Question

19. Consider the molecule SiCl4. The electronegativity values for Si and Cl are 1.8 and 3.0, respectively. Based on these values and on consideration of molecular geometry: a. Determine if the Si-Cl bond is polar or nonpolar b. Determine if the SiCl4 molecule is polar or nonpolar. Explain why you chose your answers. 20. Draw the Lewis structure for Chlorine 21. Name an element that is likely to form an ion with a +1 charge and 22. For the structure shown, the most likely elements are X= Y = 23. How does the electronegativity of K compare to that of Se? Draw Lewis structures for the following: For all except 24, there is only one possible structure. For 24, there are several alternative structures, any of which are acceptable. 24. C3H&Ch, the 3 carbons are connected in a row 25. C2H4

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Answer 1

- g. (a) Electro i & a are 1.8 and 3.0 Hence, the electonegativity difference between Si & Clis : 3 - 1-8 - 1-2 It means. Si-ci band is polar. sicly atsit C Sicly is planar molecule, where 4 dipule p moment of Si-ci bond cancel each other, Hence, Si C14 molecule . become non-polar, 20, - C . - Lewis structure of chlorine. Element 21. Top with 71 Charge 3. Na (Sodium) las Nat?] 22. X = Oxyzen (0)Y : Carbon (C) : örc=ö 23 • Electronegativity of K is much lower than electronegativity of Se. | Electronegativity of ķ: 0.8, Electro negativity of Se : 2.4) 24. C3H4C12-ci CC-H and much more structure, 25. C₂H4 C C