3. Standards 1a. Students know how to relate the position of an element in the periodic table to its atomic number and atomic mass. 1b. Students know how to use the periodic table to identify metals, semi-metals {metalloids}, non- metals, and halogens 1e. Students know the nucleus of the atom is much smaller than the atom yet contains most of its mass.

4. Purpose We will use this information to build our chemistry knowledge. We will use this information as the foundation to calculate limiting reagent problems. The standardized exams in the spring will test you on this information.

5. Objectives Know the 3 particles of the atom and where they reside Know the difference between atomic number and mass number Know how to write nuclide symbols Know the three isotopes of hydrogen Know how to calculate atomic mass Know how to calculate percent abundance

6. First Some Questions… What are atoms made up of? Protons, Neutrons and Electrons Where do you find these particles? Protons and Neutrons are located in the nucleus Electrons are located in the outer rings, outside the nucleus.

7. Vocabulary Atom- from the Greek atomos=indivisible. The atom is the smallest particle of an element that retains the properties of that element. Nucleus: the center of the atom; composed of neutrons and protons. Because the mass of the proton and the neutron is much larger than that of electrons, almost all the mass is located in the nucleus. Ion: a charged particle; # protons ≠ # electrons Electrons occupy most of the volume of an atom outside/around the nucleus.

8. Fundamental Particles Proton A positively charged particle located in the nucleus. Neutron A neutral particle located in the nucleus. Electron A negatively charged particle located outside the nucleus.

9. The Atom

10. Animation of the Atom http://vvsd.schoolwires.net/2349201028132033980/lib/ 2349201028132033980/atom_animated.gif http://vvsd.schoolwires.net/2349201028132033980/lib/ 2349201028132033980/atom_animated.gif http://vvsd.schoolwires.net/2349201028132033980/lib/ 2349201028132033980/atom_animated.gif http://vvsd.schoolwires.net/2349201028132033980/lib/ 2349201028132033980/atom_animated.gif http://www.google.com/imgres?imgurl=http://members.shaw.ca/len92/atom_animated.gif&imgrefurl=http://me mbers.shaw.ca/vict/electricity_intro.htm&h=260&w=270 &sz=6&tbnid=tAjDJsPzhGAxvM:&tbnh=95&tbnw=99&z oom=1&usg=__8fyNMhCgDiqyFH3eSESGT0PZS2o=&do cid=gQA81nwMuwx71M&sa=X&ei=ElBlUpyKFYP_igLhlI GwBg&ved=0CDgQ9QEwBA

11. Question What differentiates one atom from another atom? The number of PROTONS

12. Atomic Number (Z) Number of protons in the nucleus of an atom This number is found on the Periodic Table Atomic Number identifies an element Always a positive number (b/c it is a counting #) Tells number of electrons in a neutral atom An atom is electrically neutral

13. What does it mean to be electrically neutral? The atom has no charge The number of protons = the number of electrons

14. Question What observations can you make about atomic numbers on the periodic table? Atomic Number increases as you go across the rows from left to right.

15. Questions What is the atomic number of Chlorine? What can you tell me about its protons and electrons? What element has 20 protons? What is the relationship between the # protons and the atomic number? They’re equal.

16. Complete the Chart ElementSymbolAtomic ## Protons Potassium 5 16 Y K19 19 Boron B 5 Sulfur S 16 Yttrium 39 39

17. Atomic Structure of Potassium

18. Mass Number (A) Total number of protons and neutrons in the nucleus of an atom Always a positive number You can determine the nuclear composition of an atom from its mass number and atomic number

19. Question What do the atomic number and the mass number have in common? Both Positive integers Both have the same # of protons

20. How to find # of Neutrons Mass # - Atomic#= # Neutrons Or # protons + # neutrons= Mass # (atomic number + # neutrons)=Mass #

21. Complete the Chart Atomic#Mass##Protons#Neutrons#ElectronsChemical Symbol 910 1415 4722 5525 6C 19 9 9 F 14 29 14 Si 22 22 25 Ti 25 30 25 Mn 6 12 6 6

22. Isotopes Atoms of the same element with differing numbers of neutrons Atoms with the same atomic number but different mass number Isotopes of an element have different masses Chemical properties of different isotopes are virtually the same

23. Nuclide Symbol A=Mass # Z= Atomic #

24. Nuclide A specific kind of atom Specification of an element in terms of its nuclear composition/structure Tells number of protons and number of neutrons # protons# neutrons# electrons Chemical Symbol C6[6, 7, 8]6 Nuclide Symbol676

