Atoms: The Building Blocks of Matter CHAPTER 3
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1 Atoms: The Building Blocks of Matter CHAPTER 3
2 The Early Greek View Democritus: 400 BC World was made up of two things: Empty Space Tiny particles called atoms. Atoms were the smallest possible particle. (indivisible)
3 Each material had its own atom that differed only in size and shape. Atoms are in constant motion and able to join with different atoms to form other types of matter. General -not supported by experimental data. Democritus had a problem. -his view was not accepted.
4 Aristotlehad the accepted theory at the time. All matter was continuous and made up of only one substance called hyle. (?) View held until the 17th century.
5 John Dalton -Early 1800 s Matter was composed of atoms. Atoms were indivisible, uniformly dense, solid spheres that were not changed during chemical reactions. All atoms of the same element have the same mass and chemical behavior.
6 Law of Definite Proportions Atoms of different elements always combine in fixed whole number ratios by mass to produce specific compounds regardless of the size of the sample or the source of the compound. Water is always H 2 O
7 Law of Multiple Proportions If two or more different compounds are composed of the same two elements then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers. H 2 O AND H 2 O 2 CO AND CO 2
8 In a chemical reaction, atoms are combined, separated, or rearranged. Matter is not created or destroyed during a chemical reaction.
9 Dalton s Model of the Atom
10 Thomson s Experiment Worked with a CRT. Cathode Ray Tube
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14 Cathode Ray Tube in Action + Side = anode - Side = cathode
15 CRT (Cathode Ray Tube) glowed when struck by particles from a metal. (Cathode Ray) Particles could be deflected by a magnet. All metals had the same particle.
16 Thomson concluded that they were located in all atoms. Thomson is credited with discovering the electron. (e - )
17 Atoms are electrically neutral. Thomson concluded there also must be positive particles (Protons) in atoms. Thomson s Model of the Atom was called the plum pudding model.
18 Positive charges surrounded by negative charges spread throughout.
19 Robert Millikan Found the charge of a single electron (e - )to be -1.6 X C. (C = Coulombs -unit of electric charge) The mass of the e - was found to be 9.1 X gram.
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21 + _ Power Supply
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23 The charge on a proton (p) was found to be +1.6 X C. Equal and opposite in charge of an e -. The mass of the pwas found to be 1.67 X gram. pis 1836 X heavier than an e -.
24 Rutherford s Gold Foil Experiment
25 a
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28 Atom is mostly empty space. Found that the + charges (p) are concentrated in the center of the atom commonly known as the: Nucleus
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30 Negative charges (e - ) move at fast speed around the nucleus
31 Chadwick Discovered a neutralparticle located in the nucleus. Named it the neutron (n). nmass is approximately the same as that of a p.
32 The atom now looked like this: n n + + +n + - -
33 Bohr s Model of the Atom Planetary Model: e - orbit the nucleus (p and n) in fixed intervals like planets around the sun. Two dimensional model.
34 Nucleus contains pand n. Orbiting e -.
35 Relationships: p, n, e -, AN, AM Atoms are electrically neutral. The number of e - must equal the number of p. Each element has its own characteristic number of p. The pdetermines the elements identity.
36 Atomic Number (AN) ANshows the number of pin an atom. The ANalso indicates the number of e - in a neutral atom. Notwoelements can have the same AN.
37 e - are very small and for all practical purposes massless. Mass of a p= mass of a n. Mass of a pand n= 1 AMU. Can not have anything other than a whole number of pand n.
38 Therefore the atomic mass (AM) or atomic weight is the sum of the pand n. AM=p+ n AM ( > = < ) AN
39 AM Charge Element Symbol AN
40 36 17 Cl 0 p = n = AN = p p = e - if neutral AM = p + n e - = AN = AM = = 17 + n
41 17 0 p = O n = AN = p p = e - if neutral AM = p + n e - = AN = AM = = 8 + n
42 25 0 Mg p = 12 n = e - = AN = AM = 12 25
43 Ions Ions are charged atoms. In many cases, chemical bonding is the attraction between oppositely charged particles. (Ionic Bonding) Na + Cl - Na + HCO 3 - Baking Soda
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45 How do atoms become charged? Neutrons are neutral. Protons are charged but they are in the nucleus and can not be adjusted. Also changing the number of protons would change the element.
46 The only particle capable of being added or removed are the electrons.
47 7 3 Li 0 p = e - = n = In a neutral atom, + and - charges are balanced. AN = AM = 3 7
48 7 3 Li +1 p = e - = In a positive ion, + and - charges are unbalanced. n = AN = AM = ions are formed by removing e -.
49 7 3 Li -1 p = e - = In a negative ion, + and - charges are unbalanced. n = AN = AM = ions are formed by adding e -.
50 24 12 Mg +2 p = n = e - = AN = AM = ions are formed by removing e -.
51 79 Se -2 p = n = 45 e - = 36 AN = 34 AM = 79 - ions are formed by adding e -.
