FRIDAY, SEPTEMBER 14, 2012 - TEST ch. 3
*Pick up calculators and have out 1 sheet of paper with your name on it
for test later, calculator, & your periodic table.
*Pick up new chapter 4 Notes packet.
*Have out 1) study guide answers, 2) Notes ch. 3 packet, 3) computer
review game sheet, & 4) quiz sheet to turn in.
*DO NOT turn in openers.
*Pick up computers and log-in to podcast page.
*Complete Questions #1-39 on computer & #40-50 on paper. Show all
work for #40-50 including t-charts for conversions and sentences or
complete statements for short answer and essays.
*I will be here after school now if you need to make up work; my
appointment can rescheduled.
*Complete Chemthink.com atomic structure & isotopes
*START Notes 4.1 using computers when done with test.
*HW: Read Section 4.1 and 4.2. This will be a quick chapter too.
TESTING probably a week from Tuesday
on ch. 4 Resources
Chapter menu
Copyright © by Holt, Rinehart and Winston. All rights reserved.
MONDAY - SEPT. 17, 2012 - OPENER #5
1. What is Avogadro’s Number?
2. Define a mole. What is the relationship between moles and the
weighted average mass number found on the periodic table?
3. How many moles are found in 130.8 grams of Zn? Show
work or explain.
CW: M&M & the mole mini-lab
CW: Notes 4.1 & 4.2 started if time
HW: Read ch. 4 and answer Section review pg. 103 #1-6 with
complete statements and explanations due TUESDAY.
*Be sure you make up test if absent Friday & turn in Notes ch.3,
including add’l page of notes, review game sheet, study guide
answers, & quiz sheet. Openers are being continued in ch.4
Chapter menu
Resources
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TUESDAY- SEPT. 18, 2012 - OPENER #6
1. How fast do electromagnetic waves travel if in a vacuum?
2. What is the formula for finding the wavelength?
3. The greater amount of energy corresponds to greater
frequency; how does the wavelength correspond?
4. What is meant by quantum (or quanta)?
HW: Read 4.2 and answer Sect. Review pg. 110 #1-4 due WED.
CW: Check HW pg. 103 #1-6
CW: Spectroscope Lab with line-emission spectra
CW: QUIZ 4.1 (10 questions) - 20 points
CW: Notes 4.2 completed & (chemthink.com if not done)
*See me if absent yesterday for make-up lab activity.
*Be sure you make up test if absent Friday & turn in Notes ch.3,
including add’l page of notes, review game sheet, study guide
answers, & quiz sheet. Openers are being continued in ch.4
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Resources
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How to Use This Presentation
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select “View” on the menu bar and click on “Slide Show.”
• To advance through the presentation, click the right-arrow
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• From the resources slide, click on any resource to see a
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Chapter 4
Arrangement of Electrons in Atoms
Table of Contents
Section 1 The Development of a New Atomic Model
Section 2 The Quantum Model of the Atom
Section 3 Electron Configurations
Chapter menu
Resources
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 4
Section 1 The Development of a New
Atomic Model
Objectives
• Explain the mathematical relationship among the
speed, wavelength, and frequency of
electromagnetic radiation.
• Discuss the dual wave-particle nature of light.
• Discuss the significance of the photoelectric effect
and the line-emission spectrum of hydrogen to the
development of the atomic model.
• Describe the Bohr model of the hydrogen atom.
Chapter menu
Resources
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4.1A
Models of the Atom
>
The Development of Atomic Models
The timeline shoes the development of atomic
models from 1803 to 1911.
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4.1A
Models of the Atom
>
The Development of Atomic Models
The timeline shows the development of atomic
models from 1913 to 1932.
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4.1A
Models of the Atom
The scale model shown is a
physical model. However, not
all models are physical. In fact,
several theoretical models of
the atom have been developed
over the last few hundred
years. You will learn about the
currently accepted model of
how electrons behave in
atoms.
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4.1A
Models of the Atom
>
The Development of Atomic Models
The Development of Atomic Models
What was inadequate about
Rutherford’s atomic model?
