CHAPTER 9 Covalent Bonding
What You Will Learn… The nature of the covalent bond How to name covalently bonded groups of atoms Shapes of molecules Characteristics of covalent molecules How to compare and contrast polar and nonpolar molecules
Why It Is Important Most compounds are covalently bonded Including those in living organisms
Assignment Write out Chapter 9 vocabulary words and their definitions 14 words on page 271 PLUS the octet rule from Chapter 6
The Covalent Bond Section 9.1
Objectives Apply the octet rule to atoms that bond covalently Describe the formation of single, double, and triple covalent bonds Compare and contrast sigma and pi bonds Relate the strengths of covalent bonds to bond length and bond dissociation energy
Key Terms Covalent bond Molecule Lewis structure Sigma bond Pi bond Endothermic Exothermic
Review Do noble gases bond? Why or why not? What is an ionic bond? Fill in the blank: In an ionic bond, electrons are_________from one ion to another.
What if both atoms need valence electrons?
Sharing Electrons Another way atoms acquire noble gas configurations Occurs when BOTH atoms want to gain valence electrons
What is the Octet Rule from Chapter 6?
Covalent Bond Bond that results from sharing valence electrons Shared electrons become part of BOTH atoms’ outer energy level Most between NONMETALS
Covalent vs Ionic
Molecule Formed when two or more atoms bond covalently Covalent bonds are often called molecular bonds
Diatomic Molecules Two atoms of the same element form a bond Attractive forces = Repulsive forces Examples: H 2 O 2 N 2 Halogens: F 2, Cl 2, Br 2, I 2
Diatomic Fluorine Each Fluorine has 3 lone pairs and 1 shared pair of electrons
Single Covalent Bond 2 electrons (or 1 pair) are shared between two atoms
Single Covalent Bond
Lewis Structure Electron-dot diagrams for molecules Dots represent lone pairs of electrons A line represents shared electrons
Lewis Structures H-H H ö: H
Lewis Structures Group 7A Elements 7 valence electrons, need 1 more, form one single bond
Lewis Structures Group 6A Elements 6 valence electrons, need 2 more, form 2 single bonds
Lewis Structures Group 5A Elements 5 valence electrons, need 3 more, form 3 single bonds
Lewis Structures Group 4A Elements 4 valence electrons, need 4 more, form 4 single bonds
Practice Problems
Practice Problem Section 9.1 #1 on page 874
Sigma Bond Another name for single covalent bonds Electron pair is shared in the area centered between atoms Valence orbitals overlap end to end s and s; s and p; p and p
Multiple Covalent Bonds Atoms form noble gas configuration by sharing more than one pair or electrons between 2 atoms C, N, O, S
Double Bond 2 pairs (or 4 electrons) of electrons are shared
Triple Bond 3 pairs (or 6 electrons) of electrons are shared
Pi Bond Formed when parallel orbits overlap to share electrons Shared par occupies the space above and below the line that represents where the 2 atoms join together
Multiple Bonds 1 sigma bond At least 1 pi bond
Double Bond 1 sigma bond 1 pi bond
Triple Bond One sigma bond Two pi bonds
Pi and Sigma
Strength of Covalent Bond Distance between nuclei Bond length= distance at maximum attraction Bond dissociation energy= energy required to break bonds
Exothermic Reaction More energy is released forming new bonds than is required to break bonds in the initial reactants
Endothermic Reaction Greater amount of energy is required to break the existing bonds in the reactants than is released when the new bonds form in the products
QUESTIONS?
Homework 6-12 on page 247 Bonding Problems