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Concept explainers
1.
To draw: The Lewis structures of the given compounds.
Interpretation: The Lewis structures of the given compounds are to be drawn.
Concept introduction: The Lewis structure shows the connectivity between atoms by identifying the lone pairs of electrons in a compound. Lewis structures are also called Lewis dot structures. The valence electrons around an atom are shown by dots. Bonds between atoms are shown by lines and the lone pair of electrons is shown by a pair of dots.
The rules to draw Lewis structure are given as,
- Determine the electronegativity and the number of valence electrons contributed by each atom.
- Generally lowest electronegativity atom is the central atom.
- Write the skeleton structure of the molecule.
- Use two valence electrons to form each bond in skeleton structure between the central and outer atoms.
- Satisfy the octets of atoms by distributing remaining valence electrons as nonbonding electrons. It is usually best start with the outer atoms.
2.
To show: The kinds of orbitals that overlap to form each bond in the given compounds.
Interpretation: The kinds of orbitals that overlap to form each bond in the given compounds are to be shown.
Concept introduction: In the sigma bond formation hybridized orbitals overlap with other hybridized or unhybridized orbitals. In the formation of pi bonds only unhybridized orbitals are involved.
3.
To determine: The approximate bond angles in the given compounds.
Interpretation: The approximate bond angles in the given compounds are to be stated.
Concept introduction: All the carbon atoms with single bond formation always arranged in tetrahedral manner. In tetrahedral arrangement the bond angles between the atoms is always
The actual bond angles in “
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Chapter 1 Solutions
Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Organic Chemistry
- Draw Lewis electron dot structures for CH3Cl (methyl chloride, a topical anesthetic), H2O2 (hydrogen peroxide, with an O-O bond), and NH2OH (with an N-O bond).arrow_forwardAcrylamide, H2C=CHCONH2, is a known neurotoxin and possible carcinogen. It was a shock to all consumers of potato chips and french fries a few years ago when it was found to occur in those products. (a) Sketch the molecular structure of acrylamide and identify all bond angles. (b) Indicate which carbon-carbon bond is the stronger of the two. (c) Is the molecule polar or nonpolar? (d) The amount of acrylamide found in potato chips is 1.7 mg/kg. If a serving of potato chips is 28 g, how many moles of acrylamide are you consuming?arrow_forwardDraw the Lewis structure for each organic compound from its condensed structural formula.a. C2H4 b. CH3NH2 c. HCHOd. CH3CH2OH e. HCOOHarrow_forward
- Draw a Lewis structure for each ion. a. CH3O− b. HC2− c. (CH3NH3)+ d. (CH3NH)−arrow_forwardDraw the Lewis structure for each compound.a. Cl2O7 (no Cl¬Cl bond)b. H3PO3 (two OH bonds)c. H3AsO4arrow_forwardWhich of the following molecules has/ have resonance structures? Select one or more: a.CH2=CH2 b.CH3–OH c.CH2=CH–O– d.CH3–O–CH3arrow_forward
- Consider the molecules — BrF5. A. Draw the best Lewis structure for this molecule. Label any atoms with nonzero formal charge. B. Label each bond angle. As part of your answer be sure to include if it is more or less than the ideal bond angle. C. What is the electron geometry around the bromine atom? D. Are the bonds in the molecule polar? E. Is the overall molecule polar? — CH2 F2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. Answers for A-D here: C. Redraw the shape of the molecule. Draw all dipoles. D. Is the overall molecule polar? — Consider the molecule CH2 CF2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. C. Redraw the shape of the molecule (according to the exacting specifications of your instructor). Draw all dipoles. D. Is the overall molecule polar?arrow_forwardFill in the table. Central atom is listed first. A. Write the number of valence electrons below the formulaB. Draw the Lewis structureC & D. Write the Electron Group Geometry and Molecular Shape NamesE. Write the bond angleF. Write the molecular polarity. "P" for polar and "NP" for nonpolar. SpeciesValenceElectrons(1 pt.) LewisStructure(2 pt.) Electron PairGeometryName(1 pt.) Molecular ShapeName (1 pts.) BondAngle (1 pt.) Molecular Polarity(1 pt.) PO43- NOBr Uploadarrow_forward4. Multiple structures with the same chemical formula (number and type of each element present) but differing in the atom connectivity are called structural isomers. Use the skeletal structure below to draw a structural isomer of what you have already drawn in Table 4. H O H 0 CN H a. Label the central atoms like you did in Table 4 and name the geometries of each of them.arrow_forward
- 3. Write the Lewis dot (electron dot) symbol for each covalent molecule. Remember the number of unpaired electrons in the Lewis dot symbol of the atom determines the number of bonds each atom makes. If your molecule has unpaired electrons you are not done. If your molecule has the wrong number of bonds for some atoms it is wrong. Try a different arrangement of atoms. Working left to right will help you. Show loan pairs. a. CH3CH₂OH b. CHCl, Br C. CH3NH₂ d. CHỊCH,CH,CH,CH3 e. CH3SCH 3 4. Write the Lewis dot (electron dot) symbol for each covalent molecule. Remember the number of unpaired electrons in the Lewis dot symbol of the atom determines the number of bonds each atom makes. If your molecule has unpaired electrons you are not done. If your molecule has the wrong number of bonds for some atoms it is wrong. Try a different arrangement of atoms. Working left to right will help you. Show loan pairs. a. HCN b. CH3COOH c. H₂CCONHCH3 d. HCCH e. C6H12arrow_forward1. What is the relationship between the following compounds? H :0: H H:0: H H-C=C-C-C-C-H H-C-C-C=Ċ-H H HH H. H-C-H B. constitutional isomers C. the same structure A. isotopes D. composed of different elements E. no relationship 2. What is the correct Lewis structure for HN3, including the formal charges? CIHarrow_forward11. Which of the following statements about resonance is true? I. Resonance hybrids occur because a compound changes back and forth between two or more resonance structures. II. Resonance structures differ in the arrangement of electrons but not in the arrangement of atoms. III. Resonance hybrids contain delocalized electrons. IV. Resonance structures for a given compound always contribute equally to the resonance hybrid. V. Resonance structures occur when there are two or more valid Lewis structures for a given compound. VI. Resonance hybrids are a composite of resonance structures. a. I, II, V, VI b. I, II, V, VI c. II, III, IV, VI d. II, III, V, VI e. II, IV, V, VI 12. How many resonance forms will nitrate ion (NO3-) have? a. -1 b. 0 c. 1 d. 2 e. 3 13. A list of non-metals is given below. Which elements cannot exceed the octet rule? B Si N P O S F Cl a. Si, P, S, Cl b. B, N, O, F c. O, S, F, Cl d. B, Si, N, P e. All eight elements can exceed the octet…arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
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