1. Ms. Claudia Barahona September, 2, 2011

2.  Elements and symbols (Biosensors)  The periodic table (History, periods, groups)  Metals, Nonmetals and metalloids  Classification of groups (alkali metals, alkaline earth metals, transition metals, halogens, noble gases, etc) Classification of groups (alkali metals, alkaline earth metals, transition metals, halogens, noble gases, etc)  Ions (Cations and Anions) Ions (Cations and Anions)  Naming Ions Naming Ions

3.  Ionic charges from group members Ionic charges from group members  Ionic compounds Ionic compounds  Writing and naming Ionic compounds Writing and naming Ionic compounds

4. Representative elements Transition Metals

5.  Representative elements: IA 8A  Transition elements: B block The group number, indicates the number of valence electrons. A newer numbering system assigns group numbers of 1 ---- 18.

6.  e- in the atom’s outermost orbitals (highest principal energy level) - In charge of determining the chemical properties of elements.

7.  Characterization of the elements  Learning guide Pg 28 activity II.1. Part 1, 2 and 3

8.  Shiny 'metallic' appearance  Solids at room T° (except mercury)  High melting points  High densities  Malleable (bend or hammered)  Ductile (can be stretched into a wire)  Good heat and electrical conductors.

9.  Poor conductors of heat and electricity  Brittle solids  Lack of luster  Low melting points  Low densities

10.  Possess some characteristics of metals/some of nonmetals  Reactivity depends on properties of other elements in reaction  Often make good semiconductors

11.  By the number of elements Binary Ternary Polyatomic  By their chemical function Acids Bases Oxides Salts H.W To hand in, build a concept map on the different classification of compounds, exaplain each. Give 3 examples.

12. Chemical symbols  ONLY THE FIRST LETTER IS CAPITALIZED, if, the symbol has a second letter it is lowercase. Co ≠ CO  Russian chemist, Dmitri Mendeleev, arranged the 60 elements known at that time into groups with similar properties and placed them in order of increasing atomic masses. * The periodic table is arranged in order of increasing atomic number!!!

13.  Atomic mass or atomic weight: Weight average mass of all the natural occuring isotopes of an element  Atomic number: Is equal to the number of protons in an atom.

14.  Period: Each horizontal row.  Group/family: Each vertical column, this elements will have similar properties.

15. Representative elements Transition Metals

16.  Research the name of the different groups in the periodic table and the characteristics belonging to each group.

17.  Most of the elements in their natural state are found as compounds. Diatomic molecules  7 elements are found as diatomic molecules: H 2, N 2, O 2, F 2, Cl 2, Br 2 and I 2

18.  H.W  Learning Guide, Activity I.1, Pg 27  Part 1 and 2.

19. Universe Planet

20. Human body

23.  Octet rule: Tendency for atoms to attain a noble gas electron configuration.  Compounds are the result of the formation of chemical bonds between 2 or more different elements,  Ionic Bonds: Metal atoms lose valence e- and atoms of nonmetals gain valence e-.

24.  Forms when atoms lose or gain e- to form octets.  Cations  A metal ion is named by its element name. Example  Magnesium Ion Mg 2+  Sodium Ion Na +

25.  Anions  Negatively charge Ions.  Is named by using the first syllable of its name followed by -ide.  Examples Chloride Cl - Bromide Br -

26. Group IA – Alkali metals Ions +1 Group IIA Alkaline earth metals Ions +2 Group IIIA Ions +3

27. Nonmetals Group VA Ions -3 Group VIA Ions -2 Group VIIA Halogens Ions -1

29.  Transition metals: Form 2 or more kinds of positive ions (variable charge) because they lose their outer e- as well as e- from a lower energy level.Is not possible to predict the ionic charge from the group number. ElementPositive Ions Name of Ion CobaltCo+2Cobalt (II) Co+3Cobalt (III) LeadPb+2Lead (II) Pb+4Lead (IV)

30.  The old system of naming ions, involves latin names.  The ion with the lesser charge ends with –ous  The one with greater charges ends with –ic Metals with variable charges

32. Stock system Use the roman numeral system. The ionic charge is placed in () inmediately after the elemental name of the metal. Example: » Fe +2 Iron (II) » Fe+3 Iron (III)

33. 1. K + 2. F - 3. Na + 4. O 2 2- 5. Al 3+ 6. S 2- 7. Ga 3+ 8. PO 4 3- 9. NH 4 + 10. Cu 2+ 11. Fe 2+ 12. Pb 2+ 13. SO 4 2- 14. Pb 4+ 15. NO 3 - 16. Sn 4+ 17. Pb +4 18. Sn +2 19. N -3 20. Au +1 21. Au +3

34.  Covalent Bonds: Forms when atoms of nonmetals share valence e-.  In the formation of either and Ionic bond or a covalent bond, atoms lose, gain or share valence e-

35.  Learning Guide, Pg 31  Part 1, 2, 3 and 4  Classwork.  Learning Guide Activity II.1 Pg 31  Part 4  Assesment 7.3 Pg 224 Text Book.

36.  Classification and identification of inorganic compounds from chemical formulas  Learning guide, activity III.2 Pg 33 Part 1,2, 4

37.  Activity III.3  Wrinting names from chemical formulas  Pg 34  Part 1, 2, 3, and 5.

38.  Consist of positive and negative ions.  Ions are held together by strong electrical attractions between the opposite charges called ionic bonds.

39.  Formula: Indicates number and kinds of ions that make up the ionic compound.  The sum of the ionic charges in the formula is ALWAYS zero.

40. Binary compounds Those containing only 2 elements. 1. Identify the cation and anion. 2. Balance the charge. 3. Write the formula, cation first, using the subscript from the charge balance.

41.  The subscripts in the formula represent the number of positive and negative ions that give an overall charge of zero.

42.  Ionic compounds Cation is written first, followed by the anion. Example Na + and S -2

43.  Ionic compounds  Metal is given first, followed by the nonmetal.  Subscripts are never mention. Mg 3 N 2

44. FormulaCationAnionName NaCl FeCl 2 Fe 2 O 3 Cu 3 P CuBr 2 SnCl 2 PbS 2 Al 2 O 3

45. NameCationAnionFormula Copper (I) Oxide Magnesium chloride Nickel (III) Oxide Tin (IV) Chloride Cobalt (III) chloride Calcium Nitride Zinc bromide Gold (I) Oxide

46. compounds AcidsBasesOxidesSalts Binary Ternary Metallic Nonmetallic Binary Ternary

49.  Names of acids, usually ends in acid, and their formmulas fot one of two general patterns:  Binary acids: Named writing hydro followed by the root of the name of the halogen, then –ic and finally acid.  Ex. HCl hydrochloric acid

50.  Integrative activity III.4  Learning Guide pg 35  Part 1 and 2