1.a. Draw the Lewis structure for H3CBr H H C

1.a. Draw the Lewis structure for H$_3$CBr H H \ C - Br H b. Draw the molecule showing the shape. Include bond angles. 109.5 Br C H H c. Use the arrow notation to indicate the polarity of the following bonds in the shape in (b) C - H C - Br d. Is the molecule polar or non-polar? Explain how you decided.

For CHF2Br Draw the Lewis structure. Show the placement of all bonds and unshared (lone) pairs of electrons. c) Calculate the formal charge on each atom. Show the charges on the molecule above if the charge for the atom is something other than zero. d) The number of atoms bonded to the central atom is ______________ e) The number of unshared pairs on the central atom is ______________ f) The electronic geometry is __________________________________ g) The molecular geometry is __________________________________ h) Determine whether the bonds are polar or nonpolar. Draw arrows on each bond of the Lewis structure above to indicate the direction of electron pull for any polar bonds. Show the math you use to determine if the bonds are polar. i) Is the molecule polar or non-polar? Why?

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