1. LecturePLUS Timberlake1 The Atom Atomic Number and Mass Number Isotopes (Take out your Periodic Tables)

2. EQ’s 1.What is the Atomic Theory? 2.What is an atom and how are its components arranged? 3.What is an isotope and how are neutrons related to isotopes? 4.How are isotopes and an element’s average atomic mass related? LecturePLUS Timberlake2

3. 3 Atomic Theory Atoms are building blocks of elements Each element has similar atoms Different from atoms of other elements Two or more different atoms bond in simple ratios to form compounds

4. LecturePLUS Timberlake4 Subatomic Particles ParticleSymbol Charge Relative Mass Electron e - 1- 0 Proton p + 1+ 1 Neutron n0 1

5. LecturePLUS Timberlake5 Location of Subatomic Particles 10 -13 cm electrons protons neutrons 10 -8 cm nucleus

6. LecturePLUS Timberlake6 Atomic Number Represents the number of protons in an atom

7. LecturePLUS Timberlake7 Periodic Table Represents physical and chemical behavior of elements Arranges elements by increasing atomic number Repeats similar properties in columns known as chemical families or groups

8. LecturePLUS Timberlake8 Periodic Table 1 2 3 4 5 6 7 8 11 Na

9. LecturePLUS Timberlake9 Atomic Number on the Periodic Table 11 Na Atomic Number Symbol

10. LecturePLUS Timberlake10 All atoms of an element have the same number of protons 11 Na 11 protons Sodium

11. LecturePLUS Timberlake11 Learning Check AT 1 State the number of protons for atoms of each of the following: A. Nitrogen (N) 1) 5 protons 2) 7 protons 3) 14 protons B. Sulfur (S) 1) 32 protons 2) 16 protons 3) 6 protons C. Barium (Ba) 1) 137 protons 2) 81 protons 3) 56 protons

12. LecturePLUS Timberlake12 Number of Electrons An atom is neutral The net charge is zero Number of protons = Number of electrons Atomic number = Number of electrons

13. LecturePLUS Timberlake13 Mass Number Represents the number of protons and neutrons in an atom

14. LecturePLUS Timberlake14 Isotopes Atoms with the same number of protons, but different numbers of neutrons. Atoms of the same element (same atomic number) with different mass numbers Isotopes of chlorine 35 Cl 37 Cl17 chlorine - 35 chlorine - 37

15. ISOTOPIC NOTATION A Z X A = mass number (the total number of protons + neutrons) Z = atomic number (the total number of protons) X = element symbol

16. LecturePLUS Timberlake16 Atomic Symbols Show the mass number and atomic number Give the symbol of the element mass number 23 Na sodium-23 atomic number 11

18. READING ISOTOPIC NOTATION 46 21 Sc 46 = mass number 2125 (the total number of protons (21) + neutrons (25)) 21 = atomic number 21 (the total number of protons (21)) Sc = element symbol In a neutral atom, the number of electrons (21) is equal to the number of protons.

19. LecturePLUS Timberlake19 More Atomic Symbols 163165 O P Zn 81530 8 p + 15 p + 30 p + 8 n16 n35 n 8 e - 15 e - 30 e -

20. LecturePLUS Timberlake20 Learning Check AT 2 Naturally occurring carbon consists of three isotopes, 12 C, 13 C, and 14 C. State the number of protons, neutrons, and electrons in each of these carbon atoms. 12 C 13 C 14 C 6 6 6 #P _______ _______ _______ #N _______ _______ _______ #E _______ _______ _______

21. LecturePLUS Timberlake21 Solution AT 2 12 C 13 C 14 C 6 6 6 #P __6___ _ 6___ ___6___ #N __6___ _ _7___ ___8___ #E __6___ _ 6___ ___6___

22. LecturePLUS Timberlake22 Learning Check AT 3 An atom of zinc has a mass number of 65. A.Number of protons in the zinc atom 1) 302) 353) 65 B.Number of neutrons in the zinc atom 1) 302) 353) 65 C. What is the mass number of a zinc isotope with 37 neutrons? 1) 372) 653) 67

