Names and Formulas Ionic Compounds Binary Main Group M & NM Using Polyatomic ions

1. Names and Formulas • Ionic Compounds • Binary Main Group M & NM • Using Polyatomic ions • Transition metals with variable charges • Covalent Compounds • Names & Formulas

2. NC Essential Standards • 1.2: Understand the bonding that occurs in simple compounds in terms of bond type, strength and properties. • 1.2.1: compare the relative strength of ionic, covalent, and metallic bonds • 1.2.2: Infer the type of bond and its chemical formula formed between atoms • 1.2.3: Compare inter- and intra- particle forces. • 1.2.4: Interpret the name and formula of compounds using the IUPAC convention • 1.2.5: Compare the properties of ionic, covalent, metallic, and network compounds.

3. Language of chemistry: Standardize system to represent compounds

5. Binary Ionic Compound with Representative Metals • Example: Chlorine and magnesium • Rules for formula • Metal (cation)1st NM (anion) 2nd • Change number of each until charges = 0 • Subscripts tell the number of atoms/moles • Rules for names: • Metal 1st – metal’s element name • NM 2nd – change ending to “-ide” • No prefixes

6. Ionic compounds with polyatomic ions • Rules for formulas • Cation 1st Anion 2nd • Use parentheses around the polyatomic ion • Change number of each ion until charges = 0 • Check polyatomic ion: name, formula & charge • Rules for Names • Cation 1st Anion 2nd • Be careful about the ending (“-ate”, etc.) • No prefixes

7. Using polyatomic ions: Sodium + nitrateAmmonium + nitride Formula Name:

8. Common Polyatomic Ions

9. Memorizing polyatomic ions • Nick the Camel ate a clam for supper in Phoenix • http://www.youtube.com/watch?v=TZgv21FmEzk&list=PLs9HjZz1--dAB_gUIJJOhAu1Rrvaa56J6

10. Criss – Cross method • Use the charges (oxidation numbers) to help determine the number of atoms (moles) Al⁺³(CO₃⁻²) Check if it the smallest (simplest) ratio

11. Writing Formulas (criss –cross method)selected examples from worksheet

12. Ionic Compounds with Transition Metals • The transition metals are elements in Groups _____ to _______. • + post transition metals: under the staircase. • Transition metals can have more than one charge. • Use Roman numerals after the name. • Roman numbers: • I = II = III = IV = V=

14. Transition metals • Examples Iron II oxide Iron III oxide Write the formulas for: Copper I oxide Cobalt III chloride Tin IV sulfide Note: Check for the smallest (simplest) ratio

15. Writing Formulas (criss –cross method)selected examples from worksheet

16. Formula Writing Practice – selected examples

17. Language of chemistry: Standardize system to represent compounds

19. Inorganic Covalent Compounds Names & Formulas • Binary • Diatomic • Acids Note: Organic compounds different naming system

21. Inorganic covalent compounds

22. Earth’s atmosphere

23. Names of Binary Molecules • First-element name • 2nd – end in “ide” • Use prefixes -Always with 2nd element -With 1st element except mono- Element with lowest EN goes first On the Periodic Table – across /down

24. Practice: • Complete the table in your notes. • Write the names • Write the formula

26. Acids • Acids are molecules that are in aqueous solution (_________ in __________) and produce hydrogen ions (H¹⁺) • Typically start with H • Almost act as an ionic compound Electronegativity Difference:

27. Acids: H + Halogen • Hydro + Halogen (ic) + Acid • HBr • Hydrobromic acid

28. Oxyacids: common acids • Contains oxygen (in a polyatomic ion) • Note the endings of the anion & the acid name • H + nitrate = Nitric Acid • H + sulfate = • H + phosphate = • H + acetate =

29. 7 Diatomic Molecules • Heck No Halogens • Named with the element name

30. Common Names for 3 Molecules Molecular name and formula: common name • Dihydrogen monoxide = • Carbon tetrahydride = • Nitrogen trihydride =

31. Methane: CH₄

32. Ammonia: NH₃

33. Water: H₂0