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GENERAL CHEMISTRY AND INORGANIC CHEMISTRY Dr BÙI THỊ BỬU HUÊ College of Natural Science Chapter ATOMIC STRUCTURE AND THE PERIODIC TABLE Chapter CHEMICAL BONDS AND MOLECULAR STRUCTURE Chapter CHEMICAL THERMODYNAMICS Chapter CHEMICAL KINETICS Chapter CHEMICAL EQUILIBRIUM Chapter SOLUTIONS Chapter ACIDS AND BASES Chapter CHEMISTRY OF METALS Chapter CHEMISTRY OF NONMETALS Chapter 10 TRANSITION METALS AND COMPLEXES References Brady and Holum, 1996, Chemistry: the Study of Matter and its Changes, 2th Ed., John Wiley & Sons Inc New York Umland, Jean B., 1993, General Chemistry, West publishing company Zumdahl, Steven S., 1995, Chemical Principal, 2th Ed DC Health & company Toronto http://www.chemistry.msu.edu/Courses/ http://antoine.frostburg.edu http://chemed.chem.purdue.edu http://www.chem1.com/chemed/genchem.html http://www.cbu.edu/~mcondren/lectures.htm http://ull.chemistry.uakron.edu/GenChem/index.html Chapter ATOMIC STRUCTURE AND THE PERIODIC TABLE  Understand atomic structure of an atom including its mass number, isotopes and orbitals  Know how to account for the structure of the periodic table of the elements based on the modern theory of atomic structure  Understand general trends of several important atomic properties FUNDAMENTAL PARTICLES An atom is composed of three types of subatomic particles: the proton, neutron, and electron Particle Mass (g) Charge Proton 1.6727 x 10 -24 +1 Neutron 1.6750 x 10 -24 Electron 9.110 x 10 -28 -1 Atomic Structure Atoms consist of very small, very dense positively charged nuclei surrounded by clouds of electrons at relatively great distances from the nuclei Nuclide Symbol Mass number = number of protons + number of neutrons = atomic number + neutron number ISOTOPES Isotopes are atoms of the same element with different masses; they are atoms containing the same number of protons but different numbers of neutrons The three isotopes of Hydrogen amu = 1.660 x 10-24 g Particle Mass (g) Charge Proton 1.6727 x 10 -24 +1 Neutron 1.6750 x 10 -24 Electron 9.110 x 10 -28 -1 THE ATOMIC WEIGHT SCALE AND ATOMIC WEIGHTS  The atomic weight scale is based on the mass of the carbon-12 isotope  One amu is exactly 1/12 of the mass of a carbon-12 atom: g = 6.022 x 1023 amu or amu = 1.660 x 10-24 g 10 Atomic Radius decrease left to right across a period Zeff = Z - S where: Zeff = effective nuclear charge Z = nuclear charge, atomic number S = shielding constant 73 Atomic Radius  Increase top to bottom down a group  Increases from upper right corner to the lower left corner 74 Atomic Radius 75 Atomic Radius vs Atomic Number 76 Ionic Radii 77 Ionic Radii • Same trends as for atomic radius 78 Comparison of Atomic and Ionic Radii  Positive ions smaller than atom  Negative ions larger than atom 79 Ionic Radii Isoelectronic Series • series of negative ions, noble gas atom, and positive ions with the same electronic confiuration • size decreases as “positive charge” of the nucleus increases 80 Ionization Energy • energy necessary to remove an electron to form a positive ion • low value for metals, electrons easily removed • high value for non-metals, electrons difficult to remove • increases from lower left corner of periodic table to the upper right corner 81 Ionization Energy first ionization energy Energy to remove first electron from an atom second ionization energy Energy to remove second electron from a +1 ion, etc 82 Ionization Energy vs Atomic Number 83 Electron Affinity • Energy released when an electron is added to an atom • Same trends as ionization energy, increases from lower left corner to the upper right corner • Metals have low “EA” • Nonmetals have high “EA” 84 Magnetism • Result of the spin of electrons • Diamagnetism: no unpaired electrons • Paramagnetism: one or more unpaired electrons 85 86 87 [...]... colors 12 13 Electromagnetic Radiation νλ= c Where: ν: frequency λ: wavelength c: speed of light c = 2.99 x 10 8 m/s 14 Electromagnetic Radiation 15 Photons The quantum of electromagnetic energy, generally regarded as a discrete particle having zero mass, no electric charge, and an indefinitely long lifetime E = hν = hc/λ h = Planck's constant = 6.626 × 10 −34 J.s 16 17 18 Electromagnetic Spectrum 19 Dispersion... SPECTRA 21 ATOMIC SPECTRA 22 Bohr Model In 19 13, Niels Bohr (18 85 19 62):  The electronic energy is quantized: only certain values of electronic energy are possible  The electrons absorb or emit energy in discrete amounts as they move from one orbit to another 23 Bohr Model 24 Bohr Model for Hydrogen Atom  Allowed orbits: mvr = nh/2π r = n2a0 a0 = 5.292 x 10 11 m = 0.5292 Å n = quantum number = 1, 2,...THE ATOMIC WEIGHT SCALE AND ATOMIC WEIGHTS Atomic weight = 0.7899 (23.98504 amu) + 0 .10 00 (24.98584 amu) + 0 .11 01 (25.98259 amu) = 18 .946 amu + 2.4986 amu + 2.8607 amu = 24.30 amu 11 ELECTRONIC STRUCTURES OF ATOMS  Why do different elements have such different chemical and physical properties?  Why does chemical bonding occur at all?... an energy level higher than the ground state 27 Electron Transition in a Hydrogen Atom Lyman series → ultraviolet n >1 n =1 Balmer series → visible light n>2→n=2 Paschen series → infrared n>3→ n=3 28 29 30 Quantum Mechanics Theory of the structure and behavior of atoms and molecules 31 32 33 34 35 36 ... The three isotopes of Hydrogen amu = 1. 660 x 10 -24 g Particle Mass (g) Charge Proton 1. 6727 x 10 -24 +1 Neutron 1. 6750 x 10 -24 Electron 9 .11 0 x 10 -28 -1 THE ATOMIC WEIGHT SCALE AND ATOMIC WEIGHTS... constant = 6.626 × 10 −34 J.s 16 17 18 Electromagnetic Spectrum 19 Dispersion of White Light 20 EMISSION & ABSORPTION SPECTRA 21 ATOMIC SPECTRA 22 Bohr Model In 19 13, Niels Bohr (18 85 19 62):  The electronic... proton, neutron, and electron Particle Mass (g) Charge Proton 1. 6727 x 10 -24 +1 Neutron 1. 6750 x 10 -24 Electron 9 .11 0 x 10 -28 -1 Atomic Structure Atoms consist of very small, very dense positively