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Atomic Theory Class #1 Penny Lab ASAP. Check your grades! OB: Students will examine basic structure of the atom, learn what the numbers on the Periodic table mean, and look at electron orbitals. Take out your WHITE periodic tables now. All atoms are made up of three sub-atomic (smaller than atoms) parts. They are the 1. Parts of the atom Particle Charge Symbol Mass Location All atoms are made up of three sub-atomic (smaller than atoms) parts. They are the Parts of the atom Particle Charge Symbol Mass Location proton + + p 1 amu nucleus neutron Ø n° 1 amu nucleus e zero in high school Flying around the nucleus electron - 2. The mass of an electron is NOT ZERO, but it’s so small, about 1/1750 of a proton or neutron, that we will disregard it’s mass. It’s an intro class, and we can’t measure these masses in our class anyway, but it’s not zero in the real world. The nucleus is the small, dense center of an atom where the protons and neutrons live. Electrons fly around outside, relatively far away. In this model, the nucleus is the yellow ball in the middle. It does not show it, but inside must be three protons and probably 4 neutrons. This is a model of atom #3, which is LITHIUM. It’s a cartoon, it’s not even what we think atoms look like, but it’s cute. The mass of all atoms are measured in super tiny masses called AMU, or ATOMIC MASS UNITS. The vocabulary is building up already. This is another topic to NOT FALL BEHIND ON. Masses for the subatomic particles (approximate) Protons = 1 amu each Neutrons = 1 amu each Electrons = zero mass in high school chem 3. Atomic Mass 4. Atomic Number 5. Electron Configuration 12.011 6 2-4 6. Atomic Mass Numbers will be rounded to the nearest whole number (they are not really whole numbers, we’ll get to that later) 7. Mass Number = mass of protons plus neutrons Mass = p+ plus n° 8. The mass of mercury is 201, so mercury has a total of 201 protons plus neutrons. How many of each? Let’s learn how to figure this out Atomic Mass of Hg = 201 amu Minus the protons Equals the n° - 80 p+ 121 n° the n° + p+ = mass Or, n° = mass - p+ 9. Let’s do TIN, Sn An atom of tin = which is the total p+ + n° Minus atomic # which is the # p+ left over, which are the neutrons 9. Let’s do TIN, Sn An atom of tin = 119 amu which is the total p+ + n° Minus atomic # - 50 which is the # p+ 69 left over, which are the neutrons This works for all 118 different atoms, all of them! 10. All atoms are electrically neutral, the number of p+ = eThe positives = the negatives. Always. Every atom is neutrally charged. The positive protons + negative electrons BALANCE. 11. How many p+, n° and e- are in these atoms? In Nb Ba 11. How many p+, n° and e- are in these atoms? In Nb Ba Mass = 115 Mass = 93 Mass = 137 Minus the At # - 49 Minus the At # - 41 Minus the At # - 56 Neutrons = 66 Neutrons = 52 Neutrons = 81 12. Calcium can also be written properly as: Atomic mass Atomic number 40 20 Ca 14. Write the Formal Symbols for these atoms: mercury, chlorine, and copper Calcium can also be written properly as: 40 20 Atomic mass Atomic number Ca Write the Formal Symbols for these atoms: mercury, chlorine, and copper 201 80 Hg 35 17 Cl 64 29 Cu Electrons don’t just fly around willy nilly (I like that expression, and it fits) 15. Electrons STAY IN orbitals, which are also energy levels. 16. The further away from the nucleus, the higher the energy level the orbital is. The closer to the nucleus, the LOWER their energy level is. 17. The orbitals are only so big, they fit certain numbers of electrons. n = 1 (the first orbital) fits up to 2 electrons total n = 2 (the second orbital) fits up to 8 electrons total n = 3 (the third orbital) fits up to 8 electrons too, (sometimes up to 18) Etc. More to come on this. Let’s look at the periodic table now 18. Find silver, how many electrons does it have? 19. Find scandium, what is the electron configuration & total number of electrons? 20. Find the atom S, what is the name of this atom, how many p+ does it have? How many e- ? 21. Find oxygen, how many neutrons, what is it’s chemical symbol? Let’s look at the periodic table now 18. Find silver, how many electrons does it have? 47 19. Find scandium, what is the electron configuration & total number of electrons? 21, 2-8-9-2 20. Sulfur has 16 p+ and also has 16 e- ? 