1. THE ATOM Counting

2. The Atom- September 5  Pick up a Chemistry textbook from the shelf  Take out one piece of notebook paper, write your name, date, and title it Chapter 3 Review  Pass your Progress Reports to the middle isle  Chapter 3 Test Tomorrow!

3. Chapter 3 Test Review  Textbook p. 89-90  Copy and answer the following questions on sheet of paper. (classwork grade)  #1,3, 6, 8, 9, 14, 15, 16, 17, 18, 21, 28  You should also be able to distinguish the four experiments and scientist that lead to the understanding of the atomic structure

4. Thursday, September 6  Take out your Chapter 3 Review from yesterday  Take out one piece of paper, write name, date, and title Chapter 3 TEST  You will need a calculator and your periodic table  -------------------------------------------------  When you finish, turn in test at assignment shelf  Begin Chapter 4 Vocabulary

5. The Atom- August 27  Copy and Answer 1. How many significant figures does 0.10092 have? 2. What two subatomic particles have an amu of 1? 3. Name one component of Dalton’s Atomic Theory:

6. The Atom- August 28  Copy and Answer 1. How many protons does Indium have? 2. What is the atomic number of Cobalt? 3. How many neutrons does Mercury have?

7. The Atom- August 29  Copy and Answer in your notes  TAKE OUT YOUR HOMEWORK FROM LAST NIGHT 1. What is the mass in grams of 3.50 mol of the element Nitrogen, N? 2. How many moles does a 180 g sample of Sulfur have? 3. What is the molar mass of NaCl?

8. The Atom- August 30  Copy and Answer 1. How many moles does a 18 g sample of Calcium have? 2. What is the mass in grams of 4.50  10 8 atoms of Sulfur, S?

9. The Atom  Atomic Number Atoms of different elements have different numbers of protons Atoms of the same element all have the same number of protons The atomic number (Z) of an element is the number of protons of each atom of that element

10. Reading the Periodic Table

11. The Atom  Atomic Number

12. The Atom  Isotopes Isotopes are atoms of the same element that have different masses The isotopes of a particular element all have the same number of protons and electrons but different numbers of neutrons

13. The Atom  Mass Number The mass number (also known as atomic mass/weight) is the total number of protons and neutrons that make up the nucleus of an atom

14. The Atom  Mass Number

15. Designating Isotopes Hyphen notation: The mass number is written with a hyphen after the name of the element designating an isotope Nuclear symbol: The superscript indicates the mass number and the subscript indicates the atomic number uranium-235 Mass number  Atomic number 

16. The Atom  Designating Isotopes The number of neutrons is found by subtracting the atomic number from the mass number Nuclide is a general term for a specific isotope of an element URANIUM- 235 : primordial isotope from supernova explosion at the creation of solar system mass number − atomic number = number of neutrons 235 (protons + neutrons) − 92 protons = 143 neutrons

17. The Atom  Designating Isotopes

18. The Atom  Designating Isotopes Sample Problem How many protons, electrons, and neutrons are there in an atom of chlorine-37?

19. The Atom  Designating Isotopes Sample Problem Solution Given: name and mass number of chlorine-37 Unknown: numbers of protons, electrons, and neutrons Solution: atomic number = number of protons = number of electrons mass number = number of neutrons + number of protons

20. The Atom  Designating Isotopes Sample Problem Solution Solution: mass number of chlorine-37 − atomic number of chlorine = number of neutrons in chlorine-37 mass number − atomic number = 37 (protons plus neutrons) − 17 protons = 20 neutrons An atom of chlorine-37 is made up of 17 electrons, 17 protons, and 20 neutrons

21. Relative Atomic Masses The standard used by scientists to compare units of atomic mass is the carbon-12 atom, which has been arbitrarily assigned a mass of exactly 12 atomic mass units, or 12 amu One atomic mass unit, or 1 amu, is exactly 1/12 the mass of a carbon-12 atom The atomic mass of any atom is determined by comparing it with the mass of the carbon-12 atom

22. Average Atomic Masses of Elements Average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element Calculating Average Atomic Mass The average atomic mass of an element depends on both the mass and the relative abundance of each of the element’s isotopes

23. Average Atomic Masses of Elements Calculating Average Atomic Mass Copper consists of 69.15% copper-63, which has an atomic mass of 62.929 601 amu, and 30.85% copper- 65, which has an atomic mass of 64.927 794 amu The average atomic mass of copper can be calculated by multiplying the atomic mass of each isotope by its relative abundance (expressed in decimal form) and adding the results

