1. Physical Science Chpt. 12 & 16 Metals/NonMetals Family of Elements Chemical Naming Chemical Reactions Balancing Chemical Equations

2. Metals Good conductors of heat and electricity Shiny Hard solids Reflect light Malleable Ductile Ionic bonds/ lose electrons

3. Malleable/Ductile Malleable Hammered or rolled into sheets Ductile Hammered or rolled into thin wire

4. Alkali Metals Group 1 One electron in outer energy level Oxidation number is +1 Electron dot diagram (look at bulletin board) Highly reactive metals

6. Alkaline Earth Metals Group 2 Two electrons in outer energy level Oxidation number is +2 Electron dot diagram (see bulletin board)

8. Transition Elements Groups 3-12 Have varying electrons in outer energy level Have varying oxidation numbers Can have more than one oxidation number because of how outer energy levels are set up Transuranium elements have more than 92 protons

9. Transition Elements

10. Transition elements form compound with more than on oxidation state Compounds containing transition elements are normally highly colored Transition metals and compounds act as catalysts for a wide range of chemical reactions Form complex ions

11. Nonmetals Do NOT conduct heat or electricity Powders, liquids or gases Dull, brittle solids Not malleable or ductile Form ionic and covalent bonds Ionic gain an electron from a metal Covalent share electrons with other nonmetals

12. Hydrogen 90% of all atoms in the universe are hydrogen On earth mostly is contained in water Highly reactive One electron in outer energy level Nonmetal Covalent and ionic bonds +1 oxidation number (normally)

13. Diatomic Molecules N2N2 O2O2 H2H2 F2F2 Cl 2 Br 2 I2I2 Have two of the same element Combined together, occur like this naturally

14. Boron Group Group 13 Three outer energy level electrons Oxidation number +3 Aluminum in this family Semiconductors Conduct an electric current under certain conditions Electron dot diagram (see bulletin board)

16. Carbon Group Group 14 Four electrons in outer energy level +/- 4 oxidation number depending on what combining with Allotropes—different forms of the same element having different molecular structures, phosphorus, silicon, carbon (diamond and graphite) and many other elements

17. Carbon Group Cont. Silicon Second most abundant in Earth’s crust, silicon dioxide Electron dot diagram (see bulletin board)

19. Nitrogen Group Group 15 Five electrons in outer energy level Oxidation number -3 Share electrons— covalent bonds 80% of air is nitrogen Nitrogen forms important nitrates, ammonia, and fertilizers Phosphorus—water softeners and fertilizer Electron dot diagram (see bulletin board)

21. Oxygen Group Group 16 Six electrons in outer energy level Oxidation number -2 Oxygen Most abundant element in Earth’s crust Oxygen 20% in air Animals need for respiration Ozone O 3 Protect Earth from UV rays Electron dot diagram (see bulletin board)

23. Halogens Group 17 Seven electrons in outer energy level Oxidation numbers -1 Gain electrons from metals (ionic bonds) Halogen means salt former Fluorine Most chemically active of all elements Have many uses Electron dot diagram (see bulletin board)

25. Noble Gases Group 18 Eight electrons in outer energy level Full outer energy level Not reactive stable Neon signs Oxidation number 0 neutral Electron dot diagram (see bulletin board)

27. Chemical Naming Metals go first Change ending to -ide on nonmetals Examples Oxide chloride Don’t forget polyatomic ions page 318 Examples Iron oxide Potassium chloride Magnesium hydroxide

28. Chemical Reactions Reactants on left side Products on right side One or more substances are changed into new substances Reactants about to react Products are the new substances produced

29. Law of Conservation of Mass Matter can neither be created nor destroyed

30. Chemical Reaction Table 16-1 page 444 has symbols used in reactions Coefficients Represent the number of units of each substances taking part in a reaction Written before the compound

31. Balanced Chemical Equations 1. Must write out the compounds and elements using the correct formulas and symbols 2. Use -----  between reactants and products 3. Write out oxidation numbers, criss cross charges to get correct formula for compound 4. Place coefficients in correct places to balance the elements on each side of the equation Check the equation for atom balance

32. Chemical Equations Table 16-7 give a different way for balancing than what I will show you in class

33. Types of Chemical Reactions Synthesis Two or more substances combine to form another substance A + B --  AB Decomposition One substance breaks down, or decomposes, into two or more simpler substances AB -  A + B

34. Types of Chemical Reactions Single Displacement One element replaces another in a compound A + BC -  AC + B Metals switch D + BC  BD + C Nonmetals switch Double Displacement Takes place if a precipitate, water or gas forms When two ionic compounds in a solution combine AB + CD  AD + CB

35. Precipitate An insoluble compound formed during a double displacement reaction

36. Exothermic Reaction Some form of energy is given off during a chemical reaction

37. Endothermic Reaction Energy must be provided for the reaction to take place

38. Catalyst A substance that speeds up a chemical reaction without itself being permanently changed

39. Inhibitor A substance that slows or prohibits a chemical reaction