21. Find oxygen, how many neutrons, what is it’s chemical symbol? O has 16 n° 22. For any atom, the atomic number is the number of protons, which equals the number of electrons. The electron configuration always adds up to the atomic number. Examples: 23. Na #11 has a 2-8-1 or 2 + 8 + 1 = 11 total e― 24. C #6 has a 2-4 configuration or 2 + 4 = 6 total e― 25. K #19 has a 2-8-8-1 configuration or 2 + 8 + 8 + 1 = 19 total e― Atomic Theory Class #2 OB: students will review the models of the atom through scientific history, learning how ideas progressed and were dismissed as new information was developed. Most famous chemists had remarkable mustaches. That’s the easiest way to keep track of who’s who in science! About 2400 years ago a philosopher named Democritus said: 26. If you took anything and cut it in half, and in half, and in half, over and over, sooner or later you would get to a piece of this stuff that could not be cut in half again. That piece was called an ATOMOS (he was Greek) And that’s the start of chemistry. You could have an ATOMOS of a rock, of a fish, of a diamond, etc. The smallest piece of anything, that could not be cut again was to be known as an ATOM of that stuff. A good name, and it stuck. The first of many mustaches in our course! In the early 1800’s a man named John Dalton thought he could invent chemistry, it had to be longer than a singe word. He said… 27. 1. All substances were made up of atoms. 2. Each kind of atom had its own mass, different from the masses of the other kinds of atoms. 3. All atoms were built like billiard balls (a game he liked to play) His model was called the BILLIARD BALL MODEL Dalton came up with what is now called the 28. Atomic Theory This is so important I can’t highlight it enough! 1. All elements are composed of individual kinds of atoms. 2. Atoms of one element are identical. Atoms of different elements have different masses. 3. Atoms can physically mix with other atoms. Atoms can also chemically combine with other atoms IN SIMPLE WHOLE NUMBER RATIOS, to form new substances. 4. Chemical reactions change the arrangement of atoms, but they do not become different kinds of atoms. 29. Dalton did not know of protons, neutrons or electrons. He was brilliant, but had little science ability in 1803. You know a lot more about atoms now than he ever did! 30. Around 1897 J. J. Thomson discovers the electron! Look at the hair on that man’s lip! 31. Thomson did a variety of experiments, some using what’s called the cathode ray tube, to detect and measure electrons. He found the first subatomic particle, which was negatively charged. 32. His model of the atom is called the PLUM PUDDING MODEL, after what his wife’s dessert looked like! He put his newly discovered negative electrons into the positive “mush” of the atom. If Mrs. Thomson made him chocolate chip cookies instead, the model would be the chocolate chip cookie model, with the cookie being positive, offset by the negative electrons – the chips! He knew that the atoms were neutral. In 1908, my chemical hero, Earnest J. Rutherford discovers the nucleus! - and much more about the atom than previous scientists. Rutherford’s 33. Gold Foil Experiment He discovers the nucleus! The gold foil experiment was one of the top 10 experiments of all time, and cost him about fifty bucks. Wow! 34. Details of the GOLD FOIL experiment to memorize and share with your friends. 35. What does this gold foil experiment prove? 1. Atoms are mostly empty space since most of the alpha particles pass though the foil like it’s not really there. 2. Atoms are neutral (he knew this) so the nucleus must be dense and positively charged since the alpha particles which are positive didn’t stick, and they dinged off of something big every once in a while 3. Neutral atoms must therefore have electrons outside the nucleus flying around outside (like planets?) made sense. Problems with this new theory of Rutherford’s How can atoms be mostly empty space? How can they be mostly “not” there? How can these negative electrons fly around a positive center, but they never are attracted into this positive nucleus? Why not? They just keep flying? They never use up their energy? Ever? Really? How far away are these electrons Ernie - and do they just fly willy-nilly, or is there a system to them? Rutherford was right, but he needed some help. In 1913, one of his students, a man with a plural first name, comes to his rescue. Niels Bohr Niels Bohr is able to do some very funky math, (physics level + Nobel Prize style math) and he proves Rutherford is correct. 37. He shows that for hydrogen, if the electron fly at the right speed, and the right distance, it will somehow never run out of energy, and never collapse into the nucleus. And it doesn’t, does it? You already know he’s right even though you can’t do the math. None of the atoms collapses, not a one, and even though he can’t do the math for even 2 electrons, his proof is enough to save the modern model of the atom, central nucleus, flying electrons. 38. Niels Bohr further determines that 1. Electrons fly in specific orbits, as planets that are flying around the sun, nicely. 