1. Naming Chemical Compounds

2. Naming Ions What are ions? Atom that has gained or lost electrons Cations? Atom that has lost electrons. (+ charge) Anions? Atom that has gained electrons. (- charge) Cations and Anions are named differently.

3. Naming Cations Which elements on the periodic table are cations? (have a positive charge?) Elements on the left side Which Groups? 1A, 2A, 3A For all Cations (Elements in groups 1A, 2A, 3A) you add the work ion after the elemental name.

4. Naming Cation examples Na 1+ Sodium ion Al 3+ Aluminum ion Ca 2+ Calcium ion

5. Naming Anions Which elements on the periodic table are anions? (have a negative charge?) Elements on the right side Which Groups? 5A, 6A, 7A For all anions you add the suffix (ide) at the end of the root of each elemental name. Flourine (F -1 ) is called Flouride

6. Naming Anions Example Chlorine (Cl 1- ) Chloride Sulfur (S 2- ) Sulfide Nitrogen (N 3- ) Nitride

7. Naming Transition Metals Where are the Transition metals located? Many Transition metals for more than one ion Fe 2+, Fe 3+, Cu +, Cu 2+ Thus, when naming transition metals signify the number of electrons gained or lost after the elements name. Example: Fe 2+ and Fe 3+ becomes… Iron (II) ion and Iron (III) ion

8. Naming Transition Metals Examples Tin (Sn 2+ ) Tin (II) ion Tin (Sn 4+ ) Tin (IIII) ion Manganese (Mn 2+ ) Manganese (II) ion Manganese (Mn 3+ ) Manganese (III) ion

9. Monatomic Ions Monatomic Ions consist of a single atom with a positive or negative charge. All ions we have studied up to this point have been Monatomic Ions Now we will begin looking at Polyatomic ions.

10. Polyatomic Ions If monatomic ions are single atoms. Polyatomic ions are….? Polyatomic ions are composed of more than one atom.

11. Examples of Polyatomic Ions Examples: Sulfur and Oxygen combine to form… SO 4 2- Carbon, Hydrogen, and Oxygen form… C 2 H 3 O 2 1- These polyatomic ions are tightly connected and behave like 1 element. Tough to separate them.

12. Naming Polyatomic Ions Most polyatomic ions end in ite or ate. Luckily we do not need to memorize rules for these. You will be given a list of popular polyatomic and monatomic ions that will guide you for the rest of the year.

13. Practice Problems Answer the questions in your lab notebook Monatomic Ion Naming practice: For each question indicate the name of the ion and whether each is a cation or anion. 1.Sodium7.Chlorine 2.Calcium8.Sulfur 3.Bromine9.Oxygen 4.Potassium10.Lithium 5.Iodine11.Beryllium

14. Binary Ionic Compounds Compounds? Compounds are substances made up of 2 or more elements A Binary Ionic Compound is a substance made up of 2 ionic elements. Examples: NaCl Li 2 O BaS

15. Naming Binary Ionic Compounds To name any Binary Ionic Compound you place the name of the cation first, followed by the anion. NaCl Sodium Chloride Li 2 O Lithium Oxide BaS Barium Sulfide CuO Coppper (II) Oxide Fe 2 O 3 Iron (III) Oxide CaS Calcium Sulfide

16. Writing Binary Ionic Compound Formulas Copper (I) Sulfide, What is its chemical formula? Use The Criss Cross Method Copper (I) = Cu 1+ Sulfide = Cation Written first: Anion Second Cu 1+ S 2- Criss Cross the charges to the other element Cu 1+ S 2- Becomes Cu 2 S Examples on Board…

17. Naming Binary Compounds With Polyatomic Ions The same as before… State the name of the cation first and then the name of the anion. LiCN Lithium Cyanide NaClO Sodium Hypochlorite AgNO 3 Silver Nitrate

18. Writing Formulas for Polyatomic Ions It is the exact same as before! Criss Cross Method! Cation is written first and Anion second Calcium = Ca 2+ Acetate = C 2 H 3 O 2 1- Ca 2+ C 2 H 3 O 2 1- Then criss cross the charges Ca 1 C 2 H 3 O 22 Add parentheses. 2 acetate ions not 22 Oxygens Ca(C 2 H 3 O 2 ) 2 Examples on the Board

