Notes One Unit Eight Molecules Cross Word Answers State the three laws that support the existence of atoms List the five principles of Dalton's atomic theory. Calculate the masses of atoms in amu and gram units. Describe how the atomic mass unit was chosen. Calculate Average Atomic Mass Reading Assignment Two unit Two Next Class ova.physics.ato/ ova.physics.ato/ Pages 72-81

Laws of proportions What is the proportion for(?)… H 2 O H 2 O 2 N 2 O 3 N 2 O 5 N 2 O N 2 O 4 2:1 1:1 2:3 2:5 2:1 1:2 Multiple Proportions Definite Proportions

Law of conservation of mass DEMO NaOH/HCl phenolphthalein on a balance NaOH(aq)+HCl(aq)  H 2 O(l)+NaCl(aq)

Law of conservation of mass 2H 2 (g) + 1O 2 (g)  2H 2 O(l) H= H= O= O= Mass is conserved! 3H 2 (g) + 1N 2 (g)  2NH 3 (l) N= H= 2C 2 H 6 (g)+ 7O 2 (g)  4CO 2 (g) + 6H 2 O(l) C= H= O= =14

Three laws that support the existence of atoms 1. Law of definite proportions 2. E=MC 2 3. Law of multiple proportions

List the five(Four?) principles of Dalton's atomic theory. 1.All matter is made of indivisible and indestructible atoms. 2. All atoms of a certain element are identical in mass and properties. 3. Compounds can be formed by using two or more different kinds of atoms. 4. A chemical reaction is a rearrangementof atoms.

Carbons Mass in amu and gram units 1 amu=1/12 C-12 1 C-12 mass = amu 1amu = X grams grams/Mole!

Mass Spectroscope Neon gas e -1 beam heating element negative grid NeNe Ne Ne Ne +1

Calculating Average Atomic Mass E amu % product C-12 C = = x x % % % ÷100.00= 12.01amu 4 sd5 sd4 sd 1201

Notes Two Unit Eight The Nucleus Quiz Average Atomic Mass Describe the evidence for the existence of electrons and their presence in atoms. Explain how Rutherford's experiments led to the discovery of the nucleus. Discuss atoms of different elements in terms of the numbers of electrons, protons, and neutrons they contain. Pages 82-90

Horse Shoe Magnet Vacuum Chamber

Potassium Gas- K(g) e -1 Beam To Vacuum Pump K +1 ions Vacuum Chamber Magnet FaceTo Vacuum Pump 39 K K K +1 K +1 K Photographic Plate

Calculating Average Atomic Mass E amu % product 79 Br 81 Br = = x x % % % ÷ = amu 5 sd6 sd5 sd = amu

Cathode Ray Demo Electrons(e -1 ) leave the cathode Cathode  e -1   Anode - +

Cathode Ray Devices

Van de Graff Demo Van de Graff generator   Leyden Jar

Millikan's oil-drop experiment Charge of e -1 is equal to x Coulombs. X-ray   (+) plate  (-) plate  perfume sprayer Oil drops  0 hole  battery 

Rutherford's experiments Characteristics of atoms Radium  Lead Gold Foil  Microscope  Alpha particle     10,000 atoms thick 7999  pass through mostly empty space Small(1/10,000), 4 2 He +2 dense, and heavy positive charge core +79  +2

Atoms and their electrons, protons, and neutrons Proton(P +1 ) + Neutrons(n 0 )= Mass #(Z) AZElementP +1 n0n0 SymbolName HydrogenH H H Oxygen 8 8O 16 8 Oxygen 2657 Iron 2631 Fe Iron

Nuclear Reactions A reaction, as in fission, fusion, or radioactive decay, that alters the energy, composition, or structure of an atomic nucleus U +n  1 0 Xe n 1 0 Sr Fission: Fusion: 1 0 n+ 7 3 Li  3 1 H He n Decay: U  234 Th He Alpha Decay Th  Pa + 0  Beta Decay(e -1 )

Notes Three Unit Eight The Structure of the Atom’s Shell Describe the nature of light and how it is produced. Explain how the wavelengths of light emitted by an atom provide information about electron energy levels. Flame Tests Lab B Pages 92-95

Atomic Model Rutherford model *Mostly Empty Space Very Small, Very Dense, Positive Charged, *Nucleus… Where were the electrons? What are the electrons doing? +

Particle Model of The Electron Neils Bohr e -1 found in the empty space. He used light to define their actions. e -1 region +

Electromagnetic Spectrum gamma ray X-ray UV IRradarFM TV Short wave AM Visible Light Short wavelength Long wavelength Low Energy High Energy

Bohr’s Model of the shell *Particle Model *Circular orbits * Hydrogen only Light’s Energy e -1

The Spectroscope Helium Tube slit Prism spectrograph Bright-line Emission Spectrum

Solar Spectrum  hydrogen  helium  mercury  uranium  (92 elements)

