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Use your jigsaw notes: 1. Which atomic model showed the probable locations of electrons? 2. Which atomic model was the first to show the nucleus of an atom? 3. Which atomic model was first to show energy levels? Day 1 12-13 We have Atoms! – 1898 Marie Skłodowska Curie and Pierre Curie • Investigated radiation and its _________ behaviors. • The chemical properties of radioactive elements change as radiation _______ is emitted. We have Atoms! – 1898 Marie Skłodowska Curie and Pierre Curie • Isolated and discovered the polonium elements _________ radium and ________. We have Atoms! – 1899 Ernest Rutherford radiation to determine • Analyzed ________ composition its ___________. Alpha particles , are fairly –______________, positive charge. heavy with a ________ Beta particles , are –_____________, negative very tiny with a ________ charge. We have Atoms! – 1899 Ernest Rutherford Beta particles , are –_____________, negative very tiny with a ________ charge. Gamma rays g , have no –____________, neutral mass with a _______ charge. Radiation Penetration Radiation Separation • What does this separation pattern indicate about charges and masses of these types of radiation? larger mass and ________ positive charge –α: ______ –β: ________ smaller mass and _________ negative charge Radiation Separation • What does this separation pattern indicate about charges and masses of these types of radiation? smaller mass and _________ negative –β: ________ charge no mass and ___ no charge –γ: ___ Atoms defy what we thought we knew! - 1900 Max Planck realized that atoms have their own rules _________________. Good-bye, Newtonian physics! Hello, Quantum Physics! Atoms defy what we thought we knew! 1902 • Ernest Rutherford and Frederick Soddy discovered that radioactivity produces elements new __________ • Nuclear decay of uranium238 Atoms defy what we thought we knew! 1902 • Nuclear decay of uranium238 Mass # 238U → 234 Th + 4He 2 92 90 Atomic # uranium-238 → thorium-234 + α particle Use your notes: 1. Which type of radiation is the most dangerous (penetrating)? 2. Which type of radiation is made up of high speed electrons? Day 2 12-14 Read pages 105-109 and answer #s 9-15 on page 109 Atoms defy what we thought we knew! 1902 • Nuclear decay of uranium238 Mass # 238U → 234 Th + 4He 2 92 90 Atomic # uranium-238 → thorium-234 + α particle Mass # = protons + neutrons Atomic # = protons – periodic table Write the nuclear symbol for Carbon with 6 neutrons Write the nuclear symbol for Carbon with 8 neutrons Practice For Neon with 9 neutrons: 19 Mass #? _____ # of protons? _____ 10 10 atomic #? _____ Write the nuclear symbol: Practice If an atom has 7 protons + 9 neutrons: 16 Mass #? _____ element = ? _________ nitrogen atomic #? ____ 7 Write the nuclear symbol: Practice Uranium-239: 239 Mass #? _____ protons? ____ 92 atomic #? ____ 92 Write the nuclear symbol: Practice If an atom has 17 protons + 18 neutrons: 35 Mass #? _____ element = ? __________ chlorine atomic #? ____ 17 Write the nuclear symbol: Assignment # 1 Unit 3 Atoms defy what we thought we knew! 1909-1910 • Ernest Rutherford’s –Experiment applet #1 –Experiment applet #2 • Ernest Rutherford’s Atom’s appearance: Hollow sphere – ____________________ Dense center with positive charge – ____________________________________ Electrons occupy empty space – ________________________________ Atoms defy what we thought we knew! 1912 - 1913 • Neils Bohr - modified Rutherford’s atomic model. specific –Electrons are located in _______ energy ______. levels ______ Used this model to explain emission __________ spectra _________ Atoms defy what we thought we knew! 1912 - 1913 • Neils Bohr - modified Rutherford’s atomic model. –When an electron becomes excited (gains energy) it can jump up to a new energy level. When it falls back down to its ground state it emits energy (light). Atoms defy what we thought we knew! 1913 • Frederick Soddy coined the term isotope _______ –Atoms of the same ________ element weight –Differ in _______ radioactivity –Differ in ___________ –Examples Carbon-12 and Carbon-13 • ________________________ Uranium-236 and Uranium-238 • _________________________ Atoms defy what we thought we knew! 1913 • Henry Moseley atomic ________ numbers to –Assigned ______ each element –Realized that something in nucleus of the _______ an atom determines … Atoms defy what we thought we knew! 1913 • Henry Moseley –Realized that something in nucleus of the _______ an atom determines its position on the _______ _____. Periodic Table Atoms defy what we thought we knew! 1919 • Ernest Rutherford discovered protons _______ positive charge and are –Carry a _______ nucleus found in the ______. protons is the –The number of _______ number atom’s atomic ______ _______. artificial –Conducted the first _______ transmutation reaction, … ____________ Atoms defy what we thought we knew! 1919 • Ernest Rutherford discovered protons _______ artificial –Conducted the first _______ transmutation reaction, changing ____________ nitrogen-14 into the the element __________ element ________ oxygen-17 14N 7 + 4He 2 → 17 O 8 + 1H 1 Atoms defy what we thought we knew! 1926 quantum • Neils Bohr’s ________model of the atom –______ _____ Empty sphere Nucleus is dense center with –_______ positive _______ protons ______ Electrons found in specific –________ energy levels Atoms defy what we thought we knew! 1926 quantum • Neils Bohr’s ________model of the atom Electrons found in specific –________ energy levels –Formula for the maximum number of e- per level: e 2 2n Max # = n = number of energy level Atoms defy what we thought we knew! 1932 • James Chadwick neutrons discovered _________ charge –Have no _______ –Located in the atom’s nucleus _______ Atoms defy what we thought we knew! 1938 • Lise Meitner was the first to correctly describe a nuclear fission ________ reaction in which a large nucleus is split into two smaller nuclei of approximately equal size. 235U + 1n → 236 92 0 92 236 1 141 92 n 3( ) → Ba + Kr + 92 0 56 36 U U Today: Is matter continuous or discontinuous? • What are protons, neutrons, and electrons made of? quarks, bosons, muons, gluons, etc! • What about string theory? Is there a tiniest piece of energy that everything is made of? Today: Is matter continuous or discontinuous? Is there a tiniest piece of energy that everything is made of? • When you ask “What is the smallest piece?”, be certain to specify what you want! –Cmpd. = group of bonded atoms –Element = single atom –Atom = ?? Parts of Atoms, Isotopes, and Ions • Isotopes –Atoms of one element protons • Same number of _______ neutrons • Different numbers of ________ masses • Different ______ Parts of Atoms, Isotopes, and Ions • Ions –________ Charged atoms that have gained electrons or lost ________ –Examples • Iron loses 2 electrons +2 Fe • Chlorine gains 1 electron -1 Cl Page 104 #s 1-4 Read pages 105-109 and answer #s 9-15 on page 109