Atoms vs. Ions

1. Atoms vs. Ions • Atoms are ______________!!!!! • This means that they have _____________ • ________________

2. Charge!!! When ___________________________________________

3. Atoms vs. Ions • Atoms can gain or lose e- to form IONS • ANY charged particle is called an • Losing e- gives ______________________charge • Called ______________ • Usually formed from metals • Gaining e- gives a _______________charged ion

4. Charge!!! When an atom LOSES electrons

5. Atoms vs. Ions • Atoms can gain or lose e- to form IONS • Gaining e- gives a ________________charged ion • Called ______________________ • Usually formed from _____________

6. Charge!!! When an atom GAINS electrons

7. 15 protons

8. 12 protons

9. Quick Rehash… e- are found in __________ outside the nucleus atoms are stable when: 1) number of ______ and ________ are equal 2) when the __________ is _________ atoms will either ______ or ______ valence electrons in order to have a valence shells hold up to __________, except for the ________, which only holds __________.

10. Calculating Charge of an Ion #p+ - #e- = ionic charge

11. A Bit of Review

13. Classification of Compounds • Below is a flow chart for the classification of inorganic compounds.

14. Types of Compounds Ionic Compound : ____________________ ______________________ Examples: Non-examples:

15. Types of Compounds Molecular Compound : __________________ ____________________________ Examples: Non-examples:

16. Classification of Ions • Below is a flow chart for the classification of ions.

17. Monoatomic Cations • Metal atoms can lose valence electrons and become positively charged cations. • Na+ is named • Al3+ is named

18. Metals That Form Multiple Ions • If a metal can form more than one cation, it is named for the parent, followed by _____________________________, followed by the word “ion.” • Fe2+ is the • Fe3+ is the

19. Monoatomic Anions • Nonmetals can gain valence electrons and become negatively charged anions. • Monoatomic anions are named by dropping the end of the element name and adding ____________ • Br- is the • O2- is the • N3- is the

20. Did you get it? Element Valence e- Ion charge Ion name iodine aluminum phosphorus barium

21. 2+ Be Summary of Ions (the letters) Monatomic ions • Some charges can be predicted based on group number

22. Summary of Ions (the letters) Monatomic ions • Some charges can be predicted based on group number • Cation name is the same as element name with ion added element: zinc (Zn) ion: element: cesium (Cs) ion: • Anion name changes ending of element name to ide element: nitrogen (N) ion: element: iodine (I) ion:

23. Summary of Ions (the letters) Poly atomic ion Poly: more than one or many atomic: atoms ion: a positively or negatively charged particle Almost always anions (three exceptions)

24. Summary of Ions (the letters) V__________ O __________ S __________ metals (ALMOST) ANYTHING IN HERE CAN BE A VOS

25. Summary of Ions (the letters) Variable Oxidation State metals • Charge can NOT be predicted based on periodic table • Can assume multiple ion charges non VOS metal – potassium ion = VOS metal – lead ion = • The charge of VOS metals MUST be indicated in the name with the use of roman numerals Pb2+ = Pb4+ =

26. Summary of Ions (the letters) Practice: Give the name of the ION of each of these elements rubidium oxygen cadmium carbon selenium phosphorus fluorine lithium

27. Summary of Ions (the letters) Practice: Give the name OR symbol for these ions: tin (II) ion S2- Fe3+ copper (I) ion Mg2+ bromide Mn4+ Ag+

28. Na F

29. Na Na+ F F- sodium ion fluoride ion fluoride ion

30. Let’s bond Bond: • Ionic • Ionic: Pertaining to or occurring in the form of ions • Bond: something that binds, fastens, confines, or holds together

31. Let’s bond • Formula Unit: • An individual unit formed by the union of two or more ions (huh?)

33. Nomenclature (the words) • Ionic Compounds • MUST ________________________________________ • MUST ________________________________________ Ionic Compounds: NOT Ionic Compounds:

34. Nomenclature (the words) • Molecular Compounds • MUST ________________________________________ • MUST ________________________________________ Molecular Compounds: NOT Molecular Compounds:

35. Nomenclature (the words) • Aqueous Acids • MUST _______________________________________ • MUST _______________________________________ • MUST _______________________________________ Aqueous Acids: NOT Aqueous Acids:

36. Nomenclature (the words) Practice: State whether these are ionic, molecular, or an acid HC7H6O3(aq) Zn3P2 (NH4)2Se(aq) CCl4 HBr(aq) CH2I2 H2CrO4(aq) SrO

37. Ionic Nomenclature (the words) name to formula Step 1: Step 2: Step 3: Step 4: Note: if you need more than one polyatomic ion, you MUST ______________________!!!

38. Ionic Nomenclature (the words) formula to name

39. Fe2O3

40. Bi3N5

41. NiTeO4

42. Co2(CO3)3

43. Pb(CrO4)2

44. Summary of Ionic Nomenclature Rules • Name to formula: • Write the symbol for each ion • Use the LCM of the charges to find the number of each ion needed • Write the formula • no charges should be written in the final formula • use parenthesis if and only if you need more than 1 polyatomic • Formula to name • Write the name of the cation first, then the name of the anion • if and only if cation is VOS, include roman numeral for charge

45. Name or give the formula for the following: 1) Na2Se 2) lithium nitride 3) SrI2 4) barium sulfide 5) KCl 6) aluminum oxide Did you get it?

46. More practice on naming: 1) cadmium chlorite 2) titanium (IV) phosphate 3) calcium acetate 4) copper (II) hydride 5) tin (IV) carbonate 6) Al(OH)3 7) AgF 8) Pb(SO3)2 9) Au2Se 10) Ni(BrO)2

47. mercury (I) phosphite Ag2CO3 (NH4)3PO4 tin (IV) sulfate iron (II) hydroxide Co2(SO3)3 Mn(CrO4)2

48. Non-Metals

49. Nomenclature (the words) • Molecular Compounds • MUST contain only nonmetals • MUST be neutral (no overall charge)

50. Molecular Nomenclature (the words) name to formula Step 1: Step 2: Step 3: