1. Use with one of the gas equations (Combined, Boyle’s, or Charles’s). When you start or end at STP refer to Table A for numerical values. Keep the units the same for pressure. Temperature is ALWAYS in Kelvin

2. Heat of Fusion – Melt/Freeze Heat of Vaporization – Evaporation/Condensation Specific Heat Capacity – S, L, G Heat of Vaporization requires more energy than Heat of Fusion which is why the line segment is always longer on a heating and cooling curve.

4. Don’t forget hydronium goes hand in hand with an ACID and hydroxide goes hand in hand with a BASE. Ionic compounds that have at least one Polyatomic Ion is considered to have BOTH Ionic and Covalent Bonds in them. M(+) with NM(-) M(+) with PI(-) PI(+) with NM(-) PI(+) with PI(-)

5. SOLUBLE: Most Soluble High concentration of dissolved ions INSOLUBLE: Least Soluble Low concentration of dissolved ions PRECIPITATE

6. All slopes that are directly related to temperature are SOLIDS, all slopes that are indirectly related to temperature are GASES. The graph is based on 100 grams (ml) of water. Saturated (concentrated) – On the line. SOLUTION EQUILIBRIUM Supersaturated (concentrated) – Above the line. Unsaturated (dilute) – Below the line. When they ask how much “settled out” or “precipates” they will give you a starting temperature and an end temperature. Find saturated for both and then subtract.

7. Boiling Point occurs when the vapor pressure of the liquids are equal to the Atmospheric Pressure (101.3 kPa). The higher the Atmospheric Pressure the higher the BP. The lower the Atmospheric Pressure the lower the BP. Intermolecular Forces are DIRECTLY related to BP. The higher the BP, the stronger the IMF, the lower the BP, the weaker the IMF!!!

8. ∆H = PE p – PE R ∆H (+) = Enodthermic ∆H (-) = Exothermic First 6 reactions on this table are examples of combustion in case you forget. ENDOTHERMIC EXOTHERMIC

9. Acids react with certain metals to produce H 2 (g). Only those metals found above H 2 on Table J will react. In REDOX, the more the reactive the metal, the more easily it’s oxidized (lose electrons). In a Voltaic Cell, the more reactive metal acts as the ANODE (lose electrons). In a Single Replacement Reaction, the element by itself MUST be more reactive that the element it replaces, or else the reaction won’t occur.

10. ELECTROLYTES!!!!!!!! Anytime they ask an electrolyte question, you are looking for either an acid, or a base, or an ionic salt!! Acids have H + or H 3 O + Bases have OH -

11. The first pH # and less correlate to the first color; the second pH # and greater correlate to the second color. Acids – less than 7 Bases – Greater than 7

12. All the isotopes on this list are UNSTABLE, which means they are RADIOACTIVE, and will SPONTANEOUSLY undergo NATURAL TRANSMUTATION. Remember that when you undergo Natural Transmutation the symbol of the element has to change according to what the new atomic number is.

13. MASS CHARGE Gamma Radiation has the greatest penetrating power. Alpha Particles have the weakest penetrating power

14. ALKANES – Saturated (single bonds) ALKENES – Unsaturated (double bonds) ALKYNES – Unsaturated (triple bonds) ISOMERS – has the same molecular formula, but different structural formula.

15. Some things to look for on condensed formula: Aldehydes – CHO Ketones – CO Organic Acids – COOH Ester – COO (Acid + Alcohol)

16. Elements defined by their Atomic Number (protons) Electron Configuration (2-8-18-32); the farther away electrons are the more energy; valence electrons. Mass Number = Protons + Neutrons Groups 1,2, 13-18 (same group, same # valence electrons) TRENDS – USE TABLE S!! Metals, Non-Metals, Metalloids, Noble Gases Solids, Liquids, Gases Oxidation Numbers

17. Don’t guess … use Table S. These are the ACCEPTED VALUES for the above. Electronegativity – attraction for electrons (the greater the difference, the more polar, the higher the BP, the stronger the IMF) Ionization Energy – energy needed to lose electrons

18. Use to convert grams to moles and moles to grams. May need to first calculate the GFM, or it will be provided to you. GFM = 1 mole = 6.02x10 23 = 22.4 L

19. Mass of the whole is the GFM. You may have to calculate, or it’s provided to you. For a HYDRATE question when they ask the % composition of water in the hydrate: % comp = Hydrate – Anhydrate Hydrate X 100

20. These are used to determine the concentration of a solution. The greater the Molarity or ppm, the more concentrated it is.

21. The end result of Titration is Neutralization: PLEASE DO NOT CONFUSE THIS WITH THE MOLARITY FORMULA!! If they give you data on an acid and a base it’s Titration. If the data is only on one substance then use the Molarity formula.