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4.1A
Models of the Atom
>
The Development of Atomic Models
Rutherford’s atomic model could not
explain the chemical properties of
elements.
Rutherford’s atomic model could not explain
why objects change color when heated.
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4.1
Physics and the Quantum
Mechanical Model
Neon advertising signs are
formed from glass tubes bent in
various shapes. An electric
current passing through the gas
in each glass tube makes the
gas glow with its own
characteristic color. You will
learn why each gas glows
with a specific color of light.
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Chapter 4
Section 1 The Development of a New
Atomic Model
Properties of Light
The Wave Description of Light
• Before 1900, scientists thought light
behaved solely as a wave. This
changed when light was found to have
particle-like characteristics as well.
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Resources
Copyright © by Holt, Rinehart and Winston. All rights reserved.
Chapter 4
Section 1 The Development of a New
Atomic Model
Properties of Light
The Wave Description of Light
• Electromagnetic radiation is a form of energy that
exhibits wavelike behavior as it travels through
space.
Chapter menu
Resources
Copyright © by Holt, Rinehart and Winston. All rights reserved.
4.1
Physics and the Quantum
Mechanical Model
>
Light
According to the wave model, light consists of
electromagnetic waves.
• Electromagnetic radiation includes radio
waves, microwaves, infrared waves, visible
light, ultraviolet waves, X-rays, and gamma
rays.
• All electromagnetic waves travel in a vacuum
at a speed of approximately 2.998  108 m/s
which we will round off to 3.0 x 108 m/s.
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Chapter 4
Section 1 The Development of a New
Atomic Model
Properties of Light
The Wave Description of Light
• Together, all the forms of electromagnetic radiation
form the electromagnetic spectrum.
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Resources
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4.1
Physics and the Quantum
Mechanical Model
>
Light
Sunlight consists of light with a continuous
range of wavelengths and frequencies.
• When sunlight passes through a prism, the
different frequencies separate into a
spectrum of colors as you observed in 9th
grade.
• In the visible spectrum, red light has the
longest wavelength and the lowest frequency.
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4.1
Physics and the Quantum
Mechanical Model
>
Light
The electromagnetic spectrum consists of
radiation over a broad band of wavelengths.
(ROY G. BIV)
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4.1
Physics and the Quantum
Mechanical Model
>
Atomic Spectra
A prism separates light into the colors it contains.
When white light passes through a prism, it
produces a rainbow of colors.
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End Show
Chapter 4
Visual Concepts
Electromagnetic Spectrum
Click below to watch the Visual Concept.
http://my.hrw.com/sh/hc6_0030
36809x/student/ch04/sec01/vc0
Visual Concept
0/hc604_01_v00fs.htm
Chapter menu
Resources
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4.1
Physics and the Quantum
Mechanical Model
>
Light
Light
How are the wavelength and frequency
of light related?
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End Show
Section 1 The Development of a New
Atomic Model
Chapter 4
Properties of Light, continued
• Wavelength ( ) is the distance between
corresponding points on adjacent waves.
crest to crest
or trough to trough
• Frequency (v) is defined as the number of waves that
pass a given point in a specific time, usually one
second.  (the Greek letter nu)
Chapter menu
Resources
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Chapter 4
Section 1 The Development of a New
Atomic Model
Wavelength and Frequency
Chapter menu
Resources
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4.1
Physics and the Quantum
Mechanical Model
>
Light
The wavelength and frequency of light
are inversely proportional to each other.
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End Show
Chapter 4
Section 1 The Development of a New
Atomic Model
Properties of Light, continued
• Frequency and wavelength are mathematically related
to each other:
c=v
• In the equation, c is the speed of light (in m/s),  is the
wavelength of the electromagnetic wave (in m), and v
is the frequency of the electromagnetic wave (in s 1).
Chapter menu
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4.1
Physics and the Quantum
Mechanical Model
>
Light
• The amplitude of a wave is the wave’s height from
zero to the crest.
