Modern Atomic Theory

Question 1

What is significant about orbitals? (2 things)

Answer 1

They are where electrons are found.

Each Orbital has a characteristic energy level

Question 2

How does the amount of energy in an orbital change as the electrons get further away from the nucleus?

Answer 2

The amount of energy increases.

Question 3

Which symbols describe the energy level and shape of an electron?

Answer 3

Quantum numbers: n, l, ml, and ms.

Question 4

What are the four Quantum numbers?

Answer 4

n, l, ml, and ms.

Question 5

What is the principal quantum number?

Answer 5

n. The energy level of electrons. (alternative way of showing electrons in orbitals).

Question 6

What does the principal quantum number describe?

Answer 6

How far the electron is from the nucleus. (distance increases with value of n).

Question 7

What is complicated about the principal quantum number?

Answer 7

Not all electrons in an energy shell/level are equivalent.

Question 8

What is the second quantum number?

Answer 8

L. The Subshell type.

Question 9

What does the second quantum number describe?

Answer 9

The shape of orbitals.

Question 10

How does the value of n determine the possible L values?

Answer 10

l= n - 1

Question 11

What are the letter designations of L?

Answer 11

0=S, 1=P, 2=D, 3=F, 4=G

Question 12

How many subshell types would n=2 have?

Answer 12

2 (2s, 2p)

Question 13

How many subshell types would n=4 have?

Answer 13

4 (4s, 4p, 4d, 4f)

Question 14

What is the Magnetic Quantum Number?

Answer 14

ml. Orientation of orbital

Question 15

What does the magnetic quantum number describe?

Answer 15

How an orbital is oriented in space relative to other orbitals.

Question 16

How was the magnetic quantum number discovered?

Answer 16

Through the application of a magnetic field to a gas discharge tube. They found further splitting of emission lines.

Question 17

How does the value of L affect the value of mL?

Answer 17

mL can equal -L to +L

Question 18

How many possible orientations are in a p orbital?

Answer 18

3 (mL= -1, 0, or 1).

Question 19

What is significant about the orientations of a certain orbital?

Answer 19

The possible orbitals would all have the same energy and shape.

Question 20

How many orbitals would subshell type s have?

Answer 20

1 (mL=1)

Question 21

How many orbitals would subshell type p have?

Answer 21

3 (mL= -1, 0, 1)

Question 22

How many orbitals would subshell type d have?

Answer 22

5 (mL= -2, ,-1, 0, 1, 2)

Question 23

How many orbitals would subshell type f have?

Answer 23

7 (mL= -3, -2, -1, 0, 1, 2, 3)

Question 24

What is the spin quantum number?

Answer 24

ms. The orientation of electrons.

Question 25

What does the spin quantum number describe?

Answer 25

The orientation of the 2 electrons in each subshell or suborbital.

Question 26

How many orbitals can be in a subshell type?

Answer 26

MAX 2

Question 27

What is the ms of a pair of electrons of opposite spin?

Answer 27

ms= +1/2, -1/2.

Question 28

How is ms notated?

Answer 28

by arrows.

Question 29

What is the general formula for the number of electrons in a shell?

Answer 29

2n^2.

Question 30

How many electrons would there be in the 3rd energy level?

Answer 30

18

Question 31

How many electrons can have the same set of 4 quantum numbers?

Answer 31

ONLY ONE.

Question 32

What is the shape of an s orbital?

Answer 32

Circle

Question 33

What is the shape of a p orbital?

Answer 33

An 8

Question 34

What is the shape of a d orbital?

Answer 34

A clover.