Chapter Six: Electronic Structure

Question 1

What is this?
- the arrangement and energy of electrons in atoms

Answer 1

Electronic Structure

Question 2

Materials that glow give off light and that light possesses a broad range (______________) of colors

Answer 2

spectrum

Question 3

Energy comes in packets called…

Answer 3

quanta

Question 4

What is the 3-step explanation of discrete (line) spectra results that was created by Planck, Bohr, and Einstein?

Answer 4

1. Electrons in an atom can only occupy certain orbits
2. Energy is only absorbed or emitted to move an electron from an one energy state to another
3. The atoms absorb or radiate light to make the energy jump from one orbital to another

Question 5

∆E electron = ∆E light =….

Answer 5

hv

Question 6

What is planks constant?

Answer 6

6.626 x 10^-34

Question 7

When an electron moves closer to the nucleus it radiates ___________. The smallest package of light energy is the photon.

Answer 7

light

Question 8

Bohr model has values called “__”. they are Bohr orbitals

Answer 8

n

Question 9

(+∆E) means energy is ___________. A photon is absorbed in this instance
N final > N initial

Answer 9

absorbed

Question 10

(-∆E) means energy is _____________. A photon is emitted in this instance.
N final < N initial

Answer 10

Released

Question 11

What is this?
The energy level an electron ordinarily occupies when nonexcited

Answer 11

Ground State

Question 12

What are the two limitations of the Bohr Atomic Model?

Answer 12

1. works best for Hydrogen, but meh for others
2. With the circular orbit model, electrons would constantly be crashing into the nucleus

Question 13

Wavelength measures…

Answer 13

peak to peak

Question 14

frequency measures….

Answer 14

the # of waves passing a given observation point per unit of time

Question 15

Speed of traveling wave is what times what?

Answer 15

wavelength times frequency

Question 16

All forms of ________________ _______________ travels through space at the same speed

Answer 16

Electromagnetic Reaction

Question 17

What type of Ultraviolet Rays?
100-280

Answer 17

UVC

Question 18

What type of Ultraviolet Rays?
280-315

Answer 18

UVB

Question 19

What type of Ultraviolet Rays?
315-400

Answer 19

UVA

Question 20

What kind of effect?
Metals hold electrons but not infinitely tight. If one of the electrons absorbs a photon with enough energy, it can break free from the metal; any leftover energy after that becomes kinetic energy of the electron

Answer 20

Photoelectric Effect

Question 21

The farther the shell from the nucleus, the _____________ the energy

Answer 21

greater

Question 22

Is Shell 3 or Shell 1 more desirable?

Answer 22

Shell 1

Question 23

Principle Quantum Number (n)
- The principle quantum #, n, describes the _______ _________ in which the orbital resides
- the values of n are integers >= 1

Answer 23

energy shell

Question 24

We can only put ____ electrons in any actual orbital

Answer 24

2

Question 25

Angular Momentum Quantum # (l)
- the quantum number defines the _________ of the orbital
- allowed values of l are integers ranging from 0 to (n-1)
- the number associated with l defines the shape of the orbitals

Answer 25

shape

Question 26

if the value of l is 0, what is the shape letter?

Answer 26

s

Question 27

If the value of l is 1, what is the shape letter?

Answer 27

p

Question 28

If the value of l is 2, what is the shape letter?

Answer 28

d

Question 29

Magnetic Quantum # (ml)
- the magnetic quantum # describes the __________ - ____________ orientation of the orbital
- allowed values are integers ranging from -1 to 1

Answer 29

three-dimensional

Question 30

The way electrons are distributed in an atom is called its….

Answer 30

electron configuration

Question 31

Each statement of a configuration consists of what two things?

Answer 31

1. a number denoting the type of orbital (subshell)
2. a superscript denoting the number of electrons in those orbitals

Question 32

Who’s rule?
- for a set of orbitals in the same subshell, there must be (a) one electron in each orbital before pairing and (b) those electrons have the same spin, as much as possible

Answer 32

Hund’s Rule

Question 33

The spin of an electron describes its ______________ _____________, which affects its energy

Answer 33

magnetic field

Question 34

The spin quantum number (ms) has only two allowed values, what and what?

Answer 34

+1/2 and -1/2