Campbell Chemistry Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature

Transcription

1 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature Name: Schedule 9/1 Thurs 9/2 Fri In Class Using Lab Equipment Lab Polyatomic Ion and Elements Quiz Ionic nomenclature Homework (to be completed before coming to the NEXT class period) Study polyatomic ions and elements Over the long weekend: Watch Chapter 4 Video 1: The History of the Development of Atomic Theory Video & complete guided notes and learning check problems. 9/5 Mon Labor Day NO SCHOOL 9/6 Tues Discuss summaries and questions from video 9/7 Wed Atomic structure and identifying amounts of subatomic particles discuss and practice problems 9/8 Thurs Discuss charged particles and how those charges form chemical compounds Watch Chapter 4 Video 2: Atomic Structure Video & complete guided notes and learning check problems. Watch Chapter 4 Video 3: Elements with Charge video & complete guided notes and learning check problems. Complete Prelab for Percent Composition Lab 9/9 Fri Percent Composition Lab 9/12 Mon Late Start Continue to discuss Ionic Nomenclature (optional: watch supplemental video on ionic nomenclature in Chapter 4 playlist on my YouTube Channel) 9/13 Tues Review for Chapter 4 Test Study for Chapter 4 Test 9/14 Wed Chapter 4 Test 1

2 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature History of the Development of Atomic Theory: Video: Textbook: Chapter pages Guided Notes for Video on the History What did Democritus say about the composition of matter Name: Questions: What are the four parts of John Daltons Atomic Theory What is a cathode ray tube? What did JJ Thomson use the cathode ray tube to discover? What is the plum pudding model; draw a picture of the model. Who came up with this model? What was did Robert Millikan discover and what experiment did he use to do it? 2

3 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature Name: What were the results of Rutherford's experiment? How did these results change the model of the atom? Draw his model of the atom. What did James Chadwick discover and what year was it? Learning Check: Answer the following multiple choice questions. Check your answers at the bottom of the page. 1. Who first thought matter was made of atoms? a) Dalton b) Thomson c) Aristotle d) Democritus 2. Which one of the following associations of a scientist and a discovery is correct? A) James Chadwick - protons B) Dalton atomic theory C) E. Rutherford - nucleus D) J.J. Thomson- atoms 3. Which of the following is NOT a part of Dalton s atomic theory? a) atoms combine in simple whole number ratios to make compounds b) in a chemical reaction, elements are destroyed c) matter is composed of small particles called atoms d) atoms of each element are different Answers to the above will be discussed in class so make sure you attempt them!!! 3

4 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature Name: Atomic Structure, subatomic particles and numbers: Video: Textbook: Chapter 4.3 pages Guided Notes for Video on Atomic Structure Questions: What are the three subatomic particles? Recreate the table of particle/location/charge/mas s below: How are the atoms of each element different? What is the atomic number and how can I find out what the atomic number for an element is? How are the number of electrons related to the number of protons in a neutral atom? What is the mass number? How can I find the number of neutrons using the mass number and atomic number? What are isotopes and how are they the same? How are they different? 4

5 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature What is the atomic mass of an element? Name: For the special notation for elements what does letters X, Y and Y in the notation below mean: X YZ How many neutrons are in each of the following hydrogen atoms: How many protons, electrons and neutrons in (and name the last two): 63 Cu Check your learning Practice: What are the names of the elements below and how many protons, electrons and neutrons do they have? 11 B 56 Fe answers: Boron proton & electrons: 5, neutrons 6 Iron protons and electrons: 26 neutrons: 30 5

6 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature When elements are charged video: Video: Textbook: Chapter 7 pg Guided Notes for Video on Charge Particle How does an atom become positively charged? Name: Questions: What is the name given to a positively charged ion? If an atom gains a negative charge how could it have gained electrons? What is the name given to a negatively charged ion? How many protons, electrons and neutrons are in the following elements? 42Ca +2 16O -2 Check your learning practice: Name and determine the number of protons and electrons in each of the following also classify as an anion or cation: a. S -2 b. Fe +2 answers to above: a) Sulfur, protons: 16, electrons 18, anion b. Iron, protons: 26, electrons: 24, cation 6

