2. The History of the Atom……. Democritus was the first to theorize that all matter was composed of atoms! The name atom comes from his Greek word, “atomos”, which means not dividable or whole! Democritus’ ideas were crushed by a another Greek Philosopher, named……….

3. ………………Aristotle!!!! Aristotle asked Democritus three questions: If we are made of atoms, what holds us together? Why can’t we see these atoms? Why don’t we fall down like a bag of marbles?

4. Democritus was unable to answer these questions……. And so, people continued to think that matter was continuous - your body, the world around us was one continuous piece…. This philosophy continued for centuries…….

5. During the middle ages, science was lost to the world…… The only science that was done was performed by Arabs (Moors) out of Africa that conquered Spain!The only science that was done was performed by Arabs (Moors) out of Africa that conquered Spain! They traveled from the Middle East to Western Europe, carrying the great library of Alexandria with them!They traveled from the Middle East to Western Europe, carrying the great library of Alexandria with them! While the plague and the dark ages were killing millions, they had………..While the plague and the dark ages were killing millions, they had………..

6. EVERYTHING…..! Running water….. Dentistry….. Reading, Writing, Geometry, Calculus… Breweries……. Complex gardens and Agriculture…..

7. Science did not start up again until the Church was challenged…. The church was preventing people from coming up with new ideas and doing science! Who were some people that challenged the Church? Once the Church is challenged by thinkers, science experiments start to be done! With independence, came independent thought and ideas…..

8. During the 1700’s and 1800’s…. Scientists were discovering concepts and relationships Scientists were doing large, observable, basic experiments They weren’t doing tests with microscopes or computers! They were doing experiments with stoves, pots, ovens, and basic glassware! With observable properties came explanations!

9. Joseph Priestley……. Prepared pure Oxygen Decomposed mercuric oxide into mercury and oxygen Invented soda pop Discovered carbon dioxide and nitrous oxide (laughing gas)

10. Priestley noticed that the gas produced by heating mercuric oxide burned a candle brightly…. He called the air, “perfect air”, or “dephlogisticated air” People thought that phlogiston was a substance that was in materials When substances burned, they released phlogiston, which eventually caused flames to go out. Is this true….? He had actually discovered oxygen, but didn’t realize it!

11. Antoine Lavoisier….. Lived during the French Revolution Lived during the French Revolution Was a brilliant scientist, but a tax collector Was a brilliant scientist, but a tax collector Had his head chopped off during the revolution with royalty Had his head chopped off during the revolution with royalty

12. Lavoisier Proved….. That substances did not give off phlogiston, but used oxygen! He burned metals in the air, and weighed them before and after The substances weighed more after, because they were combining with oxygen, not giving off phlogiston!

13. By weighing the materials before and after….. Lavoisier came up with…….. Lavoisier came up with…….. The law of Conservation of Mass The law of Conservation of Mass This states: - Matter cannot be created or destroyed in a chemical reaction, simply converted from one form into another This states: - Matter cannot be created or destroyed in a chemical reaction, simply converted from one form into another The extra mass came from the oxygen in the air, which he later measured by reheating the compound formed The extra mass came from the oxygen in the air, which he later measured by reheating the compound formed

14. Joseph Proust….. Examined copper carbonate Examined copper carbonate No matter the amount, whenever decomposed it would yield 5.3 parts copper, 4.0 parts oxygen and 1.0 parts carbon No matter the amount, whenever decomposed it would yield 5.3 parts copper, 4.0 parts oxygen and 1.0 parts carbon Came up with the law of definite composition Came up with the law of definite composition All substances are composed of definite amounts of each element, no matter how much or how little of the matter there is! All substances are composed of definite amounts of each element, no matter how much or how little of the matter there is! This compound is always 5.3 parts Cu, 4.0 parts O, and 1.0 parts C!

15. John Dalton…… A schoolteacher! A schoolteacher! Devised the Law of Multiple Proportions Devised the Law of Multiple Proportions Stated that when two elements form more than one compound, they come together in whole number ratios…… Stated that when two elements form more than one compound, they come together in whole number ratios……

16. WHAT DOES THAT MEAN…? Carbon and Oxygen form two compounds: Carbon dioxide - C 1 O 2 Carbon monoxide - C 1 O 1 In carbon dioxide, C 1 O 2, carbon and oxygen combine in a 3 parts to 8 parts mass ratio In carbon monoxide, C 1 O 1, they do so in a 3 parts to 4 parts mass ratio….. Seem obvious….?

