Chemistry 3 rd 6 Weeks

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1 NAME OF UNIT UNIT III Components Unit Name ESTIMATED # OF DAYS 3 rd 6 Weeks_ Weeks 1-2 Weeks 3-4 IIIA: Writing Formulas and Naming Compounds IIIB: The Mole Short Descriptive Overview TEKS In this unit, students will learn to describe, name, and write formulas for different types of chemical compounds. 1-A, B, C 2-A, B, C, D, E, F, G, H, I 3-A, B, C, D, E, F (7) Science concepts. The student knows how atoms form ionic, metallic, and covalent bonds. The student is expected to: (A) name ionic compounds containing main group or transition metals, covalent compounds, acids, and bases, using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules; (B) write the chemical formulas of common polyatomic ions, ionic compounds containing main group or transition metals, covalent compounds, acids, and bases; (C) construct electron dot formulas to illustrate ionic and covalent bonds; In this chapter, students will be introduced to the mole as the basic SI unit for measuring the amount of a substance, as well as empirical and molecular formulas, percent composition, and hydrates. 1-A, B, C 2-A, B, C, D, E, F, G, H, I 3-A, B, C, D, E, F (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; Supporting (B) use the mole concept to calculate the number of atoms, ions, or molecules in a sample of material; (C) calculate percent composition and empirical and molecular formulas; Supporting Generalizations/Enduring Understandings 1) Binary ionic compounds are formed from a metal (cation) and a nonmetal (anion). 1) The mole is a counting unit used to express the number of particles in a sample with a given mass. 08/19/20127:34 AM 1

2 Guiding/Essential Questions Learning Targets 2) All ionic compounds have an overall charge of zero, so the total positive charge must equal the total negative change. 3) Ionic compounds are named by naming the cation first, followed by the anion. 4) Binary molecular compounds are formed from two nonmetals. 5) Molecular compounds are named by using prefixes. 1) What role do positive and negative charges play in the formation of ions? 2) How can two elements combine to form more than one chemical compound? 3) What are the rules for naming monatomic and polyatomic ions? 4) How do you write the formulas for ionic compounds? 5) What do prefixes tell you about the composition of binary molecular compounds? Performance Learning Levels create formulas for ionic compounds, covalent compounds and acids. distinguish between ionic and covalent molecules 2) Progressions define cation and anion and relate them to metal and nonmetal. 3) apply the periodic table to determine the charge of a monatomic ion. 4) define a polyatomic ion and give the names and formulas of the most common 2) The mole is used in many important conversions involving mass, volume, and 3) Anhydrous compounds are formed by heating hydrates until all of the water boils out of the compound. 1) What chemical unit could you use to measure the amount of sand in a sand sculpture? 2) What molar relationship do chemists use to solve problems? 3) What is the percent composition of a substance, and how is it calculated? Performance Levels 1) The students will quantify the amount of matter using the unit Mole. calculate common mole conversions. Learning Progressions describe how Avogadro s number is related to a mole of any substance. 3) use formulas to calculate the molar mass of a substance. 4) use the mole to convert among measurements of mass, volume, and 08/19/20127:34 AM 2

3 discover rules for naming compounds. distinguish between ionic and covalent molecules polyatomic ions. 5) apply the rules for naming and writing formulas. 5) calculate the percent composition of a substance from its chemical formula or 6) derive the empirical formula and the molecular formula of a compound from Concepts Chemical Names and Formulas Chemical Quantities (the Mole) Topics Monatomic Ions The Mole Stock System Avogadro s Number Polyatomic Ions Molar Mass Ionic Compound % Composition Molecular (Covalent) Compounds Molar Volume Prefixes STP Conversions with moles Hydrates Anhydrous Compounds Essential Facts 1) A compound is either molecular (covalent) or ionic in nature. 2) Molecular compounds are composed of two or more nonmetals. 3) A molecular formula shows the number and kinds of atoms present in a molecule of a compound. 4) Ionic composed are composed of oppositely charged ions (cations and anions) combined in electrically neutral groupings. 5) A formula unit gives the lowest wholenumber ratio of ions in the compound. 6) The charges of the ions of the 1) The SI unit that measures the amount of substance is the mole. 2) A mole of any substance is composed of Avogadro s number (6.02 x ) of representative particles. 3) The representative particle of elements is the atom, of molecular (covalent) compounds is the molecule, and of ionic compounds is the formula unit. 4) The molar mass of a substance is the mass in grams of one mole of that substance. 5) One mole of any substance contains the same number of representative particles as 08/19/20127:34 AM 3

