Draw the Lewis structure of BH4- and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has: lone pairs = single bonds = double bonds = triple bonds = atoms with a positive formal charge = atoms with a negative formal charge = Is this structure stabilised by resonance?

Draw the Lewis structure of BH4- and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has: lone pairs = single bonds = double bonds = triple bonds = atoms with a positive formal charge = atoms with a negative formal charge = Is this structure stabilised by resonance?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.89QE

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Consider one resonance structure for the azide ion, N3-1 : What is the formal charge on each nitrogen atom in this resonance structure? Enter your answer as a number preceded by the appropriate charge (+ or -), if applicable. If the formal charge is zero, enter 0 . formal charge of left N [a] formal charge of middle N [b] formal charge of right N [c]
1 ) Draw the Lewis dot structure for RbIO2RbIO2. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. b ) Draw the Lewis dot structure for NH4ClNH4Cl. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. c) Draw the Lewis dot structure for KOHKOH. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. d) Draw the Lewis dot structure for Sr(CN)2Sr(CN)2. Include all hydrogen atoms and nonbonding electrons. Show the formal charges of all atoms. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. e)
The carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]
Question 4 options: Draw the Lewis structure of CS2 and use your Lewis structure to help fill in the missing numbers. Hint: you must put a number in each box. If the answer is zero, you must enter "0". The Lewis structure has: lone pairs, single bonds, double bonds, triple bonds, atoms with a positive formal charge, and atoms with a negative formal charge. Is this structure stabilised by resonance? (Enter either yes or no below - no other words).
An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of zero. H Н—N—С- -о—с—Н H H Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges. Click and drag to start drawing a structure.
Enter a Lewis structure for each of the following ions: 1. Draw the Lewis dot structure for Al3+. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. Show the formal charge of the atom. 2. Draw the Lewis dot structure for Mg2+. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. Show the formal charge of the atom. 3. Draw the Lewis dot structure for Se2−. To change the symbol of an atom, double-click on the atom and enter the letter of the new atom. Show the formal charge of the atom. 4. Draw the Lewis dot structure for N3−N3−. Show the formal charge of the atom.
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Calculating Formal Charge: Formal charge is calculated for each atom in a structure. It provides information about the stability and reactivity of the atom in the molecule. Formal Charge = Valence Electrons - 1/2 Bonding Electrons - Non-bonding Electrons For example, the formal charge on the carbon of methane is calculated here. Carbon has 4 valence electrons. There are 8 bonding electrons around it. Formal Charge4- 12 (8) -0 Calculate the formal charge on the circled atoms in the following structures. formal charge: Incorect formal charge: formal charge: 1 Incomect