chapter 3: vocab and definitions

Question 1

electromagnetic radiation

Question 2

wave

Answer 2

regular oscillation in some particular property (position in the case of ocean waves)

Question 3

frequency

Answer 3

number of waves crests passing a point in space in one second

Question 4

wavelength

Answer 4

distance between successive wave crests

Question 5

speed of light (c)

Answer 5

2.9979 * 10^8 m/s

Question 6

photoelectric effect

Answer 6

electrons ejected from metal when light of sufficient energy hits it

Question 7

photon

Question 8

E of a photon

Question 9

Planck’s constant

Question 10

continuous spectrum

Answer 10

contains all wavelengths of visible light

Question 11

line spectrum

Answer 11

each line corresponds to a discrete wavelength

Question 12

rydberg-balmer equation

Answer 12

predicts the series of lines in an emission

Question 13

the bohr model of the hydrogen atom

Answer 13

structural model in which an electron moves around the nucleus only in circular orbits, each with a specific allowed radius

Question 14

what equation do you use to calculate the energy level of an electron transitioning from one energy level to another?

Answer 14

E = -2.178 * 10^18 J (1/nfinal^2 - 1/ninitial^2)

Question 15

absorption spectra

Answer 15

observed when sample irradiated with electromagnetic radiation transitions when electrons jump from low to higher energy states

Question 16

dual nature of light

Answer 16

wave properties and particulate properties

Question 17

heisenberg’s uncertainty principle

Answer 17

momentum and position of particle-wave cannot be simultaneously known; the position of a moving electron cannot be precisely defined because they’re delocalized (spread out waves)

Question 18

3d waves

Answer 18

orbitals (3 dimensional volume)

Question 19

shape of an orbital represents

Answer 19

region of electron density around the nucleus

Question 20

each orbital can hold

Answer 20

2 electrons max

Question 21

n - principle quantum number

Answer 21

describes orbital energy and indicates distance of e- from nucleus

Question 22

l - secondary quantum number

Answer 22

describes energy and shape of orbital; ranges from 0 to n-1

Question 23

m of l - magnetic quantum number

Answer 23

describes orientation of orbital; ranges from +l to -l

Question 24

m of s - spin quantum number

Answer 24

designates spin orientation of electron, “up” or “down”; can be +1/2 or -1/2

Question 25

pauli exclusion principle

Answer 25

in a given atom no two electrons can have the same set of four quantum numbers; electrons in an orbital have opposite spins

Question 26

polyelectronic atoms

Answer 26

atoms with more than one electron

Question 27

variations in nuclear charge and number of electrons

Answer 27

change the magnitudes of the electrical forces that hold electrons in their orbitals

Question 28

higher nuclear charge

Answer 28

higher attraction

Question 29

shielding and penetration effect

Answer 29

electrons are shielded from nuclear charge by repulsion of other electrons

Question 30

electron configuration

Question 31

aufbau principle

Answer 31

as protons are added one by one to nucleus to build up elements, electrons similarly added to hydrogen–like orbitals

Question 32

guidelines for atomic ground states

Answer 32

1. each electron in an atom occupies most stable available orbital
2. no two electrons can have identical descriptions
3. orbital capacities are as follow
   s - 2 electrons p - 6 electrons d - 10 electrons f - 14 electrons
4. higher n, less stable orbital
5. for equal n, the higher l, the less stable orbital

Question 33

hund’s rule

Answer 33

the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by Pauli principle in a particular set of degenerate orbitals

Question 34

valence electrons

Answer 34

electrons in the outermost principal quantum level of atom

Question 35

continuous spectrum

Answer 35

electromagnetic radiation given off in an unbroken series of wavelengths

Question 36

standing wave

Answer 36

localized wave phenomenon characterized by discrete wavelengths determined by the boundary conditions used to generate the waves; standing waves are inherently quantized