Ionic Compounds Containing Multivalent Ions

1. Ionic Compounds Containing Multivalent Ions Learning Goal: Students will name and determine the formula of multivalent compounds

2. Ionic Compounds Containing Transition Metals (Multivalent Compounds) • The transition metals are located in groups 3-12 of the periodic table. • The charge on transition metal ions are not easily determined by their location on the periodic table – for reasons you will learn about in Grade 12 Chemistry. • Also, many transition metals have more than one charge (known as an oxidation state).

3. Where are the transition metals?

4. Eight Important Transition Metals Highlight these on the periodic table I gave you in class. The possible charges are listed in the upper left hand corner for any multivalent metals.

5. Naming Multivalent Ions • When naming any ion that has more than one ionic charge, you MUST include a Roman numeral in brackets following the name of the ion. • The Roman numeral is equal to the charge on the ion. Examples: • Cu2+ = copper (II) ion • Sn4+ = tin (IV) ion

6. Naming Multivalent Ionic Compounds • When you name an ionic compound that contains a transition metal that is multivalent YOU MUST INCLUDE THE ROMAN NUMERAL. • CuF2is NOT named copper fluoride! • Why NOT? • Naming the compound copper fluoride does not tell us whether or not the compound contains a copper (I) or copper (II) ion. • Solution: Determine the charge on the anion first! Then determine the charge the cation must be so that the overall charge of the compound is ZERO. • We know that a fluoride ion always has a charge of 1-. • There are 2 fluoride ions in CuF2 this would result in a net charge of 2- • This means that the copper had to be 2+. • Therefore the name of the compound is: copper (II) fluoride

7. Learning Check: Whiteboards • Name the following compounds: • SnI2 • PbF4 • CuS • CaBr2 • Mn(NO3)2 • CoPO4

8. Determining the Formula of Multivalent Compounds • Write the symbol for each element in the compound. • The roman numeral will tell you the charge on the metal cation. • Determine the charge on the non-metal or polyatomic anion. • Determine how many of each you will need so that the overall charge is zero.

9. Determining the Formula for Multivalent Compounds Watch out of “ide” vs. “ate” and “ite” endings!!!! “-ide” = simple binary ionic Any other ending = polyatomic • Example: iron (II) bromide Fe2+ Br1- Br1- The chemical formula is FeBr2 cobalt (III) nitrate Co3+ NO31- NO31- NO31- The chemical formula is Co(NO3)3

10. Learning Check - Whiteboards Determine the chemical formula for each of the following: • mercury (I) oxide • tin (II) nitride • manganese (IV) phosphate • chromium (III) sulfite

12. Activity - Cubing

13. Covalent Compounds Learning Goal: Students will… Define covalent compounds Draw lewis dot diagram and structural diagrams for covalent compounds Name and determine the formula of covalent compounds

14. Agenda • Warm-up: Multivalent Compounds • Classifying Compounds • Note: Molecular Compounds • Worksheet: Naming and Determining Formula of Molecular Compounds • Whiteboard Fun!

15. Open Sort: Classifying Compounds • Cut out the table of compounds provided • Think: How will you classify the compounds? • Pair: Find a partner. • Share: Describe to your partner how you classified the compounds. Is there any compounds that look new to you?

16. What is a Covalent Compound? • A compound formed when non-metal atoms SHARE electrons. • A covalent bond forms as a result of this sharing of electrons. • WHY SHARE ELECTRONS? • By sharing valence electrons, atoms fill their outermost energy level. • Since most atoms require eight valence electrons this is known as the OCTET rule.

17. Valence • Example: • An oxygen atom has 6 valence electrons. • It would need to share two electrons with other atoms to fill its outer valence. • We say that the VALENCE of oxygen is two, since oxygen forms two bonds.

18. Forming Covalent Compounds • If you had 2 oxygen atoms, they would each need to share 2 electrons to fill their valence shell. • Since two pairs of electrons are shared between them a double bond is formed. Lone Electron Pair (unshared) Shared Pair Electrons Lewis Dot Diagram for O2

19. Forming Covalent Compounds • By sharing two pairs of electrons, each oxygen atom has filled their outer shell. • We can also write the Lewis Dot Diagram to show which electrons are being shared. • A straight line equals one pair of shared electrons. 

20. Remember… • All of the following elements are found as diatomic molecules at room temperature: HOFBrINCl

21. Drawing Lewis Dot Diagrams of Covalent Compounds • Example: HCl • Draw the lewis dot diagram for each element. • Re-arrange the electrons so that each non-metal atom achieves stability by filling its outer valence orbit.

22. Try These… • Draw the Lewis Dot Diagram for the following covalent compounds. • HINT…the atom with the highest valence (can form the most bonds) goes in the middle) • CO2 • H2O • CF4

23. Naming Covalent Compounds • When naming covalent compounds you can distinguish them from ionic compounds because… • IONIC COMPOUNDS USUALLY BEGIN WITH A METAL! • COVALENT COMPOUNDS CONTAIN TWO NON-METALELEMENTS ONLY! • Use the following system for naming covalent compounds: (prefix if more than one) non-metal + (prefix always) non-metal “ide”

24. Examples: • CO • NH3 • N2O5 • IF5 carbon monoxide PREFIXES mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8 hexa- 9 deca- 10 nitrogen trihydride dinitrogenpentoxide Iodine pentafluoride

25. Determining the Formula of Covalent Compounds • Use the prefixes to determine the subscripts in the chemical formula… • chlorine dioxide • tetraphosphorustrisulfide • sulfur hexafluoride • Diphosphoruspentaoxide ClO2 P4S3 SF6 P2O5

27. HomeworkMolecular Compounds Worksheet & Putting It All Together