IONS!

1. IONS! How they are formed

2. Valence Electrons • Valence Electrons of an atom are the electrons that are in the outermost s and p sub shells. (ONLY S AND P) • To determine how many electrons are in your valence shell, look at where your element is on the periodic table.

3. Valence Electrons • Ex. Sodium- Na- In the s-block. Only 1 electron in the outermost s sub shell. • You can look at the electron configuration to help as well • 1s22s22p63s1- The 3s sub shell is the outermost shell. It only has 1 electron in it. There fore it only has 1 valence electron

4. Valence Electrons • Lets look at something that lies in the p sub shell. • Sulfur- S - 1s22s22p63s23p4- Remember valence electrons are in both the outermost s and p sub shells • How many Valence electrons? • Lets look at Bromine. How many valence electrons does it have?

5. Valence Electrons • Hint- Column 1 will always have 1 valence electron • Column 2 will always have 2 valence electrons • Column 13 will always have 3 valence electrons • Column 14 will always have 4 valence electrons • Column 15 will always have 5 valence electrons • Column 16 will always have 6 valence electrons • Column 17 will always have 7 valence electrons • Column 18 will always have 8 valence electrons

6. Valence Electrons • How many Valence electrons do the following elements have? • Calcium – Ca • Cesium – Cs • Iodine – I • Krypton – Kr • Carbon – C • Polonium – Po

7. Lewis Dot diagrams • Lewis Dot Diagrams, or Electron dot structures, are diagrams that show valence electrons as dots

8. Lewis Dot Diagrams • Practice: How many Valence Electrons and LDD • Calcium Ca- • Cesium Cs – • Krypton Kr – • Polonium Po-

9. Octet Rule • Notice how Krypton ( a Noble Gas) Has filled up its valence electrons. This is why Noble Gases do not form ions or bond with anything. They are perfectly content with being filled all the way. • All the other elements are jealous and want to be like the Noble Gases, so they have to take on or lose electrons to take on this filled Valence Shell • Octet Rule states- Atoms react by gaining or losing electrons so as to acquire the stable elecron structure of a noble gas, usually eight electrons.

10. Cations and Anions • To become more like the noble gases, all the other elements will start to either gain or get rid of electrons to fill out a Valence Shell • Whether an element gains electrons or loses them depends on where it is on the periodic table and what kind of material it is

11. Anions • Anions are formed by non-metals (to the right of the metalloids) • Anions will gain electrons to become negatively charged ions • Because Noble Gases already have a full valence shell, you will not find them becoming ions of any sort

12. Anions • Nitrogen- forms a -3 charge • Oxygen – forms a -2 charge • Sulfur – forms a -2 charge • Fluorine – forms a -1 charge • Chlorine – forms a -1 charge • Bromine – Forms a -1 charge • Iodine – Forms a -1 charge

13. Cations • Cations are metals. The metals typically only have just the s sub shell filled in the valence shell. It is easier to lose electrons to become more like a Noble Gas then to gain them • Cations will lose electrons and then therefore become positively charged.

14. Cations • Column 1 will lose 1 Valence electron and form a +1 charge • (Hydrogen can both lose and gain 1 electron depending on what situation it is in) • Column 2 will lose 2 valence electrons and form a +2 charge

15. Practice • What Charge does each Element Make? • Sr • Al • P • Cl • Kr

16. Transition Metals (D-block) • The transition metals make multiple positive ions. • The way that you will be able decide what charge that transition metal is will be determined by either having the name written out or by looking at the chemical formula of the compound that it will make

17. When Given the Written Name • When you are given the written name of a chemical formula with a transition metal in it, it will give you a roman numeral in parenthesis. The Roman numeral is the charge that the transition metal will take • Remember that Transition metals are all going to form positive ions or cations. • Ex. Iron (II) Chloride- Fe2+ reacting with Cl1-

18. When Given the Chemical Formula • When you are given a chemical formula with a transition element in it, Determine the charge of the anion first ( Anions do not change their charge in Ionic compounds) Then give the charge to the Transition metal that will negate the negative charge • Ex. FeCl3 – Chlorine has a charge of -1. There are three chlorines. That gives a total charge of -3. To make this a neutral atom, you must have a +3 charge to balance that out. Fe (iron) must have a +3 charge.

19. Practice • Give me the charge of the transition element • Lead (IV) Bromide • Copper (I) Fluoride • ZnO • Ni2O3

20. Poly Atomic Ions • Poly atomic ions are those that are formed by more than one type of element. Can be 2 or more different elements (usually not more than 3) • Example – Nitrate Ion is NO3- • Notice that there are two different elements, Nitrogen and Oxygen

21. Common Polyatomics • Hydroxide – OH1- • Hypochlorite – ClO1- • Nitrate – NO31- • Acetate - C2H3O21- • Bicarbonate – HCO31- • Sulfate – SO42- • Carbonate – CO32- • Phospate – PO43- • Ammonium – NH41+