Chapter 7/8- Electron Configuration

Question 1

Wave definition

Answer 1

Disturbance by which energy is transmitted

Question 2

Wavelength definition

Answer 2

Distance between 2 peaks

Question 3

Amplitude definition

Answer 3

Vertical distance from midline

Question 4

Frequency definition

Answer 4

Number of waves for a particular pt per second

Question 5

Wavelength equation

Answer 5

Speed of wave= frequency x wavelength

Question 6

Speed of light?

Answer 6

3.00 x 10^8 m/s

Question 7

What happens to frequency as energy increases?

Answer 7

Increase in frequency

Question 8

What happens to wavelength as energy increases?

Answer 8

Decrease in wavelength

Question 9

S orbital

Answer 9

1 circular orbital, fits 2 electrons

Question 10

P orbital

Answer 10

Infinity shape, 3 of each

2 electrons each, 6 electrons total

Question 11

D orbital

Answer 11

X shape, 5 of each

Each fits 2, 10 electrons total

Question 12

What is n?

Answer 12

Principle quantum number
Determined energy of an orbital
1,2,3… No zero or negatives

Question 13

What is L?

Answer 13

Angular momentum quantum number
Determines shape of orbital
Ranges from 0 to n-1

Question 14

How many orbitals can be in a given value, n?

Answer 14

N^2

Question 15

How to find total number of orbitals?

Answer 15

2L+1

Question 16

What is ML?

Answer 16

Orientation
2L+1

For example, if L=2, there are 5 possible ML values

Question 17

What is Ms?

Answer 17

Electron spin, either +/- 1/2

⬆️+1/2 ⬇️-1/2

Question 18

What is q=mc🔺t?

Answer 18

Q= 🔺H, units are joules 
M= mass in kg
C= specific heat (given usually)
T= change in temperature

Question 19

Isoelectronic definition

Answer 19

Same number of electrons (f- and Na+)

Question 20

Atomic radius and trend

Answer 20

Half the distance between 2 nuclei

Atomic radius increases to the left and downward

Question 21

Ionic radius trend

Answer 21

Opposite of atomic radius

Increases upward and to the right

Question 22

Which is bigger, Ca2+ or k+?

Answer 22

K+ is bigger because it has less protons, and protons pull electrons closer to the nucleus, making the ion smaller

Question 23

Ionization energy definition

Answer 23

Minimum energy required to remove an electron from its gaseous state
Tells us how tightly an atom holds its electrons
If the IE is higher, it’s more difficult to remove an electron
Increases upward and to the right

Question 24

How does ionization relate to atomic radius?

Answer 24

Higher ionization energy means smaller radius, and vice versa

Question 25

Electron affinity definition

Answer 25

Measure of the tendency of an atom to gain an electron | Same trend as ionization energy, increases up and to the right