1 For ions we must adjust the number of electrons available, A: Add one e - to A for each negative charge Subtract one e - from A for each positive charge.

Slides:

Advertisements

Similar presentations

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 10 Structures of Solids and Liquids 10.2 Shapes of Molecules and Ions (VSEPR Theory)

Advertisements

1 Chapter 10 Molecular Structure: Solids and Liquids 10.3 Shapes of Molecules and Ions (VSEPR Theory) Copyright © 2008 by Pearson Education, Inc. Publishing.

Molecular Geometry 2-2 Ch. 6 – Molecular shape. Molecules are three-dimensional objects that occupy a three- dimensional world; In general, only the smallest.

Ch 6.5 Molecular Geometry.

Chapter 9 Molecular Geometry and Bonding Theories.

Drawing Lewis Structures and VSEPR. Draw basic Lewis dot structures of atoms and compounds. Using VSEPR, predict bond shape from electron arrangement.

Drawing Lewis Structures and VSEPR. Draw basic Lewis dot structures of atoms and compounds. Using VSEPR, predict bond shape from electron arrangement.

1 Oxidation Numbers: Rules 1)The oxidation number of the atoms in any free, uncombined element, is zero 2)The sum of the oxidation numbers of all atoms.

1 VSEPR Theory In any molecule or ion there are regions of high electron density: Bonds (shared electron pairs) Lone pairs (unshared electrons) Due to.

Lewis Structures & VSEPR. Lewis Structure Lewis Structures – shows how the _______________ are arranged among the atoms of a molecule There are rules.

Drawing Lewis Structures and VSEPR A Tutorial on Writing Lewis Dot Structure.

B. Ionic bonding and Structures of Ionic Compounds

+ Bonding Part III Unit 5: Bonding Mrs. Callender VS E P R.

I Chemical Bonding. Chemical Bond  attractive force between atoms or ions that binds them together as a unit  bonds form in order to…  decrease potential.

Shapes of molecules & ions. VSEPR theory VSEPR - the Valence Shell Electron Pair Repulsion theory is used to obtain the shape of simple molecules and.

Geometry of Molecules VSEPR Theory. Valence Shell Electron Pair Repulsion Theory (VSEPR) The geometry of the molecule at any given central atom is determined.

VSEPR Theory Valence Shell Electron Pair Repulsion.

Molecular Shape Section 9.4

Lewis Structures Electron-Dot-Diagrams For Molecules.

Monday, November 5 Take out your “VSEPR Theory” notes and new piece of paper Marshmallow lab tomorrow- Thank you Brianna L and Kristi H for donating supplies.

VSEPR Theory Valence Bond Theory Molecular Orbital Theory Molecular Geometry.

Chapter 8. Two Simple Theories of Covalent Bonding  Valence Shell Electron Pair Repulsion Theory __________ R. J. Gillespie ’s  Valence Bond Theory.

Unit 3: Chemical Bonding

IIIIII Molecular Geometry Molecular Structure. A. VSEPR Theory  Valence Shell Electron Pair Repulsion Theory  Electron pairs orient themselves so that.

IIIIII I. Lewis Diagrams Molecular Structure. A. Octet Rule n Remember…  Most atoms form bonds in order to have 8 valence electrons.

The Shape of Covalent Molecules

Section 8.2 The Nature of Covalent Bonding. The Octet Rule Atoms share electrons so they have a filled valence shell. Atoms share electrons so they have.

Predict the geometry of the molecule from the electrostatic repulsions between the electron (bonding and nonbonding) pairs. Valence shell electron pair.

Cornell Notes (Section 8.4, especially page 263  Topic: Molecular Geometry  Date: 2/7/2012  VSEPR = Valence Shell Electron Pair Repulsion  Valence.

Chemistry Unit 4 Chapter 8.  Molecule  A neutral group of atoms joined together by covalent bonds  Molecular Compound  Tend to have lower melting.

VSEPR Theory Valence Shell Electron Pair Repulsion.

Molecular Geometry and VSEPR Theory

Molecular Geometry Cocaine

Molecular Geometry VSEPR.

