Deck 4: Chemistry

Question 1

Which of the following is the correct molecular formula for acetic acid?

A)HCH?
B)CH?COOH
C)CH?OH
D)C?H?O?
E)C6H?O7

Answer 1

CH?COOH

Question 2

What is the concentration of H+ ions in a solution that has an OH- concentration of 1x10-4 molar?

A)1x10^-10 molar
B)1x10^-9 molar
C)1x10^-8 molar
D)1x10^-5 molar
E)1x10^-4 molar

Answer 2

1x10^-10 molar

Question 3

The concentration of H+ in a solution is 1x10-12. What is the pOH of the solution?

A)2
B)3
C)6
D)12
E)14

Answer 3

2

Question 4

Which of the following is the correct molecular formula for hydrobromic acid?

A)HBrO
B)HBr
C)H?Br
D)H?OBr
E)H?O?Br

Question 5

Which of the following acids is characterized as diprotic?

A)HCl
B)HF
C)H?SO?
D)HNO?
E)CH?COOH

Question 6

An activated complex is a high-energy species formed during the conversion of reactants to products in a chemical reaction.

Question 7

In this figure, which point marks the activated complex?

A)A
B)B
C)C
D)D
E)E

Question 8

Which of the following pairs of compounds are allotropes?

A)CO? and CH?
B)NH?+ and NH?
C)NaCl and LiCl
D)O? and O?
E)Ne and Ar

Question 9

Which of the following symbols represents the angular quantum number?

A)m
B)aq
C)l
D)s
E)n

Question 10

A neutral element has 45 neutrons per atom and a mass number of 80. What is the identity of this element?

A)Chlorine
B)Bromine
C)Mercury
D)Rhodium
E)Calcium

Question 11

Which of the following elements has the largest atomic radius?

A)Lithium
B)Boron
C)Fluorine
D)Potassium
E)Rubidium

Question 12

What set of coefficients correctly balances the following equation?
____CH?OH(l) + _____O?(g) --> _____CO?(g) + _____H?O(g)

A)2, 3, 2, 1
B)1, 2, 2, 1
C)2, 3, 4, 2
D)2, 3, 3, 4
E)2, 3, 2, 4

Question 13

Which of the following solutions has the highest boiling point?

A)1 M NaOH
B)1 M CaCl2
C)1 M NaCl
D)1 M KNO?
E)1 M LiCl

Question 14

75 moles of NaCl are dissolved in 1.00 kg of water. What is the boiling point of this solution (kb = .512 degrees C·kg/mol for water)?

A)101.79 degrees Celsius
B)100.00 degrees Celsius
C)98.21 degrees Celsius
D)102.22 degrees Celsius
E)100.50 degrees Celsius

Question 15

What is the expected O-C-O bond angle is a molecule of CO??

A)90 degrees
B)165 degrees
C)180 degrees
D)120 degrees
E)135 degrees

Question 16

Calculate the bond dissociation energy in the following equation, given the information below:
CH?(g) + 2O?(g) --> CO?(g) + 2H?0(g)
For reference:
DHf° C-H = 87 Kcal/mol
DHf° O=O = 118 Kcal/mol
DHf° C=O = 178 Kcal/mol
DHf° O-H = 111 Kcal/mol

A)+584 KCal
B)+216 KCal
C)-584 KCal
D)-216 KCal
E)-228 KCal

Question 17

What type of bonding does a molecule of NaCl display?

A)Ionic
B)Polar covalent
C)Nonpolar covalent
D)Metallic
E)Covalent metallic

Question 18

Which of the following laws states that it is impossible to known the position and momentum of an electron simultaneously?

A)Pauli exclusion principle
B)Heisenberg's uncertainty principle
C)Hund's rule
D)Grahm's law
E)Ampere's law

Question 19

A colloid made from a liquid dispersing medium and gas dispersed phase is called what?

A)Aerosol
B)Emulsion
C)Sol
D)Solid Foam
E)Foam

Question 20

When a hydrocarbon undergoes combustion in O?, what are the products?

A)CH? and H?O
B)CO? and H?O
C)CH? and CO?
D)C?H? and CO?
E)C?H? and CH?

