Chemistry P Syllabus
Chemistry P
Ms. Fine
Topics: First Semester: 1. Scientific Measurement 2. Atomic Structure, Electron Configuration and the Periodic Table 3. Chemical Bonding 4. Stoichiometry
Second Semester: 5. Gases 6. Solutions 7. Acids and Bases 8. Thermochemistry 9. Kinetics and Equilibrium 10. Nuclear Chemistry 11. Organic Chemistry
Grading Policy: Grading Distribution
Grading Scale A 93-100% A90-92% B+ 87-89% B 83-86% B80-82% C+ 77-79%
Tests 45% Quizzes 15% Labs 25% Assignments 15%
C CD+ D DF
73-76% 70-72% 67-69% 63-66% 60-62% 59% or less
Expectations of Students: (1) Be on Time. Be seated in your desk with the required handouts by the time the bell rings. If you are late to class, any assignments due that day are also considered late. (2) Come Prepared. Come to class with the necessary materials. This includes your binder, a pen/pencil, and a calculator. Have homework assignments completed and be ready for quizzes and tests. (3) Work On-Task. Use class time wisely to complete the work that has been assigned. Remain at your desk from the beginning of class until the bell rings unless the teacher has directed you to move or you have asked permission to use the restroom. (4) Act Respectfully. Respect the teacher, other students in the class, and the classroom. Cell phones must be turned off and out of sight during class time or they will be confiscated. (5) Follow the Safety Rules. Read the safety rules and act accordingly at all times. Ensure that these rules have been reviewed and signed by both you and your parent/guardian. Classroom Policy: Quizzes/ Tests Quizzes will be given very frequently. In the case of an absence on the day of a quiz or test, students will be required to write the missed exam during lunch on the day of their return. Labs Labs will take place on a regular basis. A report must be completed for each lab activity. Late labs will lose 20% per day late. In the case of an absence on the day of a lab, students will be required to make up the lab during the designated time. Homework Assignments Homework will be assigned daily. All homework is considered important and is expected to be completed. Review should take place on a regular basis. Students are strongly encouraged to ask for help if they are struggling with concepts. Twenty percent will be deducted for each class day the assignment is late. Notebook Notes will be taken almost every class. Students are expected to copy the notes as they will be evaluated once each unit, on the day before the unit test. The notebook grade will be entered in the assignments category. Absences It is your responsibility to obtain and make up any missed notes and assignments. Assignments are due the day after you return, unless otherwise indicated. Contacting Me: I am available in room I219 at lunch most days. I can be emailed at [email protected]. Website: All course materials can be downloaded from the website below. http://chemin10.com/samohi/chemp
Chemistry P 1st Semester Learning Targets 1. Scientific Measurement 1-1. Define matter and distinguish between a pure substance and a mixture; an element and a compound; a homogeneous mixture and a heterogeneous mixture (by definition and with examples). 1-2. Compare physical changes and chemical reactions by listing the key characteristics of each and giving examples. 1-3. Compare the three phases of matter (solid, liquid, and gas) in terms of molecular speed and molecular spacing, and be able to draw a simple diagram for each state. 1-4. Convert between scientific notation and standard form of a number. 1-5. Convert from one metric unit to another using a metric scale. 1-6. Convert temperature between Fahrenheit, Celsius, and Kelvin. 1-7. Solve conversion problems using dimensional analysis. 1-8. Read metric scales to the correct number of digits and with the correct unit. 1-9. Define density using a mathematical equation and give the appropriate units. 1-10. Perform calculations involving density, mass, and volume, giving answers with the appropriate units. 2. Atomic Structure and Electron Configuration 2-1. Give the one main contribution to the development of the atomic model from each of the following scientists: Dalton, Thomson, Rutherford, Chadwick, and Bohr. 2-2. Identify elements by both name and chemical symbol using a periodic table. 2-3. Compare protons, electrons, and neutrons in terms of charge, mass, and location in an atom. 2-4. Use the periodic table to determine the number of protons, electrons, neutrons, and atomic mass for a given element. 2-5. Define isotope and state how the atomic structure for isotopes of the same element are similar and different. 2-6. Calculate the average atomic mass from the relative abundances and masses of each isotope. 