1. What causes reactivity of elements All atoms want to have a completely full valence shell (normally 8 electrons). For the moment we will only concentrate on main group elements Noble gases are already full. Elements that are really close, desperately want to get there (halogens and alkali), and tend to be the most reactive.

2. Gaining electrons metals lose electrons, nonmetals gain electrons and metalloids can go either way is a loose rule. Obviously the quickest way for something that has more than 4 electrons to get to 8 is to gain electrons (through chemical bonds). halogens want to gain 1, oxygen group wants to gain 2, nitrogen group wants to gain 3.

3. Losing Electrons Metals will gain a full valence shell by losing electrons. (there is a full shell underneath unless it is hydrogen) alkali will lose 1 electron, alkaline earth will lose 2 etc.

4. Vocabulary Ion- charged atom or molecule Something becomes an ion by gaining or losing electrons (not protons) anion-negatively charged ion A NION A Negative ION Caused by gaining electrons cation-positively charged ion ca+ion Caused by losing electrons

5. charges on groups Alkali metals want to lose 1 electron. alkali metals form ions with a +1 charge Write this as Na + or K + alkaline earth- Ca 2+ Mg 2+ halogens want to gain one electron Cl - or Br - oxygen group wants to gain 2 O 2- or S 2-

6. Common Ion Charges

7. Ions are completely different from the element of the same name Valence electrons are mainly responsible for chemical/physical properties. alkali metals are so reactive because they “want” to get rid of that electron. An ion is the element after it got rid of the electron. Therefore the atom is nowhere near as reactive as it used to be. This is like comparing the ashes from a stick of dynamite to the stick of dynamite.

8. So are ions like noble gases? No, ions are not the same as noble gases valence electrons are mainly responsible for chemical/physical properties but not solely responsible. Protons and neutrons still have a role. When K loses an electron or Cl gains an electron it has the same number of electrons as Ar, however protons and neutrons are different. so K +, Cl -, and Ar are different things, even though they have the same number of electrons.

9. charges also affect properties Ar is neutral so it would be unaffected by a positive or negative charge. Cl - is attracted to a positive charge and repelled by a negative charge. K + would be attracted by a negative charge and repelled by a positive charge.

10. Ionic Bonding a metal will have an ionic bond with a nonmetal Something from the left bonding with something from the right

11. What are ionic bonds? ionic bonding- a transfer of electrons something gives up electron(s) something takes electron(s) for NaCl Na give an e - ;Cl takes that e -

13. -

14. What holds them together? bond implies they are stuck together, but there is nothing shared between them. Ionic bonds are held together by electromagnetic force (opposites attract) so Na + is attracted to Cl - when large amounts get together they stack in a crystal arrangement

15. Crystal Arrangement There isn’t exactly an ionic “molecule”, just a ratio of loose ions stacked together. This is sometimes called a formula unit.

16. How strongly are they held together? An ionic bond is the weakest bond that is considered a bond ionic bonding is only an attraction between particles However the attraction is strong enough to call it a bond *there are other attractive forces between particles that are not bonds

17. Salts salt does NOT just mean table salt NaCl salts are any of 1000’s of ionic crystalline solids road salt is CaCl 2 (you don’t want to eat this) salt- ionic compounds resulting from an acid-base reaction

18. Naming and determining the formula of ionic compounds

19. Determining the formula of ions Ionic compounds are neutral You need to find the lowest number of each ion to make it neutral for example: Na + and O 2- 2 sodium for every one oxygen Na 2 O

20. More examples Al 3+ and O 2- Al 2 O 3 K + and Cl - KCl the subscripts don’t effect the name if there is only one possibility still (cation)(anion)

21. Naming ionic compounds For monoatomic anions only drop the ending and add “-ide” so F - fluoride Cl -, O 2-, C 4- chloride, oxide and carbide

22. Continuing… cations keep the name of the element. When naming compounds always name the positive (cation) first and the negative (anion) last. so mixing ions of chlorine and sodium give you sodium chloride (positive) (negative)