Deck 13: (AP) Chemistry: Chemistry

Question 1

____CH₃OH_(I) + _____O₂(g) --> _____CO₂(g) + _____H₂O(g)
What set of coefficients correctly balances this equation?

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

Answer 1

2, 3, 2, 1

Question 2

Which of the following elements has the largest atomic radius?

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

Answer 2

Rubidium

Question 3

Which of the following families contains characteristically nonreactive elements?

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

Answer 3

Noble gases

Question 4

The half-life of 32 grams of a radioactive substance is 6.5 hours. How many grams of the substance remain after 19.5 hours?

A)16 grams
B)8 grams
C)4 grams
D)2 grams
E)32 grams

Question 5

Why is Rutherford's gold foil experiment significant?

A)It led to the discovery of the electron
B)It led to the discovery of the nucleus
C)It led to the discovery of the proton
D)It led to the discovery of the neutron
E)It led to the discovery of orbitals

Question 6

What is the oxidation state of chlorine in potassium perchlorate, KClO₄?

A)-7
B)-3
C)0
D)3
E)7

Question 7

Which of the following compounds contains a double bond?

A)C₂H
B)C₂H₄
C)C₃H₈
D)CH₄
E)C₄H₁₀

Question 8

Which of the following elements exists as a liquid at 25 degrees Celsius?

A)Silicon
B)Chlorine
C)Boron
D)Arsenic
E)Mercury

Question 9

A 250 ml solution of 2.0 M NaOH is diluted to 1.0 liter. What is the final concentration of the solution?

A)1.0 M
B)2.0 M
C).50 M
D)1.2 M
E).25 M

Question 10

Which if the following molecules displays sp³ hybridization?

A)BF₃
B)C₂ H₄
C)CCl₄
D)C₂ H₂
E)PF₅

Question 11

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

A)SO₄ ^2-
B)H₂ SO₃
C)H₂SO₄
D)H₂S
E)HS^-

Question 12

Which of the following molecules acts as a Lewis acid?

A)HCl
B)SO ^2-
C)CCl⁴
D)H PO⁴
E)BH³

Question 13

Which of the following symbols represents the angular quantum number?

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

Question 14

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 15

The common ion effect will occur with addition of which of the following substances to a solution of HF?

A)NaH
B)H² O
C)KF
D)CH₃.2OH
E)LiCl

Question 16

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 17

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

Question 18

What element has isotopes known as deuterium and tritium?

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

Question 19

What is the primary purpose of adding a buffer to a solution?

A)Reduce the pH of the solution
B)Raise the pH of the solution
C)Dilute the solution
D)Stabilize the pH of the solution
E)Precipitate solid out of the solution

Question 20

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 21

Which of the following species is classified as an electrolyte?

A)CH₄
B)C₆H₁₂O₆
C)N₂
D)Na⁺
E)O₃

Question 22

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

A).088 liters
B)8.8 liters
C)2.8 liters
D)4.6 liters
E)1.4 liters

Question 23

Which pair of elements and/or ions is isoelectronic?

A)F^- and Cl^-
B)O and Na
C)K⁺ and Ar
D)Mg ²⁺ and S
E)Br and Kr

Question 24

Which of the following is the correct electron configuration for F-?

A)1s² 2s² 2p⁵
B)1s² 2s² 2p⁶
C)1s² 2s² 2p⁴
D)1s² 2s² 2p³
E)1s² 2s² 2p⁶ 3s¹

Question 25

What is the correct orbital hybridization for CO₂ ?

A)sp
B)sp²
C)sp
D)sp³ d
E)sp³ d²

Question 26

Which of the following solutions is blue?

A).1 M Cu(NO₃ )₂
B).1 M NaNO₃
C).1 M CaCl₂
D).1 M KNO₃
E).1 M MgCl₂

Question 27

A saturated solution of NaCl is heated until more solute can be dissolved. How is this solution best described?

A)Dilute
B)Immiscible
C)Supersaturated
D)Unsaturated
E)Hydrophobic

Question 28

² SO_2(g) + O_2(g) --> ²SO_3(g)
What is the correct rate law for this reaction?

A)r = k[SO₂ ][O₂ ]
B)r = k[SO₃ ]
C)r = k[SO₂ ]² [O₂ ]
D)r = k[SO₃ ]²
E)r = k[SO₃ ][SO₂ ][O₂ ]

Question 29

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

A)HCH₄
B)CH COOH
C)CH₃ OH
D)C₃ H₆ O₃
E)C₆ H₈ O₇

Question 30

What is the expected O-C-O bond angle is a molecule of CO₂ ?