17. IT WASN’T…… Scientists didn’t know what was making things come together to react! In fact, They didn’t even know that atoms existed! If compounds come together in ratios, they must be made of smaller pieces!

18. John Dalton theorized that these substances were made of atoms! This led to………. This led to………. THE ATOMIC THEORY OF MATTER! All elements are made of tiny, solid, indestructible particles known as atoms All elements are made of tiny, solid, indestructible particles known as atoms All atoms of a given element are the same All atoms of a given element are the same Atoms of different elements are different Atoms of different elements are different Atoms of different elements form compounds in whole number ratios - 1 atom: 1atom, 1 atom: 2 atoms, etc. Atoms of different elements form compounds in whole number ratios - 1 atom: 1atom, 1 atom: 2 atoms, etc. A chemical reaction does not change the atoms themselves, only how they are combined to form compounds A chemical reaction does not change the atoms themselves, only how they are combined to form compounds Br H I Fe S

19. It took almost 2000 years before the idea of the atom came back! John Dalton brought Democritus’ idea back! John Dalton brought Democritus’ idea back! It seems simple, but people did not believe that matter was made of little marble-like structures called atoms! It seems simple, but people did not believe that matter was made of little marble-like structures called atoms! John Dalton’s theory was wrong in one respect…….. John Dalton’s theory was wrong in one respect……..

20. Atoms are not solid and indestructible like marbles….. They contain different parts……. However, scientists did not know this until parts of the atom were discovered….. What part of the atom do you think was discovered first…..?

21. THE ELECTRON…! Why do you think it was the first part of the atom to be discovered…..? Why do you think it was the first part of the atom to be discovered…..?

22. The electron is on the outside of the atom! The electron is on the outside of the atom! The electron is the ONLY part of the atom that can be added or removed to an atom! The electron is the ONLY part of the atom that can be added or removed to an atom! The electron is tiny and light, and that is why it can be added or removed! The electron is tiny and light, and that is why it can be added or removed! This is what we call electricity…moving electrons! This is what we call electricity…moving electrons! Technology wasn’t that good hundreds of years ago! Technology wasn’t that good hundreds of years ago! e - e - e - e - e - e - e - e - e -

23. The Early 1800’s! Lots of basic work with electricity Lots of basic work with electricity Matter has charge! Matter has charge! There are two types of “charge” in the world: There are two types of “charge” in the world:  + charged objects  - charged objects  Ben Franklin is the first to come up with these names - + and -  Franklin didn’t know that these charges were part of the atom - he didn’t even know that atoms existed, yet!

24. Cathode Ray Tube, or Crooke’s Tube This was one of the very first experiments to be done with electricity! A tube containing two metal electrodes or plates connected to a battery - and all of the gas is sucked out of the tube! William Crookes designed this tube in 1879 The cathode ray inside glows green Crookes was convinced this beam consisted of charged particles

25. So what are Cathode Rays….? J.J. Thomson, in 1897, answered this question! J.J. Thomson, in 1897, answered this question! Thomson used a Crooke’s tube and two charged plates above and below the beam Thomson used a Crooke’s tube and two charged plates above and below the beam Which way do you think the beam bent….? Which way do you think the beam bent….? The Beam was attracted to + plate, and was deflected from – plate! The Beam was attracted to + plate, and was deflected from – plate! From this, he said that the beam was made of negatively charged particles, called electrons! From this, he said that the beam was made of negatively charged particles, called electrons! He was looking at electrons, which are part of the atom! He was looking at electrons, which are part of the atom! These electrons can be easily taken off of atoms, and used as electricity! These electrons can be easily taken off of atoms, and used as electricity!

