cmcchapter05-100613132827-phpapp02

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Electrons in Atoms

Section 5.1 Light and Quantized

Energy

Section 5.2 Quantum Theory and

the Atom

Section 5.3 Electron Configuration

ExitClick a hyperlink or folder tab to view

the corresponding slides.


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Section 5.1 Light and Quantized Energy

Comparethe wave and particle natures of light.

radiation:the rays and particles alpha particles,beta particles, and gamma raysthat are emittedby radioactive material

Definea quantum of energy, and explain how it is

related to an energy change of matter.

Contrastcontinuous electromagnetic spectra and

atomic emission spectra.


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Section 5.1 Light and Quantized Energy(cont.)

electromagnetic radiation

wavelength

frequency

amplitude

electromagnetic spectrum

Light, a form of electronic radiation,has characteristics of both a wave anda particle.

quantum

Planck's constant

photoelectric effect

photon

atomic emission spectrum


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The Atom and Unanswered Questions

Recall that in Rutherford's model, theatoms mass is concentrated in the nucleusand electrons move around it.

The model doesnt explain how the electronswere arranged around the nucleus.

The model doesnt explain why negativelycharged electrons arent pulled into the

positively charged nucleus.


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The Atom and Unanswered Questions (cont.)

In the early 1900s, scientists observedcertain elements emitted visible light whenheated in a flame.

Analysis of the emitted light revealed that anelements chemical behavior is related to thearrangement of the electrons in its atoms.


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The Wave Nature of Light

Visible light is a type of electromagneticradiation, a form of energy that exhibitswave-like behavior as it travels throughspace.

All waves can be described by severalcharacteristics.


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The Wave Nature of Light (cont.)

The wavelength() is the shortestdistance between equivalent points on acontinuous wave.

The frequency() is the number of waves

that pass a given point per second.

The amplitudeis the waves height from theorigin to a crest.


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The speed of light (3.00 108

m/s) is theproduct of its wavelength and frequencyc = .


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Sunlight contains a continuous range ofwavelengths and frequencies.

A prism separates sunlight into a continuousspectrum of colors.

The electromagnetic spectrumincludes allforms of electromagnetic radiation.


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The Particle Nature of Light

The wave model of light cannot explain allof lights characteristics.

Matter can gain or lose energy only in small,specific amounts called quanta.

A quantumis the minimum amount of energythat can be gained or lost by an atom.

Plancks constanthas a value of6.626 1034J s.


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The Particle Nature of Light (cont.)

The photoelectric effectis when electronsare emitted from a metals surface whenlight of a certain frequency shines on it.


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The Particle Nature of Light (cont.)

Albert Einstein proposed in 1905 that lighthas a dual nature.

A beam of light has wavelike and particlelikeproperties.

A photonis a particle of electromagneticradiation with no mass that carries a quantumof energy.

Ephoton= h Ephotonrepresents energy.his Planck's constant.represents frequency.


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Atomic Emission Spectra

Light in a neon sign is produced whenelectricity is passed through a tube filledwith neon gas and excites the neon atoms.

The excited atoms emit light to release

energy.


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Atomic Emission Spectra (cont.)


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Atomic Emission Spectra (cont.)

The atomic emission spectrumof anelement is the set of frequencies of theelectromagnetic waves emitted by theatoms of the element.

Each elements atomic emission spectrum isunique.


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A. A

B. B

C. C

D. DA B C D

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Section 5.1 Assessment

What is the smallest amount of energythat can be gained or lost by an atom?

A. electromagnetic photon

B. beta particle

C. quanta

D. wave-particle


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A. A

B. B

C. C

D. DA B C D

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What is a particle of electromagneticradiation with no mass called?

A. beta particle

B. alpha particle

C. quanta

D. photon


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Section 5.2 Quantum Theory and the Atom

Compare the Bohr and quantum mechanical models

of the atom.

atom:the smallest particle of an element that retainsall the properties of that element, is composed ofelectrons, protons, and neutrons.

Explainthe impact of de Broglie's wave article duality

and the Heisenberg uncertainty principle on thecurrent view of electrons in atoms.

Identifythe relationships among a hydrogen atom's

energy levels, sublevels, and atomic orbitals.


