Bohr Diagrams or Shell Models

Bohr Diagrams or Shell Models
11 Na Sodium 23 Bohr Diagrams or Shell Models - +11 Model of an atom which has a nucleus surrounded by electrons in their energy levels. Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

2-8-8-2 rule 2 8 8 2 Put the number of protons in the nucleus.
First two electrons go in the first energy level or ring around the atom. The next eight go into the next energy level and so on… This works for the first 20 elements. 2 8 8 2 Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

Valence Electrons Electrons in the outermost ring are considered to be the most important because when two atoms come near one another it is these valence electrons and outer shells that interact. Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

Assignment 2-8-8-2 rule #VEs Hydrogen Helium Carbon Neon Chlorine Cl1-
Nitrogen N3- Li1+ Magnesium Iron Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

What color is the sun? Electrons…explain light
Why things come together

Contrary to popular belief, the sun is actually white!
When viewed from outside our atmosphere the sun appears white.

The Sun as Seen by ISS Why? Image via Nasa.gov

RAINBOWS! How does a Rainbow Form

White Light is Composed of all Colors: ROY G BIV
PRISM WHITE LIGHT

White Light is Composed of all Colors: ROY G BIV
PRISM How Does a Prism Work? As light enters a new material or medium (e.g. from air to glass) it changes speed which causes it to bend or refract. Different colors of light bend different amounts. Thus, white light separated into a full rainbow of colors.

Simple Refraction Demo
Arrow and a glass cup.

Why Does the Sun Appear to be Yellow?
A simple explanation is that all the particles in our atmosphere filter out all the colors but yellow making the sun appear yellow. Likewise, grass is green because the pigment chlorophyll inside of grass is very good at absorbing blue and red light, leaving the green to be reflected.

EARTH Why are Sunrises and Sunsets Red/Orange?
At dawn/dusk the sun has to travel through a longer path in the atmosphere to reach us which scatters out the blue normally making up our sky color. X EARTH The size of our atmosphere is EXTREMELY exaggerated!

If Earth was the Size of an Apple
The atmosphere would be much thinner than the skin on the apple. The atmosphere is about 60 miles thick whereas earth has a radius of about 4,000 miles.

RAINBOW How Does a Rainbow Form?
WHITE LIGHT Sunlight strikes water droplets in the atmosphere. The water droplets behave like a prism and separate the light into a full rainbow of colors. THE SUN MUST BE AT YOUR BACK TO SEE A RAINBOW

As white sunlight enters a raindrop it refracts into a full spectrum of color.
The light will then reflect or bounce off the opposite side of the drop and exit on the same side it entered (refracting again!) Refraction Reflection Refraction

Activity: Grab a spectroscope and use it to look at the following:
Sunlight (not directly) Fluorescent Light Helium Tube Oxygen Tube Hydrogen Tube Krypton Tube Use colored pencils and markers to draw the spectral lines (color pattern). Image via openstax When light passes through a diffraction grating (slit) of a certain size it the light separates into its respective colors. In this unit we want to understand what creates light and why each element has a unique set of spectral lines. In order to do that we need to take a deeper look at electrons… Angular momentum quantum number, magnetic quantum number, nodes….

Spectroscopic Analysis
Astronomy! We can’t get to the stars so spectral analysis is crucial to understand what these objects are made of. Helium was discovered on the sun before it was found on Earth.

How Light Forms 2-8-8-2 rule [1] Energy strikes an atom
[2] Electrons in their grounds state become excited and jump up to a higher energy level Light [3] Electrons in higher energy levels are unstable. They drop back down to their ground state and emit the energy they absorbed. Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding) [4] That energy is emitted as photons or small packets of light

Wave Mechanical Atom (Lab)
Understanding electrons allows us to understand light and how and why atoms join together. Electron location is based upon probability. Electrons orbits are quantized. Planetary Orbits Electrons are little circles

Each Floor is an energy level and each person an electron.
S(2) P(6) D(10) F(14) 2882 rule? Energy Level Orbitals Electrons Energy Level 5 (n=5) SPDF 32 Energy Level 4 (n=5) SPDF 32 Energy Level 3 (n=3) SPD 18 Energy Level 2 (n=2) SP 8 S.H.H.S. Energy Level 1 (n=1) S 2

STUDENTS PLEASE DON’T FART
S (2 electrons) P (6 electrons) D (10 electrons) F (14 electrons) Have students repeat and chant this

