Bonding **

Question 1

Quantum numbers

Answer 1

describe the size, shape orientation, and number of atomic orbitals an elements possesses

Question 2

principal quantum number

Answer 2

n, describes the energy level (shell) in which an electron resides and indicates the distance from the nucleus tot the electron. Its possible value range form 1 to infinity

Question 3

magnetic quantum number

Answer 3

ml, determines determines the sub shell in which an electron resides. Its possible values range from -l to +l Different orbitals have different shapes: s-orbitals are spherical, while p-orbitals are dumbbell-shaped and located on the x-, y-, or z axis

Question 4

spin quantum number

Answer 4

mx, describe the spin of an electron. Its possible values are +- 1/2

Question 5

bonding orbitals

Answer 5

are created by head-to -head or tail to til oerlap of atomic orbitals of the same sign and are energetically favorable.

Question 6

Antibonding orbitals

Answer 6

are created by head to head or tail to tail overalp of atomic orbitals that have opposite signs ad are energetically unfavorable.

Question 7

single bonds

Answer 7

sigma bonds, which contains two electrons

Question 8

double bonds

Answer 8

which contain one sigma bond and one pi bond. Pi bonds are created but sharing of electrons between two unhybridized p-orbitals that align side by side.

Question 9

Triple bonds

Answer 9

contains one sigma bond and two pi bonds

Question 10

Sp3-hybridized orbitals

Answer 10

have 25% s character and 75% p character. They form tetrahedral geometry with 109.5* bond angles. Carbons with all single bonds are sp3-hybridized.

Question 11

Sp2-hybridized orbitals

Answer 11

they have 33% s character and 67% p character. They form trigonal planar geometry with 120* degree bond angles. Carbons with one double bond are sp2 hybridized.

Question 12

Sp-hybridized orbitals

Answer 12

have 50% s character ad 50% p character. They form linear geometry with 180* bond angles. Carbons with a triple bond, or with two double bonds, are sp-hybridized.

Question 13

resonance

Answer 13

describes the delocalization of electrons in molecules that have conjugated bonds. Increases stability of a molecule. Various forms all contribute to the true identity of electron density in a molecule. the more stable the more it contributes. Resonance forms are favored if they lack formal charge, full octets on electronegative toms, or stabilize charges through induction and aromaticity.

Question 14

conjugation

Answer 14

occurs when single and multiple bonds alternate, creating a system of unhybridized p orbitals down the backbone of the molecule through which pi electrons can delocalize.

Question 15

Azimuthal quantum number

Answer 15

l determines the subshell in which an electron resides. Its possible values range from 0 to n-1. the subshell is often indicated with a letter: l=0 corresponds to s, 1 is p, 2 is d, 3 is f.