Where ? Because we are planetary creatures‚ when most people think about space colonization they usually envision homes on Mars or perhaps Earth’s moon. Colonization of those bodies is in fact much less desirable than orbital colonization‚ even though Mars and the Moon are the only practical solid bodies suitable for colonization in the solar system‚ at least for the next few centuries. Venus is far too hot. Mercury experiences extreme temperatures‚ as the days and nights are so long. Jupiter‚ Saturn
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Transition Metals 1a) The d-orbitals of a free transition metal atom or ion are degenerate (all have the same energy.) However‚ when transition metals form coordination complexes‚ the d-orbitals of the metal interact with the electron cloud of the ligands in such a manner that the d-orbitals become non-degenerate (not all having the same energy.) The way in which the orbitals are split into different energy levels is dependent on the geometry of the complex. Crystal field theory can be used to predict
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gases have full orbitals‚ so it is difficult to remove an electron from them. But‚ it does become easier the further away the electrons get from the nucleus. Ionization Energy of Alkali Metals • Alkali Metals only have one valence electron‚ so it does not take much effort to remove that one electron. • When it is removed‚ they achieve Noble Gas Configuration. Dips in Ionization Energy • There are dips at Group 2 and Group 15. • Group 2 is because it has a full s- orbital and thus has
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the same column have similar electronic and chemical properties. An s orbital has a sphere of electron density and is lower in energy than the other orbitals of the same shell. A p orbital has a dumbbell shape and contains a node of electron density at the nucleus. It is higher in energy than an s orbital. C H EM 301A - O rganic Chem istry L ecture N otes © Dr. Peter de Lijser‚ 2011 Since there is only one orbital in the first shell‚ and each shell can hold a maximum
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A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electromagnetic force attraction between opposite charges‚ either between electrons and nuclei‚ or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are "strong bonds" such as covalent or ionic bonds and "weak bonds" such as dipole-dipole interactions‚ the London dispersion force and hydrogen bonding
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of electromagnetic radiation and Planck’s quantum theory; • explain the photoelectric effect and describe features of atomic spectra; • state the de Broglie relation and Heisenberg uncertainty principle; • define an atomic orbital in terms of quantum numbers; • state aufbau principle‚ Pauli exclusion principle and Hund’s rule of maximum multiplicity; • write the electronic configurations of atoms. 26 The existence of atoms has been proposed since the time
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radiation can even produce a population inversion‚ where N2>N1 Fluorescence & Phosphorescence : a “forbidden” slow process (possible only because of spin-orbit coupling) : milliseconds to hours : picoseconds to milliseconds Molecular Orbital Diagrams for CO Particle-in-a-box model for conjugated molecules Ethylene Butadiene Octatetraene • Energy levels for a particle in a (1-D) box: En α n2/mL2 – where n is the quantum number‚ – m is the mass of the particle‚ – and L
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Electrons – Negative (-1)‚ found in orbitals‚ same number as protons Atomic Nucleus: Center of atom where protons and neutrons are confined‚ entire atom has no electric charge Orbitals: - Areas in which the probability of finding an electron is high - “S” orbitals are spherical - “P” orbitals are propeller or dumbbell shaped - Each orbital can only hold 2 electrons o Atoms with more then 2 electrons will have more then one orbital o Orbitals occupy energy shells that are associated
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Chemical bond From Wikipedia‚ the free encyclopedia A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges‚ either between electrons and nuclei‚ or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are "strong bonds" such ascovalent or ionic bonds and "weak bonds" such as dipole–dipole interactions
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Block elements are collectively known as Transition Elements because properties of these elements vary in between s-Block and p-Block elements. A transition element should have partially filled (n-1) d orbital. Group 12 elements i.e. Zn‚ Cd‚ Hg have completely filled (n-1) d-orbital in atomic & ionic state & thus these elements are considered as Typical Transition Elements. All these elements are metals. They are less electropositive than s-block elements & more electropositive than
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