Regents Chemistry Objectives

Transcription

1 Regents Chemistry Objectives Packet #1 Math & Lab Skills: 1. Be able to distinguish a qualitative from a quantitative observation. 2. Be able to distinguish an observation from a conclusion. 3. Know how to do metric conversions. 4. Be able to determine the number of significant figures in a measured quantity. 5. Be able to perform multiplication/division and add/subtract to the correct number of significant figures. 6. Know how to read measurements to the correct number of significant figures on graduated cylinders, centimeter rulers, burets, and triple beam balances. 7. Know how to calculate % error and know how to calculate density (Table T & Table S). 8. Know how to correctly graph experimental data and draw best fit lines. 9. Know how to appropriately scale the axes of a graph. Packet #2 Energy & Thermodynamics: 1. Know the definitions of a solid, liquid, and gas in terms of shape and volume. 2. Know the definitions of matter, substances, elements, compounds, and mixtures (homogenous and heterogeneous). 3. Know the difference between an element and a compound. 4. Be able to recognize an element, compound, and mixture given their symbol/formula. 5. Be able to identify the 7 diatomic molecules. 6. Know how compounds and mixtures differ. 7. Be able to determine if a mixture is homogenous or heterogeneous. 8. Know how to separate components of mixtures (filtration, distillation, evaporation and magnet). 9. Be able to draw and interpret particle diagrams of atoms, mixtures of atoms, compounds, heterogeneous and homogenous mixtures. 10. Be able to draw particle models of atoms and/or molecules in the solid, liquid, or gas states. 11. Be able to define kinetic and potential energy. 12. Know that energy is measured in joules. 13. Be able to distinguish an exothermic from an endothermic reaction given an equation (either the energy will be present in the reaction, use BARF, or Table I). 14. Know the definition of temperature and its relationship to kinetic energy. 15. Know the direction of heat flow. 16. Know that the two fixed points on a thermometer are 0 and 100ᵒC. 17. Know that when a chemical reaction is exothermic, the temperature increases, and when a chemical reaction is endothermic, the temperature decreases. 18. Understand the significance of Kelvin temperature and absolute zero. 19. Be able to perform temperature conversions from Kelvin to Celsius and Celsius to Kelvin. 20. Know the definitions of Heat of Fusion and Heat of Vaporization.

2 21. Know all the phase changes and whether they are endothermic or exothermic: melting, vaporization, sublimation, freezing, condensation, and deposition. 22. Know examples that undergo sublimation and deposition at STP. 23. Be able to use the heating and cooling graphs to do the following: Find the phases and the phase changes. Find where phases are in equilibrium Determine whether the phase change is endothermic or exothermic. Be able to describe what is happening to KE and PE during each interval. Be able to explain why the segment for evaporation/condensation is longer than the segment for melt/freeze. Be able to calculate heat equation problems using: o q = mc T o q = mhf o q = mhv 24. Be able to use Table B to find the heat constants for water. 25. Be able to identify if a physical or chemical change is occurring. Packet 3 Atomic: 1. Know where the 3 subatomic particles are found in the atom, and know their charges and masses. 2. Know that the the notations of the isotopes include 14 6C, 14 C, carbon-14, C Know that the nucleus always carries a positive charge and the number of protons (atomic number) determines the element. 4. Know how to determine the number of protons and neutrons given the atomic number and mass number. 5. Know that an atom is electrically neutral. 6. Be able to describe the various atomic models from Dalton to the Wave Mechanical Model. 7. Know what an orbital is. 8. Be able to describe Rutherford s Gold Foil experiment and state the major conclusions. 9. Be able to define an isotope. 10. Know how to calculate the average atomic mass with all the naturally occurring isotopes and their abundances. 11. Know that the farther an electron is from the nucleus, the more energy it has. 12. Know the energy changes when electrons move between the ground and excited states. 13. Know how to recognize and write an electron configuration in the ground and the excited states. 14. Know how that the bright line spectrum is created when an electron goes from the excited state back down to the ground state and releases energy. 15. Know that when an atom loses electrons it becomes (+) charged, and when an atom gains an electron it becomes (-) charged. 16. Know how to determine the number of protons and electrons in an ion. 17. Know what the configuration of an ion will look like (will look like one of the noble gases). 18. Be able to define an ion.

