Chem 1320 Final Exam (Multiple Choice)

The N--H bonds in the following compound are ______ and is formed from the_______. CH3-----::N------H | H A) σ bond; sp2--s orbital overlap B) σ bond; sp3--s orbital overlap C) π bond; sp3--s orbital overlap D) π bond; sp2--p orbital overlap E) π bond; p--p orbital overlap

B) σ bond; sp3--s orbital overlap

Which of the following substance is a strong acid? A) H2CO3 B) H3PO4 C) CH3COOH D) HNO3 E) NH3

D) HNO3

What is the mass of 4.5*10^22 Cu atoms? A) 7.47*10^-2 amu B) 63.55 amu C) 7.47*10^-2 g D) 63.55 g E) 4.75 g

E) 4.75 g 4.50*10^22 atoms *(1 mole/6.022*10^23)*(63.55g/1mole)= 4.75 grams

Which of the following compounds is ionic? A) P2O5 B) SOCl2 C) H2O D) HCl E) MgBr2

E) MgBr2

Sodium thiosulfate, Na2S2O3, is used as a "fixer" in black and white photography. Identify the reducing agent in the reaction of thiosulfate with iodine. 2S2O3^2-(aq) + I2(aq) --> S4O6^2-(aq) + 2I^-(aq) A) I^- (aq) B) S4O6^2- (aq) C) I2 (aq) D) S2O3^2- (aq) and I^- (aq) E) S2O3^2 (aq)

E) S2O3^2 (aq)

Which is the correct formula for copper(II) phosphate? A) Cu3(PO4)2 B) Cu(PO4)2 C) Cu(PO3)2 D)Cu2PO3 E) Cu2PO4

A) Cu3(PO4)2

1 barrel of oil contains 42.0 gallons. How many liters is this? (1L=1.06 qt and 4 qt=1 gallon) A) 142 L B) 158 L C) 178 L D) 9.9 L E) 11 L

B) 158 L 42.0 gallons * (4qt/1 gallon) * (1 liter/1.06 qt)

Which compound will exhibit hydrogen bonding? A) CH2F2 B) Cl2NH C) H2PCl D) HBr E) NCl3

B) Cl2NH

Which one of the following is a redox reaction? A) H2O (l) --> H^+ (aq) + OH^- (aq) B) Na2CO3(s) + 2HCl(aq) --> NaCl(aq) + CO2(g) + H2O(l) C) Na^2+(g) + SO4^2-(aq) --> BaSO4(s) D) 2Na (g) + Cl2 (g) --> 2NaCl (s) E) K2Cr2O7(aq) + 2KOH(aq) --> 2K2CrO4(aq) + H2O(l)

D) 2Na (g) + Cl2 (g) --> 2NaCl (s)

How many significant figures does the result of the following operation contain? 8.52010 * 7.90 A) 4 B) 2 C) 6 D) 3 E) 5

D) 3 The first number has 6 sig figs and the second number has 3 sig figs. In multiplication when choosing sig figs, you choose the least amount of sig figs that any of the numbers has.

Which response includes all the molecules below that do not follow the octet rule (1) H2S (2) BCl3 (3) PH3 (4) SF4 A) (2) and (4) B) (2) and (3) C) (1) and (2) D) (3) and (4) E) (1) and (4)

A) (2) and (4) (1) H--:S:--H follows octet rule (2) :::Cl--B--Cl::: | B does not follow octet rule (missing 2) Cl::: (3) H--:P--H | follows octet rule H (4) F::: | F:::--:S--F::: S does not follow octet rule (extra 2) | F:::

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron =1.675*10^-24 g) A) 160 nm B) 1.6 pm C) 0.016 nm D) 1.6*10^-4 m E) 0.16 nm

A) 160 nm

Which of the following wavelengths of electromagnetic radiation has the highest energy? A) 3.50*10^-9 m B) 8.40*10^-7 m C) 225 nm D) 2.50*10^-5 m E) 450. nm

A) 3.50*10^-9 When solving this problem there are two steps, making sure that they have the same units and the picking the smallest number which means it has the highest energy. Looking at A, B, and D, you can eliminate B and D since A is a smaller number than it. If you then convert A to nanometers, you get 3.5 nanometers which is smaller than both C and E mean A is the final answer.

