2011 Edition
2011 Edition
This is a test of your knowledge of chemistry. Use that knowledge to answer all questions in this examination. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry. You are to answer all questions in all parts of this examination according to the directions provided.
Which statement describes the modern model of the atom?
Which subatomic particles are found in the nucleus of a beryllium atom?
According to the electron cloud model of the atom, the region of space with the highest probability of locating an electron is
Which element has atoms that each contain 14 protons?
Which statement describes a chemical property of an element?
At 298 K and 101.3 kPa, oxygen exists in two gaseous forms: O2(g) and O3(g). These two forms of oxygen have
Which two terms represent types of chemical formulas?
In all chemical reactions, there is a conservation of
A sample of solid tungsten has mobile valence electrons throughout the sample. Which type of bonding is present in the sample?
Which formula represents a polar molecule?
What occurs when two fluorine atoms react to produce a fluorine molecule?
A sample of NaCl(s) and a sample of NaCl(
Which substance can not be broken down by a chemical change?
All aqueous solutions of glucose are classified as
At which pressure and temperature does a sample of He(g) behave most like an ideal gas?
The kinetic molecular theory states that the particles of an ideal gas
A reaction is most likely to occur when reactant particles collide with proper
A sample of gas is in a sealed, rigid cylinder at constant volume. Which changes occur in the force of collisions of the gas particles and frequency of their collisions when the sample is cooled?
At STP, 2.0 liters of Ar(g) contains 5.4 x
When a system is at equilibrium, the concentrations of the reactants and the products must be
Which expression represents the heat of reaction for a chemical change?
When a catalyst is added to a chemical reaction it produces
Naturally occurring chemical systems tend to undergo changes toward
Which formula represents an organic compound?
Where do oxidation and reduction occur in an electrochemical cell?
Which element is the most active nonmetal?
When a sample of solid Ca(OH)2 dissolves in water, the only negative ions in the solution are
Which products are formed when an Arrhenius acid and an Arrhenius base react?
The stability of an isotope is related to the ratio of which subatomic particles?
Which nuclear emission has the greatest mass?
Which element is listed with the number of valence electrons and the number of non-valence electrons in one of its atoms in the ground state?
An atom has a mass number of 112 and contains 48 protons. How many neutrons does this atom contain?
There is a decrease in value of which property as the elements in Period 2 are considered in order from lithium to fluorine?
What is a chemical name for NaClO3?
Which formula represents a molecule that has four electrons shared between the two atoms?
Given the balanced equation representing a reaction:
4Al(s) + 3O2(g)
What is the number of moles of Al₂O₃(s) formed when 12 moles of O₂(g) react completely?
A substance has an empirical formula of CH₂ and a molar mass of 112 g/mol. What is the molecular formula for this compound?
Compared to the vapor pressure of ethanol at 1.0 atm and 25°C, the vapor pressure of water at 1.0 atm and 25°C is
Based on Table
Based on Table F, which compound is most soluble in water?
Each of four test tubes contains a different concentration of HCl(aq) at 298 K. A 1.0-gram sample of iron filings is added to each test tube. In which test tube is the reaction occurring at the fastest rate?
Which equation represents an increase in entropy?
Given the formula representing a compound:
What is a chemical name for this compound?
Given the incomplete equation with
CH4 + Cl2 →
Which formula represents the missing product,
Which type of reaction produces ethanol and carbon dioxide from glucose, C6H12O6?
Given the balanced ionic equation:
2Fe3+(aq) + Sn2+(aq) → 2Fe2+(aq) + Sn4+(aq)
How many moles of electrons are gained by Fe3+(aq) when Sn2+(aq) loses 2 moles of electrons?
Which aqueous solution of LiCl is the best conductor of an electric current?
Given the equation representing a reaction:
NH3 + H2O → NH4+ + OH-
According to one acid-base theory, the H2O acts as an acid because it is an
Based on Table
Which statement explains the energy released by a fission reaction?
