hybridization ochem

hybridized orbitals

form when an atom (aside from hydrogen) prepares to bond, with atomic orbitals combining to create new orbitals that are more effective for bonding

sp³ hybridization

arises upon the mixing of one s with three p orbitals to form four degenerate sp³ orbitals

sp³ electronic geometry

termed tetrahedral, this can be understood by visualizing the four sp³ orbitals arranged around a central point, positioned to be as far apart as possible, resulting in a tetrahedral shape

sp³ idela bond angles

the angles between teh vertices of a tetrahedron, measured from the center, are 109.5

the presence of lone pairs will decrease the angle

sp² hybridization

arises upon the mixing of one s with two p orbitals to form three degenerate sp² orbitals, leaving behind one non-hybridized p orbital

sp² electronic geometry

trigonal planar

three sp² orbitals arranged around a central point, positioned to be as far apart as possible, forming a trigonal shape

non-hybridized p orbital must be oriented perpendicular to the plane of the hybrid orbitals

sp² ideal bond angels

the angles at two vertices of an equilateral triangle, measured from the center, correspond to 120 degrees

lone pairs will decrease this angle

sp hybridization

arises upon the mixing of one s with one p orbital to form two degenerate sp orbitals, leaving behind two non-hybridized p orbitals

sp electronic geometry

termed linear, this can be understood by visualizing the two sp orbitals arranged around a central point, positioned to be as far apart as possible, resulting in a line

the non-hybridized p orbitals must be oriented perpendicular to the plane of the hybrid orbitals

sp ideal bond angles

the angles of two vertices of a line about the center of the line correspond to 180

the presence of lone pairs will reduce this angle

electron density

areas where electrons are found

lone pair, single/double/triple bond

single electrons are not counted as a region of electron density

sigma bonds

form from the overlap of hybrid orbitals or a hybridized orbital and an unhybridized s orbital. to determine the composition of a sigma bond, identify the hybridization of the two atoms involved

pi bonds

form from the overlap of p orbitals and the composition will always be two p orbitals overlapping

the valence shell electron pair repulsion theory

builds upon hybridization by considering the influence of lone pairs on molecular geometry. the central idea of this theory is that both bonds and lone pairs trive to maximize their separation, minimizing electron pair reupulsion

electron geometry

considers all regions of electron density without distinguishing between bonding and non bonding electrons

molecular

geometry accounts for both bonding and non bonding electrons, with lone pairs influencing the overall molecular shape