Writing the standard, ground state electron configuration order.
Draw the numbers 1-7 down and put an s after them Draw the numbers 2-7 and put a p after them. Draw the numbers 3-7 and put a d after them Draw the numbers 4-7 and put an f after them Inset arrows diagonally starting with the 1s Follow the the arrows (top to bottom) and write the order out. Now insert the SPDF numbers as exponents. Aufbau Principle S(2) P(6) D(10) F(14) 2p 3p 4p 5p 6p 7p 3d 4d 5d 6d 7d 4f 5f 6f 7f 1s 2s 3s 4s 5s 6s 7s 1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p Writing the standard, ground state electron configuration order. Write out Triangle and then the Stanard Ground state E-Config 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d107p6

Containers that hold electrons
Orbital shape Containers that hold electrons 1s2 # of Electrons Energy Level 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d10

1s2 2s2 2p6 3s2 3p6 These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital 13 Al Aluminum 27 e e e e e e e e e e e e e

1s2 2s2 2p6 3s2 3p6 e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital 13 Al Aluminum 16 e e e e e e e e e e e

1s2 2s2 2p6 3s2 3p6 e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital The second two go in the 2s orbital 13 Al Aluminum 16 e e e e e e e e e

1s2 2s2 2p6 3s2 3p6 e e e e e e e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital The second two go in the 2s orbital The next six go in the 2p orbital 13 Al Aluminum 16 e e e

1s2 2s2 2p6 3s2 3p6 e e e e e e e e e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital The second two go in the 2s orbital The next six go in the 2p orbital The next two go in the 3s orbital 13 Al Aluminum 16 e

1s2 2s2 2p6 3s2 3p6 e e e e e e e e e e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital The second two go in the 2s orbital The next six go in the 2p orbital The next two go in the 3s orbital The last electron goes in the 3p orbital 13 Al Aluminum 16

1s2 2s2 2p6 3s2 3p6 1s22s22p63s23p1 e e e e e e e e e e e e e
These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Aluminum has 13 electrons The first two electrons go in the 1s orbital The second two go in the 2s orbital The next six go in the 2p orbital The next two go in the 3s orbital The last electron goes in the 3p orbital 13 Al Aluminum 16 1s22s22p63s23p1 Electron Configuration of Aluminum

1s2 2s2 2p6 3s2 3p6 These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital 8 O Oxygen 16 e e e e e e e e

1s2 2s2 2p6 3s2 3p6 e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital 8 O Oxygen 16 e e e e e e

1s2 2s2 2p6 3s2 3p6 e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital The next to go in the 2s oribtal 8 O Oxygen 16 e e e e e e

1s2 2s2 2p6 3s2 3p6 e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital The next to go in the 2s oribtal 8 O Oxygen 16 e e e e

1s2 2s2 2p6 3s2 3p6 e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital The next to go in the 2s oribtal The next 4 go in the 2p orbital 8 O Oxygen 16 e e e e

1s2 2s2 2p6 3s2 3p6 e e e e e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital The next to go in the 2s oribtal The next 4 go in the 2p orbital 8 O Oxygen 16

1s2 2s2 2p6 3s2 3p6 e e e e e e e e These orbitals are like containers that hold electrons. You must fill up one container before moving to the next. Oxygen has 8 electrons The first two electrons go in the 1s orbital The next to go in the 2s oribtal The next 4 go in the 2p orbital 8 O Oxygen 16 1s22s22p4

Practice Configuration and Boxes
Hydrogen Oxygen Fluorine Neon-21 Al3+ You have to fill up one orbital before going into the next one! HANDOUT 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d10

We are going to talk about bonding Bonding between atoms is CIM
Water sugar salt We are going to talk about bonding Bonding between atoms is CIM Why do 2h and OThere are several difference bond types in Chemistry. All are concerned with electrons. Intermolecular bonds occur between molecules (hydrogen bonding)

Pauli Exclusion Principle
Hund’s Rule Pauli Exclusion Principle Aufbau Principle __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s s p s p s d p s d p s f14 PEP: two electrons in same sub-orbital MUST have opposite spins…not just electrons but all fermions… Hund’s Rule: electrons fill each orbitql before pairing up (city bus analogy… take empty seat before pairing…) Aufbaul: electrons fill low energy to high Neon Sulfur Krypton Oxygen Nitrogen Mg2+ S2- 14C Up and Down Arrows denote electrons and their spin. Fill in the diagram and write out the electron configuration Look up Hund’s Rule and the Pauli Exclusion Principle!

