Polarity and VSEPR. Covalent Bonding SHARING OF ELECTRONS! Atoms attain an octet (also called noble gas electron configurations) by sharing electrons.

Slides:



Advertisements
Similar presentations
Chemical Bonding and Interactions
Advertisements

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?
Lewis Structures and Chemical Bonds
8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule
Lewis Dot Structures and Molecular Geometry
Structure of molecules Objectives: To understand molecular structure and bond angles To learn to predict molecular geometry from the number of electron.
SHAPES OF MOLECULES. REMINDER ABOUT ELECTRONS  Electrons have negative charges  Negative charges “repel” each other  In molecules, electrons want to.
MOLECULAR GEOMETRY VSEPR ACTIVITY. CARBON DIOXIDE Chemical formula: CO 2 # of atoms bonded to central atom: 2 # of lone pairs on central atom: 0 What.
The Sharing and Transferring of Electrons
Chemical Bonding: The Covalent Bond Model
Chemical Bonding and Molecular Structure Chapter 12 Sec Chapter 12 Sec
POLARITY.
Unit 6 Notes – Part II Mr Nelson Bonding & Lone Pairs Electron pairs that are shared are called bonding pairs Electron pairs that are not bonded.
1 Chemical Bonding 1.Lewis Dot Structures 2.Electronegativity 3.VSEPR 4.Polarity 8 - Copyright © The McGraw-Hill Companies, Inc. Permission required for.
Chapter 5 Compounds and Their Bonds
Chapter 8 – Covalent Bonding Review of Chapter 7 In Chapter 7, we learned about electrons being transferred (“given up” or “stolen away”) This type of.
HW: Read pages Draw the Lewis structure, write the formula, and indicate the shapes for the following compounds: Silicon tetrabromide Hydrogen.
Monday and Tuesday March 26 and 27. Lewis Dot Structures.
Chapter 8 Covalent Bonding. The Covalent Bond Atoms will share electrons in order to form a stable octet. l Covalent bond : the chemical bond that results.
Chapter 6.2 and 6.5 Covalent Compounds.
Chapter 8 Covalent Compounds. Covalent Bonds Sharing Electrons –Covalent bonds form when atoms share one or more pairs of electrons nucleus of each atom.
Unit 7 Molecular Geometry
Covalent Bonding.
Introductory Chemistry: Concepts & Connections Introductory Chemistry: Concepts & Connections 4 th Edition by Charles H. Corwin Chemical Bonding Christopher.
Chapter 16 Covalent Bonding
Lewis Structures Electron-Dot-Diagrams For Molecules.
Chapter 5 Molecular Compounds.
Chapter 4 Covalent Compounds.
Polarity Chapter 6.1. Review A covalent bond is formed between two non-metals. Electrons are shared. Orbitals are overlapping.
Lewis Symbols and the Octet Rule Electron Dot Symbols convenient way of showing the valence electrons of atoms. Consists of the chemical symbol and one.
Chapter 8 – Covalent Bonding
MOLECULAR GEOMETRY Determining the Structure of Molecules.
1 Covalent bonding And hybridization of electrons.
Chemistry 11 Resource: Chang’s Chemistry Chapter 9.
Chapter 6 Chemical Bonding.
Chapter 6 Covalent Compounds. 6.1 Covalent Bonds  Sharing Electrons  Covalent bonds form when atoms share one or more pairs of electrons  nucleus of.
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.
Chapter 6 Chemical Bonding. Bonding Theory and Electronegativity Atoms want to achieve noble gas configuration- 8 valence e- Some elements have stronger.
How are molecules depicted? Ch. 9, sections 3 & 4.
Chemical Bonding. Chemical Bonds A bond is a force that holds groups of two or more atoms together and makes them function as a unit. A bond is a force.
IIIIII II. Molecular Geometry Ch. 9 – Molecular Structure.
COVALENT BONDING. This occurs when two non-metallic atoms _________ electrons in order to obtain the stable number of eight electrons in their outer shells.
Polarity Ch 6.2b. Covalent Bonding  When two nonmetals meet - one atom is NOT strong enough to take electrons from the other!  So they must share them.
1 Chemical Bonds The Formation of Compounds From Atoms Chapter 11 Hein and Arena.
CHAPTER 4 CONCURRENT ENROLLMENT. LEWIS STRUCTURE Elemental symbol represents the nucleus and core electrons Elemental symbol represents the nucleus and.
Polarity Ch 6.2b.  Diatomic compounds share electrons equally.  Equal forces pulling on the shared electrons  What happens when atoms do NOT share.
VSEPR Theory. Molecular Structure Molecular structure – the three- dimensional arrangement of atoms in a molecule.
Bonding GPS 8. Why do atoms bond together? Octet Rule – an atom that has a full outer-most energy level is unreactive (usually it is full with 8 electrons,
Bonding and Structure 1 Chemical Bonding and Molecular Structure Ionic vs. covalent bonding Molecular orbitals and the covalent bond Valence electron Lewis.
Unit 6 – Bond Polarity and Lewis Dots of Molecules Chapter 9.
Ionic, Covalent, and Metallic Bonding
Covalent Bond A chemical bond in which electrons are shared. Each atom has access to a full octet (8 electrons). No electrical charges.
Chapter 9 Molecular Shape.
Chapter 14 Covalent bonding.
6.8 Shapes and Polarity of Molecules
Chapter 6 The Shape of Molecules.
Valence Shell Electron Pair Repulsion Theory
Chemical Bonding Unit 2 Topic 3 Chapter 6.
Drawing Lewis Structures
Chemical Bonds Chemistry Chapter 6.
Although all covalent bonds involve a sharing of one or more pairs of electrons between bonding atoms, most of the time this sharing is not equal. One.
Molecular Structure and Shape
ChemicalBonding Honors Only Problems and questions —
Molecular shapes.
Covalent Bonding …electrons are shared.
Chapter 8 Covalent Bonding.
Lesson Valence Shell Electron Pair Repulsion Theory (VSEPR)
VSEPR Theory Atoms in a molecule try to spread out from one another as much as possible.
Presentation transcript:

