Decide whether the Lewis structure proposed for each molecule is reasonable or not. proposed Lewis structure Is this a reasonable structure? If not, why not? molecule O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. BeH, H– Be –H The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are:U O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. CO, :0–C=0: The correct number is:| O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. OF2 The correct number is: F=0=F O No, some atoms have the wrong number of electrons around them. .. The symbols of the problem atoms are:|| * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice. Explanation Check O2021 McGraw-Hill Education. All Rights Reserved Terms of Use

Decide whether the Lewis structure proposed for each molecule is reasonable or not. proposed Lewis structure Is this a reasonable structure? If not, why not? molecule O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. BeH, H– Be –H The correct number is: O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are:U O Yes, it's a reasonable structure. O No, the total number of valence electrons is wrong. CO, :0–C=0: The correct number is:| O No, some atoms have the wrong number of electrons around them. The symbols of the problem atoms are: O Yes, it's a reasonable structure. No, the total number of valence electrons is wrong. OF2 The correct number is: F=0=F O No, some atoms have the wrong number of electrons around them. .. The symbols of the problem atoms are:|| * If two or more atoms have the wrong number of valence electrons around them, just enter the chemical symbol for the atom as many times as necessary. For example, if two oxygen atoms have the wrong number of electrons around them, enter the symbol O twice. Explanation Check O2021 McGraw-Hill Education. All Rights Reserved Terms of Use

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter7: Chemical Bonding And Molecular Structure

Section: Chapter Questions

Problem 7.92PAE

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Similar questions

Consider 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.
Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.
Fill in the blanks in each line of the following table that involves characteristics of various bonds between nonmetals. The first line is already completed as an example.
The valence shell of an atom in a legitimate Lewis structure (see Figure 2.3) has what in commonwith the valence shell of a noble gas? (Noble gases are stable elements found in the last column ofthe periodic table, e.g., He, Ne, Ar, etc.)
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar and which are nonpolar? (b) Which is the most polar bond in the molecule? Which atom is the partial negative end of this bond?
a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.
Vitamin B6 is an organic compound whose deficiency in the human body can cause apathy, irritability, and an increased susceptibility to infections. Below is an incomplete Lewis structure for vitamin B6. Complete the Lewis structure and answer the following questions. Hint: Vitamin B6 can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure below to give each atom a formal charge of zero. a. How many bonds and bonds exist in vitamin B6? b. Give approximate values for the bond angles marked a through g in the structure. c. How many carbon atoms are sp2 hybridized? d. How many carbon, oxygen, and nitrogen atoms are sp3 hybridized? e. Does vitamin B6 exhibit delocalized bonding? Explain.
Use the Molecule Shape simulator (http://openstaxcollege.org/I/6MolecShape) to build a molecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.
rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. msp;a.GeH4c.NI3b.ICld.PF3
Methylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is In this molecule, which is the (a) weakest carbon-containing bond? (b) strongest carbon-containing bond? (c) most polar bond?