7s2 6p6 5d10 6s2 4f14 5p6 5s2 4d10 4p6 4s2 3d10 3p6 3s2 2p6 2s2 Hydrogen Nitrogen Sodium Potassium Rubidium Caesium 1s2

Valence Electrons 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 7p 3d 4d 5d 6d
4f 5f 6f 7f Electrons in the outermost energy level of an atom. The most important electrons in an atom, they determine chemical bonds and properties. They are the furthest from the Nucleus and therefore, when two atoms/molecules come into contact with one another it is the outer electrons that interact first. Nucleus super dense, mostly empty space….electrons interact 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f146d10

1s22s22p63s23p64s23d104p65s2… Determine the number of Valence Electrons Carbon Neon Argon Iron First you need to determine the total number of electrons each element has. You need to write out its ground state electron configuration. Count the number of electrons in the highest energy level.

1s22s22p63s23p64s23d104p65s2… Determine the number of Valence Electrons Carbon 1s22s22p2 =4 Neon 1s22s22p6 =8 Argon 1s22s22p63s23p6 =8 Iron 1s22s22p63s23p64s23d6 =2 First you need to determine the total number of electrons each element has. You need to write out its ground state electron configuration. Count the number of electrons in the highest energy level. Handout

Column Number 1A-8A is the number of Valence electrons
Selenium Tin Strontium Krypton Iodine Potassium Sodium Gallium How Many Valence Electrons?

All column 1A elements have 1 valence electron
Hydrogen 1.0079 Alkali Metals Alkaline Earth Metals Transition Metals Lanthanides Actinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium 4.003 3 Li Lithium 6.941 4 Be Beryllium 9.0122 5 B Boron 10.811 6 C Carbon 12.011 7 N Nitrogen 14.007 8 O Oxygen 15.999 9 F Fluorine 18.998 10 Ne Neon 20.180 11 Na Sodium 22.990 12 Mg Magnesium 24.305 13 Al Aluminum 26.982 14 Si Silicon 28.086 15 P Phosphorus 30.974 16 S Sulfur 32.066 17 Cl Chlorine 35.453 18 Ar Argon 39.948 19 K Potassium 39.098 20 Ca Calcium 40.078 21 Sc Scandium 44.956 22 Ti Titanium 47.88 23 V Vanadium 50.942 24 Cr Chromium 51.996 25 Mn Manganese 54.938 26 Fe Iron 55.933 27 Co Cobalt 58.933 28 Ni Nickel 58.693 29 Cu Copper 63.546 30 Zn Zinc 65.39 31 Ga Gallium 69.732 32 Ge Germanium 72.61 33 As Arsenic 74.922 34 Se Selenium 78.09 35 Br Bromine 79.904 36 Kr Krypton 84.80 37 Rb Rubidium 85.468 38 Sr Strontium 87.62 39 Y Yttrium 88.906 40 Zr Zirconium 91.224 41 Nb Niobium 92.906 42 Mo Molybdenum 95.94 43 Tc Technetium 98.907 44 Ru Ruthenium 101.07 45 Rh Rhodium 46 Pd Palladium 106.42 47 Ag Silver 48 Cd Cadmium 49 In Indium 50 Sn Tin 118.71 51 Sb Antimony 52 Te Tellurium 127.6 53 I Iodine 54 Xe Xenon 131.29 55 Cs Cesium 132.91 56 Ba Barium 137.33 * 57-71 72 Hf Hafnium 178.49 73 Ta Tantalum 74 W Tungsten 183.85 75 Re Rhenium 76 Os Osmium 190.23 77 Ir Iridium 192.22 78 Pt Platinum 195.08 79 Au Gold 80 Hg Mercury 200.59 81 Tl Thallium 82 Pb Lead 207.2 83 Bi Bismuth 84 Po Polonium [ ] 85 At Astatine 86 Rn Radon 87 Fr Francium [223] 88 Ra [226] ** 89-103 104 Rf Rutherfordium [261] 105 Db Dubnium [262] 106 Sg Seaborgium [266] 107 Bh Bohrium [264] 108 Hs Hassium [269] 109 Mt Meitnerium [268] 110 Ds Darmstadtium 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium 116 Lv Livermorium [298] 117 Uus Ununseptium 118 Uuo Ununoctium 57 La Lanthanum 58 Ce Cerium 59 Pr Praseodymium 60 Nd Neodymium 144.24 61 Pm Promethium 62 Sm Samarium 150.36 63 Eu Europium 64 Gd Gadolinium 157.25 65 Tb Terbium 66 Dy Dysprosium 162.50 67 Ho Holmium 68 Er Erbium 167.26 69 Tm Thulium 70 Yb Ytterbium 173.04 71 Lu Lutetium 89 Ac Actinium 90 Th Thorium 91 Pa Protactinium 92 U Uranium 93 Np Neptunium 94 Pu Plutonium 95 Am Americium 96 Cm Curium 97 Bk Berkelium 98 Cf Californium 99 Es Einsteinium [254] 100 Fm Fermium 101 Md Mendelevium 258.1 102 No Nobelium 103 Lr Lawrencium 2 2A 13 3A A A A A All column 1A elements have 1 valence electron Atomic mass in [brackets] is for the most stable isotope .

