Notice. . .
A four-function or scientific calculator and a copy of the 2011 Edition Reference Tables for Physical Setting/Chemistry must be available for you to use while taking this examination.
Notice. . .
A four-function or scientific calculator and a copy of the 2011 Edition Reference Tables for Physical Setting/Chemistry must be available for you to use while taking this examination.
Which sequence of historic developments led to the modern model of the atom?
Which statement compares the energy of an electron in the third shell of a rubidium atom to the energy of an electron in a different shell of the same atom?
When an electron in an atom returns from a higher energy state to a lower energy state
The atomic mass of chlorine is the weighted average of the atomic masses of the
The elements on the Periodic Table are arranged in order of increasing
Which element symbol represents a metalloid?
Which term identifies a chemical property that can be used to differentiate a sample of sodium from a sample of gold?
Which term identifies the type of matter that is composed of two or more different elements chemically combined in a fixed ratio?
The coefficients in a balanced equation represent the
Given the equation representing a reaction:
Br + Br → Br
Which statement describes what occurs during this reaction?
Which term represents a property used to determine the degree of polarity in the bond between two atoms?
Which sample of matter has proportions of components that can be varied?
Which term identifies a form of energy?
According to the kinetic molecular theory, which statement describes the particles of an ideal gas?
A reaction most likely occurs when particles collide with proper energy and
At STP, 2.0 liters of N
Which phrase describes a factor that determines the physical state of a molecular substance?
Which combination of reactants will result in the fastest rate of reaction of a 1.0-gram sample of Zn(s) and 30. milliliters of HCl(aq) at 25°C?
Which term represents the energy absorbed or released during a chemical change?
In terms of energy and disorder, systems in nature have a tendency to undergo changes toward
A molecule of which straight chain hydrocarbon contains nine carbon atoms?
Which compound is an unsaturated hydrocarbon?
What is the number of electrons shared between the carbon atoms in an ethene molecule?
Which two terms represent types of organic reactions?
In an operating electrolytic cell, oxidation occurs at the
An Arrhenius base yields which negative ions in an aqueous solution?
Which change in the concentration of
Based on Table N, which phrase describes the half-lives and the decay modes of uranium-235 and uranium-238?
Nuclear fission reactions result in the net conversion of
What is a risk associated with the production of energy in a nuclear power plant?
Part B–1
Answer all questions in this part.
Directions (31–50): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.
The diagram below represents the path of a subatomic particle as it travels through an electric field between two charged plates.
Which subatomic particle is traveling between the charged plates?
Which electron configuration represents the electrons in a neon atom in an excited state?
Element X reacts with chlorine to form the compound XCl3. In which group on the Periodic Table of the Elements is element X located?
What is the number of moles of calcium oxide in a 238-gram sample of CaO? (gram-formula mass of CaO = 56.1 g/mol)
What is the molarity of an aqueous solution that contains 0.60 mole of KCl dissolved in 3.5 liters of solution?
Which statement describes the freezing point of a solution prepared by dissolving NH4Cl(s) in water at 25°C?
At which temperature and pressure will a sample of a real gas behave most like an ideal gas?
In a sealed, rigid cylinder with a movable piston, a sample of H2 gas occupies 30.0 L at 50.0 kPa and 200. K. What is the pressure of the gas if the volume is changed to 60.0 L and the gas is heated to 300. K?
Which statement explains why a catalyzed reaction occurs at a faster rate than the same reaction when uncatalyzed?
At standard pressure, which 10.0-gram sample of nitrogen has the greatest entropy?
Given the structural formula for an organic compound:
Which two functional groups are present in molecules of this compound?
Given the equation representing a reaction:
When the iron atoms lose 2 moles of electrons, the copper ions in
Given the equation representing a reaction:
What is the change in oxidation state for aluminum in this reaction?
Sulfuric acid,
Given the equation representing a reaction:
Which type of reaction is represented by this equation?
Which equation represents nuclear fission?
Given the particle-diagram equation:
Which type of reaction is represented by the equation?
The diagram below represents a laboratory process that is used to separate a mixture of two different liquids.
Which process is shown in this diagram?
