1. How can we describe an atom? How can atoms of the same element be both similar and different at the same time? What do we call an atom that is not neutral? How can we calculate the average mass of isotopes? How has the model of the atom evolved over time? How can we describe the modern model of the atom? How can we describe where are electrons are located within the electron cloud? How can we describe how electrons are arranged? What is electromagnetic radiation? How is light produced? - Regents Chemistry

3. AIM: How can we describe an atom? The Theory of the Atom ________________, a famous Greek teacher who lived in the 4th Century B.C., first suggested the idea of the atom. ________ __________ came up with his atomic theory based on the results of his experiments. The Atom The smallest particle of an ________________ is an atom. The atom is made up of three ________________ particles. (1)The electron was discovered in _______ by J. J. Thomson by using a cathode ray tube. The electron has a _______ charge. It’s mass is much smaller than the other 2 subatomic particles, therefore it’s mass is usually ______________. Democritus John Dalton element subatomic 1897 (−)(−) ignored

5. (2) The proton has a ______ charge, and it was discovered in _________ by E. Goldstein. (3) The neutron does not have a charge. In other words, it is ________. It was discovered in ____ by James Chadwick. The neutron has about the same _________ as the proton. * These three particles make up all the ____________________ in the Universe! * There are other particles such as neutrinos, positrons, and quarks, but are typically left for 2 nd year chemistry courses. neutral1932 mass visible matter (+) 1886

6. Nuclear Atomic Structure * The atom is made up of 2 parts/sections: (1) The ______________ --- (in the center of the atom) (2) The ____________ _________ --- (surrounds the nucleus) nucleus electron cloud (p + & n 0 ) e − cloud

7. The Nucleus * Discovered by Ernest ________________ in ________. * He shot a beam of positively charged “alpha particles”, which are ___________ nuclei, at a thin sheet of ______ _____. * 99.9% of the particles went right on through to the ______________. Some were slightly deflected. Some even ____________ ________ towards the source! This would be like shooting a cannon ball at a piece of tissue paper and having it bounce off. Rutherford1911 heliumgold foil detector bounced back

9. (1) Most of the atom is more or less _________ ___________. (2) The nucleus is very _________. (Stadium Analogy) (3) The nucleus is very ___________. (Large Mass ÷ Small Volume) (4) The nucleus is ______________ charged. empty space dense tiny positively Counting Subatomic Particles in an Atom The atomic # of an element equals the number of ____________ in the nucleus. The mass # of an element equals the sum of the _____________ and ______________ in the nucleus. In a neutral atom, the # of protons = # of ______________. To calculate the # of neutrons in the nucleus, ______________ the ___________ # from the __________ #. protons neutrons electrons subtract atomicmass

10. Atomic Models (1) Model: a ball of (+) charge containing a number of e - no ________________ often described as the “________ _______________” atom. (2) Model: a ____________ of (+) charge surrounded by a number of e - no _____________ and no e - orbitals Thomson nucleus plum pudding Rutherford nucleus neutrons

11. (3) Model: a nucleus of (+) charge that also contains ______________ nucleus is encircled by e - ’s located in definite orbits (or paths). e - ’s have ___________ energies in these orbits e - ’s do not lose energy as they orbit the nucleus (4) Mechanical Model ( Wave Mechanical Model) no definite ____________ to the e - path (“fuzzy” cloud) orbits of e - ’s based on the _________________ of finding the e - in the particular orbital shape. Atomic Models Bohr neutrons fixed Quantum shape probability

13. Bohr Atomic Model

17. Quantum Mechanical Model

19. (1) Find the # of e -, p + and n 0 for sodium. (mass # = 23) 2) Find the # of e -, p + and n 0 for uranium. (mass # = 238) 3) What is the atomic # and mass # for the following atom? # e - = 15; # n 0 = 16 Atomic # = 11 = # e - = # p + # neutrons = 23-11 = 12 Atomic # = 92 = # e - = # p + # neutrons = 238-92 = 146 Atomic # = 15 = # e - = # p + Mass # = p + + n 0 = 15+16 =31 The element is phosphorus!

