Chemical Bonding Why? To achieve stability (happiness)  Lower energy level  8 electrons –react so as to achieve the valence level configuration of NEAREST.

Slides:

Advertisements

Similar presentations

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

Advertisements

Unit 04: BONDING IB Topics 4 & 14 Text: Ch 8 (all except sections 4,5 & 8) Ch 9.1 & 9.5 Ch My Name is Bond. Chemical Bond.

VSEPR Theory Geometry of Molecules.

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Modern Chemistry Chapter 6 Chemical Bonding

Chapter 6: Bonding… Chemical Bonding  Describe covalent, ionic and metallic bonds  Classify bond type by electronegative difference  Explain why atoms.

IIIIII Molecular Geometry (p. 232 – 236) Ch. 8 – Molecular Structure.

Molecular Geometry And Polarity.

Monday and Tuesday March 26 and 27. Lewis Dot Structures.

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.

Chapter 8 Covalent Compounds. Covalent Bonds Sharing Electrons –Covalent bonds form when atoms share one or more pairs of electrons nucleus of each atom.

Molecular structure and covalent bonding Chapter 8.

Coulomb Forces: A Simplified View of Bonding

Polarity Chapter 6.1. Review A covalent bond is formed between two non-metals. Electrons are shared. Orbitals are overlapping.

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Unit 6: Chemical Bonding Refer to Ch. 8 & 9 for supplemental reading.

Polarity. Compound Review  Compound: a chemical combination of two or more elements  Why do elements chemically combine?  They want to achieve full.

CMH 121 Luca Preziati Chapter 3: Chemical Bonds Molecule = A group of at least two atoms, linked together by chemical bonds DEF Chemical Bond = An interaction.

Chemical Bonding Chap. 6 What is a bond? a strong attractive force that exists between the e - of certain atoms. 1.

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

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc. Permission required.

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.

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

 no simple, and yet complete, way to define this  forces that hold groups of atoms together and make them function as a unit  a bond will form if the.

IIIIII II. Molecular Geometry Ch. 9 – Molecular Structure.

IIIIII 8.4 and 8.5 Ch. 8 – Molecular Structure. A. VSEPR Theory n Valence Shell Electron Pair Repulsion Theory n Electron pairs orient themselves in order.

Valence Shell Electron Pair Repulsion Theory –Electron pairs orient themselves in order to minimize repulsive forces.

CHM 108 SUROVIEC SPRING 2014 Chapter 10. I. VSEPR Theory A simple model that we can use to look at molecular shapes is the VSEPR (valence shell electron.

Unit 6: Chemical Bonding Refer to Ch. 8 & 9 for supplemental reading.

Bonding Where the magic of chemistry takes place!.

Objectives VESPR Theory Continue with Lewis dot Drawings.

Chapter 9 Molecular Shape.

COVALENT BONDING.

6.8 Shapes and Polarity of Molecules

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Valence Shell Electron Pair Repulsion Theory

7.10 – NOTES Shapes for Covalent Structures

BONDING Unit 6.

VSEPR and Exceptions to the Octet Rule

Drawing Molecules and Shapes

MOLECULAR GEOMETRY Topic # 18

Electron Sharing can be EQUAL or UNEQUAL

3.2 VSEPR Theory. 3.2 VSEPR Theory VSEPR Theory Valence Shell Electron Pair Repulsion Predicts the 3-D geometry of molecules (covalent compounds) The.

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Ch. 6 – Molecular Structure

Molecular Shapes and Hybrid Orbitals

Chemical Bonding Unit 2 Topic 3 Chapter 6.

My Name is Bond. Chemical Bond

GEOMETRY AND POLARITY OF MOLECULES

Drawing Lewis Structures

Drawing Molecules and Shapes

7.7 – NOTES Shapes for Covalent Structures

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.

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.

VSEPR Theory Geometry of Molecules.

Valence Shell Electron Pair Repulsion Theory

Polar Vs. Non Polar Molecule Practice

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.

Drawing Molecules and Shapes

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.

Warm up Draw lewis structures for the compounds below: CF4 BF3 CO2.

Lesson Valence Shell Electron Pair Repulsion Theory (VSEPR)

Drawing Molecules and Shapes

VSEPR Theory Geometry of Molecules.

Polar and Non-polar Covalent Bonds

Presentation transcript:

Chemical Bonding Why? To achieve stability (happiness)  Lower energy level  8 electrons –react so as to achieve the valence level configuration of NEAREST inert gas How? 1. Ionic Bond: ◦Transfer of electrons from Metal (low IE/EN) to non-metal (High IE/EN) ◦Larger difference in IE/EN 2. Covalent Bond:  between NON-metals  b/w items with similar IE/EN (small difference)  Due to SHARING of electrons 

2. Covalent Bond:  between NON-metals  b/w items with similar IE/EN (small difference)  Due to SHARING of electrons * In a given covalent bond each element contributes 1 electron to the pair shared* *BOND FORMATION: due to an overlap of atomic orbitals on the valence level * Identical Bonds: identical in every way, strength, length etc

Go to smartboard.

Bonding cont’d Sigma Bonds: the first bond formed between two atoms - it will use hybrid orbitals Pi Bond ( π bond): the second/third bond formed between two atoms PURE ‘P’ for PI bonds

Go to smartboard

So..... Why do we care??? Knowing # of bonds and # of lone pairs allows us to determine shape of a molecule and then in term helps to determine polarity!! Woot woot

Remember hyperlink on title VSEPR Theory Valence Shell Electron Pair Repulsion Theory  Electron pairs around the atom place themselves AS FAR APART as possible (Bonding or nonbonding lone pairs)  Determines geometry of a molecule based on Lewis structures  Lone pairs on the central atom have basically the same affect as a bonded pair of e -

Electron Pair Geometry 3 e - pairs4 e - pairs 5 e - pairs 6 e - pairs

Variations on Trigonal Planar

seesaw

Polarity – Bonds and Molecules Bond Types: 1. Ionic: transfer of electrons 2. Covalent: equal sharing of e - pair 3. Polar Covalent: unequal sharing of e - pair, creates dipoles (slight charges), determined by Δ EN of the elements

Determining Polarity smartboard

Classify the following as polar or nonpolar A) BeI 2 b) CF 4 c) CH 2 O d) CO 2 e) BF 2 Cl f) CH 3 Cl g) SF 6 h) SCl 2

Intermolecular Forces Two types of forces 1. Intramolecular: within a molecule (ionic/covalent bonds) 2. Intermolecular: between molecules

Wrap up Video Intermolecular Forces

Work: pg. 260 ◦#1)a,b,f 2) a,d 3) b,c 4. a) b) 5) think about it Pg. 264 #9) a,d 11 Pg. 266 #5, 7 – great test questions