Bonding

Question 1

Ionic

Answer 1

electrons transfered from one atom to the other to fill the valence shells

Question 2

Covalent

Answer 2

electrons are shared between atoms to fill both valence shells

Question 3

The first three quantum number: n,l, m describe the ____, shape, number and _______ an element possesses.

Answer 3

size, orientation of atomic orbitals

Question 4

Principal Quantum Number, n

Answer 4

energy level of a given electron in an atom, measure of size

smaller the number, clsoer to the shell and lower its energy

Question 5

Azimuthal Quantum Number, l

Answer 5

subshells, range from 0 to n-1

energy increases as l increases

Question 6

l = 0,1,2,3 corrisponds to

Answer 6

s,p, d, and f subshells respectively

Question 7

Magnetic quantum number, ml

Answer 7

within each subshell lies orbitals

range from -l to l for a given subshell (l)

Question 8

s orbital

Answer 8

spherical and symmetrical around the nucleus

Question 9

p orbital

Answer 9

two lobes located about the nucleus and contains a node

x, y and z axis is how it can be positioned

-1 0 and 1 are its possibilities as l = 1

Question 10

node

Answer 10

area where probability of finding an electron is 0

Question 11

d orbital

Answer 11

4 symetrical lobes and contains 2 nodes

4 of the orbitals are clover shaped and the fifth is a donut wrapped around the center of a p orbital

Question 12

Spin QUantum Number, ms

Answer 12

each orbital holds 2 electrons that are distinguished by +/- 1/2

Question 13

Molecular orbitals

Answer 13

when two atomic orbitals combine, obtained by adding/subtracting the wave functions of atomic orbitals

Question 14

Bonding Orbital

Answer 14

if signs of the wave functions of atomic orbitals are the same

low energy, more stable

Question 15

Antibonding Orbital

Answer 15

if signs of the wave functions of atomic orbitals are different

less stable, high energy

Question 16

Sigma Bond

Answer 16

molecular orbital formed by head-head or tail-tail overlap

all single bonds and accomodate 2 electrons

free rotation

Question 17

Pi Bond

Answer 17

when two p-orbitals line up in parallel (side by side) and electron clouds overlap

1 in double bonds, 2 in triple bonds

lock atoms in position

Question 18

It is important to remember pi bonds cannot form without the existance of a_____ . Individual pi bonds are ___ than sigma bonds in strength, hence it is possible to break one bond and leave a single bond in tact.

Answer 18

sigma bond

weaker

Question 19

Hybrid Orbitals/sp3

Answer 19

formed by mixing different types of orbitals aka s and p orbitals to make equivalent sp orbitals

seen in carbon to create equivalent electron bonds

Question 20

How much s character is in a sp^3 orbital?

Answer 20

1 s , 3 ps or 25% s and 75% p

Question 21

sp2 hybridization

Answer 21

1s with 2 p

33% s and 66% p

seen in alkenes, the third p is un-hybridized and participates in pi bond while the hybridized bonds form the sigma

120 degrees apart

Question 22

sp hybridization

Answer 22

in triple bonds, 2 p orbitals are needed to form the pi bond and the thrid p combines with s to form two sp orbitals

50-50 character

180 degrees apart

Question 23

Resonance

Answer 23

occurs in molecules that have conjugated bonds

true form is the hybrid of resonance structures, the true electron density will favor the more stable form of resonance structures

Question 24

Conjugation

Answer 24

altering single and multiple bonds as it aligns unybridized p orbitals down the backbone of the molecule

Question 25

Pi electrons _____ through the p-orbital system to add stability to the molecule

Answer 25

delocalize

Question 26

Resonance Stability

Answer 26

either no formal charge, negative charge on most electronegative atom, induction and aromaticity