Part J Electronic Configuration, Periodic Table and periodic trends 4 slides per page

Part J Electronic Configuration, Periodic Table and periodic trends 4 slides per page

Info icon This preview shows pages 1–4. Sign up to view the full content.

View Full Document Right Arrow Icon
1/28/2014 1 Electronic Configuration, Periodic Table, and Chemical Periodicity Hydrogen Atoms under Magnification: Direct Observation of the Nodal Structure of Stark States Stodona et al. Phys. Rev. Lett. 110, 213001 (2013) Properties of Atomic Orbitals and Electrons DEGENERATE orbitals – Orbitals that have the same energies ; only p, d, and f have degenerate orbitals s has 0, p has 3, d has 5 and f has 7 GROUND STATE atom– all of its electrons are present in their respective orbitals (with the specific energy level) EXCITED STATE atom– one or more electrons absorb energy and are promoted on the next empty orbital VALENCE ELECTRONS– the electrons at the outermost orbitals . These electrons are responsible for the CHEMICAL CHARACTERISTICS of a given element. Properties of Atomic Orbitals
Image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
1/28/2014 2 PARAMAGNETIC Atoms with unpaired electrons are called paramagnetic . Paramagnetic atoms are attracted to a magnetic field (Unpaired electrons have their spins aligned or ) DIAMAGNETIC Atoms with paired electrons are called diamagnetic . Diamagnetic atoms are repelled by a magnet. (Paired electrons have their spins unaligned ↓↑ ) Paired electrons have no net magnetic field How do you place electrons in an orbital? - Maximum of 2 electrons per orbital - Place them SINGLY FIRST BEFORE PAIRING (Hund’s Rule) - Ex. Placeelectrons in o 1s -___ o 2p -___ ___ ___ o 3d-___ ___ ___ ___ ___ z y x p p p 2 2 2 z y x xz yz xy d d d d d 1s 2 2p 6 3d 10 How do we arrange electron orbitals in an atom? - According to increasing energy! - ↑ n value, ↑energy! - The arrangement of orbitals is based on calculated energies from Hψ= Eψ Aufbau Principle Orbitals are arranged by INCREASING ENERGY Describes how the periodic chart is a function of electronic configurations 4s lower than 3d! AufbauPrinciple and Electron Configurations f 7 f 6 f 5 4f d 7 d 6 d 5 4d 3d p 7 p 6 p 5 4p 3p 2p s 7 s 6 5s 4s 3s 2s s 1
Image of page 2
1/28/2014 3 Writing Electronic Configurations Hund’s Rule –in filling-up orbitals, electrons must occupy them singly first before pairing Pauli’s Exclusion Principle –no two electrons should
Image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 4
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

What students are saying

  • Left Quote Icon

    As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

    Student Picture

    Kiran Temple University Fox School of Business ‘17, Course Hero Intern

  • Left Quote Icon

    I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

    Student Picture

    Dana University of Pennsylvania ‘17, Course Hero Intern

  • Left Quote Icon

    The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

    Student Picture

    Jill Tulane University ‘16, Course Hero Intern