The Atom and Its Properties

The Atom and Its PropertiesChapter 4 NucleusChapter 5 Electron Configuration1Chapter 4 ObjectivesDescribe an atoms structure and differentiate among the particles that make it up.Identify the numbers associated with elements and explain their meaning .Realize that the number of protons in a nucleus defines an element.Calculate the average atomic mass given isotopes and relative abundance

2Last point will be Illustrated with Bead Activity later in the week.

2Chapter 4.1Daltons Atomic TheoryAtomChapter 4.2ElectronNucleusProtonNeutron

Chapter 4.3Atomic NumberIsotopeMass NumberAMU (Atomic Mass Unit)Average Atomic Mass

3Chapter 4 Vocabulary3Modern View of the AtomThe nucleus is where the protons and neutrons are located and contain most of the atoms mass.

44Protons, Neutrons and ElectronsParticleSymbolChargeRelative MassElectrone-1-1/1840Protonp+1+1Neutronn00~155Sometimes Atomic Symbols are Displayed as:

66Isotope ExamplesIsotopeAtomicNumberMassNumberNumberProtonsNumber NeutronNumber ElectronCr-52334222286245277Whats all this amu business?To simplify a system of indicating atomic masses since protons and neutrons have such extremely small masses, scientists have assigned the carbon-12 atom a mass of exactly 12 atomic mass units. (amu)

The mass of 1 amu (1/12 the mass of carbon-12) is very nearly equal to the mass of a single proton or neutron but not the same.

1 amu = 1.66 x 10-24 grams88Isotopes and Mass NumberYour text (p. 119) shows how to calculate the mass number for Cl given the % abundance of the isotopes.Lets do this for another element: Li6Li is 7.59 % abundant; 6.015 amu7Li is 92.41% abundant; 7.015 amu

Method 1: Use percentages. Think of this as a sample of 100 atoms.99In Tabular FormSpeciesMass (amu)Abundance%Mass x Abundance(Weighted share)6Li (isotope)6.0157.5945.657Li (isotope)7.01592.41648.26Li (100 atoms)100.00694.41Li (atom)6.941010The average mass of an atom is found by weighting the natural abundances of its isotopes.

Lithium (Method 2): Change % to fraction.6Li 6.015 amu 7.59% = 0.07597Li 7.015 amu 92.41% = 0.9241 Mass (amu) Frac abund Mass share Avg mass = 6.015 amu x 0.0759 = 0.46 amu 7.015 amu x 0.9241 = 6.48 amu 6.94 amu/atom11Average Atomic Mass11Displayed on Periodic Table

1212

1313Electrons in AtomsChapter 514Lot of notes for this chapter. Make Handouts.

Chapter 5 ObjectivesCompare wave and particle matters of lightSee how frequency of light emitted by an atom is unique to that atomCompare and contrast the Bohr and quantum mechanical models of the atomExpress the arrangements of electrons in atoms through orbital notations, electron configurations, and electron dot structures1515Chapter 5 VocabularyChapter 5.1Electromagnetic RadiationWavelengthFrequencyAmplitudeElectromagnetic SpectrumQuantumPhotoelectric EffectPhotonAtomic Emission Spectrum16Chapter 5.2Ground StateQuantum NumberQuantum Mechanical Model of the AtomAtomic OrbitalPrincipal Quantum NumberPrincipal Energy LevelEnergy Sublevel16Wave Nature of LightElectromagnetic radiation displays wavelike behavior as it travels through spaceWaves can be described by several common characteristics

1717Characteristics of a WaveWaves transfer energyProperties of waves:Frequency ( pronounced nu) - Number of vibrations per unit time Hz (cycle/second)Wavelength () - Distance between points on two consecutive wavesSpeed of wave is Frequency x wavelength Speed = x

Frequency is the number of waves that hit this point in one second.Amplitude1818Example of waves transferring energy: Hearing objects in a room vibrate from loud sound waves, ocean waves breaking on the shoreline.