19. Practice!!!! Either name the compound or write the chemical formula for the compound. 1. CaCl 2 2. Sodium Hydroxide 3. MgSO 4 4. Magnesium Sulfate 5. Cr(NO 3 ) 3 6. Cesium Sulfide 7. NaCl 8. Sodium Iodide 9. NaClO 4 10. Magnesium Hydroxide

20. Quiz Write the name or formula for the following compounds. 1. Cesium Sulfide 2. NaCl 3. Sodium Iodide 4. NaClO 4 5. Magnesium Hydroxide 6. Magnesium Sulfate Write the name for the following ions. 1. Sodium 2. Chlorine 3. Calcium 4. Sulfur

21. Binary Molecular Compounds Binary Molecular Compounds are compounds made up of 2 or more nonmetals. What type of bond is typically bonded between 2 nonmetals? Covalent bond.

22. Naming Binary Molecular Compounds Use the prefixes stated below. 1 atom = mono- 2 atom = Di- 3 atom = Tri- 4 atom = Tetra- 5 atom = Penta- 6 atom = Hexa- 7 atom = Hepta- 8 atom = Octa- 9 atom = Nona- 10 atom = Deca-

23. Naming Binary Molecular Compounds N 2 O 2 Nitrogens 1 Oxygen Prefix for 2 and 1? Diand Mono Put the di in front of Nitrogen Dinitrogen Put the mono in front of oxygen and add ide Monoxide Put the 2 together. Dinitrogen Monoxide

24. Naming Binary Molecular Compounds P 2 O 3 2 Phosphorous 3 Oxygen Prefix for 2 and ? Diand Tri Put the di in front of Phosphorous Diphosphorous Put the tri in front of oxygen and add ide Trioxide Put the 2 together. Diphosphorous Trioxide

25. Naming Binary Molecular Compounds CO Monocarbon Monoxide? NOPE!!! When there is one atom of the first element you drop the mono Carbon Monoxide CO 2 Carbon Dioxide

26. Writing formulas for Binary Molecular Compounds To write formulas for these compounds you use the prefix in the name to tell you the element’s subscript. Carbon Tetrabromide 1 carbon 4 bromines. Use them as subscripts. CBr 4 Chlorine Triflouride 1 Chlorine and 3 Flourides ClF 3

27. Practice 1. NI 3 2. BCl 3 3. N 2 O 3 4. Cl 2 O 7 5. Silicon Tetraflouride 6. Carbon Tetrachloride 7. Iodine Dioxide

28. Naming Acids Name of the anion ends in ide the acid names begins with hydro and then ends in ic. Followed by the work acid. HCl – Hydrogen Chloride Hydrochloric acid Name of the anion ends in ite, change the ite to ous followed by the word acid. H 2 SO 4 - Hydrogen Sulfite Sulfurous acid Name of the anion ends in ate, change the ate to a ic followed by the word acid. HNO 3 – Hydrogen Nitrate Nitric acid

29. Naming Acids Naming common Acids Anion Ending ExampleAcid NameExample -ide Chloride, Cl - Hydro-(stem)-ic acidHydrochloric acid -ite Sulfite, SO 3 2- (stem)-ous acidSulfurous Acid -ate Nitrate, NO 3 - (stem)-icNitric Acid

30. Writing Formulas for Acids Use the reverse rules for writing formulas Hydrobromic Acid Hydro in front and ic at end. = anion ends in ide Must be Hydrogen and Bromide ions HBr Phosphourus Acid ous ending means = anions ends in ite Must be Hydrogen and Phosphite ions H 3 PO 4 Formic Acid Ic ending means = anion ends in ate Must be Hydrogen and Formate ions HCOOH

31. Names and Formulas for Bases Same as other ionic compounds Name of cation followed by name of anion NaOH Sodium Hydroxide Formulas use the Criss Cross Method Aluminum Hydroxide Al 3+ OH 1- Al(OH) 3

32. Practice In your lab notebook write the name of the acid or base. Or write the formula of the acid or Base. 1. HNO 2 2. HCN 3. HMnO 4 4. H 2 S 5. Carbonic Acid 6. Sulfurous Acid 7. Iron (III) Hydroxide 8. Strontium Hydroxide 9. LiOH 10. Mg(OH) 2 11. Pb(OH) 2