26. He also found that a magnet could move the beam as well!

27. The cathode ray tube was the beginning to the modern day….. TELEVISION! Black and White….. Color…….

28. Millikan Oil-Drop Experiment Robert Millikan in 1909 figured out the exact charge and mass of an electron Robert Millikan in 1909 figured out the exact charge and mass of an electron He placed oil drops in a box, and hit them with electrons He placed oil drops in a box, and hit them with electrons The oil drops were sprayed into the upper chamber The oil drops were sprayed into the upper chamber Some drops gained – charge (static electricity) Some drops gained – charge (static electricity)

29. Then Millikan adjusted the charge on the plates in the bottom of the box Then Millikan adjusted the charge on the plates in the bottom of the box The - particles attracted to the upper plate, because it was positive The - particles attracted to the upper plate, because it was positive It repelled the bottom plate, because it was negative It repelled the bottom plate, because it was negative This suspended the drop in space- he made them float in mid air! This suspended the drop in space- he made them float in mid air! From this he calculated the charge and mass of an electron, knowing the charge on the plates From this he calculated the charge and mass of an electron, knowing the charge on the plates The smallest change between two drops was taken to be charge of an electron The smallest change between two drops was taken to be charge of an electron - +

30. Now that we have found negative particles…. Eugen Goldstein in 1886 used a Crooke’s tube with holes in the negative end and discovered positive particles Eugen Goldstein in 1886 used a Crooke’s tube with holes in the negative end and discovered positive particles He shot a cathode beam (beam of electrons) at hydrogen atoms He shot a cathode beam (beam of electrons) at hydrogen atoms

31. The electrons from the atoms went with the beam of electrons to the + plate The electrons from the atoms went with the beam of electrons to the + plate He also saw + particles moving backwards towards the + plate and going through the holes! He also saw + particles moving backwards towards the + plate and going through the holes! He named these + particles “protons”! He named these + particles “protons”! + + +

32. Who puts all of this information together into “The Big Picture”? J.J. Thomson theorized that these negative and positive particles were actually part of matter - part of the atom! We are all made of charge! He develops the first working model of the atom, known as the PLUM PUDDING MODEL! This rejected Dalton’s idea that atoms were solid particles like marbles that weren’t made of smaller pieces NOT TRUE!

33. Why was any of this IMPORTANT…? People didn’t believe in atoms, and didn’t understand what things like electricity and light were! People didn’t believe in atoms, and didn’t understand what things like electricity and light were! Thomson showed that electricity was nothing more than a flow of little negative particles called electrons! Thomson showed that electricity was nothing more than a flow of little negative particles called electrons! And electrons, along with protons, make up every atom, in every person, plant, building and object in the universe And electrons, along with protons, make up every atom, in every person, plant, building and object in the universe We are made of charged particles - the same particles that we use for electricity! We are made of charged particles - the same particles that we use for electricity!

34. Why is Thomson’s model wrong….? A scientist named Ernest Rutherford figured it out! A scientist named Ernest Rutherford figured it out! He shoots big heavy alpha (  ) particles at ultra thin gold foil He shoots big heavy alpha (  ) particles at ultra thin gold foil Most of the particles went straight through, and did NOTHING. Most of the particles went straight through, and did NOTHING. A very few were deflected, and some even bounced straight back! A very few were deflected, and some even bounced straight back! Rutherford described this as a bowling ball being sent at a piece of paper, full speed, and bouncing back! Rutherford described this as a bowling ball being sent at a piece of paper, full speed, and bouncing back!

35. The Gold Foil Experiment…. What is happening? Why are the alpha particles bouncing off?

36. Gold Foil Experiment…..

37. What is going on….? Most of the alpha particles are going straight through! Most of the alpha particles are going straight through! A few of the alpha particles are bouncing off of something! A few of the alpha particles are bouncing off of something! Alpha particles are big, and positive! Alpha particles are big, and positive! What could they be bouncing off of? What could they be bouncing off of? They must be bouncing off of something that is…. They must be bouncing off of something that is…. Positive! Positive! And big! And big! Rutherford theorized that all of the protons weren’t scattered about, like in a chocolate chip cookie, but were all concentrated into a tiny, dense center, which he called the nucleus! Rutherford theorized that all of the protons weren’t scattered about, like in a chocolate chip cookie, but were all concentrated into a tiny, dense center, which he called the nucleus! The electrons must be orbiting around this nucleus! Why????? The electrons must be orbiting around this nucleus! Why?????