2-7. Define valence electrons and determine the number of valence electrons for an atom. 2-8. Locate rows/periods and groups/families on the periodic table. 2-9. Draw the Bohr diagram for an atom showing protons and neutrons and the number of electrons in each shell. 2-10. Draw the Bohr diagram for the ion of an element, showing how the atom establishes a full valence shell. 2-11. Determine the noble gas that the atom resembles once it forms an ion. 2-12. Define ion and determine the charge for the ion of an element from the periodic table. Determine the number of electrons for an ion. Give the symbol for the ion. 2-13. Define cation and anion. 2-14. List the four different kinds of atomic orbitals by their letter designation and state the number of electrons that each can hold. 2-15. Give orbital notation for a given atom/ion. 2-16. Write electronic configuration for a given atom/ion. 2-17. Write noble gas configuration for a given atom/ion. 2-18. Discuss the development of the periodic table by Mendeleev. 2-19. Locate and state important properties of main chemical families including the alkali metals, alkaline earth metals, transition metals, halogens, noble gases, lanthanides, actinides, and hydrogen. 2-20. Compare metal, nonmetal, and semimetal/metalloid elements in terms of properties and location on the periodic table and give examples of each. 2-21. Define atomic radius explain periodic trends in this property as they relate to atomic structure. 2-22. Define ionization energy and explain periodic trends in this property as they relate to atomic structure. 2-23. Define electronegativity and explain periodic trends in this property as they relate to atomic structure. 2-24. Define ionic radius and relate the size of an anion to a neutral atom of the same element and a cation to a neutral atom of the same element.
3. Chemical Bonding 3-1. Draw electron dot diagrams for atoms, showing the correct number of valence electrons. 3-2. Draw Lewis structures for ionic and covalent compounds from the elements bonding. 3-3. Predict the charges of metal and nonmetal ions from the periodic table. 3-4. Name and write formulas for ionic compounds including compounds with multivalent ions (using roman numerals) and those with polyatomic ions. 3-5. Name and write formulas for acids. 3-6. Name and write formulas for covalent compounds (using prefixes). 3-7. Given any compound, classify as ionic, acid, or covalent and determine the appropriate name. 3-8. Identify diatomic elements and give each with the correct name and formula. 3-9. Compare covalent and ionic compounds in terms of the types of elements involved in bonding and electronic structure. 3-10. Draw Lewis structures for molecules from chemical formulas. 3-11. Assign bond orders for a molecule from the Lewis structure 3-12. Assign shapes to molecules using VSEPR Theory and draw the VSEPR diagram for a molecule. 4. Stoichiometry 4-1. Determine the percent composition for a compound from the chemical formula. 4-2. Determine the percent composition of water in a hydrate. 4-3. Define the quantity one mole by stating Avogadro’s number. 4-4. Determine the number of atoms of each element in a given compound from the chemical formula. 4-5. Define molar mass. 4-6. Determine the molar mass for a given element/compound with the appropriate units. 4-7. Perform conversions between moles, mass, and atoms/molecules and solve problems involving these quantities, giving answers with the appropriate units. 4-8. State the conditions of STP. 4-9. Give Avogadro’s Law by stating volume of one mole of gas at STP. 4-10. Perform calculations for gases at STP involving volume, moles, mass, and atoms/molecules. 4-11. Name and write formulas for hydrates. 4-12. Define evaporation/boiling, condensation, melting, freezing, sublimation, and deposition by stating the beginning phase and ending phase for each change. 4-13. Identify the reactants and products in a chemical equation. 4-14. State the Law of Conservation of Mass. 4-15. Balance chemical equations beginning with either chemical names or formulas. 4-16. Classify reactions as synthesis, decomposition, single replacement, double replacement, neutralization, or combustion. 4-17. Predict the products of a reaction given the formulas or names of reactants. 4-18. Label the state of a substance in a chemical reaction as solid (s), liquid (l), gas (g), or solution (aq). 4-19. Define stoichiometry. 4-20. Determine mole ratios for a reaction from the balanced chemical equation in order to convert between the moles different substances. 4-21. Perform stoichiometric calculations involving mass of a reactant or product, giving answers with the appropriate units.
