1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table.

Please note that "geometry" refers to the molecular or ionic geometry. :0: A. The Lewis diagram for PO2(OH), is: 0-H -P. :0: The electron-pair geometry around the P atom in PO2(OH)2 is There are lone pair(s) around the central atom, so the geometry of PO2(OH)2 is .. B. The Lewis diagram for CO2 is: 0=c=0 Recall that for predicting geometry, double and triple bonds count as only one electron pair. The electron-pair geometry around the C atom in CO, is There are lone pair(s) around the central atom, so the geometry of CO, is

In the BEST Lewis structure for the molecule XeF2, how many non-bonding lone pairs (1 pair = 2) of electrons are found on the central atom?

6. CO2 a. Lewis structure e. aloq hud c. Electronic geometry_ d. Molecular shape_ Bond angle? b. Draw the different bonds and label their polarity.

Page 4 of 4 are created 1016 words 2 14. For a bent molecule with three atoms, what is the relationship between the partial charges and the direction of the molecular dipole? 15. Why is it important to take both the polarity of the bonds and the shape of the molecule into consideration when determining the polarity of the molecule? IX English (United States) # 3 B OCT 19 the electronegatively an I $ 4 Accessibility: Investigate U A % 5 A is closer to Focus MacBook Pro ||| < 6 :E 6 P 13 less than 2. A & GE 7 8 O 150% De по

If 100.0 mL of potassium dichromate solution (10.0 g of K2Cr207 per liter) was mixed with 75.0 mL of a ferrous sulfate solution (80.0 g of FESO4:7H20 per liter), and the resulting solution titrated with 5.58 mL of a KMNO4 solution, what is the molarity of the potassium permanganate solution?

8. Classify the bonds in the following compounds as non-polar covalent, polar covalent, or ionic. The number in the bracket indicates the difference in the electronegativity. Write the structure to indicate the flow of electrons. KI (1.7)       NH3( 0.9)     CO (1.0)     CaO (2.5)     NO (0.5).

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Predicting deviations from ideal bond angles.

Following is a molecule with polar bonds whose shape was obtained using the VSEPR theory. Specify the molecular shape of this molecule, and whether the molecule is polar or nonpolar. (Hint: In terms of polarity, see whether the dipoles in the molecule cancel or not. A molecule containing polar bonds can be nanpolar if the dipoles cancel each other. You can imagine the dipoles as ropes pulling on the central atom–If the pulls cancel each other, that is, the central atom cannot move, then the molecule is nonpolar. If on the other hand the opposite is true, then the molecule is polar.) O trigonal pyramidal shape, nonpolar O trigonal planar shape, nonpolar O tetrahedral shape, polar O trigonal pyramidal shape, polar O trigonal planar shape, polar