38. Rutherford’s “nuclear” model!

39. What is the relative size of the atom….? An atomic model the size of Busch Stadium and parking would contain a pea sized nucleus containing 95.95% of the atoms mass. An atomic model the size of Busch Stadium and parking would contain a pea sized nucleus containing 95.95% of the atoms mass. The pea at the pitcher’s mound would be the nucleus, and an ant crawling on the parking lot outside would be an electron! The pea at the pitcher’s mound would be the nucleus, and an ant crawling on the parking lot outside would be an electron! The atom is mostly….. The atom is mostly….. Empty space! Nothing! Empty space! Nothing!

40. So is this the final model of the atom today…? No! No! A scientist named Neils Bohr, a great friend of Einstein, noticed something weird about Hydrogen A scientist named Neils Bohr, a great friend of Einstein, noticed something weird about Hydrogen A hydrogen atom consists of 1 electron orbiting 1 proton…. A hydrogen atom consists of 1 electron orbiting 1 proton…. Atoms can give off light when they are excited with electricity! Atoms can give off light when they are excited with electricity! Think about light bulbs, neon lights, headlights…. Think about light bulbs, neon lights, headlights…. With one electron, how many different types of energy or colors of light do you think hydrogen can give off….? With one electron, how many different types of energy or colors of light do you think hydrogen can give off….?

41. …. Only one color of light! Bohr excited hydrogen atoms with high voltage electricity Bohr excited hydrogen atoms with high voltage electricity Hydrogen gave off violet light…. Hydrogen gave off violet light…. The violet light was actually FOUR DIFFERENT COLORS OF LIGHT, as viewed through a prism The violet light was actually FOUR DIFFERENT COLORS OF LIGHT, as viewed through a prism How can one electron give off four colors of light??? How can one electron give off four colors of light???

42. HOW IS THIS POSSIBLE…? It doesn’t make sense that one electron can give off four different colors of light! It doesn’t make sense that one electron can give off four different colors of light! Hydrogen, with only one electron, should be giving off just one color! Hydrogen, with only one electron, should be giving off just one color! Bohr came up with an explanation for this…. Bohr came up with an explanation for this…. It involved changing the current accepted model of the atom! It involved changing the current accepted model of the atom! It doesn’t make sense that one electron can give off four different colors of light! It doesn’t make sense that one electron can give off four different colors of light! Hydrogen, with only one electron, should be giving off just one color! Hydrogen, with only one electron, should be giving off just one color! Bohr came up with an explanation for this…. Bohr came up with an explanation for this…. It involved changing the current accepted model of the atom! It involved changing the current accepted model of the atom!

43. Bohr came up with a new model for the atom… Bohr suggested that it electrons could move to many locations or “energy levels” within the atom! Bohr suggested that it electrons could move to many locations or “energy levels” within the atom! The electron was moving to more than one location in the atom! The electron was moving to more than one location in the atom! In Bohr’s Model of the atom, electrons orbit the nucleus like planets orbit the sun. It is called THE PLANETARY MODEL. In Bohr’s Model of the atom, electrons orbit the nucleus like planets orbit the sun. It is called THE PLANETARY MODEL. When electrons jump up to different energy levels, they eventually fall back down and give off light! When electrons jump up to different energy levels, they eventually fall back down and give off light!

44. Electron can jump up, and when they fall back down, they give off colors of light!Electron can jump up, and when they fall back down, they give off colors of light!

45. The colors we see for Hydrogen……

46. Different substances give off different colors….Why?

47. Carbon Helium Neon Different elements have different electrons, that can jump to different places in the atom!

49. Electrons in Energy Levels Level maximum number of electrons Level maximum number of electrons 12 12 28 28 318 318 432 432

50. Another problem with the puzzle…. Werner Heisenberg, a famous German scientist, suggested that it was impossible to know exactly where an electron was at all times! Werner Heisenberg, a famous German scientist, suggested that it was impossible to know exactly where an electron was at all times! To watch an electron orbit the nucleus would require light! To watch an electron orbit the nucleus would require light! Shining light on an electron might do what….? Shining light on an electron might do what….? Move it! Move it! And electrons are so small, and move so fast, that we would lose where it would go! And electrons are so small, and move so fast, that we would lose where it would go! The Heisenberg Uncertainty Principle: It is impossible to simultaneously know an electron’s location and speed around the nucleus of an atom. The Heisenberg Uncertainty Principle: It is impossible to simultaneously know an electron’s location and speed around the nucleus of an atom. Unknown new location Photon of light