Question 21

Which of the following is not true about complex ions?

A)Complex ions are formed with a metal as the central atom
B)The other molecules that bond to the metal are called ligands
C)Ligands act as Lewis Acids
D)The coordination number of a complex ion refers to the number of bonds the center atom forms
E)All of the above are true

Question 22

H?S + H?O --> HS- + H?O+
In the reaction above, what is the conjugate base of H?S?

A)H?O
B)HS-
C)H?O+
D)H?S has no conjugate base
E)H?S acts as its own conjugate base

Question 23

Which of the following compounds will not form an electrolytic solution when dissolved in water?

A)NaCl
B)KCl
C)NaNO?
D)CH?
E)LiNO?

Question 24

+ e- --> Ag(s)
In an electrolytic cell, where could this chemical reaction occur?

A)Anode
B)Cathode
C)Salt bridge
D)In solution
E)This reaction could not occur in an electrolytic cell

Question 25

Which of the following is the correct electron configuration for copper?

A)[Ar] 4s²3d⁹
B)[Ar] 4s¹3d⁹
C)[Ar] 3s²3d⁹
D)[Ar] 3s¹3d¹⁰
E)[Kr] 4s²3d⁹

Question 26

Which of the following statements about electrostatic energy is false?

A)It is a form of potential energy, not kinetic energy
B)It is a form of kinetic energy, not potential energy
C)Electrostatic energy is stored in point charges, like electrons and protons
D)The electrostatic energy of one charge alone is zero
E)Electrostatic energy is equal to the work it takes to move two charges close together

Question 27

Which of the following solutions is blue?

A).1 M Cu(NO?)2
B).1 M NaNO?
C).1 M CaCl2
D).1 M KNO?
E).1 M MgCl2

Question 28

How many electrons are in the outermost shell of aluminum?

A)13
B)10
C)8
D)7
E)3

Question 29

A neutral element has a mass number of 23 and 12 neutrons. What is the identity of this element?

A)Sodium
B)Magnesium
C)Vanadium
D)Krypton
E)Iodine

Question 30

A neutral element has a mass number of 129 and 75 neutrons. What is the identity of this element?

A)Copper
B)Tungsten
C)Rhenium
D)Uranium
E)Xenon

Question 31

The emission spectrum of an element is:

A)The spectrum given off by a heated gas when its excited electrons release photons
B)The spectrum observed from a cool gas, where black lines on the spectrum indicate photons used to excite electrons
C)The spectrum given off by a cool gas when its excited electrons release photons
D)The spectrum observed from a heated gas, where black lines on the spectrum indicate photons used to excite electrons.
E)The range of gases emitted during a chemical reaction.

Question 32

Calculate the change in entropy of the following equation:
FeCl_3(s) + 3Na_(s) --> Fe_(s) + 3NaCl_(s)

A)52.1 J/K
B)-52.1 J/K
C)64.1 J/K
D)-64.1 J/K
E)-11.6 J/K

Question 33

What is the formal charge of the Nitrogen atom in NO?-?

A)-2
B)-1
C)0
D)+1
E)+2

Question 34

A fixed quantity of a gas undergoes a change in temperature from 100 K to 200 K and a change in pressure from 2 atm to 1 atm. After theses changes, the volume of the gas is

A)Half of the original volume
B)Unchanged
C)Twice the original volume
D)Four times the original volume
E)Eight times the original volume

Question 35

00 moles of N2 are held in a 10.0 liter container at 25.0 degrees Celsius. What is the pressure of the system?

A)3.32 atm
B)4.00 atm
C).763 atm
D)5.11 atm
E)4.89 atm

Question 36

0 gram sample of a radioactive element decays to 5.0 grams in 15 hours. What is the half-life of this element?

A)3 hours
B)2 hours
C)6 hours
D)7)5 hours
E)5 hours

Question 37

Which of the following doesn't apply to Henry's law?

