Early Ideas about Matter
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1 Early Ideas about Matter
2 atom The smallest piece of the element with all the chemical properties of the element an old and new idea
3 Greeks Discontinuists Democritus Continuists Aristotle
4 Discontinuists Democritus Believed there was a smallest piece atomos = indivisible
5 Continuists Continuists thought there was no smallest piece they believed a bar of gold, for example, could be cut into smaller pieces forever
6 Aristotle s ideas There are four elements earth, air, fire, and water all matter is composed of these four elements in different proportions
7 The Alchemists Tried to turn lead into gold put more fire into it the medicine stone would cure the Pb developed many lab techniques and apparatus
8 The Renaissance A new approach to science experiment to test if the hypothesis is true many of Aristotle s ideas were shown to be wrong
9 Law of Conservation of Mass Lavoisier> France, 1790 s Matter (or mass) is neither created nor destroyed in an ordinary chemical reaction
10 Lavoisier did three important things: 1. brought in an entire new language for chemistry 2. established the correct identity of the elements and distinguished them from compounds, showing that those are combinations of elements 3. introduced the art of precise measurements. He turned chemistry into a physical science and can properly regarded as the father of modern chemistry.
11 Law of Definite Proportions In a given compound, elements are always combined in the same proportion by mass. Ex: H 2 O is always 11% H, 89% O by mass.
12 Dalton s Atomic Theory All matter is composed of atoms atoms are indestructible billiard ball model In a chemical reaction, are rearranged atoms conservation of mass
13 All atoms of the same element are identical Atoms of one element are different from the atoms of any other element elements could be identified and distinguished from each other
14 Atoms combine to form compounds in small whole number ratios. Ex: could be XY, X 2 Y, XY 2, etc, but never X 1 1/2Y
15 What came next? 49 new elements were discovered between new particles were discovered alpha, beta, gamma - radiation particles smaller than atoms
16
17 1897: JJ Thomson discovered electrons smaller than atoms negatively charged Robert Millikan problem with Dalton s model 1914 Rutherford s Gold Foil Experiment nuclear model of atom
18 Gold Foil experiment setup
19 Gold Foil Experiment - results
20 The repulsive force between the positively charged nucleus and positive alpha particles caused the deflections.
21 Early Ideas about Matter
22 Modern atom Nucleus in geometric center of the atom very small and dense nearly all of the atom s mass gives the atom its identity protons (+) and neutrons Nucleus held together by the strong force
23 Electron cloud gives the atom its size mostly empty space electrons electrons do not orbit like planets; more like bees/beehive
24 Summary of the subatomic particles Name Abbr Where Charge mass Who? Proton P+ Nucleus u Rutherf ord Neutro n Electro n No Nucleus u Chadwi ck e- Electron cloud u Thoms om
25 Summary of the subatomic particles particle where? Mass who? Proton p + Nucleus 1.007amu Rutherford Neutron n o Nucleus 1.008amu Chadwick Electron e - Electron cloud amu Thomson
26 Atomic Number (Z) the number of protons in the nucleus of an atom gives the atom it s identity also, equal to the number of electrons in a neutral atom
27 Mass Number (A) Equal to the number of protons plus the number of neutrons in the nucleus of an atom #n o = mass # - atomic # #n o = A - Z
28 Important note! The atomic number of an element is on the periodic table, but the mass number is usually not! The location of the numbers on the periodic table is at the printer s discretion
29 The good news: all atoms of the same element have the same atomic number The bad news: not all atoms of the same element have the same mass number What is different? The number of neutrons
30 isotopes Atoms of the same element with different mass numbers different numbers of neutrons different versions of the same element no difference in chemical properties only fundamental difference is in mass
31 Isotope symbols The elements symbol, plus... the mass # (A) is written in the upper left corner the atomic # (Z) is written in the lower left corner Kr
32 Examples of isotope symbols Compare carbon-12, carbon-13, and carbon-14 each have the same number of protons, but a different number of neutrons
33 Examples of isotope symbols 12 C 6p + 6n o 6 13 C 6p + 7n o 6 14 C 6p + 8n o 6
34 Isotopes and Mass Number
35 Ions An atom that is no longer neutral #p + #e - No change in the nucleus, so the same element, but now with a + or - charge
36 How does an atom become an ion? The atom either gains or loses electrons The nucleus is not directly involved in ionization The term used when a neutral atom becomes an ion The number of protons does not change
37 How does an atom become an ion? If the atom gains electrons, it becomes negatively charged Ex: If a sulfur atom, with it s 16 protons and 16 electrons gains two electrons It now has a charge of (+16) + (-18) = -2
38 How does an atom become an ion? If the atom loses electrons, it becomes positively charged Ex: If an aluminum atom, with it s 13 protons and 13 electrons loses three electrons It now has a charge of (+13) + (-10) = +3
39 anions Atoms that have gained one or more electrons Become negative (-) ions Usually nonmetals
40 cations Atoms that have lost one or more electrons Become positive (+) ions Usually the metals
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