51. So what does THAT mean??? Electrons travel around the nucleus, and we can’t be sure where they are some of the time! Electrons travel around the nucleus, and we can’t be sure where they are some of the time! Erwin Schrodinger used complicated mathematics and probability to calculate where electrons were most likely to be located. Erwin Schrodinger used complicated mathematics and probability to calculate where electrons were most likely to be located. This new model, called the Quantum Mechanical Model predicts the probability of where the electron is going to be 90% of the time! This new model, called the Quantum Mechanical Model predicts the probability of where the electron is going to be 90% of the time! It is also called the electron cloud model or the 90% probability model! It is also called the electron cloud model or the 90% probability model! It means that we THINK that the electron is located in some region or “cloud” of space, 90% of the time! But if we went looking for it by shining light on it, it might move to some unpredictable location! It means that we THINK that the electron is located in some region or “cloud” of space, 90% of the time! But if we went looking for it by shining light on it, it might move to some unpredictable location!

52. A model where we don’t know where the electron is??? But Schrodinger did calculations to figure out exactly where in the energy levels we could probably find the electron…. These locations were called sublevels…. Even within these sublevels, Schrodinger figured out what shape an electron would be located in when it moved……called an orbital! So remember, electrons don’t travel in nice circular orbits…they travel in unpredictable, wavelike patterns in a 3-dimensional area….These areas are called sublevels…..the electron could be there at any time! It would be like taking a snapshot picture….The orbital is a collection of all of the potential snapshots… A model where we don’t know where the electron is??? But Schrodinger did calculations to figure out exactly where in the energy levels we could probably find the electron…. These locations were called sublevels…. Even within these sublevels, Schrodinger figured out what shape an electron would be located in when it moved……called an orbital! So remember, electrons don’t travel in nice circular orbits…they travel in unpredictable, wavelike patterns in a 3-dimensional area….These areas are called sublevels…..the electron could be there at any time! It would be like taking a snapshot picture….The orbital is a collection of all of the potential snapshots… Sounds really vague and inaccurate, huh?

53. Why do we care about where the electrons are so much??? The electrons are the outside part of the atom! The electrons are the outside part of the atom! They are the only part of the atom that can be added or removed! They are the only part of the atom that can be added or removed! They are what make an atom “react”! Where they are has everything to do with how an atom will “react”! They are what make an atom “react”! Where they are has everything to do with how an atom will “react”!

54. Insert figure 5.31 s, p, d, and f Sublevels

55. Some hints…. 1.Any energy level “n” has exactly n sublevels in it 2.Each sublevel has a specific number of orbitals, as seen on the chart below 3.Since electrons don’t like each other, having the same charge and repelling each other, an orbital can hold a maximum of only 2 e -. This is known as the Pauli Exclusion Principle. 4.Remember - a sublevel simply tells us where an electron is located, and an orbital tells us something about the shape that it moves within as it travels in a wave! Some hints…. 1.Any energy level “n” has exactly n sublevels in it 2.Each sublevel has a specific number of orbitals, as seen on the chart below 3.Since electrons don’t like each other, having the same charge and repelling each other, an orbital can hold a maximum of only 2 e -. This is known as the Pauli Exclusion Principle. 4.Remember - a sublevel simply tells us where an electron is located, and an orbital tells us something about the shape that it moves within as it travels in a wave! n# sublevels“names” 11s 22s, p 33s, p, d 44s, p, d, f 54s, p, d, f 3 2 1 level 2 6 10 135135 spdspd 2626 1313 spsp 21s Max no. of e - No. of orbitalsublevel 8 18 105d 147f 63p 21s Max no. of e - No. of orbitalsublevel

56. Who wants to draw complicated atoms with these sublevels and orbitals included in the picture…? Instead, we can use shorthand for where the electrons are located! There are two shorthand ways of indicating where electrons are located: Electron Configurations Orbital Diagrams Let’s look at each and discuss why we use them!

