Chem 111 Final Test review

8. Which of the intermolecular forces is the most important contributor to the high surface tension shown by water? A) dipole-dipole forces B) dispersion forces C) hydrogen bonding D) ion-dipole forces

C)

9. A 250. mL sample of gas at 1.00 atm and 20.0°C has the temperature increased to 40.0°C and the volume increased to 500. mL. What is the new pressure? A) 0.374 atm B) 0.468 atm C) 0.534 atm D) 1.87 atm

C)

8. A 65 mL sample of argon gas has a temperature of 325°C. What will the temperature be in °C when the volume of the gas is decreased to 25 mL at constant pressure? A) 65°C B) 125°C C) -43°C D) 1280°C

C) -43 C

9. A piece of metal ore weighs 8.25 g. When a student places it into a graduated cylinder containing water, the liquid level rises from 21.25 mL to 26.47 mL. What is the density of the ore? (4 points) A) 0.3 12 g/mL B) 0. 633 g/mL C) 1. 58 g/mL D) 3.21 g/mL

C) 1.57 g/ml

1. What is the molar mass of aspartic acid, C4O4H7N? A) 43 g/mol B) 70 g/mol C) 133 g/mol D) 197 g/mol

C) 133

3. What is the mass of 8.50 × 1022 molecules of NH3? A) 0.00830 g B) 0.417 g C) 2.40 g D) 120 g

C) 2.40g

5. A sailor circumnavigated the earth and covered 4,264,000 meters. Express this number in standard scientific notation. A) 4.264 × 10^-7 m B) 4.264 × 10^-6 m C) 4.264 × 10^6 m D) 4.264 × 10^7 m

C) 4.264 * 10^6

13. A mixture of the gases N2, O2, and He has a total pressure of 760 mm Hg. If the partial pressure of N2 is 90 mm Hg and of O2 is 270 mm Hg, what is the partial pressure of He? A) 1120 mm Hg B) 760 mm Hg C) 400 mm Hg D) 360 mm Hg

C) 400mmHg

19. Which group of elements are found as diatomic molecules? A) alkali metals B) alkaline earth metals C) halogens D) noble gases

C) halogens

2. To simplify comparisons, the energy value of fuels is expressed in units of A) kcal. B) kcal/mol. C) kcal/g. D) kcal/L.

C) kcal/g

2. The number of orbitals in a given subshell, such as the 5d subshell, is determined by the number of possible values of (2 points) A) n. B) l. C) ml. D) ms.

C) ml

3. The combustion reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) can be classified as a(n) (2 points) A) acid-base neutralization reaction. B) double replacement reaction. C) oxidation-reduction reaction. D) precipitation reaction.

C) oxidation-reduction reaction

2. The reaction Na3PO4(aq) + 3 AgNO3(aq) → Ag3PO4(s) + 3 NaNO3(aq) is best classified as a(n) (2 points) A) acid-base neutralization reaction. B) oxidation-reduction reaction. C) precipitation reaction. D) single replacement reaction.

C) precipitation reaction

6. The nighttime and daytime temperatures on Mercury are 13 K and 683 K respectively. The melting point and boiling point of sulfur is 246°F and 832°F. Which of the following statements is true? On Mercury sulfur exists A) only in the liquid state. B) only in the solid state. C) as both a liquid and a gas. D) as both a liquid and a solid.

D) as both a liquid and a solid

A sample of gas has a volume of 135 mL at 0.600 atm. What would be the volume if the pressure is decreased to 0.200 atm while temperature is held constant? A) 45.0 mL B) 135 mL C) 180 mL D) 405 mL

D)

4. How many oxygen atoms are in 3.00 g of sodium dichromate, Na2Cr2O7? A) 0.0801 oxygen atoms B) 9.85 × 1020 oxygen atoms C) 6.90 × 1021 oxygen atoms D) 4.83 × 1022 oxygen atoms

D) 4.83*10^22

10. Which of the following compounds is an Arrhenius base in water? A) CH3OH B) CH3CO2H C) HOCl D) KOH

D) KOH

7. In which of the following sets do all species have the same number of protons? A) Br-, Kr, Sr2+ B) C, N3-, O2- C) Mg2+, Sr2+, Ba2+ D) O, O2-, O2+

