Honors Chemistry Practice Exam

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• A substance that dissolves in water to give a solution that does not conduct an electric current.
• If no more solute can dissolve at a given temperature, the solution is
• Describes mathematically the wave properties of electrons and other very small particles?
• Define a strong acid and a weak acid, with examples and how to compare strength.
• The smallest unit of an element that retains the chemical properties of the element is called the
• Which intermolecular force involves a hydrogen atom bonded to a highly electronegative atom being attracted to a lone pair on another electronegative atom in a nearby molecule?
• Which term describes liquids that do not mix to form a single phase?
• What is the covalent bond in which two atoms share one pair of electrons called?
• Which term best describes variants of the same element that differ in the number of neutrons?
• Which term represents the number of atoms or molecules in one mole (6.022 x 10^23)?
• If 0.75 moles of solute are dissolved in 0.50 kilograms of solvent, what is the molality?
• Calculate the molarity of a solution prepared by dissolving 0.750 moles of solute in 1.20 liters of solution.
• Which law states that mass is conserved during chemical and physical changes?
• A solution that contains more dissolved solute than a saturated solution under the same conditions.
• In Henderson-Hasselbalch calculations, if [A-] equals [HA], what is the pH relative to the pKa?
• Which term describes a mixture where the dispersed phase particles are smaller than in suspensions but larger than those in solutions, forming colloidal dispersions?
• What term describes a solution that has dissolved more solute than the typical saturation limit under the same temperature?
• Which term describes a molecule or part of a molecule that contains both positively and negatively charged regions?
• Which term describes a structural formula in which electrons are represented by dots or dashes between two atomic symbols representing covalent bonds?
• What is the standard enthalpy change of formation for a pure element in its standard state?
• Write the general formula for a combustion reaction of a hydrocarbon CxHy with O2 and the products.
• Which quantity is defined as moles of solute per kilogram of solvent?
• What term describes the amount of a substance required to form a saturated solution with a given amount of solvent at a specific temperature?
• Which term describes an atom that includes a nucleus and electrons?
• Which term describes a covalent bond in which the bonding electrons are equally attracted to both bonded atoms?
• The net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent is called what?
• Which term is defined as a measure of the amount of solute in a given amount of solvent or solution?
• Which term refers to the set of all wavelengths or frequencies of electromagnetic radiation?
• A gas mixture contains 2.0 moles N2 and 3.0 moles Ar in a 10.0 L container at 298 K; calculate the partial pressure of each using the ideal gas law.
• Which set of quantum numbers correctly designates the energy level, subshell shape, orbital orientation, and electron spin for an electron in an atom?
• Which spectrum shows a discrete set of lines corresponding to transitions between energy levels?
• Which principle states that electrons fill the lowest-energy orbitals first before occupying higher-energy orbitals?
• Dissolution of ammonium nitrate in water is what type of enthalpy change?
• For a buffer containing 0.50 M acetic acid (Ka = 1.8×10^-5) and 0.50 M sodium acetate, what is the pH? (use Henderson-Hasselbalch)
• Which intermolecular force arises from temporary dipoles due to fluctuating electron distribution?
• What is the electron configuration for Fe2+?
• Which statement best describes the Law of Conservation of Mass in ordinary chemical and physical changes?
• Which statement best distinguishes endothermic and exothermic reactions with respect to energy diagrams?
• Which pair forms a buffer solution?
• Which statement correctly defines standard state conditions and standard enthalpy of formation?
• Which term describes the energy associated with constructing a crystal lattice relative to the energy of all constituent atoms separated by infinite distances?
• Which term indicates the main energy level occupied by the electron?
• Which term is defined as a formula that shows the location of the atoms relative to one another in a molecule and indicates the number and location of chemical bonds?
• Which term refers to a distinct species of atom defined by the total number of protons and neutrons in its nucleus?
• Specify the properties of atomic orbitals and the properties of electrons in orbitals.
• Which term describes the mass in grams of one mole of a substance?
• Which concept describes the mixing of atomic orbitals to produce new orbitals of equal energy?
• Explain ozone depletion conceptually and how CFCs contribute.
• A chemical compound whose simplest units are molecules is called a
• What term describes a particle of electromagnetic radiation that has zero mass and carries a quantum of energy?
