Concept explainers
(a)
Interpretation:
The group number of the nitrogen should be determined according to the periodic table and whether the group number is matched with the number of dots on nitrogen in Figure 2.1 should be checked.
Concept Introduction :
In the periodic table, elements are arranged in order of increasing
Nitrogen present in the fifth column and the second period of the periodic table.
(b)
Interpretation:
The number of line bonds that are attached to
Concept Introduction :
A number of line bonds indicate the number of line bonds to the atom in the Lewis structure.
(c)
Interpretation:
Number of nonbonded electrons drawn on
Concept Introduction :
The number of nonbonded electrons are free electrons that can be seen on the atom in the Lewis structure. These are shown by using dots on the atom.
(d)
Interpretation:
The formal charge of each atom in
Concept Introduction :
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
The number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pairs of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure
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Organic Chemistry: A Guided Inquiry
- 1. a)draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula CN- b) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula BrI3arrow_forwardDraw the Lewis structures (with formal charges) of each of the species in the indicated pair and use the lewis stucture to answer which has the longer bond? and which has the stronger bond? 1.) O2 or O2^2+ 2.) NO- or NO^3- 3.) F2 or F2^2+ 4. NO2+ or NO2^3- 5.) OF2 or FO+arrow_forward1.a)draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula OF2 b) draw the complete Lewis structure (atoms, dots, lines, dashes, wedges, formal charges) for the formula CH2Cl2arrow_forward
- 3.A. Add all implied hydrogen atoms and any missing lone pairs of electrons. There are many possible ways to get a negative charge on carbon, but only one with filled octets.arrow_forward2. In biologically relevant molecules, carbon and the halogens don't have a charge. In contrast, nitrogen (neutral or positively charged) and oxygen (neutral or negatively charged) don't always appear in their uncharged form. Consider the following questions. a. Add any unshared pairs of electrons necessary to complete the Lewis structure shown for formaldehyde (note: there are no formal charges in this molecule). b. Assign any formal charges necessary to complete the structure shown for the acetylide anion. c. Recalling that atoms want a complete octet, add unshared pairs of electrons, and assign formal charges as appropriate to the Lewis structure of the amino acid aspartic acid as it would exist at a physiological pH of ~7.4 (aspartic acid has an overall -1 charge at this pH). A. H O H formaldehyde B. H C C: C. H H \/ acetylide anion H-N O=C H он O H aspartic acidarrow_forwardPlease answer these questions on your Page 1 (1) Give a reasonable Lewis structure, including formal charges, for HNC (N.B. N is the central atom). H, N, and C are in groups 1, 5, and 4 and their atomic numbers are 1, 7, and 6. (2) Give a reasonable Lewis structure, including formal charges, for ClO (N.B. Cl is the central atom). Cl and O are in groups 7 and 6 and their atomic numbers are 17 and 8. (3) Give a reasonable Lewis structure, including formal charges, for XeO₂F3 (N.B. Xe is the central atom). Xe, O, and F are in groups 8, 6, and 7 and their atomic numbers are 54, 8, and 9. (4) Give a reasonable Lewis structure, including formal charges, for XeO3F2 (N.B. Xe is the central atom). Xe, O, and F are in groups 8, 6, and 7 and their atomic numbers are 54, 8, and 9. (5) Give a reasonable Lewis structure, including formal charges, for O. O is in group 6 and its atomic number is 8.arrow_forward
- 4. The following are valid Lewis structures for CH3SOCH3. Label the formal charges and circle the best Lewis structure. H :ö: H H :0 H a) H-C=S-C-H b) Н—С—S— С-н H. H. H. H. Н :0: Н H :ö: H d) H-C=$-C-H c) Н—С—$—С-н H. H. H Harrow_forward3. Molecule: CH4 indicate the number of available electrons that are in the molecule. ae = Trial Structure: in the space to the right connect all of the atoms to the central atom and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? Circle the correct ne = ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom Hybridization:arrow_forwarda) Draw all the possible Lewis structures for the following ions: SeCl4 PO43- BrO3 b) Assign formal charges to each atom in each resonance structure (Show all your work on paper) c) indicate the most plausible Lewis structure. (Show all your work on paper) d) Indicate the approximate bond angles for each ion. (e) determine the names for the molecular geometry. (Show all your work on paper) (d) determine if the molecule is polar or non-polar;arrow_forward
- 5. Molecule: XeFs* indicate the number of available electrons that are ae = in the molecule. Trial Structure: in the space to the right connect all of the atoms to the central atom and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization:arrow_forwardWrite a single Lewis structure that obeys the octet rule for SO3 and assign the formal charges on all the atoms. (There should be one double bond in the structure.) Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons and formal charges. [] H N. P. F Br More Press SPACE to add C atom on the canvas. Press (TAB to go to the structure. Press %23 Formal.. amazun P Type here to search B. Master. 10804arrow_forwardhelp on all 3 parts of this question please. every time o go to submitt it its saying I put them in the wrong order. A) Arrange the following elements in order of increasing electronegativity:iodine, bromine, astatine, chlorine B) Arrange the following elements in order of increasing electronegativity:carbon, germanium, silicon, tin C)Arrange the following elements in order of increasing electronegativity:cesium, lead, thallium, bariumarrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning