Chemistry Chapter 5 Test

Front 1

List 5 examples of electromagnetic radiation

Back 1

Radiowaves, microwaves, infared, visible light, ultraviolet light

Front 2

Photoelectric effect

Back 2

When Light or a certain frequency shines on a metal, the metal glows

Front 3

Wavelength and frequency are _________ related.

Back 3

inversely

Front 4

Energy and frequency are _________ related.

Back 4

Directly

Front 5

Energy and Wavelength are ________ related.

Back 5

Inversely

Front 6

Wave-particle nature

Back 6

It behaves like a wave but can be measured like a particle.

Front 7

2 differences between red and green light on the electromagnetic spectrum

Back 7

Green has a greater frequency

Red has a greater wavelength

Front 8

Put in order of increasing wavelength: ultraviolet light, microwaves, radio waves, X-rays

Back 8

X-rays, ultraviolet light, microwaves, radiowaves

Front 9

Electromagnetic wave relationship formula

Back 9

c = λv

Front 10

c = λv

c=

λ=

v=

Back 10

c= constant speed of a wave =3.00x10^8

λ= wavelength in meters (m)

v= Frequency in Hertz (Hz) or 1/s

Front 11

Formula for energy of a photon

Back 11

E=hv

Front 12

E=hv

E=

h=

v=

Back 12

E= Energy in Joules (J)

h= Planck's constant, =6.626x10^-34Js (Joule seconds)

v= frequency in Hertz (Hz) or 1/s

Front 13

Wavelength

Back 13

the distance between 2 corresponding points on a wave

Front 14

Frequency (v)

Back 14

the occurrance of a wave

Front 15

Electromagnetic radiation

Back 15

A form of energy that travels as a wave

Front 16

Electromagnetic spectrum

Back 16

Includes all forms of EM radiation (radiowaves, microwaves, infared, visible light, ultraviolet, X-ray, gamma rays)

Front 17

The speed of light

Back 17

3.0x10^8 m/s

Front 18

Quantum

Back 18

a minimum amount of energy that can be lost or gained by an atom

Front 19

Photons

Back 19

Massless particles that carry a quantum of energy

Front 20

Planck's constant

Back 20

relates energy with frequency

h=6.626x10^-34js

Front 21

Electron configuration

Back 21

the use of orbitals to tell the exact location of every electron of an atom (assume ground state), arrangement of electrons

Front 22

Aufbau Principle

Back 22

electrons fill an atom by lowest energy levels and orbital first

Front 23

Diagonal rule

Back 23

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f

Front 24

Hund's rule

Back 24

orbitals of equal energy fill with 1 electrons before 2 (doesn't apply to s)

Front 25

electron capacity

Back 25

s=2e-

p=6e-

d=10e-

f=14e-

Front 26

Pauli Exclusion Principle

Back 26

only 2 electrons can occupy each orbital variation and must be opposite in their spin

Front 27

highest occupied level

Back 27

electrons in the outermost ring (from config)

Front 28

valence electrons

Back 28

electrons in the highest occupied level used for chemical bonding

Front 29

Bohr

Back 29

-Presented the "Planetary Model" of the atom

-Electrons stay in orbits as close as possible to the nucleus with minimum energy (ground state)

-Electrons could jump orbits when energy is absorbed by the atom (excited state)

-When electrons absorb this energy they quickly release it in the form of light (back to ground state)

Front 30

Planetary model

Back 30

electrons travel in specific orbits around the nucleus

Front 31

Problems with Bohr's Planetary Model

Back 31

-Only explained hydrogen atom (with 1 electron)

-Didn't account for other chemical behavior of atoms

-Conclusion: there really are no circular orbits of electrons

Front 32

Heisenberg

Back 32

Tried and used methods to detect electrons

Idea: to detect electrons which behave like light using light (photons)

Impossible to take a measurement of an object without disturbing the object (light interferes with electron movement)

Front 33

Heisenberg Uncertainty Principle

Back 33

It is impossible to determine the location and speed of an electron simultaneously

-the more you know about one quantity, the less you can know about the other

Front 34

Schrodinger

Back 34

Derived a mathematical equation that treats electrons as waves; the "Wave Mechanical Model"

-Plots 3-D regions around the nucleus where electrons are probably located at any given point in time

-3-D region called an Orbital (a section of empty space)

Front 35

Orbital

Back 35

Section of empty space

Front 36

Main Energy Level (Ring or shell)

Back 36

Theoretically levels go from 1-infinity

Actuall levels 1-7

Front 37

Orbital shape (subshell)

Back 37

Sphere (s), propeller (p), double propeller (d), flower petals (f)