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

Question 31

Which of the following elements is the most electronegative?

A)Cesium
B)Sodium
C)Lithium
D)Boron
E)Fluorine

Question 32

An intermediate species exists as an energy minimum between two activated complexes.

Question 33

Which shape most accurately describes the shape of an s orbital?

A)Cloverleaf
B)Dumbbell
C)Cone
D)Rectangular prism
E)Sphere

Question 34

CH₃ COOH + H₂ O --> CH₃ COO- + H₃ O+
Which of the following descriptions best characterizes CH3COO- in the reaction above?

A)Cation
B)Conjugate acid
C)Conjugate base
D)Indicator
E)Neutral species

Question 35

Which of the following is the correct molecular formula for magnesium phosphate?

A)MgPO₄
B)Mg3(PO₄ )₂
C)Mg(PO₄ )₂
D)MgP
E)MgP₂

Question 36

Which of the following descriptions most accurately characterizes the molecular geometry of H₂ O?

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

Question 37

The half-life of 14 grams of a substance is 3 hours. How many grams of the substance remain after 6 hours?

A)3.5 grams
B)7.0 grams
C)14 grams
D)28 grams
E)7.5 grams

Question 38

Which of the following acids is characterized as diprotic?

A)HCl
B)HF
C)H₂ SO₄
D)HNO₃
E)CH₃ COOH

Question 39

Na⁺_(aq) + Cl-_(aq) + Ag⁺_(aq) + NO_3-(aq) --> AgCl(s) + Na⁺_(aq) + NO_3-(aq)
In the equation above, which species are classified as spectator ions?

A)Na⁺ alone
B)NO_3- alone
C)Na⁺ and NO_3-
D)Ag⁺ alone
E)Ag⁺ and Cl^-

Question 40

Which of the following elements is most easily oxidized?

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

Question 41

What type of bonding does a molecule of O_s display?

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

Question 42

Which of the following compounds contains an oxygen atom with a -1 oxidation number?

A)H₂ O
B)CO₂
C)Na₂ O₂
D)Al₂ O₃
E)MgO

Question 43

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 44

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 45

This figure displays an endothermic reaction.

Question 46

This figure shows the reaction progress diagram for an exothermic reaction.

Question 47

Fe3+ has a larger ionic radius than Fe2+.

Question 48

F- has a smaller atomic radius than F.

Question 49

Galvanic cells require energy input.

Question 50

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 51

You have a closed container filled with 1L of pure air at STP. Assume that this air is made of only nitrogen (79%) and oxygen (21%). What are the partial pressures of nitrogen and oxygen in the box?Hint: XN = PN/PTotal= NN/NTotal

A)P_N = 0.5 atm P_O = 0.5 atm
B)P_N = 1.0 atm P_O = 1.0 atm
C)P_N = .21 atm P_O =.79 atm
D)P_N = .79 atm P_O = .21 atm
E)P_N = .75 atm P_O = .25 atm

Question 52

Which of the following is not true about colloids?

A)Colloids are not solutions
B)Colloids are made of larger particles that most solutions.
C)The dispersing medium has a higher concentration than the dispersed phase
D)The dispersing phase is in higher concentration than the dispersing medium.
E)Colloids are homogeneous mixtures.

Question 53

² Na + ² HCl --> ² NaCl + H₂
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 54

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 55

Which of the following assumptions about gases is not found in the Kinetic Theory of Gases?

A)Gas particles are infinitely small
B)Gas particles are in constant motion
C)Gas particles are in random motion
D)Gases experience intermolecular forces
E)Energy is proportional to temperature

Question 56

Which of the following is not a part of the first and second laws of thermodynamics?

A)Energy can exist as light, heat, chemical energy, or electrical energy
B)Energy can be created and destroyed
C)Energy is always conserved
D)Entropy is the measure of the randomness/disorder of a system
E)If no energy enters or leaves the system during a reaction, the potential energy at the final state will be less than the initial state.

Question 57

Given the following experimental values, for the reaction A + B --> C, figure out the rate constant (k).Initial values: [A] = 0.0100M; [B] = 0.0100M; Rate = 5.00 * 10-6 M/sExperiment 1: [A] = .0200M; [B] = 0.100M; Rate = 2.50 * 10-5 M/sExperiment 2: [A]= 0.0100M; [B]=0.0200M; Rate = 5.00 * 10-6 M/s

A)k = 5.00 * 10-² M*s
B)k = 5.00 * 10-² /(M*s)
C)k = 5.00 * 10-² /(M2*s)
D)k = 5.00 * 10-³ M*s
E)k = 5.00 * 10-³ /(m*s)

Question 58

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