Chapter 3: Atomic Structure Overview SP2020

1

Part 1: Waves of Light

I. Definitions: Please use your textbook, notes, lecture PPT, or other resources to write the definition of each term.

• Electromagnetic Radiation –

• Electromagnetic Spectrum –

• Wavelength (λ) –

• Frequency (ν) –

• Hertz (Hz) –

II. Calculating Wavelength and frequency, using c= ν λ, c = 2.998 x !"# $%

a. Violet light has a wavelength of 4.10 x 10()* m. What is the frequency?

b. Green light has a frequency of 8.12 x 10), Hz. What is the wavelength?

any form of radiant energy inthe electromagneticChp .3 pg781 spectrum

a continuous range of radiant energy that includes gamma rays ,Xrays , Ultravioletradiation,visible light , infraredradiation,and radio waves

Red orange yellow Green Blue Indigoviolet

RadioWaves Microwaves Infrared Ultraviolet tray Gamma Ray

Low High

Longest Shortest

oatwugnthfwodinstfosneamwa.ms'- towestthe number of crests of awave that

pass a stationary point of reference per second

SI unit for frequency1 HE = 15' = I cycle per second

= V = ,f= 3%71147=7.32×10" Hz

E-¥ - X - E -- %7E.no#aa$=3.6axio-7m

Chapter 3: Atomic Structure Overview SP2020

2

c. A helium laser emits light with a wavelength of 633 nm. What is the frequency of the light?

d. What is the wavelength of light with a frequency of 7.66 x 1014 Hz?

Part 2: Atomic Spectra, Particles of Light,

III. Definitions: Please use your textbook, notes, lecture PPT, or other resources to write the definition of each term.

• Fraunhofer Lines:

• Atomic Emission VS Atomic Absorption:

• Quantum:

• Planck Constant:

• Quantum Theory:

o Quantized:

o Photon:

IV. Calculating Energy Using E = h‧ν, E = -./ , h = 6.626 x !"(01 J‧s

a. Calculate the energy of a photon of radiation with a frequency of 8.5 x 10)2 Hz.

b. Calculate the energy of a gamma ray photon whose frequency is 4.05 x 10*3 Hz.

c. What is the energy of light whose wavelength is 4.06 x 10()) m?

6.33×10-7mm

v= Tf , 3 x108 m/s

mm

¥¥ = 4.74×10"

Az

-✓ r

YI =x -- I . 37%4704%31--3 .

aaxio -7

a set of dark lines in the otherwise continuous solar spectrum

Emission - characteristic patterns of brigades produced when atoms are vaporized in high-temp. flames or electrical

Absorption- characteristic patterns of dark lines produced when an extremal source q radiation passesthrough discharges

free f gaseous atoms

Smallest discrete quantity of a particular poem of energy

(h) proportionality constant between the energy and frequency q(Mao Planck) electromagnetic radiation expressed

in E-ha,h = 6.626×10

-34J.s

a model based on the idea that energy is absorbed and emitted in discrete

quantities ofenergy called quanta.

having values restricted to whole number multiples of a specificbase value

a quantum of electromagnetic radiation

•*o

E-hv =/6 .

626×10-34JOH ( 8 . 5×10's

=5

.

63×10-18 J

E-hv = ( 6.626×10-34 (4.05×10204/3) = 2.68 x 10-13

E-had = 16.626×10-3457131108451 = 4.89×10-15J4.06 x 10-"m

Chapter 3: Atomic Structure Overview SP2020

3

d. One of the electron transitions in a hydrogen atom produces infrared light with a wavelength of 7.464 × 10-6 m. What amount of energy causes this transition?

Part 3: Photoelectric Effect

V. Definitions: Please use your textbook, notes, lecture PPT, or other resources to write the definition of each term.

• Photoelectric Effect –

• Threshold Frequency (v0) –

• Work Function (φ) –

o Equation:

o E.g. The work function of lead is 4.27 x 10()4 J.

§ What is the minimum frequency of radiation required to eject photoelectrons from a lead surface?

§ Could visible light produce the photoelectric effect in lead?

Part 4: Hydrogen Spectrum and Bohr Model

VI. Definitions/People: Please use your textbook, notes, lecture PPT, or other resources to write the definition of each term.