Amplitude is the intensity of the wave. Wavelength and frequency do not affect the intensity. Think of intensity as the volume of a sound wave. The frequency (pitch) and wavelength are still the same, just louder.

Speed refers to how fast the wave moves along the x-axis. Use a surfing analogy.

Electromagnetic Spectrum

Note: All EM Radiation travels at 3.00 x 108 m/s1919Electromagnetic SpectrumThe speed of light (3.00 108 m/s) is the product of its wavelength and frequency c = .

2020

The Electromagnetic Spectrum all light is energy2121Electromagnetic SpectrumGamma Rays Highest frequency, shortest wavelength. Can pass through most substancesX Rays Lower frequency than Gamma rays. Can pass through soft body tissue but cant pass through bone.Ultraviolet (UV) Rays Part of sunlight that causes sunburn2222Our atmosphere (magnetosphere) filters out most of the high frequency light. Mostly just UV to IR waves get through.Electromagnetic SpectrumVisible Light Sensitive to our eyes. Allows us to see colorInfrared Less energy and longer wavelength than visible light. Felt as heat given off a heater or near a fireRadio Waves Lowest frequencies on the EM spectrum. Used by radio and over-the-air TV.2323l x n = cl = c/n= 3.00 x 108 m/s 6.0 x 104 /s l = 5.0 x 103 mIts a radio wave (~103 meters)

An electromagnetic wave has a frequency of 6.0 x 104 Hz.Convert this frequency into its corresponding wavelength. Which region of the EM spectrum does this correspond to?

7.12424PracticeProblemsWhat is the frequency of green light, which has a wavelength of 520 nm.A radio station broadcasts at 94.7 MHz. What is the wavelength of the broadcast?Answers2525Nature of LightMax Planck (1858-1947) studied the different light emitted from heated objectsMatter can only gain or lose energy in small specific amounts

2626Nature of LightA quantum is the minimum amount of energy that can be gained or lost by an atomThe energy of EM radiation is proportional to its frequency (E )2727PhotonsAlbert Einstein (1879-1955) proposed that while a beam of light had wavelike characteristics, it also can be thought of as a stream of tiny particles (or bundles of energy) called photonsEach photon carries a quantum of energy

2828Particle Nature of LightThe photoelectric effect is when electrons are emitted from a metals surface when light of a certain frequency shines on it.

2929E = h x nE = 6.63 x 10-34 (Js) x 1.95 x 1018 /sE = 1.29 x 10 -15 J

7.2When copper is bombarded with high-energy electrons, X rays are emitted. Calculate the energy (in Joules) of the X-rays if their frequency is 1.95 x 1018 Hz.

3030Each element has only certain specific frequencies of light that are emitted when atoms absorb energy and become excitedWhere do we see this?fireworksneon signsstarsCh. 5.2 Quantum Theory of the Atom3131Hydrogen Spectrum

3232Balmer PlotIn 1885, Johann Balmer observed the lines of the spectrum fit this surprisingly simple formula:

Where n1 =2 and n2 = 3, 4, 5, etc.

3333Balmer PlotRH is the slope of this line, 1.0972 x 107 m-13434Electronic Energy TransitionsNeils Bohr (1885-1962) proposed the model the hydrogen atom (1913) to explain the discreet nature of the hydrogen spectrum.

3535Electronic Energy TransitionsNeils Bohrs model the atom (1913)Electrons exist only in discrete, allowable energy levelsEnergy is involved in moving electrons from one energy level to anotherPrincipal quantum number (n) - specifies the electrons major energy levelThe lowest energy is n=1, the next lowest in n=2, etc. 3636Bohrs Model of the Atom (contd)37

Bohr suggested that an electron moves around the nucleus in only certain allowed circular orbits.n = 1n = 237Energy Absorption/Emission

38

3939Atomic Emission Spectra

4040Origin of Line Spectra

Balmer series41Transitions to n = 1 are in UV (Lyman series are high energy); transitions to n = 2 are in visible (Ballmer series medium energy); transitions to n = 3 are in IR (Paschen series are low energy) in IR

The bigger the line, the greater the energy (frequency) of the photon.