24. Average Atomic Masses of Elements Calculating Average Atomic Masses (0.6915 × 62.929 601 amu) + (0.3085 × 64.927 794 amu) = 63.55 amu The calculated average atomic mass of naturally occurring copper is 63.55 amu

25. The Atom  Average Atomic Masses of Elements Sample Problem What is the average atomic mass units (amu) for the following isotopes? 23.66% - 56.3345 amu 37.84% - 57.1033 amu 38.50% - 56.5677 amu

26. 23.66% - 56.3345 amu 37.84% - 57.1033 amu 38.50% - 56.5677 amu (.2366 x 56.3345) + (.3784 x 57.1033) + (.3850 x 56.5677) = = 56.72 amu

27. The MOLE  Relating Mass to Number of Atoms The Mole The mole is the SI unit for amount of substance A mole (abbreviated mol) is the amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12

28. The MOLE  A dozen of something is =  A pair of something is =  A ream of paper is =  A trio of something is=

29. The Mole “If I have a dozen gumballs in my hand, and Bob has a dozen sticks of gum in his hand, who has more pieces of gum?”

30.  Just as a dozen is ALWAYS 12 of something, a MOLE is the same number regardless of what you are talking about.  A mole is always 6.02 x 10 23  That is 602,000,000,000,000,000,000,000.

31. AVOGADRO’S Number Avogadro’s number = 6.022× 10 23 the number of particles in exactly one mole of a pure substance Number of molecules in one mole of a chemical compound -OR- Number of atoms in a chemical element

32.  How many cats are in a mole?  How many donuts are in a mole?  How many molecules are in a mole?  How many atoms are in a mole?

33. Molar Mass The mass of one mole of a pure substance is called the molar mass of that substance Molar mass is usually written in units of g/mol The molar mass of an element is numerically equal to the atomic mass of the element in atomic mass units

34. The Atom  Relating Mass to Number of Atoms Gram/Mole Conversions Chemists use molar mass as a conversion factor in chemical calculations For example, the molar mass of helium is 4.00 g He/mol He To find how many grams of helium there are in two moles of helium, multiply by the molar mass

35. The Atom  Relating Mass to Number of Atoms Conversions with Avogadro’s Number Avogadro’s number can be used to find the number of atoms of an element from the amount in moles or to find the amount of an element in moles from the number of atoms In these calculations, Avogadro’s number is expressed in units of atoms per mole

37. Relating Mass to Number of Atoms

38. Sample Problem What is the mass in grams of 3.50 mol of the element copper, Cu?

39. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Given: 3.50 mol Cu Unknown: mass of Cu in grams Solution: the mass of an element in grams can be calculated by multiplying the amount of the element in moles by the element’s molar mass

40. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Solution: The molar mass of copper from the periodic table is rounded to 63.55 g/mol

41. Relating Mass to Number of Atoms Sample Problem A chemist produced 11.9 g of aluminum, Al. How many moles of aluminum were produced?

42. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Given: 11.9 g Al Unknown: amount of Al in moles Solution: the moles of an element can be calculated by dividing the amount of the element in grams by the element’s molar mass

43. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Solution: The molar mass of aluminum from the periodic table is rounded to 26.98 g/mol

44. Relating Mass to Number of Atoms Sample Problem How many moles of silver, Ag, are in 3.01  10 23 atoms of silver?

45. Relating Mass to Number of Atoms Sample Problem Solution Given: 3.01 × 10 23 atoms of Ag Unknown: amount of Ag in moles Solution: the moles of an element can be calculated by dividing the atoms of the element in moles by Avogadro's number of atoms

46. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Solution:

47. Relating Mass to Number of Atoms Sample Problem What is the mass in grams of 1.20  10 8 atoms of copper, Cu?

48. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Given: 1.20 × 10 8 atoms of Cu Unknown: mass of Cu in grams Solution:

49. The Atom  Relating Mass to Number of Atoms Sample Problem Solution Solution: The molar mass of copper from the periodic table is rounded to 63.55 g/mol

50. Moles, Molecules, and Grams How many molecules are there in 24 grams of FeF 3? 1.Find the molecular weight of FeF 3: 2.Set up your dimensional analysis: 62.845 g

51. Moles, Molecules, and Grams How many grams are the in 7.4 x 10 (23) molecules of AgNO 3? 1.Find the molecular weight of AgNO 3 : 2.Set up your dimensional analysis: 169.87 g