• If 25.0 mL of 0.100 M HCl is titrated with 0.150 M NaOH, what is the pH at the equivalence point? (Assume a strong acid–base reaction)
• Which term refers to the discrete values used to describe properties of electrons in atoms (such as n, l, m_l, and m_s)?
• Balance the combustion of propane: C3H8 + O2 → CO2 + H2O; provide the balanced coefficients.
• The strong affinity of water molecules for particles of dissolved substances that leads to electrolytic dissociation is called what?
• Which intermolecular attraction arises from the uneven distribution of electrons and the creation of temporary dipoles?
• Which statement correctly describes the solubility product constant Ksp and precipitation prediction?
• A solution that contains the maximum amount of dissolved solute.
• What is the maximum number of electrons that can occupy the n = 3 electron shell?
• Which statement best describes the Arrhenius definition of acids and bases?
• Which statement correctly contrasts molality and molarity?
• Orbitals of equal energy are each singly occupied before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin is described by
• A substance that dissolves in water to produce a solution that conducts electricity is called an
• Which property describes the ability to be drawn into a wire?
• Three dimensional region around the nucleus that indicates the probable location of an electron?
• Which is the dissolving medium in a solution?
• What term describes the smallest stable unit of a substance that retains its chemical properties?
• A state in which an atom has a higher potential energy than it has in its ground state?
• What is the standard unit for molality?
• What is the term for the number of waves that pass a given point each second?
• The law that states a chemical compound always contains the same elements in exactly the same proportions by weight is known as the
• Determine oxidation state for C in CO2 and CH4.
• Which statement best describes colligative properties and two examples?
• The process described as combining of atoms of elements to form new substances is called
• Which expression is a valid way to express concentration using mass percent?
• All of the frequencies or wavelengths of electromagnetic radiation.
• An outer main energy level occupied by eight electrons is an example of
• Which term is defined as a measure of the amount of solute in a given amount of solvent or solution?
• In an ideal gas mixture, which statement is true about partial pressures?
• Ionic compounds conduct electricity in which state?
• How is ΔHrxn defined in terms of formation enthalpies when using Hess's law?
• Which is the correct unit for molality?
• Particles intermediate in size between those in solutions and suspensions form mixtures known as colloidal dispersions.
• The interaction that binds protons and neutrons, protons and protons, and neutrons and neutrons together in the nucleus is known as
• Which term describes the ability to be drawn into a wire?
• Which term describes a chemical compound whose smallest discrete units are molecules?
• Which quantum number defines the orientation of an orbital in space?
• Write the net ionic equation for the reaction of Na2SO4 and BaCl2 in solution; determine the precipitate.
• A diagram or graph that indicates the degree to which a substance emits radiant energy with respect to wavelength?
• Dissolving ammonium nitrate in water is endothermic; what observable temperature change occurs?
• A chemical substance that has had its water of crystallization removed is described as what?
• Which describes a catalyst's role in a reaction mechanism, with an example?
• A solution with [H+] = 1.0e-4 M has pH and pOH values; calculate pH and pOH.
• If a reaction has ΔH > 0 and ΔS > 0, what happens to ΔG as temperature increases?
• Which expression correctly represents the instantaneous rate law for a first-order reaction in terms of concentration?
• How is the average atomic mass calculated from isotopes? Choose the correct method.
• Liquids that dissolve freely in one another in any proportion are known as what?
• A solution contains 0.010 moles of a nonvolatile solute in 1.00 kg water. Using π = MRT with T = 298 K, R = 0.0821 L atm mol−1 K−1, and M ≈ 0.010 M, what is the osmotic pressure?
• What term describes the mass in grams of one mole of a substance?
• What is the pH of a 0.01 M NaOH solution?
• The Group 18 elements (He, Ne, Ar, Kr, Xe, Rn) are commonly known as
• Which quantum number is symbolized by l and indicates the shape of an orbital?
• Which term refers to a chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement?
• The law stating that a chemical compound has fixed, definite mass ratios of elements is known as
• Which statement best describes conductivity for metallic, ionic, and covalent bonds in solids and liquids?
• Balance the combustion equation of the hydrocarbon C2H6 with O2 to form CO2 and H2O.
• In a calorimetry experiment, which relations are used to determine ΔHrxn from calorimeter data?
• At standard temperature and pressure, how many liters does one mole of an ideal gas occupy?
• A unit of mass that describes the mass of an atom or molecule is the
• Liquids that are not soluble in each other are called what?
