The Modern Periodic Table

1. The Modern Periodic Table • Moseley • Set it up by ______________rather than ____________ • Periodic Law – properties occur in a repeating pattern when set up by atomic number.

2. The Modern Periodic Table • Periods (series) • Groups (families) • 2 different labeling systems

3. A few definitions… • Main Group Elements: • Groups ____________________ • Transition Elements: • Groups _____________________

5. Groups of Elements • Vertical columns are called groups • Group 1 = _____________________ • Group 2 = _____________________ • Group 17 = _____________________ • Group 18 = _____________________

6. The Modern Periodic Table • Representative elements • Also known as main group elements • Transition metals • Inner transition metals • Lanthanide series • Actinide series

7. Diatomic Elements • Elements that exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements).

8. Diatomic Elements • Elements the exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements). H2, N2, O2, F2, Cl2, Br2, I2 Examples of when these elements are NOT diatomic

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

10. Charge!!! When ___________________________________________

11. 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

12. Charge!!! When an atom LOSES electrons

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

14. Charge!!! When an atom GAINS electrons

15. 15 protons

16. 12 protons

17. 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 __________.

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

19. A Bit of Review

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

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

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

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

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

26. 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

27. 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

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

29. 2+ Be Summary of Ions (the letters) Monatomic ions • Some charges can be predicted based on group number

30. 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:

31. 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)

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

33. 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+ =

34. 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

35. 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+

36. Na F

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

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

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

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

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

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

44. 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

45. 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 ______________________!!!

46. Ionic Nomenclature (the words) formula to name

47. Fe2O3

48. Bi3N5

49. NiTeO4

50. Co2(CO3)3