52 Isotopes Atoms of the same element which differ slightly in atomic mass. Same element -same properties. Electrons are considered massless and the number of protons can not change.
53 Therefore the different masses are caused by different numbers of neutrons.
54 Note: when dealing with single atoms, the mass will be a whole number. A group of atoms will yield an average mass which will be fractional.
55 How do we know there are different isotopes? A mass spectrograph is used to deflect ions of an element as they move through a magnetic field.
56 Mass Spectrometer and Its Data a A a
57 Lightest Isotope Heaviest Isotope
58 A stream of Mg +2 ions is shot through a magnetic field. The following is observed. Magnet Ion Gun 25 Mg 24 Mg Ion Detector Screen
59 Sample Problems with Isotopes: Magnesium is made up of two different isotopes: 68.8% 24 Mg and 31.2% 25 Mg What is the (AMM) - average molar mass?
60 Percentages are based on 100. Assume a 100 particle sample. AMM = (68.8X 24) + (31.2 X 25) 100 % 24 Mg % 25 Mg AMM=24.3 grams
61 An element has an AMM of grams. There are two isotopes: 63 Cu and 64 Cu What are the percentages of each isotope?
62 Since percentages are based on 100, assume a 100 particle sample. X = 64 Cu (100 - X) = 63 Cu
63 63.54 = (100 -X) 63 + (X) AMM % 64 Cu % 63 Cu 100 particle sample
64 6354 = (100-X) 63 + (X) = X + 64X 6354 = X 54 = X Therefore: 54% = 64 Cu 100 -X 46% = 63 Cu
65 Rb is made up of two isotopes: 84 Rb and 86 Rb and has an AMM of grams. What are the percentages of each isotope?
66 The Mole
67 S X X X X C K 2 Cr 2 O 7
68 How Many Is A Mole? One mole is the amount of a substance that contains 6.02 X particles X is called Avogadro s number or A.N.
69 A.N.in Perspective. Grain of rice: Mass = 1.75 X 10-5 kg What would be the mass of 1 mole of rice? (6.02 X grains) 1.75X10-5 kg X grain 6.02 X grains= mole 1.05 X kg mole
70 1.05 X kg X 1 car = 1.8 X 10 3 kg 5.9 X cars 5.9 X cars = 5 X 10 9 people 1 X 10 6 cars person
71 41 grains of salt grams/grain 6.02x10 23 grains x grams grain = 4.64x10 21 grams
72 A 1 mole of salt grains cube. 27 miles per side. The same cube as viewed by a random location in Tampa Bay.
73 What about 1 mole of humans? How much space would we have if we just considered dry land? That would give just every human a square space that is millimeters on a side.
74 Why is it so huge? It s huge because molecules and atoms are super super tiny. You need a whole bunch of them to make up something that you can actually measure.
75 MOLAR MASS Molar Mass: Mass of one mole of any element or compound. From the periodic table: Aluminum has a mass of: AMU 1 AMU = 1.66 X grams
76 THEREFORE: AMU X atom 1.66 X grams = AMU 4.48 X grams atom
77 Now, suppose we have grams of Al g Al X 1 atom Al = 4.48 X g Al 6.02 X atoms Al
78 Therefore: The mass of 1 mole of Al (6.02 X atoms) is grams. The mass, in grams, of one mole of atoms is numerically the same as the mass in AMU of one of the atoms.
79 One mole Al = 6.02 X atoms grams One mole Fe = 6.02 X atoms 55.8 grams
80 Simple Problems If you collect 26.0 grams of C, how many moles of C do you have? 26.0 g C X 1 Mole C 12.0 g C By Definition: = 2.17 moles C Off the P.T.
81 Helpful Chart
82 Periodic Table 6.02 X grams moles particles Molecules, atoms, or formula units
83 More Examples If 3.0 moles of Fe were used in an experiment, how many atoms of Fe were used? 3.0 moles Fe X 6.02 x 1023 atoms = 1 mole Fe By Definition x atoms Fe
84 If 3.00 moles of Fe were used in an experiment, how many grams of Fe were used? 3.00 moles Fe X 55.8 gram Fe = From 1 mole Fe P.T. 167 grams Fe
85 111.6 grams of Fe is equal to how many atoms of Fe? g Fe X 1 mole Fe X 55.8 grams From P.T x atoms = 1 mole Fe x atoms Fe By Definition
86 115 grams of Na is needed, how many atoms of Na is this? 115 g Na X 1 mole Na X 23.0 g Na From P.T x atoms Na = 1 mole Na 3.01 x atoms Na By Definition
87 2.107 X atoms of P are used to make a match. How many grams of P is this? X atom P 24 X 1 mole P X 6.02 x atom P 31.0 grams P = 1 mole P g P
88 225 grams of potassium is needed, how many moles of potassium is this? 3.52 X atoms of Zn are used to make a batch of pennies. How many grams of Zn is this? 2.50 moles of oxygen gas was used to burn a sample of hydrogen gas. How many grams of oxygen gas was burned?
89 The End
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