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2. The valence electrons in an atom have HIGH POTENTIAL ENERGY By bonding with other atoms, potential energy is decreased creating stable compounds.

3. Symbols of atoms with dots to represent the valence-shell electrons. (The valence- are the e- directly involved in bonding). Ar Mg C

4. The Noble Gases do not react with other elements because they are already STABLE. The outer most “s” and “p” orbitals are completely filled with 8 electrons, satisfying the octet rule. Ne

5. Elements combine with each other to achieve noble gas electron configurations or (8 outer e-) **The exceptions to the octet rule are Hydrogen and Helium (they only need 2)

6. The forming of chemical compounds results in chemical change. Compounds are made up of chemically united elements Compounds have completely different characteristics than its component elements Compounds are NEUTRAL

7. 2H 2 O = H 2 O = HHO H 2 O HHO Subscript = # of atoms Coefficient = # of molecules

8. N: 1 H: 5 O: 1

10. The Gaining and Losing of Electrons to form IONS. (An ion is an atom with a charge.)

11. sharing of electrons

12. Soluble in water Do not transmit electric current Brittle High melting and boiling points

13. Ionization Energy: the amount of energy needed to remove an e- from an atom. Nonmetals have high ionization energy because they are closer to satisfying the octet rule! Metals have a low ionization energy

14. the higher the electronegativity the greater the ability to pull electron to itself The nature of a bond is determined by differences in electronegativity. The GREATER the electronegativity difference, the MORE ionic the bonding.

15. Ionic compounds result when metals react with nonmetals Metals lose electrons to achieve a stable outer energy level Positive ions form when electrons are given away Group 1 metals  ion 1+ Group 2 metals  ion 2+ Group 13 metals  ion 3+

16. 1. Write the symbol for the cation (+) followed by the symbol for the anion (-). 2. Put any polyatomic ions (see green boxes) in parenthesis 3. Write the oxidation numbers above the appropriate ions 4. Use the criss-cross method to deterimine # of atoms (do not criss-cross ones) 5. Make sure the sum of all ox# is ZERO. 6. Reduce

17. Na  – e   Na + Sodium Atom Sodium Ion 11 p+ 11 e- 0 11 p+ 10 e- 1+ 

18. + e   1- Fluoride Atom Fluoride Ion 17 p+ 17 e- 0 17 p+ 18e- 1-

19. Na  +  Na 1+1-

20. YOUR TURN … Using dot diagrams, draw the Lewis structures that result when the following elements form ionic bonds: A.Potassium + chlorine B.Magnesium + fluorine

21. Potassium + Chlorine Magnesium + Fluorine K Cl K + FMg + F F

22. Oxidation: the process of losing electrons ▪ Creates an ion with a + charge ▪ Creates cations Reduction: the process of gaining electrons ▪ Creates an ion with a – charge ▪ Creates anions

23. 1. Write the name of the cation (+) 2. Write the name of the anion (-) with an ide suffix NaCl Sodium and Chlorine Sodium Chloride

24. The oxidation number is not always the same, it varies. The variable oxidation states are represented with a roman numeral in parentheses and are located in groups 3-12 on the periodic chart. Copper Copper (I) = Cu+ Copper (II) = Cu2+

25.  Write the symbol for the cation followed by the symbol for the anion.  Write the oxidation numbers above the appropriate ions.  Criss-Cross Copper(III) Oxide: CuO Cu 2 O 3 Copper(I) Oxide: CuO Cu 2 O 3+2- 1+ 2-

26. SO 4 Sulfate2- C 2 H 3 0 2 Acetate1- NO 3 Nitrate1- NO 2 Nitrite1- NH 4 Ammonium1+ HCO 3 Bicarbonate1- CO 3 Carbonate2- OHHydroxide1- ClO 3 Chlorate1- PO 4 Phosphate3-

27. 1. Write the name of the cation (+) 2. Write the name of the anion (-) 3. If either is a polyatomic ion write the name of the polyatomic ion (you don’t need to change any suffixes) Na(OH) Sodium Hydroxide

28.  Write the symbol for the cation followed by the symbol for the anion.  Put all polyatomic ions in parentheses!!  Write the oxidation numbers above the appropriate ions.  Criss-Cross Calcium Phosphate: Ca(PO 4 ) Ca 3 (PO 4 ) 2 Ammonium Phosphate: (NH 4 )(PO 4 ) (NH 4 ) 3 (PO 4 ) 2+ 3 - 1+ 3 -

29. Cu(OH) Copper (I) Hydroxide Ni 2 O 3 Nickel (III) Oxide 1-= 01+ 2- 6-=03+

30. sharing of electrons

31.  Between nonmetallic elements of similar electronegativity.  Formed by sharing electron pairs  Stable non-ionizing particles, they are not conductors at any state  Examples; O 2, CO 2, C 2 H 6, H 2 O, SiC

32. Water is a polar molecule because oxygen is more electronegative than hydrogen, and therefore electrons are pulled closer to oxygen.

33.  A polar molecule has a (+) and a (-) end.  A nonpolar molecule does not have charged ends.

34. Metal + Nonmetal --> ionic compound (usually) Metal + Polyatomic ion —> ionic compound (usually) Nonmetal + Nonmetal —> covalent compound (usually) Hydrogen + Nonmetal —> covalent compound (usually)

35.  The chemical symbol for the atom is surrounded by a number of dots corresponding to the number of valence electrons

36. 1. Write the name of the cation (+) with appropriate prefix (do NOT use mono for the cation) 2. Write the name of the anion (-) with the appropriate prefix CO 2 Carbon Dioxide

37. 1:mono 2:di 3:tri 4:tetra 5:penta 6:hexa

38.  Formula weight is the sum of the atomic masses.  Example- CO 2  Mass, C + O + O 12.011 + 15.994 + 15.994 43.999