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Section 5.2 Quantum Theory and the Atom(cont.)

ground state

quantum number

de Broglie equation

Heisenberg uncertaintyprinciple

Wavelike properties of electrons helprelate atomic emission spectra, energystates of atoms, and atomic orbitals.

quantum mechanical modelof the atom

atomic orbital

principal quantum number

principal energy level

energy sublevel


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Bohr's Model of the Atom

Bohr correctly predicted the frequency linesin hydrogens atomic emission spectrum.

The lowest allowable energy state of an atomis called its ground state.

When an atom gains energy, it is in anexcited state.


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Bohr's Model of the Atom (cont.)

Bohr suggested that an electron movesaround the nucleus only in certain allowedcircular orbits.


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Each orbit was given a number, called thequantum number.


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Hydrogens single electron is in then

= 1orbit in the ground state.

When energy is added, the electron moves tothe n= 2 orbit.


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Bohrs model explained the hydrogensspectral lines, but failed to explain anyother elements lines.

The behavior of electrons is still not fully

understood, but it is known they do not movearound the nucleus in circular orbits.


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The Quantum Mechanical Model of the Atom

Louis de Broglie (18921987)hypothesized that particles, includingelectrons, could also have wavelikebehaviors.


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The Quantum Mechanical Model of the Atom(cont.)

The figure illustrates that electrons orbit thenucleus only in whole-numberwavelengths.


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The de Broglie equationpredicts that allmoving particles have wave characteristics.

represents wavelengthshis Planck's constant.

mrepresents mass of the particle.represents velocity.


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Heisenberg showed it is impossible to takeany measurement of an object withoutdisturbing it.

The Heisenberg uncertainty principle

states that it is fundamentally impossible toknow precisely both the velocity and positionof a particle at the same time.

The only quantity that can be known is theprobability for an electron to occupy a certainregion around the nucleus.


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Schrdinger treated electrons as waves ina model called the quantum mechanicalmodel of the atom.

Schrdingers equation applied equally well to

elements other than hydrogen.


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The wave function predicts a three-dimensional region around the nucleuscalled the atomic orbital.


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Hydrogen Atomic Orbitals

Principal quantum number(n) indicatesthe relative size and energy of atomic

orbitals.

nspecifies the atoms major energy levels,

called the principal energy levels.


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Hydrogen Atomic Orbitals (cont.)

Energy sublevelsare contained within theprincipal energy levels.


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Each energy sublevel relates to orbitals ofdifferent shape.


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A. A

B. B

C. C

D. DA B C D

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Which atomic suborbitals have adumbbell shape?

A. s

B. fC. p

D. d


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A. A

B. B

C. C

D. D


A B C D

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Who proposed that particles could alsoexhibit wavelike behaviors?

A. Bohr

B. EinsteinC. Rutherford

D. de Broglie


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Applythe Pauli exclusion principle, the aufbau

principle, and Hund's rule to write electron

configurations using orbital diagrams and electron

configuration notation.

electron:a negatively charged, fast-moving particlewith an extremely small mass that is found in all formsof matter and moves through the empty spacesurrounding an atom's nucleus

Definevalence electrons, and draw electron-dot

structures representing an atom's valence electrons.


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Section 5.3 Electron Configuration(cont.)

electron configuration

aufbau principle

Pauli exclusion principle

Hund's rule

valence electrons

electron-dot structure

A set of three rules determines thearrangement in an atom.


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Ground-State Electron Configuration

The arrangement of electrons in the atomis called the electron configuration.

The aufbau principlestates that eachelectron occupies the lowest energy orbital

available.


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Ground-State Electron Configuration (cont.)


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The Pauli exclusion principlestates thata maximum of two electrons can occupy asingle orbital, but only if the electrons haveopposite spins.

Hunds rulestates thatsingle electrons with thesame spin must occupy eachequal-energy orbital before

additional electrons withopposite spins can occupythe same energy levelorbitals.


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Noble gas notation uses noble gassymbols in brackets to shorten innerelectron configurations of other elements.


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The electron configurations (for chromium,copper, and several other elements) reflectthe increased stability of half-filled andfilled sets of s and d orbitals.


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Valence Electrons

Valence electronsare defined aselectrons in the atoms outermost orbitals

those associated with the atoms highestprincipal energy level.