Notice that the energy levels get closer to each other the higher they go.

Note the difference between absorption of energy and emission of energy:

Absorption of energyelectron jumps upEmission of energy electron drops down

Do burning salts as a demo here. (Flame Tests Made Easy in demo folder)Then give out POGIL activity after next slide which shows spectra of other elements. Also, show them H2 gas tube & spectra while they are working on POGIL.

4242Schrodinger applied idea of e- behaving as a wave to the problem of electrons in atoms.He developed the WAVE EQUATIONSolution gives set of math expressions called WAVE FUNCTIONS.Treated electrons as wavelike particles that became the Quantum Mechanical Model of the Atom.

E. Schrodinger1887-1961Quantum or Wave Mechanics43

Wave motion: wave length and nodesQuantization in a standing wave44Waves

Hydrogen Atom Solution

Where:a0 is the Bohr Radius given by

Generalized Laguerre Polynomial

Constant = 2.18 x 10-18 Jm is mass of electron

a0 = 4oh2/me2m here is quantum number4545For a hydrogen atom the coefficient of 1/n2 is a constant of value 2.18 x 10-18 J

4646Atomic Orbitals-Hydrogen

4747OrbitalsNo more than 2 e- assigned to an orbitalOrbitals grouped in s, p, d (and f) sublevels

s orbitalsd orbitalsp orbitals48

s orbitalsd orbitalsp orbitalss orbitalsp orbitalsd orbitalsNo.orbs.No. e-135261049Energy Levels and SublevelsSublevels are grouped in energy level.Each energy level has a number called the PRINCIPAL QUANTUM NUMBER, n which indicates relative size and energy of the orbitalsRow on PT indicates n

50Energy Levels and Sublevels

n = 1n = 2n = 3n = 451QUANTUM NUMBERSThe shape, size, and energy of each orbital is a function of quantum numbers:n (principal) Energy Levell (angular) sublevel (s, p, d, or f) which is its shape

Note: There are other quantum numbers that we will NOT discuss in detail. The n and l are sufficient.52SymbolValuesDescription

n (principal)1, 2, 3, ..Orbital size and energy levell (angular) 0, 1, 2, 3, n-1Orbital shape s, p, d, f, n-1 or type (energy sublevel)

QUANTUM NUMBERSMore commonly noted as:53Levels and SublevelsWhen n = 1, then l = 0 Therefore, in n = 1, there is just 1 type of subleveland that sublevel has a single orbitalThis sublevel is labeled s (ess)Each level has 1 orbital labeled s, and it is SPHERICAL in shape.

54Types of Atomic Orbitals

55Types of Atomic Orbitals56

56s Orbitals Always SphericalDot picture of electron cloud in 1s orbital.

Surface density4r2y versus distanceSurface of 90% probability sphere See Active Figure 6.1357p OrbitalsThe three p orbitals lie 90o apart in space

582px Orbital

3px Orbital

59

Hydrogen-like Orbitals(at most two electrons/orbital)nSublevel(l)OrbitalsMax. Orbital n2Max Elec 2n21 ss122 s p spx, py, pz483s p d spx, py, pzdxy,dxz,dyz,dx2-y2, dz29184s p d fspx, py, pzdxy,dxz,dyz,dx2-y2, dz2And 7 f orbitals

16326060Chapter 5.3 Vocabulary61Electron configurationAufbau principlePauli Exclusion PrincipleHunds RuleValence ElectronElectron Dot Structure

61Electron ConfigurationsAn atoms electron configuration is the arrangements of electrons in the atom.Electrons are arranged to minimize energy.In other words, electrons fill up the lowest energies possible first. This is the Aufbau Principle.6262Assigning Electrons to AtomsElectrons generally assigned to orbitals of successively higher energy.For H atoms, E depends only on n.For many-electron atoms, energy depends on both n and l.63Energy Level Diagram of Hydrogen

