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Name: __________________________________ Section 14.2 Periodic Trends Guided Reading Assignment Directions: Read the assigned pages from our text book to fill in the blanks. TRENDS IN ATOMIC SIZE (Page 400) Group Trends 1. Atomic size generally ____________ as you move down a group of the periodic table. 2. As you descend, electrons are added to successively higher ________________ ____________________ ________________ and the nuclear charge increases. 3. The outermost orbital is ________________ as you move downward. 4. 5. 6. 7. 8. 9. Periodic Trends Atomic size generally _______________ as you move from left to right across a period. As you go across a period, the ______________ _____________ ___________ remains the same. Each element has one more _____________ and one more ______________ than the preceding element. The electrons are added to the ____________ principal energy level. The effect of the increasing nuclear charge on the outermost electrons is to ____________ ___________ ____________ to the nucleus. Atomic size therefore ___________________. TRENDS IN IONIZATION ENERGY (Page 401-403) 10. When an atom gains or loses an _______________, it becomes an ion. 11. The energy required to overcome the attraction of the nuclear charge and remove an electron from a gaseous atom is called the _________________ _____________. 12. Removing one electron results in the formation of a positive ion with a ____________ charge. 13. The energy required to remove this first outmost electron is called the _____________ _______________ ____________. Group Trends 14. The first ionization energy generally ________________ as you move down a group of the periodic table. 15. This is because the size of the atoms ____________ as you descend, so the outermost electron is farther from the nucleus. 16. The outermost electron should be more _____________ ____________, and the element should have a ______________ ionization energy. Periodic Trends 17. For the representative elements, the first ionization energy generally ____________ as you move from left to right across a period. 18. The nuclear charge _______________ and the shielding effect is constant as you move across. 19. A greater attraction of the nucleus for the electron leads to the ____________ in the ionization energy. TRENDS IN IONIC SIZE (Page 404) Group Trends 20. Positive ions are always ______________ than the neutral atoms from which they form. 21. This is because the loss of __________________ electrons results in increased attraction by the nucleus for the fewer remaining electrons. Periodic Trends 22. Going from left to right across a row, there is a gradual _______________ in the size of positive ions. 23. Then beginning with Group 5A, the negative ions, which are much _________________, gradually decrease in size as you continue to move right. 24. The ionic radii of both anions and cations _______________ as you go down each group. TRENDS IN ELECTRONEGATIVITY(Page 405) 25. The ___________________ of an element is the tendency for the atoms of the element to attract electrons when they are chemically combined with atoms of another element. 26. AS you can see, (from examining Table 14.2), electronegativity generally ____________________ as you move down a group. 27. As you go across a period from left to right, the electronegativity of the representative elements __________________. 28. The metallic elements at the far left of the periodic table have ______________ electronegativities. 29. By contrast, the nonmetallic elements at the far right (excluding the noble gases) have _____________ electronegativities.. 30. The electronegativity of cesium, the least electronegative element, is ___________. 31. The electronegativity of fluorine, the most electronegative element, is _____________. 32. Because fluorine has such a strong tendency to attract electrons, when it is chemically bonded to any other element it either ___________the shared electrons or forms a _____________ ion. 33. In contrast, cesium has the ______________ tendency to attract electrons. 34. It loses the electron ____________________ and forms a positive ion.