Covalent Bonding The joining of two or more elements through the sharing of valance electrons to form a molecule Purpose: To form a stable octet between.

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Presentation transcript:

Covalent Bonding The joining of two or more elements through the sharing of valance electrons to form a molecule Purpose: To form a stable octet between the elements

Types of Covalent Bonds Non-Polar: equal sharing of the valance electrons. Polar: unequal sharing of the valance electrons.

Non-Polar Shape of molecule is symmetrical. Homonuclear molecules. Diatomic molecules: N2, O2, F2, Cl2, Br2, I2, and H2 Makes the #7

Polar Shape of the molecules is asymmetrical due to unequal sharing of the electrons. Heteronuclear: one nuclear charge is stronger than another. Polarity is the function of the change in electronegativity (DEN) Increase DEN, = more ionic chstc.

Polar Molecules Rank these in decreasing covalent characteristics: H2O, N2, NO3- , NaBr2, CO2 Solution: 1. Identify the electronegativity for each element in the molecule. 2. Less covalent > 1.7 > more covalent. N2 > NO3- > CO2 > H2O > NaBr2

Lewis Dot Structure Pictorial representation of valance electrons. Stick structure

Octet Rule Representative elements share electrons to take on a Noble gas electron configuration. Each element in a molecule will follow the octet rule.

Shared Electrons Formula to determine the number of shared electrons: N – A = S N = # of electrons needed to form a Noble gas configuration. A = # of electrons available in the valance. S = # of electrons shared

Bonding Sigma Bonds are the single electron overlap of the s orbital. Forms single bonds, end-to-end. Pi Bonds are the overlap of the s and p orbitals. Forms double and triple bonds w/ s end-to-end and p side-to-side.

Practice Problems CO2 N2 CS2 HNO3 NO31- Which are polar? Which are non-polar? Which are non-polar with polar bonds?

Resonance Equally acceptable formulas. HNO3 NO31-

Limits to the Octet Rule Most beryllium compounds Most Group IIIA elements Compound which require more than 8e- in the valance. Compounds containing d or f transitional elements ‘S’ with an odd number of electrons

Practice Problems CCl4 CO2 N2O5 N2O S3O5 NF3

Naming Molecules Follows the rules as ionic compounds except prefixes are used to note ‘how many’. Table 8-3, page 248.

Molecular Structure VB Theory : Valance Bond Theory, orbital overlaps VSEPR Theory: Valance Shell Electron Pair Repulsion Theory Electrons arrange to max the distance between electrons Bonding pairs v. Unshared pairs

Molecular Geometry Linear (2) Trigonal Planar Tetrahedral Trigonal Pyramidal Angular (Bent) Trigonal Bipyramidal Octehedral

Linear Formula AB2 w/ no unshared pairs VSEPR: bonding angle of 180o VB: sp overlap Forms a polar bond and a non-polar molecule.

Trigonal Planar Formula of AB3 and no unshared pairs. VSEPR: bonding angle of 120o VB: SP2 overlap Polar bond w/ non-polar molecule

Tetrahedral Formula of AB4 w/ no unshared pairs. VSEPR: bonding angle of 109.5o VB: sp3 overlap Forms polar bonds and non-polar molecule.

Trigonal Pyramidal Formula AB3 w/ one unshared pair on A. General: subtract 2.5o for each unshared pair. VSEPR: bonding angle of 107o VB: sp3 overlap w/ a polar bond and a polar molecule

Angular (Bent) Formula AB2 w/ 2 unshared pairs on A VSEPR: bonding angle of 104.5o VB: sp3 overlap w/ polar bonds and polar molecule.

Linear Formula AB w/ 3 unshared pairs VSEPR: bonding angle of 102o VB: sp3 overlap w/ polar bonds and polar molecule.

Trigonal Bipyramidal Formula AB5 w/ no unshared pairs VSEPR: bonding angles at 90o, 120o and 180o VB: sp3d overlap w/ polar bonds and polar molecule.

Octahedral Formula AB6 w/ no unshared pairs VSEPR: bonding angles of 90o, 120o and 180o VB: sp3d2 overlap w/ polar bonds and molecule

Molecules Molecule VB VSEPR Shape NI3 PH3 CH4 SF6 H2S PF5 BeCl2