Ch 3 - Bonding Flashcards
Covalent
Electrons shared between atoms
Ionic bonds
Electrons transferred from one atom to another.
Principle quantum number
N corresponds to energy level and therefore size of a given electron in an atom
1-infinity but mcat stops at 7
Azimuthal quantum number
L Describes shape values range from 0 to n-1 and correspond to s, p, d, f orbitals 0 - s 1 - p 2 - d 3 - f Energy increase as number increase
Magnetic quantum number
m sub l
Describes orientation
Ranges from negative L to positive L
Spin quantum number
m sub s
Describes spin and is either +1/2 or -1/2
Molecular orbitals
Obtained by adding or subtracting wave functions. Math not on mcat
Bonding orbital - signs of wave functions are same (+,+ or -,-) lower energy more stable
antibonding opposite of above
Sigma bond
Head to head or tail to talk overlap
All single bonds are sigma
Pi bonds
Triple and double bonds contain two pi and one sigma or one pi and one sigma bond
Shorter and shorter in length and the more bonds the more difficult to break. Although alone these bonds are easier to break than sigma
Resonance structures
Resonance structures differ in their placement of electrons in hybridized p-orbitals and require bond conjugation to delocalize electrons in a molecule.
Occurs in molecules with conjugated bonds
Hybrid orbitals
Mixing different orbitals
sp3 sp2 sp
sp3 hybridization
Tetrahedral geometry
25% s
75% p
sp2 hybridization
Alkenes
33% s
67% p
The three sp2 orbitals are 120 degrees apart
Sp hybridization
Triple bond
50% s
50% p
Conjugation
Requires alternating single and multiple bonds because this pattern aligns a number of unhybridized p-orbitals down the backbone of the molecule
