Unit 3 Review

Question 1

Which orbital ring has the lowest potential energy?

Answer 1

N=1

Question 2

Which orbital ring has the strongest attractions?

Answer 2

N=1

Question 3

More protons in the nucleus, more _____?

Answer 3

More attractions

Question 4

What does an increased number of attractions mean for ionization energy and size of the atom?

Answer 4

IE is high, size is small

Question 5

What is the core shell of an atom?

Answer 5

The innermost shell

Question 6

What is the valence shell of an atom?

Answer 6

The outermost shell

Question 7

What are orbitals?

Answer 7

Sub-sub-groups for shells and only two electrons can occupy the space

Question 8

What subshell has the lowest energy?

Answer 8

4s^2

Question 9

What is the third and fourth shell electronic configuation for an atom

Answer 9

4s^2, 3d^10, 4p^#

Question 10

What can be classified as an electron domain?

Answer 10

Lone pair (valence electrons not shared with another atom), single/double/triple bonds

Question 10

What is the octet rule?

Answer 10

When atoms combine, the most stable structures are where the atoms have a full valence shell (8 electrons)

Question 11

What happens when atoms form bonds?

Answer 11

They bring down the total energy due to delocalization which then stabilizes the atoms

Question 12

What is considered an electron domain?

Answer 12

A lone pair, a single bond, a double bond, and a triple bond

Question 13

How can you tell which molecule to distribute electrons to?

Answer 13

Distribute to the molecule with stronger IMFs (larger number of protons, more electronegative)

Question 14

Can bonding patterns be ignored to fulfill the octet rule?

Answer 14

YES

Question 15

What is a polar bond?

Answer 15

Partial charges in both atoms

Question 16

What is bond polarity directly proportional to?

Answer 16

The numerical difference between electronegativity values

Question 17

What molecules have partial negative charges?

Answer 17

Molecules with the most electronegativity

Question 18

What molecules have partial positive charges

Answer 18

Molecules with the least electronegativity

Question 19

What is molecular polarity?

Answer 19

The sum of bond polarity; if it equals 0, the bond is non polar, if it is greater than zero, the bond is polar

Question 20

What are easy ways to tell if a molecule is polar?

Answer 20

If it has more than one element surrounding the central atom and if the central atom has a lone pair

Question 21

If a molecule is bent it is most likely…

Answer 21

POLAR

Question 22

If a molecule only contains hydrogen and carbon, it is…

Answer 22

NONPOLAR

Question 23

What is an isomer?

Answer 23

Molecules with the same chemical formula, but different spacial arrangements of atoms

Question 24

What properties are higher if IMFs are higher?

Answer 24

Density, viscosity, boiling point, melting point, and sublimation point

Question 25

Do nonpolar molecules have IMFs?

Answer 25

NO, not without induced parital charges

Question 26

How do induced partial charges occur?

Answer 26

External charges perturbing/polarizing (interacting with) the electron cloud can create induced dipoles induced dipoles=induced dipole forces=dispersion forces

Question 27

What are dispersion forces and what molecules do they occur to?

Answer 27

They are directly proportional to polarizability, a higher number of electrons and size means stronger forces, and it occurs to any molecule

Question 27

When is polarizability larger?

Answer 27

It is larger with more electrons over a larger volume and a more exposed area

Question 28

What are dipole-dipole forces and what molecules to they occur to?

Answer 28

They are directly proportional to molecular polarity, the more polar the molecule, the stronger the forces, occurs to only POLAR molecules

Question 29

What are hydrogen bonding forces and what molecules do they occur to?

Answer 29

They are polar molecules of hydrogen covalently bonded with either nitrogen, oxygen, or flourine, occurs only to POLAR HYDROGEN molecules

Question 30

How do h-bonding forces increase in strength?

Answer 30

If the number of hydrogen sites increase

Question 31

Can lone pairs be linear?

Answer 31

NO

Question 32

How do all molecules interact?

Answer 32

By dispersion forces created by interactions between induced dipoles

Question 33

How do you get stronger dispersion forces?

Answer 33

By making it easier to create induced dipoles (more polarizable molecules in the atom)

Question 34

More polarizability...

Answer 34

STRONGER dispersion forces

Question 35

What molecular geometry do only carbon atoms have?

Answer 35

Tetrahedral

Question 36

Non polar atoms can only have what type of molecular forces?

Answer 36

Dispersion forces

Question 37

What molecules can bind with hydrogen to make hydrogen bonding forces true?

Answer 37

ONLY H-N, H-O, and H-F

Question 38

What is the only requirement to have dispersion forces?

Answer 38

To have induced partial charges

Question 39

What is polarizability?

Answer 39

The ability to have induced dipoles

Question 40

To determine polarizability:

Answer 40

The larger the size and number of electrons, the more polarizable it is