D) O,O2-,O2+

1. Consider the reaction shown: C3H8 + 5 O2 → 3 CO2 + 4 H2O + 488 kcal We can say that this reaction is ________ and that the sign of ΔH is ________. A) endothermic; positive B) exothermic; positive C) endothermic; negative D) exothermic; negative

D) exo, negative

12. Which of the following is not a state function? A) altitude B) heat C) internal energy D) volume

B) heat

12. What is the molecular geometry of AsCl3? A) T-shaped B) tetrahedral C) trigonal planar D) trigonal pyramidal

D)

8. Which of the following have the same number of valence electrons? A) K, As, Br B) B, Si, As C) N, As, Bi D) He, Ne, F

C)

15. Which ionization process requires the most energy? A) P(g) → P+(g) + e- B) P+(g) → P2+(g) + e- C) P2+(g) → P3+(g) + e- D) P3+(g) → P4+(g) + e-

D)

17. Which species does not have an octet of electrons for its outer core? A) C4- B) P3- C) O2- D) Mg+

D)

9. The property of a liquid that measure the liquid's resistance to flow is A) boiling point. B) heat of vaporization. C) surface tension. D) viscosity.

D)

9. Which one of the following is expected to exhibit resonance? A) NH4+ B) HCN C) CO2 D) NO2-

D)

7. Identify the following as redox or non-redox reactions. Support your answer with oxidation numbers. i) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2 KNO3 (aq)

+2, +5, -2 +1, +6, -2 +2, +6, -2 +1, +5, -2 Redox reaction? ____no___________ Species reduced: _____ none_________ Species oxidized: ____ none__________

2 SO2 (g) + O2 (g) → 2 SO3 (g)

+4, -2 0 +6, -2 Redox reaction? _______ yes___________ Species reduced: O2 to O(2-) (in SO3)_ Species oxidized: S(+4) (in SO2) to S(+6) (in SO3)_

8. Determine the oxidation state for sulfur in each of the following compounds. Show your work or provide your reasoning for each compound. S8 H2S SO2 H2SO3

0 -2 +4 +4

9. Determine the oxidation number for each atom in the following compounds: Show your work. MgSO3 Al(NO2)3

2+,4+,2- 3+,3+,2-

10. Because of the high heat and low humidity in the summer in Death Valley, California, a visitor requires about one quart of water for every two miles traveled on foot. Calculate the approximate number of liters required for a person to walk 10. kilometers in Death Valley. (4 points) A) 2.9 L B) 12 L C) 30 L D) 47 L

2.9L

7. If heat is consumed during a reaction, the reaction is said to be ________. A) endothermic B) exothermic C) endergonic D) exothermic

A) endo

11. Methane and oxygen react to form carbon dioxide and water. What mass of water is formed if 3.2 g of methane reacts with 12.8 g of oxygen to produce 8.8 g of carbon dioxide? A) 7.2 g B) 8.8 g C) 14.8 g D) 16.0 g

7.2g A)

6. A reaction is said to be ________ if the bonds formed during the reaction are stronger than the bonds broken. A) exothermic B) endothermic C) exergonic D) spontaneous

A) exo

1. The scientific principle which explains the observation that the amount of heat transfer accompanying a change in one direction is numerically equal but opposite in sign to the amount of heat transfer in the opposite direction is A) the Law of Conservation of Energy. B) the Law of Conservation of Mass. C) the Law of Conservation of Mass and Energy. D) the Law of Definite Proportions.

A)

12. What is the ground-state electron configuration of the ion Hg2+? A) [Xe]4f145d10 B) [Xe]4f145d86s2 C) [Xe]4f145d106s2 D) [Xe]4f145d106s26p2

A)

4. Which of the following molecules does not have a dipole moment? A) CH2=CH2 B) NH3 C) CH3NH2 D) HCl

A)

5. The mixing of which pair of reactants will result in a precipitation reaction? (2 points) A) Cu(NO3)2(aq) + Na2CO3(aq) B) K2SO4(aq) + Cu(NO3)2(aq) C) NaClO4(aq) + (NH4)2S(aq) D) NH4Br(aq) + NaI(aq)

A)

6. Which of the following represent electron configurations that are allowed but do not represent ground-state configurations? (A) [Ne]3s13p5 (B) [Kr]4d125s25p3 (C) [Ar]3d104s24p2 A) only (A) B) only (B) C) (A) and (B) D) (B) and (C)