Directions: Record your answers in the spaces provided. Some questions may require the use of the 2011 Edition Reference Tables for Physical Setting/Chemistry.
Base your answers on the information in each question and on your knowledge of chemistry.
A sample of a molecular substance starting as a liquid at 97.0ºC and 1 atm is cooled for 10. minutes. The heat of fusion for this substance is 148 joules per gram. This cooling process is represented on the graph provided.
State what happens to the average kinetic energy of the molecules in the sample during the first 3 minutes.
State, in terms of carbon-carbon bonds, why ethane is saturated.
Draw a structural formula for 1-butanol.
Describe what happens to the boiling points of the alcohols as the number of carbon atoms per molecule increases.
State the oxidation number of the silver atoms in the Ag(s) electrode.
State the form of energy that is converted to electrical energy in this operating cell.
Write a balanced half-reaction equation for the oxidation reaction that occurs when the cell operates.
During a titration, 10.0 mL of HCl(aq) is exactly neutralized by adding 20.0 mL of 0.10 M NaOH(aq). The NaOH(aq) has a pH value of 13.0. During this laboratory activity appropriate safety equipment is used and safety procedures are followed.
State the color of bromthymol blue after it is added to a sample of the NaOH(aq) solution.
State, in terms of ions, why the HCl(aq) solution can conduct electricity.
Show a numerical setup for calculating the molarity of the HCl(aq), using the titration data.
A phosphorus radioisotope decays by positron emission and has a half-life of 2.50 minutes. This reaction is represented by the equation below.
State, in terms of elements, why the equation represents a transmutation reaction.
Compare the energy of an electron in the fourth shell of a gallium atom to the energy of an electron in the first shell of the same atom.
State how a bright-line spectrum from a sample of an element viewed through a spectroscope can be used to identify the element as gallium.
Show a numerical setup for calculating the atomic mass of gallium.
Ammonium sulfate is a fertilizer produced by the reaction between ammonia and sulfuric acid. The unbalanced equation for this reaction is shown below.
NH3 + H2SO4 → (NH4)2SO4
State why the equation represents a synthesis reaction.
State, in terms of element classification, why the bonding in a sample of sodium chloride is ionic.
A student investigating the properties of solutions dissolved 44.0 grams of KCl(s) in 200. grams of water at 30.°C. During this laboratory activity appropriate safety equipment was used and safety procedures were followed.
Classify, in terms of saturation, the type of solution produced by the student.
Based on Table G, state what happens to the solubility of KCl in water as temperature increases from 30.°C to 70.°C.
Compare the boiling point of the solution at standard pressure to the boiling point of water at standard pressure.
In a process used for centuries, limestone containing calcium carbonate is heated to produce calcium oxide and carbon dioxide gas. When placed in a sealed, rigid container, the reaction is reversible, allowing CaO and CO2 to react to produce CaCO3. These reactions produce an equilibrium system as represented by the equation below.
Compare the rate of the forward reaction to the rate of the reverse reaction in this equilibrium system.
Explain, in terms of collisions between CaO and CO2, why adding more CO2(g) to this equilibrium increases the amount of CaCO3(s) in the system.
State the pH value when the H+ ion concentration in the original NaOH(aq) has increased by a factor of 10 compared to its original value.
Explain, in terms of both protons and neutrons, why an atom of Ga-69 and an atom of Ga-71 are classified as different isotopes of the same element.
Identify the noble gas that has atoms with the same electron configuration as a chloride ion when both the atoms and the ions are in the ground state.
In the drawing space, draw a Lewis electron-dot diagram for the ion in this table that has the greatest percentage of ions in seawater.
State, in terms of electrons, why the radius of a Mg2+ ion is smaller than the radius of a Mg atom.
Using the key below, draw at least two water molecules in the box, showing the orientation of each water molecule toward the Na+ ion.
On the labeled axes in the drawing space, draw a potential energy diagram for the forward reaction in this system.