All column 2A elements have 2 valence electrons
1 H Hydrogen 1.0079 Alkali Metals Alkaline Earth Metals Transition Metals Lanthanides Actinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium 4.003 3 Li Lithium 6.941 4 Be Beryllium 9.0122 5 B Boron 10.811 6 C Carbon 12.011 7 N Nitrogen 14.007 8 O Oxygen 15.999 9 F Fluorine 18.998 10 Ne Neon 20.180 11 Na Sodium 22.990 12 Mg Magnesium 24.305 13 Al Aluminum 26.982 14 Si Silicon 28.086 15 P Phosphorus 30.974 16 S Sulfur 32.066 17 Cl Chlorine 35.453 18 Ar Argon 39.948 19 K Potassium 39.098 20 Ca Calcium 40.078 21 Sc Scandium 44.956 22 Ti Titanium 47.88 23 V Vanadium 50.942 24 Cr Chromium 51.996 25 Mn Manganese 54.938 26 Fe Iron 55.933 27 Co Cobalt 58.933 28 Ni Nickel 58.693 29 Cu Copper 63.546 30 Zn Zinc 65.39 31 Ga Gallium 69.732 32 Ge Germanium 72.61 33 As Arsenic 74.922 34 Se Selenium 78.09 35 Br Bromine 79.904 36 Kr Krypton 84.80 37 Rb Rubidium 85.468 38 Sr Strontium 87.62 39 Y Yttrium 88.906 40 Zr Zirconium 91.224 41 Nb Niobium 92.906 42 Mo Molybdenum 95.94 43 Tc Technetium 98.907 44 Ru Ruthenium 101.07 45 Rh Rhodium 46 Pd Palladium 106.42 47 Ag Silver 48 Cd Cadmium 49 In Indium 50 Sn Tin 118.71 51 Sb Antimony 52 Te Tellurium 127.6 53 I Iodine 54 Xe Xenon 131.29 55 Cs Cesium 132.91 56 Ba Barium 137.33 * 57-71 72 Hf Hafnium 178.49 73 Ta Tantalum 74 W Tungsten 183.85 75 Re Rhenium 76 Os Osmium 190.23 77 Ir Iridium 192.22 78 Pt Platinum 195.08 79 Au Gold 80 Hg Mercury 200.59 81 Tl Thallium 82 Pb Lead 207.2 83 Bi Bismuth 84 Po Polonium [ ] 85 At Astatine 86 Rn Radon 87 Fr Francium [223] 88 Ra [226] ** 89-103 104 Rf Rutherfordium [261] 105 Db Dubnium [262] 106 Sg Seaborgium [266] 107 Bh Bohrium [264] 108 Hs Hassium [269] 109 Mt Meitnerium [268] 110 Ds Darmstadtium 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium 116 Lv Livermorium [298] 117 Uus Ununseptium 118 Uuo Ununoctium 57 La Lanthanum 58 Ce Cerium 59 Pr Praseodymium 60 Nd Neodymium 144.24 61 Pm Promethium 62 Sm Samarium 150.36 63 Eu Europium 64 Gd Gadolinium 157.25 65 Tb Terbium 66 Dy Dysprosium 162.50 67 Ho Holmium 68 Er Erbium 167.26 69 Tm Thulium 70 Yb Ytterbium 173.04 71 Lu Lutetium 89 Ac Actinium 90 Th Thorium 91 Pa Protactinium 92 U Uranium 93 Np Neptunium 94 Pu Plutonium 95 Am Americium 96 Cm Curium 97 Bk Berkelium 98 Cf Californium 99 Es Einsteinium [254] 100 Fm Fermium 101 Md Mendelevium 258.1 102 No Nobelium 103 Lr Lawrencium 2 2A 13 3A A A A A All column 2A elements have 2 valence electrons Atomic mass in [brackets] is for the most stable isotope .