Chemistry P 2nd Semester Learning Targets 5. Gases 5-1. Define pressure using a mathematical equation. 5-2. Perform calculations involving pressure, force, and area. 5-3. Describe how pressure is measured using a barometer. 5-4. Convert pressure between the units of atmospheres, Pascals, and millimeters of Mercury. 5-5. Perform calculations involving Dalton’s Law of partial pressures. 5-6. Perform calculations involving Boyle’s Law, Charles’ Law, and Gay-Lassac’s Law. 5-7. Solve combined gas law problems. 5-8. Perform calculations using the Ideal Gas Law. 5-9. Perform stoichiometric calculations involving volume of gases at STP. 6. Solutions 6-1. Define a solution and give examples. 6-2. Define solute and solvent and determine the solute and solvent for a given solution 6-3. Define molarity using a mathematical equation and give the appropriate units. 6-4. Perform calculations involving molarity/solution concentration. 6-5. Perform calculations involving solution dilution. 6-6. Define dissociation and describe the interactions between water and ionic compounds that lead to dissociation. 6-7. Write dissociation equations for ionic compounds and represent dissociation equations using a diagram showing ions and water molecules. 6-8. Calculate the concentration of ions in a solution from the concentration of the ionic compound. Compare unsaturated and saturated solutions. 6-9. Determine if a compound is soluble or insoluble in water using a solubility table 6-10. Define precipitate in terms of solubility. 6-11. Write the formula equations, complete ionic equation, and net ionic equation for a precipitation reaction, giving the appropriate state for each substance. 6-12. Describe the effect of temperature on solubility. 6-13. Perform stoichiometric calculations involving molarity of solutions. 7. Acids and Bases 7-1. Define and give examples of acids and bases. 7-2. Give the common properties of acids and bases including colors seen when each is combined with indicators such as phenolphthalein, bromothymol blue, and cabbage juice. 7-3. Calculate pH, pOH, [H+], and [OH‒] for acids and bases. 7-4. Classify a solution as acidic, basic, or neutral from the pH. 8. Thermochemistry 8-1. Define temperature and heat and give appropriate units for each. 8-2. Describe and graph the temperature changes for a heating or cooling curve, and label each part of the curve with the appropriate phase(s). 8-3. Determine the melting/freezing point and boiling/condensing point from a heating or cooling curve. 8-4. Describe what is happening to particles at each region of a heating/cooling curve including where particles begin to move faster/slower and where bonds between particles are broken/formed. 8-5. Define heat of vaporization and heat of fusion and give the appropriate unit for each. 8-6. Perform calculations involving heat of vaporization and heat of fusion for phase changes of substances. 8-7. Define specific heat capacity and give the appropriate units. 8-8. Perform calculations involving specific heat capacity for heating and cooling of substances. 8-9. Define heat of reaction/enthalpy and give the appropriate units. 8-10. Define exothermic and endothermic reactions and give examples of each. 8-11. Determine if a reaction is exothermic or endothermic from the chemical equation or ∆H value. 8-12. Given the ∆H value, add the heat term to the appropriate side of a chemical reaction.
8-13. Calculate the heat of a reaction from tabulated heats of formation. 8-14. Interpret a potential energy diagram to determine heat of reaction and activation energy. 9. Chemical Equilibrium 9-1. Define entropy and enthalpy and determine the enthalpy drive and entropy drive of a chemical reaction in order to predict if a reaction will favor the products, reactants, or establish equilibrium. 9-2. State Le Chatelier’s principle. 9-3. Predict the shift on an equilibrium from changing concentration, temperature, and pressure/volume. 9-4. Write a Keq expression for an equilibrium. 9-5. Calculate Keq for reaction from the concentration of each chemical at equilibrium. 9-6. From the value of Keq, state whether an equilibrium favors the reactants or products. 9-7. Calculate the concentration of a chemical in an equilibrium from Keq and the concentration of other chemicals at equilibrium. 10. Nuclear Chemistry 10-1. Write the nuclide symbol for a given isotope. 10-2. Describe alpha, beta, and gamma radiation and give the appropriate symbol for each 10-3. Define a transmutation and state what types of radiation can lead to a transmutation. 10-4. Define penetrating power and rank alpha, beta, and gamma radiation according to their strength. 10-5. Complete nuclear reactions including those involving alpha, beta or gamma radiations as well as neutrons and protons. 10-6. Define half-life. 10-7. Perform calculations involving half-life in order to solve for mass and time. Organic Chemistry 11-1. Name and draw hydrocarbons including alkanes, cycloalkanes, alkenes, cycloalkenes, and alkynes. 11-2. Match the structure with the correct name for molecules containing common functional groups including alkyl halides, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines, and amides. 11-3. Complete ester condensation reactions.