3 Packet #4 Periodic Table: 1. Know that the Periodic Table is arranged in order of increasing atomic number. 2. Know where metals, non-metals, metalloids, and noble gases are located on the PT. 3. Know the physical and chemical properties of metal, non-metals, metalloids, and noble gases. 4. Know at STP, which elements are solid, liquid, and gas. 5. Know the common names for group 1, group 2, groups 3-12, group 17, and group Know what elements in the same group and elements in the same period have in common. 7. Know why elements in the same group are more similar than elements in the same period. 8. Know the definitions of Ionization Energy, Electronegativity, Atomic Radius, and Ionic Radius. 9. Be able to describe how the succession of elements within the same group/period demonstrates characteristic trends in IE, EN, and AR. 10. When an atom gains one or more electrons, it becomes negatively charged and the radius increases. 11. When an atom loses one or more electrons, it becomes positively charges and the radius decreases. Packet #5 Naming, Balancing, Reaction Types: 1. Know how to identify an ionic compound vs. a covalent compound. 2. Know that the sum of the oxidations states of a compound have to equal Know how to name an ionic compound in which the metal has only 1 oxidation number. 4. Know how to name an ionic compound in which the metal has more than 1 oxidation number using the Stock System. 5. Know how to name ternary ionic compounds that include polyatomic ions (Table E). 6. Know how to name covalent compounds using the appropriate prefixes when necessary. 7. Know that in all chemical reactions there is a conservation of mass, charge, and energy; this is why we have to balance using the smallest whole number coefficient. 8. Be able to determine if a reaction is classified as a synthesis reaction, a decomposition reaction, a single replacement reaction, a double replacement reaction, or a combustion reaction. 9. Know how to write the chemical formula of a compound given its name. Packet #6 Moles & Stoichiometry: 1. Know the definition of a mole. 2. Know how to calculate the GFM (gram formula mass) of a substance (including a hydrate). 3. Know the definition of Avogadro s #. 4. Know that GFM = 1 mole = 6.02 x particles= 22.4L. 5. Know the difference between an Empirical Formula (EF) and Molecular Formula (MF). 6. Know how to calculate the MF using the EF and the mass of the MF. 7. Know how to convert Grams Moles and Moles Grams (Table T). 8. Know how to calculate % Composition (Table T). 9. Know how to calculate the % Composition of a hydrate in a lab set-up (H-A/H x 100). 10. Know how to set up a Mole-Mole problem using a balanced equation.

4 Packet #7 Chemical Bonding: 1. Know that when a bond is broken, energy is absorbed; when a bond is formed energy is released (BARF). 2. Atoms attain a stable valence electron configuration by bonding with other atoms. Noble gases have stable valence configurations and tend not to bond. 3. Be able to determine the noble gas configuration of an atom when bonding occurs. 4. Electron dot diagrams (Lewis structures) can represent the valence electron arrangement in elements, compounds and ions. 5. Two major categories of compounds are ionic and molecular (covalent) compounds. 6. Chemical bonds are formed when valence electrons are: a. Transferred from one atom to another (ionic) b. Shared between atoms (covalent) c. Mobile electrons within a metal (metallic) 7. Be able to demonstrate bonding concepts using Lewis Dot Structures representing valence electrons for both ionic and covalent compounds. 8. Know that a Polar molecule means that electrons are unequally distributed. 9. Know that a Non-Polar molecule means that electrons are equally distributed. 10. Know that an ionic compound is essentially extremely polar. 11. Know that ionic bonds will have an EN difference > Know the characteristics of an ionic compound. 13. Know that covalent bonds have an EN difference < Know how to determine if a covalent bond is a Polar or Non-Polar Bond (EN difference). 15. Know how to determine is a covalent compound is a Polar or a Non-Polar Molecule (SNAP). 16. Know that the greater the EN difference is, the more Polar the substance is. 17. Know that Polar Molecules will have a δ + and δ - end. The end with the higher EN is δ - and the end with the lower EN is δ Know what is meant by likes dissolve in likes. 19. Know the 3 types of intermolecular forces: a. Hydrogen Bond H 2 O, NH 3, HF b. Dipole Attraction All other polar asymmetrical molecules c. Van der Waals (London Dispersion Forces) For the Non-polar symmetrical molecules. 20. Know which end of an ionic compound would be attracted to which end of a water molecule (molecule-ion attraction). Packet #8 Gas Laws: 1. Be able to define what is meant by vapor and vapor pressure. 2. Know the relationship between temperature and pressure. 3. Know the relationship between pressure and the number of particles. 4. Know the relationship between temperature (KE) and the speed of the particles. 5. Know the meaning of STP (Table A).