All column 3A elements have 3 valence electrons and so on…
1 H Hydrogen 1.0079 Alkali Metals Alkaline Earth Metals Transition Metals Lanthanides Actinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium 4.003 3 Li Lithium 6.941 4 Be Beryllium 9.0122 5 B Boron 10.811 6 C Carbon 12.011 7 N Nitrogen 14.007 8 O Oxygen 15.999 9 F Fluorine 18.998 10 Ne Neon 20.180 11 Na Sodium 22.990 12 Mg Magnesium 24.305 13 Al Aluminum 26.982 14 Si Silicon 28.086 15 P Phosphorus 30.974 16 S Sulfur 32.066 17 Cl Chlorine 35.453 18 Ar Argon 39.948 19 K Potassium 39.098 20 Ca Calcium 40.078 21 Sc Scandium 44.956 22 Ti Titanium 47.88 23 V Vanadium 50.942 24 Cr Chromium 51.996 25 Mn Manganese 54.938 26 Fe Iron 55.933 27 Co Cobalt 58.933 28 Ni Nickel 58.693 29 Cu Copper 63.546 30 Zn Zinc 65.39 31 Ga Gallium 69.732 32 Ge Germanium 72.61 33 As Arsenic 74.922 34 Se Selenium 78.09 35 Br Bromine 79.904 36 Kr Krypton 84.80 37 Rb Rubidium 85.468 38 Sr Strontium 87.62 39 Y Yttrium 88.906 40 Zr Zirconium 91.224 41 Nb Niobium 92.906 42 Mo Molybdenum 95.94 43 Tc Technetium 98.907 44 Ru Ruthenium 101.07 45 Rh Rhodium 46 Pd Palladium 106.42 47 Ag Silver 48 Cd Cadmium 49 In Indium 50 Sn Tin 118.71 51 Sb Antimony 52 Te Tellurium 127.6 53 I Iodine 54 Xe Xenon 131.29 55 Cs Cesium 132.91 56 Ba Barium 137.33 * 57-71 72 Hf Hafnium 178.49 73 Ta Tantalum 74 W Tungsten 183.85 75 Re Rhenium 76 Os Osmium 190.23 77 Ir Iridium 192.22 78 Pt Platinum 195.08 79 Au Gold 80 Hg Mercury 200.59 81 Tl Thallium 82 Pb Lead 207.2 83 Bi Bismuth 84 Po Polonium [ ] 85 At Astatine 86 Rn Radon 87 Fr Francium [223] 88 Ra [226] ** 89-103 104 Rf Rutherfordium [261] 105 Db Dubnium [262] 106 Sg Seaborgium [266] 107 Bh Bohrium [264] 108 Hs Hassium [269] 109 Mt Meitnerium [268] 110 Ds Darmstadtium 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium 116 Lv Livermorium [298] 117 Uus Ununseptium 118 Uuo Ununoctium 57 La Lanthanum 58 Ce Cerium 59 Pr Praseodymium 60 Nd Neodymium 144.24 61 Pm Promethium 62 Sm Samarium 150.36 63 Eu Europium 64 Gd Gadolinium 157.25 65 Tb Terbium 66 Dy Dysprosium 162.50 67 Ho Holmium 68 Er Erbium 167.26 69 Tm Thulium 70 Yb Ytterbium 173.04 71 Lu Lutetium 89 Ac Actinium 90 Th Thorium 91 Pa Protactinium 92 U Uranium 93 Np Neptunium 94 Pu Plutonium 95 Am Americium 96 Cm Curium 97 Bk Berkelium 98 Cf Californium 99 Es Einsteinium [254] 100 Fm Fermium 101 Md Mendelevium 258.1 102 No Nobelium 103 Lr Lawrencium 2 2A 13 3A A A A A All column 3A elements have 3 valence electrons and so on… Atomic mass in [brackets] is for the most stable isotope .

