Final Exam

Question 1

What are the three laws of thermodynamics?

Answer 1

Energy never created or destroyed
Entropy of the universe increases in spontaneous, unchanged in equilibrium
Entropy of a perfect crystalline substance is zero at the absolute zero of temperature

Question 2

What is the atomic number equal to?

Answer 2

Number of protons

Question 3

What is the mass number equal to?

Answer 3

Number of protons and neutrons

Question 4

What are the two types of ions?

Answer 4

Cation - positive charge

Anion - negative charge

Question 5

How many nanometers are in one meter?

Answer 5

1 X 10^9

Question 6

What is the unit for frequency?

Answer 6

Hertz

1/s

Question 7

What does heisenburgs uncertainty principle state?

Answer 7

Can not know position and momentum of a particle at the same time

Question 8

What are the quantum numbers?

Answer 8

n - energy or distance from nucleus (1,2,3…..)
L - Shape (0,1,2 … n-1)
ML - Orientation in space ( -L to L)
Ms - Electron spin ( + .5 or - .5)

Question 9

What are the shapes of the orbitals based on the L numbers?

Answer 9

0 = S-orbital
1 = P-orbital
2 = D-orbital
3 = F-orbital
4 = G-orbital

Question 10

What happens in an excited state?

Answer 10

An electron gets bumped up a level

Always add or subtract from the orbital with the largest n followed by highest L

Question 11

What does isoelectronic mean?

Answer 11

Any atom/ion with the same electronic configurations

Question 12

What is the ionization energy?

Answer 12

Energy required to remove an electron

Question 13

Why does ionization energy increase from left to right?

Answer 13

The force holding the electrons increases, closer to full orbital

Question 14

Why does ionization energy decrease from top to bottom?

Answer 14

As you go down n increases, therefore so does the radius

Force on electrons is decreased as R goes up

Question 15

Why does atomic radius increase from top to bottom?

Answer 15

There are more orbitals

Question 16

Why does atomic radius decrease from left to right?

Answer 16

Elements with more protons in a period will have more attraction making the radius smaller

Question 17

What is electronegativity?

Answer 17

The ability to attract electrons in a chemical bond

Question 18

What is formal charge and how do you calculate it?

Answer 18

Mechanism that compares valence electrons in an atom

FC = (number of valence electrons) - (number of lone pair electrons) - .5(number of bonding electrons)

Question 19

What is a resonance structure?

Answer 19

The location of the double bonds can change and the resonance structure is like a hybrid

Question 20

What is the steric number?

Answer 20

Number of bonded atoms and lone pairs on a central atom

Question 21

What are isotopes?

Answer 21

Same number of protons, different number of neutrons

Question 22

What are paramagnetic?

Answer 22

Has at least one unpaired electron

Question 23

What is diamagnetic?

Answer 23

No unpaired electrons

Question 24

What are the bonding electron pairs, arrangement, angle, and shape?

Answer 24

2 - Linear - 180 - Linear
3 - Trigonal Planar - 120 - trigonal planar
4 - Tetrahedral - 109.5 - Tetrahedral
5 - Trigonal bipyramidal-120 or 90-trigonal bipyramid
6 - Octahedral - 90 - octahedral

Question 25

What are the bonding electrons, lone pair electrons, arrangement, angle and shape?

Answer 25

2 - 1 - Trigonal planar - <109.5 - Trigonal Pyramidal 3 - 2 - Trigonal bipyr - 120, 90 - TShaped 4 - 1 - Trig bipyr - 120,90 - See saw 4 -2 - Octahedral - 90 -Square Planar 5 - 1 - Octahedral - 90 - square pyramidal

Question 26

What is the hybridizarion based on the steric number?

Answer 26

2 - sp 3 - sp2 4 - sp3 5 - sp3d

Question 27

What is the bond order?

Answer 27

.5(electrons in bonding pair) - .5(electrons in antibonding)

Question 28

What are the two exceptions for molecular orbitals?

Answer 28

O2, ne2 and F2 have r2p before the pi2p

Question 29

What is the triple point?

Answer 29

Intersection of three phase boundries, all three exist simultaneously

Question 30

What is the critical point?

Answer 30

Where the gas and liquid line terminate

Question 31

What is the order of strengths with internolecular forces?

Answer 31

``` Hydrogen Dipole - dipole Polar Dipole induced Dispersion ```

Question 32

What are the atoms that hydrogen bonds can form with?

Answer 32

Oxygen Nitrogen Fluorine

Question 33

According to simple collision theory what three things must happen for a reaction to occur?

Answer 33

Collision between reactant particles Correct oroentation of collision particles Minimum energy must be met to get it activated

Question 34

What must a molecule have to be dipole?

Answer 34

Must be polar

Question 35

How do you tell if a molecule is polar?

Answer 35

A molecule is polar if there are lone pairs on central atom or the centeal atom is bonded to different atoms

Question 36

How are intramolecular forces related to boiling and melting point?

Answer 36

The stronger the intramolecular forces the higher the melting point and lower the boiling point

Question 37

What is a buffer system?

Answer 37

A solution that resists change in pH | Consists of a weak acid and a weak base

Question 38

What is a system?

Answer 38

Substance of interest

Question 39

What are the surroundings?

Answer 39

All matter around the system