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NAME:_______________________ 4.3 What is ionization energy? DATE:____________ AHS Instructor Ms. Kasia Room 109/110 UNIT 4 THE PERIODIC TABLE 4.3 What is ionization energy? AIM: DO NOW: Take our your Chemistry Reference Tables. Turn to the Periodic Table of Elements (Page 8). 1. What is the trend for atomic radius as you move from left to right on the period? 2. What causes this trend? ACTIVITY Directions: Using Table S, order the following from least first ionization energy to greatest first ionization energy. Se S Te O P ________________________________________________________________________________________ Least Greatest What do you notice? Al Si Cl Na Ar Mg P ________________________________________________________________________________________ Least Greatest What do you notice? IONIZATION ENERGY TERM IONIZATION ENERGY DEFINITION WHY? GOING ACROSS PERIOD GOING DOWN THE GROUP Directions: Indicate the trend as you move UP A GROUP and as you move ACROSS A PERIOD. NAME:_____________________________ 4.3 What is ionization energy? DATE:________ AHS Instructor Ms. Kasia Room 109 UNIT 4 THE PERIODIC TABLE 4.3 What is ionization energy? Directions: Answer each question below to the best of your ability. Ask if you have questions. 1. Order from LEAST IONIZATION ENERGY to GREATEST IONIZATION ENERGY. a. Sr Sn I Rb Sn Xe Te ________________________________________________________________________________________ b. Ra Ba Sr Ca Mg Be ________________________________________________________________________________________ c. F Cl Br I At ________________________________________________________________________________________ d. Mn Sc Ti Cr Co ________________________________________________________________________________________ 2. Which general trend is found in Period 2 on the Periodic Table as the elements are considered in order of increasing atomic number? (1) Decreasing atomic mass (2) Decreasing electronegativity (3) Increasing atomic radius (4) Increasing first ionization energy Explain how you found your answer 3. As the elements are considered from top to bottom in Group 15 of the Periodic Table, the ionization energy (1) Decreases (2) Increases (3) Remains the same Explain how you found your answer 4. Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? (1) The atomic radius decreases, and the first ionization energy generally increases. (2) The atomic radius decreases, and the first ionization energy generally decreases. (3) The atomic radius increases, and the first ionization energy generally increases. (4) The atomic radius increases, and the first ionization energy generally decreases. Explain how you found your answer 5. As one proceeds from left to right across Period 3 of the Periodic Table, there is a decrease in (1) Ionization energy (2) Metallic characteristics (3) Electronegativity (4) Valance electrons 6. If the elements are considered from top to bottom in Group 17, the number of electrons in the outermost shell will (1) Decrease (2) Increase (3) Remain the same Explain how you found your answer Explain how you found your answer 7. As we move across a period on the periodic table, the ionization energy_________________________ 8. As we move down a group on the periodic table, the ionization energy_________________________ 9. Circle the element in each pair with the higher ionization energy. USE YOUR KNOWLEDGE OF THE TRENDS! 1 Li Na 2 Sc Ti 3 Pd Ag 4 Al Si 5 Cl Br 10. Circle the atom in each pair that has the largest atomic radius 1 Al B 2 S O 3 Br Cl 4 Na Al 5 O F 11. Why does fluorine (F) have a higher ionization energy than iodine (I) _____________________________________________________________________________________