The document discusses several key concepts in chemistry including: 1) The attraction between atoms in molecules and crystalline structures is a chemical bond such as ionic bonds formed between oppositely charged ions. 2) Metals form cations by losing electrons and bonding with other metal atoms via delocalized electrons allowing for conductivity. 3) Ionic compounds are formed between metallic cations and nonmetallic anions with ionic bonds between oppositely charged ions that results in crystalline solids.

2. The attraction between atoms in a molecule or crystalline structure When elements react atoms must collide

3. Bond that results when metal atoms release their valence electrons to a pool of electrons shared by all the metal atoms Holds metals together Results in high conductivity, malleability, and ductility

4. Composed of positively and negatively charged atoms Metals on left form compounds with nonmetals on right Form ionic bonds- a chemical bond between two ions with opposite charges

5. EXAMPLE: NaCl

7. Crystalline solids High melting and boiling points Shatter May be water soluble

8. Electrically neutral because same number of protons and electrons Gaining or losing 1 or more electrons, atom can be converted into charged particle called ion. Ion - an atom or group of atoms that has a positive or negative charge

9. Cations - positive ion, fewer electrons than protons, lose electrons Positive charge on a cation= number of electrons lost Ex. Neutral Mg atom loses 2 electrons  Mg 2+ ion Anions- negative ion, more electrons than protons, gain electrons negative charge on nonmetal anion equals the number of electrons gained Ex. S  gains 2 electrons, sulfide ion S 2-

11. Charge on atom Group 1,2,3 A form charges equal to the group number (+1, +2, +3) Nonmetals 5, 6, 7 A have negative charge usually equal to 8 – A group # (-3, -2, -1)

12. More than one stable ion Examples: Fe 2+ and Fe 3+ Cu + and Cu 2+ Many transition metals form 2 + ions.

13. Octet rule : atoms become stable by having 8 electrons in their outer energy level except some of the smallest atoms which have only 2 Noble gases lack reactivity (stable)(8 electron) Elements stable by achieving configuration of valence electron of 1 of noble gases. (Share or transfer electrons) Main group metals react so have an electron configuration like the noble gas before them Main group nonmetals react so they have an electron configuration like that of the noble gas after them

15. Dots around atomic symbol represent the number of valence electrons Write electron dot for Radon (Rn), Lead (Pb), and Xenon (Xe)

17. *How many electrons must be gained or lost to satisfy octet rule? Group 1A 2A 3A 4A 5A 6A 7A 8A # Valence electrons # e- gained/ lost * Charge on stable ion

19. MUST BE ELECTRICALLY NEUTRAL (0) Have the lowest possible number of each type of atom (Formula unit) Subscripts indicate number of ions Cations always written first and charges are not included!!

20. Cation first, anion second Cation of Main Group elements Simply use the name of element it is formed from Ex: Na + , sodium ion Cation of Transition Metals Use name of the element it is formed from AND charge designated by a Roman Numeral in ( ) Ex: Fe 3+ , Fe (III) ion

21. Anion Replace ending of name with _____________ Examples: fluoride, chloride, bromide oxide, sulfide, selenide, nitride, phosphide, arsenide Name the following ionic compounds: MgCl 2 FeF 3 LiBr ZnO Al 2 O 3 Na 2 S

22. Table 3-8, p.96

23. Several atoms bound together that collectively have a charge: 3- Example: phosphate ion

25. Name the following ions: NO 3 - CN - OH -

26. Write the formulas of the following ions: Phosphate ion Ammonium ion Permanganate ion

27. Parentheses may be needed for polyatomic ions EXAMPLE: aluminum hydroxide ____________________ ammonium phosphate___________________ sodium sulfate_________________________

28. p.95a

29. A Little Trick Magnesium phosphate

30. 1. List Cation first, anion second Ex. NaCl NOT ClNa Don’t write charges of ions Ex. KF NOT K + F - Use parentheses around a polyatomic ion formula if it has a subscript Ex. Al 2 (SO 4 ) 3 NOT AL 2 SO 4 3

31. Name the following compounds: CuO NaNO 3 NH 4 Cl

32. Write formulas for the following compounds: Barium Hydroxide Copper (II) carbonate Magnesium bicarbonate