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Create groups for these Scientist and explain your groupings (use the information you got from your research) Work Involved: Periodic Table/Trends & Elements Dmitri Mendeleev - Periodic Law Worked with Meyer and Bunsen J.W. Dobereiner - Periodic Law Periodic Trends Glenn Seaborg - Discovery of 10 elements beyond Uranium Lothar Meyer - Periodic classification of the elements Atomic Theories Hantaro Nagaoka - Center of atom was highly positively charged (made Saturnian Model) John Dalton - Proposed atomic theory Democritus - Proposed ideals that later were expanded upon which then became the official atomic theory Niels Bohr - Developed the Bohr Model (orbital model) Atoms & Atomic Properties Antoine Henri Becquerel - Discovered radioactivity & SI measure of radioactivity James Chadwick - Discovery of neutron J.J. Thompson - Discovery of electron Plum pudding model Ernest Rutherford - Gold foil experiment Discovered Half-Life Developed Rutherford model Louis de Barogilie - Barogilie Hypothesis All matter has wave properties Marie & Pierre Curie - Discovered radioactivity and 2 elements Made Curie's Law Made "The Curie" (inofficial measurement of radioactivity) Robert Milikan - Determined weight and charge of a single electron 42
Research the Scientist and summarize their contributions to the Atomic Theory Antoine Henri Becquerel First person to discover radioactivity (SI unit for radioactivity is the becquerel [Bq]) Niels Bohr Developed the Bohr Model (orbit model of the atom where electrons can only reside in specific energy levels) Louis de Barogilie Broglie hypothesis: proposed that all matter has wave properties Glenn Seaborg Hantaro Nagaoka Democritus Marie and Pierre Curie Eugene Goldstein Dmitri Mendeleev His work led to development of the actinide concept & the arrangement of the actinide series. Seaborg was the principal or co-discoverer of ten elements: plutonium, americium, curium, berkelium, californium, einsteinium, fermium, mendelevium, nobelium and element 106 Believed center of atom was highly positively charged mass which established stable electron orbits (developed Saturnian model) Created his own theory: everything is composed of "atoms", which are physically indivisible, there is empty space between atoms, they are indestructible, are constantly & always have been in motion, infinite kind of atoms & number of atoms, which differ in shape and size. Discovery of radioactivity (alongside Antoine Becquerel) & two radiocative elements Developed "The Curie" (a measure of radioactivity) Discovered the anode ray (beam of positive ions that is created by certain types of gas discharge tube) Also discovered the proton. . He formulated the Periodic Law, created a farsighted version of the periodic table of elements, and used it to correct the properties of some already discovered elements. J.J. Thomson Discovered cathode rays of negative particles (which he termed as electrons), developed Plum Pudding model James Chadwick Discovery of neutron Erwin Shrodinger Developed Quantum Field Theory, expanded upon the quantum mechanical model made by Barogilie John Dalton Lothar Meyer Robert Millikan Proposed an atomic theory, the main points of which were: Elements are made of atoms, atoms of an element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties, atoms cannot be subdivided, created, or destroyed. Atoms of different elements combine simple whole-number ratios to form chemical compounds Best known for his part in the periodic classifcation of the elements (or the periodic table), and he worked with Mendeleev & Bunsen Determined the charge of one electron and using the known mass-charge ratio, and was able to calculate the mass in one electron. Discovered photoelectric effect, and conducted the oil drop experiment. J.W. Dobereiner Worked on periodic trends and the periodic law Ernest Rutherford Performed the gold foil experiment - discovered that the mass and positive charge of an atom is in the nucleus. Discovered the concept of radioactive half-life Created the Rutherford model of the atom 43
Page 1 and 2: Chemistry Notebook By: Joel J
Page 3 and 4: Unit 1 Measurement Lab Separation o
Page 5 and 6: Unit 5 (28 days) Chapter 10 Chemica
Page 7 and 8: 30. Always lubricate glassware (tub
Page 10 and 11: Chapter 1 Unit 1 Introduction to Ch
Page 13 and 14: To use the Stair-Step method, find
Page 15 and 16: Using SI Units Match the terms in C
Page 17 and 18: Standards of Measurement Fill in th
Page 19 and 20: SCIENTIFIC NOTATION RULES How to Wr
Page 21 and 22: Convert each number from Scientific
Page 23 and 24: Significant Figures Rules There are