2. He showed that each orbit was really also an energy level. The smallest orbit closest to the nucleus was the lowest energy level. 3. Electrons could gain a specific amount of energy, an amount called a _______________, which enable the electrons to “jump” up to a ______________________ energy level or orbit. 38. Niels Bohr further determines that 4. Since every atom was unique (different numbers of protons and electron configurations) it took ___________ amounts of energy to make these upward “jumps” possible. 5. The electrons, in this new ___________ state, were less stable than the were in the normal or ___________ state. They’d have to give back this UNIQUE AMOUNT of energy the just gained in order to return to the ground state. Orbits was wrong, we understand them as ORBITALS now. 39. The modern model of the atom has been developed by many scientists over a long period of time. 40. It’s called the Wave-Mechanical Model because the electrons sometimes act like waves of energy, and sometimes like little bits of mechanical matter with a negative charge. 41. Because of the new math, the QUANTUM MATH, this model is more concerned with the STATISTICAL PROBABILITY of finding an electron’s location MOST OF THE TIME Electron orbitals are still energy levels, they just aren’t so neat. In this model/diagram, imagine that this is a photograph of a Helium atom (impossible really) taken about 1000 times on to the same piece of film, then printed overlapping. Each dot represents where the electrons were at some point. Electrons are a lot like Teenagers. Atomic Theory Class #3 OB: The Patterns of the Electron Orbitals, Ground State vs. Excited State, and SPECTRA Take out your periodic tables NOW, fill in the chart of the electron configurations Copy the electron configurations from Periodic Table Group 1 Group 2 Group 15 Group 16 Group 17 Group 18 42 lithium beryllium nitrogen oxygen fluorine neon 43 sodium magnesium phosphorous sulfur chlorine argon 44 rubidium strontium antimony tellurium iodine xenon These are the GROUND STATES or Lowest energy states (this is NORMAL) Copy the electron configurations from Periodic Table 42 43 44 Group 1 Group 2 Group 15 Group 16 Group 17 Group 18 lithium beryllium nitrogen oxygen fluorine neon 2-1 2-2 2-5 2-6 2-7 2-8 sodium magnesium phosphorous sulfur chlorine argon 2-8-1 2-8-2 2-8-5 2-8-6 2-8-7 2-8-8 rubidium strontium antimony tellurium iodine xenon 2-8-18-8-1 2-8-18-8-2 2-8-18-18-5 2-8-18-18-6 2-8-18-18-7 2-8-18-18-8 These are the GROUND STATES or Lowest energy states (this is NORMAL) 45. The 1st orbital holds up to _____electrons. The 2nd orbital holds up to ______ electrons 46. The 3rd orbital holds up to _______ (or _____ !) electrons (it’s funky) 47. The 4th orbital holds up to _______ (or _____!) electrons (it’s also funky) 48. All electron configurations on the periodic table are in the LOWEST ENERGY state, also called the ___________________________________________________________ 45. The 1st orbital holds up to 2 electrons. The 2nd orbital holds up to 8 electrons 46. The 3rd orbital holds up to 8 or 18 electrons (it’s funky) 47. The 4th orbital holds up to 18 or 32 electrons 48. All electron configurations on the periodic table are in the LOWEST ENERGY state, also called the Ground State, which is NORMAL Fill in POSSIBLE EXCITED STATE electron configuratons for these atoms ground state A possible excited state 49 Lithium 2-1 Lithium 50 Silicon 2-8-4 Silicon 51 Potassium 2-8-8-1 Potassium 52 Aluminum 2-8-3 Aluminum 53 Boron Boron 2-3 Fill in POSSIBLE EXCITED STATE electron configurations for these atoms ground state A possible excited state 49 Lithium 2-1 Lithium 1-2 50 Silicon 2-8-4 Silicon 2-7-5 51 Potassium 2-8-8-1 Potassium 2-8-7-2 52 Aluminum 2-8-3 Aluminum 2-7-4 53 Boron Boron 2-3 2-2-1 (or 1-8-5, or 2-8-3-1) (or 2-7-8-2) (or 2-7-3-1, or 2-8-2-1) (or 1-4, or even 2-1-1-1) In INTRO CHEM it is NOT POSSIBLE for you, or me, to know exactly which electrons move “up” to higher orbitals. Keep it Simple Silly Rabbits, or else you will get confused. 54. Ground + Excited State electron configurations have the _______________________, they are just in _______________ places. 55. What is KISS? _________________________________________________________ And that means what here?? 56. How do electrons get excited? They absorb energy in ______________ ________________ and release it as __________________________ light called ____________________________. 54. Ground + Excited State electron configurations have the Number of Electrons, they are just in Different places. 55. What is KISS? And what does it mean here? Keep it simple silly, don’t move a bunch of electrons around, you will lose count and make silly errors. 