1. Writing Formulas and Naming Compounds Chapter 7 Take a bag of “ions” make as many combinations as you can. Write the names and formulas. In your notebook, write a few of these, and summarize what you learned today. 3+ 3- Homework 1: Outline Chapter 7 Homework 2: names and symbols of first 30 elements HW 3: 1-6 page 171, 2 Honors #23,24 page 182 also

2. Lets picture what happens Na + + Cl - are attracted to each other. Na + and O 2- are attracted to each other. Na + Cl - O 2- Na + NaCl Na 2 O

3. Your turn: Use the following ions to make as many compounds as you can. You may use page 169 of your text book. potassium magnesium Gallium Lithium chloride oxide hydroxide phosphide phosphate Cl 1- O 2- (OH) 1- P 3- PO 4 3- Li 3 PGaPMg 3 P 2 K3PK3PP 3- Ga(OH) 3 Mg(OH) 2 KOH(OH) 1- Li 2 OGa 2 O 3 O 2- KClCl 1- Li 1+ Ga 3+ Mg 2+ K+K+ MgCl 2 GaCl 3 LiCl K 2 OMgO LiOH

4. K+Mg 2+ Ga 3+ Li + Cl - O 2- OH - P 3- Potassium chloride Potassium oxide Potassium hydroxide Potassium phosphide Magnesium chloride Magnesium oxide Magnesium hydroxide Magnesium phosphide gallium phosphide

5. Rubric for notebook turn in: Due Dates: M 4 th T 5 th W 8 th Th 9 F 11 th Name: Period Points A B C Fassignmentmultiplier extra credit1 10 8 7 1HW 1 outline C 71.5 10 8 7 1HW 2 symbols and names1 10 8 7 1HW 3 (1-6) (23,24 H)1 10 8 7 1HW 4 25,261 10 8 7 1HW 5 8,9, 271 10 8 7 1 what I learned (writing formulas)1 10 8 7 1class notes1 5 points extra if turned in on time.

6. Oxidation number The charge on a monatomic ion is called the oxidation number. An ion with more than one atom, has a different oxidation number on each atom, so the sum of the oxidation numbers equals the charge of the ion. Table 7.3 lists some common oxidation numbers.

7. Reading Isotopes S 32 16 2- Mass number Charge or oxidation number atomic number = number of protons

8. Reading Isotopes F 19 9 1- Mass number Charge or oxidation number atomic number = number of protons

9. What is the oxidation numbers of sulfur in this compound? CaSO 4 2+ 4 of 2- = -8 ? 0 = 2 - 8 + ? ? = 6

10. What is the oxidation numbers of phosphorous in this compound? Na 3 PO 4 3 sets of 1+ 4 of 2- = -8 ? 0 = 3 - 8 + ? ? = 5

11. HW 3: 1-6 starting page 171 Write the formula for the following compounds: –calcium chloride –sodium cyanide –magnesium oxide Ca Cl 2 NaCN Mg MAKE SURE THE CHARGES ARE BALANCED! O

12. HW 3: 1-6 starting page 171 Write the formula for the following compounds: –silver and fluorine –nickel (II) and sulfur –chromium (III) and bromine Ag F NiS Cr MAKE SURE THE CHARGES ARE BALANCED! Br 3

13. 4. Write formulas for the following. barium sulfate barium sulfide magnesium phosphate strontium bromide chromium (III) acetate Ba 2+ SO 4 2- S 2- Mg 2+ PO 4 3- Sr 2+ Br 1- Cr 3+ C 2 H 3 O 2 1- BaSO 4 BaS Mg 3 (PO 4 ) 2 …….

14. mass number = number of protons + number of neutrons atomic number = number of protons # neutrons = mass # - atomic # # electrons = # protons Explain lead-207’s parts Pb 207 82 mass number atomic number

15. Naming Binary inorganic compounds. Al 2 S 3 Aluminum Al 3+ Sulfide S 2- K3PK3P Potassium K + Phosphide P 3- The charges not needed for naming most compounds The charges are only needed for writing chemical formulas.

16. Naming Binary inorganic compounds containing transition metals. Cr 2 S 3 chromium (III) Cr 3+ Sulfide S 2- Cu 3 P copper (I) Cu + Phosphide P 3- The charges ARE needed for naming these compounds The charges are also needed for writing chemical formulas.

17. To name covalent compounds Covalent compounds are composed of two or more nonmetals which share electrons. (Some metalloids are covalently bonded as well). USE PREFIXES mono = 1 penta = 5 di = 2 hexa = 6 tri = 3 hepta = 7 tetra = 4 octa = 8

18. prefix if not mono-name of less electronegative atom, prefix of second atom– ending ide Naming covalent compounds CO 2 CO P 2 O 5 mono = 1 penta = 5 di = 2 hexa = 6 tri = 3 hepta = 7 tetra = 4 octa = 8 carbon di ox ide carbon mon ox ide di phosphorous pent ox ide Try SF 6 sulfur hexafluoride

19. Naming Organic Compounds Organic compounds have one or more carbons, surrounded with hydrogens. They may have double or triple bonds, and may include oxygen, or other atoms. They are named by counting the “carbon backbone” and applying a prefix “Functional Groups” provide the rest of the name. meth = 1 eth = 2 prop = 3 but = 4 pent = 5 hex = 6 hept = 7 oct = 8 non = 9 …

20. Naming Organic Compounds Butane = 4 carbons CH 3 CH 2 CH 2 CH 3 Heptane = 7 carbons CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 CH 3 Octane = 8 carbons CH 3 CH 2 CH 2 CH 2 CH 2 CH 2 CH 2 CH 3 meth = 1 eth = 2 prop = 3 but = 4 pent = 5 hex = 6 hept = 7 oct = 8 non = 9 …