Presentation on theme: "Hybridization, Polarity, & Electronegativity"— Presentation transcript:
1Hybridization, Polarity, & Electronegativity Lots of multisyllabic words, I know
2Overlap and BondingWe think of covalent bonds forming through the sharing of electrons by adjacent atoms.In such an approach this can only occur when orbitals on the two atoms overlap.
3HybridizationAtomic orbitals (s, p, d, f) cannot adequately explain the bonding in moleculesConsider CH4 … how do we get the tetrahedral shape out of the above orbitals
4Hybridization Consider beryllium: An averaging of atomic orbitals into a new set of “hybrid orbitals”Consider beryllium:In its ground electronic state, it would not be able to form bonds because it has no singly-occupied orbitals.
5Hybridization Consider beryllium: if it absorbs the small amount of energy needed to promote an electron from the 2s to the 2p orbital, it can form two bonds.
6Hybrid OrbitalsMixing the s and p orbitals yields two degenerate orbitals that are hybrids of the two orbitals.These sp hybrid orbitals have two lobes like a p orbital.One of the lobes is larger and more rounded as is the s orbital.
7Hybrid OrbitalsThese two degenerate orbitals would align themselves 180 from each other.This is consistent with the observed geometry of beryllium compounds: linear.
8Hybrid OrbitalsWith hybrid orbitals the orbital diagram for beryllium would look like this.The sp orbitals are higher in energy than the 1s orbital but lower than the 2p.
9Hybrid Orbitals Think about Boron What’s its electron configuration? How many bonds does it normally form?How?
17Practice ProblemsSpecify the electron-pair and molecular geometry for each underlined atom in the following list. Describe the hybrid orbital set used by this atom in each molecule or ion.BBr3CO2CH2Cl2CO3-2
19Types of Covalent Bonds According to the valence bond theory, bond formation requires that two orbitals on adjacent atoms to overlap….So what about multiple bonds…Draw C2H4Is there room in between the two atoms for two pairs of electrons to share space?NO
20Types of Covalent Bonds Sigma (σ)Formed from the overlap of hybrid orbitals. Electron density along the internuclear axis… between the centers of the atoms…
21Types of Covalent Bonds Pi (π)Formed from the overlap of unhybridized p-orbitals. Electron density is above and below the internuclear axis, between the atomic centers
22Types of Covalent Bonds Draw Aceylene:C2H2In triple bonds, two sp orbitals form a bond between the carbons, and two pairs of p orbitals overlap in fashion to form the two bonds.Or there is always one sigma bond… anything more is a pi bond
23Molecular Orbital Theory ATOMSElectrons inOrbitalss, p, d, f, etcMOLECULESExperimental GeometriesLinear, trigonal planar, tetrahedralMolecular Orbital Theory:Atomic orbitals from all atoms combine to form new orbitals resulting in known geometriesHybridization: Atomic orbitals from single atoms combine to form new orbitals resulting in known geometriesVESPER: Electrons repel; moleular shapes result.
24Molecular Orbital Theory Molecular orbitals are formed by combinations of atomic orbitals from different atoms.There are bonding and antibonding orbitalsWithout significant electrons density between them, the nuclei will repel each other… creating antibonding orbitals
25Molecular Orbital Theory First Principle of MO Theorythe total number of molecular orbitals is always equal to the total number of atomic orbitals contributed by the atoms that have combined.Second Principle of MO TheoryThe bonding molecular orbital is lower in energy than the parent orbitals, and the antibonding orbital is higher in energy
26Molecular Orbital Theory Third Principle of MO TheoryElectrons of the molecule are assigned to orbitals of successively higher energyFourth Principle of MO TheoryAtomic orbitals combine to form molecular orbitals most effectively when the atomic orbitals are of similar energy
27Molecular Orbital Theory # of molecular orbitals = # of atomic orbitalsEqual # of bonding and antibonding orbitalsAntibonding orbitals ALWAYS higher in energy than its BONDING COUNTERPARTBasically, it means that these guys will fill in from the bottom up… from lower energy to higher energy…
28Molecular Orbital Theory Can use this to calcualte bond orderBond Order = ½ [(# e- in bonding orbitals) – (# of e- in antibonding orbitals)]What is the bond order of Ne2+?Bond order = (8-7)/2 = ½