For each of the following molecules draw the Lewis structure on a separate sheet of paper.

Draw the Lewis structures of the neutral atom of Nitrogen and the ion of Nitrogen. Determine also the number of electrons gained or lost in forming an ion.                          ------------------IN SHORT------------------- Draw the Lewis Structures for:  1. Neutral Atom of Nitrogen 2. Ion of Nitrogen      - Determine also the number of electrons gained or lost in forming an ion. NOTE : The Answer must be two different Lewis Structures, one for the Neutral Atom of Nitrogen and one for the Ion of Nitrogen. Both are different from each other so the answer should have 2 forms of lewis structures.

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

184. Subject  :- Chemistry

Use this condensed chemical structure to complete the table below

Consider the following incomplete structures. On your rough sheet, complete their correct Lewis structures (including minimizing formal charge) by adding electrons/bonds where necessary. Which statement below is true of the completed Lewis structures? Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. The NOCI," exhibits both formal charges and resonance hybrids, while the BrOCI," exhibits resonance hybrids but no formal chargés None of these. The NOCI, exhibits formal charges but no resonance hybrids, while the BrOCI," exhibits both formal charges and resonance hybrids The NOCI, exhibits both residual formal charges and resonance hybrids, while the BrOCI, exhibits formal charges but no resonance hybrids At least one atom in each molecule exhibits formal charges, and the molecules have no resonance hybrids The BrOCI, exhibits formal charges but no resonance hybrids, while the NOCI, exhibits resonance hybrids but no formal…

Paraphrasing .ewriting Tool Car note Pirate Ship BLACKBOARD [Review Toplcs) [References) Unshared, or lone, electron pairs play an important role in determining the chemical and physical properties of organic compounds. Thus, it is important to know which atoms carry unshared pairs. Use the structural formulas below to determine the number of unshared pairs at each designated atom. Be sure your answers are consistent with the formal charges on the formulas. The number of unshared pairs at atom a is 0 0 b c CH,-CH2-0-H a The number of unshared pairs at atom b is 3 0. The number of unshared pairs at atom c is o e. The number of unshared pairs at atom a is The number of unshared pairs at atom b is „CH2 The number of unshared pairs at atom c is Submit Answer Retry Entire Group 9 more group attempts remaining (Previous Next> FE 1 18 étv S ali Z W MacBook Air DII 888 F10 FO F3 F4 & dele 4 6. 8 { P R Y F G J K L V M command option B

Why is this theory successful? Can you name some of the limitations of the theory? Drag the appropriate items to their respective bins. to determine the shape of the molecule or ion to determine the formulas of ionic compounds Lewis theory allows us to account for the paramagnetism of some species (e.g. oxygen) to determine how the bonds in the molecules and ions form to predict what molecules or ions will be stable, which will be more reactive, and which will not exist to account for the low melting points and boiling points of molecular compounds compared to ionic compounds Lewis theory does not allow us Reset Help

Please refer to the example image to answer. You must use CER, claim-evidence-reasoning. Make sure that your answer is CLEAR.  Claim is your answer to the question. Evidence is from the image and reasoning is your explanation.  Proper evidence for all Lewis structures include: Carbon or most electronegative atom in center. Octet of electrons surrounding each atom. Total number of electrons depicted equals same total number of valence electrons from each participating atom. Make sure to refer to the example image because it shows the correct Lewis structures. The question you're answering is about the students drawing of CH20.

Show how these pairs of elements combine into octet-rule molecular compounds, as in the first example. First, draw their atomic Lewis structures, then use any number of these atoms to build an O.R. molecule, with multiple bonds if needed (you may not add a charge to make it O.R. as an ion!). Draw the O.R. Lewis structure, write its formula and chemical name. Atoms O.R. molecule Formula Name Carbon dioxide •¢. and ö. ö=c=ö CO2 H + Se I + S