Week 1

Question 1

Inorganic Chem is the study of?

Answer 1

“Everything else”

Question 2

What is included in the “everything else”

Answer 2

geometries, coordination numbers, coordination complexes, more orbitals, more electrons, solid state chemistry

Question 3

What does the atomic # A =?

Answer 3

protons + # neutrons

Question 4

relative mass of proton, neutron, electron

Answer 4

p= 1837
n=1839
e=1

Question 5

1 amu = ?

Answer 5

1.661x10^-24 g

Question 6

Isotopes of Hydrogen

Answer 6

Hydrogen (Protium)
Deuterium
Tritium

Question 7

Relative atomic mass (Ar) of the element (in amu)

Answer 7

– the weighted mean of the mass numbers of all the isotopes of this element.
75.77 % of 35Cl and 24.23% 37Cl
Ar= 0.7577×35 + 0.2423×37 = 35.484
Ar= 0.7577x34.97 + 0.2423x36.97 = 35.4

Question 8

How is the periodic table arranged?

Answer 8

1) Relative weight (shared by rows)

2) Reactivities (shared by columns)

Question 9

What is an allotrope?

Answer 9

One of two or more distinct forms of an element (oxygen & ozone)

Question 10

What do groups and periods tell about electrons

Answer 10

Period - max n (principal quantum number)

Group - number of valence electrons for s and d

Question 11

How many electrons, protons and neutrons does 19F have?

Answer 11

Protons - 9
Neutrons - 10
Electrons 9

Question 12

What did Louis de Broglie do?

Answer 12

“Any moving particle or object has an associated wavelength”
Found the relation between wavelength and momentum of particles
h/p=wavlength, h being Planck’s constant

Question 13

What was Schrodinger’s thing?

Answer 13

Energy is limited to discrete values and specific for a system; an electron cannot have energy that is not one of these values
***ONLY ONE-ELECTRON particles

Question 14

What is the principal quantum number?

Answer 14

n

This indicates SIZE of the orbital and all positive integers only

Question 15

What is the angular momentum quantum number?

Answer 15

L

SHAPE of orbital, represented by (n-1) to infinity

Question 16

What is the magnetic quantum number?

Answer 16

mL

SPATIAL directions and is represented from -L to +L

Question 17

What is the spin quantum number?

Answer 17

mS
direction of the spin (up or down)
Value of +1/2 or -1/2

Question 18

What is the Aufbau principle?

Answer 18

the ground state energy config of electrons starts low energy orbitals and then progressively moves higher

Question 19

What is Hund’s Rule?

Answer 19

When electrons are placed in degenerate orbitals, the ground state has as many electrons as possible in different orbitals and with parallel spin

Question 20

What does degenerate mean in chemistry?

Answer 20

of equal energy

Question 21

What is the Pauli exclusion principle?

Answer 21

No two electrons can have the same set of 4 quantum numbers (every electron has a unique ‘address’ if you will)

Question 22

What are the coinciding quantum numbers for the l orbitals?

Answer 22

s-0
p-1
d-2
f-3