C) Br < As < O D) As < O < Br E) O < Br < As

E

The element that corresponds to the electron configuration 1s22s22p6 is ________. A) sodium B) magnesium C) lithium D) beryllium E) neon

E

Which reaction below represents the second ionization of Sr? A) Sr(g) → Sr+(g) + e− B) Sr2+(g) + e− → Sr+(g) C) Sr+(g) + e− → Sr(g) D) Sr−(g) + e− → Sr2−(g) E) Sr+(g) → Sr2+(g) + e−

E

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Sr atom. A) n = 5, l = 0, ml = 0, ms = -1/2 B) n = 4, l = 1, ml = 1 ms = -1/2 C) n = 5, l = 0, ml = 0, ms = +1/2 D) n = 4, l = 1, ml = -1, ms = +1/2 E) n = 5, l = 1, ml =1, ms = +1/2

A

No two electrons can have the same four quantum numbers is known as the A) Pauli exclusion principle B) Hund's rule C) Aufbau principle D) Heisenberg uncertainty principle

A

The complete electron configuration of argon, element 18, is ________. A) 1s22s22p63s23p6 B) 1s22s22p103s23p2 C) 1s42s42p63s4 D) 1s42s42p10 E) 1s62s62p23s4

A

Which of the following statements is TRUE? A) An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. B) An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy. C) It is possible for two electrons in the same atom to have identical values for all four quantum numbers. D) Two electrons in the same orbital can have the same spin. E) None of the above are true.

A

Which reaction below represents the electron affinity of Li? A) Li(g) + e− → Li−(g) B) Li(g) → Li+(g) + e− C) Li(g) + e− → Li+(g) D) Li+(g) → Li(g) + e− E) Li+(g) + e− → Li(g)

A

Choose the statement that is TRUE. A) Outer electrons efficiently shield one another from nuclear charge. B) Core electrons effectively shield outer electrons from nuclear charge. C) Valence electrons are most difficult of all electrons to remove. D) Core electrons are the easiest of all electrons to remove. E) All of the above are true.

B

For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1. A) 656.3 nm B) 486.2 nm C) 364.6 nm D) 2.057 × 10-3 nm

B

Give the ground state electron configuration for I. A) [Kr]5s24d105p6 B) [Kr]5s24d105p5 C) [Kr]4d105p6 D) [Kr]5s25p6 E) [Kr]5s25d105p6

B

Give the ground state electron configuration for Mg2+. A) 1s22s22p63s2 B) 1s22s22p6 C) 1s22s22p63s23p2 D) 1s22s22p63s23p6 E) 1s22s22p63s1

B

Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle) to the Zn atom. A) n = 4, l = 3, ml = 3, ms = +1/2 B) n = 3, l = 2, ml = 2, ms = -1/2 C) n = 3, l = 1, ml = 1, ms = -1/2 D) n = 3, l = 2, ml = 2, ms = +1/2 E) n = 4, l = 1 ml = 0, ms = +1/2

B

Choose the ground state electron configuration for Cr3+. A) [Ar]4s13d2 B) [Ar] C) [Ar]4s23d6 D) [Ar]3d3 E) [Ar]4s23d1

D

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. A) n = 2, l = 2, ml =+1 B) n = 2, l = 2, ml =0 C) n = 3, l = 2, ml =-3 D) n = 4, l = 3, ml =-2 E) n = 4, l = 2, ml =+4

D

Give the ground state electron configuration for Pb. A) [Xe]6s26p2 B) [Xe]6s25d106p2 C) [Xe]6s25f146d106p2 D) [Xe]6s24f145d106p2 E) [Xe]6s24f145d106s26p2

D

Give the ground state electron configuration for Se2−. A) [Ar]4s23d104p4 B) [Ar]4s23d104p2 C) [Ar]4s24p6 D) [Ar]4s23d104p6 E) [Ar]4s23d84p6

D

Give the number of valence electrons for Cd. A) 8 B) 10 C) 12 D) 2 E) 6

D

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle) to the Ne atom. A) n = 2, l = 1, ml = 1, ms = +1/2 B) n = 3, l = 0, ml = 1, ms = +1/2 C) n = 3, l = 2, ml =1, ms = +1/2 D) n = 2, l = 1, ml = 1, ms = -1/2 E) n = 3, l =2, ml = 1, ms = -1/2

D

How many of the following elements have 2 unpaired electrons in the ground state? C Te Hf Si A) 1 B) 2 C) 3 D) 4

D

How many orbitals are there in the fourth shell? A) 3 B) 4 C) 6 D) 16

D

How many unpaired electrons are present in the ground state C atom? A) 5 B) 3 C) 1 D) 2 E) 4

D

How many valence electrons does an atom of Al possess? A) 1 B) 2 C) 5 D) 3 E) 8

D

Identify the correct values for a 2p sublevel. A) n = 3, l = 1, ml = 0 B) n = 2, l = 1, ml = +2 C) n = 1, l = 0, ml = 0 D) n = 2, l = 1, ml = 0 E) n = 4, l = -1, ml = 0

D

Place the following in order of increasing IE1. K Ca Rb A)Ca < K < Rb B) Rb < Ca < K C) Ca < Rb < K D)Rb < K < Ca E)K < Ca < Rb

D

The condensed electron configuration of krypton, element 36, is ________. A) [Kr]4s23d8 B) [Ar]4s4 C) [Kr]4s43d8 D) [Ar]3d104s24p6 E) [Ar]4s43d4

D

What is the photoelectric effect?

Many metals emit electrons when light of high enough energy is shone on them. This observation brought the classical view of light into question.

Give the value of l for a 3p sublevel. A) 1 B) -4 C) -1 D) 2 E) -2

a

How many subshells are there in the shell with n = 4? A) 3 B) 4 C) 6 D) 18

b

In which orbital below would an electron (on average) be closest to the nucleus? A) 2p B) 4s C) 2s D) 5d E) 2p

c

identify the correct values for a 1s sublevel. A) n = 3, l = 1, ml = 0 B) n = 2, l = 1, ml = 1 C) n = 1, l = 0, ml = 0 D) n = 2, l = 0, ml =-1 E) n = 4, l = -1, ml = -2

c

Give an example of a d orbital.

dyz, dxy, dxz, dx2-y2, or dz2