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End Show
Physics and the Quantum
Mechanical Model
>
Light
CLICK HERE TO SEE SIMULATION
Simulation 3
Explore the properties of electromagnetic
radiation.
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End Show
SAMPLE PROBLEM 5.1
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SAMPLE PROBLEM 5.1
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SAMPLE PROBLEM 5.1
SHOW WORK IN YOUR NOTES!
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SAMPLE PROBLEM 5.1
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End Show
Practice Problems
for Sample Problem 5.1
TO CHECK WORK, CLICK BELOW.
CLICK HERE
Problem-Solving 5.15 Solve
Problem 15 with the help of an
interactive guided tutorial.
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Chapter 4
Section 1 The Development of a New
Atomic Model
The Photoelectric Effect
• The photoelectric effect refers to the emission
of electrons from a metal when light shines on
the metal.
The Particle Description of Light
• Planck said that the object emits energy in small
specific packets called quanta. A quantum of
energy is the minimum quantity of energy that
can be lost or gained by an atom.
• (quanta - is plural for quantum)
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Chapter 4
Section 1 The Development of a New
Atomic Model
Photoelectric Effect
Chapter menu
Resources
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Chapter 4
Visual Concepts
Photoelectric Effect
Click below to watch the Visual Concept.
http://my.hrw.com/sh/hc6_003036809x/student/ch0
Visual Concept
4/sec01/vc01/hc604_01_v01fs.htm
Chapter menu
Resources
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Chapter 4
Visual Concepts
Energy of a Photon
Click below to watch the Visual Concept.
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Visual Concept
ch04/sec01/vc03/hc604_01_v03fs.htm
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Chapter 4
Section 1 The Development of a New
Atomic Model
The Photoelectric Effect, continued
The Particle Description of Light, continued
• German physicist Max Planck proposed the following
relationship between a quantum of energy and the frequency
of radiation:
E = hv
• E is the energy, in joules, of a quantum of radiation, v is
the frequency, in s−1, of the radiation emitted, and h is a
fundamental physical constant now known as Planck’s
constant; h = 6.626  10 34 J• s.
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Chapter 4
Section 1 The Development of a New
Atomic Model
The Photoelectric Effect, continued
The Particle Description of Light, continued
• Einstein said that electromagnetic
radiation has a dual wave-particle
nature. Light exhibits many wavelike
properties; it can also be thought of as a
stream of particles.
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Chapter 4
Section 1 The Development of a New
Atomic Model
The Photoelectric Effect, continued
The Particle Description of Light, continued
• A photon is a particle of electromagnetic
radiation having zero mass and carrying a
quantum of energy.
• The energy of a particular photon depends on the
frequency of the radiation.
Ephoton = hv
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4.1
Physics and the Quantum
Mechanical Model
>
Quantum Mechanics
Quantum Mechanics
How does quantum mechanics differ
from classical mechanics?
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4.1
Physics and the Quantum
Mechanical Model
>
Quantum Mechanics
In 1905, Albert Einstein successfully explained
experimental data by proposing that light could
be described as having a dual wave-particle
nature. Light exhibits many wavelike properties;
it can also be thought of as a stream of particles.
• The quanta behave as if they were particles.
• Light quanta are called photons.
In 1924, De Broglie developed an equation that
predicts that all moving objects have wavelike
behavior.
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4.1
Physics and the Quantum
Mechanical Model
>
Quantum Mechanics
Today, the wavelike properties of beams of
electrons are useful in magnifying objects. The
electrons in an electron microscope have much
smaller wavelengths than visible light. This
allows a much clearer enlarged image of a very
small object, such as this mite.
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Physics and the Quantum
Mechanical Model
>
Quantum Mechanics
Simulation 4
Simulate the photoelectric effect. Observe the
results as a function of radiation frequency
and intensity.
NOT LOADING ON 9-13-12 at school or at home????
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4.1A
Models of the Atom
>
The Bohr Model
The Bohr Model
What was the new proposal in the Bohr
model of the atom?
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4.1A
Models of the Atom
>
The Bohr Model
Bohr proposed that an electron is found
only in specific circular paths, or orbits,
around the nucleus.
