Chemistry in the Community Outline
A. Sources and uses of water 1. Direct and indirect uses of water and their importance. 2. Identify techniques of water purification. 3. Describe the function and process of the hydrologic cycle and indicate the primary storage reservoirs of the Earth's water supply.
B. Look at the water and its contaminants 1. Classify matter in terms of elements, compounds, and mixtures 2. Distinguish between different type of mixtures: solutions, colloids and suspensions. 3. Distinguish among a chemical symbol, formula and chemical equation. 4. Describe the three basic subatomic particle: protons, neutrons, and electrons. 5. Determine the formula and name of a simple ionic compound when provided with anion's and cation's names and charges
C. Investigating the fish kill 1. Use solubility curves to describe the effect of temperature on solubility and calculate percentage of saturation. 2. Define the terms insoluble, unsaturated, saturated, and supersaturated. 3. Calculate the concentration of a solution. 4. Evaluate the risks of contaminants in our water supply, with particular attention heavy metal ions of lead and mercury 5. Given the pH of a substance, classify it as acidic, basic, or neutral. 6. Describe the solubiltiy of a molecular substance in water. 7. Use the polarity of water molecules to explain water's ability to dissolve ionic solid.
D. Water purification and treatment 1. Compare and contrast natural and artificial water purification. 2. Assess the risks and benefits of water softening and chlorination
E. Putting it all together 1. Town council meeting to determine the cause of the fish kill and how to stop the problem in the future. (Possible other activity)
II. Materials: Structures And Uses
A. Why we use what we do. 1. Distinguish between chemical and physical properties and/or changes in matter when given specific examples 2. Classify selected elements as metals, nonmetals or metalloids based on observation of chemical and physical properties and the periodic table. 3. Use the periodic table to: a. Predict physical and chemical properties of an element. b. Identify elements by their atomic atomic masses and numbers. c. Determine properties of elements by the number and arrangement of electrons in the atom.
B. Earth's Mineral Resources 1. Describe the three major parts of the Earth. 2. List and describe the factors that determine the feasibility of mining a particular ore at a particular site. 3. Explain why more active metals are more difficult to refine and process than less active metals. 4. Describe the process of oxidation-reduction 5. Describe the three most common methods of separating a metal from its ore.
C. Conservation 1. State the Law of Conservation of Matter and apply it by balancing chemical equations 2. Write balanced chemical equations and relate them to the Law of Conservation of Matter. 3. Define the term mole and calculate the molar mass of a compound when provided with the formula and the atomic masses of the elements. 4. Distinguish between renewable and nonrenewable resources, and identify the methods of conserving our resources.
D. Materials: Designing For Properties 1. Describe the differences in the properties of an element due to the arrangement of the element's atoms 2. Describe the difference between the properties of annulment and the properties of an alloy 3. Describe how the conductivity of a material can be changed 4. Describe how the properties of a material may be changed by applying a coating
E. Putting It all Together 1. Use the concepts of the properties of materials to design a new coin for a county. (Possible other activity)
III. Petroleum: Breaking And Making Bonds
A. Petroleum - What is it? 1. Describe the chemical make up of petroleum, how it differs from other natural resources. 2. Describe the process of fractional distillation and name the typical products manufactured from each fraction. 3. Represent the covalent bonding in hydrogen bonding by electron dot structures and molecular formulas. 4. Write the general formulas for the first ten alkanes 5. Define the term isomer and draw the structural formula for the first three isomers of a given compound.
B. Petroleum as an energy source 1. Explain endothermic and exothermic reactions in terms of breaking bonds and forming bonds 2. Identify energy conversions and explain energy conversion efficiency. 3. Define the terms, heat of combustion and specific heat and calculate energies of various combustion reactions. 4. Write balances equations for the combustion of hydrocarbon fuels, including energy changes. 5. Explain the term octane number, state it relationship to grades of gasoline, identify two ways of increasing octane numbers.
C. Petroleum as a building source 1. Compare saturated and unsaturated hydrocarbons in terms of molecular models, formulas, structures, and physical and chemical properties. 2. Identify functional groups for common alcohols, ethers, carboxylic acids, and esters 3. Describe polymerization and give one example if addition and condensation reactions
D. Energy Alternatives to Petroleum 1. Describe major sources of energy and alternative sources of fuels and builder molecules for the future 2. describe alternative fuels that maybe used to extend, supplement, or replace petroleum as Earth's primary fuel
E. Putting It All Together Evaluate the ARL 600 TV ad, then produce and write and automobile commercial message. (Possible other activity)
IV. Chemistry and the Atmosphere
A. Gases in the Atmosphere 1. Earth's atmosphere is composed of a mixture of gases, primary nitrogen, oxygen and water vapor 2. Pressure involves a force applied over a particular area. Air pressure is often measured in units of atmosphere (atm), pascals (Pa) or millimeters of mercury (mm Hg) 3. The volume of a sample of gas in a flexible container decreases if external pressure is increased. Boyle's law describes this inverse relationship. 4. The volume of a sample in a flexible container at constant pressure increases if its temperature is decreased. Charle's law describes this relationship. 5. The pressure exerted by a sample of gas in a rigid container increases if its temperature is increased and decreases if its temperature is decreased. 6. The kinetic molecular theory states that gases are composed of particles of negligible sizes that are in a constant state of motion and engage in elastic collisions. the average kinetic energy of a gas sample is directly proportional to a gas sample. 7. Equal numbers of gas molecules at the same temperature and pressure occupy the same volume. One mole of a gas at OoC and 1 atm pressure occupies a volume of 22.4 liters. 8. The coefficients in a balanced chemical equation involving a gas indicate the relative volumes of gaseous reactants or products.
