1. The Atom

3. Elements and Symbols C = Carbon N = Nitrogen O = Oxygen Cl = Chlorine Ba = Barium U = ? Cf = ? Bk = ? Md = ? Es = ?

4. K = Pb = W = Sb = Co = Cu = Cr = Mg = Mn =

5. Atom: basic unit of matter –Smallest unit of matter that individually retains the chemical characteristics of an element –Consists of a dense central region, called a nucleus, surrounded by a negatively charged cloud –Contains three types of subatomic particles: Proton Neutron Electron

6. The Proton Charge = + 1.602×10 −19 C –Called “ +1 ” for clarity Located in nucleus of atom Mass = 1.672 x 10 –24 g –Approx. 1 unified atomic mass unit (u) –1 u = 1.66 x 10 –24 g 1/12 the weight of a Carbon-12 atom

7. The Neutron No charge (0 C) Located in nucleus Mass = 1.675 x 10 –24 g –Approx. = 1 u

8. The Electron Charge = –1.602 x 10 –19 C –Called “ –1 ” Located outside nucleus in an e- “ cloud ” Mass = 9.109 x 10 -28 g –Approx. = 0 u

9. Plum Pudding Model J.J. Thomson 1904

10. Gold Foil Experiment Ernest Rutherford 1909 Proved J.J. Thomson ’ s theory wrong Evidence for existence of protons

12. Evidence of Electrons

15. Dmitri Mendeleev (1834-1907) Russian chemist –Arranged elements in horizontal rows in order of increasing atomic weight –Started new rows in order to make columns of chemicals with similar characteristics –Left spaces open for elements yet to be discovered

21. Classification of the Periodic Table Classification by Physical Properties

22. Metals Shiny Conduct electricity Ductile –Can be drawn through wires Malleable (Shapeable) High M.P. & B.P Solids @ room temp Except Hg

23. Non-Metals Don ’ t tend to conduct well Not usually ductile Tend to be brittle Low M.P. & B.P. Many are gases at r.t.

24. Metalloids Have chemical characteristics in between those of metals and non-metals Includes elements: B (Boron), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), Polonium (Po), Astatine (At)

25. Classification by Electronic Properties

26. Alkali Metals Group 1 (1A) Li, Na, K etc. Soft, shiny metals Conduct heat and electricity React violently with H 2 O –Form H 2 (g) and alkaline (basic) solutions

27. Akali(ne) Earth Metals Group 2 (2A) Be, Mg, Ca etc. Not as reactive as Alkali Metals, but still quite reactive Tend to make basic solutions when placed in water

28. Transition Metals Groups 3-12 Tend to have high densities and B.P. All are metals Often used for electrical conduction Often have vivid colors when in solution –Used for pigments

29. Colors of Transition Metal Compounds Iron Cobalt Nickel CopperZinc

30. Lanthanides Elements 57-71 –Lanthanum (La) to Lutetium (Lu) Commonly used in lasers Can deflect UV and infrared rays

31. Actinides/Actinoids Elements 89-103 –Actinium (Ac) to Lawrencium (Lr) Only Actinium, Thorium (Th), and Uranium (U) occur naturally –Others created by neutron bombardment Radioactive

32. Groups 13(3A) – 16(6A) No common name Boundary between metals and non-metals occurs here Contain elements abundant in earth ’ s crust, atmosphere, and living things Contains the metalloids

34. Halogens Group 17 (7A) Love to form salts with metals –NaCl, KBr, CaCl 2 Like to form diatomic molecules –F 2, Cl 2, Br 2

35. Noble Gases Group 18 (8A) Very unreactive Don ’ t like to bond to other molecules Generally not abundant

36. Diatomic Molecules Molecules consisting of only two atoms of either the same or different elements –O 2 –CO Homonuclear Diatomic Molecule: a molecule made of two atoms of the same element –H 2 Heteronuclear Diatomic Molecule: a molecule made of two atoms that are different elements –NO Dinitrogen (N 2 )