56. How do electrons get excited? They absorb energy in Unique quantities, and release it as Visible light called SPECTRA. THINK Atom Number of protons in nucleus with positive charge pulling on the electrons Ground State Possible Excited State 57 Sodium Na ______ protons 2-8-1 2-7-2 58 Magnesium Mg ______ protons 2-8-2 2-7-3 Why is the spectra different for Na and Mg if they both move 1 electron nd rd from 2 to 3 orbital? THINK Atom Number of protons in nucleus with positive charge pulling on the electrons Ground State Possible Excited State 57 Sodium Na 11 protons 2-8-1 2-7-2 58 Magnesium Mg 12 protons 2-8-2 2-7-3 With different numbers of protons pulling inward, it takes a different (unique) amount of energy to excite electrons in these different atoms. No matter how the energy was added in, the energy coming out is emitted as visible light, which we can see (you can see). 59. Each unique amount of energy given off is visible as different colors, which we can see with our eyes. This light given off WHEN ELECTRONS RETURN TO THE GROUND STATE IS CALLED _____________________________ 60. The spectra is a ______________________ of light, we see as one color but is made up of __________________ colors. Our eyes blend it into one shade. Inexpensive devices (similar to prisms) break up this single color spectra, into what is called a _____________________-graph. Each line is part of the spectra, and is like a UNIQUE finger print for that atom or compound. Scientists (and you too) will be able to determine what atoms are present by what spectra is emitted by unknown substances. We just compare the spectra measured, to the known spectrographs. This can be used in a lab to do CSI work, or through telescopes - to know what substances exist on other planets. The unique spectra that the same throughout the Universe. No matter how the energy was added in, the energy coming out is emitted as visible light, which we can see (you can see). 59. Each unique amount of energy given off is visible as different colors, which we can see with our eyes. This light given off WHEN ELECTRONS RETURN TO THE GROUND STATE IS CALLED SPECTRA 60. The spectra is a Mixture of light, we see as one color but is made up of MANY colors. Our eyes blend it into one shade. Inexpensive devices (similar to prisms) break up this single color spectra, into what is called a SPECTRAGRAPH. Each line is part of the spectra, and is like a UNIQUE finger print for that atom or compound. Scientists (and you too) will be able to determine what atoms are present by what spectra is emitted by unknown substances. We just compare the spectra measured, to the known spectrographs. This can be used in a lab to do CSI work, or through telescopes - to know what substances exist on other planets. The unique spectra that the same throughout the Universe. Atomic Theory Class #4 OB: what are isotopes and why are they so important? You will need a calculator and your reference tables out. Take out your 39 atoms handout as well, it’s going into the in box soon. John Dalton once said that all atoms of an element are identical, because at that time he could not imagine that there were any subatomic particles. He thought all the differences in atoms were that they had different masses, and that alone accounted for all the different properties. He was the father of modern chemistry, and you already are more educated than him. It turns out he was half right. He should have said that: All Atoms Of An Element Are Chemically Identical. They all react alike, & they have the same chemical properties. They are NOT PHYSICALLY IDENTICAL. 61. But, some atoms have a ______________________________________________. These “different” atoms are called ______________ There are 118 types of atoms, but there are almost __________________ different kinds of atoms. 62. Each kind of atom comes in a variety of masses, each type of atom forms many different ___________. 61. But, some atoms have a different number of neutrons. These “different” atoms are called ISOTOPES There are 118 types of atoms, but there are almost 1500 different kinds of atoms. 62. Each kind of atom comes in a variety of masses, each type of atom forms many different ISOTOPES. FILL IN THIS CHART of the common Isotopes of Neon ISOTOPE → 63 # protons 64 # electrons 65 # neutrons 66 MASS in amu Neon-20 Neon-21 Neon-22 FILL IN THIS CHART of the common Isotopes of Neon ISOTOPE → Neon-20 Neon-21 Neon-22 63 # protons 10 p+ 10 p+ 10 p+ 64 # electrons 10 e- 10 e- 10 e- 65 # neutrons 10 n° 11 n° 12 n° 66 MASS in amu 20 amu 21 amu 22 amu 67. These 3 different ISOTOPES of neon are _____________ identical but all have a different _______. 