1 0110 F24 Outline of Possible Exam 1 Material.pdf

OpenStax Possible Exam 1 Material Chapter 1 Essential Ideas Section 1.1 Chemistry in Context Strive to recognize chemistry in everyday life Understand and apply the scientific method Describe how you have used the scientific method Explain the difference between a theory and a l...

OpenStax Possible Exam 1 Material Chapter 1 Essential Ideas Section 1.1 Chemistry in Context Strive to recognize chemistry in everyday life Understand and apply the scientific method Describe how you have used the scientific method Explain the difference between a theory and a law Distinguish between o Macroscopic domain o Microscopic domain o Symbolic domain Section 1.2 Phases and Classification of Matter Distinguish between a o solid o liquid o gas o plasma Distinguish between o mass o weight Become familiar with the law of conservation of mass Use the law of conservation of mass in calculations Distinguish between elements and compounds Distinguish between a pure substance and a mixture Distinguish between a physical change and a chemical change Understand that physical properties allow us to characterize, purify, and identify substances Differentiate between a homogeneous mixture and a heterogeneous mixture Understand the term phase as it relates to mixtures and to states of matter Section 1.3 Physical and Chemical Properties Explain the difference between physical and chemical properties Distinguish between o extensive physical properties o intensive physical properties Recognize o physical changes o chemical changes Identify in the periodic table o metallic elements o nonmetallic elements o metalloids OpenStax Possible Exam 1 Material Section 1.4 Measurements Understand that measurements include o magnitude o unit o uncertainty Determine the number of significant digits in a number Use o significant figures to indicate the precision of a measured value o scientific notation to represent numbers o the seven base units (table 1.2, page 30, OpenStax text) o the SI prefixes (table 1.3, page 31, OpenStax text) o derived units, such as volume and density o carry out density calculations Section 1.5 Measurement Uncertainty, Accuracy, and Precision Use scientific notation in calculations Report the correct number of significant digits in the result of a calculation Recognize quantities that are exact numbers Round answers to calculations to the correct number of significant digits Correctly apply the terms precision and accuracy Section 1.6 Mathematical Treatment of Results Convert between C, F, and K Perform calculations using the factor-label method or dimensional analysis Understand that an equality provides two conversion factors Understand the molar mass is a conversion factor Chapter 2 Atoms, Molecules, and Ions Section 2.1 Early Ideas in Atomic Theory Understand postulates of Dalton’s atomic theory as related to o Atomic theory o Element o Compound o Chemical reaction Atomic symbols o Recognize atomic symbols; understand their meaning o Become familiar with the symbols listed in Table 2.1 Understand the deductions obtained from Dalton’s atomic theory o Law of multiple proportions Section 2.2 Evolution of Atomic Theory Become familiar with experiments by o J. J. Thompson (~1897); atoms are not indivisible particles; obtained mass to charge ratio of electron OpenStax Possible Exam 1 Material o Robert Milliken (~1909); oil drop experiments; determined charge of electron o Ernest Rutherford (~1911); gold foil experiments; nuclear model of the atom o Frederick Soddy (early 1900’s); isotopes o James Chadwick (~1932) provided evidence for neutrons Section 2.3 Atomic Structure and Symbolism Know the structure of the atom Nucleus o Protons (positive) o Neutrons (neutral) o Electrons (negative) Know the relative masses and charges of protons, neutrons and electrons (table 2.2, page 80, OpenStax text) Recognize that the o atomic number (Z) is the number of protons in the nucleus o mass number (A) is the total number of protons and neutrons in an atom’s nucleus Distinguish between atoms and ions o Atoms are neutral o Ions are charged ▪ Cations are positive ▪ Anions are negative Recognize the symbols of the elements in the periodic table Become familiar with the elements that the symbols represent Write the symbols for isotopes of elements Calculate the o average mass of an atom of an element o percent composition of a sample of an element Section 2.4 Chemical Formulas Recognize chemical formulas Distinguish between formulas for ionic compounds and molecular compounds Recognize o structural isomers o geometric isomers Section 2.5 The Periodic Table Mendeleev (1869); Meyer (1870) Be familiar with the periodic law Be familiar with the organization of the periodic table o Elements arranged according to increasing atomic number. o Elements in the same row are in the same period (period goes across the periodic table). o Elements in the same column are in