CHE_106_Lecture15_2009

CHE_106_Lecture15_2009 - Chemistry 106 Lecture 15 Topic:...

Info iconThis preview shows pages 1–10. Sign up to view the full content.

View Full Document Right Arrow Icon
Chemistry 106 Lecture 15 Topic: Electron Configurations Chapter 6.7-6.9
Background image of page 1

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

View Full DocumentRight Arrow Icon
EXAM 2 The Second Exam will be held on Thursday October 29 at regular class time (3:30-4:50). The Exam will be held in two locations: Life Sciences Building (LSB) Room 001 Students with last names starting with A-F will meet in LSB. Gifford Auditorium (same as lecture) Students with last names starting with G-Z will meet in Gifford.
Background image of page 2
Exam Details Exam #2 will cover Chapters 4, 5, and 6. Primarily based on homework and lecture material. Exam will be multiple choice (25 questions). You need to bring a #2 pencil. You need a calculator. You will be given a copy of the Periodic Table from the textbook. You will be provided with a table of numerical constants.
Background image of page 3

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

View Full DocumentRight Arrow Icon
Quantum Numbers and Atomic Orbitals According to quantum mechanics, each electron is described by four quantum numbers . – Principal quantum number (n) – Angular momentum quantum number ( l ) – Magnetic quantum number (m l ) size shape orientation The first three define the wave function in space for a particular electron. The fourth quantum number refers to the magnetic property of electrons. No two e - can have the same 4 quantum numbers! – Spin quantum number (m s )
Background image of page 4
higher energy even higher energy Energy is released.
Background image of page 5

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

View Full DocumentRight Arrow Icon
Quantum Numbers and Atomic Orbitals l = 0 to ( n - 1) m l = - l to + l This table gives you the relationships among the quantum numbers up to n = 4.
Background image of page 6
The spin quantum number (m s ) refers to the two possible spin orientations of the electrons residing within a given orbital. ch rbital can hold only two electrons Quantum Numbers and Atomic Orbitals Each orbital can hold only two electrons whose spins must oppose one another. – The possible values of m s are +1/2 and –1/2.
Background image of page 7

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

View Full DocumentRight Arrow Icon
Quantum Numbers and Atomic Orbitals l = 0 to ( n - 1) m l = - l to + l # electrons = 2 x #orbitals 2 This table gives you the relationships among the quantum numbers up to n = 4. 8 18 32
Background image of page 8
Electron pairs residing in the same orbital are required to have opposing spins. – This spinning causes electrons to behave like ny bar magnets. tiny bar magnets. – This can be seen experimentally with a single
Background image of page 9

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

View Full DocumentRight Arrow Icon
Image of page 10
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 38

CHE_106_Lecture15_2009 - Chemistry 106 Lecture 15 Topic:...

This preview shows document pages 1 - 10. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online