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Name ______________________________ Chemistry 4-12 Date _________________ Period ____ Review Guide for Periodic Trends 1) A period is a ________________________ _______________________ on the Periodic Table. (vertical, horizontal) (row, column) 2) A group is a ________________________ _______________________ on the Periodic Table. (vertical, horizontal) (row, column) ATOMIC RADIUS 3) Atomic radius is the distance between the ___________________________ and the ______________________________________________________________________. 4) Atomic radius generally _____________________ as you move down a group. Valence electrons (increases, decreases) occupy _________________________ principal energy levels as you move down a group. As a result, the (lower, higher) electrons are ___________________________ from the nucleus. Thus, the electrons are (closer, further) ________________________ held by the nucleus and the atomic radius is ___________________. (tightly, loosely) (small, large) 5) Atomic radius generally ____________________ as you move left-to-right across a period. This (Increases, decreases) is because within a period, all electrons are being added to the _____________________ shell. But, at (same, different) the same time, protons are being added to the nucleus, making it ________________ positively charged. (more, less) Thus, the nucleus attracts the electrons more strongly, having the atom’s shell pull _____________ to the (closer, farther) nucleus. The valence electrons are held ___________________ towards the nucleus of the atom. As a (closer, farther) result, the atomic radius ____________________ left-to-right. (increases, decreases) Chemistry 4-12 IONIZATION ENERGY 6) Ionization energy is the amount of energy needed to _________________ an ________________ (remove, add) (proton, electron) from an atom. The smaller the ionization energy, the ______________ it is to remove an electron. (easier, harder) 7) Ionization energy ____________________ as you go left-to-right on the Periodic Table. (increases, decreases) Elements on the left side of the Periodic Table have _______________ ionization energies, because they (lower, higher) have a greater willingness to ______________ electrons in effort to have a full valence shell (8 valence (lose, gain) electrons). Elements on the right side of the Periodic Table have ______________ ionization energies, (lower, higher) because their valence shell is already nearly filled. 8) As you move down a group, ionization energy generally ________________. This is because the (increases, decreases) number of principal energy shells ____________________ down a group and thus there is an (increase, decrease) ____________________ distance between the valence electrons and nucleus, or a greater atomic radius. (increased, decreased) 9) Group 18 (noble gases) possess very __________________ ionization energies because they have full (high, low) valence shells. ALKALI METALS WITH WATER DEMO 10) In the video demo, we watched 3 different alkali metals (Li, Na, and K) react with ____________. (oil, water) The reactions were similar between all 3 metals because they are all found in the same _____________ (group, period) and have the same number of _______________________________. Thus, all three metals have (inner electrons, valence electrons) similar chemical ___________________________. Lithium (Li) reacted the ___________________ (formulas, properties) (most, least) vigorously, while potassium (K) reacted the ___________________ vigorously. (most, least) 11) As you go down Group 1, reactivity __________________. (increases, decreases) Chemistry 4-12 ELECTRONEGATIVITY 12) Electronegativity is the _______________________ of ________________________ by an atom. (attraction, repulsion) (protons, electrons) The larger the electronegativity, the __________________ an atom attracts electrons. (more, less) 13) As you move to the right across a period of elements, electronegativity ____________________. (increases, decreases) 14) Most atoms prefer to fulfill the ______________ rule (having the valence shell comprise of 8 electrons). Elements on the left side of the Periodic Table have less than a half-full valence shell. Thus it is easier (takes less energy) to lose electrons to create a full valence shell, rather than gain electrons. Thus atoms on the left-side of the P.T. have a low attraction for electrons and have _____________ (low, high) electronegativities. 15) Elements on the right side of the Periodic Table have more than a half-full valence shell, and it is easier (takes less energy) to gain electrons to create a complete valence shell of 8 electrons. Thus atoms on the right-side of the P.T. have a high attraction for electrons and have _____________________ (low, high) electronegativities. 16) As you move down a group, electronegativity generally _________________. This is because the (increases, decreases) there is an ____________________ distance between the valence electrons and nucleus, or a greater (increased, decreased) atomic radius. 17) Group 18 (noble gases) possess a complete valence shell and do not usually attract electrons, thus they _______________ have electronegativity values. (do not, always) Chemistry 4-12 Practice Questions 1. Of the following elements, which would have the largest radius? 1) 2) 3) 4) Lithium (Li) Neon (Ne) Boron (B) Nitrogen (N) (2) Period 2 (4) Group 1 11. Which elements have the most similar chemical properties? (1) K and Na (3) K and Ca (2) K and Cl (4) K and S 2. Nitrogen has a larger atomic radius than Oxygen. 