Chemistry Matter and Measurement 1

1. REVIEW CHAPTERS 1, 2, 3 0 Chemistry Matter and Measurement 1 • Chapter Overview •  1.1 Chemical Foundations • 1.2 Scientific Method :Observation – hypothesis – • law – theory - experiment • 1.3-1.7 Classification of Matter • A. Physical property • Observable without changing the identity • B. Chemical Property • Observable only by changing the identity- • Chemical reactions • Physical Change • Chemical Change

2. 1 Units of Measurements (table 1.1 and 1.2) • SI units: length, mass, time, temperature, amt of substance • meter, kilogram, second, Kelvin , mole • 2Uncertainity in Measurements • Precision and Accuracy, standard deviation and % error • 3 Significant Figures and Calculation- exponential notation • Significant figures • Significant Figures in Calculations • -Multiplication and Division: Answer with lowest Sig. Fig • -Add/Subtract: Answer with least decimal place • -All together- Do parentheses first, then add/subtract-with decimal places, then multiply-Divide minimum sig fig. Table 1.2 • Significant Figures: Writing Numbers to Reflect Position • A. How many digits can I report? How many should I report? • B. Certain digits and estimated digits • C. Counting significant figures • 1. All nonzero digits are significant 1234 = 4 Sig fig • 2. Interior zeros are significant 505 = 3 sig fig • 3. Trailing zeros after a decimal are significant 55.00 = 4 sig fig • 4. Leading zeros are not significant 0.012 = 2 sig fig • 5. Zeros at the end of a number, without a decimal point, are ambiguous 150 = ambiguous • D. Exact numbers

3. 4 Converting from One Unit to Another (UNIT 1 to UNIT 2) • A. Units are important, most numbers get one • B. Include units in all calculations • C. Conversion factors (Unit you have comes in the bottom, unit you want comes in the TOP) • Unit 1 X Unit 2 = UNIT 2 • Unit 1 • D. Significant figure of the final answer depends on UNIT 1 given in problem NOT the sig. fig of the conversion factor(s) • Temperature: Random Molecular and Atomic Motion • Conversions And 1.8 Density (D= Mass/Volume) A. Mass per unit volume (D= Mass/Volume) B. Derived unit Volume = Mass/Density Mass = Density X Volume C. Can be used as a conversion factor between mass and volume

4. Atoms, Molecules and Ions 2/3 0 • 2.1 and 2.2Laws of Chemical Combination, Chemical Laws • 2.3 John Dalton and the Atomic Theory of Matter • 2.1 Divisible Atoms (Protons(+1, 1u), electrons(-1, 1/2000th u), neutrons(0,1u)) • Isotopes – atoms of same element having different mass no. (due to DIFFERENT # of neutrons) • 2.2-2.4 Atomic Masses Calculation problems ( Isotopes and abundances) • Isotope symbols for atoms and ions • 2.5 The Periodic Table: Elements Organized • Looking for Patterns: The Periodic Law and the Periodic Table • A. Mendeleev (1834 - 1907) • B. Periodic law • C. Metals • D. Nonmetals • E. Metalloids, also known as semiconductors • F. Individual group names • 1. Group 1 – alkali metals • 2. Group 2 – alkali earth metals • 3. Group 7 – halogens • 4. Group 8 – noble gases

5. 2.6Molecules and Ions • Nomenclature (between 2 or more non metals!!!) • Use of prefix and suffix (di, tri etc) • Prefix)name of first element + (prefix) base name of second element + ide • More positive non metal written first • 2.7 Ions and Ionic Compounds • Naming Ionic Compounds • A. Type I compounds • 1. Metal in compounds forms only one type of ion • 2. Most main group metals form type I compounds • B. Naming type I binary ionic compounds • 1. Name of cation (metal) + (base name of anion + ide) • 2. Example, NaCl is sodium chloride • C. Type II compounds • 1. Metal forms more than one type of ion • 2. Transition metals usually, but not exclusively, form type II compounds • D. Naming type II binary ionic compounds • 1. Name of cation + (charge of cation) + (base name of anion + ide) • 2. Charge of cation given in roman numerals • 3. FeCl3 is iron (III) chloride • E. Naming ionic compounds containing a polyatomic ion • 1. Use the same procedure as ionic compounds • 2. Use name of polyatomic ion, not constituent atoms • 3. Example, NaNO3 is sodium nitrate

6. 3. 6 Acids, Bases, and Salts (Nomenclature of acids) Naming Acids A. Molecular compounds that dissolve in water to form H+ ions B. Binary acids 1. Hydrogen and nonmetal 2. (Hydro + base name of nonmetal + ic) + acid 3. Example, HCl is Hydrochloric acid C. Oxyacids 1. Hydrogen and polyatomic oxyanion 2. Oxyanions ending with –ate a. (Base name of oxyanion + ic) + acid b. Example, HNO3 is nitric acid 3. Oxyanions ending with –ite a. (Base name of oxyanion + ous) + acid b. Example, HNO2 is nitrous acid

7. Combined concepts from Chapter 2 and 3 2.9 Counting by weight, The Mole and Molar Mass 2.10 Molecular Masses and Formula Masses, Percent Composition 3 Emprical/Chemical Formulas from Mass Percent Composition 3.1 Chemical Equations 3.2 Writing and Balancing Chemical Equations

8. Chapter 3 Some Electrical Properties of Aqueous Solutions

10. Reactions Involving Oxidation and Reduction-Redox, Single Dispalcement Reactions • -Oxidation involves LOSS of Electrons “OIL” • Reduction involves GAIN of Electrons “RIG” • Oxidation Number (ON) rules: 2 Single -displacement reaction,. Activity series in metals Look up Single-Double displacement lab for Practice

11. 0 EXAM 1- 100 POINTS 10 points Bonus question!! Part 1 Multiple Choice –Show calculations for partial/full credit 15 questions Part 2 Density, Moles, atomic mass, empirical formulas, yield, limiting agent questions, Single-Double displacement reactions Bonus question: