chem301 class notes - Erin Marek 9/20/07 1. What type of...

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Unformatted text preview: Erin Marek 9/20/07 1. What type of orbital is represented by these quantum numbers: n = 4, l = 3, m 1 = 2, m s = +1/2 Choices: 2s 3s 4s 5s 2p 3p 4p 5p 2d 3d 4d 5d 2f 3f 4f 5f 2. An orbital has a principal quantum number of 3. The magnetic quantum umber is -1. What shape of orbital could this be? (s, p,d ,or f) Tyndall effect: the degree of scattering of light depends on the wavelength of the photons and the size of the particles. Demo: adding HCl to beakers of water. One turns blue because of the scattering of light in the water. Hs.utexas.edu for homework changes (mostly with off campus places) Pauli Exclusion Principle: no two electrons can have the same set of 4 quantum numbers (1, 0, 0, 1/2 can only be used for one electron) Aufbau principle: describes the electron filling order in atoms. Goes from bottom to top and based on energy raking. The order of orbital levels is : 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p Ions atoms constantly losing and gaining electron because the aspire to be noble gasses. Cl vs. Cl + 17 18 Periodic Properties: Atomic radii Ionization energy Electron affinity Ionic affinity Ionic radii Electronegativity I. Columns (groups)-principal number increases> Orbitals are located further from nucleus avg. distance from nucleus I I. Rows (periods)-positive nuclear charge increases> Greater attractive force on valence electrons effective nuclear charge Atomic radius is the distance between two nuclei between atoms. Ionization energy First ionization enerdy The minimum amount of energy required to remove the most loosely bound electron from an isolated gaseous atom to form a 1+ion Second ionization energy The amount of energy required to remove the second electron from a gaseous 1+ion Which element would be most easily ionized? Indium (In) Furthest out so easiest to remove outer one Electron affinity: amount of energy absorbed when an electron is added to an isolated gaseous atom to form an ion with a -1 charge. Affinity>0 means energy is absorbed (unfavorable) Affinity<0 means energy is released (favorable for adding an electron) 9/25/07 What type of ion would be expected to be favored for each element? Na Na + or Na- F F + or F- What are the electron configurations of the two C isotopes? (login to hs instead of hw) Exam covers CH 3, 12, 13-I Practice exam online Exam practice: Monday 1 st 7-9 Electron affinity: (do not readily acquire an electron on their own, unlike the halogens) Attaching an electron to form an ion Electronegativity: a measure of the relative tendency of an atom to attract electrons to itself when chemically combined with another element Fluorine is the most electronegative Cesium and francium are the least electronegative elements Key property that influences how atoms(bond?) Ionic Radii: Cations are always smaller than their respective neutral atoms Anions are always larger than their neutral atoms Chapter 13 Ionic and covalent bonds Chlorine, oxygen and nitrogen are found in pairs.Chlorine, oxygen and nitrogen are found in pairs....
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This note was uploaded on 06/25/2008 for the course CH 301 taught by Professor Fakhreddine/lyon during the Fall '07 term at University of Texas at Austin.

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chem301 class notes - Erin Marek 9/20/07 1. What type of...

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