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Matter Matter 1. Where do atoms come from? 2. Are new atoms being made right now on the earth? 3. If so, how? Where? 4. Are new atoms being made anywhere right now? 5. If so, how? Where? Matter Elements 1. Elements - contain only one type of atom 2. 90 naturally occuring elements (Uranium, 92 heaviest naturally occuring) 3. Transuranium (synthetic) elements 4. Types of elements a) Monoatomic – Fe, Au b) Molecular – H2, N2, O2, P4, C60 Matter Matter Origin of the Elements Matter Origin of the Elements Matter Supernova Remnant Matter Origin of the Elements Abundance (by mass) Earth’s Crust: 46% O Body: 65 % O Universe: 90% H and 10% He Matter History: The Atom Democritus 1. Atomos – Indivisible (~400 B.C.) 2. Smallest particle of a substance that retains the properties of that substance 3. Only “Atoms and the Void” Matter Matter History: The Atom John Dalton’s Atomic Theory (1803) a. All matter is made of indivisible particles called atoms b. Atoms of same element have same properties c. Atoms combine in small, whole # ratios d. Chemical reactions are merely the rearrangement of atoms Matter Symbols for Elements Jons Berzelius – standardized names and symbols of the elements Strontium = Sr Matter Matter Names for Elements a. Greek & Latin Na = Natrium K = Kalium Li = Lithos b. Places (Ge, Fr, Cf) Y, Yb, Er, Tb = Ytterby c. Scientists (Es, Fm, Cm) Matter History: The Electron J.J. Thomson (1897) – discovered the electron with a Cathode Ray Tube Matter History: The Electron Matter History: The Electron Matter History: The Electron Matter History: The Electron Matter Matter History: The Electron Thomson Plum Pudding Model Matter History: The Nucleus Rutherford (1911) 1. Discovered Nucleus 2. Gold Foil Experiment Matter History: The Nucleus 1:8000 bounced back (10,000 miles/s) Matter Matter History: The Nucleus Matter History: The Nucleus 3. Results a. Nucleus is heavy and dense b. 99.9% of atom’s mass is in the nucleus c. Electrons “orbit” the nucleus d. Most of the atom is empty space Matter Matter History: The Proton Rutherford (1914) 1. Had been suspected to exist since 1886 (Goldstein’s canal rays) 2. 1836 times heavier than the electron Matter History: The Neutron 1. Discovered last (1932) by Chadwick 2. Roughly same mass as proton Matter The World’s Most Famous Neutron Matter Particle Charge Mass Proton +1 ~1 g/mol Electron -1 0.00055 g/mol (1/1836) Neutron 0 ~1 g/mol Matter Matter Scanning Tunneling Microscope History: The Atom Matter History: The Atom Matter Protons, Neutrons and Electrons Reading the boxes 3 9 Li 6.941 F 18.994 Matter Isotopes 1. Isotopes – Atoms with the same # of protons, but different # of neutrons 2. Elements often exist as a mixture of isotopes Protons Copper-63 Copper-65 Neutrons Electrons p n E Isotopes 92Zr 38 50 38 11 13 11 55 79 55 233Th Matter Isotopes • Cancer treatment (60Co gives off gamma rays) • Medical Tracers (24Na for circulatory system) • 14C dating a. Mummies b. Shroud of Turin 4. Nuclear fuel (235U and 239Pu) Matter Isotopes 1. Some