Given the equation representing a system at equilibrium:
Which statement describes the base in the forward reaction?
The graph below shows the decay curve for a 20.0-milligram sample of a radioactive isotope.
What is the half-life of this isotope?
Part B–2
Answer all questions in this part.
Directions (51–65): Record your answers in the spaces provided. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.
Based on Table F, identify one positive ion that forms an insoluble compound with iodide ions in an aqueous solution.
Base your answers to questions 52 through 54 on the information below and on your knowledge of chemistry.
The number of subatomic particles in four different atoms, represented by the letters
Subatomic Particles in Four Different Atoms
Atom | Number of Protons | Number of Neutrons | Number of Electrons |
|---|---|---|---|
L | 32 | 32 | 32 |
M | 33 | 32 | 33 |
Q | 33 | 34 | 33 |
R | 34 | 34 | 34 |
State the number of valence electrons in an atom of M in the ground state.
Compare the mass of a proton in atom R to the mass of an electron in atom R.
Compare the radius of a potassium ion in the ground state to the radius of a potassium atom in the ground state.
Identify the noble gas that has atoms in the ground state with the same electron configuration as a potassium ion, K+, in the ground state.
In the drawing space, draw a Lewis electron-dot diagram of a bromide ion, Br-.
Identify the type of bonding in a sample of solid potassium.
State, in terms of valence electrons, why the bonds in a molecule of hydrogen sulfide are covalent.
Explain, in terms of charge distribution, why a molecule of H2S is a polar molecule.
Base your answers to questions 61 through 63 on the information below and on your knowledge of chemistry.
An equilibrium system in a sealed, rigid container is represented by the equation below.
Compare the rate of the forward reaction to the rate of the reverse reaction in this system.
State the effect on the concentration of iodine gas when hydrogen gas is added to this equilibrium system.
Draw a potential energy diagram on the labeled axes in the drawing space for the forward reaction.
Complete the nuclear equation in the drawing space for the decay of radon-222 by writing a notation for the missing product.
Part C
Answer all questions in this part.
Directions (66–85): Record your answers in the spaces provided. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.
Identify the element classification of these three elements.
Determine the mass number of an atom of sulfur that contains 18 neutrons.
State the trend in atomic radius as these three Period 3 elements on the Periodic Table are considered in order of increasing atomic number.
Identify which of these three elements is a gas at STP.
Base your answers to questions 70 through 72 on the information below and on your knowledge of chemistry.
Silicon carbide, SiC, is a compound used for making sandpaper and for cutting and polishing metals and glass. The balanced equation below represents the production of silicon carbide.
Show a numerical setup for calculating the gram-formula mass of silicon dioxide.
Write a chemical name for the product, CO, in the equation.
Determine the number of moles of carbon that are required to produce 4.0 moles of silicon carbide, SiC.
Base your answers to questions 73 through 75 on the information below and on your knowledge of chemistry.
At standard pressure, a student heated a 120.-gram sample of H2O(s) at
Identify the physical change that takes place during interval BC of the heating curve.
State what happens to the average kinetic energy of the molecules in the H2O sample during interval CD.
Base your answers to questions 76 through 78 on the information below and on your knowledge of chemistry.
The structural formulas of two of the three isomers of pentane and their boiling points at standard pressure are shown below.
Write the general formula of the homologous series to which these compounds belong.
State, in terms of strength of intermolecular forces, why the boiling point of dimethylpropane is lower than the boiling point of pentane.
In the drawing space, draw a structural formula of the third pentane isomer, 2-methylbutane.
Base your answers to questions 79 through 81 on the information below and on your knowledge of chemistry.
In a laboratory activity, a student constructs an electrochemical cell. The diagram and the ionic equation below represent this cell and the reaction that occurs. During this laboratory activity appropriate safety equipment is used and safety procedures are followed.
State the form of energy that is converted to electrical energy in this type of cell.
Write a balanced equation for the reduction half-reaction that occurs in this cell.
Identify the positive ion present in the HCl(aq).
State the color of bromcresol green if it is added to a sample of the sodium hydroxide solution.
State, in terms of ions, why a sample of the 0.10 M NaOH is a good conductor of electricity