1) True 2) False 3. An atom with an atomic radius smaller than that of Sulfur (S) is __________. 1) Oxygen (O) 2) Selenium (Se) 3) Calcium (Ca) 4) None of the above 4. Which two elements have the most similar chemical properties? (1) aluminum and barium (3) chlorine and sulfur (2) nickel and phosphorus (4) sodium and potassium 5. As the atoms of the metals of Group 1 in the ground state are considered in order, from top to bottom, the number of occupied principal energy levels (1) decreases (2) increases (3) remains the same 6. Which element is in Group 2 and Period 7 of the Periodic Table? (1) magnesium (3) radium (2) manganese (4) radon 7. Given the representation of chlorine above, which circle would represent an atom of fluorine? (1) b (2) c (3) d (4) none of these 8. Which electron configurations represent the first two elements in Group 17 of the Periodic Table? (1) 2-1 and 2-2 (3) 2-7 and 2-8-7 (2) 2-2 and 2-3 (4) 2-8 and 2-8-7 9. Which is the electron configuration of an atom of Period 3 element? (1) 2-1 (3) 2-5 (2) 2-3 (4) 2-8-1 10. In which category of elements in the Periodic Table do all of the atoms have valence electrons in the second principal energy level (second shell)? (1) Group 2 (3) the alkaline earth family 12. Using the diagrams above, which of these elements would have the lowest ionization energy? (1) a (2) b (3) c (4) d 13. An atom of an element has 28 innermost electrons and 7 outermost electrons. In which period of the Periodic Table is this element located? (1) 5 (3) 3 (2) 2 (4) 4 14. Atoms of elements in a group of the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms’ (1) number of principal energy levels (2) number of valence electrons (3) atomic structure (4) atomic masses 15. Which group below contains elements with the greatest variation in chemical properties? (1) Li, Be, B (3) B, Al, Ga (2) Li, Na, K (4) Be, Mg, Ca 16. The chemical properties of the elements are periodic functions of their atomic (1) masses (3) numbers (2) weight (4) radii 17. All of the atoms of the elements in Period 2 have the same number of (1) protons (3) valence electrons (2) neutrons (4) occupied principal energy levels Chemistry 4-12 18. Which is the electron configuration of an atom of a Period 3 element? (1) 2-1 (2) 2-3 (3) 2-5 (4) 2-8-5 19. In the ground state, atoms of the elements in Group 15 of the Periodic Table all have the same number of (1) filled principal energy levels (2) occupied principal energy levels (3) neutrons in the nucleus (4) electrons in the valence shell 20. Which of the Group 15 elements can lose an electron most readily? (1) N (2) P (3) As (4) Bi 21. Which element is a member of the halogen family (Group 17)? (1) K (2) B (3) I (4) S 22. In which group does each element have a total of four electrons in the outermost principal energy level? (1) 1 (2) 18 (3) 16 (4) 14 23. The electron dot structure for elements in Group 14 is (1) X (2) X (3) X (4) X 24. Elements in Group 18 (1) have 3 valence electrons in the last shell (2) have 18 valence electrons in the first energy level (3) have a complete outer shell (4) have an incomplete outer shell 25. An atom of which of the following elements has the smallest atomic radius? (1) Li (2) Be (3) C (4) F 26. Which of the following atoms has the largest atomic radius? (1) Na (2) K (3) Mg (4) Ca 27. Which element has the highest ionization energy? (1) sodium (3) calcium (2) aluminum (4) phosphorus 28. Which element in Group 1 has the greatest tendency to lose an electron? (1) cesium (3) potassium (2) rubidium (4) sodium 29. Which of the Group 15 elements can lose an electron most readily? (1) N (2) P (3) Sb (4) Bi 30. Which first ionization energy is the most probable for a very reactive metal? (1) 380 kjoules/mol (3) 1681 kjoules/mol (2) 1086 kjoules/mol (4) 2372 kjoules/mol 31. A nonmetal could have an electronegativity of (1) 1.0 (2) 2.0 (3) 1.6 (4) 2.6 32. Of all the elements, the one with the highest electronegativity is found in Period (1) 1 (2) 2 (3) 3 (4) 4 33. A metal can have an electronegativity of (1) 4.0 (2) 1.0 (3) 3.5 (4). 3.2 34. Which electronegativity is possible for a Group 1 metal? (1) 1.0 (2) 2.0 (3) 3.0 (4) 4.0 35. According to Reference Table S, which of the following elements has the smallest atomic radius? (1) nickel (3) calcium (2) cobalt (4) potassium 36. Which electron configuration represents the atom with the largest atomic radius? (1) 2-1 (2) 1 (3) 2-2 (4) 2-3 37. Which of the following elements has the largest atomic radius? (1) beryllium (3) calcium (2) magnesium (4) strontium 38. Which element in Period 3 has the largest atomic radius? (1) Cl (2) Al (3) Na (4) P 39. As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the atomic radius of each successive element compare? (1) the relative electronegativity decreases, and the atomic radius decreases (2) the relative electronegativity decreases, and the atomic radius increases (3) the relative electronegativity increases, and the atomic radius decreases (4) the relative electronegativity increases, and the atomic radius increases *40. Which element’s ionic radius is smaller than its atomic radius? (1) neon (3) sodium (2) nitrogen (4) sulfur *41. An ion of which element is smaller than its atom? (1) F (2) O (3) Cl (4) Na *42. An ion of which element is larger than its atom? (1) Al (2) Br (3) Ca (4) Sr *43. Which atom has a radius larger than the radius of its ion? (1) Cl (2) Ca (3) S (4) Se 4-12 Review Guide Answer Key 1. 1 2. 1 3. 1 4. 4 5. 2 6. 3 7. 1 8. 3 9. 4 10. 2 11. 1 12. 4 13. 4 14. 2 15. 1 16. 3 17. 4 18. 4 19. 4 20. 4 21. 3 22. 4 23. 4 24. 3 25. 4 26. 2 27. 4 28. 1 29. 4 30. 1 31. 4 32. 1 33. 1 34. 1 35. 1 36. 1 37. 4 38. 3 39. 3 40. 3 41. 4 42. 2 43. 2