| (D) describe metallic bonding and explain metallic
properties such as thermal and electrical conductivity, malleability,
and ductility; and
(E) classify molecular structure for molecules with
linear, trigonal planar, and tetrahedral electron pair geometries
as explained by Valence Shell Electron Pair Repulsion (VSEPR) theory.
(8) Science concepts. The student can quantify the
changes that occur during chemical reactions. The student is expected
to:
(A) define and use the concept of a mole;
(B) calculate the number of atoms or molecules in a
sample of material using Avogadro's number;
(C) calculate percent composition of compounds;
(D) differentiate between empirical and molecular formulas;
(E) write and balance chemical equations using the
law of conservation of mass;
(F) differentiate among double replacement reactions,
including acid-base reactions and precipitation reactions, and oxidation-reduction
reactions such as synthesis, decomposition, single replacement, and
combustion reactions;
(G) perform stoichiometric calculations, including
determination of mass and gas volume relationships between reactants
and products and percent yield; and
(H) describe the concept of limiting reactants in a
balanced chemical equation.
(9) Science concepts. The student understands the principles
of ideal gas behavior, kinetic molecular theory, and the conditions
that influence the behavior of gases. The student is expected to:
(A) describe and calculate the relations between volume,
pressure, number of moles, and temperature for an ideal gas as described
by Boyle's law, Charles' law, Avogadro's law, Dalton's law of partial
pressure, and the ideal gas law; and
(B) describe the postulates of kinetic molecular theory.
(10) Science concepts. The student understands and
can apply the factors that influence the behavior of solutions. The
student is expected to:
(A) describe the unique role of water in solutions
in terms of polarity;
(B) apply the general rules regarding solubility through
investigations with aqueous solutions;
(C) calculate the concentration of solutions in units
of molarity;
(D) calculate the dilutions of solutions using molarity;
(E) distinguish among types of solutions such as electrolytes
and nonelectrolytes; unsaturated, saturated, and supersaturated solutions;
and strong and weak acids and bases;
(F) investigate factors that influence solid and gas
solubilities and rates of dissolution such as temperature, agitation,
and surface area;
(G) define acids and bases and distinguish between
Arrhenius and Bronsted-Lowry definitions and predict products in acid-base
reactions that form water; and
(H) define pH and calculate the pH of a solution using
the hydrogen ion concentration.
(11) Science concepts. The student understands the
energy changes that occur in chemical reactions. The student is expected
to:
(A) describe energy and its forms, including kinetic,
potential, chemical, and thermal energies;
(B) describe the law of conservation of energy and
the processes of heat transfer in terms of calorimetry;
(C) classify reactions as exothermic or endothermic
and represent energy changes that occur in chemical reactions using
thermochemical equations or graphical analysis; and
(D) perform calculations involving heat, mass, temperature
change, and specific heat.
(12) Science concepts. The student understands the
basic processes of nuclear chemistry. The student is expected to:
(A) describe the characteristics of alpha, beta, and
gamma radioactive decay processes in terms of balanced nuclear equations;
and
(B) compare fission and fusion reactions.
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| Source Note: The provisions of this §112.35 adopted to be effective August 4, 2009, 34 TexReg 5062; amended to be effective August 24, 2010, 35 TexReg 7230; amended to be effective August 27, 2018, 42 TexReg 5052 |
