Week 2/Tu: Lecture Units 2 & 3
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1 Week 2/Tu: Lecture Units 2 & 3 Unit 1: Introduction -- Course Outline & Rules -- SI units & Dimensions -- Calculations, Accuracy & Precision Unit 2: Atomic Theory & Nomenclature -- States of Matter -- Mixtures, Compounds, Elements -- Periodic Table, first look Unit 3: Atomic Theory -- nuclei, isotopes, nuclear mass -- elemental and masses on Periodic Table -- compounds and their masses GT Seaborg gets his name on Periodic Table
2 Week 2/Tu: Dimensional Analysis What is the value of 3.01*R, where R is the gas constant? = 3.01 * J/K-mol = J/K-mol = 25.0 J/K-mol (proper sig-fig) What is the mass of 1.5 L of water? Facts: density of water = 1.0 g/cm 3 = 1.5 L * 1.0 g/cm 3 * 1000 cm 3 /L = 1500 g = 1.5 kg (proper sig-fig) Gasoline in Windsor, Canada is selling for CA$ / L, what is this in US$ / Gal? Facts: 1 Gal = L, 1 US$ = CA$ = CA$/L * 1 US$/ CA$ * L/Gal = US$/Gal = US$/Gal (proper sig-fig)
3 Week 2/Tu: What are Chemicals? Matter (Pure) Substance physical separation Mixture of Substances Element 81 non-rad chemical separation Compound Homogeneous (Solution) Heterogeneous Mixture Molecular (covalent) Ionic Note difference between Chemical & Physical change Chemical properties: extensive, depend on amount intensive, independent of amount
4 Week 2/Tu: Periodicity of Elements How many kinds of elements are there? Let s look at a collection of the first few, alphabetical list: Name Mass Character Apparent Rxn* Similar Element? (g/mol) in Water in Air Beryllium 9.0 metal none none many Boron 10.8 brown powder none none? Carbon 12 black powder none burns? Fluorine 19 yellow gas violent none Chlorine forms strong acid Hydrogen 1 colorless gas none** vigorous burn? Lithium 7 metal violent corrodes Sodium forms strong base Nitrogen 14 colorless gas none** none? Oxygen 16 colorless gas none** none? Notes: * while you are waiting, ** dissolves
5 Week 2/Tu: Mendeleev s Periodic System Dmitri Mendeleev (1869) gets the credit for creating the first periodic table almost 150 years ago based on his observations of the reactions of the then-known elements with oxygen, hydrogen and their atomic mass. He notably left gaps in his table when necessary for example, Gallium was discovered after this table was published. The chemical symbols, one or two letters based on the name, were already in use. Note that the name need-not be in English!
6 Week 1/Th: What are THE ELEMENTS?
7 Week 2/Tu: Dalton s Atomic Theory About 200 years ago John Dalton (1803) revived the Atomic Theory of Matter with five postulates: 1. All matter is composed of atoms 2. All atoms of a given element are identical 3. Atoms combine in whole number ratios to form compounds 4. Chemical reactions are rearrangements of atoms 5. Atoms are indivisible After all these years and the overall success and power of chemical sciences: only #5 is wrong given that electrons, ions & nuclei exist and #2 is true on average some have 2 or more isotopes
8 Week 2/Tu: Atoms & Nuclei Work by Faraday and others showed that atoms could be separated into positive and negative ions; later Rutherford and his graduate students showed that the centers of atoms were tiny and positively charged and the negative charge was spread out around the center. Atoms ~ 0.1 nm Nuclei ~ 1 fm We now know that atoms of all elements consist of a tiny nucleus with a positive electric charge that is surrounded by a cloud of electrons. The nucleus was later shown to hold two kinds of particles: protons (massive, positive) and neutrons (massive, neutral). The chemical nature is determined by the number of protons.
9 Week 2/Tu: Chemical Symbols We need to specify three items in order to describe an atom completely! number of protons: Z -- chemical element symbol, atomic number number of neutrons: N -- mass number, A = N+Z number of electrons? relatively few ions in nature, write charge state = the number of protons minus number of electrons; omit zero A Z X q N Protons Neutrons Electrons 1 H => 1 1 H0 0 2 H => 2 1 H As 3+ => 75 33As
10 Week 2/Tu: (average) Atomic Mass Note that the mass shown in the Periodic Table is the average value for the isotopes that we have here on earth. The number of isotopes of each element depends on nuclear structure theory beyond this course! Fraction Isotope mass Fluorine, 19 F * Atomic mass = Hydrogen, 1 H * à H * à Atomic mass = in Periodic Table Neon, 20 Ne * à Ne * à Ne * à 2.03 Atomic mass = in Periodic Table
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