68. They have the same number of protons + electrons, but different numbers of _____________. 69. Only the ______ is affected, not their chemical ________. 67. These 3 different ISOTOPES of neon are CHEMICALLY identical but all have a different _______. 68. They have the same number of protons + electrons, but different numbers of NEUTRONS. 69. Only the MASS is affected, not their chemical PROPERTIES. Carbon has 2 main isotopes, C-12 and C-14. The carbon 14 is the radioactive kind, which we will discuss in great detail later in the year. C-12 makes up 99.45% of all the carbon in the world. C-14 makes up the rest, just 0.55% of the carbon. 70. Together they make up 100% of the carbon. 71. What is the ACTUAL average atomic mass of carbon atoms, the number on the periodic table in the atomic mass space? ________________ Here’s how we figure that out (do this math): (12 amu)(.9945) = (14 amu)(0.0055) = ______________________ (12 amu)(.9945) = 11.934 amu (14 amu)(0.0055) = 0.077 amu 12.011 amu Just like the periodic table says. Decimals come about because the proportions or percentages of the isotopes are not even steven. Most of the carbon is C-12, so the weighted average atomic mass is very close to 12. The most common isotope is the one that has the mass closest to the mass on the periodic table. Average Weighted Atomic Mass is the mass listed on our periodic tables. They take into account the mass of each isotope AND the proportions that those isotopes make up of all of that kind of atom. Scientists measure these proportions all the time (and sometimes it changes the numbers on the periodic table when they realize that the proportions are a little different than they thought. 73. The mass of an isotope (in HS Chem) is always a WHOLE NUMBER of amu, because they have a whole number of ______________ + _______________. But the PROPORTIONS are funky, which is where the decimals come from. Average Weighted Atomic Mass is the mass listed on our periodic tables. They take into account the mass of each isotope AND the proportions that those isotopes make up of all of that kind of atom. Scientists measure these proportions all the time (and sometimes it changes the numbers on the periodic table when they realize that the proportions are a little different than they thought. 73. The mass of an isotope (in HS Chem) is always a WHOLE NUMBER of amu, because they have a whole number of PROTONS + NEUTRONS. But the PROPORTIONS are funky, which is where the decimals come from. 74. A new element named Arbuiso is discovered (A). It has two isotopes, A-44 and A-45. 95.00% of all this Arbuiso has mass of 44 amu, while the rest has mass of 45 amu. What is the weighted average atomic mass of this cool new metallic element? 74. A new element named Arbuiso is discovered (A). It has two isotopes, A-44 and A-45. 95.00% of all this Arbuiso has mass of 44 amu, while the rest has mass of 45 amu. What is the weighted average atomic mass of this cool new metallic element? (44 amu)(.9500) = 41.80 amu (45 amu)(.0500) = + 2.25 amu 44.05 amu average weighted atomic mass 75. Unknown element X has three isotopes, X-23, X-24, and X-25. The first isotope makes up 75.00% of all of this element. X-24 makes up 20.0%, while the last isotope X-25 makes up just 5.0% of all this unknown element. What is it’s average weighted atomic mass? (hint, same type of math, but there are 3 lines this time) 75. Unknown element X has three isotopes, X-23, X-24, and X-25. The first isotope makes up 75.00% of all of this element. X-24 makes up 20.0%, while the last isotope X-25 makes up just 5.0% of all this unknown element. What is it’s average weighted atomic mass? (hint, same type of math, but there are 3 lines this time) (23 amu)(.750) = 17.25 amu (24 amu)(.200) = 4.80 amu (25 amu)(.050) = + 1.25 amu 23.3 amu Does that make sense, about 23 amu? Review 76. State the Objective #1 in the NYS Chemistry Curriculum for Chemistry… Review 76. State the Objective #1 in the NYS Chemistry Curriculum for Chemistry… The modern model of the atom has evolved over a long period of time through the work of many scientists. Scientist Name 77 78 79 80 81 82 many Model Name Details 77 Scientist Name Model Name Details Democritus (not a scientist) x The smallest part of anything was to be called “atomos” which is Greek for Atom 78 John Dalton Billiard Ball Atoms were like small hard spheres of different mass. 4 part Atomic Theory (important and coming soon) 79 J. J. Thomson Plum Pudding Discovered the Electron, put it “into” a positive mush, that kept atoms neutral. x Gold foil experiement proves electrons fly around the outside of a positive nucleus. (coming soon) Niels Bohr Planetary Put electrons into energy levels called ORBITS, discovered and explained spectra many Modern, or WaveMechanical Electrons are not in orbits, but rather in energy levels called orbitals. Fuzzier and more in tune with complex quantum math. 80 Ernest J. Rutherford 81 82 83. The 4 points of Dalton’s Atomic Theory 1. 