An element A combines with Fluorine to form an ionic compound having the formula AF3. What is the formula of the ionic compound formed between sulfur and A? A) A2S3 B) A3S2 C) AS3 D) A3S E) AS

A) A2S3 Fluorine always has a negative 1 charge. so therefore in the compound AF3, A would have a positive 3 charge. Sulfur always has a negative 2 charge. with this information you can conclude that A would have a 2 subscript and S would have a 3 subscript.

Predict the formula for the ionic compound formed between barium and phosphorus. A) Ba3P2 B) Ba2P3 C) Ba2P D) BaP E) BaP2

A) Ba3P2

Which of the following gases will be the slowest to diffuse through a room? A) Carbon dioxide, CO2 B) methane, CH4 C) water, H2O D) neon, Ne E) hydrogen sulfide, H2S

A) Carbon dioxide, CO2

Select the net ionic equation for the reaction between sodium chloride and mercury (1) nitrate. 2NaCl (aq) + Hg2(NO3)2 (aq) --> NaNO3 (aq) + Hg2Cl2 (s) A) Hg2^2+(aq) + 2 Cl^- (aq) --> Hg2Cl2(s) B) NaCl (aq) --> Na^+ (aq) + Cl^- (aq) C) Hg2^2+ (aq) --> Hg2(s) D) Na^+ (aq) + NO3^- (aq) --> NaNO3 (aq) E) Hg2(NO3)2 (aq) --> Hg2^2+ (aq) + 2NO3-(aq)

A) Hg2^2+(aq) + 2 Cl^- (aq) --> Hg2Cl2(s)

Which of the following has a ΔHf=0 Kj/mol? A) N2 (g) B) H2O (l) C) NO (g) D) Fe^+2 (aq) E) CS2 (l)

A) N2 (g)

Which ground-state atom has an electron configuration described by the following orbital diagram? [Ar] ^v ^v ^v ^v ^v ^v ^v ^ ^ 4s 3d 4p A) Selenium B) Tellurium C) Germanium D) Phosphorus E) None of these

A) Selenium

Which of the following processes always results in an increase in then energy of the system? A) the system gains heat and has work done on it by the surroundings. B) the system loses heat and does work on the surroundings. C) the system gains heat and does work on the surroundings. D) the system loses heat and has work done on it by the surroundings. E) None of these is always true.

A) the system gains heat and has work done on it by the surroundings.

A molecule has a central atom surround by 2 lone pairs and atoms. Geometry about the central atom is: A) trigonal bipyramidal B) octahedral C) trigonal planar D) T-shaped E) see-saw Hint: choose two

A) trigonal bipyramidal D) T-shaped

1.0 M aqueous solutions of the following substances are prepared. Which one would you expect to have the lowest electrical conductivity? A) CH3CH2OH (ethanol) B) KBr C) HClO4 D) NaOH E) CH3COOH (acetic acid)

A)CH3CH2OH

What is the formal charge on the oxygen atom in N2O? A) -2 B) -1 C) 0 D) +1 E) +2 Hint: the structure is linear and the atoms are arranged in the following order: NNO)

B) -1 :N triple bond (N+)---(O-):::

In a chemical equation, C2H6O + PCl3 --> C2H5Cl + H3PO3, when the reaction was carried out, the actual yield of C2H5Cl was calculated as 97.3% of the theoretical value. If the theoretical yield should have been 2.04 moles how many grams of C2H5Cl were actually obtained? A) 123 grams B) 128 grams C) 132 grams D) 135 grams E) 138 grams

B) 128 grams 2.04 moles of C2H5Cl *(64.52 grams of C2H5Cl/1 mole of C2H5Cl)= 131.62 grams of C2H5Cl 131.62 grams of C2H5Cl * 97.3%=128 grams

