Chapter 10 1 Jan 13 2010 v2

Chapter 10 1 Jan 13 2010 v2 - Chemistry 1B10W: Professor...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
10-1 Chapter 10: The Shapes of Molecules 10.1 Depicting Molecules and Ions with Lewis Structures 10.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory and Molecular Shape Chemistry 1B10W: Professor Rettig - Chapter 10, Lecture 1, Jan. 13, 2010 Announcements: 1. Chapter 10 ARIS and Recommended Homework is on iLearn now - see Schedule/Homework Assign. ARIS Chapter 9 due Friday, 11 pm; Chapter 10 Due Tuesday Jan. 20, 11 pm. 2. Still about 35 students not registered in ARIS . Also about 30-50 students have NOT yet entered their external ID in ARIS. Get this done! Students Review : Chapters 8,9 - Lewis Dots and Octets, tendency to achieve noble gas electron configuration . Atom sizes, electronegativity trends.
Background image of page 1

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

View Full DocumentRight Arrow Icon
10-2 Figure 9.3 Lewis Electron-Dot Symbols for Elements in Periods 2 and 3 Generalize this to ionic and covalent compounds (Chapter 9). Overall picture: atoms, either free or bound in compounds, tend to achieve a duet of electrons (He, H) or an octet of electrons. The octet is so common in compounds because there are usually one s and three p orbitals* available to fill with electrons. Often electrons are shared and are counted twice. * particularly for non-hydrogen and non-metal atoms; for metals the orbitals usually "empty" to get to filled s, p for the nearest noble gas
Background image of page 2
10-3 Figure 8.25 Main-Group Ions and the Noble Gas Configurations Non metals that are inherently attractive to electrons tend to gain electrons up to the "limit" - beyond which another electron would have to "jump out" to an unstable n+1 orbital Metals lose electrons relatively easily, until the "limit" is reached where another electron would have to come from an n-1 orbital duet, octets
Background image of page 3

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

View Full DocumentRight Arrow Icon
10-4 We “Invent” Convenient Bonding Pictures to Reflect REALITY What is this reality? It is the sum of all experimental measurements that can be done concerning the actual location of atoms in molecules, plus the stability (energy measurements) of molecules, along with the variety of energy changes that can be induced in molecules. A few examples will be given (e.g. equal bond lengths in carbonate ion, actual bond lengths in carbonate ion, bond length patterns in gaseous sulfuric acid, vibrational specta).
Background image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 23

Chapter 10 1 Jan 13 2010 v2 - Chemistry 1B10W: Professor...

This preview shows document pages 1 - 5. Sign up to view the full document.

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