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.

Slides:

Advertisements

Similar presentations

How is VSEPR theory used to predict molecular structure?

Advertisements

Valence Shell Electron Pair Repulsion Theory Based on electrostatic “like repels like” – electrons repel other electrons So Electron pairs (both shared.

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 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.

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.

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

HONORS REVIEW.  What are valence electrons?  What are valence electrons Electrons in the outermost energy level.

The Nature of Covalent Bonding

- 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.

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.

VSEPR Valence Shell Electron Pair Repulsion Theory Predicting Molecular geometry or molecular shapes.

Covalent Bonds. Gases, liquids, or solids (made of molecules) Low melting and boiling points Poor electrical conductors in all phases Many soluble in.

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

Unit 7 Lewis Structures and VSEPR. Lewis Structures Show the valence electrons and bonds for a compound. 1. Draw the electron dot for each element.

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

MOLECULAR GEOMETRY AND POLARITY

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.

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

Honors Chemistry Lewis Structures and VSEPR Theory.

Section 12.3 Lewis Structures 1.To predict the electron arrangement in molecules 2.To learn to write simple Lewis structures 3.To learn to write Lewis.

Chapter 16 Covalent Bonding

Lewis Structures Electron-Dot-Diagrams For Molecules.

Chapter 4 Covalent Compounds.

Molecular Shape and Polarity The Importance of Geometry in Determining Physical Properties.

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

Lewis Structures & Molecular Geometries. Why Compounds Form Nobel gases do not form bonds because they have completely filled energy levels and do not.

Objectives  I can draw simple Lewis structures of molecules.

AP Chapter 7 Covalent Bonding Lewis Structures A Lewis structure shows the distribution of outer (valence) electrons in an atom, molecule, or polyatomic.

Molecular Shape and Polarity The Importance of Geometry in Determining Physical Properties.

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

Covalent Compounds Chapter Covalent Bonds. Covalent Bond The sharing of electrons between atoms Forms a molecule To have stable (filled) orbitals.

CHAPTER 4 Covalent Molecules General, Organic, & Biological Chemistry Janice Gorzynski Smith.

Review Double and Triple Bonds

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.

IIIIII I. Lewis Diagrams (p ) Ch. 6 – Molecular Structure.

Lewis Structures & VSEPR Meyer Lewis Structures Lewis Structure – Picture of a molecule – Uses lines to indicate chemical bonds – Uses dots to indicate.

Section 8.3 Bonding Theories. VSEPR Theory Electron dot structures fail to reflect the three dimensional shapes of the molecules. VSEPR Valence Shell.

VSEPR THEORY Chemistry. Polyatomic Ions  Ions that are composed of covalently bound atoms.  Add or subtract electrons for charge when finding total.

Molecular Geometry Ms. Murphy Chemistry Newington High School.

Covalent Compounds. Resonance Resonance structures are those that occur when it is possible to draw two or more valid electron dot structures that have.

Section 12.3 Lewis Structures 1.To learn to write Lewis structures 2.To learn to write Lewis structures for molecules with multiple bonds Objectives.

Objectives VESPR Theory Continue with Lewis dot Drawings.

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.

Nature of Covalent Bonding Part 1: Single Covalent Bonds.

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

Chapter 9 Molecular Shape.

Section 4: Molecular Shapes

CHEMISTRY Matter and Change

VSEPR Theory Valence Shell Electron Pair Repulsion

Ch. 8-3 I Bonding Theories Covalent Bonding.

Ch. 6.5 Bonding Theories Molecular Geometry.

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

Valence Shell Electron Pair Repulsion

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

Chapter 8 Section 3 Molecular Structures.

Chapter 10 Molecular Structure: Solids and Liquids

Drawing Molecules and Shapes

Chapter 10 Properties of Solids and Liquids

Molecular Structure and Shape

Valence Shell Electron Pair Repulsion

Molecular Shapes It mean the 3-D arrangement of atoms in a molecule

Molecular Geometry.

Shapes of Covalent Molecules

Valence Shell Electron Pair Repulsion

Drawing Molecules and Shapes

Presentation transcript:

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 a filled valence shell. Most want 8 electrons in the outer shell- like the noble gases. Most want 8 electrons in the outer shell- like the noble gases. Hydrogen and Helium are exceptions! Hydrogen and Helium are exceptions!

Who is likely to form covalent bonds? Non-metallic atoms in Groups 4A, 5A, 6A, and 7A Non-metallic atoms in Groups 4A, 5A, 6A, and 7A

Types of Covalent Bonds Single Single Double Double Triple Triple

Single Covalent Bonds Formed when a pair of electrons (two total electrons) are shared between atoms. Formed when a pair of electrons (two total electrons) are shared between atoms. Showed by two dots in an electron dot diagram Showed by two dots in an electron dot diagram Showed by a dash in a structural diagram Showed by a dash in a structural diagram

Unshared electron pairs Indicated by dots Indicated by dots Also called lone pairs or non-bonding pairs Also called lone pairs or non-bonding pairs

Double and Triple Covalent Bonds A double bond is formed when two electron pairs are shared between atoms. A double bond is formed when two electron pairs are shared between atoms. A triple bond is formed when three electron pairs are shared between atoms. A triple bond is formed when three electron pairs are shared between atoms.

Why do polyatomic ions have a charge? If the charge on a polyatomic ion is negative, there are extra electrons added to the valence electrons: If the charge on a polyatomic ion is negative, there are extra electrons added to the valence electrons:

Resonance A way to envision bonding in certain molecules. A way to envision bonding in certain molecules. A resonance structure: one that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion. A resonance structure: one that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion.

Ozone: Example of Resonance

VSEPR Theory Molecules are three dimensional Molecules are three dimensional VESPR Theory accounts for this VESPR Theory accounts for this Stands for: Stands for: Valence Shell Electron Pair Repulsion

VSEPR Continued This theory states that unshared electron pairs push away from each other so they stay as far away from each other as possible. This theory states that unshared electron pairs push away from each other so they stay as far away from each other as possible. The result: the bonds “bend” to form angles with the central atom and give molecules three-dimensional shapes The result: the bonds “bend” to form angles with the central atom and give molecules three-dimensional shapes

# atoms ShapeAngleExample 2Lineardiatomic 180º N2N2N2N2 3Lineartriatomic CO 2 3Benttriatomic 105º H2OH2OH2OH2O 4TrigonalPlanar 120 ⁰ AlCl 3 4Pyramidal 107º NH 3 5Tetrahedral 109.5º CH 4