Complete the following chart, in order from left to right Isotope~Mass Number~Protons~Neutrons~Electron~ ^14 N ? ? ? ? A) 7, 7, 7, 7 B) 14, 7, 7, 7 C) 7, 14, 7, 7 D) Some Other Answer E) 14, 7, 14, 7

B) 14, 7, 7, 7

A sample of carbon dioxide gas at 125 degrees C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increase to 321 L at 125 degrees C? A) 359 torr B) 212 torr C) 289 torr D) 356 torr E) 441 torr

B) 212 torr since the temperature does not change it does not need to be considered in the formula PV/T=PV=T 248 torr*275 L= P* 321 L 212.46 torr=P

The number of pi bonds in the molecule below is H H | | H--C (triple) C--C--C--C (triple) C--H | | H H A) 2 B) 4 C) 6 D) 10 E) 15

B) 4 there is 1 pi bond for each double bond and 2 pi bonds for each triple bond

What mass of C6H12O6 (glucose) is needed to prepare 450 mL of a 0.650 M solution of glucose in water? A) 0.692 g B) 52.7 g C) 293 g D) 125 g E) 0.293 g

B) 52.7 g the molarity solution can be rewritten as .65moles/L. After rewriting it you can cross multiply .65 moles/L=X moles/.45L you get .2925 moles which you then need to covert into grams by multiplying it by the molar mass of glucose (180.16 g/ mole) which gives you 52.7 grams

PbS is heated in air to form lead (II) oxide. What mass of Pbs is converted to lead (II) oxide if 975 kJ of heat are liberated? 2PbS(s) + 3O2(g) --> 2PbO(s) + 2SO2(g) ΔH=-827.4 kj A) 282 g B) 564 g C) 203 g D) 406 g E) 478 g

B) 564 g

13. Calculate the average atomic mass of element X using the following data: Isotope--Abundance--Mass ^6 X 7.5% 6.0151 amu ^7 X 92.5% 7.0160 amu A) 6.02 amu B) 6.94 amu C) 6.50 amu D) 6.51 amu E) 7.02 amu

B) 6.94 amu

Arrange the following ions in creasing ionic radius: Al^3+, Mg^2+, Na^+, O^2- A) Al>Mg>Na>O B) O>Na>Mg>Al C) Al>Mg>O>Na D) Na>Mg>Al>O E) O>Al>Mg>Na

B) O^2-, Na^+, Mg^2+, Al^3+

The strongest intermolecular forces experienced between molecutes of nitrogen monoxide are: A) covalent bonds B) dipole-dipole interactions C) ionic bonds D) hydrogen bonds E) London Forces

B) dipole-dipole interactions

Ibuprofen is used as an analgesic for relief of pain, and also to help reduce fever. What i the hybridization state of carbon indicated by the arrow in the structure of ibuprofen shown below? CH---:C===O: | OH A) sp B) sp2 C) sp3 D) sp3d E)sp3d2

B) sp2 count the electron areas around the carbon. You get 3. so you have 1 s and 2 p.

Given H2(g) + 1/2O2(g) --> H2O(l), ΔH=-286 kJ/mole, deterimine the standard enthalpy change for the reaction 2H2O (l) -->2H2(g) + O2(g). A) ΔH= -572 kJ/mol B) ΔH= +573 kJ/mol C) ΔH= +286 kJ/mol D) ΔH= -143 kJ/mol E) ΔH= -286 kJ/mol

B) ΔH= +573 kJ/mol

Cold packs, whose temperatures are lowered when ammonium nitrate dissolves in water, are carried by athletic trainers when transporting ice is not possible. Which of the following is true of this reaction? A) ΔH=0, since cold packs are sealed B) ΔH>0, process is endothermic C) ΔH>0, process is exothermic D) ΔH<0, process is exothermic E) ΔH<0, process is endothermic

B) ΔH>0, process is endothermic

How many resonance structures can be drawn for ozone? A) 1(ozone does nor display resonance) B) 2 C) 3 D) 4 E) 5

B)2 1st: :::O---:O===O:: 2nd: ::O===O:---O:::

A system delivers 1275 J of heat while the surrounding perform 855 J of work on it. Calculate ΔU in J. A) 420 J B) -1275 J C) -420 J D) -2130 J E) 2130 J

C) -420 J Performing work means that it is positive 855. and giving off the 1275 makes it negative.

