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FAU / Chemistry / CHM 2045 / What is the formula to be used in ephoton?

What is the formula to be used in ephoton?

What is the formula to be used in ephoton?

Description

School: Florida Atlantic University
Department: Chemistry
Course: General Chemistry 1
Professor: Daniel huchital
Term: Spring 2017
Tags: General Chemistry and Chemistry
Cost: 50
Name: Exam 3 Study Guide
Description: Chapters 6, 7, 8.1, and 8.2.
Uploaded: 11/10/2017
8 Pages 993 Views 3 Unlocks
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Exam 3Don't forget about the age old question of Who are the organizational stakeholders in a college university?

Chapter 6                                        

  • Wavelength (lambda - 2)
  • Distance between peaks
  • Frequency (nu - v)
  • Number of waves passing a point in

a given amount of timeIf you want to learn more check out Are homology and homoplasy the same?

C = ২v                                                ২ =                 v =

C = speed of light = 3.00 108 ms-1If you want to learn more check out Who built the hagia sophia in constantinople and why is it so important?
We also discuss several other topics like Photosynthesis consists of the light reactions and what?

  • Wavelength and frequency are inversely related
  • The higher one is, the lower the other

If you want to learn more check out What are the legal forms that used for ownership of a business?

Electromagnetic Radiation SpectrumWe also discuss several other topics like What is the purpose of self-management and responsibility for an action?

Higher frequency

Lower frequency

                                                      Visible                           radio        

Y rays - x rays - uv - light - IR - microwave - FM - AM - long radio waves

                 

             p-bl-G-Y-O-R

Shorter wavelength

Longer wavelength

  • Wavelength is usually given in nm but needs to be in m for calculation     1m = 1.10-9nm

  • The higher and shorter the frequency and wavelength the more energy

        the lower and longer the frequency and wavelength the less energy

  • A spectrum is continuous or lined. Continuous is where colors blend together, lined has distinct lines of color

  • Quantanization
  • Max Planck proposed FM radiation was emitted in packets of quanta (now photons)

Energy = hr

h = planck’s constant *will be provided on exam

h = 6.62 10-34 J.S

Atomic Spectra

  • Hydrogen

Equation to calculate ૨ of red, green, and blue lines

n

line

3

red

*4 lines in emission

Spectrum in visible region

Balmer Equation

4

green

= R [- ]

5

blue

6

violet

Bohr Model

-  calculate En for different energy states in J/atom or KJ/mole

orbitals / energy states

*expressed in n = 1, 2, 3, etc.

En =

n = 1 is the ground state-closest to nucleus

        Excited states is any level > 1

electrons can move to different levels

  • Absorbs energy when moving to a higher excited level / state
  • Emit release energy when moving to lower excited level / state

Ephoton =

many transition possible

* the greater the distance the more energy absorbed or emitted

10 transitions for 5 energy levels

*the energy levels farther from nucleus slowly get closer together

Orbitals

S = circle

P = dumbell

d = four-leaf clover

  • Solutions to Schrödinger’s equation yield probability in 3D for likelihood of finding an electron around the nucleus

Quantum Numbers & Electron Orbitals

  • QN come from Schrödinger’s equation - describe location of electron
  • 3 QN

Principal QN - “n” - energy and size

Angular Momentum QN - “ℓ” - shape

Magnetic QN - “me” - number of orbitals in subshell - orientation

Principal QN

n = 1, 2, 3, 4, . . . .

how many shells - size

Angular Momentum QN

ℓ = 0, 1, 2, . . . . up to n - l

*if n = 3, ℓ = 0, 1, 2

Magnetic QN

mℓ = -ℓ, . . ., 0, . . . , ℓ

*if ℓ = 2, mℓ = -2, -1, 0, 1, 2 - so there are 5 orbitals

ℓ determines shape

# of orbitals in subshell

ℓ = 0 → S orbital O

1

*each subshell contains

2ℓ = 1 orbitals

ℓ = 1 → p orbital

3

ℓ = 2 →d orbital

5

ℓ = 3 → f orbital

7

Magnetism

  • unaffected or slightly repelled is diamagnetic
  • Attracted to magnetic field is paramagnets

Arrangement of Electrons

  • Each orbital can only hold 2 electrons, to distinguish them from each other we use the 4th QN - “ms”

ms determines spin - clockwise or counterclockwise

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