Search found 9 matches
Search found 9 matches • Page 1 of 1
Since we haven't covered some of the practice problems in the workbook for quiz #3 do we still turn it in to our discussion? Even though the problems aren't needed for quiz #3 this week?
- Wed Nov 02, 2016 3:48 am
- Forum: *Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)
- Topic: Which Diagram to draw in a bond with both elements Z<8 and Z>8 [ENDORSED]
- Replies: 8
- Views: 878
I don't know if you mean a bond between an atom with close to eight electrons and an atom with far fewer. I don't see a molecule like CF existing because if it bonded their would be 3 unbonded electrons left on the carbon. otherwise when you're focusing on drawing the lewis structures just pay atten...
- Tue Oct 25, 2016 9:30 pm
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron configuration with noble gas abbrevation
- Replies: 2
- Views: 488
Im pretty sure you use argon because the extra electron gives it the same electron configuration as argon.
- Thu Oct 13, 2016 6:56 pm
- Forum: Properties of Light
- Topic: Practice Quiz 1 Question [ENDORSED]
- Replies: 5
- Views: 790
Unless he specifies, I don't think it matters if you leave it in meters or nanometers. Typically yes the SI unit is meters, but if the question ever asks to compare it to the line spectrum then its easier to compare it when your answer is in nanometers.
- Wed Oct 05, 2016 6:06 pm
- Forum: DeBroglie Equation
- Topic: Wavelength of Ejected Electron [ENDORSED]
- Replies: 3
- Views: 500
You use the De Broglie equation thats lambda = h (planks constant) / p (momentum) because it is used to calculate the wavelength of any object. All matter has wavelike properties but only can be measured if it has a small mass and a high velocity like an electron. So the ejected electron is moving s...
- Tue Sep 27, 2016 4:49 pm
- Forum: Empirical & Molecular Formulas
- Topic: Calculating Molecular and Empirica Formulas
- Replies: 5
- Views: 884
Most of the answers I have encountered in the homework have been close enough to round up or down ( ex: 5.02 or 4.98) but I feel that if its fairly off you may have to multiply to get closer to whole number or maybe you messed up somewhere in your earlier calculations. However if you are doing the p...