What color is the sun?

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

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

RAINBOWS!RAINBOWS! How does a Rainbow Form

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

White Light is Composed of all Colors: ROY G BIV 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. WHITE LIGHT PRISM How Does a Prism Work?

Simple Refraction Demo Arrow and a glass cup.

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. Why Does the Sun Appear to be Yellow?

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. Why are Sunrises and Sunsets Red/Orange? EARTH X 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.

WHITE LIGHT How Does a Rainbow Form? 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

Activity: Grab a spectroscope and use it to look at the following: Sunlight (not directly) Fluorescent Light Helium Tube Oxygen Tube Hydrogen Tube Use colored pencils and markers to draw the spectral lines (color pattern). Explain the differences that you see. Activity: Grab a spectroscope and use it to look at the following: Sunlight (not directly) Fluorescent Light Helium Tube Oxygen Tube Hydrogen Tube Use colored pencils and markers to draw the spectral lines (color pattern). Explain the differences that you see. 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… Image via openstax

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 [1] Energy strikes an atom [2] Electrons in their grounds state become excited and jump up to a higher energy level [3] Electrons in higher energy levels are unstable. They drop back down to their ground state and emit the energy they absorbed. [4] That energy is emitted as photons or small packets of light Light rule

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

STUDENTS PLEASE DON’T FART S (2 electrons) P (6 electrons) D (10 electrons) F (14 electrons)

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

1s 2 Energy Level Orbital shape # of Electrons Containers that hold electrons 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 14 6d 10

Practice Configuration and Boxes Hydrogen Oxygen Fluorine Neon-21 Al 3+ You have to fill up one orbital before going into the next one! 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 14 6d 10 HANDOUT

__ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 NeonSulfurKryptonOxygenNitrogenMg 2+ S 2-14 C Hund’s RulePauli Exclusion PrincipleAufbau Principle Fill in the diagram and write out the electron configuration

1s 2 4f 14 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 6s 2 7s 2 5p 6 6p 6 4d 10 5d 10 HydrogenLithiumSodiumPotassiumRubidiumCaesium

Valence Electrons 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. 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 7p 3d 4d 5d 6d 7d 4f 5f 6f 7f 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 14 6d 10

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 … Determine the number of Valence Electrons Carbon Neon Argon Iron 1.First you need to determine the total number of electrons each element has. 2.You need to write out its ground state electron configuration. 3.Count the number of electrons in the highest energy level.

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 … Determine the number of Valence Electrons Carbon 1s 2 2s 2 2p 2 =4 Neon 1s 2 2s 2 2p 6 =8 Argon 1s 2 2s 2 2p 6 3s 2 3p 6 =8 Iron 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 =2 1.First you need to determine the total number of electrons each element has. 2.You need to write out its ground state electron configuration. 3.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?

1 H Hydrogen Alkali Metals Alkaline Earth Metals Transition Metals LanthanidesActinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium Al Aluminum Si Silicon P Phosphorus S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenum Tc Technetium Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium * Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium [ ] 85 At Astatine Rn Radon Fr Francium [223] 88 Ra Radon [226] ** 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 [269] 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium unknown 116 Lv Livermorium [298] 117 Uus Ununseptium unknown 118 Uuo Ununoctium unknown * 57 La Lanthanum Ce Cerium Pr Praseodymium Nd Neodymium Pm Promethium Sm Samarium Eu Europium Gd Gadolinium Tb Terbium Dy Dysprosium Ho Holmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium ** 89 Ac Actinium Th Thorium Pa Protactinium U Uranium Np Neptunium Pu Plutonium Am Americium Cm Curium Bk Berkelium Cf Californium Es Einsteinium [254] 100 Fm Fermium Md Mendelevium No Nobelium Lr Lawrencium [262] 1 1A 2 2A A 14 4A 15 5A 16 6A 17 7A 18 8A All column 1A elements have 1 valence electron Atomic mass in [brackets] is for the most stable isotope.