All column 8A elements have 8 valence electrons except helium (2ve)
1 H Hydrogen 1.0079 Alkali Metals Alkaline Earth Metals Transition Metals Lanthanides Actinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium 4.003 3 Li Lithium 6.941 4 Be Beryllium 9.0122 5 B Boron 10.811 6 C Carbon 12.011 7 N Nitrogen 14.007 8 O Oxygen 15.999 9 F Fluorine 18.998 10 Ne Neon 20.180 11 Na Sodium 22.990 12 Mg Magnesium 24.305 13 Al Aluminum 26.982 14 Si Silicon 28.086 15 P Phosphorus 30.974 16 S Sulfur 32.066 17 Cl Chlorine 35.453 18 Ar Argon 39.948 19 K Potassium 39.098 20 Ca Calcium 40.078 21 Sc Scandium 44.956 22 Ti Titanium 47.88 23 V Vanadium 50.942 24 Cr Chromium 51.996 25 Mn Manganese 54.938 26 Fe Iron 55.933 27 Co Cobalt 58.933 28 Ni Nickel 58.693 29 Cu Copper 63.546 30 Zn Zinc 65.39 31 Ga Gallium 69.732 32 Ge Germanium 72.61 33 As Arsenic 74.922 34 Se Selenium 78.09 35 Br Bromine 79.904 36 Kr Krypton 84.80 37 Rb Rubidium 85.468 38 Sr Strontium 87.62 39 Y Yttrium 88.906 40 Zr Zirconium 91.224 41 Nb Niobium 92.906 42 Mo Molybdenum 95.94 43 Tc Technetium 98.907 44 Ru Ruthenium 101.07 45 Rh Rhodium 46 Pd Palladium 106.42 47 Ag Silver 48 Cd Cadmium 49 In Indium 50 Sn Tin 118.71 51 Sb Antimony 52 Te Tellurium 127.6 53 I Iodine 54 Xe Xenon 131.29 55 Cs Cesium 132.91 56 Ba Barium 137.33 * 57-71 72 Hf Hafnium 178.49 73 Ta Tantalum 74 W Tungsten 183.85 75 Re Rhenium 76 Os Osmium 190.23 77 Ir Iridium 192.22 78 Pt Platinum 195.08 79 Au Gold 80 Hg Mercury 200.59 81 Tl Thallium 82 Pb Lead 207.2 83 Bi Bismuth 84 Po Polonium [ ] 85 At Astatine 86 Rn Radon 87 Fr Francium [223] 88 Ra [226] ** 89-103 104 Rf Rutherfordium [261] 105 Db Dubnium [262] 106 Sg Seaborgium [266] 107 Bh Bohrium [264] 108 Hs Hassium [269] 109 Mt Meitnerium [268] 110 Ds Darmstadtium 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium 116 Lv Livermorium [298] 117 Uus Ununseptium 118 Uuo Ununoctium 57 La Lanthanum 58 Ce Cerium 59 Pr Praseodymium 60 Nd Neodymium 144.24 61 Pm Promethium 62 Sm Samarium 150.36 63 Eu Europium 64 Gd Gadolinium 157.25 65 Tb Terbium 66 Dy Dysprosium 162.50 67 Ho Holmium 68 Er Erbium 167.26 69 Tm Thulium 70 Yb Ytterbium 173.04 71 Lu Lutetium 89 Ac Actinium 90 Th Thorium 91 Pa Protactinium 92 U Uranium 93 Np Neptunium 94 Pu Plutonium 95 Am Americium 96 Cm Curium 97 Bk Berkelium 98 Cf Californium 99 Es Einsteinium [254] 100 Fm Fermium 101 Md Mendelevium 258.1 102 No Nobelium 103 Lr Lawrencium 2 2A 13 3A A A A A All column 8A elements have 8 valence electrons except helium (2ve) Atomic mass in [brackets] is for the most stable isotope .

Lewis Dot Structures Column # 1 A-8A = #V.E.s
Dot structures dots represent valence electrons. Valence electrons are electrons in the outermost energy level of an atom. Important for Bonding!!! Six V.E.s +8 The shell model on the right shows an oxygen atom with 8 total electrons. How many of them are valence electrons? O We draw it like this: The element symbol in the middle with dots drawn around it. Starting from the right, draw one dot on each side in a clockwise fashion and then double up the dots if necessary. Key Concept: Shell diagrams show ALL electrons Lewis Dot Structures show only the outermost ring (valence electrons)

Lewis Dot Structures Column # 1 A-8A = #V.E.s
Draw Dot Structures C Carbon is in Column 4A so it has four Valence electrons!

Lewis Dot Structures 1VE X 2VEs 3VEs 4VEs 5VEs 6VEs 7VEs 8VEs

Period 2 Lewis Structures
1VE Li 2VEs Be 3VEs B 4VEs C 5VEs N 6VEs O 7VEs F 8VEs Ne