7 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature Ionic Nomenclature: Optional Supplemental Video: Textbook: Chapter 7 pages Guided Notes Ionic Nomenclature What is an ionic compound? Name: Questions: What is a binary compound? What is a ternary compound? What are the rules for naming a binary ionic compound? What are the names of: K 2S MgF 2 Al 2O 3 You Try: BeS Li 3 N What are the rules for naming a ternary ionic compound? What are the names of: Ca3(PO4)2 NaOH (NH4)2CO3 You Try: BaSO 3 Li 2SO 4 7

8 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature Why do elements form compounds? Name: ON YOUR PERIODIC TABLE WRITE THE CHARGE OF THE IONS FORMED BY ELEMENTS IN GROUP I, II, III, AND V, VI, VII What are the five steps for writing formulas show the steps with: Sodium Flouride write the formulas for the following compounds: calcium chloride Aluminum Nitrate When do you put a parenthesis around a polyatomic ion? 8

9 Unit 2: Chapter 4 Atomic Theory and Structure and Ionic Nomenclature More examples: Sodium Oxide Aluminum Sulfide Name: Barium Sulfate You Try: Potassium Bromide Calcium Sulfide Aluminum Phosphide Magnesium Chlorite Lithium Nitrate 9

10 Ionic Nomenclature Practice Anions Cl -1 Br -1 S -2 P -3 OH -1-1 NO 3-2 SO 4-2 SO 3 C 2H 3O PO 4 Cations Na +1 NaCl Sodium chloride K +1 Ca +2 Mg +2 Mg(OH) 2 Magnesium Hydroxide Al +3 NH

11 Unit 2: Chapter 4 Practice Problems History of the Atom in Class Practice: 1. An atom is defined as the smallest part of an element that a. contains at least one proton, neutron, and electron. b. retains the chemical identity of that element. c. can carry an electric charge. d. is affected in a cathode ray tube. 2. The fact that carbon dioxide always contains 73 percent oxygen by mass is an illustration of a. the ideas of Democritus. c. the law of constant composition. b. the law of conservation of matter. d. Dalton's atomic theory of matter. 3. A spherical atom of uniformly distributed positive charge with embedded negatively charged electrons is a description of: a. Dalton s atomic theory b. Rutherford s nuclear model of the atom c. the subatomic particles which make up atoms d. Thomson s plum pudding model 4. A cathode ray consists of a. protons. c. neutrons. b. electrons. d. gamma rays. 5. The electron was discovered by a. Thomson. c. Millikan. b. Faraday. d. Rutherford. 6. The scientist who measured the mass of the electron was a. Thomson. c. Millikan. b. Faraday. d. Rutherford. 7. The experiment that revealed the charge of the electron involved the use of a. gold foil. c. oil droplets. b. photographic film. d. cathode ray tubes. 8. The experiment that revealed that the mass of an atom was concentrated at its center involved the use of a. gold foil. c. oil droplets. b. photographic film. d. cathode ray tubes. 9. Rutherford called the core of the atom the a. neutron. c. nucleus. b. proton. d. electron. 10. Which of the following is not one of the three fundamental particles that makeup atoms? a. electron c. neutron b. proton d. alpha particle 11. Which of the following particles is normally found outside the nucleus of the atom? a. electron c. neutron b. proton d. alpha particle 11

12 Unit 2: Chapter 4 Practice Problems Atomic Structure in Class Practice 12. Write the symbol of the element and how many electrons and protons are contained in an atom of each of the following neutral elements? Name Symbol # protons # electrons Name Symbol # protons # electrons a. arsenic d. gold b. fluorine e. molybdenum c. polonium f. barium 13. Identify the atom containing the following number of proton. List the name and symbol. a. 74 d. 20 b. 49 e. 70 c. 93 f Identify the atom containing the following number of electrons (in a neutral atom). List the name and symbol. a. 34 d. 5 b. 31 e. 82 c. 94 f One of the four naturally occurring isotopes of chromium has a mass number of 53. Determine the number of protons, electrons, and neutrons in an atom of this isotope and write its symbol. The other three naturally occurring isotopes of chromium have mass numbers of 50, 52, and 54. Describe how atoms of these isotopes differ from the isotope mentioned for chromium having a mass number of Determine the number of protons, neutrons, and electrons in the following: Rn 93 Np 17. Determine the number of protons and electrons in each of the following also classify as an anion or cation: a. N -3 c. Cr +7 b. Ba List the name and symbol of the element that has an approximate average atomic mass of: a. 40 c. 181 b

