1 / 12

Review sessions Saturday (11/23), 11:00 am, in CP-145 Sunday (11/24), 10:00 am, in CP-145

Review sessions Saturday (11/23), 11:00 am, in CP-145 Sunday (11/24), 10:00 am, in CP-145 Exam Tuesday, 11/26 8:30pm to 10:30pm, AHC3-Room 110 Coverage Chapter 6 6.4 to 6.9 Chapter 7 ALL Chapter 8 ALL Chapter 9 ALL Chapter 10 ALL. Chapter 6

branden-hood
Download Presentation

Review sessions Saturday (11/23), 11:00 am, in CP-145 Sunday (11/24), 10:00 am, in CP-145

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Review sessions Saturday (11/23), 11:00 am, in CP-145 Sunday (11/24), 10:00 am, in CP-145 Exam Tuesday, 11/26 8:30pm to 10:30pm, AHC3-Room 110 Coverage Chapter 6 6.4 to 6.9 Chapter 7 ALL Chapter 8 ALL Chapter 9 ALL Chapter 10 ALL

  2. Chapter 6 Quantum numbers, restrictions, meaning Electron configurations for atoms (long and short method) Filling order for orbitals Pauli principle Aufbau principle Hund’s rule Orbital filling diagrams Anomolous electron configurations (d4, d9)

  3. Quantum Numbers The quantum numbers and their possible values are as follows. Principal quantum number. Determines the energy, the average distance between the electron and the nucleus, and orbital size. Angular momentum quantum number. Determines the shape of the electron cloud (orbital shape - s ( = 0) d ( = 2) p ( = 1) f ( = 3) Magnetic quantum number. Determines the orientation of the orbital. Spin quantum number. Determines the orientation of the electron spin. n = 1, 2, 3, …  = 0, 1, …, (n-1) m  = 0, 1, 2, …,   ms =  1/2

  4. Mnemonic Device For Energy Ordering We may use the following mnemonic device for the order in energy of the orbitals. The order in which the labels are crossed out below is the order of energies. Maximum # electrons 2 (for s orbital), 6 (for set of p orbitals), 10 (for set of d orbitals), etc. 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f … 6s 6p 6d 6f … So 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f ...

  5. Anomalous Electron Configurations The rules we have given for predicting electron configurations for atoms work most of the time. However, there are occasional cases where the actual electron configuration is different from the predicted configuration. Element Predicted Actual Cr (24 e-) [Ar] 4s2 3d4 [Ar] 4s1 3d5 Mo (42 e-) [Kr] 5s2 4d4 [Kr] 5s1 4d5 Cu (29 e-) [Ar] 4s2 3d9 [Ar] 4s1 3d10 Ag (47 e-) [Kr] 5s2 4d9 [Kr] 5s1 4d10

  6. Chapter 7 Electron configurations and common ions for main group elements Electron configurations for cations (period 4 and below) Trends sizes of atoms sizes of ions 1st ionization energy metallic character electronegativity

  7. Chapter 8 Ionic bonding; Lewis structures for ions; trends in lattice energy Covalent bonding – Lewis structures when octet rule is obeyed Polar bonds and polar molecules Resonance structures and formal charge Exceptions to octet rule less than an octet odd number of electrons expanded octet Average bond enthalpy and its use

  8. Chapter 9 VSEPR theory counting electron containing regions electron (cloud) geometry and molecular geometry Common geometries and bond angles Hybrid orbitals and relationship to # electron containing regions Sigma and pi bonds MO theory, bonding and antibonding Mos, bond order, etc.

  9. electron cloud hybridization electron cloud molecular geometry regions geometry (# bonds) 2 sp linear linear (2) 3 sp2 trig. planar trig. planar (3); nonlinear (2) 4 sp3 tetrahedral tetrahedral (4); trig. pyramid (3); nonlinear (2) 5 sp3d trig. bipyramid trig. bipyramid (5); see-saw (4); t-shape (3); linear (2) 6 sp3d2 octahedral octahedral (6); square pyramid (5); square planar (4)

  10. Chapter 10 The ideal gas law and its use (pV = nRT) Dalton’s law of partial pressures (pi = Xi ptotal) Kinetic theory, average speed of molecules (urms = [3RT/M]1/2) van der Waals equation p = nRT - an2 (V – nb) V2

  11. Problems If  = 1 What kind of orbital do you have? What are the possible values for m? Give the electron configuration for the following P, Br, Cu, O2-, Pd2+ From the atoms Mg, Sr, S, Te Which atom is largest? Which atom is smallest? Which atom has the largest 1st ionization energy? Which element is most metallic?

  12. Problems Give Lewis structures, electron geometry, molecular geometry, and hybridization for the following OCS, NH4+, CH3CHO (both C atoms) SF4, XeCl2 A gas sample is a mixture of two gases, Ar and CO2, with XAr = 0.43. The temperature and pressure of the gas are T = 320. K and p = 845. torr. How many grams of argon and how many grams of CO2 are there in 1.000 L of the gas mixture?

More Related