5 6. Be able to explain that boiling occurs with the vapor pressure of a liquid is equal to the atmospheric pressure. 7. Be able to use Table H to find the normal boiling points of the four liquids and the temperature they will boil at if the atmospheric pressure increases or decreases. 8. Be able to use the combined Gas Law P 1 V 1 /T 1 = P 2 V 2 /T Know Boyle s Law, the relationship between pressure and volume when temperature remains constant; P 1 V 1 = P 2 V Know the graph of pressure and volume. 11. Be able to describe the relationship between pressure and volume of an ideal gas at constant temperature. 12. Know Charles s Law, the relationship between volume and temperature when pressure remains constant; V 1 /T 1 = V 2 /T Know the graph of volume and temperature. 14. Be able to describe the relationship between volume and temperature of an ideal gas at constant pressure. 15. Be able to look up the conditions of STP and use them to solve a gas equation. 16. Be able to explain the four points of the Kinetic Molecule Theory (Combined Gas Law). 17. Know the conditions of pressure and temperature that must exist for an Ideal Gas to exist. 18. Know the conditions of pressure and temperature that must exist for a Real Gas to exist. 19. Know two real gases that behave most like ideal gases. 20. Know that equal volumes of gases at the same temperature and pressure have the same number of molecules (Avogadro s Law). 21. Know that less massive gases diffuse faster than more massive gasses. 22. Know how to determine which compounds have the strongest/weakest intermolecular forces on Table H. Packet #9 Solutions: 1. Know that a solution is a homogenous mixture. 2. Know that a solution is made up of a solute and a solvent. 3. Know the difference between dilute and concentrated. 4. Know that ionic compounds dissociate in water. 5. Know that when there are a lot of ions in solution, the solution is an electrolyte. 6. Know the relationship between solubility of a solid solute and temperature. 7. Know the relationship between solubility of a gas solute and temperature. 8. Know the relationship between solubility of a gas and pressure. 9. Know that changes in pressure do NOT affect the solubility of a solid solute. 10. Know how to read Table G based on 100 grams of water. 11. Know what the definition of saturated, unsaturated, and supersaturated are and how to determine what type of a solution is formed based on Table G. 12. Know how to determine how much solute settles out (precipitates) out of solution using Table G. 13. Know the synonyms for soluble and insoluble.

6 14. Know how to interpret Table F (soluble/insoluble). 15. Know that a saturated solution is said to be at equilibrium. 16. Know how to determine Molarity (Table T); you may have to convert L ml and convert grams to moles. 17. Know how to determine ppm (Table T); you may have to add the solute to the solvent to get the grams of solution. 18. Know that adding a salt to a solvent will increase the boiling point and decrease the freezing point (colligative properties). Packet #10 Acids, Bases, & Salts: 1. Know the characteristics of an acid: aqueous, H + /H 3 O +, ph, litmus, phenolphthalein, electrolyte, and Table J. 2. Know the characteristics of a base: aqueous, OH -, ph, litmus, phenolphthalein, and electrolyte. 3. Know that Table K & L identify some common acids and bases. 4. Know that a salt is ionic and is an electrolyte when aqueous. 5. Know the definition of an Arrhenius Acid and Base. 6. Know the definition of a Bronsted-Lowry (Alternate Acid/Base Theory) Acid/Base (BAAD). 7. Know how to determine conjugate acid/base pairs. 8. Know the general reactants and products of a neutralization reaction. 9. Know how to predict the products of a neutralization reaction. 10. Know that neutralization is the end result of titration. 11. Know how to use the titration equation. 12. Know how the concentration of H + determines the ph of a substance (1.0 x 10-3 = ph 3). 13. Know that ph + POH = Know that every step on the ph scale is 10x. 15. Know that as ph increases, H 3 O + decreases, and as ph decreases, H 3 O + increases. 16. Acid: H 3 O + > OH -, Base: H 3 O + < OH -, Neutral H 3 O + = OH Know how to use Table M (Indicators) to determine ph. Packet #11 Kinetics & Equilibrium: 1. Know how to explain Collision Theory in terms of rate of reaction: 2. Know how concentration, temperature, and surface area affect collisions/rate of reaction. 3. Know how the nature of the reactant (ionic/covalent) affects collisions/rate of reaction. 4. Know how the addition of a catalyst speeds up collisions/rate of reaction/lowers activation energy. 5. Know how to label all parts of a PE diagram. PE reactants PE products Activation energy for forward and reverse reactions Heat of reaction (change in enthalpy, H) PE activated complex