B. Radiation And Climate 1. Electromagnetic radiation includes xrays, gamma rays, ultraviolet (UV), visible, and infrared (IR) radiation, radio waves, and microwaves. The energy transmitted by radiation varies according to wave length-the shorter the wavelength, the higher the energy. 2. Earth's atmosphere protects living organisms by absorbing and distributing solar energy. 3. Electromagnetic radiation can interact with matter to transfer energy.
C. Acids in the Atmosphere 1. Rain water is naturally acidic, but contaminants in the atmosphere can produce precipitation that is even more acidic than normal. 2. Sulfur oxides and nitrogen oxides generated form natural and human sources contribute to acid rain 3. Acids produce hydrogen or hydronium ions in water, while bases produce hydroxide ions. Strong acids and bases ionize completely; weak acids and bases ionize only partially. 4. Acidic solutions contain a higher concentration of hydrogen ions than hydroxide ions; Basic solutions contain a higher concentration of hydroxide ions than hydrogen ions. Neutral solutions contain equal concentrations of hydrogen and hydroxide ions. 5. pH is a measure of the molar concentration of hydrogen ions in a solution. solutions with a pH 7.0 at room temperature are neutral ,while those with a lower pH are acidic and those with higher pH are basic. 6. Acid precipitation can lower the pH of lakes and streams, which can adversely affect aquatic life. 7. A buffered solution is capable of neutralizing limited amounts of either an acid or base, thus resulting in a pH change.
D. Air Pollution-Sources, Effects, And Solutions 1. Air Pollution is a result of contributions from both primary and secondary sources. 2. Photochemical smog can intensify due to temperature inversions and adverse wind patterns 3. Air pollution can be reduced by catalysts and other chemical technologies. 4. Chlorofluorocarbons (CFC) can destroy stratosphere ozone.
E. Putting It All Together 1. Air quality in the LHMP (Possible other activity)
V. Industry: Applying Chemical Reactions
A. The Chemistry of Nitrogen 1. Fertilizers contain many essential nutrients including nitrogen, phosphorus, and potassium 2. The element nitrogen is transformed chemically as it cycles through living systems and the physical environment. 3. The atoms in nitrogens gas are only accessible and useful to most products living things if they first converted to nitrogen-containing compounds. 4. The relative tendency of an atom to attract electrons within a chemical bond can be estimated by the electronegativity of that element.
B. Nitrogen and Industry 1. Within a system is in dynamic equilibrium, the rate of the forward reaction equals and is thus balanced by the rate of the reverse reaction. 2. A change in temperature or concentration within a system at equilibrium may cause the equilibrium position to shift to favor formation of more reactants or products. The direction of this change can be predicted by LeChatelier's Principle. 3. The rate of a particular reaction depends on the temperature, concentration of the reactants, and the influence of a catalyst. 4. Ammonia, which has many important uses, is commonly produced industrial by the Habor-Bosch process. 5. Initiatives such as Responsible Care, Green Chemistry, and EPA standards stress conservation, safety, and pollution prevention in decisions regarding manufacturing, storing, transporting, and disposing of chemical materials.
C. Metal Processing and Electrochemistry 1. An operating voltaic cell, which is based on a spontaneous oxidation-reduction reaction, converts chemical energy to electrical energy. The magnitude of the current generated by a cell depends in part on its electrical potential. 2. The activity series can be used to predict the direction of electron flow within a particular voltaic cell. 3. Any oxidation-reduction canoe described in terms of two half reactions. Batteries based on a particular oxidation-reduction reaction and consisting of one or more voltaic cells, provide convenient, portable ways to energize many common electrical devices. 4. The Hall-He'roult process is an industrially important way to produce aluminum cations (Al+3) to aluminum metal. 5. All technologicals-new and old-have both positive and negative consequences. Benefit-burden analysis can help guide decisions about selecting and using these technologies.
