อะตอมและตารางธาต เคม ม.4 1 ใบงานว ชาเคม 1 (Chemistry Worksheets) เร อง อะตอมและตารางธาต () ของ เลขท ห อง สอนโดย คร อ งคาร เทพร ตนน นท สาน กงานเขตพ นท การศ กษาม ธยมศ กษา เขต 11 โรงเร ยนสวนศร ว ทยา จ งหว ดช มพร Name Class No.
อะตอมและตารางธาต เคม ม.4 2 Worksheet 1 Atomic Structure Problem 1. Draw Doltan Atomic Model 2. Draw Thomson Atomic Model 3. Draw Rutherford Atomic Model 4. Draw Bohr Atomic Model 5. Complete the chart for the three sub-atomic particles. Particle name Mass Charge Location in atom Proton Neutron Electron 6. The nitrogen atom has 7 protons and 7 neutrons. Calculate: the atomic number the mass number 7. The phosphorus atom has 15 protons and 16 neutrons. Calculate: the atomic number the mass number 8. If a sulfur atom is neutral in charge and contains 16 protons in the nucleus, how many electrons are present outside the nucleus? 9. Write the nuclear symbol for lithium, with 3 protons and 4 neutrons.
อะตอมและตารางธาต เคม ม.4 3 10. Fill in the blanks for the following nuclear symbols: Element Atomic Number Mass Number # of Protons # of Neutrons # of Electrons 11 5 B 30 14 Si 11. Consider the following table on composition of some atoms. 23 12 Mg 2+ 40 20Ca 3+ 70 31Ga 2+ 35 17Cl 3-32 16S 2-121 51Sb 3- Atom # Protons # Neutrons # Electrons Atomic No. Mass No. Symbol I 26 29 26 II 25 29 24 III 18 20 18 IV 27 33 28 V 34 45 37 12. An isotope of silver has 47 protons, 46 electrons and 60 neutrons. What is the atomic number? What is the mass number? Write the complete isotopic symbol for the element. 13. In a nuclear reactor, an isotope of uranium called U-235 is used. It has 92 protons and a mass number of 235. What is the atomic number? How many electrons? What is the mass number? Write the isotopic symbol 14. Which of the following pairs of elements has the most neutrons? a. 19 19 9 F, 10Ne b. 44 44 20Ca, 22Ti 15. What is the number of protons in an atom equal to? 16. How can you determine the mass number of an atom? 17. In an atom, what two particles are found in equal quantities? 18. How is the number of neutrons determined?
อะตอมและตารางธาต เคม ม.4 4 19. Can an atom s atomic number change? Why or why not? 20. Carbon (C) Carbon (C) atomic number = 6 atomic number = 6 mass number = 12 mass number = 14 protons electrons neutrons protons electrons neutrons What is the difference between the two carbon atoms? What are the two sets of atoms called? 21. For each of the following,check the blank for isotope, isotone, isobar or isoelectronic Nuclear symbols isotope isotone isobar isoelectronic 30 14 Si & 30 15P 19 9 F & 20 10Ne 16 8 O & 18 8O 20 10 Ne & 24 12Mg 2+ 3 2 He & 4 2He 79 34 Se 2- & 80 35Br - 37 17 Cl & 37 18Ar 24 12 Mg 2+ & 19 9F - Isotope is same Isobar is same Isotone is same Isoelectronic is same
อะตอมและตารางธาต เคม ม.4 5 WorkSheet 2 Atomic Structure Problem Fill in the blanks with Proton, Neutron and Electron 1. Located outside the nucleus. 2. Discovered by Chadwick. 3., Called nucleons. 4. Carries a positive charge. 5. Discovered first. 6. Called the atomic number. 7. Has a diameter size of 10-18 km. 8. Located in the energy levels. 9., Have a mass of 1 amu 10. + is the symbol for its charge. 11. Responsible for compound formation. 12. Discovered by J.J. Thomson. 13. - is the symbol for its charge. 14. Carries a negative charge. 15. Determines isotopes. 16., Located in the nucleus 17., Carries the charge to give the atom zero charge. 18., Makes up the major portion of atomic mass. 19. Responsible for chemical reaction. 20. Carries a neutral charge. 21. Moves from place to place. 22. Determines the kind of element. 23. 0 is the symbol for its charge. 24. Equals the number of proton in a neutral atom. 25. Has a mass of 1/1836 amu. 26. Responsible for the charge of the nucleus. 27., Diameters are 10-14 km. 28. Responsible for the charge of energy levels.
