Question

For each of the following molecules, determine: (a) whether it has polar bonds; (b) what its...

For each of the following molecules, determine: (a) whether it has polar bonds; (b) what its molecular shape is; (c) whether the molecule is polar. You will need to draw the Lewis structures first.

(i) NH3. N is the central atom.

(ii) BI3. B is the central atom.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Draw the Lewis structures and determine which of these molecules has a central atom that unavoidably...
Draw the Lewis structures and determine which of these molecules has a central atom that unavoidably violates the octet rule. Please note that NO3 has an odd number of electrons. But you must decide where the missing electron will be. Does the central atom violate the octet rule or do the oxygen atoms? Use formal charges to decide. IN THE ANSWER THAT YOU GIVE DO NOT DRAW THE STRUCTURE. JUST TELL ME THE ANSWER. EXPLANATION NOT WANTED. NO3- CS2 SO3...
-label the polar bonds in each molecule with its correct molecular shape, and then decide if...
-label the polar bonds in each molecule with its correct molecular shape, and then decide if the molecule is polar or nonpolar. How do you know when dipoles cancel or reionforce? 1. CH2F2 2. CCl4
Consider the following statements and determine which are true and which are false. SeF4 is a...
Consider the following statements and determine which are true and which are false. SeF4 is a polar molecule. NO3- has only two resonance Lewis structures. Bond angles for IF6+ are 60 °. The formal oxidation state of an atom in a molecule (or molecular ion) can be calculated as: (the number of valence electrons on a free atom) minus (half the number of electrons in bonds to that atom) minus (the number of unshared electrons assigned to the atom in...
The N2F2 molecule has the two nitrogens as the central atoms. State the hybridization that exists...
The N2F2 molecule has the two nitrogens as the central atoms. State the hybridization that exists at the nitrogen atoms.Draw the Lewis structure and predict the ideal bond angles around nitrogen in N2F2 using the molecular shape given by the VSEPR theory. Explain why some molecules of N2F2 are found to be polar and others are non-polar. (You may use diagrams to illustrate your answer.)
Determine whether the bonds in each of the following compounds are polar or nonpolar covalent bonds:...
Determine whether the bonds in each of the following compounds are polar or nonpolar covalent bonds: H2 H2O Cl2 HCl CO2 Type Answer or Dont Bother Answering
Classify each of the following bonds as nonpolar covalent, polar covalent, or ionic. If a bond...
Classify each of the following bonds as nonpolar covalent, polar covalent, or ionic. If a bond is polar covalent, identify the atom that has the partial negative charge and the atom that has the partial positive charge. If a bond is ionic, identify the ion that has the negative charge and the ion that has the positive charge. a. N−O d. H−I g. Se−I j. F−P b. Al−Cl e. Br−Cl h. N−Sr c. Cl−N f. Cl−S i. O−F
Identify the electron pair geometry and the molecular structure of each of the following molecules: (a)...
Identify the electron pair geometry and the molecular structure of each of the following molecules: (a) ClNO (N is the central atom) (b) CS2 (c) Cl2CO (C is the central atom) (d) Cl2SO (S is the central atom) (e) SO2F2 (S is the central atom) (f) XeO2F2 (Xe is the central atom) (g) ClOF2 + (Cl is the central atom)
Draw the correct Lewis structure and calculate the formal charge of each atom in the N2O...
Draw the correct Lewis structure and calculate the formal charge of each atom in the N2O molecule (N is the central atom.). Use the resonance structure of the molecule N=N and N=O bonds, (i.e., N=N=O) to determine the formal charges. A. N = 0; N = –1, O = +1 B. N = +1; N = 0, O = -1 C. N = -1; N = +1, O = 0 D. N = 0; N = 0, O = 0...
Hydrogen peroxide is a syrupy, viscous water-soluble compound. This is expected based on the structure. The...
Hydrogen peroxide is a syrupy, viscous water-soluble compound. This is expected based on the structure. The Lewis structure has _______ total valence electrons. There are _______ bonding pairs and _______ non-bonding pairs. The electron pair geometry around each oxygen atom is _______ giving a _______ shape at each oxygen atom. The central bond is _______ (polar/nonpolar) and the peripheral bonds are _______ (polar/nonpolar) with the dipole vectors pointing _______ (away from/towards) the oxygen atoms. Overall the bond dipoles _______ (add...
Which of the following molecules has polar bonds and is nonpolar? A. HF B. ICl3 C....
Which of the following molecules has polar bonds and is nonpolar? A. HF B. ICl3 C. NF3 D. SF4 E. BF3 SF4 is not the right answer because it is not symmetrical (Bonding Geometry: Seesaw, Electron Geometry: Trigonal Bipyramidal). So then please explain how any of these can be non-polar
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT