Whole Year Review in 34 minutes. Seat belts on, copy quickly.

1. Whole Year Review in 34 minutes. Seat belts on, copy quickly. All of this material is in your BASICS handouts, which are all online (in color). Breeze through everything, good luck tomorrow. 20 multiple choice questions, some naming/formulas, dimensional analysis, vocabulary. Balance your need for success with your legitimate need for sleep. Too late means too tired to do well. Relax, all my students for the previous 10 years have been in your seats (so to speak). They are all having nice lives now. You will too.

2. Measurement Density formula on reference table SF count, review the significance of significant figures Qualitative (I am tall) vs. quantitative measures (I am 68.5 inches tall) Precise vs. accurate measures Percent error always gets a sign, formula on reference table Converting Kelvin to Centigrade, formula on reference table Density is a constant, all listed on table S Melting point = freezing point boiling point = condensation point Melt/freeze, vaporize/condense, sublimation/deposition Melting points and boiling points on reference tables. Note solids, liquids, and gases

3. Dimensional Analysis or unit conversion math lets you convert from unit to unit, by multiplying by conversion factors which all equal 1 (with UNITS) but not without! Each equality makes two different conversion factors, but you must use units. Units MUST CANCEL. Always start at the beginning, over 1. Use the UNITS you NEED, skip the ones you don’t. There are many units on the reference tables, use any units you need to make changes. Sometimes things take 2 or 3 or even 4 steps to convert. Using units YOU don’t know, or make believe units, is easy as pie. Start at the beginning, and make sure your units cancel out until your last unit is the ONE YOU WANT in the answer. DO NOT CHEAT with units, they either work or they don’t. Write big enough to see what you write, write units ALWAYS. 1 mL = 1 cm3 in volume. NO SUCH THING as mL3 Volume is 3D, not cm2 or cm or whatever

4. Lower density will always float on higher density (oil floats on vinegar) Do not say IT, say what you mean and mean what you say. READ ALL CHOICES in multiple choice problems. Do the math, know the answer, then FIND IT in the choices. If you have time, figure out why the other 3 are wrong choices. Matter has mass and takes up space (has volume) Pure stuff includes all elements and all compounds. These are homogeneous. Mixed stuff includes all mixtures. It’s homogenous sometimes (solutions) but not always. Sometimes it’s heterogeneous (mish-mash tossed together). Mixtures can be separated by taking advantage of differences in physical properties such as: Particle size, magnetic attraction, melting point, freezing point, boiling point, density, using these processes: filtration, chromatography, magnets, distillation, etc. Compounds have formulas and your compound is identical to mine. Mixtures are just roughly put together.

5. Matter comes in 3 phases Solids – which hold their shapes, particles stuck together, have low compressibility, and are usually the most dense phase. Liquids – which take the shape of the bottom of their container, particles sticky but not stuck together, have low compressibility, are still pretty dense. Gases – which fill any size container they are put into (pressure drops accordingly) particles not touching, flying fast in straight lines, very compressible, very low density. Particle diagrams are cartoons that “show” matter in various phase, or show mixtures, compounds, elements, diatomic elements, etc. The law of conservation of matter: Matter cannot be created or destroyed in any chemical reaction or in any physical change (phase change). Law of conservation of energy: energy cannot be created or destroyed in any chemical reaction or in any physical change (phase change). TOPIC-B are INDICATORS that a chemical reaction has taken place, but are not RULES. Exceptions exist. Reactants chemically combine into products In both physical and chemical changes, particles are rearranged, but in chemical reactions there is NEW stuff formed, with new properties.

6. Democritus, Dalton, Thompson, Rutherford, Bohr, and the Wave Mechanical or modern models of the atom. Atomos, atomic theory (look that up), electrons in plum pudding – cathode ray tube, gold foil with positive nucleus, flying electrons, electron in ORBITS or energy levels, spectra, now in ORBITALS, statistical model or cloud of probability to find electrons. 2-8-8 or 18. All noble gases have only full electron orbitals. All atoms are neutral, but metals will lose enough electrons to gain noble gas configurations (isoelectric), becoming + cations. Nonmetals gain enough electrons to do the same, becoming – anions. Metals and nonmetals from the periodic table combine to form neutral ionic compounds. The ion charges criss cross to determine ratios. Transitional metals sometimes make multiple + cations and we use roman numerals to keep track of them I II III IV V VI VII VIII Table E has all the polyatomic ions on it, which work the same as monoatomic ones, but sometimes with ( ) if there are multiple polyatomic ions in a compound.

7. 1st name rules, 2nd name rules. -ide endings. Molecular compounds form with only nonmetals, we use selected oxidation states to figure out what is possible and what’s not. Prefixes used in names. Mono, di, tri, tetra, penta, hexa, hepta, oct, non, deca Isotopes are chemically identical atoms of the same name, but have different numbers of neutrons (and therefore a different mass. Mass of an atom = mass of protons + mass of neutrons. Each is 1 amu in high school. Electrons have no mass in high school. Decimals come about from the very carefully measured proportions found in nature. The mass rounded to the nearest whole number gives you the mass of the most common isotope (almost always). (mass in amu)(proportion found in nature as a decimal) = (mass of other isotope in amu)(it’s proportion as a decimal) = (mass of another isotope in amu)(it’s proportion) = Sum these up to get the “weighted average atomic mass” on the periodic table

8. Electrons on periodic table configurations are in ground state (lowest energy) or normal places. Add energy of ANY KIND, say heat, or electricity, etc. And these electrons take the exact amount each needs to get “EXCITED” and jump up to a higher energy orbital or higher energy level. This is unstable, when the electron returns to ground state it must first emit this gained energy AS VISIBLE LIGHT called spectra. Each atom/substance has unique number of electrons so each needs unique energy to get excited. Law of conservation of energy means that each releases this exact, unique amount of energy that can be measured. Neon (or other gases) in lamps emits a particular color we see with our eyes. This is actually the MIXTURE of the colors our eyes blend into one color. The refractive lenses can break this mixture into the SPECTRA lines, which are unique and can be measured quantitatively.

10. 1 – alkali metals 2 – alkaline earth metals 3-12+ - transitional metals 17 - halogens 18 - noble gases Inner transitional metals are all squeezed into group 3, under Y. 7 metalloids – elements that ARE metals but have some nonmetallic properties, or ARE nonmetals, but with some metallic properies include: B, Si, Ge, As, Sb, Te, and At They touch the staircase on the table, so do Al and Po, but they are the (dog food) exceptions to this rule. Metals to the left of the stairs (except H) and nonmetals to the right. Metalloids are a dual name, not separate from metals/nonmetals. Acids and bases on on Tables K and L (just in case). On the next page are metal, nonmetal, and metalloid properties (memorize more or less)

12. You’ve seen this all before, you’ll do as well as you should. If you do well, good. If you don’t – oh well. You will all go to college, no matter what. Study, think, and stay ahead of the curve. I am truly impressed this year, as a group I’d bet on you all big time. Peace, love, and chemistry. See you tomorrow.