isotopes are more common 2. Hydrogen example 1H 2H (deuterium) 3H (tritium) 3. Atomic Mass – Weighted Average of the isotopes Matter Matter Average Atomic Mass 4. What is the ave atomic mass of Gallium if it exists as 60.30% 69Ga (68.926 g/mol) and 39.70% 71Ga (70.926 g/mol)? (Ans: 69.72 g/mol) Matter Average Atomic Mass 5. Out of 400 chlorine atoms, 302 are 35Cl (34.969 g/mol), and 98 are 37Cl (36.966 g/mol). Average atomic mass? 6. What is average atomic mass of Copper if 69.09% exists as 63Cu (62.9298 g/mol) and the rest exists as 65Cu (64.9278 g/mol)? (0.6909)(62.9298) = 43.48 ( )(64.9278) = 20.07 63.55 g/mol Matter Ions • • Cation – positive ion (more p than e) Anion – Negative ion (more e than p) p n e 9 26 17 10 30 18 10 23 18 16O223Na+ p n e Ions 13C 90Sr 16 16 14 16 18 18 35 44 36 19 21 18 24Mg2+ 15N3- Matter Group the following Au C Be C60 Te H2O P4 N2 NH3 S8 O2 P2O5 C2H4 Cl2 C6H12O6 Matter Compounds 1. Compounds - Composed of two or more different elements 2. Examples H2O, CH4, NaCl, Fe2(SO4)3 3. Are there more elements or compounds? Elements – Compounds - Matter What is a Molecule? 1. Group of atoms held together by covalent and polar covalent bonds (SHARING) 2. Usually composed of non-metals 3. Separate (discrete) groups of atoms 4. Molecular Elements - H2, P4 Molecular Compounds - CH4, H2O2 Matter Diatomic Molecular Elements H2 N2 O2 F2 Cl2 Br2 I2 Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine Iodine Matter Diatomic Elements Matter Matter Diatomic Elements Matter What is an Ionic Compound? 1. Usually start with a metal 2. Composed of ions – No sharing but stealing of ecation – positive ion anion – negative ion 3. Example: NaCl, CaCl2, FeSO4 4. Formula Unit – instead of molecule Matter Matter Ionic or molecular? HCl CO2 H2O BaF2 VO3 Write the formula for the compound between: Na+ and O2Al3+ and O2K+ and PO43Ba2+ and NO3- BrK+ Ca2+ Al3+ NH4+ Cu2+ O2- N3- NO3- SO42- Matter CO32- Protons C= O= NH4+ Electrons Matter The Key to the Universe Quarks Protons Neutrons Electrons Elements Compounds Matter 10. (d) Matter 11.a) 193, 79 b) 132, 52 d) 39, 17 13. protons neutrons 92 142 92 143 92 146 21.Palladium (Pd) 23. 1H is the most common c) 118, 53 electrons 92 92 92 15 Matter Isotope Isotopic Notation Tungsten184 184 Sodium23 23 Astatine200 200 Promethi um-148 Palladium -109 Atomic # Mass # Protons Neutrons Electrons 74W 74 184 74 110 74 11Na 11 23 11 12 11 85 200 85 115 85 61 148 61 87 61 46 109 46 63 46 85At 148 61P m 109 Pd 46 Vanadium -48 48 23V 23 48 23 25 23 Scandium -50 50 21Sc 21 50 21 29 21 Matter Ion Protons Neutrons Electrons Ion 14N+ 7 7 6 80Br- 15N2+ 7 8 5 24Mg2+ 14N- 7 7 8 27Al3+ 81Br- 35 46 36 27Al2+ 56Fe2+ 26 30 24 19F- 31P3- 15 16 18 238U2+ 119Sn4+ 50 69 46 123I- a) 24.28 g/mol Matter b) 12.01 g/mol c) 63.55 g/mol d) 6.925 g/mol e) 20.192 g/mol f) 28.09 g/mol g) 178.55 g/mol h) Boron-11 i) Bromine – 80 j) Chlorine - 35 28. 64.27 g/mol Matter 58.a) 38, 36 b) 15, 18 c) 23, 20 d) 15, 14 e) 40, 42 60.a) Sn2+ b) Ic) AlO2- d) ClF3+ 48 Ca(ClO4)2 Mg3(PO4)2 Matter 51 b) Ni(ClO4)2 53 a) Al2S3 Cr2(C2O4)3