20. * An atom can gain or lose electrons to become electrically charged. * Cation = (___) charged atom created by ___________ e-’s. * Cations are ______________ than the original atom. * _____________ generally form cations. * Anion = (___) charged atom created by _____________ e-’s. * Anions are ____________ than the original atom. * _______________ generally form anions. Practice Problems: Count the # of protons & electrons in each ion. a) Mg +2 p + = _____ e − = ______ b) F −1 p + = _____ e − = ______ +losing smaller Metals −gaining larger Nonmetals 1210 9

21. REMEMBER  P….E….N

22. Element NameSymbolAtomic #AMU# of Protons # of Electrons # of Neutrons K19 5 16 23 10 48 25 14 Potassium39 20 51 Si 32 23 48 25 S V 10 23 20 5 6 11 5 B Boron Sulfur Vanadium Neon Cadmium Manganese Silicon Ne Cd Mn 112 55 28 16 48 14 25 16 19 10 14 16 28 10 64 30

23. * AIM: How can atoms of the same element be both similar and different at the same time?- Isotopes

24. * An isotope refers to atoms that have the same # of ___________, but they have a different # of ___________. * Because of this, they have different _________ #’s (or simply, different ___________.) * Isotopes are the same element, but the atoms weigh a different amount because of the # of ______________. Examples---> (1) Carbon-12 & Carbon-13 (2) Chlorine-35 & Chlorine-37 (The # shown after the name is the mass #.) * For each example, the elements have identical ___________ #’s, (# of p + ) but different _________ #’s, (# of n 0 ). * Another way to write the isotopes in shorthand is as follows: CCl 12 6 35 17 The top number is the ________ #, and the bottom # is the __________ number. Calculating the # n 0 can be found by _____________ the #’s! protons neutrons mass masses neutrons atomic mass atomic subtracting

25. Isotopes

26. (1) Find the # e -, p + and n 0 for Xe-131. 2) Find the # e -, p + and n 0 for 3) Write a shorthand way to represent the following isotope: # e - = 1 # n 0 = 0 # p + = 1 Cu 63 29 Atomic # = 54 = p + = e − n 0 = 131 − 54 = 77 Atomic # = 29 = p + = e − n 0 = 63 − 29 = 34 Atomic # = p + = e − = 1 mass # = n 0 + p + = 1+ 0 = 1 H-1 orH 1 1

27. * What do we call an atom that is not neutral?How can we calculate the average mass of isotopes? Element Name SymbolAtomic #Mass ##Protons#Electrons#Neutrons 17 22 Ar 9 Complete The Chart in your notes

28. Nucleons: particles in the nucleus (protons and neutrons) Nuclear Charge: charge of the nucleus (same as # of protons) Examples: 1. How many nucleons are there in an atom with an atomic number of 20 and 23 neutrons? 2. What is the nuclear charge of an Iron atom? 43 26

29. * Based on the relative mass of Carbon-12 which is exactly _______. * 1 p + ≈ __ atomic mass unit (amu) 1 n 0 ≈ __ amu 1e - ≈ __ amu * The atomic masses listed in the Periodic Table are a “weighted average” of all the isotopes of the element. 12 110 Weighted Average Practice Problems: (1) Mrs. Smith’s geometry semester grades are calculated using a weighted average of three category scores: Major Grades= 60% of your grade Minor Grades= 30% of your grade Semester Exam=10% of your grade If a student had the following scores, what would they receive for the semester? Major= 80 (B − ) Minor= 60 (D −) Semester Exam=65 (D)

30. Step (1): Multiply each score by the % that it is weighted. Step (2): Add these products up, and that is the weighted average! 60% x 80 = 48.0 30% x 60 = 18.0 10% x 65 = 6.5 Add them up!! A “normal average” would be calculated by simply adding the raw scores together and dividing by 3… 80 + 60 + 65 = 205 ÷ 3 = 68.3 = D + 72.5 (C−)

31. Practice Problems: (2) In chemistry, chlorine has 2 isotopes: Cl-35 (75.8% abundance) Cl-37 (24.23 % abundance) What is the weighted average atomic mass of chlorine? 35 x 0.758 = 26.53 37 x 0.2423 = 8.9651 Add them up!!! (3) Oxygen has 3 isotopes: O-16 (99.76%) O-17 (0.037%) O-18 (0.2%) Estimate oxygen’s average atomic mass. + 35.4951 amu Barely over 16.0 amu

