Concept explainers
(a)
Interpretation:Whether there is any box in the table in model 5 having N atom with zero bonds and 3 lone pairs.
Concept introduction:Losing 1 electron around an atom from its ground state gives a +1 formal charge to that atom. Adding extra electron to an atom will give a negative charge to the atom.
(b)
Interpretation: Whether there is any box in the table in model 5 having O atom with 3 bonds and zero lone pairs.
Concept introduction: Losing 1 electron around an atom from its ground state gives a +1 formal charge to that atom. Adding extra electron to an atom will give a negative charge to the atom.
(c)
Interpretation: The reasons for the statement being true should be explained.
Concept introduction: Losing 1 electron around an atom from its ground state gives a +1 formal charge to that atom. Adding extra electron to an atom will give a negative charge to the atom. The occurrence of formal charges can be determined by counting the number of bonds & lone pair.
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Organic Chemistry: A Guided Inquiry
- Add formal charges to CH,. Note the presence of the lone pair. Add formal charges to CH,. Select Draw Rings More Erase Select Draw Rings More Erase H. // C H. -:- H. H C H. Which atoms have a complete octet? Add a lone pair to NH,. Add a formal charge, MacBook Pro ofarrow_forwardAssignment Score: OResources Give Up? O Hint 58.7% Check Answer Question 2 of 30 <. Consider the structure shown. :O: Determine the number of shared and unshared electrons in the structure. shared (bonding) electrons: unshared (lone, nonbonding) electrons: Determine the number of shared and unshared pairs of electrons in the structure. shared (bonding) pairs of electrons: unshared (lone, nonbonding) pairs of electrons: Determine the total number of valence electrons in the structure. total valence electrons:arrow_forwardMatch the atom with it's formal charge. C -H H ... H-C-P -c-H ai bi Prompts a Submitted Answers Choose a match Choose a match Choose a match Iarrow_forward
- . Answer the following questions about compound A. [2] [1] A Label the shortest C- C single bond. Explain b. Label the longest C – C single bond. Explain c. Considering all the bonds, label the shortest C – C bond. Explain. d. Label the weakest C – C bond. Explain. e. Label the strongest C - H bond. f. Explain why bond [1] and bond [2] are different in length, even though they are both C– C single а. lain. bonds.arrow_forwarda.)Draw a Lewis diagram for POBr3 in which all atoms have a formal charge of zero . b.)Draw a Lewis structure for POBr3 in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms. c.)Based on formal charge, which is the best Lewis structure for the molecule?octet rule satisfied for all atoms or smallest formal chargearrow_forwardWould you mind to check all the answer on this table because I try to understand the line bond structure and re-draw structure my homework? Could you help me with this question CS2?arrow_forward
- Q4. Draw all the resonance contributing structures for each of the molecules or ions below. Be sure to include the curved arrows that indicate which pairs of electrons are moving in going from one resonance structure to the next. Be certain to show all valence electrons and all formal charges. a) CH3NO2 b) CH3CH=CHCH2arrow_forwardCheck the box next to each molecule on the right that has the shape of the model molecule on the left: molecules model (check all that apply) olo O C,H, О НОСІ You can drag the slider to rotate the model molecule. O CO, O N,H, O None of the above Note for advanced students: the length of bonds and size of atoms in the model is not necessarily realistic. The model is only meant to show you the general geometry and 3D shape of the molecule.arrow_forward2. Indicate the formal charge on each carbon atom in the examples below. All lone pairs are shown. H H HC- -H H—C—H H C H H H- H C -H H 3. Keeping in mind that all row two elements need to have 8 electrons and each bond contains two electrons, draw the missing lone pair electrons on each O or N below. Then, assign the missing formal charges to each O or N. +*+*arrow_forward
- Atom A has 4 valence electrons. Atom Z has 6 valence electrons. For the AZ3-2 ion, answer the following questions about its Lewis dot structure (drawn according to Chm 130 guidelines). a. How many valence electrons are in the structure? b. How many single bonds are in the structure? c. How many double bonds are in the structure? d. How many triple bonds are in the structure? e. How many lone pairs are on the central atom in the structure? f. What is the shape of the structure? g. What are the bond angles of this ion?arrow_forwardSC ! F1 Q @ 2 F2 W #3 Which structure has a formal charge of -1 on the carbon shown with a "C"? Note that the atom of interest in each case includes any hydrogens or lone pairs that are present. =C- (b) (c) (d) O a.. O b.. O c.. O d.. A Moving to another question will save this response. >> 20 F9 F10 F3 F4 E @ $ 4 R % F5 T MacBook Air F6 6 Y & 7 F7 U * 00 8 DII FB ( 9 ) 0 I P a F11arrow_forwardWould you mind to check all the answer on this table because I try to understand the line bond structure and re-draw structure my homeworkarrow_forward
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