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Chapter 4
Section 1 The Development of a New
Atomic Model
Bohr Model of the Hydrogen Atom
• Niels Bohr proposed a hydrogen-atom model that
linked the atom’s electron to photon emission.
• According to the model, the electron can circle the
nucleus only in allowed paths, or orbits.
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4.1A
Models of the Atom
>
The Bohr Model
Each possible electron orbit in Bohr’s model has
a fixed energy.
• The fixed energies an electron can have are
called energy levels.
• A quantum of energy is the amount of energy
required to move an electron from one energy
level to another energy level.
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4.1A
Models of the Atom
>
The Bohr Model
Like the rungs of the
strange ladder, the
energy levels in an atom
are not equally spaced.
The higher the energy
level occupied by an
electron, the less energy
it takes to move from
that energy level to the
next higher energy level.
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Chapter 4
Visual Concepts
Quantization of Energy
Click below to watch the Visual Concept.
http://my.hrw.com/sh/hc6_003036809x/student
Visual Concept
/ch04/sec01/vc02/hc604_01_v02fs.htm
Chapter menu
Resources
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Chapter 4
Section 1 The Development of a New
Atomic Model
Bohr Model of the Hydrogen Atom
• The energy of the electron is higher when the
electron is in orbits that are successively farther
from the nucleus.
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Bohr Model
The electron is in the lowest energy state
when it is in the orbit closest to the nucleus.
When an electron is in an orbit farther
from the nucleus it is in an excited state.
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Chapter 4
Visual Concepts
Bohr Model of the Atom
Click below to watch the Visual Concept.
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Visual Concept
x/student/ch04/sec01/vc05/hc604_01_
v05fs.htm
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Chapter 4
Section 1 The Development of a New
Atomic Model
Bohr Model of the Hydrogen Atom, continued
• When an electron falls to a lower energy level, a
photon is emitted, and the process is called
emission.
• Energy must be added to an atom in order to move
an electron from a lower energy level to a higher
energy level. This process is called absorption.
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Chapter 4
Visual Concepts
Absorption and Emission Spectra
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Visual Concept
dent/ch04/sec01/vc04/hc604_01_v04fs.htm
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Chapter 4
Section 1 The Development of a New
Atomic Model
Photon Emission and Absorption
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Chapter 4
Section 1 The Development of a New
Atomic Model
The Hydrogen-Atom Line-Emission Spectrum
• The lowest energy state of an atom is its ground
state.
• A state in which an atom has a higher potential
energy than it has in its ground state is an
excited state.
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Chapter 4
Section 1 The Development of a New
Atomic Model
The Hydrogen-Atom Line-Emission Spectrum,
continued
• When investigators passed electric current
through a vacuum tube containing hydrogen gas
at low pressure, they observed the emission of a
characteristic pinkish glow.
• When a narrow beam of the emitted light was
shined through a prism, it was separated into
four specific colors of the visible spectrum.
• The four bands of light were part of what is
known as hydrogen’s line-emission spectrum.
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Chapter 4
Section 1 The Development of a New
Atomic Model
Hydrogen’s Line-Emission Spectrum
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4.1
Physics and the Quantum
Mechanical Model
>
Atomic Spectra
The frequencies of light emitted by an
element separate into discrete lines to give
the atomic emission spectrum of the
element.
Mercury
Nitrogen
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Section 1 The Development of a New
Atomic Model
Chapter 4
The Hydrogen-Atom Line-Emission Spectrum,
continued
• Each element has it’s own line-emission
spectrum where a beam of light is separated in
specific colors of the visible spectrum.
• The emission of a continuous range of frequencies
of electromagnetic radiation is a continuous
spectrum.
• Whenever an excited hydrogen atom falls to its
ground state, it emits a photon of radiation.
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4.1
Physics and the Quantum
Mechanical Model
>
Atomic Spectra
When light from a helium lamp passes through a
prism, discrete lines are produced. Each
element has it’s own spectrum.
