Quantum Model of the Atom

Question 1

Wavelength

Answer 1

the distance between 2 corresponding point on the wave (successive peaks/troughs OR two matching points on the wave)
- each color of visible light has different wavelengths

Question 2

Amplitude

Answer 2

the height of the wave determines the intensity of the light
- the larger the amplitude, the greater the intensity of light
- amplitude is independent of wavelength

Question 3

Frequency

Answer 3

the number of crests that pass a given point per second
- is INVERSELY PROPORTIONAL to the wavelength

Question 4

Electromagnetic Spectrum

Answer 4

radio waves, microwaves, infrared light, visible light, ultraviolet light, x-rays, gamma rays
- all are form of light that differ only in their wavelength and frequencies
- light = electromagnetic spectrum
- light is collectively referred to as electromagnetic radiation

Question 5

The Photoelectric Effect

Answer 5

the emission of electrons or other charged particles from a material when it absorbs electromagnetic radiation (LIGHT)
- higher energy = increases KE of electrons, not number released
- increasing the brightness of the light at the same frequency causes more electrons to be emitted and vice versa

Question 6

Photoelectron

Answer 6

electrons ejected through the photoelectric effect

Question 7

Photon

Answer 7

when light behaves as a stream of tiny particles; the particles
- low energy photons correspond to long wavelength and low frequency light
- high energy photons correspond to short wavelength and high frequency light

Question 8

Work

Answer 8

to be ejected via the photoelectric effect, the photon must have greater than or equal energy than the work function of the metal

Question 9

Work Function

Answer 9

minimum energy necessary to remove an electron from the surface of the metal in a vacuum
- different metals have different work functions

Question 10

Threshold Frequency

Answer 10

the frequency of the photon is the minimum frequency necessary to eject a photoelectron

Question 11

Light Absoprtion

Answer 11

an atom absorbs light energy from the surroundings and gains energy

Question 12

Light emission

Answer 12

an atom has excess energy and gives off some energy by emitting light

Question 13

Absorbance Spectrum

Answer 13

the precise wavelengths that are absorbed by an atom of an element
- gaseous atoms of an element only absorb light at particular frequencies/energies

Question 14

The Bohr Hypothesis

Answer 14

• electrons must be found at certain orbits from the nucleus
• electrons travel in circular paths around the nucleus
• first model to place electrons in DISCRETE ENERGY LEVELS (orbit = energy level)

Question 15

Ground State

Answer 15

the energy level closest to the nucleus (lowest energy level)

Question 16

Excited State

Answer 16

when an atom absorbs light of a specific energy and an electron moves up an energy level

Question 17

Emission Spectra

Answer 17

the spacing between the electronic energy levels is different for each type of atom

Question 18

Emission Spectrum

Answer 18

energy is absorbed by an atom and then released as light
- unique for each element
- LINE SPECTRUM: the emission spectrum consists of individual lines

Question 19

IONIZATION

Answer 19

removing an electron results in an ion, so the process is called IONIZATION, and the energy associated with the transition is called IONIZATION ENERGY

Question 20

Rydberg Equation

Answer 20

allows you to calculate the wavelength or energy of the emission line that results from any electronic transition in an hydrogen atom

Question 21

Orbital

Answer 21

region of space surrounding the nucleus where an electron is likely to be found
- CAN HOLD A MAX OF TWO ORBITALS

Question 22

Subshell

Answer 22

group of orbitals that all have the same energy - s,p,d,f

Question 23

Shell

Answer 23

principal energy level; grouping of subshells