Ms. Fine
Topics: First Semester: 1. Scientific Measurement 2. Atomic Structure, Electron Configuration and the Periodic Table 3. Chemical Bonding 4. Stoichiometry
Second Semester: 5. Gases 6. Solutions 7. Acids and Bases 8. Thermochemistry 9. Kinetics and Equilibrium 10. Nuclear Chemistry 11. Organic Chemistry
Grading Policy: Grading Distribution
Grading Scale A 93-100% A90-92% B+ 87-89% B 83-86% B80-82% C+ 77-79%
Tests 45% Quizzes 15% Labs 25% Assignments 15%
C CD+ D DF
73-76% 70-72% 67-69% 63-66% 60-62% 59% or less
Expectations of Students: (1) Be on Time. Be seated in your desk with the required handouts by the time the bell rings. If you are late to class, any assignments due that day are also considered late. (2) Come Prepared. Come to class with the necessary materials. This includes your binder, a pen/pencil, and a calculator. Have homework assignments completed and be ready for quizzes and tests. (3) Work On-Task. Use class time wisely to complete the work that has been assigned. Remain at your desk from the beginning of class until the bell rings unless the teacher has directed you to move or you have asked permission to use the restroom. (4) Act Respectfully. Respect the teacher, other students in the class, and the classroom. Cell phones must be turned off and out of sight during class time or they will be confiscated. (5) Follow the Safety Rules. Read the safety rules and act accordingly at all times. Ensure that these rules have been reviewed and signed by both you and your parent/guardian. Classroom Policy: Quizzes/ Tests Quizzes will be given very frequently. In the case of an absence on the day of a quiz or test, students will be required to write the missed exam during lunch on the day of their return. Labs Labs will take place on a regular basis. A report must be completed for each lab activity. Late labs will lose 20% per day late. In the case of an absence on the day of a lab, students will be required to make up the lab during the designated time. Homework Assignments Homework will be assigned daily. All homework is considered important and is expected to be completed. Review should take place on a regular basis. Students are strongly encouraged to ask for help if they are struggling with concepts. Twenty percent will be deducted for each class day the assignment is late. Notebook Notes will be taken almost every class. Students are expected to copy the notes as they will be evaluated once each unit, on the day before the unit test. The notebook grade will be entered in the assignments category. Absences It is your responsibility to obtain and make up any missed notes and assignments. Assignments are due the day after you return, unless otherwise indicated. Contacting Me: I am available in room I219 at lunch most days. I can be emailed at [email protected]. Website: All course materials can be downloaded from the website below. http://chemin10.com/samohi/chemp
Chemistry P 1st Semester Learning Targets 1. Scientific Measurement 1-1. Define matter and distinguish between a pure substance and a mixture; an element and a compound; a homogeneous mixture and a heterogeneous mixture (by definition and with examples). 1-2. Compare physical changes and chemical reactions by listing the key characteristics of each and giving examples. 1-3. Compare the three phases of matter (solid, liquid, and gas) in terms of molecular speed and molecular spacing, and be able to draw a simple diagram for each state. 1-4. Convert between scientific notation and standard form of a number. 1-5. Convert from one metric unit to another using a metric scale. 1-6. Convert temperature between Fahrenheit, Celsius, and Kelvin. 1-7. Solve conversion problems using dimensional analysis. 1-8. Read metric scales to the correct number of digits and with the correct unit. 1-9. Define density using a mathematical equation and give the appropriate units. 1-10. Perform calculations involving density, mass, and volume, giving answers with the appropriate units. 2. Atomic Structure and Electron Configuration 2-1. Give the one main contribution to the development of the atomic model from each of the following scientists: Dalton, Thomson, Rutherford, Chadwick, and Bohr. 2-2. Identify elements by both name and chemical symbol using a periodic table. 2-3. Compare protons, electrons, and neutrons in terms of charge, mass, and location in an atom. 2-4. Use the periodic table to determine the number of protons, electrons, neutrons, and atomic mass for a given element. 2-5. Define isotope and state how the atomic structure for isotopes of the same element are similar and different. 2-6. Calculate the average atomic mass from the relative abundances and masses of each isotope. 