In a chemical reaction, C2H6O + SOCl2 --> C2H5Cl + H2SO3, when the equation is balanced the sum of the coefficients of the reactants and products should be A) 4 B) 5 C) 6 D) 7 E) 8

C) 6 you first have to balance the equation. which would make it 2(C2H6O) + SOCl2 --> 2(C2H5Cl) + H2SO3. Then add them up 2+1+2+1=6

How many valence electrons does S^2- have? A) 6 B) 16 C) 8 D) 2 E) 4

C) 8

Which of the following make an isoelectronic pair: Cl^-, O^2-, F, Ca^2+, Fe^3+ A) O and F B) F and Cl C) Cl and Ca D) Ca and Fe E) None of these

C) Cl^- and Ca^2+

Arrange the following in terms of increasing electronegativity values. Ga, P, As, Ge A) P<Ga<Ge<As B) As<P<Ga<Ge C) Ga<Ge<As<P D) Ge<P<As<Ga E) Ga<P<As<Ge

C) Ga<Ge<As<P Ga=1.6 Ge=1.8 As=2.0 P=2.1

Which of the following ionic solids would have the largest lattice energy? A) KF B) KI C) LiF D) LiI E) NaF

C) LiF

For which of the following reactions is the enthalpy change equal to the third ionization energy of vanadium? A) V^3+(g) + e^-1 --> V^2+(g) B) V^3+(g) --> V^4+ (g) +e^-1 C) V^2+(g) --> V^3+(g) +e^-1 D) V(g) --> V^3+(g) +3e^-1 E) V^2-(g) + e^- --> V^3-

C) V^2+(g) --> V^3+(g) + e^-

Which element has the following ground-state electron configuration? [Xe] 6s2 4f14 5d4 A) Re B) Mo C) W D) Pm E) Np

C) W Go to Xe then start at the next row and count over 20 elements.

Which of the following elements is chemically similar to magnesium? A) iron B) nickel C) calcium D) potassium E) sulfur

C) calcium This is because it is in the same column.

An endothermic reaction causes the surroundings to A) release CO2 B) warm up C) decrease in temperature D) become acidic E) condense

C) decrease in temperature

A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0 degrees C. How many moles of nitrogen are in the container? A) 2.27 mol B) 3.69 mol C) 227 mol D) 0.271 mol E) 206 mol

D) 0.271 moles First we need to convert the pressure and the temp to the correct units. 375 torr*(1 atm/760 torr)= 0.493 atm 37.0 degrees C +273= 310 degrees K use the equation PV=nRT. solve for n (0.493 atm)*(14.0 L)= n*0.0821 (L*atm)/(mole*k)*310 K 6.902 L*atm = n*25.451 L*atm/mole 0.271 mole=n

the molar mass of Ni(H2O)6Cl2 is A) 157.69 g B) 193.00 g C) 227.61 g D) 237.69 g E) 296.83 g

D) 237.69 gram

What are the conditions of STP? A) 273.15 degrees C and 760 torr B) 0 degrees C and 760 atm C) 0 degrees K and 1 atm D) 273.15 degrees K and 760 torr E) None of these choices is correct

D) 273.15 degrees K and 760 torr

Based on the Lewis structure the number of electron domains around the arsenic atom in the AsCl3 molecule is A) 1 B) 2 C) 3 D) 4 E) 5

D) 4 Cl::: | :Al---Cl::: | Cl:::

The correct name for NH4NO3 is A) hydrogen nitrate B) hydrogen nitrogen oxide C) ammonium nitrogen trioxide D) ammonium nitrate E) ammonia nitrogen oxide

D) Ammonium Nitrate

Which of the following atoms has the greatest electron affinity (largest positive value)? A) Ga B) S C) Li D) Br E) P

D) Br It is the element that is lowest and farthest to the right on the periodic table.

