Topics for Test on Chapter 6: The Periodic Table & Periodic Law
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1 Topics for Test on Chapter 6: The Periodic Table & Periodic Law Regions of the Periodic Table (know where they are and the properties) - Metals - Nonmetals - Metalloids - Hydrogen - Alkali Metals - Alkaline Earth Metals - Transition Metals - Lanthanide Series - Actinide Series - Halogens - Noble Gases Valence Electrons - What are they? - How many valence electrons does an element have? 1
2 Periodic Trends Atomic Radius - How is it measured? - What are the trends? - Why do the trends occur? Ionic Radius - How do positive and negative ions form? - What are they called? - What is the change in size with a positive and negative ion? Ionization Energy - What is it? - What are the trends? - Why do the trends occur? - What is second and third ionization energy and when does a big jump in ionization energy occur? Electronegativity - What is it? - What are the trends? - Why do the trends occur 2
3 Throwback Thursdays!!! 1. What is the difference between the independent and dependent variable? 2. How many significant figures does a number have? (example:.00670) 3. Calculations with correct significant figures (example: ) 4. Converting one metric unit to another metric unit (keeping in mind significant figures - example: ml to L) 5. Is a change a chemical or physical change? (example: snow melting, iron rusting,...) 6. Percent by mass problems (example: what is the percent of oxygen in a compound that contains 12.6 g of oxygen and 46.3 g of nitrogen, and 5.67 g of hydrogen. 7. Number of neutrons, protons, and electrons mass number and atomic number. (example: How many p +, n, and e - does the atom 40 19K have?) 8. Writing nuclear equations (example: what is the equation for the alpha decay of curium-249) 9. Writing electron configurations(example: Mg 1s 2, 2s 2, 2p 6, 3s 2 ) 10. Writing orbital diagrams (example: ) 1s 2s 2p 3s 3
4 Write the letter that corresponds to the correct description of the element 1. This element is a noble gas 2. This element is radioactive 3. This element is somewhat reactive in oxygen and water 4. This element is a transition metal 5. This element is a member of the alkali metals 6. This element is an inner transition metal, but is not radioactive 7. This element is more reactive than the element in #3 8. This element is reactive non metal 9. This element is a semi conductor 10. This element is the most abundant element in the universe 11. This element has properties similar to nitrogen 12. This element is a non reactive non metal 13. This element is malleable and ductile 14. This element is a member of the halogen family 15. This element has an valence electron configuration of s 2 p This element has 3 valence electrons 17. This element has 8 valence electrons 18. This element only has to gain one electron to have a noble gas configuration 19. This element has to lose 2 electrons to have noble gas configuration 4
5 20. Circle the element with the following property a. The element with the greater radius K K + b. The element with the greater atomic radius Na Cl c. The element with the greater ionization energy Mn Tc d. The element with the greater radius O O 2- e. The element with the greater electronegativity Mg Si f. The element with the greater ionization energy K Zn g. The element with the greater atomic radius Cr Se h. The element with the greater ionization energy Br F i. The element with the greater radius Al 3+ Al j. The element with the greater electronegativity Br I k. The element with the greater atomic radius S Se 21. Pick two of the problems from # 20 and explain fully WHY the trend takes place. 5
6 22. Circle the word that completes the following statements correctly. a. As the atomic radius decreases, there is (more/less) proton/electron attraction, thus ionization energy (increases/decreases) b. Magnesium has a (larger/smaller) atomic radius than strontium because electrons are added to (the same/higher) energy level(s). c. Boron has a very (high/low) fourth ionization energy because the electron being removed is a (valence/core) electron. d. F - has a (smaller/larger) radius than F because in F - there are (more/less) electrons being attracted to the same number of protons in the nucleus. Additional problems from our book Page 198: 32, 38, 40, 41, 43, 45, 49, 56, 58, 59, 60, 61, 62, 63, 66, 68, 69 6
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