Concept explainers
(a)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(b)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(c)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(d)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(e)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(f)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(g)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
(h)
Interpretation:
The Lewis structure for the given compound is to be drawn; the contribution of bond dipole moments to the molecular dipole moment is to be shown and whether the compound have a large, small or zero dipole moment is to be predicted.
Concept introduction:
The Lewis structures are diagrams that give information about the bonding electron pairs and the lone pairs of electrons in a molecule. Similar to electron dot structure in Lewis diagram the lone pair electrons are represented as dots and they also contain lines which represent bonding electron pairs in a bond.
The polarity of an individual bond is measured as its bond dipole moment. A quantity that describes two opposite charges separated by a distance is the dipole moment.
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EP ORGANIC CHEMISTRY -MOD.MASTERING 18W
- REPRESENTATIONS OF ORGANIC MOLECULES Identifying isomers and resonance structures Determine the relationship between Structure A and Structure B in each row of the table. Structure A Structure B Relationship H. o isomers H. H H -H H-C- C-O -H- O resonance structures H H. H H Н—С—Н o neither H o isomers H :0: :0-H H. H H- C-C C-H H-C=C C=C-H O resonance structures H. H. H o neither o isomers :o: H H. H- O resonance structures H H H. H o neither 72°F DELL :ö: IIarrow_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_forward10-066: Comparing Dipole Moments Compare the dipole moments of the following pairs of molecules and determine whether the first is "Greater Than", "Less Than" or "Equal to" the second. The dipole moment of CIO2 is ... the dipole moment of SO2 The dipole moment of AsF3 is ... the dipole moment of AsF5 The dipole moment of H20 is the dipole moment of H2S Dipole moment of HBr is The dipole moment of ICl is ... dipole moment of IF the dipole moment of HCl Submit Answer Tries 0/5arrow_forward
- 1. ClO3 2. O3 3. ClO2- 4. ClO2 Are these free radicals yes or no?arrow_forward4. 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_forwardents V Soul (TV series) O REPRESENTATIONS OF ORGANIC MOLECULES Drawing a skeletal structure from a Lewis structure Convert the Lewis structure below into a skeletal structure. Н—С— Н H. H- H- Н—С—Н H. HH H. H- Н—С—С—С—С—С—С—С- Н C=C H- H. H. H. Н—С— Н H. ct+ Click and drag to start drawing a structure. HIC CIH HICarrow_forward
- Determine the Lewis structures of the following compounds, and determine which ones have dipole moments. For each molecule that has a dipole moment, draw a ball-and-stick model and include an arrow to indicate the direction of the dipole moment. * Your answer is incorrect. Write the Lewis structure of the CH ✔Draw Your Solution eTextbook and Medial Hint Your answer is incorrect. Write the Lewis structure of the CHCl3. Hint Draw Your Solution * Your answer is incorrect. Write the Lewis structure of the CH₂Cl₂. ✔Draw Your Solution Hintarrow_forward2. From the models of SF4, BrF3, and XeF4, deduce whether different atom arrangement, called geometrical isomers, are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction, Preferred Molecular Compound Electron Dipole Reason Geometry Moment (Polarity) geometry SF4 BRF3 XeF4 3. Using the Lewis structure predict the geometrical structures of the following ions and state the hybridization of the central atom. Ion Electron Geometry Molecular Formal Charge Central Atom Geometry of Central Hybridization Atom CO32- NO3- BF4arrow_forwardConsidering the position of the elements in the periodic table and their relative electronegativities and bond polarities, which bond is longest? a. carbon - Oxygen triple bond b. carbon - Oxygen single bond c. carbon - Carbon single bond d. carbon - Carbon double bond e. carbon - Nitrogen triple bond Which bond is the strongest? a. carbon - Nitrogen triple bond b. carbon - Nitrogen double bond c. carbon - Hydrogen bond d. carbon - Carbon triple bond e. carbon - Carbon single bondarrow_forward
- 3. Use electronegative trends to predict which bond in each of the following groups will be the most polar and indicate the bond polarity (show the partial positive and negative ends) of the bond. You may (but are not required to) check your answer by using the table of electronegative values. а. С- Н, Si — Н, Sn - H b. Al – Br, Ga – Br, In – Br, с. С-Оor Si - O d. 0-F or O- Cl Tl – Br - 4. Ch 8, Problem 54 For each of group, order the atoms and/or ions by decreasing size. Justify each answer. a. V, V2*, v3+, vs+ c. Te, I, Cs", Ba? e. O?, s?, Se?, Te?- b. Na", K*, Rb*, Cs* d. P, P', P², p³- 2+arrow_forwardDetermine if the structural formula below is an acceptable Lewis structure for organic compounds. Point out the problems in cases where structure is invalid. CH3 CH2 CH-CH-CH-C-CH3 ČH3 ČH3 A. The structure is not correct because carbon can only form four bonds or less. In the case of more or fewer bonds the atom will have a charge. B. The structure is not correct because carbon can form more than four bonds or less. In the case of more or fewer bonds the atom will have a charge. C. This structure is the correct Lewis structure. D. The structure is not correct because carbon can only form four bonds or more. In the case of only fewer bonds the atom will have a charge.arrow_forward3. 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_forward
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