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Physics and the Quantum
Mechanical Model
>
An Explanation of Atomic Spectra
Animation 6
Learn about atomic emission spectra and
how neon lights work.
THIS ANIMATION WOULD NOT LOAD 9-13-12 at home.
I’LL SHOW REAL DEMONSTRATION WITH LINE SPECTRA WITH
SPECTROSCOPES IN CLASS THIS WEEK FROM DIFFERENT GASES.
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4.1A
Models of the Atom
>
The Quantum Mechanical Model
The Quantum Mechanical Model
What does the quantum mechanical
model determine about the electrons in
an atom?
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4.1A
Models of the Atom
>
The Quantum Mechanical Model
QUANTUM MECHANICAL MODEL
The quantum mechanical model
determines the allowed energies an
electron can have and how likely it is to
find the electron in various locations
around the nucleus.
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4.1A
Models of the Atom
>
The Quantum Mechanical Model
Austrian physicist Erwin Schrödinger (1887–
1961) used new theoretical calculations and
results to devise and solve a mathematical
equation describing the behavior of the electron
in a hydrogen atom.
The modern description of the electrons in
atoms, the quantum mechanical model, comes
from the mathematical solutions to the
Schrödinger equation.
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4.1A
Models of the Atom
>
The Quantum Mechanical Model
The propeller blade has the same probability
of being anywhere in the blurry region, but
you cannot tell its location at any instant. The
electron cloud of an atom can be compared to
a spinning airplane propeller.
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4.1A
Models of the Atom
>
The Quantum Mechanical Model
In the quantum mechanical model, the
probability of finding an electron within a
certain volume of space surrounding the
nucleus can be represented as a fuzzy cloud.
The cloud is more dense where the probability
of finding the electron is high.
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4.1A Section Quiz.
Assess students’ understanding of
the concepts in Section
5.1.
Continue to:
-or-
Launch:
Section Quiz
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4.1A Section Quiz.
1. Rutherford's planetary model of the atom
could not explain
a. any properties of elements.
b. the chemical properties of elements.
c. the distribution of mass in an atom.
d. the distribution of positive and negative
charges in an atom.
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4.1A Section Quiz.
2. Bohr's model of the atom proposed that
electrons are found
a. embedded in a sphere of positive charge.
b. in fixed positions surrounding the nucleus.
c. in circular orbits at fixed distances from the
nucleus.
d. orbiting the nucleus in a single fixed
circular path.
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4.1A Section Quiz.
3. What is the lowest-numbered principal energy
level in which p orbitals are found?
a. 1
b. 2
c. 3
d. 4
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Chapter 4
Visual Concepts
Comparing Models of the Atom
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Visual Concept
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5.3 Section Quiz.
1. Calculate the frequency of a radar wave with
a wavelength of 125 mm.
a. 2.40 109 Hz
b. 2.40 1024 Hz
c. 2.40 106 Hz
d. 2.40 102 Hz
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5.3 Section Quiz.
2. The lines in the emission spectrum for an
element are caused by
a. the movement of electrons from lower to
higher energy levels.
b. the movement of electrons from higher to
lower energy levels.
c. the electron configuration in the ground
state.
d. the electron configuration of an atom.
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5.3 Section Quiz.
3. Spectral lines in a series become closer
together as n increases because the
a. energy levels have similar values.
b. energy levels become farther apart.
c. atom is approaching ground state.
d. electrons are being emitted at a slower
rate.
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Physics and the Quantum
Mechanical Model
>
Concept Map 5
Concept Map 5 Solve the
concept map with the help of an
interactive guided tutorial.
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Online Self-Check Quiz
Complete the online 4.1 Quiz and record
answers. Ask if you have any questions
about your answers.
click here for online Quiz 4.1
(10 questions)
You must be in the “Play mode” for the
slideshow for hyperlink to work.
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VIDEOS FOR ADDITIONAL INSTRUCTION
Additional Videos for Section 4.1 The Development of a New Atomic Model
Electromagnetic Spectrum (9:55)
Photoelectric Effect (7:36)
Wavelength (5:50)
Frequency - Period (4:37)
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