Lecture 11-7-2024

Question 1

What does the quantum number m subscript s stand for?

Answer 1

orientation

Question 2

What are the two values of m sub s?

Answer 2

1/2 and -1/2

Question 3

Because electrons have orientation, there is a _______ field

Answer 3

magnetic

Question 4

What principle says no two electrons in an atom can not have the same 4 quantum numbers?

Answer 4

Pauli’s exclusion principle

Question 5

What are the four quantum numbers?

Answer 5

n, l, ml, ms

Question 6

How do you calculate the number of nodes?

Answer 6

n-1

Question 7

_____ has maximum probability close to nucleus

Answer 7

2p

Question 8

True or False: n increases as weird Y^2 goes away from the nucleus

Answer 8

True

Question 9

All orbitals with the same principal quantum number have _______ energy

Answer 9

degenerate

Question 10

T or F: A larger n values means a higher energy

Answer 10

True

Question 11

Electrons in the ______ state have the lowest energy possible

Answer 11

ground

Question 12

What principle says:
That electrons are filled into atomic orbitals in the increasing order of orbital energy level

Answer 12

Aufbau Principle

Question 13

What principle/ Rule says:
that electrons fill a suborbital as singles before they start forming doubles

Answer 13

Hund’s Rule

Question 14

__________- not attracted to magnetic field

Answer 14

Diamagnetic

Question 15

______-attracted to magnetic field

Answer 15

paramagnetic

Question 16

_________-strongly attracted to a magnetic field

Answer 16

ferromagnetic

Question 17

T or F: Magnetic properties are not dependent on configuration

Answer 17

FALSE

Question 18

Diamagnetic has to with all _____ electrons

Answer 18

paired

Question 19

paramagnetic has to do with ____ electrons

Answer 19

unpaired

Question 20

ferromagnetic has do with _______ unpaired electonrs

Answer 20

many

Question 21

Give me the list of electron configuration

Answer 21

1s, 2s, 3s, 2p, 4s, 3p, 5s, 4p, 3d, 5s, 5p, 4d, 7s, 6p, 5d, 4f, 8s, 7p, 6d, 5f