57. Electron Configurations We use this shorthand to indicate where electrons live… We use this shorthand to indicate where electrons live… We use numbers to indicate the energy level, letters to indicate the shape or sublevel, and superscripts (exponents) to indicate how many electrons there are in a particular sublevel! We use numbers to indicate the energy level, letters to indicate the shape or sublevel, and superscripts (exponents) to indicate how many electrons there are in a particular sublevel! For example, Lithium would be written as: For example, Lithium would be written as: Li = 1s 2 2s 1 Li = 1s 2 2s 1 Notice there are 3 electrons total - 2 electrons in the s sublevel of the 1st energy level, and 1 electron in the s sublevel of the 2nd energy level! Notice there are 3 electrons total - 2 electrons in the s sublevel of the 1st energy level, and 1 electron in the s sublevel of the 2nd energy level! Li = 1s 2 2s 1 energy level sublevel # of electrons

58. What energy level would an electron fill first…? The lowest possible energy level, of course! The lowest possible energy level, of course! Electrons are negative! Electrons are negative! They want to be as close to the nucleus as possible! They want to be as close to the nucleus as possible! This is the lowest energy, most stable location.. This is the lowest energy, most stable location.. This is known as the Aufbau Principle… This is known as the Aufbau Principle…  Electrons fill lowest energy levels first! Can we write the electron configuration for sodium, then? Can we write the electron configuration for sodium, then? Sodium has…. Sodium has…. 11 electrons! 11 electrons! We know that electrons would first occupy the first energy level! We know that electrons would first occupy the first energy level! Once that is filled, they would then fill the second, and then the third, etc. Once that is filled, they would then fill the second, and then the third, etc. Na = 1s 2 2s 2 2p 6 3s 1

59. Inverted Triangle Apartment Building Floor = n Apt = orbital (s, p, d, f) s = 1 bedroom = 2 e- p = 3 bedroom = 6 e- d = 5 bedroom = 10 e- f = 7 bedroom = 14 e- (2 e- per room)

60. Electron Configurations Notice the violation of the Aufbau Principle….

61. 7s 7p.......... 6s 6p 6d 6f.... 5s 5p 5d 5f.. 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s Electron Configurations Look at potassium… 19 electrons… You would think its configuration would be… K = 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 Instead, it is… K = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 This is known as a violation of the Aufbau Principle! Why would an atom DO THIS????

62. Insert figure 5.36

63. The second way to show where electrons are located is called an orbital diagram… This is a better way of actually seeing where electrons are! This is a better way of actually seeing where electrons are! We draw square boxes to indicate sublevels…. We draw square boxes to indicate sublevels…. We draw up and down arrows to indicate electrons… We draw up and down arrows to indicate electrons… Oxygen would be written like this…. Oxygen would be written like this…. O = Each box represents a shape - a sphere, a figure 8, etc.Each box represents a shape - a sphere, a figure 8, etc. Notice anything weird about this…?Notice anything weird about this…? The last two electrons filled separate orbitals first!The last two electrons filled separate orbitals first! Why would they fill separate p orbitals first, instead of just going into the same orbital?Why would they fill separate p orbitals first, instead of just going into the same orbital? Electrons repel each other, and want to stay as far away from each other as possible!Electrons repel each other, and want to stay as far away from each other as possible! This is known as Hund’s rule - electrons fill singly occupied orbitals first!This is known as Hund’s rule - electrons fill singly occupied orbitals first! An orbital diagram….

64. Marble Model Plum Pudding Model The Nuclear Model The Planetary Model

65. Why is learning about the atom important….? The atom was considered to be an “imaginary” thing, something that people laughed at! The atom was considered to be an “imaginary” thing, something that people laughed at! Roosevelt trusted Einstein, and funded his secret research known as the “Manhattan Project” Roosevelt trusted Einstein, and funded his secret research known as the “Manhattan Project” In a few short years, the idea of an invisible atom had been developed into a city-destroying weapon - the atomic bomb! They figured out they could split atoms apart, and this would release tons of energy! In a few short years, the idea of an invisible atom had been developed into a city-destroying weapon - the atomic bomb! They figured out they could split atoms apart, and this would release tons of energy!

66. In Hiroshima, of a resident civilian population of 250,000 it was estimated that 45,000 died on the first day and a further 19,000 during the subsequent four months. In Nagasaki, out of a population of 174,000, 22,000 died on the first day and another 17,000 within four months. Over 90% of each city was destroyed. Only two atomic bombs have ever been used in wartime history - The U.S. used them both against Japan to end World War II…. The first video shows one of the actual bombs being detonated….The second, the first testing of a “Hydrogen” Bomb…