อะตอมและตารางธาต เคม ม.4 6 Worksheet 3 Wave and Bohr Atomic Model One full wave (cycle) Wave train two or more waves Amplitude measures the energy of a transverse wave a) measured from the equilibrium position to the top of a crest or the bottom of a trough (see vertical arrow) Wavelength length of a single wave cycle (horizontal arrow double sided arrow) Frequency- number of waves that pass a point in a given amount of time Speed = wavelength x frequency The time from the beginning to the end of the wave train in each situation is 2 second. Wave 1 a) How many waves are there in this wave train? b) Wavelength cm c) Amplitude cm d) frequency Hz e) speed cm/s Wave 2 a) How many waves are there in this wave train? b) Wavelength cm c) Amplitude cm d) frequency Hz e.) speed cm/s
อะตอมและตารางธาต เคม ม.4 7 Wave 3 a) How many waves are there in this wave train? b) Wavelength cm c) Amplitude cm d) frequency Hz e.) speed cm/s Bohr Model Diagrams Use the information provided for each element to draw Bohr Model diagrams. Rather than drawing individual protons and neutrons, you may simply label how many of each there are in the nucleus (e.g. He: 2p, 2n). Then, draw the individual electrons on the appropriate energy levels (keep in mind the maximum number of electrons allowed on each level). 1. Beryllium atomic #: 4, # of n: 5 2. Sodium atomic #: 11, # of n: 12 3. Sulfur atomic #: 16, # of n: 16 4. Calcium atomic #: 20, # of n: 20
อะตอมและตารางธาต เคม ม.4 8 WAVELENGTH, FREQUENCY, & ENERGY PROBLEMS Wavelength Ranges for Visible Light: Red 700-650 nm Orange 649-580 nm Yellow 579-575 nm Green 574-490 nm Blue 489-455 nm Indigo 454-425 nm Violet 424-400 nm 1. Which has the longer λ, blue or indigo light? 2. Which has the greater ν, red or yellow light? 3. Which has the greater energy, a photon of yellow light or a photon of green light? 4. Which has the longer wavelength, light with a frequency of 7.32 x 10 14 Hz or a frequency of 6.0 x 10 14 Hz? 5. Which has higher energy, light with a λ of 674 nm or a λ of 480 nm? 6. Which has a higher frequency, orange light or indigo light? 7. Find the color of light whose frequency is 5.21 x 10 14 Hz. 8. What is the frequency of light if its wavelength is 5.4 x 10-5 cm? 9. Find the wavelength in nanometers of light whose frequency is 7 x 10 14 Hz. 10. Is the light in # 10 visible? 12. How many Joules of energy are there in one photon of yellow light whose wavelength is 630 nm? 13. Find the color of light whose photon has 4.75 x 10-19 J of energy.
อะตอมและตารางธาต เคม ม.4 9 Worksheet 4 Electron Configuration 1. Write a ground state electron configuration (using spdf configuration). N : Na : P : K : Fe : Mn : Sr : 2. Write a ground state electron configuration ((using spdf configuration). O 2- : Fe 2+ : B 3+ : K + : Br - : Cr 6+ : 3. If each orbital can hold a maximum of two electrons, how many electrons can each of the following hold? A) 2s B) 5p C) 4f D) 3d 4. Shape of an s orbital How many s orbitals? 5. Shape of an p orbital How many p orbitals? 6. How many d orbitals? How many d electrons? 7. How many f orbitals? How many f electrons?
อะตอมและตารางธาต เคม ม.4 10 8. Which of the following notations shows the electron configuration of a neutral atom in an excited state? Name the element, and explain how you know it is excited: A) 1s 2 2s 2 2p 1 B) 1s 2 2s 2 2p 3 3s 1 C) 1s 2 2s 2 2p 6 3s 2 3p 1 D) 1s 2 2s 2 2p 6 3s 2 3p 3 4s 1 9. For the following elements list the shorthand electron configuration (noble gas configuration): A) Boron B) Cadmium C) Phosphorus D) Manganese E) Antimony 10. For the following elements list the orbitals diagram of electron configuration: A) Nitrogen B) Calcium C) Iron D) Chlorine E) Rubidium
อะตอมและตารางธาต เคม ม.4 11 Worksheet 5 Periodic Table 1. Periodic means 2. What is a group (or family)? What is a period? 3. How can you determine the number of electrons in an element s outer energy level by the group it s in? 4. What is the octet rule? 5. Why do elements that make positive ions occur on the left side of the periodic table while those that make negative ions occur on the right? 6. Complete the following table. Group Common Name Charge on Ions of this Group 1A 2A 3A 6A 7A 8A 7. Predict the charges on ions of the following atoms. Ra As Te Cs In At Ga S Sr 8. a) In group 1, which element is the most active? b) Metallic activity tends to (increase, decrease) as one goes down Group 1. 9. a) Which element is most active in group 7A? b) Nonmetal activity tends to (increase, decrease) as one goes down Group 7A.
