Molecular Geometry and VSEPR Theory 9/13/10. the properties of molecules depend not only on the bonding of atoms but also on the molecular geometry, or.

Slides:

Advertisements

Similar presentations

Molecular Geometries and Isomers

Advertisements

Molecular Geometry and Bonding Theories. The properties of a molecule depend on its shape and and the nature of its bonds. In this unit, we will discuss.

Molecular Geometry.

1 Chapter 4 Compounds and Their Bonds 4.7 Shapes and Polarity of Molecules Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.

1 Shapes of Molecules Determined by number of valence electrons of the central atom 3-D shape a result of bonded pairs and lone pairs of electrons Use.

General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 5.8 Shapes and Polarity of Molecules Chapter 5 Compounds and Their Bonds © 2013.

Shapes of Molecules Determined by number of valence electrons of the central atom 3-D shape a result of bonded pairs and lone pairs of electrons Use VSEPR.

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

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

Warm-Up: to be turned in Write the electron configuration, noble-gas configuration and orbital notation for: Sulfur and Calcium.

Section 6.5 – Molecular Geometry

Chapter 4 Forces Between Particles

Modern Chemistry Chapter 6 Chemical Bonding

Chemistry 101 : Chap. 9 Molecular Geometry and Bonding Theories (1) Molecular Shape (2) The VSEPR Model (3) Molecular Shape and Molecular Polarity (4)

Molecular Geometry  3-D arrangement of molecules.

HW: Read pages Draw the Lewis structure, write the formula, and indicate the shapes for the following compounds: Silicon tetrabromide Hydrogen.

Molecular Geometry Chapter 6.5.

Section 9-4 Summarize the VSEPR bonding theory.

VSEPR Theory Valence Shell Electron Pair Repulsion.

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.

1 Chapter 4 Compounds and Their Bonds 4.7 Shapes and Polarity of Molecules Copyright © 2009 by Pearson Education, Inc. °

VSEPR Theory Valence Bond Theory Molecular Orbital Theory Molecular Geometry.

Molecular Geometry Chemistry Mrs. Deiseroth. Molecular Geometry the 3-D arrangement of a molecule’s atoms in space the polarity of each bond, along with.

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

Section 3.3 – Part A Pg Objective: 1) Apply VSEPR theory to predict molecular shapes.

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

Chemical Bonding Chapter 6. Molecular Geometry VSEPR Valence – Shell, Electron Pair Repulsion Theory.

Resonance  A molecule or polyatomic ion for which 2 or more dot formulas with the same arrangement of atoms can be drawn is said to exhibit RESONANCE.

Molecular Structure Molecular geometry is the general shape of a molecule or the arrangement of atoms in three dimensional space. Physical and chemical.

Molecular Geometry. Basic Terminology Molecule Group of atoms held together by covalent bonds Bond Length Distance between 2 bonded atoms Bond Energy.

MOLECULAR SHAPES. What is the shape of this gerber daisy? Looks two-dimensional but in reality it is three-dimensional.

MOLECULAR SHAPES. What is the shape of this gerber daisy? Looks two-dimensional but in reality it is three-dimensional.

 Basic Terminology  Molecule  Group of atoms held together by covalent bonds  Bond Length  Distance between 2 bonded atoms  Bond Energy  Energy.

After today, you will be able to… Explain Valence Shell Electron Pair Repulsion Theory (VSEPRT) Use structural formulas to describe the molecular geometry.

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

 Basic Terminology  Molecule  Group of atoms held together by covalent bonds  Bond Length  Distance between 2 bonded atoms  Bond Energy  Energy.

Section 8.13 Molecular Structure: The VSEPR Model VSEPR: Valence Shell Electron-Pair Repulsion. ▪Used to predict a 3-dimensional shape of a molecule ▪Based.

VSEPR Notes & Lab GT Chemistry 12/15/14. Drill Draw Lewis structures for –CH 3 Br –NH 3 –HCl (that’s hydrogen chloride, not carbon/iodine) –AlF 3 HW:

VSEPR Theory Valence Shell Electron Pair Repulsion.

