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CHM 101: Wijesinghe

  • Page ID
    2144
  • Template:Chem101Wijesinghe

    Chapter 1:   Measurements

    • Write the names and abbreviations for the metric or SI units used in measurements of length, volume, mass, temperature, and time.
    • Write a number in scientific notation.
    • Identify a number as measured or exact; determine the number of significant figures in a measured number.
    • Adjust calculated answers to give the correct number of significant figures.
    • Use the numerical values of prefixes to write a metric equality.
    • Write a conversion factor for two units that describe the same quantity.
    • Use conversion factors to change from one unit to another.
    • Calculate the density of a substance; use density to calculate the mass or volume of a substance.

    Chapter 2:   Energy and Matter

    • Classify properties/changes as either physical or chemical.
    • Given a temperature, calculate a corresponding temperature on another scale.
    • Classify matter as pure substances or mixtures.
    • Identify energy as potential or kinetic; list some different types of energy.
    • Identify the units of energy and write the specific heat expressions.
    • Use specific heat to calculate heat loss or gain, temperature change, or mass of a sample.

    Chapter 3:  Atoms and Elements

    • Write the name of an element from its symbol or its period and group number.
    • Given the name of an element, write its correct symbol; from the symbol, write the correct name.
    • Use the periodic table to identify the group and the period of an element
    • Describe the electrical charge and location in an atom for a proton, a neutron, and an electron.
    • Given the atomic number and the mass number of an atom, state the number of protons, neutrons, and electrons.
    • Give the number of protons, electrons, and neutrons in the isotopes of an element.

    Chapter 4:  Nuclear Chemistry

    • Describe alpha, beta, positron, and gamma radiation
    • Write and equation showing mass numbers and atomic numbers for radioactive decay
    • Given the half-life of a radioisotope, calculate the amount of radioisotope remaining after one or more half-lives
    • Describe the processes of nuclear fission and fusion

    Chapter 5: Compounds and Their Bonds 

    • Using the periodic table, write the electron-dot symbol for a representative element.
    • Using the octet rule, write the symbols of the simple ions for the representative elements.
    • Using charge balance, write the correct formula for an ionic compound.
    • Given the formula of an ionic compound, write the correct name.
    • Write a formula of a compound containing a polyatomic ion.
    • Given the formula of a covalent compound, write its correct name; given the name of a covalent compound, write its formula.

    Chapter 6: Chemical Reactions and Quantities

    • Use atomic masses to determine the mass of a sample of atoms, the number of atoms in a sample, and formula masses of compounds.
    • Given the chemical formula of a substance, calculate its molar mass.
    • Given the number of moles of a substance, calculate the mass in grams; given the mass, calculate the number of moles.
    • Given the formula of a compound, calculate the percent composition. From the percent composition, determine the empirical formula of a compound.
    • Determine the molecular formula of a substance from the empirical formula and molar mass.

    Chapter 7: Gases

    • Describe the kinetic theory of gases and the properties of gases.
    • Describe the units of measurement used for pressure and change from one unit to another.
    • Use the pressure-volume relationship (Boyle’s law) to determine the new pressure or volume of a certain amount of gas at a constant temperature.
    • Use the temperature-volume relationship (Charles’ law) to determine the new temperature or volume of a certain amount of gas at a constant pressure.
    • Use the temperature-pressure relationship (Gay-Lussac’s law) to determine the new temperature or pressure of a certain amount of gas at a constant volume.
    • Describe the relationship between the amount of gas and its volume and use this relationship in calculations.
    • Use the ideal gas law to solve for P, V, T, or n of a gas when given three or four values in the ideal gas equation. Calculate density, molar mass, or volume of a gas in a chemical reaction.
    • Use partial pressures to calculate the total pressure of a mixture of gases.

    Chapter 8: Solutions

    • Identify the solute and solvent in a solution.  Describe the formation of a solution.
    • Identify solutes as electrolyte or nonelectrolyte
    • Define solubility; distinguish between an unsaturated and a saturated solution.
    • Calculate the percent concentration of a solute in a solution; use percent concentration to calculate the amount of solute or solution.
    • Calculate the molarity of a solution; use molarity to calculate the moles of solute or the volume of solution.  Describe the dilution of a solution.
    • Identify a mixture as a solution, a colloid, or suspension.  Describe how the particles of a solution affect the physical properties of a solution.

    Chapter 9: Chemical Equilibrium

    • Describe how temperature, concentration, and catalysts affect the rate of a reaction.
    • Use the concept of reversible reactions to explain chemical equilibrium.
    • Calculate the equilibrium constant for a reversible reaction given the concentrations of reactants and products Use an equilibrium constant to predict the extent of reaction and to calculate equilibrium concentrations.
    • Use Le Chatelier’s Principle to describe the changes made in equilibrium concentrations when reaction conditions change.

    Chapter 10: Acids and Bases

    • Describe and name Arrhenius and Bronsted-Lowry acids and bases; identify conjugate acid-base pairs.
    • Use the ion-product constant of water to calculate the [H3O+] and [OH-] in an aqueous solution.
    • Predict whether a salt will form an acidic, basic or neutral solution.
    • Describe the role of buffers in maintaining the pH of a solution