อะตอมและตารางธาต เคม ม.4 12 10. Choose the element in each pair that has the largest radius: a) K or Br b) F or Br c) He or Rn 11. Name all the elements called metalloids. 12. Periodic Table Scavenger Hunt 1. Which element is a metal: Ba (56) or At (85)? 2. Which period is Ca (20) in? 3. What is the number of the group N (7) is in? 4. Which element is an alkali metal: Rb (37) or Al (13)? 5. Which element is a halogen: Na (11) or Cl (17)? 6. Which element is a noble gas: Ne (10) or Br (35) or O (8)? 7. Which element is the most active nonmetal? 8. Which element is the most active metal? 9. Which element has the largest radius: Na (11) or Cs (55)? 10. Which element would be a positive ion in a compound: Sr (38) or Te (52)? 11. How many electron dots should As have? 12. Which element has the highest ionization energy: K (19) or Kr (36)? 13. When Te (52) is an ion in a compound, what charge does it have? 14. How many is an octet of electrons? 15. Which element has 5 valence electrons? B (5) or P (15)? 16. Which element has 18 electrons when it is an ion with a 1 charge? 17. What atomic number would an isotope of U (92) have?
อะตอมและตารางธาต เคม ม.4 13 Worksheet 6 Periodic Table Use a periodic table to help you answer the following questions. 1. Which element in the second period has the greatest atomic radius? 2. Which of the group IIIA elements is the largest? 3. Of the halogens, which has the smallest radius? 4. Which of the alkaline earth metals is the largest? 5. Which of the transition metals has the smallest atomic radius? 6. Which of the noble gases is the smallest? 7. The atomic radius of which element is the largest? 8. Which of the metalloids has the smallest atomic radius? 9. Which of the rare earth elements is the smallest? 10. Are metal ions larger or smaller than the neutral atoms they came from? 11. Are cations larger or smaller than the neutral atoms they came from? 12. Are ions of alkali metals larger or smaller than ions of alkaline earth metals from the same period? 13. Which of the group IIIA elements has the largest ionization energy? 14. Of the halogens, which has the smallest electronegativity? 15. Which of the alkaline earth metals has the smallest electronegativity? 16. Which of the transition metals has the largest ionization energy? 17. Which of the group IVB metals is the least active? 18. Which of the halogens is the most active? 19. Which of the transition metals in the fifth period has the largest EN? 20. Which of the group four metals has the largest ionization energy? 21. Which of the non-metals in the third period is the most active?
อะตอมและตารางธาต เคม ม.4 14 Worksheet 7 Periodic Trends 1. Provide definitions for the following: Ionization Energy: Electron Affinity: Electronegativity : 2. Fill in the blank: IE, EN EA as you move up a group, and as you move from right to left in a period. 3. Answer the following questions by circling the correct element. 1. Which is more electronegative? Na Rb 2. Which has the smallest radius? Mo Y 3. Which has the lower ionization energy? Ga Se 4. Which has the higher electron affinity? Al S 5. Which is less electronegative? Ir Co 6. Which has the larger radius? W Os 7. Which has the higher ionization energy? Be Ba 8. Which has the lower electron affinity? Rb Sr 9. Which has the smallest radius? Au Ag 10. Which is less electronegative? Br F
อะตอมและตารางธาต เคม ม.4 15 4. Draw arrows that indicate the direction that each trend (IE, EA, EN) increases on the periodic table. F Fr 5. Order the following in terms of increasing ionization energy: Mn, Co, V, Sc, Zn 6. Order the following in terms of increasing electron affinity: Al, In, Tl, B, Ga 7. Order the following in terms of decreasing atomic radius: Ba, Cs, Hf, La, Ta 8. Order the following in terms of increasing electronegativity: N, F, C, O, B 9. Order the following in terms of increasing melting point : Al, Si, K, O, Se 10. Order the following in terms of increasing boiling point : Rb, Na, Al, F, Cl 11. Choose T for a true statement, F for a false statement. T F 1. Technetium is more electronegative than zirconium. T F 2. Sulfur has a smaller atomic radius than silicon. T F 3. Potassium has a higher ionization energy than cesium. T F 4. Chlorine is less electronegative than fluorine. T F 5. Aluminum has a higher chemical activity than sodium. T F 6. Tin has a larger electron affinity than iodine. T F 7. Arsenic is more likely to gain an electron than bromine. T F 8. Manganese has a lower electron affinity than nickel. T F 9. Calcium will lose an electron easier than beryllium.