37. Allotropism The existence of multiple pure forms of an element, in the same phase (solid, liquid, or gas), that differ in structure Different forms are called allotropes Can exhibit varied physical properties and chemical behaviors Don ’ t confuse allotropes with isotopes!!! O2O2 O3O3

39. Which atom does the picture below represent?

40. Atomic # –# of protons Atomic symbol Atomic Mass Atomic Weight Mass # Molar Mass

41. HCFePdW Number of Protons Number of Electrons Number of Neutrons

43. Identify the atomic mass, number of protons, and number of neutrons for the following elements.

44. Isotopes Atoms of the same element that have different atomic masses –Same number of protons –Different # of neutrons

47. Problems 1)Lithium has two natural isotopes, 6 Li and 7 Li, which have percent abundances of 7.5% and 92.5% respectively. What is the average atomic mass of Lithium? 2)Using the percent abundances below, calculate the average atomic mass for Carbon C-12 = 98.890% C-13 = 1.110% C-14 = 0.0000000001% 3)Antimony (Sb) has two stable isotopes, 121 Sb and 123 Sb with masses of 120.9038 u and 122.9042 u, respectively. Calculate the percent abundances of these two isotopes

49. Atomic Orbitals and Electron Configurations

50. Atomic Orbitals Orbital: a specific region in an atom thought to posses the highest probability of containing the electron in question at any one time –Only hold maximum of two electrons at a time –4 basic types: s, p, d, f

51. S orbitals Spherical shape Lowest energy of the orbitals

52. P Orbitals Higher energy than s orbitals Dumb bell shaped Come in 3 ’ s p x, p y, p z

53. D Orbitals Higher energy than s and p orbitals Double dumb bell shape or single dumb bell with a donut Come in 5 ’ s d xy, d xz, d yz, d x2-y2, d z2

54. F Orbitals Higher energy than s, p, and d Come in 7 ’ s

55. How do we know where our electrons are? Electrons will seek the lowest E orbital available first

56. Hydrogen Helium 1 Lithium? Pauli Exclusion Principle: orbitals may hold up to two electrons. The electrons must be of opposite spin

59. Hund ’ s Rule: electrons pair only after each orbital of equal energy is occupied by a single electron

60. Problems Determine the electron configurations for the following atoms 1)N 2)O 3)Ne 4)Na 5)Mg 6)Al 7)S 8)Fe 9)W

61. Noble Gas Abbreviation The electron configuration of the noble gas that precedes the element in question is represented by the noble gas ’ bracketed symbol –Example: C = 1s 2 2s 2 2p 2 = [He] 2s 2 2p 2 Write the electron configurations for Vanadium and Bismuth

62. Exceptions to the Rules Cr Cu

63. Review Problems 1)Which of the following is considered qualitative data and which is quantitative? a)Temperature b)Creepiness 2)Juan likes to drive fast. If he regularly speeds along at 160 km/hr, how quickly is he going in miles/hr? In in/s?

64. 3)You have a box that emits a wave that has a wavelength of 5.0 x 10 -7 m. Using the electromagnetic spectrum below, predict what comes out of this box.

66. 4)In the Macy's Thanksgiving day parade, 2009, a Smurf made his debut. His white cap contained 36,763 L of helium and it was about 1/10 of his body size. Using this information, calculate the volume of the entire float. If the density of helium is 0.000178 g/cm 3, what is the mass of the helium for the entire float in kg?

68. 5)Identify which of the following are heterogeneous mixtures and which are homogeneous mixtures (solutions) a)Jim Beam b)Orange juice c)Chicken noodle soup d)7 up (fresh) e)Blood f)Clorox bleach

69. 6)What are the electron configuration and orbital box diagram for Phosphorous? 7)Which element has the chemical symbol Ag? 8)What are the electron configuration and orbital box diagram for Ag?