A)

7. What is the ground-state electron configuration of tellurium? A) [Kr]4d105s25p4 B) [Kr]5s25p65d8 C) [Kr]5s25p4 D) [Kr]4f144d105s25p4

A)

9. For the reaction given below, what quantity of heat will be produced if 90.0 g of C3H8 are consumed in the reaction? C3H8 + 5 O2 → 3 CO2 + 4 H2O + 488 kcal A) 996 kcal B) 488 kcal C) 332 kcal D) 239 kcal

A)

Which is not a correct statement of Charles's Law? A) For a gas sample at constant pressure, temperature and volume are inversely proportional. B) volume α temperature C) V/T = a constant D) v1/t1 = v2/t2

A)

1. According to the balanced equation shown below, 1.00 mole of oxalic acid, H2C2O4, reacts with ________ moles of permanganate ion, MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) A) 0.400 B) 1.00 C) 2.00 D) 2.25

A) .4

2. What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change in temperature? A) 190 mm Hg B) 380 mm Hg C) 570 mm Hg D) 760 mm Hg

A) 190mmHg

5. In which of the following sets do all species have the same number of electrons? A) Br-, Kr, Sr2+ B) C, N3-, O2- C) Mg2+, Sr2+, Ba2+ D) O, O2-, O2+

A) Br-,Kr,Sr2+

6. What is the empirical formula of a substance that contains 2.64 g of C, 0.444 g of H, and 3.52 g of O? A) CH2O B) C2H4O2 C) C2H4O3 D) C3H4O4

A) CH2O

14. Which is a measure of the sum of the kinetic and potential energies of each particle in the system? A) E, the internal energy B) G, the Gibbs free energy C) H, the enthalpy D) T, the temperature

A) E

1. The reaction HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l) is best classified as a(n) (2 points) A) acid-base neutralization reaction. B) oxidation-reduction reaction. C) precipitation reaction. D) single replacement reaction.

A) acid-base neutralization reaction

4. Of the following elements, which has the highest electronegativity? A) P B) S C) Sc D) As

B) S

1. Volume and pressure are ________ proportional. A) directly B) inversely C) all of the above D) none of the above

B)

13. Which two ions have the same electron configuration in the ground state? A) Rb+ and Cs+ B) Ba2+ and I- C) Se2+ and I- D) Fe2+ and Fe3+

B)

14. List the elements Cs, Ca, Ne, Na, Ar in order of decreasing first ionization energy. A) Ar > Ca > Cs > Na > Ne B) Ne > Ar > Ca > Na > Cs C) Ne > Ar > Na > Cs > Ca D) Ne > Na > Cs > Ca > Ar

B)

16. Which combination always results in a reaction being spontaneous? A) ΔH is negative and ΔS is negative. B) ΔH is negative and ΔS is positive. C) ΔH is positive and ΔS is negative. D) ΔH is positive and ΔS is positive.

B)

18. Predict the product(s) when the reactants Be(s) + Br2(l) are mixed. A) BeBr(s) B) BeBr2(s) C) Be2Br(s) D) BeBr3(s)

B)

2. Which electrostatic forces hold atoms together in a molecule? A) electron-electron forces B) electron-nucleus forces C) nucleus-nucleus forces D) all three forces

B)

5. Consider the reaction shown: N2 + O2 → 2 NO ΔH = 43.2 kcal When 50.0 g of N2 react, ________ kcal will be ________. A) 43.2; produced B) 77.1; consumed C) 77.1; produced D) 2160; consumed

B)

7. Which is expected to have the largest dispersion forces? A) C2H6 B) C8H18 C) N2 D) CO2

B)

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

B)

5. How many lone pairs of electrons are on the P atom in PF3? A) 0 B) 1 C) 2 D) 3

B) 1

7. How many lone pairs of electrons are on the Xe atom in XeF6? A) 0 B) 1 C) 2 D) 3

B) 1

2. What is the mass of a single chlorine molecule, Cl2? A) 5.887 × 10-23 g B) 1.177 × 10-22 g C) 35.45 g D) 70.90 g

B) 1.177*10^-22g molar mass/6.02*10^23

1. How many protons (p), neutrons (n), and electrons (e) are in one atom of ? A) 12 p, 12 n, 12 e B) 12 p, 11 n, 12 e C) 12 p, 11 n, 10 e D) 12 p, 11 n, 14 e

