Development Of Quantum Theory

Question 1

Heisenberg Uncertainty Principle

Answer 1

States that it is impossible to know simultaneously both the momentum p and the position x of a particle with certainty.

Question 2

Orbital

Answer 2

A region where an electron is likely be found because we can’t know exactly where an electron is at any given time.

Question 3

What are quantum numbers of an atom?

Answer 3

Used to determine electron configuration of an tom and the probable location of the atom’s electrons.

Question 4

Principal Quantum #?

Answer 4

n, which defines size/energy level.

Question 5

Angular Momentum Quantum #?

Answer 5

l, which defines shape.

Question 6

Magnetic Quantum #?

Answer 6

m subscript l, defines orientation.

Question 7

Electron Spin Quantum #?

Answer 7

m subscript s, defines specific electron.

Question 8

Larger n = in terms of size?

Answer 8

Larger orbital

Question 9

Larger n = in terms of energy?

Answer 9

Higher energy level

Question 10

What is the allowed values for n as an integer?

Answer 10

Starting with 1

Question 11

What is a shell in terms of n?

Answer 11

Collection of orbitals with the same value of n.

Question 12

What is a typical shape of s orbital?

Answer 12

Sphere shaped.

Question 13

What is a typical shape of p orbital?

Answer 13

Dumbbell shaped.

Question 14

What is typical shape for d orbital?

Answer 14

Cloverleaf shaped.

Question 15

What is a typical shape for f orbital?

Answer 15

Tetrahedral shaped.

Question 16

What are possible l values if n = 1? What are possible orbital values?

Answer 16

0, s

Question 17

What are possible l values if n = 2? What are possible orbital values?

Answer 17

0,1 and s,p

Question 18

What are possible l values if n = 3? What are possible orbital values?

Answer 18

0,1,2 and s,p,d

Question 19

What are possible l values if n= 4? What are possible orbital values?

Answer 19

0,1,2,3, and s,p,d,f

Question 20

Shell

Answer 20

A shell that holds subshells.

Question 21

Subshells

Answer 21

Subshells that hold electrons and there are types of subshells that move along the shells (s,p,d,f).

Question 22

How many possible orientations does s orbitals have?

Answer 22

1 possible orientation, so only one s orbital in an s subshell.

Question 23

How many possible orientations does p orbitals have?

Answer 23

3 Different orientations, so three p orbitals in each p subshell.

Question 24

How many possible orientations does d orbitals have?

Answer 24

5 Different orientations so five d orbitals in each d subshell.

Question 25

How many possible orientations does f orbitals have?

Answer 25

7 Different orientations so seven f orbitals in each f subshell.

Question 26

What are the possible values of m sub l if l = 1? What are possible orbitals?

Answer 26

0, and s orbital.

Question 27

What are the possible values of m sub l if l = 1? What are possible orbitals?

Answer 27

-1, 0, 1 and 3 p orbital positions.

Question 28

What are the possible values of m sub l if l = 2.? What are possible orbitals?

Answer 28

-2,-1,0,1,2 and 5 d orbital positions.

Question 29

What are the possible values of m sub l if l = 3? What are possible orbitals?

Answer 29

-3,-2,-1,0,1,2,3 and 7 different orbital positions.

Question 30

What is m sub s?

Answer 30

Specifies the spinning orientation of the electron, either as -1/2 or +1/2. (spin up or spin down).