1. GO 4 Apply simplified chemical nomenclature in describing elements, compounds and chemical reactions 4-2Read and interpret chemical formulas for Ionic compounds

2. Guided Question How do we uses the information from the periodic table to write a chemical name and chemical formula for an Ionic Compound?

3. 3.1 Naming Compounds  When two or more elements bond together, they form one compound  A compound may be described by its proper name or its common name  A compound may also be described by its chemical formula H 2 O CO 2 NaCl  Chemical formulas indicate which elements (symbols) are in the compound and in what ratios (subscripted numbers)

4. IUPAC  IUPAC stands for the “International Union of Pure and Applied Chemistry” (1920) An international group that decides how to name compounds and approves the names of new elements This single method of naming compounds was universally adopted by all chemists/scientists We will be learning this strict set of rules to name compounds Until 1920, there was not a universal system of naming so there were many names for the same compound!

5. the compound is aqueous (dissolved in water) eg. C 12 H 22 0 11(aq) the compound is aqueous (dissolved in water) eg. C 12 H 22 0 11(aq)aq the compound is a gas eg. H 2 O (g) the compound is a gas eg. H 2 O (g)g the compound is a liquid eg. H 2 O (l) the compound is a liquid eg. H 2 O (l)l the compound is a solid eg. H 2 O (s) the compound is a solid eg. H 2 O (s)s DescriptionSymbol Physical states are shown with all chemical formulas! States are at the end, subscripted, in brackets.States are at the end, subscripted, in brackets.

6. Working with Compounds  Go to pg. 142 – Working with compounds  As a class we will go through the table

7. 3.2: Ionic Compounds  Ionic compounds are created with ionic bonds  Ionic bonds occur as a result of opposite charge attraction caused by one atom of a metal group giving away one or more of it’s electrons to a non-metal atom. This results in two IONS which are now attracted to each other. NaCl e-e- Na + Cl - e-e- becomes:

8. So what are IONS? Atoms that have lost or gained electrons are now IONS: Anions are negatively charged ions resulting from GAINING one or more electrons ex. Cl - is a chloride ion Cations are positively charged ions resulting from LOSING one or more electrons ex. Na + is a sodium ion Cations and anions are naturally attracted to one another (opposite charges attract) – this attraction is called an ionic bond!

10. What motivates an atom to become an ion?  The ultimate goal of each element is to have the same number of electrons as the NEAREST noble gas  An element can either gain an electron(s) or lose an electron(s) to reach this goal

11. Examples  Sodium - Draw a Bohr diagram of sodium  What would it like to do to have a full outer energy level (be like its nearest noble gas)?  Oxygen – Draw a Bohr diagram of oxygen  What would it like to do to have a full outer energy level (be like its nearest noble gas)?

12. 11 p+ 12 n° 2e – 8e – 1e – Na 8 p+ 8 n° 2e – 6e – O

13. IONS 11 p+ 12 n° 2e – 8e – Na + 8 p+ 8 n° 2e – 8e – O 2 -

15. Where can you find ion charges?  Besides drawing the Bohr diagram every time, you can look at the periodic table to find what ions you are working with?  B – shows what ions are possible for titanium  Does anyone know what A, C, D and E stand for?

16. Ionic Compounds - Writing the Formula  Binary ionic compounds are made up of one metal ion and one non-metal ion.  All ionic compounds have an overall (net) electrical charge of zero ex. sodium chloride Na + (sodium ion) and Cl - (chloride ion) form NaCl (s) (sodium chloride)  The positive charge on the sodium ion “cancels” out the negative charge on the chloride ion so the net electrical charge is zero (1 + + 1 - = 0)  NaCl (s) is called the chemical formula

