Concept explainers
(a)
Interpretation: The legitimate Lewis structure of
Concept introduction: A Lewis structure is a diagrammatic view of a molecule, where lone pair of electrons are represented as dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
(b)
Interpretation: The legitimate Lewis structure of
Concept introduction: A Lewis structure is a diagrammatic view of a molecule, where lone pair of electrons is represented in dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
(c)
Interpretation: The legitimate Lewis structure of
Concept introduction: A Lewis structure is a diagrammatic view of a molecule, where lone pair of electrons is represented in dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
(d)
Interpretation: The legitimate Lewis structure of
Concept introduction: A Lewis structure is a diagrammatic view of a molecule, where lone pair of electrons is represented in dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
(e)
Interpretation: The legitimate Lewis structure of
Concept introduction: A Lewis structure is a diagrammatic view of a molecule, where lone pair of electrons is represented in dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
(f)
Interpretation: The legitimate Lewis structure of
Concept introduction: A Lewis structure is a diagrammatic view of a molecule, where lone pair of electrons is represented in dots, bonds are represented with lines & formal charge of each atom is mentioned near the atom.
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Organic Chemistry: A Guided Inquiry
- hy do atoms form bonds with one another? What can make a molecule favored compared with the lone atoms?arrow_forwardConsider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.arrow_forwardWrite Lewis structures and predict the molecular structures of the following. (See Exercises 25 and 26.) a. OCl2, KrF2, BeH2, SO2 b. SO3, NF3, TF3 c. CF4 SeF4, KrF4 d. IF5, AsF5 Which of these compounds are polar?arrow_forward
- A molecular compound is composed of 58.8% Xe, 7.2%. O, and 34.0%. F, by mass. If the molecular weight is 223 amu, what is the molecular formula? What is the Lewis formula? Predict the molecular geometry using the VSEPR model.arrow_forwardBest Lewis Formula and Molecular Geometry A student writes the Lewis electron-dot formula for the carbonate anion, CO32, as a Does this Lewis formula obey the octet rule? Explain. What are the formal charges on the atoms? Try describing the bonding for this formula in valence bond terms. Do you have any difficulty doing this? b Does this Lewis formula give a reasonable description of the electron structure, or is there a better one? If there is a better Lewis formula, write it down and explain why it is better. c The same student writes the following resonance description for CO2: Is there something wrong with this description? (What would you predict as the geometries of these formulas?) d Is one or the other formula a better description? Could a value for the dipole moment help you decide? e Can you write a Lewis formula that gives an even better description of CO2? Explain your answer.arrow_forwarda Carbonyl fluoride, COF2, is an extremely poisonous gas used in organofluorine synthesis. Give the valence bond description of the carbonyl fluoride molecule. (Both fluorine atoms are attached to the carbon atom.) b Nitrogen, N2, makes up about 80% of the earths atmosphere. Give the valence bond description of this molecule.arrow_forward
- The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds. Why?arrow_forwardPredict the molecular structure and bond angles for each molecule or ion in Exercises 87 and 93. a. CCl4 b. NCl3 c. SeCl2 d. ICl a. NO2, NO3, N2O4 (N2O4 exists as O2NNO2.) b. OCN, SCN, N3 (Carbon is the central atom in OCN and SCN.)arrow_forwardConsider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6. These 12 compounds arc all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structure. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule docs not.) See Exercises 115 and 116 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.arrow_forward
- Which of the molecules in Exercise 121 have net dipole moments (are polar)?arrow_forward1. Determine the Lewis structure, shape, and polarity of the following molecules a. BrO2-, bromite ion b. BrO3-, bromate ion c, Cl207, dichlorine heptoxide 2. Write all the valid Lewis structures of bromate ion.arrow_forwardDraw Lewis structures for the following molecules. Describe how the bond angles would bealtered based on the Lewis structure.a. CH2Sb. SCl2 Draw the Lewis structure for each of the following molecules. Calculate the formal charges ofeach atom in the following molecules and the overall charge of the molecule. (Show calculations)a. PBr3b. O3 c. NH4+arrow_forward
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