Atomic Theory of Matter
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1 Atomic Theory of Matter The theory that atoms are the fundamental building blocks of matter John Dalton ( ) Postulates of Dalton s Theory 1) Each element is composed of extremely small particles called atoms 2) All atoms of a given element are identical to one another in mass and other properties, but the atoms of one element are different from the atoms of all other elements 3) Atoms of an element are not changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions 4) Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms
2 Law of Constant Proportion The elemental composition of pure substances is never varies Joseph Proust ( ) Law of Conservation of Mass The total mass of substances present at the end of a chemical process is the same as the mass of substances present before the process took place. Lavoisier ( )
3 Discovery of the electron () J. J. Thompson 1897 Determined: charge/mass ratio
4 Millikan Oil Drop Experiment 1909 Determined charge of an (1.6 x C)
5 Plum Pudding Model of the Atom J. J. Thomson Plum Pudding Model ~1900 Negative charges spread (like raisins) in uniform clump of positive matter (pudding)
6 Radioactivity Spontaneous emission of radiation Studied by Becquerel, and the Curies Ernest Rutherford discovered three types of radiation
7 Ernest Rutherford Discovery the Atomic Nucleus Aimed a radiation at Au foil Monitored the scattered particles
8 Ernest Rutherford Discovered the Atomic Nucleus Since most particles went through: - Plum pudding model incorrect - Most of the atom is EMPTY - The + portion is small and dense
9 Nucleus Contains Protons (+) and Neutrons (neutral) Rutherford discovers the proton in 1919 James Chadwick discovers neutron in 1932 Trinity Bomb atomic mass unit (amu) = x g
10 Scanning Tunneling Microscope (STM)
11 Modern View of Atom - Small positively charged, massive nucleus surrounded by light electrons in large orbits N P P P N N P N P N P N - Nucleus contains protons and neutrons - The number of protons determines which element it is - The number of equals the number of protons for nuetral atoms Nucleus - Different isotopes of an element have different number of nuetrons.
12 Atomic Symbols The mass of an atom in atomic mass units (amu) is the total number of protons and neutrons in the atom. P N N P N P N P N P N P Atomic Mass (Protons + Neutrons) 12 6 C Nucleus Atomic Symbol Atomic Number (Z) (# Protons, same elements same Z)
13 Isotopes Atoms of the same element with different masses. Isotopes have different numbers of neutrons C 12 6 C 13 6 C 14 6 C P N N P N N P N N P P N P N P N P N N P P P N P N N
14 Mass Spectroscopy
15 Periodic Table - Table of elements arranged by atomic number - The rows on the periodic chart are periods. - Columns are groups. - Elements in the same group have similar chemical properties. Non-Metals Metals
16 Periodicity When one looks at the chemical properties of elements, one notices a repeating pattern of reactivities.
17 Groups
18 Chemical Formulas CH 4 Number of atoms in the molecule Empirical formulas give the lowest wholnumber ratio of atoms of each element in a compound. C n H 2n O n = C n (H 2 O) n Molecular formulas give the exact number of atoms of each element in a compound. C 6 H 12 O 6
19 Chemical Formulas Structural formulas show the order in which atoms are bonded. Perspective drawings also show the thredimensional array of atoms in a compound.
20 Ions X X Ion = an atom or molecule that has a charge (neg. or pos.) Positive ions are called cations Negative ions are call anions
21
22
23 Ionic Compounds Writing Ionic Formulas:
24 Nomenclature for Inorganic Compounds -Write the name of the cation. -If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion, simply write the name of the polyatomic ion. - If the cation can have more than one possible charge, write the charge as a Roman numeral in parentheses NaCl = sodium chloride CuCl 2 = copper (II) chloride
25 Nomenclature for Inorganic Compounds -Write the name of the cation. -If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion, simply write the name of the polyatomic ion. - If the cation can have more than one possible charge, write the charge as a Roman numeral in parentheses NaCl = sodium chloride CuCl 2 = copper (II) chloride
26 Pattern in Oxyanion Nomenclature ClO 4 - perchlorate ClO 3 - chlorate ClO 2 - chlorite ClO - hypochlorite NO 3 - nitrate NO 2 - nitrite PO 4-3 phosphate PO 3-3 phosphite PO 2-3 hypophosphite SO 4-2 sulfate SO 3-2 sulfite
27 Acid Nomenclature
28 Nomenclature of Binary Compounds The less electronegative atom is usually listed first. A prefix is used to denote the number of atoms of each element in the compound (mono- is not used on the first element listed, however.) H 2 O = dihydrogen monoxide Ending on the more second atom ends with ide: CCl 4 carbon tetrachloride If the prefix ends with a or o and the name of the element begins with a vowel, the two successive vowels are often elided into one: N 2 O 5 = dinitrogen pentoxide
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