• Which term refers to orbitals that explain the geometry of chemical bonds between atoms?
• If 3.0 moles of solute are dissolved in 2.0 kilograms of solvent, the molality is?
• Which statement most accurately differentiates strong electrolytes and weak electrolytes?
• The number of protons in the nucleus of an atom is called the
• A combination of chemical symbols and numbers to represent a substance is a
• The arrangement of electrons in an atom is called the
• Which statement correctly describes trends in atomic radii across a period and down a group, and the underlying cause?
• Define Bronsted-Lowry acid and base and provide an example of a conjugate acid-base pair.
• Determine the percent composition by mass of H2O.
• A solution that contains less solute than a saturated solution does and that is able to dissolve additional solute.
• An electron occupies the lowest-energy orbital that can receive it is described by the
• Which term means capable of being dissolved?
• Which force is a hydrogen-bonding interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom?
• The sum of the protons and neutrons in the nucleus is known as the
• Which statement correctly describes how Kc behaves with temperature and concentrations?
• What is the electron configuration of the chloride ion Cl−, and why does it resemble argon?
• The emission of a continuous range of frequencies of electromagnetic radiation?
• Which concept describes the mixing of atomic orbitals of similar energy on the same atom to form new orbitals of equal energy?
• Calculate ΔTf for a solution with 2.0 m of nonvolatile solute in a solvent with Kf = 1.86 °C/m.
• Which of the following expresses the common solubility rules for nitrates, chlorides, sulfates, carbonates, and hydroxides?
• What is the pH of a solution containing [H+] = 1.0e-3 M (a strong acid)?
• The minimum amount of energy that can be gained or lost by an atom.
• Which term describes a substance that contains no water of crystallization?
• If 0.30 moles of solute are dissolved in 0.10 kilograms of solvent, what is the molality?
• Which term describes a bonding type where electrons are largely free to move throughout the substance's lattice?
• Which statement about ozone-depleting processes involving CFCs is correct?
• Explain oxidation-reduction and assign oxidation numbers in a redox reaction: MnO4- to Mn2+ in acidic solution.
• The number of moles of solute per liter of solution is known as what?
• The distance between corresponding points on adjacent waves is called what?
• Which term describes the ability of a substance to be hammered into thin sheets?
• Which covalent bond involves a pair of electrons being shared unequally, resulting in partial charges on the atoms?
• Which term describes chemical bonding that results from the sharing of electron pairs between two atoms?
• Which rule states that electrons in singly occupied orbitals must have the same spin?
• Which term describes a discrete packet of energy?
• Which term refers to the emission of electrons from a metal when light shines on the metal?
• The energy required to break the bonds in 1 mol of a chemical compound is the
• What concept describes bonding that cannot be correctly represented by a single Lewis structure?
• A 2.50 g sample of sodium chloride is dissolved to 500.0 mL. What is the molarity of the solution?
• Which term describes the complete set of wavelengths and frequencies of electromagnetic radiation?
• Which theory states that electron pairs repel and molecules adjust their shapes to maximize distance between them?
• A buffer solution contains 0.40 M acetic acid and 0.20 M acetate. With Ka 1.8×10^-5, calculate pH using Henderson-Hasselbalch.
• Which subshell corresponds to the azimuthal quantum number l = 1?
• A solute particle that is surrounded by solvent molecules is described as what?
• What term describes a compound composed of ions bound together by electrostatic attraction?
• Which law states that when two elements form more than one compound, the ratio of the masses of one element that combines with a fixed mass of the other is in small whole-number ratios?
• A 0.50 mole sample of gas is measured at standard temperature and pressure. What is its volume at STP?
• No two electrons in the same atom can have the same set of four quantum numbers is the
• The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid; this relation is described by which law?
• Which term refers to a bond type in which two atoms share more than one electron pair, such as a double or triple bond?
• Which term is defined as the weighted average of the atomic masses of an element's isotopes?
• What term describes the concentration of a solution expressed as moles of solute per kilogram of solvent?
• In the reaction between Na2SO4 and BaCl2, which ions are spectators?
• Which principle states you cannot know both position and velocity exactly at the same time?
• Which quantum number is symbolized by m and indicates the orientation of an orbital around the nucleus?
• What term describes a bond in which the atoms share more than one pair of electrons, such as a double bond or a triple bond?