CHEMISTRY Matter and Change

Arrangement of Two Electron Pairs on Be

TOPIC: Molecular Geometry (Shapes of Molecules) Essential Question: How do you determine the different shapes of molecules?

Timberlake LecturePLUS

VSEPR and Exceptions to the Octet Rule

Ch. 6 – Molecular Structure

MOLECULAR GEOMETRY Topic # 18

Ch. 6.5 Bonding Theories Molecular Geometry.

Bellwork Monday Draw the following Lewis dot structures. CCl4 NH4+

Valence Shell Electron Pair Repulsion

MOLECULAR GEOMETRY Bonding Unit.

II. Molecular Geometry (p. 183 – 187)

Chapter 6 – 3 Molecular Geometry (p. 214 – 218)

Bonding Unit Part B) Structures and Shapes

Ch. 6 – Molecular Structure

Chapter 8 Section 3 Molecular Structures.

Important Information:

Molecular Structure Molecular Geometry.

Molecular Geometry and VSEPR Theory

Molecular Geometry VSEPR Theory

GEOMETRY AND POLARITY OF MOLECULES

Chapter 10 Molecular Structure: Solids and Liquids

Valence Shell Electron Pair Repulsion

Molecular Geometry 11/8 Opener:

Molecular Structure and Shape

Unit 3: Chemical Bonding

Molecular Structure II. Molecular Geometry.

II. Molecular Geometry (p. 183 – 187)

Molecular Shapes VSEPR Model

Molecular Geometry.

6.5 VSEPR Theory and Molecular Shapes

Valence Shell Electron Pair Repulsion

II. Molecular Geometry (p. 183 – 187)

II. Molecular Geometry (p. 183 – 187)

Polar and Non-polar Covalent Bonds

Valence Shell Electron Pair Repulsion (VSEPR) Theory

Presentation transcript:

1 For ions we must adjust the number of electrons available, A: Add one e - to A for each negative charge Subtract one e - from A for each positive charge The Octet Rule: Examples NH 4 + BF 4 –

2 Example: CO 3 2-

3 Resonance There are three possible structures for CO 3 2- The double bond can be placed in one of three places These are called equivalent resonance structures The real structure of the CO 3 2- anion is an average of these three resonance structures

4 Resonance There are no single or double bonds in CO 3 2- All three bonds are equivalent They are intermediate between the single and double bond

5 Resonance: Other Examples SO 3

6 Resonance: Other Examples NO 3 –

7 Resonance: Other Examples SO 4 2–

8 Exceptions to the Octet Rule In those cases where the octet rule does not apply, the substituents attached to the central atom nearly always attain noble gas configurations The central atom does not have a noble gas configuration but may have fewer than 8 or more than 8 electrons

9 Examples BBr 3 AsF 5

10 Assignments & Reminders Go through the recent lecture notes Read Chapter 7 completely, except for Sections 7-7 & 7-8 Homework #4 due by Oct. 3 p.m. Review 5:15 p.m. on Sunday

11 CHAPTER 8 Molecular Structure & Covalent Bonding Theories

12 Stereochemistry The study of the three-dimensional shapes of molecules With the knowledge acquired so far we will be able to predict the shapes of molecules and ions Our instrument – Valence Shell Electron Pair Repulsion theory (VSEPR theory – R. J. Gillespie)

13 VSEPR Theory In any molecule or ion there are regions of high electron density: Bonds (shared electron pairs) Lone pairs (unshared electrons) Due to electron-electron repulsion, these regions are arranged as far apart as possible Such arrangement results in the minimum energy for the system

14 BeCl 2

15 BBr 3

16 CH 4

17 PCl 5

18 SF 6

19 Five Basic Geometries Linear Trigonal Octahedral Trigonal bipyramidal Tetrahedral

20 SiF 4

21 NH 3

22  Electronic geometry  Distribution of regions of high electron density around the central atom  Molecular geometry  Arrangement of atoms around the central atom Electronic Geometry and Molecular Geometry

23 H2OH2O