1 H Hydrogen Alkali Metals Alkaline Earth Metals Transition Metals LanthanidesActinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium Al Aluminum Si Silicon P Phosphorus S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenum Tc Technetium Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium * Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium [ ] 85 At Astatine Rn Radon Fr Francium [223] 88 Ra Radon [226] ** 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 [269] 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium unknown 116 Lv Livermorium [298] 117 Uus Ununseptium unknown 118 Uuo Ununoctium unknown * 57 La Lanthanum Ce Cerium Pr Praseodymium Nd Neodymium Pm Promethium Sm Samarium Eu Europium Gd Gadolinium Tb Terbium Dy Dysprosium Ho Holmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium ** 89 Ac Actinium Th Thorium Pa Protactinium U Uranium Np Neptunium Pu Plutonium Am Americium Cm Curium Bk Berkelium Cf Californium Es Einsteinium [254] 100 Fm Fermium Md Mendelevium No Nobelium Lr Lawrencium [262] 1 1A 2 2A A 14 4A 15 5A 16 6A 17 7A 18 8A All column 2A elements have 2 valence electrons Atomic mass in [brackets] is for the most stable isotope.

1 H Hydrogen Alkali Metals Alkaline Earth Metals Transition Metals LanthanidesActinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium Al Aluminum Si Silicon P Phosphorus S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenum Tc Technetium Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium * Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium [ ] 85 At Astatine Rn Radon Fr Francium [223] 88 Ra Radon [226] ** 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 [269] 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium unknown 116 Lv Livermorium [298] 117 Uus Ununseptium unknown 118 Uuo Ununoctium unknown * 57 La Lanthanum Ce Cerium Pr Praseodymium Nd Neodymium Pm Promethium Sm Samarium Eu Europium Gd Gadolinium Tb Terbium Dy Dysprosium Ho Holmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium ** 89 Ac Actinium Th Thorium Pa Protactinium U Uranium Np Neptunium Pu Plutonium Am Americium Cm Curium Bk Berkelium Cf Californium Es Einsteinium [254] 100 Fm Fermium Md Mendelevium No Nobelium Lr Lawrencium [262] 1 1A 2 2A A 14 4A 15 5A 16 6A 17 7A 18 8A All column 3A elements have 3 valence electrons and so on… Atomic mass in [brackets] is for the most stable isotope.

1 H Hydrogen Alkali Metals Alkaline Earth Metals Transition Metals LanthanidesActinides Other Metals Metalloids Other Nonmetals Halogens Noble Gases 2 He Helium Li Lithium Be Beryllium B Boron C Carbon N Nitrogen O Oxygen F Fluorine Ne Neon Na Sodium Mg Magnesium Al Aluminum Si Silicon P Phosphorus S Sulfur Cl Chlorine Ar Argon K Potassium Ca Calcium Sc Scandium Ti Titanium V Vanadium Cr Chromium Mn Manganese Fe Iron Co Cobalt Ni Nickel Cu Copper Zn Zinc Ga Gallium Ge Germanium As Arsenic Se Selenium Br Bromine Kr Krypton Rb Rubidium Sr Strontium Y Yttrium Zr Zirconium Nb Niobium Mo Molybdenum Tc Technetium Ru Ruthenium Rh Rhodium Pd Palladium Ag Silver Cd Cadmium In Indium Sn Tin Sb Antimony Te Tellurium I Iodine Xe Xenon Cs Cesium Ba Barium * Hf Hafnium Ta Tantalum W Tungsten Re Rhenium Os Osmium Ir Iridium Pt Platinum Au Gold Hg Mercury Tl Thallium Pb Lead Bi Bismuth Po Polonium [ ] 85 At Astatine Rn Radon Fr Francium [223] 88 Ra Radon [226] ** 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 [269] 111 Rg Roentgenium [272] 112 Cn Copernicium [277] 113 Uut Ununtrium unknown 114 Fl Flerovium [289] 115 Uup Ununpentium unknown 116 Lv Livermorium [298] 117 Uus Ununseptium unknown 118 Uuo Ununoctium unknown * 57 La Lanthanum Ce Cerium Pr Praseodymium Nd Neodymium Pm Promethium Sm Samarium Eu Europium Gd Gadolinium Tb Terbium Dy Dysprosium Ho Holmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium ** 89 Ac Actinium Th Thorium Pa Protactinium U Uranium Np Neptunium Pu Plutonium Am Americium Cm Curium Bk Berkelium Cf Californium Es Einsteinium [254] 100 Fm Fermium Md Mendelevium No Nobelium Lr Lawrencium [262] 1 1A 2 2A A 14 4A 15 5A 16 6A 17 7A 18 8A 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!!! +8 The shell model on the right shows an oxygen atom with 8 total electrons. How many of them are valence electrons? Six V.E.s 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) 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 X2VEs 3VEs 4VEs 5VEs 6VEs 7VEs 8VEs

