Week 12 notes
Week 12 notes CHEM 120
Popular in College Chemistry I
Popular in Chemistry
This 0 page Class Notes was uploaded by Leslie Pike on Friday November 13, 2015. The Class Notes belongs to CHEM 120 at Western Kentucky University taught by Dr. Darwin Dahl in Summer 2015. Since its upload, it has received 50 views. For similar materials see College Chemistry I in Chemistry at Western Kentucky University.
Reviews for Week 12 notes
Report this Material
What is Karma?
Karma is the currency of StudySoup.
You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!
Date Created: 11/13/15
Chem 120 notes Week 12 Niels Bohr came up with the energy shell model for the atom This is NOT the Rutherford planetary model and the electrons do NOT quotorbitquot the nucleus like planets orbiting the sun Electrons oat around in their set energy levels Light is emitted when an electron jumps from a higher energy level to a lower energy level Light is absorbed when an electron jumps from a lower energy level to a higher energy level The energy of an electron is equal to the negative Rydberg constant Dr Dahl will provide this on exams divided by the quantum number squared The change in energy when an electron changes states is described by the following equation 1 1 AEZRH 2 2 I ll I lf Note THIS IS BACKWARDS from the way these normally work In this case we have INITIAL MINUS FINAL instead of the other way around The Balmer series is when an electron jumps from a higher energy state to n2 Light in the visible spectrum is emitted during this jump The Schrodinger wave equation describes the probability of where an electron will be at any given time Nprincipa quantum number It can be any positive integer It represents the energy level or the shell o L angular momentum quantum number It can be any whole number up to N1 It represents whether the subsheII is s p d or f The s subshell has an angular momentum quantum number of 0 p is 1 d is 2 f is 3 Mmagnetic quantum number It ranges from to 0 to I it can be any integer value between these values It represents the orbital for example px py and pz 0 MS is the spin It can be 12 or 12 The ground state of an atom means that the atom is not an ion it has an equal number of protons and electrons The ground state electron con guration for magnesium is 1522522p63sz This can be abbreviated as Ne3sz because ground state magnesium has a neon core and then an extra 35 subshell When subshells ll one electron is put in each orbital rst Then a second electron is put in each orbital Subshells ll in order of energy level There are exceptions to this rule namely when the d subshell has 4 electrons and when the d subshell has 9 electrons In these cases one of the electrons in the s subshell will go back into that last d orbital A paramagnetic atom has at least 1 unpaired electron A diamagnetic atom has no unpaired electrons Noble gases are diamagnetic as are groundstate aIkaIi earth metals All elements want to achieve noble gas con guration This means that they have all of their shells full When alkali metals exist in the 1 state they have the same con guration as the noble gas right behind them Na has the same electron con guration as Ne When halogens exist in the 1 state they have the same electron con guration as the noble gas in front of them F39 has the same electron con guration as Ne Elements with the same electron con guration are known as isoelectronic Ne Na F39 and 0239 are all isoelectronic
Are you sure you want to buy this material for
You're already Subscribed!
Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'