2-7. Define valence electrons and determine the number of valence electrons for an atom. 2-8. Locate rows/periods and groups/families on the periodic table. 2-9. Draw the Bohr diagram for an atom showing protons and neutrons and the number of electrons in each shell. 2-10. Draw the Bohr diagram for the ion of an element, showing how the atom establishes a full valence shell. 2-11. Determine the noble gas that the atom resembles once it forms an ion. 2-12. Define ion and determine the charge for the ion of an element from the periodic table. Determine the number of electrons for an ion. Give the symbol for the ion. 2-13. Define cation and anion. 2-14. List the four different kinds of atomic orbitals by their letter designation and state the number of electrons that each can hold. 2-15. Give orbital notation for a given atom/ion. 2-16. Write electronic configuration for a given atom/ion. 2-17. Write noble gas configuration for a given atom/ion. 2-18. Discuss the development of the periodic table by Mendeleev. 2-19. Locate and state important properties of main chemical families including the alkali metals, alkaline earth metals, transition metals, halogens, noble gases, lanthanides, actinides, and hydrogen. 2-20. Compare metal, nonmetal, and semimetal/metalloid elements in terms of properties and location on the periodic table and give examples of each. 2-21. Define atomic radius explain periodic trends in this property as they relate to atomic structure. 2-22. Define ionization energy and explain periodic trends in this property as they relate to atomic structure. 2-23. Define electronegativity and explain periodic trends in this property as they relate to atomic structure. 2-24. Define ionic radius and relate the size of an anion to a neutral atom of the same element and a cation to a neutral atom of the same element.
3. Chemical Bonding 3-1. Draw electron dot diagrams for atoms, showing the correct number of valence electrons. 3-2. Draw Lewis structures for ionic and covalent compounds from the elements bonding. 3-3. Predict the charges of metal and nonmetal ions from the periodic table. 3-4. Name and write formulas for ionic compounds including compounds with multivalent ions (using roman numerals) and those with polyatomic ions. 3-5. Name and write formulas for acids. 3-6. Name and write formulas for covalent compounds (using prefixes). 3-7. Given any compound, classify as ionic, acid, or covalent and determine the appropriate name. 3-8. Identify diatomic elements and give each with the correct name and formula. 3-9. Compare covalent and ionic compounds in terms of the types of elements involved in bonding and electronic structure. 3-10. Draw Lewis structures for molecules from chemical formulas. 3-11. Assign bond orders for a molecule from the Lewis structure 3-12. Assign shapes to molecules using VSEPR Theory and draw the VSEPR diagram for a molecule. 4. Stoichiometry 4-1. Determine the percent composition for a compound from the chemical formula. 4-2. Determine the percent composition of water in a hydrate. 4-3. Define the quantity one mole by stating Avogadro’s number. 4-4. Determine the number of atoms of each element in a given compound from the chemical formula. 4-5. Define molar mass. 4-6. Determine the molar mass for a given element/compound with the appropriate units. 4-7. Perform conversions between moles, mass, and atoms/molecules and solve problems involving these quantities, giving answers with the appropriate units. 4-8. State the conditions of STP. 4-9. Give Avogadro’s Law by stating volume of one mole of gas at STP. 4-10. Perform calculations for gases at STP involving volume, moles, mass, and atoms/molecules. 4-11. Name and write formulas for hydrates. 4-12. Define evaporation/boiling, condensation, melting, freezing, sublimation, and deposition by stating the beginning phase and ending phase for each change. 4-13. Identify the reactants and products in a chemical equation. 4-14. State the Law of Conservation of Mass. 4-15. Balance chemical equations beginning with either chemical names or formulas. 4-16. Classify reactions as synthesis, decomposition, single replacement, double replacement, neutralization, or combustion. 4-17. Predict the products of a reaction given the formulas or names of reactants. 4-18. Label the state of a substance in a chemical reaction as solid (s), liquid (l), gas (g), or solution (aq). 4-19. Define stoichiometry. 4-20. Determine mole ratios for a reaction from the balanced chemical equation in order to convert between the moles different substances. 4-21. Perform stoichiometric calculations involving mass of a reactant or product, giving answers with the appropriate units.