7 6. Know how to differentiate an endothermic (+ΔH) vs. exothermic (-ΔH) PE diagram (ΔH = PE product PE reactant ). 7. Know how to determine whether reactions on Table I are endothermic or exothermic. 8. Know how to describe phase equilibrium and solution equilibrium. 9. Know how to describe chemical equilibrium in terms of rate of reaction/constant concentration. 10. Know how to describe Le Chatelier s Principle in terms of stress and shift. 11. Know how to determine the effects of an equilibrium reaction when there is a change in concentration, temperature, and pressure. 12. Know what it means for a reaction to go to completion and that the production of a gas, water, or a precipitate are evidences for this. 13. Know the conditions of energy (enthalpy) and entropy that are required for a spontaneous reaction to occur. 14. Know what happens when a common ion is added to a reaction (Common-Ion Effect). 15. Be able to sketch an endothermic or exothermic potential energy diagram. 16. Be able to sketch a potential energy diagram with and without a catalyst. 17. Know the definition of activation energy. Packet #12 REDOX: 1. Know the definition of oxidation and reduction. 2. Know the definition of a reducing agent and an oxidizing agent. 3. Know how to assign oxidation numbers to substances. 4. Know how to use Table J to determine if a single replacement reaction will occur spontaneously. 5. Know that a Voltaic Cell (Galvanic Cell) converts chemical energy into electrical energy spontaneously. 6. Know that the anode is the site of oxidation and the cathode is the site of reduction. 7. Know the functions of the electrodes, wire, and salt bridge. 8. Know that an Electrolytic Cell converts electrical energy into chemical energy non-spontaneously (electrolysis). 9. Know that electroplating is electrolysis in which the object being plated acts as the cathode. Packet #13 Organic Chemistry: 1. Know what makes a molecule classified as organic. 2. Know characteristics of an organic compound. 3. Know what a Hydrocarbon is. 4. Know how to use Table Q to determine if a hydrocarbon is classified as an alkane, alkene, or an alkyne based on the general formula. 5. Know which hydrocarbon is classified as saturated and unsaturated and why. 6. Know how to write the chemical formula, write the condensed formula, and draw the structural formula for hydrocarbons. 7. Know what the alkyl group is and how to use them as side chains off of organic compounds.

8 8. Know how to use Table R to identify other classes of organic compounds based on their functional groups. 9. Know how to write the chemical formula, write the condensed formula, and draw the structural formula of these organic compounds. 10. Know that Alcohols and Organic Acids have the highest boiling points and that hydrocarbons with an equivalent number of carbons would have the lowest. 11. Know how to recognize the various organic reactions and be able to predict missing products or reactants (Addition. Substitution, Fermentation, Esterfication, Saponification, Combustion, Polymerization). Packet #14 Nuclear Chemistry: 1. Know how to determine if an isotope is radioactive based on the ratio of neutrons to protons. 2. Know how to read the symbols of the decay modes on Table O including the mass and the charge of the particle or ray. 3. Know the definition of transmutation. 4. Know how a magnet can separate alpha, beta, and gamma particles. 5. Know that Hydrogen-1 = Hydrogen, Hydrogen 2 = Deuteron, Hydrogen -3 = Tritium. 6. Know how to recognize a Natural Transmutation from an Artificial Transmutation. 7. Know how to use Table N to determine the decay mode of a radioisotope. 8. Know how to use Table N to write a complete Natural Transmutation, or fill in a missing reactant or product. 9. Know how to fill in a missing reactant/product in either a Natural or Artificial Transmutation (equal mass and charge on both sides of the reaction). 10. Know that Fission and Fusion are types of Artificial Transmutations. 11. Know how to recognize a Fission reaction vs. a Fusion reaction. 12. Know which produces more energy, a Fission or Fusion reaction. 13. Know why the mass of the products are slightly less than the mass of the reactants in a Fission/Fusion reaction. 14. Know the important benefits/risks of nuclear energy vs. chemical energy. 15. Know the various isotopes that are useful in everyday life. Know the isotope and what it s used for. 16. Know how to determine the half-life of a radioisotope. 17. Know how to determine the fraction remaining of a radioisotope after a period of time. 18. Be able to calculate the mass of a radioisotope before or after decay has occurred. 19. Know that nothing can change the half-life of a radioisotope.