• Johannes Robert Rydberg –

o Equation:

• Johann Balmer –

• Niels Bohr –

o Equation –

• Ground State –

• Excited State –

E- hfeduryy.YII.to#otzYn;MI= "c;9%9Y%m, = a.uomo-" t

the release of electrons from material as aresult of electromagnetic radiation striking it

the minimum frequency of light required to produce thephotoelectric effect

the amount of energy needed to dislodge an electron from the surface

of a material

to = huo

-

E-¥ = Vo - I = " f. s -- 6.44×10"

Az

Bohr's Modeln- 4

- n=3

.¥.

n' Ina.

Kiss is n"

published amore general empirical equation nucleus

I 1854- 1919)for predicting wavelengths of hydrogen

's spectral lines• -

• FEET¥ - RH ( Ip -⇒ •

Rits l .097 x I O-Znm" •

formulated an empirical equation that predicts( 1825- 1898) wavelength

x.tn:951Brackettseries

Bohr's Model - why hydrogen atoms hose and gain discretequanta A pashen( 1885- 1962) energy ( infrared)

-whytheir electrons do not spiralinto their nuclei

Balmer

E- -2.178×10- "J Lutz) (visible light)

A E- -2.178×10-''J ( http -⇒

the most stable,lowest energystate of

a particle

any energy above the ground state

Lyman(ultraviolet)

Chapter 3: Atomic Structure Overview SP2020

4

• Electron Transition –

VII. Calculating Energy of a Transition Label whether it’s an emission or an absorption.

a. n = 5 à 4

b. n = 2 à 1

c. n = 1 à 3

d. n = 4 à 1

e. n = 5 à 3

Part 5: More Examples

Perform the following calculations. Be sure to highlight the frequencies (it will help you in part six).

1. A mysterious wave has a frequency of 2.5 x 1013 Hz. What is the corresponding wavelength?

2. Another mysterious wave is about the size of a butterfly, or 0.010 m. What is the frequency of this wave?

movement of an electronbetween energy levels

at -2.asxio-ish's,

-÷)AE -

-R" (Ta - ¥) = - 2.178×157 ( tf -⇒

= - 4.90×10-20

AE -2.178×10-'8J ( http -÷)

---2.178 xD

-'8J ( t - I,)= - I . 63×10-18 J

E-- -2.178×10'8J(T - f)

= I . 936×10-18J

E = -2 .178×10

" J (T - ⇒= -2

.04 x 10

-"J

E = -2 . I 78×10- ' 8J (gt-⇒

=- l . 55×10

- ' 9J

¥ =

C- iv. x -E = 1269711857¥02 . x =1.2×10-5 m

in

> Microwaves

a- f. = 2%76%412=3.0 no" Hz-

Chapter 3: Atomic Structure Overview SP2020

5

3. In a different type of wave, the energy per photon was determined to be 2.12 x 10-16 J. What is the frequency of this wave?

4. Yesterday in Tallahassee, a strange wave in the atmosphere affected people’s ability to hear deep sounds. If the wavelength was a one kilometer, how much energy per photon did the wave contain?

5. Scientists in Siberia detected a wave with an energy of 3.85 x 10-13 J/photon. What was the wavelength?

6. One of the six groups of waves has a wavelength about the size of a virus cell. The frequency associated with these types of waves is 1.9 x 1016 Hz. How much energy per photon is there in one of these waves? Also, what is the approximate length of a virus cell?

Part 6:

On the blank lines above or below the following diagram, write the frequency corresponding to the different waves. In the parentheses, write the question number from which the frequency value came from.

_________Hz( ) _______Hz( ) ________Hz( )

v-E-lfe.LY#iI=s.zoxio'7HzxITnkm--1000M 2

.

" ÷ t.io#st..sn..aa.o.xa....o...k:::÷o÷÷radiowaves-E-h.no#..r=f::sIToItII,

"""÷÷÷÷÷÷¥c.mgV= 5.81×1020 Hg

T

UltraE- h.ve/6.63xio-34J.dll.9x1OheYsXfX=Ev=2?a9Yf%71I= 1.26×10

- "J = 1.57×10-8M

:3?¥%o¥; 8×1020 s 1.9×10"

6fpppqgf 30×10"

2

3. 3.20×10"

Hz4. 2.99×10543S. 8×1020436. 1.9×10"Hz fa

-Gamma has the tfreqnency, toHB 2.99×105 4

Radiowaves hashed 3.20×10" g 2.5×10"

y

Chapter 3: Atomic Structure Overview SP2020

6

__________Hz( ) __________Hz( ) ________Hz( )