6464Assigning Electrons to SubshellsIn H atom all subshells of same n have same energy. In many-electron atom:a) subshells increase in energy as value of n + l increases.b) for subshells of same n + l, subshell with lower n is lower in energy.65

Many-Electron Atoms Orbitals and Their Energies66

After playing the video, have the students do the Virtual Investigations lab Electron Configuration. Give a packet to each student in a group, but only collect 1/group. Make sure the one they hand in has all of their names on it. They can answer the questions in the packet from these notes, and their book (if they have it).

Later in class or next class I can briefly go over Aufbau and slides 84 96. Continue with valence electrons & Ch. 6.

I can also give The Atom and Its Properties WS 7 Notation and Dot Structure that they can work on too.

66Aufbau Diagram -- Filling Electron Orbitals 1s 2s 3s 4s 5s 6s 7s 8s

2p 3p 4p 5p 6p 7p

3d 4d 5d 6d 4f 5f67Havent gotten this far. What orbitals are being filled with elements 110-118?Start heren + l = 1n + l = 2n + l = 3n + l = 4n + l = 5n + l = 6n + l = 7n + l = 8The orbital with the lower n is lower in energy if the n+l number is the same.67Writing Atomic Electron ConfigurationsTwo ways of writing configs. One is called the spdf notation.11svalue of nvalue of lno. ofelectronsspdf notationfor H, atomic number = 168Pauli Exclusion PrincipleNo two electrons in the same orbital can have the same spin. One electron is spin up, the other is spin down.

69Writing Atomic Electron ConfigurationsTwo ways of writing configs. Other is called the orbital box notation.

It would be a violation of the Pauli exclusion principle to have both of these electrons as spin up or both as spin down.70Electron Configurations and the Periodic Table

71LithiumGroup 1 (1A)Atomic number = 31s22s1 3 total electrons

72Interactive Periodic TableGround State Electron Configurations73

.73CarbonGroup 14 (4A)Atomic number = 61s2 2s2 2p2 6 total electrons

Here we see for the first time HUNDS RULE. When placing electrons in a set of orbitals having the same energy, we place them singly as long as possible.

74Electron Configuration for Elements 11-1875

Noble gas notation uses noble gas symbols in brackets to shorten inner electron configurations of other elements.75

SodiumGroup 1 (1A)Atomic number = 111s2 2s2 2p6 3s1 or neon core + 3s1[Ne] 3s1 (uses noble gas notation)Note that we have begun a new period.All Group 1A elements have [core]ns1 configurations.76Electron Configurations and the Periodic Table

77Transition Metals

All 4th period elements have the configuration [argon] nsx (n - 1)dy and so are d-block elements.

CopperIronChromium78

79Electrons in Energy LevelsElectrons fill up levels from lowest energy to highest energy (Aufbau Principle)

Outermost electrons are called Valence Electrons.When atoms come close together it is the Valence Electrons that interact.

8080Valence ElectronsHow to determine which electrons are in outer shell?Write down electron configuration of an element in noble-gas configurationWhatever electrons are displayed in the highest energy shell (n) only are valence electrons (Main Group elements)8181Lewis Dot DiagramsHow do we represent Valence Electrons?By a Lewis Dot DiagramRules for Lewis Dot Diagrams:Use the Elemental SymbolUse 1 dot to represent each valence electronThe symbol represents the nucleus and all the inner (core) electrons. Examples: . .. .. Li, Be: , C, Cl:, :Ne: . .. ..8282Valence ElectronsExamplesO given by [He]2s22p4 so it has 6 valence electrons. Ga given by [Ar]3d104s24p1 has 3 valence electrons.8383Electron Dot Representation

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Sine(angle)

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Sheet1

Sine(angle)

Sheet2

Sheet3