Patterns in Electron Configuration
* ** Patterns in Electron Configuration

H 1s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d10 He 1s2 Li 2s1 Be
C 2p2 N 2p3 O 2p4 2p5 Ne 2p6 Na 3s1 Mg 3s2 Al 3p1 Si 3p2 3p3 3p4 Cl 3p5 Ar 3p6 K 4s1 Ca 4s2 Sc 3d1 Ti 3d2 V 3d3 Cr 3d5 Mn Fe 3d6 Co 3d7 Ni 3d8 Cu 3d10 Zn Ga 4p1 Ge 4p2 As 4p3 Se 4p4 Br 4p5 Kr 4p6 Rb 5s1 Sr 5s2 Y 4d1 Zr 4d2 Nb 4d4 Mo 4d5 Tc Ru 4d7 Rh 4d8 Pd 4d10 Ag Cd In 5p1 Sn 5p2 Sb 5p3 Te 5p4 I 5p5 Xe 5p6 Cs 6s1 Ba 6s2 * Hf 5d2 Ta 5d3 W 5d4 Re 5d5 Os 5d6 Ir 5d7 Pt 5d9 Au 5d10 Hg 6p1 Pb 6p2 Bi 6p3 Po 6p4 At 6p5 Rn 6p6 Fr 7s1 Ra 7s2 ** Rf 6d2 Db 6d3 Sg 6d4 Bh 6d5 Hs 6d6 Mt 6d7 Ds 6d8 Rg 6d10 Cn La 5d1 Ce 4f15d1 Pr 4f3 Nd 4f4 Pm 4f5 Sm 4f6 Eu 4f7 Gd 4f75d1 Tb 4f9 Dy 4f10 Ho 4f11 Er 4f12 Tm 4f13 Yb 4f14 Lu Ac 6d1 Th Pa 5f26d1 U 5f36d1 Np 5f46d1 Pu 5f6 Am 5f7 Cm 5f76d1 Bk 5f9 Cf 5f10 Es 5f11 Fm 5f12 Md 5f13 No 5f14 Lr

Why does each element have a unique set of spectral lines?
Each color of light has a specific size/wavelength/energy. Each atom has a unique electron configuration resulting in different amounts of energy being given off when an electron jumps back down. Also each atom has difference energy characteristics since the number of protons differs between atoms. Every color of light has a specific size and energy. Opposites attract Nucleus pulling electrons. More protons the stronger the pull. Different energy to jump.

Emission Spectra and Bohr-Rydberg
Limitations of the Bohr Model The Bohr Model was an important step in the development of atomic theory. However, it has several limitations. It is in violation of the Heisenberg Uncertainty Principle. The Bohr Model considers electrons to have both a known radius and orbit, which is impossible according to Heisenberg. The Bohr Model is very limited in terms of size. Poor spectral predictions are obtained when larger atoms are in question. It cannot predict the relative intensities of spectral lines. It does not explain the Zeeman Effect, when the spectral line is split into several components in the presence of a magnetic field. The Bohr Model does not account for the fact that accelerating electrons do not emit electromagnetic radiation. Hydrogen gas when viewed through a spectroscope gives off four discrete lines. We are going to use the Rydberg equation based off the Bohr model to calculate the wavelength of these lines.

Show Work N= 6 N= 4 N= 4 N= 3 N= 2 N= 1
Calculate the wavelength of light emitted by a hydrogen atom for the cases below where an electron is dropping down to lower energy levels emitting a photon. Convert all wavelengths into nanometers. Indicate where it falls on the electromagnetic spectrum and its color (if visible)! Draw a visual depiction of the cases mirroring the pattern of the image on the right. Use Plank’s formula to calculate the energy of the photon after finding lambda in J and eV. An electron jumps from n = 3 to n=2. An electron jumps from n = 4 to n=2 An electron jumps from n = 5 to n=2 An electron jumps from n = 6 to n=2 An electron jumps from n = 2 to n=1 Show Work N= 6 N= 4 N= 4 .25-91/90 N= 3 λ = wavelength of light in meters r = Rydberg constant = x 107m-1 nf = final energy level ni = initial energy level E = energy in joules c= speed of light = 3.00 x 108m/s h = Plank’s Constant = × m2 kg / s 1 Joule = 6.242x1018eV N= 2 N= 1

nf = 2 ni =3 r = constant An electron jumps from n = 3 to n=2. N= 6
λ = wavelength of light in meters r = Rydberg constant = x 107m-1 nf = final energy level ni = initial energy level E = energy in joules c= speed of light = 3.00 x 108m/s h = Plank’s Constant = × m2 kg / s 1 Joule = 6.242x1018eV N= 2 N= 1

nf = 2 ni =3 r = constant An electron jumps from n = 3 to n=2.
A nanometer is x10-9 so we move the decimal right two places Red light

An electron jumps from n = 3 to n=2.
Red light A nanometer is x10-9 so we move the decimal right two places N= 6 N= 4 N= 4 N= 3 Photon: Red Light N= 2 λ = wavelength of light in meters E = energy in joules c= speed of light = 3.00 x 108m/s h = Plank’s Constant = × m2 kg / s 1 Joule = 6.242x1018eV N= 1