Polarity and VSEPR

Covalent Bonding SHARING OF ELECTRONS! Atoms attain an octet (also called noble gas electron configurations) by sharing electrons. EXCEPTION TO OCTET? HYDROGEN – ONLY WANTS 2 ELECTRONS

How the Sharing Happens Hybridization (mixing) of the outer valence electron shells for each atom involved For example: Bonds = overlapping hybrid orbitals

Example: Methane (CH 4 )

Electron Sharing Isn’t Always Equal WHY? ELECTRONEGATIVITY DIFFERENCES! RESULT: Partial positive and partial negative charges

Two Types of Covalent Bonds 1.Polar Covalent -Must indicate charge distribution when drawing -2 acceptable methods: 2.Nonpolar Covalent - Equal or balanced charge distribution

Polar Covalent Bonds Example Species: HCl (Hydrogen Chloride) What periodic trend is involved here? Is the sharing of electrons equal or unequal? Which atom wants electrons more, H or Cl?

Nonpolar Covalent Bonds Example Species: What periodic trend is involved here? Is the sharing of electrons in H 2 equal or unequal?

Which is Which? Bond Energy  Polar bonds generally have higher bond energies (energy necessary to separate the two atoms) than the nonpolar bonds of the parent atoms For example: It takes more energy to separate HF than either H 2 or F 2

Class Questions – Higher Bond Energy? HCl or H 2 NaF or F 2

Thank you, Linus Pauling Pauling has devised a scale for electronegativity based on difference in bond energy SEE THE BACK OF YOUR NOTES HANDOUT for these electronegativity values

Electronegativity Difference Define: ΔEN = Electronegativity Difference = X A – X B X A = Element with higher electronegativity X B = Element with lower electronegativity

What do you think? Which bond type has the greatest electronegativity difference and why?

Predicting the Bond Bond TypeElectronegativity Difference Nonpolar0-0.4 Polar Ionic> 1.7

Practice: YOU DO Calculate the ΔEN for a bond in an H 2 O molecule Classify this bond as nonpolar covalent, polar covalent, or ionic Draw the Lewis dot structure for this molecule Symbolize the partial +/- charges Is H 2 O (the entire molecule) polar? Why/Why Not?

Water is a polar molecule

Molecules: Polar or Not? 2 Factors – Polarity of the individual bonds in the molecule – Shape or geometry of the molecule Pathways to the solution 1. If all bonds are nonpolar, then whole molecule is nonpolar, regardless of its shape 2.If bonds are polar, must look at symmetry of molecule to see if polarity of bonds cancels out

Symmetry or Not?

Example #1: Carbon Disulfide POLAR OR NOT?

Example #2: Nitrogen Trichloride POLAR OR NOT?

Determining Molecular Geometry VSEPR = Valence Shell Electron Pair Repulsion – Assume regions of electron density around atom will be as far apart as possible – Regions of electron density: LONE PAIRS and BOND PAIRS – MULIPLE BONDS count as one bond pair

Electronic Structure (Family) Molecular Structure (Geometry) Areas of e - Density # Of Bonds# Of Lone Pairs Bond Angles Molecular Polarity * **

Determing Molecular Shape: Steps 1.Draw the Lewis Structure 2.Count the number of lone pairs and bond pairs on the central atom 3.Obtain the general shape from the table on your notes handout 4.Alter the shape for repulsion between lone pairs of electrons

Example: IF 3 (Iodine Trifluoride)