Spectrum Example #1 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

Spectrum Example #2 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

Spectrum Example #3 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

Spectrum Example #4 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

Identifying Elements with Flame Tests NaKLiBa

Notes Four Unit Eight Electron Arrangements For Elements Compare the atomic models of Rutherford and Bohr. Describe the quantum mechanical interpretation of electrons in atoms. State Pauli's exclusion Principle, the aufbau principle, and Hund's rule, and describe their roles in determining the electron configuration of atoms. Pages

Atomic Model Rutherford model *Mostly Empty Space Very Small, Very Dense, Positive Charged, *Nucleus… Where were the electrons? What are the electrons doing? + Quantum Amount Bohr model

De Broglie’s Wave model for Electrons Wave Nature Different solutions for e -1 actions. e -1 ’s act as a particle or a wave. e -1 ’s absorb or release Quantum Amount of NRG. Demo of waves on a string

Standing Waves

S Orbital X-axis y-axis z-axis

p Orbitals Shapes x-axis z-axis y-axis

p Orbitals Assembled x-axis z-axis y-axis

Quantum Model for The Shell of The Atom

Electron Order of Filling Aufbau principle fill the lowest energy level first

Orbital Filling Diagram Write the orbital filling diagram for Ne. How many electrons does Ne have? Final Answer Short Hand Answer 10 e -1        1s 2 2s 2 2p 6 [He] 2s 2 2p 6 attract

Orbital Filling Diagram Write the orbital filling diagram for Na. How many electrons does Na have? Final Answer Short Hand Answer 11 e -1        1s 2 2s 2 2p 6 [Ne] 3s 1 1 

Orbital Filling Diagram Write the orbital filling diagram for Cl. How many electrons does Cl have? Final Answer Short Hand Answer 17 e -1            1s 2 2s 2 2p 6 3s 2 3p 5 [Ne] 3s 2 3p 5

Notes Five Unit Eight Electron Dot diagrams Quantum Numbers Pages

Electron Dot Diagram for Neon        [He] 2s 2 2p 6 Ne ● ● ● ● ● ● ● ●

Electron Dot Diagram for Sodium        [Ne] 3s 1  Na ●

Electron Dot Diagram for Chlorine            [Ne] 3s 2 3p 5 ● ● ● ● ● ● ● Cl

Quantum Numbers Addresses for electrons Four numbers for each address No two addresses are the same First number is n=1, 2, 3, 4, 5, 6, 7(Distance From the Nucleus) Second number is l = 0, 1, 2, 3 s p d f Third number is m l = 0 = +1, 0, -1 = +2, +1, 0, -1, -2 = +3, +2, +1, 0, -1, -2, -3 p orbital d orbital f orbital Forth number is m s = +1/2 or -1/2 s orbital

NodalPlane

P orbital Nodal planes ( l =0) X-axis y-axis z-axis ?

P orbital Nodal planes ( l =1) x-axis z-axis y-axis

x y z Nodal planes ( l =2)

 n= l=l= m l =ms =ms = /2 Quantum Numbers l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

 n= l=l= m l =ms =ms = 310-1/2 Quantum Numbers l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

 n= l=l= m l =ms =ms = 700+1/2 Quantum Numbers l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

n=ml =ml =ms =ms = /2 l=l=  Quantum Numbers

Quantum Number for Last e -1 in In  n=5 l=l= 1ml=ml=+1 ms=ms=+1/2 Many e -1 does In have? 49 e -1 Short hand element? Kr Many e -1 does Kr have? 36 e -1    How many e -1 to account for? 13 e -1 Quantum #’s for Last e -1 Short-hand fills to where? Fill-in Valence13 e -1

Final quiz Review

Average Atomic mass quiz Example AMU Abundance(%) K K K X = ÷ 99.94= SD 0

Spectrum Example #3 n=1 n=2 n=3 n=4 n=5 n=6 energy RedOrangeYellow Green BlueindgoViolet Ground State Excited State Quantum Amount

Orbital Filling Diagram Write the orbital filling diagram for Cu. How many electrons does Cu have? Final Answer Short Hand Answer 29 e -1                1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 9 [Ar] 4s 2 3d 9 

Electron Dot Diagram for Selenium                [Ar] 4s 2 3d 10    4p 4 Se ● ● ● ● ● ●

Quantum Number for Last e -1 in Cd n=4 l=l= 2ml=ml=-2 ms=ms=-1/2 How many e -1 does Cd have? 48 e -1 Short hand element? Kr Many e -1 does Kr have? 36 e -1     How many e -1 to account for? 12 e -1 Quantum #’s for Last e -1 Short-hand fills to where? Fill-in Valence12 e -1 l = 0(s), 1(p), 2(d), 3(f) = m s = +1/2 or -1/2 =  

Nuclear Reactions U +n  1 0 Cs n 1 0 Rb Fission: Decay: U  235 Th He Alpha Decay

Wave model for shell of the atom

Hund's rule Hund's rule: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied.

Pauli's exclusion Principle