B) 12p,11n,12e

12. How many grams of O2 are contained in a 25.0 L sample at 5.20 atm and 28.0°C? A) 1810 g B) 168 g C) 84.2 g D) 5.26 g

B) 168g

8. How many resonance structures are required in the electron-dot structure of CO32-? A) two B) three C) four D) five

B) 3

5. How many anions are in 0.500 g of MgBr2? A) 1.64 × 1021 anions B) 3.27 × 1021 anions C) 2.22 × 1026 anions D) 4.43 × 1026 anions

B) 3.27*10^21 anions

7. Which one of the following is an empirical formula? A) C2F6 B) H2SO4 C) N2H4 D) P4O10

B) H2SO4

6. In which set do all elements tend to form cations in binary ionic compounds? A) Li, B, O B) Mg, Cr, Pb C) N, As, Bi D) O, F, Cl

B) Mg,Cr,Pb

4. Water (H2O), methyl alcohol (CH3OH), ethyl alcohol (CH3CH2OH), ethylene glycol (HOCH2CH2OH), and sucrose (C12H22O11) are commonly classified as (2 points) A) bases. B) nonelectrolytes. C) strong electrolytes. D) weak electrolytes.

B) non-electrolytes

1. What are the possible values of l if n = 5? A) 5 B) 0, 1, 2, 3, or 4 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)0,1,2,3,4

1. What is the oxidation half reaction in the following chemical reaction? Cr2O72-(aq) + 6 Cl-(aq) + 14 H+(aq) → 2 Cr3+(aq) + 3 Cl2(aq) + 7 H2O(l) A) Cr2O72-(aq) + 14 H+(aq) + 6e- → 2 Cr3+(aq) + 7 H2O(l) B) Cr2O72-(aq) + 14 H+(aq) → 2 Cr3+(aq) + 7 H2O(l) + 6e- C) 2 Cl-(aq) → Cl2(aq) + 2e- D) Cl2(aq) + 2e- → 2 Cl-(aq)

C)

10. A sample of helium has a volume of 480 mL at 47.0°C and 740 mm Hg. The temperature is lowered to 22.0°C and the pressure to 625 mm Hg. What is the new volume? A) 266 mL B) 373 mL C) 524 mL D) 616 mL

C)

10. Entropy is used to A) explain how energy is stored. B) explain how an exothermic reaction can become endothermic. C) indicate the disorder of a system. D) explain why most chemical reactions are exothermic.

C)

10. What geometric arrangement of charge clouds is expected for an atom that has five charge clouds? A) tetrahedral B) square planar C) trigonal bipyramidal D) octahedral

C)

11. How many grams of N2 are contained in an 11.2 liter sample at STP? A) 7.00 B) 11.2 C) 14.0 D) 28.0

C)

11. Which of the following is not a type of energy or energy transfer? A) chemical energy B) heat C) temperature D) work

C)

12. Which element has the ground-state electron configuration [Xe]6s25d14f7? A) Pt B) Eu C) Gd D) Tb

C)

13. The first law of thermodynamics A) defines chemical energy. B) defines entropy. C) is a statement of conservation of energy. D) provides a criterion for the spontaneity of a reaction.

C)

15. What is expected when the reaction shown below takes place in a thermally-insulated container outfitted with a movable piston at a constant atmospheric pressure of 1 atm? 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) A) Volume will decrease and work will be done by the system. B) Volume will decrease and work will be done on the system. C) Volume will increase and work will be done by the system. D) Volume will decrease and work will be done on the system.

C)

16. Which of the following atoms with the specified electronic configurations would have the lowest first ionization energy? A) [He]2s22p3 B) [Ne]3s23p4 C) [Xe]6s1 D) [Xe]6s24f145d106p1

C)

17. For the conversion of water to ice at 25°C and 1 atm, A) ΔG is negative and ΔH is negative. B) ΔG is negative and ΔH is positive. C) ΔG is positive and ΔH is negative. D) ΔG is positive and ΔH is positive.