23. LecturePLUS Timberlake23 Learning Check AT 4 Write the atomic symbols for atoms with the following: A. 8 p +, 8 n, 8 e - ___________ B.17p +, 20n, 17e - ___________ C. 47p +, 60 n, 47 e - ___________ 16 O 8 37 Cl 17 107 Ag 47

24. LecturePLUS Timberlake24 Learning Check AT 5 An atom has 14 protons and 20 neutrons. A.Its atomic number is 1) 142) 163) 34 B. Its mass number is 1) 142) 163) 34 C. The element is 1) Si2) Ca3) Se D.Another isotope of this element is 1) 34 X 2) 34 X 3) 36 X 16 14 14

25. LecturePLUS Timberlake25 Masses of Atoms A scale designed for atoms gives their small atomic masses in atomic mass units (amu) An atom of 12 C was assigned an exact mass of 12.00 amu Relative masses of all other atoms was determined by comparing each to the mass of 12 C An atom twice as heavy has a mass of 24.00 amu. An atom half as heavy is 6.00 amu.

26. LecturePLUS Timberlake26 Atomic Mass Listed on the periodic table Gives the mass of “average” atom of each element compared to 12 C Average atom based on all the isotopes and their percent abundance (% abundance) Atomic mass is not a whole number Na 22.99

27. LecturePLUS Timberlake27 Learning Check AT6 Using the periodic table, specify the atomic mass of each element (round to the tenths place): A.calcium__________ B. aluminum__________ C. lead__________ D. barium__________ E. iron__________ 40.1 amu 27.0 amu 207.2 amu 137.3 amu 55.8 amu

28. LecturePLUS Timberlake28 Calculating Atomic Mass Percent abundance of isotopes Mass of each isotope of that element Weighted average = mass isotope 1 (%) + mass isotope 2 (%) + … 100 100

29. LecturePLUS Timberlake29 Atomic Mass of Magnesium Isotopes Mass of Isotope Abundance 24 Mg =24.0 amu 78.70% 25 Mg = 25.0 amu 10.13% 26 Mg = 26.0 amu 11.17% Atomic mass (average mass) Mg = 24.3 amu Mg 24.3

30. LecturePLUS Timberlake30 Learning Check AT7 Gallium is a metallic element found in small lasers used in compact disc players. In a sample of gallium, there is 60.2% of gallium-69 (68.9 amu) atoms and 39.8% of gallium-71 (70.9 amu) atoms. What is the atomic mass of gallium ?

31. LecturePLUS Timberlake31 Solution AT7 Ga-69 (%/100) 68.9 amu x 60.2 = 41.5 amu for 69 Ga 100 Ga-71 (%/100) 70.9 amu x 39.8 = 28.2 amu for 71 Ga 100 Atomic mass Ga = 69.7 amu

32. LecturePLUS Timberlake32 Finding An Isotopic Mass A sample of boron consists of 10 B (mass 10.0 amu) and 11 B (mass 11.0 amu). If the average atomic mass of B is 10.8 amu, what is the percent abundance of each boron isotope?

33. LecturePLUS Timberlake33 Assign X and Y values: X = % 10 B Y = % 11 B Determine Y in terms of X X + Y = 100 Y = 100 - X Solve for X: X (10.0) + (100 - X )(11.0) = 10.8 100 100 Multiply through by 100 10.0 X + 1100 - 11.0X = 1080

34. LecturePLUS Timberlake34 Collect X terms 10.0 X - 11.0 X = 1080 - 1100 - 1.0 X = -20 X = -20 = 20 % 10 B - 1.0 Y = 100 - X % 11 B = 100 - 20% = 80% 11 B

35. LecturePLUS Timberlake35 Learning Check AT8 Copper has two isotopes 63 Cu (62.9 amu) and 65 Cu (64.9 amu). What is the percent abundance of each isotope? (Hint: Check periodic table for atomic mass)

36. LecturePLUS Timberlake36 Solution AT8 2) 70% Solution 62.9X + 6490 = 64.9X = 6350 -2.0 X = -140 X = 70%