2. 3. 4. 83. The 4 points of Dalton’s Atomic Theory 1. All elements are composed of individual kinds of atoms. 2. Atoms of one element are identical. Atoms of different elements have different masses. 3. Atoms can physically mix with other atoms. Atoms can also chemically combine with other atoms IN SIMPLE WHOLE NUMBER RATIOS, to form new substances. 4. Chemical reactions change the arrangement of atoms, but they do not become different kinds of atoms. 84. Draw the Gold Foil Experiment with labels 84. Draw the Gold Foil Experiment with labels 85. Explain what Rutherford Discovered and detail the problems with his new ideas. 85. Explain what Rutherford Discovered and detail the problems with his new ideas. With the Gold Foil experiment, Rutherford showed: An atom consists of a positively charged nucleus and is surrounded by electrons that spin around it. Electrons and neutrons are held together by opposite charge. The size of the nucleus is extremely small as compared to the size of the whole atom. The atom's entire mass is concentrated in the nucleus. Problems: He could not explain the stability of an atom, why didn’t the electrons collapse to the + charged nucleus, or fly away? The electrons revolving around should lose energy, which should slow them, causing collapse into the nucleus, but this didn’t seem to happen. The atom being 99% empty space should also mean we should almost be able to walk through walls, or see through everything, but we can’t. 86. Describe the Bohr Model (planetary) and spectra. 86. Describe the Bohr Model (planetary) and spectra. Bohr mathematically proved that if the electron of the hydrogen atom traveled at a set distance, at a set speed from the nucleus, somehow, it would never lose energy and never fly away and never be sucked in to the positive center of the atom. The math was too hard to prove for any other atom, but he concluded, they existed, the electrons spun around those nuclei, so just because he couldn’t do the math didn’t mean it wasn’t still true for them. 86. Describe the Bohr Model (planetary) and spectra. He further stated that the electrons all existed in ORBITS, and that each orbit was also an energy level. Electrons in the lower orbits had less energy than electrons in the higher orbits. And, he showed that the electrons lived in the ground state, or lowest energy levels possible most of the time. That was their NORMAL state. When looking at the atoms in increasing atomic number, the electrons filled these orbits in a simple pattern, lowest energy levels first. 86. Describe the Bohr Model (planetary) and spectra. Finally, electrons of an atom could gain a specific amount (a quanta) of energy, and get excited. The electron could move up to a higher energy orbit. This was unstable, and when the electron returned to the ground state, this unique quanta of energy was released, as unique visible light called spectra. We see spectra as a mixture of color (one color) but the light is many specific colors, all at specific wavelengths, a sort of optical fingerprint for each substance. 87. What’s the difference between orbit & orbital? 87.What’s the difference between orbit & orbital? Bohr said orbit for energy level. Now we have electrons in energy levels called ORBITALS. Orbit implies radius and a “neat” simple spinning around the nucleus. Orbital means “zone”, which is fuzzier in shape. NEAT ORBITS FUZZY ORBITALS 88. What’s the difference between SPECTRA and a SPECTRAGRAPH? The word “open” has neon gas that is excited by electricity. The spectra given off we see as ORANGE light with our eyes. That’s the mixture we see all at once. As seen through a refractive lens, we can see the unique colors that are broken apart by the prism of the lens. For a few dollars more the device used to see this, with numerals to measure the wavelengths in nanometers (quantitative measuring) Atom Ground state electron configuration Possible excited state configuration # of electrons is always 89 Mg – 12 2-8-2 2-7-3 12 90 Al – 13 2-8-3 2-7-4 13 91 C–6 2-4 2-3-1 6 92 Ca – 20 2-8-8-2 2-8-8-1-1 20 93 Fe – 26 2-8-14-2 2-8-13-3 26 Mark the correct electron configurations OK. Fix any that are wrong and state why they are wrong below. 94. Mg ground 2-8-2 OKAY 95. F ground 2-7 OKAY 96. He ground 2 OKAY 97. Ne ground 2-8-8 X 2-8 only 98. Mg excited 1-9-2 X only 8e- in 2nd orbital 99. He excited 1-1 OKAY 100. Ne excited 2-8-7-1 X 2-7-1 for neon 101. F excited 2-8 X only 9 total e- for F 102. P ground 2-9-4 X only 8e- in 2nd orbital