C)

3. N2 + O2 → 2 NO ΔH = 43.2 kcal Based on the reaction shown, which statement is true? A) 43.2 kcal are consumed when 1.00 g of N2 reacts. B) 43.2 kcal are consumed when 1.00 g of O2 reacts. C) 43.2 kcal are consumed when 1.00 mole of O2 reacts. D) 43.2 kcal are produced when 1.00 mole of NO is produced.

C)

3. Which has a dipole moment? A) CO2 B) CO32- C) SO2 D) SO42-

C)

5. A sealed container with gas at 2.00 atm is heated from 20.0 K to 40.0 K. The new pressure is A) 0.500 atm. B) 1.00 atm. C) 4.00 atm. D) 2.14 atm.

C)

5. Molybdenum has an anomalous electron configuration. Write the electron configuration of Mo using shorthand notation. A) [Kr] 5s0 4d6 B) [Kr] 5s0 4d0 5p6 C) [Kr] 5s1 4d5 D) [Kr] 5s2 4d4

C)

5. Which has the smallest dipole-dipole forces? A) CH3F B) HCl C) N2 D) CO

C)

6. If the temperature of a 1.75 liter sample of gas is changed from 30.0°C to 20.0°C at constant pressure, what will be the new volume? A) 1.17 L B) 1.57 L C) 1.69 L D) 1.81 L

C)

6. Which reaction is an example of both a precipitation and a neutralization? A) H3PO4 (aq) + 3 KOH (aq) → K3PO4 (aq) + 3 H2O (l) B) (NH4)2CO3 (s) → 2 NH3 (g) + CO2 (g) + H2O (l) C) H2SO4 (aq) + Ba(OH)2 (aq) → BaSO4 (s) + 2 H2O (l) D) 2 C (s) + O2 (g) → 2 CO (g)

C)

1. Elements in a periodic group have similar A) chemical properties. B) densities. C) masses. D) physical properties.

Chemical properties

3. What are the possible values of n and ml for an electron in a 5d orbital? (2 points) A) n = 1, 2, 3, 4, or 5 and ml = 2 B) n = 1, 2, 3, 4, or 5 and ml = -2, -1, 0, +1, or +2 C) n = 5 and ml = 2 D) n = 5 and ml = -2, -1, 0, +1, or +2

D)

4. Consider the reaction shown: P4 (s) + 10 Cl2 (g) → 4 PCl5 (s) + 452 kcal When 50.00 g of P4 react, ________ kcal will be ________. A) 182.4; consumed B) 452; produced C) 729.7; produced D) 182.4; produced

D)

4. Which of the following is not a valid set of quantum numbers? (2 points) A) n = 2, l = 1, ml = 0, and ms = -1/2 B) n = 2, l = 1, ml = -1, and ms = -1/2 C) n = 3, l = 0, ml = 0, and ms = 1/2 D) n = 3, l = 2, ml = 3, and ms = 1/2

D)

6. Which of the following compounds exhibits hydrogen bonding? A) CH3Cl B) HI C) H3C-O-CH3 D) NH3

D)

7. What will be the new volume when 128 mL of gas at 20.0°C is heated to 40.0°C while pressure remains unchanged? A) 64.0 mL B) 120. mL C) 128 mL D) 137 mL

D)

8. Entropy can be defined as A) the amount of energy required to rearrange chemical bonds. B) the amount of energy required to initiate a reaction. C) the number of chemical bonds which are changed during a reaction. D) the amount of disorder in a system.

D)

1. The bonds in the polyatomic ion CO32- are classified as A) ionic B) metallic C) nonpolar covalent D) polar covalent

D)

2. Consider the reaction shown: 2 CO (g) + O2 (g) → CO2 (g) + 135.2 kcal This reaction is ________ because the sign of ΔH is ________. A) endothermic; positive B) exothermic; positive C) endothermic; negative D) exothermic; negative

D) exo, negative

1. Covalent bonding is a A) gain of electrons. B) loss of electrons. C) transfer of electrons. D) sharing of electrons.

D) sharing of electrons

3. Which group of elements reacts violently with water? A) halogens B) noble gases C) alkali metals D) alkaline earth metals

alkali metals

4. Which of the following elements is classified as a semimetal? \ A) calcium B) germanium C) fluorine D) uranium

germanium

2. Which of the following underlined items is not an extensive property? A) the color of a cobalt compound B) the diameter of a soap bubble C) the mass of a diamond D) the volume of a glucose solution

the color of a cobalt compound