OCR Unit 3 Periodic Trends Review PDF

## Unit 3 (periodic trends) Review 1. What did Dmitri Mendeleev base his periodic table on? - Increasing atomic mass 2. What did Henry Mosely base his periodic table on? - Increasing atomic # 3. What is periodic law? - When elements are arranged by increasing atomic #, there is a period...

## Unit 3 (periodic trends) Review 1. What did Dmitri Mendeleev base his periodic table on? - Increasing atomic mass 2. What did Henry Mosely base his periodic table on? - Increasing atomic # 3. What is periodic law? - When elements are arranged by increasing atomic #, there is a periodic pattern in their chemical and physical properties 4. What is a group on the periodic table? - A column/family 5. What is a period on the periodic table? - A row 6. Do elements in the same group or period have similar properties? - Same group 7. What are the names of the following groups on the periodic table? If I give you an element, make sure you know what group it belongs to. - a. Group 1 : Alkali metals - b. Group 2 : Alkaline earth metals - c. Group 3-12 : transition metals - d. Group 17 : halogens - e. Group 18 : noble gases 8. Which of the groups listed in #7 is the most reactive and which group is the least reactive? - Most - Alkali metals - Least - Noble Gases 9. Where are the metals, metalloids, and nonmetals on the periodic table? - Metals - left - Metalloids - staircase - Nonmetals - right 10. What sub-level block are representative elements? - s+p 11. What are the four shapes for the sub-levels? - Sphere (s) - Dumbbell (p) - Clover (d) - Double Clover (f) 12. What does malleable, ductile, and brittle mean? - Malleable - can be hammered into shapes - Ductile - can be shaped into wires. - Brittle - hard, but can break or shatter easily 13. What is the relationship between charge and attractive force in Coulomb's law? - As charge increases, attractive force increases 14. What is the relationship between distance and attractive force in Coulomb's law? - As distance increases, attractive force decreases. 15. Make sure you know how to determine the electron configuration of an element. You will be able to use the sublevel chart. - a. Nitrogen (N) : 1s² 2s² 2p³ - b. Sodium (Na) : 1s² 2s² 2p⁶ 3s¹ - c. Cobalt (Co) : 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁷ - d. Sulfur (S) : 1s² 2s² 2p⁶ 3s² 3p⁴ 16. What is the atomic radius? - 1/2 the distance between two nuclei of the same element. 17. What is electronegativity? - Electronegativity is the tendency for an element to attract electrons from a different element when chemically combined. 18. What is ionization energy? - Ionization energy is the amount of energy required to remove an electron from a gaseous atom. 19. After you remove the 1st electron in an atom, does it require more or less energy to remove the 2nd electron? - It requires more energy. 20. What is a positive ion called? - Cation 21. What is a negative ion called? - Anion 22. Draw arrows on the periodic table below to show increasing atomic radius, 1st ionization energy, and electronegativity. - Image description: Periodic table with arrows pointing in the following directions: - Atomic Radius: Points to the left and down - Ionization Energy: Points to the right and up - Electronegativity: Points to the right and up 23. Make sure you know how to determine which element has a greater atomic radius, electronegativity, and ionization energy. - Circle that atom with the larger atomic size: - a) Mg or **Ca** c) N or **Si** - b) Ga or **Br** d) Rb or **P** - Circle the atom with the larger 1st ionization energy: - a) O or **S** c) K or **F** - b) Al or **Cl** d) Al or **Fe** - Circle the atom with the larger electronegativity: - a) B or **In** c) P or **Ga** - b) K or **Li** d) N or **Al** - Circle the atom or ion that is larger: - a) F^-1 or **F** c) Mg⁺² or **Mg** - b) Cr⁺² or **Cr⁺³** d) P¹ or **P^-3**