D. Putting It Together 1. Town Council Meeting - A chemical plant for Riverwood - Confronting a final choice (Possible other activity)
VI. Atoms: Nuclear Interactions
A. The Nature Of Atoms 1. Radiation can be classified as either ionizing or nonionizing radiation. 2. The constituent atoms of a radioactivity substance are unstable and undergo spontaneous changes in nuclear structure. Radioactivity usually results in the emission of alpha, gamma, and beta radiation. 3. Rutherford's gold foil experiment resulted in a model of the atom having tiny, massive, positive charged region at the center of the atom-the nucleus-with negatively charged electrons surrounding the nucleus. 4. Atoms of an element having different numbers of neutrons are isotopes of that element. Isotopes that are radioactive are called radioisotopes.
B. Nuclear Radiation 1. Radiation emitted by naturally occurring radioisotopes is the source of background radiation in the environment. 2. Alpha, beta, and gamma radiation differ in properties, including the extent of shielding required to stop the radiation. Three key factors in minimizing exposure to radiation are shielding, exposure, and proximity. 3. Ionizing radiation has sufficient energy to break chemical bonds. 4. The emissions of nuclear radiation changes the composition of the nucleus. These changes are represented by nuclear reactions. 5. Ionization radiation may be detected by its interaction with matter using a variety of detectors such as unexposed photographic film, scintillation counters, solid-state detectors, cloud chamber, or Geiger counters.
C. Using Radioactivity 1. Half-life is a measure of the time required for a radioisotope to decay. The essentially unchangeable half-lives vary form element to element. 2. Radioisotopes can be used as tracers for diagnostic purposes 3. Ionization radiation emitted by some radioisotopes can be used to kill cancer cells. 4. The artificial conversion or transmutation of one element to another can be accomplished by bombarding nuclei with subatomic particles or other nuclei.
D. Nuclear Energy-Benefits and Burdens 1. Certain large nuclei, upon bombardment with neutrons, split into two smaller nuclei and several additional neutrons. This process is referred to as nuclear fission. 2. The strong force holds the nucleus of an atom together. Nuclear reactions result in a small mass loss, which is converted into large amounts of energy. 3. A critical mass of fissionable material is required to sustain a change reaction. 4. The electricity produced by nuclear power plants originates from the energy released by fission of U-235 in a controlled chained reaction. 5. Nuclear fission results from the combination of two relatively small nuclei into new, more massive atom. This process, which powers the sun and other stars, requires extremely high temperature and pressure. 6. Permanent disposal of nuclear waste poses problems related to the volume, level of radioactivity, and half-lives and radioisotopes present in the waste.
E. Putting It Together 1. The truth about nuclear energy (Possible other activity)
VII. Food: Matter And Energy For Life
A. Food As Energy 1. The technique of calorimetry can be used to determine the quantity of energy contained in a particular food. 2. Energy flows from the sun to plants, then in turn to herbivores, to carnivores, and decomposers. as the energy flows as indicated, most is used to maintain cellular functions. 3. The energy contained in food is released when cellular reactions break the bonds of complex organic molecules, forming lower-energy molecules. the released energy is temporarily stored in phosphate bonds of ATP and is used to power various cellular functions. 4. The energy required by a human to complete a physical activity depends on the particular activity, time involved, and weight of the person engaged in the activity.
B. Energy Storage And Use 1. Fat and carbohydrate molecules are composed of carbon, hydrogen,and oxygen. Differences in structure between fat and carbohydrate molecules account for their different properties and energy content. 2. Carbohydrates including simple sugars such as glucose and also substances involving chemical combinations of two or more simple-sugar units. 3. A triglyceride (a typical fat molecule) is formed by a condensation reaction between three fatty acid molecules and a glycerol molecule. 4. Fats may be saturated (all C-C bonds) or unsaturated (some C-c bonds). Unsaturated fats can become more saturated through hydrogenation. 5. Cis and trans isomers are distinguished by how two functional groups are positioned on either side of a C=C double bond. 6. Chemical reactions involve substances interacting in certain fixed ratios. the limiting reactant determines the quantity of product that can be produced.
C. Proteins, Enzymes, And Chemistry 1. Proteins, the major structural component of living tissue, perform many cellular functions. 2. Amino acids-small molecules that contain at least one amino group and at least one carboxylic acid group-are chemically combined to form protein polymers. The human body is unable to synthesize all the types of amino acids it needs: essential amino acids must be obtained directly from foods. 3. Some protein molecules function as enzymes-biological catalysts that speed up cellular reactions.
D. Other Substances In Foods 1. Vitamins, organic molecules, necessary for basic life functions, are classified as fat-soluble or water-soluble. 2. A titration can be used to determine the amount or concentration of solute in a particular solution. 3. Minerals are elements that are essential to life. 4. Food additives are used to increase the nutritive value, storage life, visual appeal, or ease of production of foods. 5. Chromatography is a useful technique for separating and identifying the components of a solution.
E. Putting It Together 1. Inventory and analysis of your diet (Possible other activity)
Note there is more material here than can be covered in one year. After parts I-IV which covers most of the basic chemistry, parts of sections or some of the sections will be covered. |