Balmer, Lyman and Paschen Series for H

Full Electromagnetic Spectrum
do notes God’s Xylophone Usually Vibrates in Many Rooms Large wavelength (low energy) to Small (high energy) Gamma rays : we go into space and die! Sun emits these… High energy –nuclear bomb-- incredible hulk….cancer X rays pass through skin and flesh easily but not bone….x-ray images Ultraviolet – what give us sunburn…blacklights – bees see in ultraviolet – CSI blood, other bodily fluids Visible the light we see Intrared – see heat signatures Microwaves how our microwaves work…send out waves of certain size… 380 to 700 nm = 3.8x to 7 x 10-7 Radar used for wx radar Radio—listen to tunes

- - + Hydrogen Atom 1 2 3 4 5 6 Visible Balmer Series Ultraviolet
410nm Balmer Series 434nm 486nm 656nm Ultraviolet 1875nm 122nm - Lyman Series + 103nm Infrared 1282nm Paschen Series 1 97nm 1094nm 2 95nm - 3 94nm 4 5 Hydrogen Atom 6 Energy Level (n)

- - Hydrogen Atom + 1 2 3 4 5 6 Visible Balmer Series Energy Level (n)
410nm 434nmc 486nm 656nm - + 1 2 - 3 4 5 Energy Level (n) 6

Hydrogen Atom - + -

Who do the same energy level transitions (e. g
Who do the same energy level transitions (e.g. 3-2) in different elements produce different wavelength of light?

Light is Electromagnetic Radiation
Visible Light is just a small part of the total spectrum of Light

Violet ~400nm Blue Green Yellow Orange Red ~700nm ~475nm ~525nm ~570nm
Visible light runs roughly from high energy, short wavelength (380nm) violet light (to low energy, long wavelength (750nm) red light. The majority of the color range that the human eye can see falls between 400 and 700nms. Other light exists, we can feel the heat (infrared radiation) from a stove or camp fire, but we can’t see it. ~475nm ~525nm ~570nm ~ 589nm Estimate the size of the ewavelenths of ~ 700nm ~ 400nm

Full Electromagnetic Spectrum
do notes God’s Xylophone Usually Vibrates in Many Rooms Large wavelength (low energy) to Small (high energy) Gamma rays : we go into space and die! Sun emits these… High energy –nuclear bomb-- incredible hulk….cancer X rays pass through skin and flesh easily but not bone….x-ray images Ultraviolet – what give us sunburn…blacklights – bees see in ultraviolet – CSI blood, other bodily fluids Visible the light we see Intrared – see heat signatures Microwaves how our microwaves work…send out waves of certain size… 380 to 700 nm = 3.8x to 7 x 10-7 Radar used for wx radar Radio—listen to tunes

Violet ~400nm Blue ~475nm Green ~525nm Yellow ~570nm Orange ~ 589nm Red ~650nm

Heinrich Hertz, James Watt and Samuel Morse
Watt = 1J/s = light bub 40 watts….

A Wave is a transfer of energy

Anatomy of a Wave The amplitude of a wave is the wave’s height from zero to the crest. The wavelength, represented by  (the Greek letter lambda), is the distance between the crests. The frequency, represented by  (the Greek letter nu), is the number of wave cycles to pass a given point per unit of time. The SI unit of cycles per second is called a hertz (Hz). Hertz has no known association with rental company…

High vs Low Frequency High frequency more energy….why UV rays harmful…fortunately sun shields us…

Make Low and High Frequency waves
Set up a meter stick and have students make waves of varying amplitude…and frequency

Sample Problems What is the frequency of radiation with a wavelength of 5.00 x 10-8m? In what region of the electromagnetic spectrum is this radiation? Calculate the wavelength of light emitted by the sodium lamp shown to the right if the frequency of the radiation is 5.10 x 1014Hz. In what region of the electromagnetic spectrum is this radiation? Sodium vapor lamps produce a yellow glow. x10^15 freq 5.87 x10^-7 or 587 nanometers

1. ) A laser emits light of frequency 4. 74 x 1014 sec-1
1.) A laser emits light of frequency 4.74 x 1014 sec-1. What is the wavelength of the light in nm? 2.) A certain electromagnetic wave has a wavelength of 625 nm. a.) What is the frequency of the wave? b.) What region of the electromagnetic spectrum is it found? 3.) How many minutes would it take a radio wave to travel from the planet Venus to Earth? (Average distance from Venus to Earth = 28 million miles). 4.) The blue color of the sky results from the scattering of sunlight by air molecules. The blue light has a frequency of about 7.5 x 1014 Hz. Calculate the wavelength, in nm, associated with this radiation.

Some Infrared Photos

Image top is a cup of coffee

Ultraviolet Radiation
BLACK LIGHTS Usee Black light markers, show minerals…

Flame Test Lab!!!!!

Bohr Diagrams or Shell Models

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