the same group (group goes down the periodic table). Distinguish between metals and nonmetals according to OpenStax Possible Exam 1 Material o Position in the periodic table o Physical properties Identify the o Alkali metals o Alkaline earth metals o Chalcogens o Halogens o Noble gases o Transition metals o Inner transition metal ▪ Lanthanides ▪ Actinides Be familiar with trends in effective nuclear charge and electronegativity Section 2.6 Molecular and Ionic Compounds Recognize that chemical reactions involve rearrangement of atoms and electrons Atoms combine so that (in general) each atom can achieve an octet o Some atoms become ions that engage in ionic bonds o Some atoms share electrons to form covalent bonds Ionic compounds form from ionic bonds Molecular compounds form from covalent bonds Section 2.7 Chemical Nomenclature (Naming) Distinguish between o organic and inorganic compounds o molecular and ionic compounds Name o binary compounds o ionic compounds (Including those with metals that have variable charges) o ionic hydrates o molecular inorganic compounds o binary acids o oxoacids Know the six common strong acids and the six common strong bases Always remember that the stronger acid has the weaker, more stable, conjugate base. OpenStax Possible Exam 1 Material Chapter 3 Composition of Substances and Solutions Section 3.1 Formula Mass and the Mole Concept Determine the formula mass of a molecule, an ionic compound, or a polyatomic ion Understand that the mole is the SI unit for chemical quantity o 1 mol = 6.02 x 1023 atoms, molecules, etc. o The value 6.02214179 x 1023 is called Avogadro’s number. Understand o # of atoms in mole of A = # of atoms in mole of B o mass of a mole of A  mass of a mole of B Recognize that the molar mass of a substance is the mass (g) of a mole of that substance o Molar mass units are grams per mol (g/mol). Understand that the molar mass of any element, numerically, is equal to that element’s atomic mass in amu Become proficient at converting between mass, moles, number of molecules, and number of atoms in a substance Section 3.2 Determining Empirical and Molecular Formulas Become proficient at determining o percent composition from ▪ The masses of atoms in a substance (Example 3.9, Pages 144-145) ▪ The molecular formula of a substance (Example 3.10, Pages 145-146) o Empirical formula from ▪ Masses of the elements in a substance (Example 3.11, Pages 147-148) ▪ Percent composition (Example 3.12, Pages 148-149) o Molecular formula from empirical formula and molecular mass of the substance (Example 3.13, Pages 150-151) Section 3.3 Molarity Understand that o Concentration is the amount of a solute in a solution. o Solute is the dissolved substance. o Solvent is the liquid in which the solute is dissolved. o Solution is the combination of the solute and the solvent. Distinguish between o solute, solvent, and solution o concentrated and dilute solutions Recognize molarity as a common concentration term o Molarity = (moles of solute)/ (volume of solution) o Units: M = mol/L Become proficient at calculating OpenStax Possible Exam 1 Material o Molar concentration (Example 3.14, page 153) o Moles and volumes from molar concentration (Example 3.15, page 153) o Molar concentration from solute mass (Example 3.16, pages 153- 154) o Mass of solute in each volume of solution (Example 3.17, pages 154-155) o Volume of solution containing a given mass of solute (Example 3.18, page 155-156) Section 3.4 Other Units for Solution Concentrations Become proficient at calculations that involve o mass percentage (Examples 3.22 and 3.23, pages 160-161) o volume percentage (Example 3.24, pages 161-162) o mass-volume percentage (Example 3.25, page 162) o parts per million and parts per billion (Example 3.25, page 163) Chapter 4 Stoichiometry of Chemical Reactions Section 4.1 Writing and Balancing Chemical Equations Write balanced chemical equations from names of substances in the reaction Identify and recognize o Reactants o Products o Phase labels o Stoichiometric coefficients Recognize molecular and molar interpretations of chemical equations (Pages 176-177) Balance chemical equations Write balanced o molecular equations o complete ionic equations o net ionic equations Explain the usefulness and application of net ionic equations Section 4.2 Classifying Chemical Reactions Distinguish between redox reactions and other reactions Recognize the differences and similarities between precipitation reactions and acid-base reactions Recognize, from a complete balanced equation whether a precipitate has formed Distinguish between strong and weak acids and bases Recognize neutralization reactions Determine whether a redox reaction has occurred o assign oxidation states o identify species that is ▪ oxidized ▪ reduced Recognize that single displacement and combustion reactions are redox reactions. Recognize that decomposition reactions and combination reactions might be redox.