Electromagnetic Radiation, Quantum Numbers and Arrangement of Electrons

Question 0

Electromagnetic radiation is ____ and ____; travels in ____

Answer 0

Light, energy, waves

Question 1

–Electromagnetic radiation–

Answer 1

–ELECTROMAGNETIC RADIATION–

Question 2

Left side of the spectrum: ____ wavelengths and ____ frequencies

Answer 2

Longer, lower

Question 3

Right side of the spectrum: ____ wavelengths and ____ frequencies

Answer 3

Shorter, higher

Question 4

Wavelength*

• symbol:
• unit:

Answer 4

Distance between corresponding points on adjacent waves

• λ
• Nanometers (Nm)

Question 5

Frequency*

• symbol:
• unit:

Answer 5

The number of waves that pass a given point in a specific time (usually 1 second)

• ν
• Hertz (Hz) number of waves/second

Question 6

Speed*

• symbol:
• unit:

Answer 6

How fast the light form travels

• c
• meters/second (m/s)

Question 7

The relationship between wavelength (λ) and frequency (ν) is ____ proportional

Answer 7

Inversely

• λ decreases (shorter) then ν increases (more # waves/second)
• λ increases (longer) then ν decreases (less # waves/second)

Question 8

Quantum*

Answer 8

Minimum quantity of energy that can be gained or lost by an atom

Question 9

Photon*

Answer 9

“Tiny packet” of energy released

Question 10

____ and ____ both indicate that energy is like matter that they come in little bundles like a particle traveling in waves… but no not have mass or volume

Answer 10

Quanta, photons

Question 11

Dual-wave particle nature

Answer 11

• photons (quanta)–energy traveling in waves, like matter in small packets
• electron–matter with mass + volume, like energy, movement is as waves

Question 12

Photoelectric effect*

Answer 12

When light is put into atoms there is a change in the electrons
-occurs at specific wavelength and frequency of energy

Question 13

Energy has a ____ relationship

Answer 13

Direct

• as frequency increases then energy increases
• as frequency decreases then energy decreases

Question 14

States of an atom

Answer 14

STATES OF AN ATOM

Question 15

What are the 2 states of an atom?

Answer 15

1. Ground

2. Excited

Question 16

Ground state

Answer 16

Lowest energy state of atom, electrons in normal positive/lowest energy

Question 17

Excited state

Answer 17

High energy state of an atom, photons of energy are added so electrons are at highest energy positions

Question 18

• adding ____ to an atom in a set amount causes electrons to move from ____ state to ____ state
• when electrons return to the ____, atoms release the ____ and part of it is visible as ____ ____

Answer 18

Energy, ground, excited

Ground, energy, one color

Question 19

Spectrum*

Answer 19

Visible light radiation is divided into bands of color

-produced by a spectroscope~ instrument with a prism or diffraction that can separate electromagnetic radiation by specific wavelengths

Question 20

What are the 3 types of spectrums?

Answer 20

1. Continuos
2. Emission
3. Absorption

Question 21

1. Continuous spectrum

Answer 21

• unbroken bands of color for the wavelengths in visible part of electromagnetic radiation
• no spaces/division between colors
• stars+sun/lightbulbs

Question 22

2. Emission spectrum

Answer 22

• separate bands of color that are separated apart at specific wavelength
• specific for each element
• one color spectrum is visible with eyes

Question 23

3. Absorption spectrum

Answer 23

• bands of color with dark lines where energy (light) is absorbed
• dark lines determine composition
• dark lines match up with bright line

Question 24

-Quantum numbers-

Answer 24

–QUANTUM NUMBERS–

Question 25

Bohr

Answer 25

Developed a model of the atom- “planetary model”

-his model only worked for hydrogen

Question 26

De Brogile

Answer 26

Determined electrons have wave-like properties

-found electrons exist at specific frequencies (energy waves)

Question 27

Heisenberg Uncertainty Principle

Answer 27

States it’s not possible to determine both the position (location) and the velocity (speed) of the electron at the same time

Question 28

Orbital*

Answer 28

3 dimensional region above and around the nucleus where electrons are located

• different types and positions in the electron cloud
• they can only hold two electrons

Question 29

2. Angular momentum quantum number

Answer 29

• indicates shape of orbital
• symbol: cursive L
• range: 0 to 3
• represents sublevels within an energy level
• sublevels s,p,d,f

Question 30

3. Magnetic quantum number

Answer 30

• indicates orientation of orbital around nucleus (x-y-z axes)
• symbol: m
• range: +3 to -3
• represents number of orbitals within each sublevel
• orbitals hold up to 2 electrons

Question 31

4. Spin quantum number

Answer 31

• indicates spin direction of electron
• symbol: s
• range: +1/2 to -1/2
• spin must be in opposite directions like up or down; left or right

Question 32

-arrangement of electrons-

Answer 32

–ARRANGEMENT OF ELECTRONS–

Question 33

Electron arrangement*

Answer 33

• show how electrons occur in orbitals of atom
• different for each element –> elements have diff # of electrons
• show ground state for electrons

Question 34

Aufbau principle*

Answer 34

• electrons must fill lowest energy orbitals
• exceptions-groups with Cr/Cu (lowest energy in 3d not 4s)
• also with elements in the same group below them

Question 35

Pauli exclusion principle*

Answer 35

• no two electrons in an element will have the same set of quantum numbers
• only 2 electrons per orbital and must have opposite spins

Question 36

Hund’s rule*

Answer 36

-electrons are distributed among the orbitals (with the same energy) in order to give a maximum number of unpaired electrons

Question 37

What are the 3 types of electron arrangement

Answer 37

1. Orbital notation
2. Electron configuration notation
3. Noble gas notation

Question 38

1. Orbital notation

Answer 38

• line to represent orbital

- arrows show electrons –> max 2, opposite directions

Question 39

2. Electron configuration notation

Answer 39

• principle quantum number
• sublevel letter for angular momentum quantum number
• superscript for number of electron

Question 40

3. Noble gas notation

Answer 40

-chemical symbol of noble gas in [ ] for filled energy level

• Use noble gas in period before the element
• continue with principal quantum number and sublevel letter for angular momentum quantum number
• superscript for number of electrons

Question 41

Why use electron dot diagram?

Answer 41

• show number of valence electrons
• most atoms can hold and want to hold 8 electrons in their valence shell in order to be chemically stable

Chemical stability = full valence shell (octet)
Full s and p orbitals

Question 42

Filling electron dot diagram

Answer 42

• determine number of valence electron

- electron dot diagrams are more simplistic than writing out full energy level diagram

Question 43

Quantum numbers*

Answer 43

Specify properties (locations) of orbitals and property (spin) of electron

Question 44

What are the 4 different quantum numbers?

Answer 44

1. Principle (main level)
2. Angular (shape)
3. Magnetic (orientation)
4. Spin (electron spin)

Question 45

1. Principle quantum number

Answer 45

-indicates main level (distance from nucleus)
-symbol: n
-range: 1 to 7
-corresponds to energy level (period #)
n=1: 2e n=2: 8e n=3: 18e n=4: 32e