A)k changes based on the type of gas and temperature,
B)Increasing pressure increases the partial pressure of the gas
C)The concentration of dissolved gas also depends on the solvent; some gases dissolve easier in water than other solvents
D)At constant temperature, C1/P1=C?/P2
E)The value of k for CO? is the same for water and ethanol

Question 38

Which if the following molecules displays sp3 hybridization?

A)BF₃
B)C?H?
C)CCl₄
D)C?H?
E)PF₅

Question 39

Which of the following expressions correctly gives the units for the ideal gas constant, R?

A)(atm)(K) / (mol)(l)
B)(atm)(K)(mol) / (l)
C)(atm)(mol) / (l)(K)
D)(atm)(l) / (mol)(K)
E)(mol)(K) / (atm)(l)

Question 40

What element has isotopes known as deuterium and tritium?

A)Bromine
B)Helium
C)Oxygen
D)Hydrogen
E)Chlorine

Question 41

Which of the following substances will turn blue litmus paper red?

A)HCl
B)H?O
C)NaCl
D)NaOH
E)NH?

Question 42

Consider the following system at equilibrium:
² NOCl(g) <--> ² NO(g) + Cl₂ (g)
According to Le Chatelier's principle, what will occur when the equilibrium concentration of NOCl(g) is reduced?

A)The equilibrium concentration of NO(g) alone decreases
B)The equilibrium concentration of Cl₂ (g) alone decreases
C)The equilibrium concentrations of both NO(g) and Cl₂(g) decrease
D)The equilibrium concentration of NO(g) alone increases.
E)There will be no effect on the concentrations of NO(g) and Cl₂(g)

Question 43

²Na + 2HCl -->² 2NaCl + H?
If you start with 5g Na and 5g HCl, which is the limiting reactant? How much of the excess reactant is left at the end of the reaction?

A)Limiting reactant: HCl Excess: 3.15g Na
B)Limiting reactant: Na Excess: 2.93g HCl
C)Limiting reactant: HCl Excess: 2.93g Na
D)Limiting reactant: Na Excess: 1.85g HCl
E)Limiting reactant: HCl Excess: 1.85g Na

Question 44

Which of the following is not true about London dispersion forces?

A)They are the weakest intermolecular forces
B)They arise from temporary dipoles
C)Dispersion forces are weakest between molecules that are easily polarized
D)Larger atoms form dipoles easier than smaller atoms, so their dispersion forces are stronger
E)Molecular shape affects the strength of London Dispersion forces

Question 45

Which of the following compounds is classified as a metallic oxide?

A)H?O
B)Na?O
C)CO?
D)NO?
E)SO?

Question 46

How many liters of .50 M HBr are required to neutralize 350 mL of 2 M KOH?

A).088 liters
B)8.8 liters
C)2.8 liters
D)4.6 liters
E)1)4 liters

Question 47

What type of molecular geometry does NH? display?

A)Tetrahedral
B)Trigonal pyramidal
C)Linear
D)Bent
E)Square planar

Question 48

Sulfur tetrafluoride contains a middle sulfur atom surrounded by four substituent fluorine atoms and one lone pair of electrons. What molecular geometry does sulfur tetrafluoride have?

A)Linear
B)Tetrahedral
C)See-saw
D)T-shape
E)Bent

Question 49

What is the mass in grams of 1.34x1021 molecules of CO??

A).0979 grams
B)9.79 grams
C).00223 grams
D).223 grams
E)44.0 grams

Question 50

A species undergoes alpha emission to form 234Fr. What is this species?

A)²³⁶Ra
B)²³⁶Rn
C)²³⁴Rn
D)²³⁸Ac
E)²³⁶Ac

Question 51

Which of the following elements is most easily oxidized?

A)Nitrogen
B)Fluorine
C)Lithium
D)Neon
E)Sulfur

Question 52

Which of the following is false about the ionic character of bonds?

A)Covalent bonds never have ionic character
B)Covalent bonds have some ionic character because not all electron sharing is equal
C)Due to partial ionic character, one atom in a covalent bond will have a partial positive charge
D)Due to partial ionic character, one atom in a covalent bond will have a partial negative charge
E)The ionic character of a bond is due to the polarity of the atoms in the bond.

Question 53

What is the percentage composition by mass of hydrogen in the compound CH?OH?