The effective nuclear charge (Zeff) felt by the outermost electrons is the strongest for which of the following elements? A) P B) Al C) D D) Cl E) Si

D) Cl It the element that is farthest to the right for these five elements.

Which bond is the most polar? A) H---C B) H---N C) H---P D) H---O E) H---Se

D) H---O

List all types of bonding present in the compound CaCO3 I. Ionic Bond II. Polar covalent bond III. nonpolar covalent bond A) I only B) II only C) III only D) I and II E) II and III

D) I and II Ca-C bond: 1.5---Ionic Bond C-O bond: 1---Polar Covalent Bond

The oxidation numbers of P, S and Cl in H2PO2^-, H2S and KClO4 are , respectively A) -1, -2, +3 B) +1, +2, +7 C) -1, -2, +7 D) -1, -1, +3 E) +1, -2, +7

E) +1, -2, +7

A standard solution of 0.243 M NaOH was used to determine the concentration of a hydrochloric acid solution. If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid what is the molar concentration of the acid? A) 0.888 M B) 2.43 M C) 2.26 M D) 0.0524 M E) 1.13 M

E) 1.13

What is the energy in joules of a mole of photons associated with red light of wavelength 7.00*10^2 nm? A) 12.4 kJ B) 4.72*10^-43 J C) 256 kJ D) 2.12*10^42 J E) 1.71*10^5 J

E) 1.71*10^5 joules

What is the approximate bond angle around the indicated carbon atom? C----C (triple) (O+): A) 60 B) 90 C) 109.5 D) 120 E) 180

E) 180 the bond has two electron pair areas and no lone electrons making it linear

A possible set of quantum nmbers for the last electron aded to complete an atom of gallium (Ga) in its ground state is n l ml ms A) 4 0 0 -1/2 B) 3 1 0 1/2 C) 4 1 0 +1/2 D) 3 1 1 +1/2 E) 4 2 1 +1/2

E) 4, 2, 1, +1/2

Select the precipitate that forms when aqueous ammonium sulfide reacts with aqueous copper(II) nitrate. A) Cu2S B) NH4(NO3)2 C) CuSO4 D) NH4NO3 E) CuS

E) CuS

Which of the following compounds have a dipole moments I. ::O==C==O:: II. H--:N==C==O:: III.H--:N==C==S:: IV. (:c-) triple bond (O+:) A) II B) III C) II and III D) I, II, and III E) II, III, and IV

E) II, III, and IV

Which statement is false? A) the molecules of an ideal gas are relatively far apart. B) Molecules of greater mass have a lower average speed than those of less mass at the same temperature. C) Molecules of a gas undergo many collisions with each other and the container walls. D) the average kinetic energies of molecules from samples of different "ideal" gases is the same at the same temperature. E) all molecules of an ideal gas have the same kinetic energy at constant temperature.

E) all molecules of an ideal gas have the same kinetic energy at constant temperature.

Which of the following may be changed in order to balance a chemical equation? A) the mass of the products B) the mass of the reactants C) the identity of the products D) the identity of the reactants E) the coefficients in the reaction

E) coefficients in the reaction

Which of the following describes Dalton's law? A) the temperature of a gas is proportional to its volume B) only one variable can be changed from an initial state to a final state for a gas C) gas particles take up no space D) the pressure of a gas is proportional to its volume E) the total pressure of a gas mixture is the sum of the partial pressures of each gas in the mixture

E) the total pressure of a gas mixture is the sum of the partial pressures of each gas in the mixture

Which electronic geometry would describe an atom bearing five electron bonding domains? A) triangular planar B) octahedral C) tetraheddral D) linear E) trigonal bipyramidal

E) trigonal bipyramidal