4 Processes and Skills representative elements can be determined by the position of these elements in the periodic table. 7) Most transition metals have more than one common ionic charge. 8) A polyatomic ion is a group of atoms that behaves as a unit and has a charge. 9) Binary ionic compounds are named by writing the name of the cation followed by the name of the anion. 10) When a cation can have more than one ionic charge, a Roman numeral is used in the name. 11) Ternary ionic compounds contain at least one polyatomic ion. These compounds are named by writing the name of the cation followed by the name of the anion. 12) Binary molecular compounds are composed of two nonmetallic elements. 13) The name of a binary molecular compound always ends in ide. 14) Prefixes are used to show how many atoms of each element are present in a molecule of the compound. 1) Distinguish between ionic and molecular compounds. 2) Define cation and anion and relate them to metal and nonmetal. 3) Use the periodic table to determine the charge of a monatomic ion. 4) Define a polyatomic ion and give the names and formulas of the most common polyatomic ions. 5) Apply the rules for naming and writing formulas for ionic compounds. 6) Apply the rules for naming and writing one mole of any other substance. 6) One mole of any gas at STP (1 atm pressure and 0 C) occupies a volume of 22.4 L. 7) The percent composition is the percent by mass of each element in a compound. 8) An empirical formula is the simplest whole-number ratio of atoms of the elements in a compound. 9) A molecular formula gives the true formula of the compound. 1) Describe how Avogadro s number is related to a mole of any substance. 2) Calculate the mass of a mole of any substance. 3) Use the molar mass to convert between mass and moles of a substance. 4) Use the mole to convert among measurements of mass, volume, and 5) Calculate the percent composition of a substance from its chemical formula or 08/19/20127:34 AM 4

5 Language of Instruction Formative Assessment (for learning) Summative Assessment (of learning) Required Lab formulas for binary molecular compounds. Anion, Binary Compound, Cation, Chemical Formula, Formula Unit, Ion Ionic Compound, Molecular Compound, Molecular Formulas, Molecule, Monatomic Ion, Polyatomic Ion, Quaternary Compound, Ternary Compound. Bonding Quiz or Stated Question Naming and the Mole Test 100 Reproducible Activities: Chemistry by Instructional Fair, Inc (workbook) p. 38,39,40,44,45,46,48 6) Derive the empirical formula and the molecular formula of a compound from Anhydrous, Avogadro s Number, Empirical Formula, Molecular Formula, Gram Formula Mass, Gram Molecular Mass, Hydrate, Molar Mass, Molar Volume, Mole, Percent Composition, Representative Particle, STP. Mole Quiz 100 Reproducible Activities: Chemistry by Instructional Fair, Inc (workbook) p. 49,50,51,52,53,54,55,56, Reproducible Activities: Physical Science by Instructional Fair, Inc (workbook) p. 53 Other Resources Chapter 6 Chapter 7 Textbook Correlation Link to Environmental Awareness, p. 160 Challenge/Extension Chemistry Serving the Consumer, p. 164 Chemistry in Careers (Pharmacist), p. 870 Other Curricular Connection (ELA, Math, S.S., Technology) Chemistry Serving the Environment, p. 196 Chemistry in Careers (Ecologist), p /19/20127:34 AM 5