CHAPTER 4: Matter is Made up of Atoms
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1 CHAPTER 4: Matter is Made up of Atoms
2 ATOMS & THEIR STRUCTURE Aristotle thought matter was made of air, earth, fire and water.
3 Democritus (250 B.C.)- Said the world is made of empty space & tiny particles called atoms
4 DEVELOPMENT OF THE ATOMIC THEORY (3 SCIENTISTS INVOLVED) 1. Lavoisier ( )- Law of Conservation of Matter The Father of Modern Chemistry
5 2. PROUST (1799) Law of definite proportionselements that make up compounds are found in fixed proportions Joseph Proust
6 3. DALTON S ATOMIC THEORY 1. All matter is made of atoms. 2. Atoms are indivisible 3. All atoms of 1 element are alike, but are different than atoms of other elements
7 Was he right? 1. All matter is made of atoms. 2. Atoms are indivisible 3. All atoms of 1 element 3. All atoms of 1 element are alike, but are different than atoms of other elements
8 DISCOVERY OF ATOMIC STRUCTURE 4 SCIENTISTS JJ Thomson (1897) 1. Discovered the electron during his vacuum tube/cathode ray experiments.
9 2. JJ s Plum Pudding model
10 3. When studying Ne he discovered isotopesatoms of an element that are alike chemically, but differ in mass. *Same # protons, different # neutrons 4. His work led to the discovery of the neutron
11 NAGAOKA Saturnian model or early planetary model
12 RUTHERFORD A. Gold foil experiment 1. shot positive particles through a thin sheet of Au. 2. Most went straight through, but others were deflected.
13 WHY?
14 CONCLUSIONS DRAWN FROM THE GOLD FOIL EXPERIMENT 1. Most of the atom is empty space. 2. Discovery of the nucleus- small, dense, positively charged central core of the atom
15 NEILS BOHR (1913) 1. Given credit for the planetary model of the atom. 2. Was more specific than Nagaoka because he concluded that electrons are arranged in E levels.
16 BOHR S STATEMENTS ABOUT ELECTRONS 1. Said that electrons absorb E & move to higher states. 2. These excited electrons give off that E as light waves & fall back to a lower E level.
17 Neils Bohr s Atomic Model An excited electron jumps to an outer E level. It falls back, releasing light waves. The packet of light released is called a photon. +
18 The atom is not flat! Nucleus Electron Orbit Energy Levels
19 Our View of Electrons Today E levels are not neat orbits E levels are spaces around the nucleus where electrons are most likely to be found
20
21 Dalton JJ Thomson Nagaoka Today s model Bohr Rutherford
22 Subatomic Particles Subatomic particle Mass in µ Charge Protons 1.01 Positive Neutrons 1.01 Neutral Electrons Negative Mass of atoms is measured in atomic mass units (µ, or amu)
23 Determining Atomic Structure 1. Atomic numberthe # of protons in the nucleus & the # of electrons if the atom is neutral 2. Atomic mass/mass numberthe sum of protons + neutrons in the nucleus
24
25 Atomic mass Carbon C Atomic number 6 # protons = 6 # neutrons = 12-6= 6 # electrons = 6
26 You try it How many protons, neutrons, and electrons are present in nitrogen? p = 7 e = 7 n = 14-7=7 Try bromine p = 35 e = 35 n = 45
27 Why isn t atomic mass a whole number? It is a weighted average of all isotopes of an element. The isotope most common in nature is the one that has a mass closest to the one found on the periodic table. Ex: Most C has a mass of 12. The most common isotope of carbon is therefore C-12
28 Electrons in Energy Levels 1 st E level can hold a max of 2 electrons 2 nd E level can hold 8 3 rd can hold 18 4 th can hold 32
29 Drawing atoms Draw an atom of beryllium #p= 4 #n=9-4=5 #e=4 # valence electrons = 2 4 Beryllium Be Valence electrons = # electrons in outermost E level
30 Try to draw an atom of phosporus on your own Valence = 5 P=15 N=16
31 This is P-31. P=15 N=16
32 This is P-33. P=15 N=18 The only thing different is the # of neutrons
33 This is a neutral atom of P-31 Drawing ions To draw a +1 ion, take away 1 electron P=15 Now the N=16 atom has a +1 charge
34 Drawing ions To draw a -1 ion, add 1 electron P=15 Now the N=16 atom has a -1 charge
35 Drawing ions What do you do to make the atom have a -3 charge? P=15 N=16
36 IN SUMMARY You have learned about: The development of the atomic theory The discovery of atomic structure How to construct a model of an atom of any element using the periodic table
37 The End!!!!!!!!!
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