• Which term describes an ion formed from more than one atom?
• Which principle guides the order in which orbitals are filled to achieve minimum energy?
• Which term is the SI base unit used to measure the amount of a substance, defined so that one unit contains as many particles as there are atoms in 12 g of carbon-12?
• What is an ion made of two or more atoms called?
• Which statement best describes an endothermic reaction?
• A substance that dissolves in water to give a solution that conducts electric current.
• Which statement correctly describes Ka and acid strength?
• What term describes water molecules surrounding ions or molecules in a solution?
• Which statement is true about the solubility product constant Ksp and precipitation?
• The spin quantum number has two possible values, +1/2 and -1/2, which indicate the two fundamental spin states of an electron in an orbital. What are these values?
• The noble-gas configuration describes an outer main energy level that is occupied by how many electrons in most cases?
• Which term describes the set of all wavelengths of electromagnetic radiation?
• Mass percent concentration is defined as the mass of solute divided by the mass of solution times 100. Which option expresses this formula correctly?
• For the reaction 3 H2 + N2 → 2 NH3, If you have 4.0 g H2 and 28.0 g N2, which is limiting and what is the theoretical NH3 yield (in grams)?
• Without water, especially water of crystallization, the substance is described as what?
• Predict the hybridization and molecular geometry for carbon dioxide and methane.
• Rapid escape of a gas from a liquid where it is dissolved is called what?
• 0.50 moles solute in 0.25 kilograms of solvent yields molality of?
• Light is scattered by colloidal particles dispersed in a transparent medium.
• What is the formula for percent yield?
• In solution equilibrium, the rate of dissolution equals the rate of crystallization.
• State Hess's law and give a simple example.
• For the reaction N2(g) + 3 H2(g) ⇌ 2 NH3(g) with Kc = 1.0×10^-3 at a given temperature, what happens if NH3 is added?
• It is impossible to know exactly both the velocity and the position of a particle at the same time?
• Which form of energy exhibits wavelike behavior as it travels through space?
• Which term describes the building block that defines the empirical formula of an ionic compound in a fixed ratio of ions?
• Which term describes a force that attracts electrons from one atom to another, transforming a neutral atom into an ion?
• Which term refers to the maximum amount of solute that can dissolve at a given temperature?
• According to Le Chatelier's principle, what happens when more product is added to an equilibrium mixture?
• An electron configuration notation that shows only the valence electrons is called
• Which term describes the energy associated with creating a crystal lattice from separated atoms?
• Which statement correctly describes the difference between instantaneous rate and average rate for a first-order reaction and how to determine from a rate law?
• The physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates.
• An atom that has the same number of protons as other atoms of the same element but a different number of neutrons is called an
• In acid-base chemistry, what does pKa represent?
• The substance being dissolved in a solution is called the solute.
• A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms is called
• The simplest structural unit of an element or compound is a
• Explain Gibbs free energy and the sign that indicates spontaneity at constant T and P.
• Which term describes the general distribution of electrons among the orbitals and subshells of an atom?
• What term refers to the collection of atoms corresponding to an ionic compound's formula such that the molar mass of the compound is the same as the mass of 1 mol of formula units?
• Which statement is false about molarity and molality?
• What term describes a bond formed by the attraction between positively charged metal ions and the electrons around them?
• What is the lowest energy state of an atom called?
• Symbolized by n, indicates the main energy level occupied by the electron.
• Using Hess's law and standard enthalpies of formation, which expression gives ΔHrxn for the formation of products from reactants?
• Which term refers to the specific arrangement where an outer main energy level is filled with eight electrons?
• In hydrogen's emission spectrum, the Balmer series corresponds to transitions to which energy level, and where do the emitted lines appear?
• Predict the effect of increasing temperature on equilibrium position for endothermic and exothermic reactions.
• Given isotopes 12C (98.89%) and 13C (1.11%) with masses 12.0000 amu and 13.00335 amu, respectively, what is the average atomic mass?
• Which concept uses a set of numbers to describe the properties of electrons in orbitals?
• A covalent bond in which electrons are shared unequally, producing partial charges, is called
• An atom that is identified uniquely by the number of protons and neutrons in its nucleus is called a
• Using VSEPR, predict the shapes of ammonia and water and explain lone-pair effects.
• Which covalent bond is characterized by electrons being equally attracted to both bonded atoms?