32. (4) Copper has an average atomic mass of 63.546 amu. It contains only two natural isotopes, which are Cu-63, with an isotope mass of 62.940 and Cu-65 with an isotope mass of 64.928. What are the percent of the two isotopes in naturally occurring copper? Avg. Atomic Mass = (% Cu-63 x Mass Cu-63 ) + (% Cu-65 x Mass Cu-65 ) 63.546 = (% Cu-63 x 62.940) + (% Cu-65 x 64.928) % Cu-63 + % Cu-65 = 100% % Cu-63 + % Cu-65 = 1 OR

33. Page 13 in your packets # 1 and 2

35. Diagram: The energy levels in an atom are sort of like _________ of a ladder. The more energy an electron has, the __________ away from the nucleus it usually will be. The energy levels are not evenly spaced. They get ___________ together as you travel farther away. To move from one “rung” to another requires a “____________” of energy. AIM: How can we describe where electrons are located? - Energy Levels rungs farther closer quantum

36. continuous energy levelsquantized energy levels

37. * Describe the ______________ of the e - ’s around the nucleus. * Quantum #’s are sort of like a home _____________ for the electron. * This information about the location of the e - ’s in an atom can be used to: (1) determine chemical & physical _____________ for the elements. (2) show how the _______________ __________ is organized. (3) show _____ and _____ elements combine to form compounds. location address properties Periodic Table howwhy

38. s s s s p p p f d d

41. Practice Problems: Write the electron configuration notation for each of the following atoms: * H * C * Fe * Br 1 2-4 2-8-14-2 2-8-18-7

42. October 9 th, 2014 Complete questions 11-20 on the worksheet I asked you to print last night

43. * How do electron configurations relate to the chemical and physical properties of an element? * All elements with the _________ outer shell e - configurations have ________ properties. * This means that elements in the same ____________ group have similar properties. Examples: (1) Li, Na, K, Rb, and Cs all have __ lone “__” e - for their last orbital... (_____, _____, _____, etc.) This makes all of them ___________ reactive. They all react with __________ to produce hydrogen gas. (2) Ne, Ar, Kr, Xe, and Rn all have the outer energy level completely __________ with electrons...(________, ________, ________, etc.) This makes all of them ______________. They do not produce __________________! same similar vertical 1s 2s 1 3s 1 4s 1 verywater filled2s 2 2p 6 3s 2 3p 6 4s 2 4p 6 inert compounds

44. * When atoms get hit with energy (by _____________ them with electricity or by ____________ them up), the electrons absorb this energy and __________ to a higher energy level. Figure (a) * As they immediately fall back down to the “____________ state”, they give off this energy in the form of a particle of ___________ (or other types of electromagnetic radiation) called a _____________. Figure (b) zapping heating jump ground light photon

46. Complete the first page of the electron configuration packet Valence electrons are the electrons in the last shell Kernal electrons are all the electrons other than the ones in the last shell

47. * Each photon emitted has a specific ___________ (or frequency). * The color of the light that is given off depends on how _____ the electron _______ (which depends on how big of a jump it originally made.) The farther the fall, the ___________ energy the photon has. color farfell greater

49. Friday 10/10/14 – D day : DO NOW: Answer the following questions 1. What is the excited state 2. What is the ground state (where can you find the ground state configurations for a given element 3. What is the ground state configuration for Ne 4. Write a possible excited state for S 5. What happens to electrons as they move from an excited state to the ground state?

50. * Since electrons are located only in certain __________ levels (or orbitals) around the nucleus, only certain specific _________ of light are emitted. * Scientists use a _________________ to separate these colors into bands of light. These bands of color look like a ______ code of color which is characteristic of that element. No two elements produce the same ______________ of colors. This can be used to distinguish one element from another contained in a sample. (See Fig. 13.11) energy color spectroscope bar spectrum

51. Hydrogen Spectrum Neon Spectrum

52. CONCLUSION :

53. Hydrogen Helium Neon Sodium Mercury Emission Spectrum Lab