A)12.6 percent
B)9)4 percent
C)49.9 percent
D)37.5 percent
E)74.9 percent

Question 54

Which of the following families contains characteristically nonreactive elements?

A)Alkali metals
B)Alkaline earth metals
C)Halides
D)Halogens
E)Noble gases

Question 55

What term classifies a phase change from a solid directly to a gas?

A)Vaporization
B)Deposition
C)Effervesence
D)Fusion
E)Sublimation

Question 56

Which of the following compounds has a single pi bond? Hint: draw structures of each.

A)Ammonia
B)Sulfuric Acid
C)Methane
D)Hydrogen cyanide
E)Hydrogen Peroxide

Question 57

What property of a metal refers to its ability to be hammered into sheets?

A)Ductility
B)Thermal conductivity
C)Electrical conductivity
D)Malleability
E)Density

Question 58

Which of the following sets of quantum numbers is not possible for an electron?

A)n = 4, l = 2, ml = -1, s=-1/2
B)n = 3, l = 3, ml = -1, s=-1/2
C)n = 2, l = 1, ml = 1, s=-1/2
D)n = 5, l = 3, ml = -2, s=1/2
E)n = 4, l = 3, ml = 2, s=1/2

Question 59

What type of radioactive emission does not have mass?

A)Beta emission
B)Alpha emission
C)Positron emission
D)Gamma emission
E)All types of radioactive emission have mass

Question 60

What is the order of reaction for the following equation? A + B --> 2C

A)Zero order
B)First order
C)Second order
D)Third order
E)Fourth order

Question 61

Which of the following factors does NOT affect the rate of a chemical reaction?

A)The presence of a catalyst
B)Temperature
C)Concentration of reactants
D)Surface area of reactants
E)Type of vessel holding the reactants

Question 62

+ HCl(aq) --> This reaction forms an aqueous compound and a gas as products. What is the identity of the gas?

A)Cl₂(g)
B)HCl(g)
C)Mg(g)
D)H?(g)
E)MgCl₂(g)

Question 63

Which of the following statements best describes chemical reduction?

A)A loss of neutrons
B)A gain of neutrons
C)A loss of protons
D)A loss of electrons
E)A gain of electrons

Question 64

Which of the following straight-chain hydrocarbons is classified as saturated?

A)C?H?
B)C?H?
C)C?H?
D)C?Hl₁₀
E)C?H?

Question 65

The following list shows the ionization energies for sodium (Na) in order from first to fourth ionization energies: 495.8 kJ/mol; 4562.4 kJ/mol; 6912 kJ/mol; 9543 kJ/mol.Compare it to the same list for Magnesium and explain why the second ionization energy for Magnesium is much lower than the second ionization energy of sodium.In order from first ionization energy to fourth for Magnesium: 737.7 kJ/mol; 1450.6 kJ/mol; 7732.6 kJ/mol; 10,540 kJ/mol.

A)Magnesium is a metal, and they always have lower second ionization energies. Sodium is a salt, so it doesn't give away more than one electron.
B)Magnesium is always a +2 ion, so the energy required to give away two electrons is low.
C)By giving away one electron, Na reaches a noble gas configuration, so giving away a second electron takes a lot of energy.
D)Since it has two electrons to give away before reaching noble gas configuration, the second ionization energy of Magnesium is low.
E)Both C and D.

Question 66

Na⁺(aq) + Cl^-(aq) + Ag⁺(aq) + NO?^-(aq) --> AgCl(s) + Na⁺(aq) + NO?^-(aq)
In the equation above, which species are classified as spectator ions?

A)Na⁺ alone
B)NO?^- alone
C)Na⁺ and NO?^-
D)Ag⁺ alone
E)Ag⁺ and Cl^-

Question 67

Examine the following titration curves. Which of the four represents the titration curve for a strong base and weak acid?

A)The top left graph
B)The top right graph
C)The bottom left graph
D)The bottom right graph
E)None of the above

Question 68

Which of the following acids is classified as weak?

A)CH?COOH
B)HCl
C)HBr
D)HClO?
E)H?SO?