Download Chemistry Objectives

Chemistry Objectives
Law of Conversation, Measurement, and Lab Equipment/Safety
Students will describe and apply the law of conservation of mass.
• Identify energy transformations as exothermic and endothermic processes.
• Identify lab equipment necessary to complete an investigation.
• Identify and apply the appropriate metric unit
• Classify matter according to its composition.
• Distinguish among elements, compounds, homogeneous mixtures, and heterogeneous mixtures.
• Relate the properties of matter of its structure.
• Distinguish between physical and chemical properties.
• Contrast chemical and physical changes.
• Apply the law of conservation of matter to chemical changes.
• Perform / model lab safety and lab equipment usage.
• Convert within the metric system.
• Interpret graphs for heating and cooling processes that involve a change of state.
• Identify phase changes: melting, freezing, boiling, condensation, sublimation.
• Apply laboratory safety guidelines to ensure safety and success in conducting investigations.
Parts of Atoms and Nuclear Changes
Students will describe and apply the history of atomic theory.
• Explain the progression of the atomic model including the contributions of Democritus, Lavoisier,
Proust, Dalton, Thomson, Millikan, Rutherford, Chadwick, Bohr, deBroglie, Heisenberg, and
Schrodinger.
• Identify and describe the atom in terms of subatomic particles, mass number, atomic number,
isotopes, and atomic mass.
• Illustrate the modern model of an atom.
• Understand the arrangement of elements of the periodic table in terms of sequence, the placement of
elements into groups, and regions of the chart and writing chemical symbols.
• Interpret the information available in an element block of the periodic table.
• Recognize and explain Bohr model as an electron distribution into energy levels within the electron
cloud.
• Describe how valence electrons configuration can be expressed as electron dot structures for
representative elements.
• Recognize and explain how electrons are configured within the electron cloud of an atom.
• Write electron configurations.
Periodic
Students will be able to interpret periodic properties of the elements.
• Identify the names and symbols of all main group elements and other common transition elements;
such as scandium, titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, zinc,
silver, platinum, gold, mercury.
• Identify metals, non-metals, metalloids and the position on the periodic table.
• Understand how electron configuration places elements on the periodic table and classify an
element as a metal, nonmetal, or metalloid using the periodic table.
• Demonstrate the correlation between atomic properties (such as atomic size and ionization
energy), electron configuration, and the placement of the elements on the periodic table.
• Relate an element’s valence electron structure to its position in the periodic table.
• Describe and compare the properties of metals, nonmetals, and metalloids.
• Predict chemical behavior of the main group elements
• Relate chemical behavior to electron configuration and atomic size.
• Relate the chemical and physical properties of the transition elements to their electron
configurations.
• Compare the number of electrons in the outer energy level of metals, nonmetals, and
metalloids.
Compounds
Students will be able to interpret the formula and name of a compound and how the
formula represents the structure of the compound.
• Write electron dot structure for covalently bonded molecules.
• Interpret the information in a chemical formula.
• Relate the names and formulas of compounds to the ion charges.
• Use ionic and covalent bonding concepts to correctly write the formulas of inorganic
compounds.
• Name inorganic ionic and molecular compounds.
• Explain formation of polar bonds and polar molecules of water molecules as an outcome of
covalent bonds.
• Compare and contrast characteristic properties of ionic, covalent, and polar covalent bonds.
• Describe the nature of covalent bonds in the formation of single, double, and triple bonds.
Reactions (20 days; Ch. 6)
Students will understand chemical changes can be represented with balanced chemical
equations.
• Identify equation symbols and how to balance chemical equations.
• Identify the type of chemical reaction from examination of the equation.
• Identify the five observations that indicate a chemical reaction has occurred; gas given off,
change in temperature, change in color, odor emitted, precipitate formed.
• Classify a reaction as belonging to one of the five major types.
• Explain the factors that affect the rate of reactions
• Demonstrate how chemical equations describe chemical reactions.
• Illustrate how to balance chemical reactions by changing coefficients.
• Determine the affect an inhibitor, a catalyst, concentration, and temperature have on the rate
of chemical reactions.
• Determine how the values for total mass before and after a reaction demonstrate the law of
conversation of mass.
• Investigate and determine whether a reaction is exothermic or endothermic.
Water and Its Solutions
Students will apply the unique physical and chemical properties of water to the structure of
the water molecule.
• Identify the unique properties of water; liquid at room temperature, high boiling point,
exists in all three states on earth, has a high specific heat, is a versatile solvent, and has a
high heat of vaporization.
• Model the three-dimensional geometry of a water molecule.
• Relate the physical properties of water to the molecular model.
• Compare and contrast the ability of water to dissolve ionic and covalent compounds.
• Investigate and understand the nature of solution formation as an interaction of solvent and
solute.
• Understand the factors affecting solubility.
• Explain the nature of solutions in terms of electrolytic properties and “like dissolves like.”
• Differentiate between hard, soft and distilled water and compare the ability of soap to form
suds in the three types of water.
Acids and Bases
Students will apply the properties of acids and bases to their reactions.
• List properties and name acids and bases.
• Understand and the concentration of hydroxide ions determines the strength of bases.
• Understand the concentration of hydronium ions determines the strength of acids
• Compare and contrast acids and bases.
• Distinguish between strong and weak acids and bases.
• Identify the indicators measure pH.
• Relate pH to strengths of acids and bases.
• Identify the pH ranges of acids and bases.
• Explain the differences in reaction rates of a given metal with two different acids.
• Characterize each of the following solutions as unsaturated, saturated, or supersaturated.