13 Unit 2: Chapter 4 Practice Problems 19. Place the appropriate name and number in the space provided name protons electrons neutrons atomic number mass number Xe 35Br N Cl Sr Ionic Nomenclature 20. Write the name for: Write the formula for: 1. CaCO3 17. sodium nitrite 2. Ca(ClO2)2 18. Aluminum hydroxide 3. LiC1 19.ammonium hydroxide 4. Ca3(PO4)2 20. Aluminum sulfate 5. Ba(OH)2 21. barium chlorite 6. Na2S 22. barium nitride 7. AlCl3 23. potassium sulfate 8. NaOH 24. calcium oxide 9. (NH4)2SO4 25. barium sulfite 10. NH4NO2 26. potassium carbonate 11. Ca(HCO3)2 27. lithium sulfide 12. Ba(ClO3)2 28. ammonium nitrate 13. Mg(NO3)2 29. calcium phosphate 14. KF 30. aluminum acetate 15. K2SO3 31. magnesium sulfide 16. KClO2 32. aluminum bromide 13

14 Unit 2: Chapter 4 Answers to Practice Problems 1 b 2 c 3 d 4 b 5 a 6 c 7 c 8 a 9 c 10 d 11 a. 12. a) As, 33 b) F, 9 c) Po, 84 d) Au, 79 e) Mo, 42 f) Ba, a) Tungsten, W b) Indium, In c) Neptunium, Np d) Calcium, Ca e) ytterbium, Yb f) argon, Ar 14. a) Selenium, Se b) Gallium, Ga c) plutonium, Pu d) Boron, B e) Lead, Pb f) iron, Fe Cr p & e: 24, n: 29, isotopes differ by the number of neutrons so Cr-50 has 26 neutrons Cr-52 has 28 and Cr-54 has 30 neutrons 16. Rn p & e: 86, n: 132 Np p&e: 93, n: a) anion, p: 7, e: 10 b) cation p: 56, e: 54 c) cation p: 24, e: a) calcium, Ca b) titanium, Ti c) tantalum, Ta Xe Br N Cl Sr Name: zirconium xenon bromine mercury radium nitrogen chlorine strontium p e n atomic number mass number Write the name for: Write the formula for: 1. CaCO 3 calcium carbonate 17. sodium nitrite NaNO 2 2. Ca(ClO 2) 2 calcium chlorite 18. Aluminum hydroxide Al(OH) 3 3. LiC1 lithium chloride 19.ammonium hydroxide NH 4OH 4. Ca 3(PO 4) 2 calcium phosphate 20. Aluminum sulfate Al 2(SO 4) 3 5. Ba(OH) 2 barium hydroxide 21. barium chlorite Ba(ClO 2) 2 6. Na 2S sodium sulfide 22. barium nitride Ba 3N 2 7. AlCl 3 aluminum chloride 23. potassium sulfate K 2SO 4 8. NaOH sodium hydroxide 24. calcium oxide CaO 9. (NH 4) 2SO 4 ammonium sulfate 25. barium sulfite BaSO NH 4NO 2 ammonium nitrite 26. potassium carbonate K 2CO Ca(HCO 3) 2 calcium bicarbonate 27. lithium sulfide Li 2S 12. Ba(ClO 3) 2 barium chlorate 28. ammonium nitrate NH 4NO Mg(NO 3) 2 magnesium nitate 29. calcium phosphate Ca 3(PO 4) KF potassium fluoride 30. aluminum acetate Al(C 2H 3O 2) K 2SO 3 potassium sulfite 31. magnesium sulfide MgS 16. KClO 2 potassium chlorite 32. aluminum bromide AlBr 3 14