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Chapter 8 Shape of molecules
VSEPR- Stands for: Valence-shell electron pair repulsion theory. States that pairs of valence e- arrange as far apart as possible.
Ball-and-stick models- 3D physical model –ball = atom –Sticks/spring = single bonds –curved springs/more then one spring = multiple bonds.
Bond angle- The geometric angle between 2 adjacent bonds in a molecule.
Drawing 3D Single Double Triple Lone Pairs
Common Shapes: –Linear -atoms connect in a straight line. –Lewis Dot Diagram:
Common Shapes: –Bent molecules have a lone pair Involves O or S Lewis Dot Diagram: 104.5°
Common Shapes: –Trigonal planar- triangular and flat shape. Involves B or Al –Lewis Dot Diagram:
Common Shapes: –Tetrahedral –3 sided pyramid w/ four surfaces. Involves C or Si –Lewis Dot Diagram:
Common Shapes: –Pyramidal -central atom bonded to 3 other atoms and has an unshared pair of valence e- Involves N or P –Lewis Dot Diagram: 107.5°
All geometries in book w/ names and angles – section 8-1 Linear Tetrahedral Trigonal planar Pyramidal Bent 104.5° 107.5°
Bond length- Down a group bonds lengthen Multiple bonds (double/triple) are shorter than single. Skagen’s HomepageChemistry Resources1 st slide
Chapter 8 Shape of molecules
8-2 Polarity Dipole- One side of a molecule has a negative charge and the other side has a positive charge Polarity- Is determined by the shape of a molecule and polarity of its bonds
Polar Non symmetrical Pyramidal and Bent are always polar - other shapes can be as well Symmetrical Linear, trigonal planer, and tetrahedral are possible non polar molecules Non-Polar
Non-symmetric, Polar Symmetric, Non-polar
If the molecule is: Covalent The bonds are polar. If the shape is Non-symmetric Symmetric The molecule is polar The molecule is non- polar Ionic or two of the same element
Chapter 9 Notes – Part III Mr Nelson Polarity But just because a molecule possesses polar bonds does not mean the molecule as a whole will be polar.
MOLECULAR SHAPE HOW DOES SHAPE AND POLARITY DETERMINE FUNCTION AND PROPERTIES OF MOLECULES?
Molecular Shape VSEPR (Valence Shell Electron Pair Repulsion) Theory.
Valence Shell Electron Pair Repulsion Theory Based on electrostatic “like repels like” – electrons repel other electrons So Electron pairs (both shared.
X. VSEPR Theory – Valence Shell Electron Pair Repulsion theory. [Remember: Like charges repel!] Valence Shell Electron Pair Repulsion theory. [Remember:
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. REMINDER ABOUT ELECTRONS Electrons have negative charges Negative charges “repel” each other In molecules, electrons want to.
Basic Chemistry Copyright © 2011 Pearson Education, Inc. 1 Chapter 10 Structures of Solids and Liquids 10.2 Shapes of Molecules and Ions (VSEPR Theory)
1,000,0001,000,000 500,000500,000 250,000250,000 125,000125,000 64,00064,000 32,00032,000 16,00016,000 8,0008,000 4,0004,000 2,0002,000.
Molecular shapes Balls and sticks. Learning objectives Apply VSEPR to predict electronic geometry and shapes of simple molecules.
- Lewis structures and bonds - bonding theories
Molecular Shapes Chapter 6 Section 3. Molecular Structure It mean the 3-D arrangement of atoms in a molecule Lewis dot structures show how atoms are bonded.
Polar vs. Non Polar Molecules. Covalent/Molecular Compounds All molecular compounds are either polar or nonpolar.
Chemistry 20 - Chapter Molecular Shapes. VSEPR Theory VSEPR stands for Valence Shell Electron Pair Repulsion. VSEPR stands for Valence Shell Electron.
Chem. 1-2 Chapter 8 Molecular Shape. Formulas Molecular Formula: –Specifies how many atoms are in a single molecule of a compound: –Ex. Glucose is C 6.
Monday and Tuesday March 26 and 27. Lewis Dot Structures.
VSEPR Theory Valence Shell Electron Pair Repulsion.
Polarity Chapter 6.1. Review A covalent bond is formed between two non-metals. Electrons are shared. Orbitals are overlapping.
Chapter 8 Molecular Shape The shape of a molecule can be important in determining its chemical reactions Molecular shape is often very important in the.
Molecular Geometry. 2-D and 3-D Lewis Structures explain the two dimensional structure of molecules In order to model the actual structure of a molecule.
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