Electron-dot structureconsists of theelements symbol representing the nucleus,surrounded by dots representing theelements valence electrons.


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Valence Electrons (cont.)
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A. A

B. B

C. C

D. DA B C D

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In the ground state, which orbital does anatoms electrons occupy?

A. the highest available

B. the lowest availableC. the n= 0 orbital

D. the d suborbital


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A. A

B. B

C. C

D. D


A B C D

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The outermost electrons of an atom arecalled what?

A. suborbitals

B. orbitalsC. ground state electrons

D. valence electrons


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Chemistry Online

Study Guide

Chapter Assessment

Standardized Test Practice

Image Bank

Concepts in Motion
http://www.glencoe.com/http://www.glencoe.com/


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Section 5.1 Light and QuantizedEnergy

Key Concepts

All waves are defined by their wavelengths, frequencies,amplitudes, and speeds.c =

In a vacuum, all electromagnetic waves travel at thespeed of light.

All electromagnetic waves have both wave and particleproperties.

Matter emits and absorbs energy in quanta.Equantum = h


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Section 5.1 Light and QuantizedEnergy(cont.)

Key Concepts

White light produces a continuous spectrum. Anelements emission spectrum consists of aseries of lines of individual colors.


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Section 5.2 Quantum Theory andthe Atom

Key Concepts

Bohrs atomic model attributes hydrogens emissionspectrum to electrons dropping from higher-energy tolower-energy orbits.

E = E higher-energy orbit - E lower-energy orbit = E photon = h

The de Broglie equation relates a particles wavelengthto its mass, its velocity, and Plancks constant.

= h / m

The quantum mechanical model of the atom assumesthat electrons have wave properties.

Electrons occupy three-dimensional regions ofspace called atomic orbitals.


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Key Concepts

The arrangement of electrons in an atom is calledthe atoms electron configuration.

Electron configurations are defined by the aufbauprinciple, the Pauli exclusion principle, and Hunds rule.

An elements valence electrons determine the chemicalproperties of the element.

Electron configurations can be represented usingorbital diagrams, electron configuration notation, andelectron-dot structures.


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A. A

B. B

C. CD. D

A B C D

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The shortest distance from equivalentpoints on a continuous wave is the:

A. frequency

B. wavelengthC. amplitude

D. crest


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A. A

B. B

C. CD. D

A B C D

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The energy of a wave increases as ____.

A. frequency decreases

B. wavelength decreases

C. wavelength increases

D. distance increases


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A. A

B. B

C. CD. D

A B C D

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Atoms move in circular orbits in whichatomic model?

A. quantum mechanical model

B. Rutherfords modelC. Bohrs model

D. plum-pudding model


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A. A

B. B

C. CD. D

A B C D

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It is impossible to know precisely both thelocation and velocity of an electron at thesame time because:

A. the Pauli exclusion principle

B. the dual nature of light

C. electrons travel in waves

D. the Heisenberg uncertaintyprinciple


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A. A

B. B

C. CD. D

A B C D

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How many valence electrons does neonhave?

A. 0

B. 1C. 2

D. 3


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A. A

B. B

C. CD. D

A B C D

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Spherical orbitals belong to whichsublevel?

A. s

B. pC. d

D. f


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A. A

B. B

C. CD. D

A B C D

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What is the maximum number of electronsthe 1s orbital can hold?

A. 10

B. 2C. 8

D. 1


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A. A

B. B

C. CD. D

A B C D

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In order for two electrons to occupy thesame orbital, they must:

A. have opposite charges

B. have opposite spinsC. have the same spin

D. have the same spin and charge


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A. A

B. B

C. CD. D

A B C D

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How many valence electrons does boroncontain?

A. 1

B. 2C. 3

D. 5


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A. A

B. B

C. CD. D

A B C D

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What is a quantum?

A. another name for an atom

B. the smallest amount of energy

that can be gained or lost byan atom

C. the ground state of an atom

D. the excited state of an atom


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Figure 5.11 Balmer Series

Figure 5.12 Electron Transitions

Table 5.4 Electron Configurations and OrbitalDiagrams for Elements 110

Table 5.6 Electron Configurations andDot Structures
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