25. Complete the Chart Atomic#Mass##Protons#Neutrons#ElectronsChemical Symbol 910 1415 4722 5525 6C 19 9 9 F 14 29 14 Si 22 22 25 Ti 25 30 25 Mn 6 12 6 6 Nuclide Symbol

26. 3 Isotopes of Hydrogen Isotope Of Hydrogen Nuclide Symbol # protons# neutrons# electrons Deuterium 1 1 1 Protium 1 0 1 Tritium 1 2 1

27. Nuclides By specifying the nuclear structure, then you call it a nuclide. But if you say Carbon atom, you do not know which Carbon atom it is, therefore you don’t know how many neutrons it has Example: Brothers and Sisters- You are members of the Jones family, but you have not specified which Jones member you are referring to. If you say Jimmy Jones, then we know exactly which member you are referring to. Just like when you say carbon-13, we know exactly which kind of carbon atom, the one 7 neutrons in the nucleus.

28. Write the nuclide name and nuclide symbol # protons# neutrons# electronsNuclide Name Nuclide Symbol 172018 20 18 9214692 Chlorine-37 Anion Calcium-40 Cation Uranium-238

29. Atomic Mass A weighted average of the atoms in a naturally occurring sample of the element. Naturally occurring: no matter where you get the sample from, it will have the same percentages of isotopes.

30. Construct a Fruit Basket Fruit TypeWeight of Each Piece 2 grapefruit14 oz 4 apples10 oz 3 pears7 oz 1 kiwi3 oz What is the Average Weight?

31. Fruit Basket Average weight=9.2oz Each type of fruit makes a different contribution to the overall weight How many pieces of fruit actually weigh 9.2 ounces? None! What does 9.2 oz mean? Fictitious non-existent piece of fruit

32. Atomic Mass If you have a recipe, you could count items to put in, say 200 chocolate chips, 3 eggs, etc. But suppose I have a recipe to make a compound. I need 100 hydrogen atoms and 50 oxygen atoms-you cannot count atoms or pluck them out with atomic tweezers! So instead they are massed. Careful here, the mass of an object is completely different from the weight of an object.

33. Question What accounts for the mass of the atom? # protons & # neutrons in the nucleus

34. Atomic Mass Know that 1.0 amu is defined as exactly 1/12 the mass of a atom. Carbon-12 has 6 protons and 6 neutrons, therefore 1 proton or 1 neutron = ~1 amu 1 amu = 1.6606 x 10 -24 grams Since the mass mostly depends on # protons and # neutrons, you’d think atomic mass would be a whole number, but it isn’t. How come?

35. Atomic Mass In nature, most elements exist as a mixture of 2 or more isotopes. Each isotope of an element has a fixed, constant mass and fixed constant relative abundance. Relative abundance- The amount (%) of the isotope present in a sample of the element Sample of carbon from anywhere in the world; coal from S. Africa, W. Virginia or Pennsylvania → 99% C-12 and 1% C-13 Atomic Mass on the periodic table takes into account the larger and smaller masses of the isotopes → Idea of weighted average

36. Calculating Atomic Mass To calculate atomic mass you need to know 3 things: # of stable isotopes Mass of each isotope % abundance of each isotope

37. Example: Chlorine Calculation mass of isotope X relative abundance + mass of isotope X relative abundance =_______amu (34.969)(.7577) + (36.935)(.2423) = That’s the same value on the periodic table! IsotopeMass of IsotopeRelative AbundanceAtomic Mass Cl-3534.96975.77% Cl-3736.93524.23% 35.45 amu

38. Question How many chlorine atoms actually have a mass of 35.45 amu? NONE So the atomic mass, in amu, is the average of a fictitious non-existent atom of an element.

39. Example: Copper Calculation IsotopeMass of IsotopeRelative AbundanceAtomic Mass Cu-6362.9298amu69.09% Cu-6564.927830.91% (62.9298)(.6909)+(64.9278)(.3091)=63.5464 amu

40. Calculating Relative Abundance To Calculate % Abundance: Make a Chart Isotopic Mass x % Abundance of each isotope Set-up equation Solve for “x” Plug in “x” value to solve for “y”

41. Example IsotopeMass of IsotopeRelative AbundanceAtomic Mass B-1010.013 B-1111.009 1.00 x + y = 1.00 y = 1 – x 10.013 (x) + 11.009 (1 –x) = 10.811 10.013x + 11.009 -11.009x = 10.811 -0.996x = -0.198 x =.1987 y= 1-.1987 y=.8013 B-10 = 19.87% B-11 = 80.13% x 1- x

42. The End