Chapter 4: Light and Electronic Structure

Question 1

electromagnetic radiation

Answer 1

energy traveling in waves from charged particles

Question 2

electromagnetic spectrum

Answer 2

the complete range of electromagnetic waves placed in order of increasing frequency

Question 3

visible spectrum

Answer 3

small band of electromagnetic radiation we perceive as light

Question 4

wavelength (𝜆)

Answer 4

distance between two consecutive wave points; measured in meters or nanometers

Question 5

frequency (𝜈)

Answer 5

number of waves passing a point per second

Question 6

hertz (Hz)

Answer 6

the unit of frequency, equal to one cycle per second; 1s^-1

Question 7

wavelength and frequency relationship

Answer 7

inversely related to each other; as the wavelength decreases, the frequency increases & vice versa

Question 8

speed of light (c)

Answer 8

𝜆𝜈, equal to 3.00 × 10^8 m/s

Question 9

photon

Answer 9

small packet of light energy

Question 10

energy of a photon (E)

Answer 10

E = hν or E = hc/λ

Question 11

Planck’s constant (h)

Answer 11

6.63 × 10^-34 J·s, relates energy and frequency

Question 12

line spectra

Answer 12

the emission of light only at specific wavelengths

Question 13

Niels Bohr

Answer 13

physicist who proposed that electrons orbit the nucleus in the same way that planets orbit around the sun, orbits that were closer to the nucleus were lower in energy; he also proposed that electrons can jump from one energy level to another by absorbing light

Question 14

Bohr model

Answer 14

model explaining emission spectra with energy levels

Question 15

energy levels

Answer 15

discrete levels where electrons reside

Question 16

quantum model

Answer 16

model that describes electrons as both particles and waves; indicates where electrons are most likely to be found

Question 17

uncertainty principle

Answer 17

the idea put forth by Werner Heisenberg that the behavior of subatomic particles is uncertain; it is impossible to know the exact velocity and location of a particle

Question 18

principal quantum number (n)

Answer 18

whole number indicating energy level of electrons

Question 19

sublevel

Answer 19

energy levels divided into s, p, d, f

Question 20

orbital

Answer 20

region where electrons are likely found

Question 21

Aufbau Principle

Answer 21

electrons fill lowest energy levels first

Question 22

Pauli Exclusion Principle

Answer 22

no more than two electrons per orbital

Question 23

Hund’s Rule

Answer 23

single electrons occupy orbitals before pairing

Question 24

electron configuration

Answer 24

arrangement of electrons in an atom’s orbitals

Question 25

noble gas shorthand

Answer 25

abbreviated electron configuration using noble gases

Question 26

valence electrons

Answer 26

electrons in the outermost shell involved in bonding

Question 27

inner electrons

Answer 27

electrons not involved in bonding, lower energy

Question 28

outer electrons

Answer 28

electrons beyond the noble gas configuration

Question 29

octet rule

Answer 29

atoms prefer to have eight electrons in valence shell

Question 30

energy level 1 (n=1)

Answer 30

contains one s sublevel, holds 2 electrons

Question 31

energy level 2 (n=2)

Answer 31

contains one s and one p sublevel, holds 8
electrons

Question 32

energy level 3 (n=3)

Answer 32

contains one s, one p, and one d sublevel - holds 18 electrons

Question 33

energy level 4 (n=4)

Answer 33

contains one s, one p, one d, and one f sublevel - holds 14 electrons

Question 34

ion electron configuration

Answer 34

adjust configuration based on ion charge

Question 35

relative energy levels

Answer 35

energy increases in the order s<p<d<f