Page 25 and 26: How Many Significant Digits for Eac
Page 27 and 28: The following rule applies for mult
Page 29 and 30: 1qt=32 oz 1gal = 4qts 1.00 qt = 946
Page 31 and 32: Chapter 5 Electrons in Atoms The st
Page 33 and 34: Atoms Are Building Blocks Atoms are
Page 35 and 36: Electrovalence Don't get worried ab
Page 37 and 38: Summary Atoms are essentially the b
Page 39 and 40: Electron Configuration Color the su
Page 41 and 42: Electron Configuration In order to
Page 43: Calcium (Ca) Nickel (Ni) Carbon (C)
Page 47 and 48: Using Wikipedia, define the 8 categ
Page 49 and 50: Ionization Energy Define Ionization
Page 51 and 52: Ion Size Define Ion Size: Ion size
Page 53 and 54: Chapter 7 Ionic and Metallic Bondin
Page 55 and 56: 10. Name __________________________
Page 57 and 58: The Nucleus A typical model of the
Page 59 and 60: Gamma Radiation After a decay react
Page 61 and 62: This analysis shows that sodium has
Page 63 and 64: Metals, with only a few electrons i
Page 65 and 66: POLAR BONDING results when two diff
Page 67 and 68: Step 6 Put the atoms in the structu
Page 69 and 70: Trigonal Planal Molecular Geometry
Page 71 and 72: Tetrahedral Molecular Geometry Orbi
Page 73 and 74: Bent Molecular Geometry Orbital Equ
Page 75 and 76: T-Shaped Molecular Geometry Orbital
Page 77 and 78: Square Planar Molecular Geometry Or
Page 79 and 80: sp 3 d 2 AX6 None 90 Octahedral sp
Page 81 and 82: Chapter 9 Unit 4 Chemical Names and
Page 83 and 84: Learning Goals: Describe the proper
Page 85 and 86: Unit 5 Chapter 10 Chemical Quantiti
Page 87 and 88: www.youtube.com/watch?v=AsqEkF7hcII
Page 89 and 90: Categories of Reactions All chemica
Page 91 and 92: List what type the following reacti
Page 93 and 94: How to Balance Chemical Equations A
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Step 5 Balance the hydrogen atoms n
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6) ___ Mn(NO2)2 + ___ BeCl2 ___ Be
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The Learning Goal for this assignme
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Stoichiometry and Balanced Equation
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Step 1: 200g C3H8 is equal to 4.54
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Stoichiometry and balanced equation
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%yield = 6.1 tons × 100 = 64% 9.6t
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Use the space provided to write out
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Unit 6 Chapter 13 States of Matter
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uniform internal structure, and amo
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Volume Pressure Temperature is Aver
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Volume and temperature (in Kelvins)
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120
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Combined Gas Law: This gas law comb
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Unit 7 Chapter 16 Solutions The stu
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Part 5: Molarity Molarity (M) is th
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The Time-Temperature Graph We are g
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Step Two: solid ice melts Now, we c
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Step Four: liquid water boils Now,
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The following table summarizes the
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The Learning Goal for this section
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B. decreasing the concentration of
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everse reaction rate as well. 11. I
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Unit 8 Chapter 19 Acid and Bases Th
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The Learning Goal for this section
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This would be a generic base: XOH -
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HCl + H2O ⇌ H3O + + Cl¯ HCl - th
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Several categories of substances ca
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1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
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2. What is the oxidation number of
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Table E Selected Polyatomic Ions Fo
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Table H Vapor Pressure of Four Liqu
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Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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