CHEM139 Final Exam Study Guide page 1 of 9 CHEM 139: Final Exam Study Guide Chapter 1 • Know the Scientific method • Know the definitions for hypothesis, scientific law, and scientific theory. Chapter 2 • Length, mass, weight, volume - Know 1 cm3≡1 mL and 1 dm3≡1 L • Significant figures and Scientific notation - Rounding, in addition or subtraction, in multiplication or division - Keep as many sig figs until final answer • Scientific notation • Metric system - Know all the metric prefixes given on p. 9 in the Chapter 2 lecture notes - Be able to perform metric-metric conversions using these prefixes • Use the metric-English conversions provided (1 in. ≡2.54 cm; 1 lb=453.6 g; 1 qt=946 mL) • Volume by calculation - Vrectangular solid = length x width x thickness • Volume by displacement • Density: d =mV - Calculate density, mass, or volume - Identify what items sink or float given densities of liquids and solids. • Temperature - Know the formulas for converting ˚F-to-˚C or ˚C-to-˚F and K-to-˚C or ˚C-to-K • Percentage: ratio of parts per 100 parts - Given amount of part and whole, calculate % - Use a given % to solve for part or whole - Calculate weighted averages keeping track of sig figs and decimal places when appropriate. Chapter 3 • Know that matter is studied at the macroscopic, microscopic, particulate (molecular) levels • Physical states of matter - Determine physical state of substances (solids, liquids, gases) given descriptions of volume, shape, particles moving, etc. • Be able to identify properties and changes as physical or chemical - Know terms for changes of state: - Melting, freezing, vaporizing, condensation, sublimation, deposition • Classification of matter – Classify substances as elements, compounds, or mixtures – Classify molecular-level images as elements, compounds, or mixtures and solids, liquids, or gases – Distinguish between homogeneous and heterogeneous mixtures • Chemical reaction: - reactants: starting materials - products: substances produced in reaction • Law of Conservation of Mass - Solve problems conserving mass.CHEM139 Final Exam Study Guide page 2 of 9 Chapter 10 kinetic energy (KE): energy associated with an object’s motion - Faster objects have higher KE. - Know the relative kinetic energy of solids, liquids, and gases potential energy (PE): energy due to its position or composition (chemical bonds) heat: energy is transferred from a hotter substance to a cooler substance – Identify what lost heat and gained heat given different scenarios. Endothermic versus Exothermic changes: – endothermic: a change requiring energy – exothermic: a change that releases energy Endothermic versus Exothermic changes: – Determine if a physical change or chemical change is exothermic or endothermic. • Law of Conservation of Mass - Solve problems conserving mass. • Law of Conservation of Energy - Know 6 forms of energy: heat, chemical, light, electrical, mechanical, and nuclear joule (J): SI unit of energy; 1 kJ=1000 J calorie (cal): energy needed to raise the temperature of 1 g of water by 1˚C Be able to carry out calculations involving energy in J, cal, Cal, and kilowatt-hours (kW·h). specific heat (in J/g⋅˚C): amount of heat to raise temp. of 1 gram of a substance by 1˚C. - Recognize that the higher the heat capacity of a substance, the more heat it can absorb before its temperature rises. Chapter 4 • Know Rutherford’s Alpha Scattering Experiment and what was determined from it (atomic nucleus, atom mostly empty space, relative size of atom relative to its nucleus) • Subatomic particles – proton (p+): +1 charge, inside nucleus – neutron (n): neutral, inside nucleus – electron (e–): –1 charge, outside nucleus • Electrostatic force: force resulting from a charge on particles - Objects w/ like charges repel one another. - Objects w/ unlike charges attract each other. • Know definitions of isotope, atomic mass • Atomic notation: atomic number = Zmass number = AE = element symbol mass # (A): # of protons + # of neutrons atomic # (Z): # of protons=# of electrons • Determine # of protons, neutrons, and electrons for any given isotope or ion. • Know the atomic mass reported on the Periodic Table is the weighted average of all naturally occurring isotopes for that element. • Use the Periodic Table to identify the most abundant isotope of any element given its naturally occurring isotopes. • Use the Periodic Table to identify those elements whose naturally occurring isotopes are all radioactive and unstable. • Determine the number of atoms of an element in a compound given the chemical formula.CHEM 139 Final Exam Study Guide page 3 of 9 Chapter 4 (Continued) The Periodic Table column = group, family row = period, series Representative Elements: A Group Elements Group IA: alkali metals (except H) Group IIA: alkaline earth metals Group VIIA: halogens Group VIIIA: noble gases Transition Metals/Elements: B Group Elements Inner Transition Elements: - Elements in lanthanide and actinide series • Metals, nonmetals, and semimetals: - Know properties of metals and nonmetals - Location on Periodic Table and properties • Know which elements exist as solids, liquids, gases at room temperature (25˚C) • Know the names and symbols for all elements included in Ch. 4 notes, p. 11, Ti (titanium), and Sr (strontium). Spelling counts! Chapter 11 Wavelength (λ) is inversely related to frequency (ν) and energy (E): – As λ↑ → ν↓, Ε↓ or As λ↓ → ν↑, Ε↑ Electromagnetic Spectrum: – continuum of radiant energy – gamma (γ) rays to radio waves Know the people and ideas associated with the Classical Model of Matter – Dalton, Thomson, Rutherford, Maxwell Planck and Quantum Theory – proposed energy is absorbed and emitted as bundles = quanta – single bundle of energy = quantum Einstein and the Photoelectric Effect – Experimental evidence for light existing as particles = photons Bohr Model of the Atom – Electrons move in quantized orbits called “energy levels” around nucleus – Know if energy is gained or lost for e-s moving from one energy level to another. – ground state: e-s in lowest E level(s) – excited state: e-s in higher E level(s) before