Curriculum Documents by Quarter - Science Grade 10 Chemistry

Learning Objectives

• Theory
• Scientific law
• Electron
• Proton
• Neutron
• Nucleus
• Atomic number
• Mass number
• Isotope
• Electromagnetic spectrem
• Energy level
• Electron cloud
• Valence electron
• Lewis dot diagram
• Orbital
• Electron configuration
• Periodicity
• Periodic law
• Period
• Group
• Noble gas
• Metal
• Transition element
• Metalloid
• Nonmetal
• Halogen
• Alkali metal
• Alkaline earth metal
• Lanthanide
• Actinide

Skills

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• Identify and explain some of the physical properties that are used to classify matter, e.g., density, melting point, and boiling point.
• Explain the difference between mixtures and pure substances.
• Describe the four states of matter (solid, liquid, gas, plasma) in terms of energy, particle motion, and phase transitions.
• Distinguish between chemical and physical changes.
• Trace the development of atomic theory and the structure of the atom from the ancient Greeks to the present ( Dalton , Thompson, Rutherford , Bohr, and modern theory).
• Interpret Dalton 's atomic theory in terms of the Laws of Conservation of Mass, Constant Composition, and Multiple Proportions.
• Identify the major components of the nuclear atom (protons, neutrons, and electrons) and explain how they interact.
• Understand that matter has properties of both particles and waves.
• Describe the electromagnetic spectrum in terms of wavelength and energy; identify regions of the electromagnetic spectrum.
• Write the electron configurations for elements in the first three rows of the periodic table.
• Explain the relationship of an element's position on the periodic table to its atomic number and mass.
• Use the periodic table to identify metals, nonmetals, metalloids, families (groups), periods, valence electrons, and reactivity with other elements in the table.
• Relate the position of an element on the periodic table to its electron configuration.
• Identify trends on the periodic table (ionization energy, electronegativity, electron affinity, and relative size of atoms and ions).
• Explain how atoms combine to form compounds through both ionic and covalent bonding.
• Predict chemical formulas based on the number of valence electrons.
• Name and write the chemical formulas for simple ionic and molecular compounds, including those that contain common polyatomic ions.

Atoms form bonds by the interactions of their valence electrons.

The conservation of atoms in chemical reactions leads to the ability to calculate the mass of products and reactants.

The behavior of gases can be explained by the Kinetic Molecular Theory.

Oxidation-reduction reactions occur by electron transfer and constitute a major class of chemical reactions. Examples of redox reactions occur everywhere; their consequences are experienced daily.

§   How do we as scientists organize our knowledge of the universe?

§   How do we as scientists use evidence, models, and explanations to communicate about our discoveries?

§   How do we as scientists measure change?

§   What forces cause change?

§   What is the relationship between structure and function in objects, organisms, and systems?

Vocabulary

• Compounds
• Octet rule
• Ion
• Ionic compound
• Ionic bond
• Crystal
• Covalent bond
• Covalent compound
• Molecule
• Electrolyte
• Interparticle force
• Formula unit
• Oxidation number
• Polyatomic ion
• Hydrate
• Hygroscopic
• Deliquescent
• Anhydrous
• Binary compound

• Distillation
• Allotrope
• Organic compound
• Inorganic compound
• Hydrocarbon
• Reactant
• Product
• Coefficient
• Synthesis
• Decomposition
• Single replacement
• Double replacement
• Combustion
• Equilibrium
• Soluble
• Insoluble
• Activation energy
• Concentration
• Limiting reactant
• Catalyst
• Enzyme

Skills

• Explain how atoms combine to form compounds through both ionic and covalent bonding.
• Draw Lewis dot structures for simple molecules.
• Predict chemical formulas based on the number of valence electrons.
• Name and write the chemical formulas for simple ionic and molecular compounds, including those that contain common polyatomic ions.
• Balance chemical equations by applying the law of conservation of mass.
• Recognize synthesis, decomposition, single displacement, double displacement, and neutralization reactions.
• Determine molar mass, percent compositions, empirical formulas, and molecular formulas.
• Understand the mole concept in terms of number of particles, mass, and gaseous volume.
• Using the kinetic molecular theory, explain the relationship between pressure and volume (Boyle's law), volume and temperature (Charles' law), and the number of particles in a gas sample (Avogadro's hypothesis).
• Explain the relationship between temperature and average kinetic energy.
• Perform calculations using the ideal gas law.

All energy can be considered to be either kinetic energy, which is the energy of motion; potential energy, which depends on relative position; or energy contained by a field, such as electromagnetic waves.

Heat consists of random motion and the vibrations of atoms, molecules, and ions. The higher the temperature, the greater the atomic or molecular motion.

The behavior of gases can be explained by the Kinetic Molecular Theory.

§   How do we as scientists organize our knowledge of the universe?

§   How do we as scientists use evidence, models, and explanations to communicate about our discoveries?

§   How do we as scientists measure change?

§   What forces cause change?

§   What is the relationship between structure and function in objects, organisms, and systems?

Vocabulary

Skills

·          Relate chemical changes and macroscopic properties

·          Demonstrate how chemical equations describe chemical reactions.

·          Balance chemical equations by changing coefficients.

·          Recognize synthesis, decomposition, single displacement, double displacement, and neutralization reactions.

·          Demonstrate factors that influence the rate and direction of a reaction.

·          Relate the properties of a solid, liquid and gas to the kinetic theory of matter.

·          Interpret changes in temperature and changes of state of a substance in terms of the kinetic theory of matter.

·          Convert temperatures in Kelvin to Celsius.

The driving forces of chemical reactions are energy and entropy. This has important implications for many applications (synthesis of new compounds, meteorology, and industrial engineering).

§   How do we as scientists organize our knowledge of the universe?

§   How do we as scientists use evidence, models, and explanations to communicate about our discoveries?

§   How do we as scientists measure change?

§   What forces cause change?

§   What is the relationship between structure and function in objects, organisms, and systems?

Vocabulary

Skills

• Interpret the law of conservation of energy.
• Explain the relationship between energy transfer and disorder in the universe.
• Analyze the energy changes involved in physical and chemical processes using calorimetric measures.
• Apply Hess's law to determine the heat of reaction.
• Explain the significance of carbon in organic molecules.
• Recognize the six most common elements in organic molecules (C, H, N, O, P, S).
• Describe the composition and functions of the four major categories of organic molecules (carbohydrates, lipids, proteins, and nucleic acids).