อะตอมและตารางธาต เคม ม.4 16 Worksheet 8 Oxidation Number Find the Oxidation number of underline elements. 1. CO 2. CH 4 3. SO 3 4. Al 2 O 3 5. S 2 Cl 2 6. BaSO 4 7. MgCrO 4 8. Sr(NO 3 ) 2 9. IF 3 10. K 2 MnO 4 11. [Fe(CN) 6 ] 3-12. Cr(OH) 3 13. NiCl 2.6H 2 O 14. K 3 [Fe(CN) 6 ] 15. [Cu(NH 3 ) 4 ]SO 4 16. [Mn(H 2 O) 6 ] 3+ 17. (NH 4 ) 2 [NiCl 4 ] 18. Co(BrO 3 ) 3 19. Pb(ClO 2 ) 4 20. PbCl 2.Pb 3 (PO 4 ) 2
อะตอมและตารางธาต เคม ม.4 17 Worksheet 9 Nuclear Equation Complete the bank. 1. 3 1H ----> + 0-1e 2. 232 92U ----> 228 88Ra + 3. 144 58Ce ----> 144 59Pr + 4. 65 30Zn ----> + 0 +1e 5. 40 19K ----> + 0 +1e 6. 7 4Be* ----> 7 4Be + 7. 1 0n + 235 92U ----> 141 55Cs + +3 1 0n 8. 222 86Rn ----> + 4 2He 9. 129 53I ----> 129 54Xe + 10. 1 1H + 1 1H ----> + 0 +1e 11. 239 94Pu ----> + 4 2He 12. 15 8O ----> 15 7N + Radioactive decay Parent Daughter Equation 180 Hg 176 Pt 223 Th 223 Pa 60 Co* 60 Co 137 I 136 I 53 Co 52 Fe 40 K 40 Ar 90 Nb 90 Zr 209 Bi 210 Bi 31 S 31 P Using your knowledge of nuclear chemistry, write the equations for the following processes: 1) The alpha decay of radon-198 2) The beta decay of uranium-237 3) Positron emission from silicon-26 4) Sodium-22 undergoes electron capture 5) When protactinium-229 goes through two alpha decays, francium-221 is formed.
อะตอมและตารางธาต เคม ม.4 18 Worksheet 10 HALF-LIFE Use Reference Table on side to assist you in answering the following questions. half lifes: As-81 = 33 seconds, Au-198 = 2.69 days, C-14 = 5730 years 1. How long does it take a 100.00g sample of As-81 to decay to 6.25 g? 2. How long does it take a 180g sample of Au-198 to decay to 1/8 its original mass? (Ans. 8.07 days) 3. What percent of a sample of As-81 remains un-decayed after 43.2 seconds? 4. What is the half-life of a radioactive isotope if a 500.0 g sample decays to 62.5 g in 24.3 hours? (Ans. 8.1 hours) 5. How old is a bone if it presently contains 0.3125g of C-14, but it was estimated to have originally contained 80.000g of C-14?
อะตอมและตารางธาต เคม ม.4 19 6. How much of a 100.0 gram sample of gold-198 is left after 8.10 days if its half-life is 2.70 days?(ans. 12.5 gram) 7. A 50.0 grams sample of nitrogen-16 decays to 12.5 grams in 14.4 seconds. What is its half-life? 8. The half-life of potassium-42 is 12.4 hours. How much of a 728 gram sample is left after 62.0 hours? (Ans. 22.75 gram) 9. What is the half-life of technetium-99 if a 500.0 gram sample decays to 62.5 grams in 639,000 years? 10. The half-life of thorium-232 is 1.4 x 10 10 years. If there are 25.0 grams of the sample left after 2.8 x 10 10 years, how many grams were in the original sample? (Ans. 100 gram)
Atom and periodic table Angka Teprattananan