Period 2 Lewis Structures 1VE Li2VEs Be3VEs B4VEs C5VEs N6VEs O7VEs F8VEs Ne

* ** * Patterns in Electron Configuration

H 1s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 He 1s 2 Li 2s 1 Be 2s 2 SPDF B 2p 1 C 2p 2 N 2p 3 O 2p 4 F 2p 5 Ne 2p 6 Na 3s 1 Mg 3s 2 Al 3p 1 Si 3p 2 P 3p 3 S 3p 4 Cl 3p 5 Ar 3p 6 K 4s 1 Ca 4s 2 Sc 3d 1 Ti 3d 2 V 3d 3 Cr 3d 5 Mn 3d 5 Fe 3d 6 Co 3d 7 Ni 3d 8 Cu 3d 10 Zn 3d 10 Ga 4p 1 Ge 4p2 As 4p 3 Se 4p 4 Br 4p 5 Kr 4p 6 Rb 5s 1 Sr 5s 2 Y 4d 1 Zr 4d 2 Nb 4d 4 Mo 4d 5 Tc 4d 5 Ru 4d 7 Rh 4d 8 Pd 4d 10 Ag 4d 10 Cd 4d 10 In 5p 1 Sn 5p 2 Sb 5p 3 Te 5p 4 I 5p 5 Xe 5p 6 Cs 6s 1 Ba 6s 2 * Hf 5d 2 Ta 5d 3 W 5d 4 Re 5d 5 Os 5d 6 Ir 5d 7 Pt 5d 9 Au 5d 10 Hg 5d 10 Ti 6p 1 Pb 6p 2 Bi 6p 3 Po 6p 4 At 6p 5 Rn 6p 6 Fr 7s 1 Ra 7s 2 ** Rf 6d 2 Db 6d 3 Sg 6d 4 Bh 6d 5 Hs 6d 6 Mt 6d 7 Ds 6d 8 Rg 6d 10 Cn 6d 10 * La 5d 1 Ce 4f 1 5d 1 Pr 4f 3 Nd 4f 4 Pm 4f 5 Sm 4f 6 Eu 4f 7 Gd 4f 7 5d 1 Tb 4f 9 Dy 4f 10 Ho 4f 11 Er 4f 12 Tm 4f 13 Yb 4f 14 Lu 5s 1 ** Ac 6d 1 Th 6d 2 Pa 5f 2 6d 1 U 5f 3 6d 1 Np 5f 4 6d 1 Pu 5f 6 Am 5f 7 Cm 5f 7 6d 1 Bk 5f 9 Cf 5f 10 Es 5f 11 Fm 5f 12 Md 5f 13 No 5f 14 Lr 6d 1

Why does each element have a unique set of spectral lines? 1.Each color of light has a specific size/wavelength/energy. 2.Each atom has a unique electron configuration resulting in different amounts of energy being given off when an electron jumps back down. 3.Also each atom has difference energy characteristics since the number of protons differs between atoms.

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

Full Electromagnetic Spectrum

Some Infrared Photos

Ultraviolet Radiation BLACK LIGHTS

Flame Test Lab!!!!!