17. Ex.2 Chemical Name: calcium chloride calcium ion has a charge of 2 + chloride ion has a charge of 1 - calcium ion (Ca 2+ ) and 2 chloride ions 2(Cl - ) ( +2) + 2 (-1) = 0 Chemical Formula: CaCl 2(s) To get a net electrical charge of zero we will need two chloride ions because each chloride ion has only 1 negative charge and 1 calcium ion has a charge of positive 2

18. Ex.3 Chemical Name: aluminum chloride aluminum ion has a charge of 3 + chloride ion has a charge of 1 - aluminum ion (Al 3+ ) and 3 chloride ions 3(Cl - ) (+3) + 3(-1) = 0 Chemical Formula: AlCl 3(s) To get a net electrical charge of zero we will need three chloride ions because each chloride ion has only 1 negative charge and 1 aluminum ion has a charge of positive 3

19. Step-By-Step of what we just did... Rules for Writing Chemical Formulas for Ionic Compounds 1. Write the metal ion symbol first, then the non-metal ion 2. Figure out how many of each ion is required to balance the charges 3. Write the formula by indicating how many atoms of each element are in it by using a subscript those numbers. If the subscript is a 1, DO NOT write it in.

20. Short-cut method: CrissCross Na + (sodium ion) and Cl - (chloride ion) Na + Cl - Na 1 Cl 1 NaCl Ca 2+ (calcium ion) and O 2- (oxide ion) Ca 2+ O 2- Ca 2 O 2 CaO (reduce to simplest whole number ratio)  This method ‘criss-crosses’ the ion charges to the subscript position  IF you use criss-cross, be careful to simplify the formula keeping whole numbers!

21. You Try it! Write the proper chemical formula for the following ion combinations Ca 3 P 2(s) Ca 2+ + P 3- H 2 S (s) H 1+ + S 2- PbO 2(s) Pb 4+ + O 2- AlN (s) Al 3+ + N 3- Fe 2 O 3(s) Fe 3+ + O 2- MgBr 2(s) Mg 2+ + Br 1- Cu 3 N 2(s) Cu 2+ + N 3- KF (s) K 1+ + F 1- CompoundIonsCompoundIons Remember, all ionic compounds are solids at room conditions...

22. Naming Ionic Compounds From the chemical formula, can find the name of a compound. To do this, you need to know how to name a cation (the metal ion) and an anion (the non- metal ion): cation – simply the element name followed by “ion” transition metals have more than one charge possible, use Roman numerals after the metal name to indicate which ion is present - transition metals have more than one charge possible, use Roman numerals after the metal name to indicate which ion is present anion – change the end of the element name to ‘-ide’ followed by “ion”

23. Name the compound by writing the name of the cation (metal) then the name of the anion (non-metal) ex. CaF 2(s) Ca 2+ and F 1- name of the cation = calcium name of the anion = fluoride Name of the compound: calcium fluoride

24. ex. CuF 2(s) Cu 2+ and F 1- Name of the cation = copper(II) Name of the anion = fluoride Name of the compound: copper(II) fluoride Why do we need to specify which copper it is? Because there are two options Cu 2+ or Cu 1+

25. POLYATOMIC IONS Polyatomic ions are a group of atoms that together carry a negative charge (anion) or a positive charge (cation) The entire group of atoms behaves as one ion The entire group will carry the net charge (not just one of the atoms) Most polyatomic ions are negative (anions). The most common polyatomic cation is NH 4 +, the ammonium ion.

26. ex. chemical formula: CaCrO 4(s) calcium ion (Ca 2+ ) and chromate ion (CrO 4 2- ) name of the cation: calcium name of the anion: chromate Don’t change the names of ions from the polyatomic ion table – leave them alone! Name of the compound: calcium chromate Naming the compound from the chemical formula:

27. Determining the chemical formula from the name: ex. Compound Name: magnesium nitrate magnesium ion has a charge of 2 + nitrate ion has a charge of 1 - magnesium ion (Mg 2+ ) and 2 nitrate ions 2(NO 3 - ) Chemical Formula: Mg(NO 3 ) 2(s)