Chemistry P 2nd Semester Learning Targets 5. Gases 5-1. Define pressure using a mathematical equation. 5-2. Perform calculations involving pressure, force, and area. 5-3. Describe how pressure is measured using a barometer. 5-4. Convert pressure between the units of atmospheres, Pascals, and millimeters of Mercury. 5-5. Perform calculations involving Dalton’s Law of partial pressures. 5-6. Perform calculations involving Boyle’s Law, Charles’ Law, and Gay-Lassac’s Law. 5-7. Solve combined gas law problems. 5-8. Perform calculations using the Ideal Gas Law. 5-9. Perform stoichiometric calculations involving volume of gases at STP. 6. Solutions 6-1. Define a solution and give examples. 6-2. Define solute and solvent and determine the solute and solvent for a given solution 6-3. Define molarity using a mathematical equation and give the appropriate units. 6-4. Perform calculations involving molarity/solution concentration. 6-5. Perform calculations involving solution dilution. 6-6. Define dissociation and describe the interactions between water and ionic compounds that lead to dissociation. 6-7. Write dissociation equations for ionic compounds and represent dissociation equations using a diagram showing ions and water molecules. 6-8. Calculate the concentration of ions in a solution from the concentration of the ionic compound. Compare unsaturated and saturated solutions. 6-9. Determine if a compound is soluble or insoluble in water using a solubility table 6-10. Define precipitate in terms of solubility. 6-11. Write the formula equations, complete ionic equation, and net ionic equation for a precipitation reaction, giving the appropriate state for each substance. 6-12. Describe the effect of temperature on solubility. 6-13. Perform stoichiometric calculations involving molarity of solutions. 7. Acids and Bases 7-1. Define and give examples of acids and bases. 7-2. Give the common properties of acids and bases including colors seen when each is combined with indicators such as phenolphthalein, bromothymol blue, and cabbage juice. 7-3. Calculate pH, pOH, [H+], and [OH‒] for acids and bases. 7-4. Classify a solution as acidic, basic, or neutral from the pH. 8. Thermochemistry 8-1. Define temperature and heat and give appropriate units for each. 8-2. Describe and graph the temperature changes for a heating or cooling curve, and label each part of the curve with the appropriate phase(s). 8-3. Determine the melting/freezing point and boiling/condensing point from a heating or cooling curve. 8-4. Describe what is happening to particles at each region of a heating/cooling curve including where particles begin to move faster/slower and where bonds between particles are broken/formed. 8-5. Define heat of vaporization and heat of fusion and give the appropriate unit for each. 8-6. Perform calculations involving heat of vaporization and heat of fusion for phase changes of substances. 8-7. Define specific heat capacity and give the appropriate units. 8-8. Perform calculations involving specific heat capacity for heating and cooling of substances. 8-9. Define heat of reaction/enthalpy and give the appropriate units. 8-10. Define exothermic and endothermic reactions and give examples of each. 8-11. Determine if a reaction is exothermic or endothermic from the chemical equation or ∆H value. 8-12. Given the ∆H value, add the heat term to the appropriate side of a chemical reaction.
8-13. Calculate the heat of a reaction from tabulated heats of formation. 8-14. Interpret a potential energy diagram to determine heat of reaction and activation energy. 9. Chemical Equilibrium 9-1. Define entropy and enthalpy and determine the enthalpy drive and entropy drive of a chemical reaction in order to predict if a reaction will favor the products, reactants, or establish equilibrium. 9-2. State Le Chatelier’s principle. 9-3. Predict the shift on an equilibrium from changing concentration, temperature, and pressure/volume. 9-4. Write a Keq expression for an equilibrium. 9-5. Calculate Keq for reaction from the concentration of each chemical at equilibrium. 9-6. From the value of Keq, state whether an equilibrium favors the reactants or products. 9-7. Calculate the concentration of a chemical in an equilibrium from Keq and the concentration of other chemicals at equilibrium. 10. Nuclear Chemistry 10-1. Write the nuclide symbol for a given isotope. 10-2. Describe alpha, beta, and gamma radiation and give the appropriate symbol for each 10-3. Define a transmutation and state what types of radiation can lead to a transmutation. 10-4. Define penetrating power and rank alpha, beta, and gamma radiation according to their strength. 10-5. Complete nuclear reactions including those involving alpha, beta or gamma radiations as well as neutrons and protons. 10-6. Define half-life. 10-7. Perform calculations involving half-life in order to solve for mass and time. Organic Chemistry 11-1. Name and draw hydrocarbons including alkanes, cycloalkanes, alkenes, cycloalkenes, and alkynes. 11-2. Match the structure with the correct name for molecules containing common functional groups including alkyl halides, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines, and amides. 11-3. Complete ester condensation reactions.
