Chem test 3

Hybridization of central atom

linear/linear sp trigonal planar/ trigonal planar/bent sp2 tetrahedral/tetrahedral/trigonal bypyrimadal/bent sp3

london dispersion forces

non polar molecules temporary dipoles are formed as a result of momentary uneven distribution of electrons stringest with large long molecules

ionic bond

oppositely charged ions , stringest with large charges and small bond lenghts

hydrogen binds

polar molecules with h bund to small electronegative atom , usually small dipole forced

dipole forces

polar molecules, partial charges not so as strong

Linear

sp

trigonal planar

sp2

trigonal bypyrimidal

sp3d

Octahedral

sp3d2

delocalization

the spreading of electron in alternating single and double bonds over 3+ atoms in a molecule

A π bond could be formed from the overlap of which two orbitals?

two unhybridized p orbitals

A molecule that contains delocalized electrons ________

will have at least two resonance structures.

Which of these molecules have delocalized electrons?

Draw the Lewis structure of each molecule and determine which has resonance. Resonance results in alternate ways to distribute electrons but still maintains a valid Lewis Structure. CO₃²⁻ has delocalized electrons. CO₃²⁻

bond order

You can calculate the bond order using this formula: BO=1/2 (numberofbondingelectrons−numberofantibondingelectrons) Benzene has σ and π bonds and the bond order will be a combination of both. To calculate bond order for σ bonds, there are 2 bonding electrons and 0 antibonding electrons.BO=1/2(2−0)=1 To calculate bond order for π bonds, there are 6 bonding electrons and 0 antibonding electrons. This is if there were six full pi bonds, but because this is a resonance structure it is divided by two.

The term 'delocalization' refers to

electrons being shared via π bonds between more than just two atoms.