Molecular Geometry VSEPR.

Molecular Geometry VSEPR Theory- “Valence- shell, electron-pair repulsion” states that repulsion between the sets of valence-level electrons surrounding.

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

Molecular Geometry (VSEPR)

Timberlake LecturePLUS

Ch. 6 – Molecular Structure

MOLECULAR GEOMETRY Topic # 18

Ch. 6.5 Bonding Theories Molecular Geometry.

Valence Shell Electron Pair Repulsion

MOLECULAR GEOMETRY Bonding Unit.

II. Molecular Geometry (p. 183 – 187)

Valence Shell Electron Pair Repulsion Theory

Molecular Shapes VSEPR Theory

Ch. 6 – Molecular Structure

Molecular Geometry and VSEPR Theory

Important Information:

Molecular Structure Molecular Geometry.

Molecular Geometry and VSEPR Theory

Molecular Geometry VSEPR Theory

GEOMETRY AND POLARITY OF MOLECULES

Valence Shell Electron Pair Repulsion

Chapter 10 Properties of Solids and Liquids

Molecular Geometry VSEPR Theory- “Valence- shell, electron-pair repulsion” states that repulsion between the sets of valence-level electrons surrounding.

Molecular Geometry 11/8 Opener:

Valence Shell Electron Pair Repulsion Theory

Molecular Structure II. Molecular Geometry.

II. Molecular Geometry (p. 183 – 187)

6.5 VSEPR Theory and Molecular Shapes

Valence Shell Electron Pair Repulsion

II. Molecular Geometry (p. 183 – 187)

II. Molecular Geometry (p. 183 – 187)

Presentation transcript:

Molecular Geometry and VSEPR Theory 9/13/10

the properties of molecules depend not only on the bonding of atoms but also on the molecular geometry, or 3-D arrangement of a molecule’s atoms in space. molecular polarity = the uneven distribution of molecular charge (NOT electrical charge, which refers to the charges within the atoms themselves) the polarity of a molecule determines its chemical and physical properties this is especially important for molecules of liquids and solids, because they are so close together (when compared to the molecules of gases) unfortunately, the chemical formula of a compound does not tell you much about its molecular geometry, so we have a theory to help….

VSEPR (Valence-Shell, Electron-Pair Repulsion) Theory = states that the repulsion between the sets of valence-level electrons in an atom causes these sets of electron pairs to be oriented as far apart as possible in all three dimensions. rules of VSEPR theory: 1.all diatomic (2-atom) molecules Ex: HCl = are “linear” (duh). 2.3-atom molecules can be one of 3 different shapes, depending on the number of unshared pairs the central atom has: a.if it has no unshared pairs, then Ex: BeF 2 = the shape is “linear.” (AB 2 ) angle = 180  b.if it has one unshared pair, then Ex: SnCl 2 = the shape is “angular.” (AB 2 E) angle = 120 

c.if it has two unshared pairs, then Ex: H 2 O = the shape is “bent.” (AB 2 E 2 ) angle = 105  3.4-atom molecules can be one of two different shapes, again, depending on the number of USPs the central atom has: a.if it has no USPs, then the shape Ex: BF 3 = is “trigonal-planar.” (AB 3 ) angle = 120  b.if it has one USP, then the shape Ex: NH 3 = is “trigonal-pyramidal.” (AB 3 E) angle = 107 

c.if it has one USP, then the shape Ex: NH 3 = is “trigonal-pyramidal.” (AB 3 E) angle = 107  3.5-atom molecules can be only one Ex: CH 4 = shape: “tetrahedral.” (AB 4 ) angle =  4.6-atom molecules can be only one Ex: PCl 5 = shape: “trigonal-bipyramidal.” (AB 5 ) angles = 90  on z-axis,120  on x & y-axis 5.7-atom molecules can be only one Ex: SF 6 = shape: “octahedral.” (AB 6 ) angles = 90  on z-axis, 90  on x & y-axis