Chemistry: ch. 4 quantum numbers part 1

Give the N and L values 1s

N=1 L=0

Give the N and L values 2p

N=2 L=1

Give the N and L values 3s

N=3 L=0

Give the N and L values 4d

N=4 L=2

Give the N and L values 5f

N=5 L=3

What is ml?

Where a specific orbital electron belongs

How many possible orbitals are there for n= -4 -10

-16 -100

Deduce the maximum number of electrons that can occupy an: -s orbital -The sublevel of p orbitals -The sub level of D orbitals -The sub level of F orbitals

-2 -6 -10 -14

The ml values for a d orbital are

-2, -1, 0, 1, 2

Which orbital destinations are theoretically possible? -7s -1p -5d -2d -4f -5g -6i

-7s -5d -4f -5g -6i

What are the possible ml values for each of the following types of orbitals? -s -p -d -f

0 -1,0,1 -2,-1,0,1,2 -3,-2,-1,0,1,2,3

The allowed values of l for the level with n=2 are

0, 1

They allowed values of L for the level with n=4 are

0,1,2,3

The number of orbitals what's the quantum numbers n=3,l=2, and ml=0 is

1

The maximum number of electrons with quantum numbers with n=3 and l=2 is

10

Place the following orbitals in order of increasing energy: 1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p

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

The number of orbitals with n=3 and l=1 is

3

How many electrons can inhabit all of the n=4 orbitals?

32 electrons

Name the orbital N= 3 L=2

3d

Name the orbital N= 3 L=1

3p

Name the orbital N= 3 L=0

3s

The sub level with the quantum numbers n=4,l=2 is

4d

Name the orbital N= 5 L=0

5s

The number of orbitals in a level with n=3 is

9

State the 4 quantum numbers and the possible values they may have

Primary energy level: 1,2,3,4,5,6,7 Sub level: 0,1,2,3 Orbital: -3,-2,-1,0,1,2,3 Spin: 1/2,-1/2