Lewis structures for compounds

Draw three Lewis structures for compounds with the vjfARis formula C2H2F2. Indicate which of the compound(s)... 

In Lewis theory, we combine the Lewis structures of elements to form Lewis structures for compounds. We represent ionic bonding-the bonding between a metai and a nonmetai through the transfer of electrons-by moving dots from the Lewis structure of the metai to the Lewis structure of the nonmetal. The metal becomes a cation and the nonmetal becomes an anion (see Section 3.3). For example, sodium and chlorine have the following Lewis structures ... 

EXAM PLE 9.10 Writing Lewis Structures for Compounds Having Expanded Octets Write the Lewis structure for Xep2. ... 

All the following compounds are charactenzed by ionic bonding between a group I metal cation and a tetrahedral anion Wnte an appropriate Lewis structure for each anion remembenng to specify formal charges where they exist... 

Phenol has different chemical properties from those of typical alcohols. Display the electrostatic potential map for phenol. Does this suggest that phenol is likely to be a stronger or weaker acid than any of the compounds discussed above Compare the electrostatic potential map for 4-nitrophenol to that for phenol. What effect does substitution by nitro have on acid strength Explain your result by considering charge delocalization in the conjugate base. Draw all reasonable Lewis structures for phenoxide anion and for 4-nitrophenoxide anion. Which is more delocalized Is this consistent with experimental pKa s ... 

Oxalic acid, H2C204, is a poisonous compound found in rhubarb leaves. Draw the Lewis structure for oxalic acid. There is a single bond between the two carbon atoms, each hydrogen atom is bonded to an oxygen atom, and each carbon is bonded to two oxygen atoms. 

Several compounds have the formula C3H60. Write Lewis structures for two of these compounds where the three carbon atoms are bonded to each other in a chain. The hydrogen and the oxygen atoms are bonded to the carbon atoms. 

Sei f-Test 2.4A Write the Lewis structure for the interhalogen compound chlorine... 

Write the complete Lewis structure for each of the following compounds (a) formaldehyde, HCHO, which as its aqueous solution formalin is used to preserve biological specimens (b) methanol, CH3OH, the toxic compound also called wood alcohol (c) glycine, H2C(NH2)COOH, the simplest of the amino acids, the building blocks of proteins. 

Write the complete Lewis structure for each of the following compounds (a) ammonium chloride (b) potassium phosphide (c) sodium hypochlorite. 

The boranes are electron-deficient compounds (Section 3.8) we cannot write valid Lewis structures for them, because too few electrons are available. For instance, there are 8 atoms in diborane, so we need at least 7 bonds however, there are only 12 valence electrons, and so we can form at most 6 electron-pair bonds. In molecular orbital theory, these electron pairs are regarded as delocalized over the entire molecule, and their bonding power is shared by several atoms. In diborane, for instance, a single electron pair is delocalized over a B—H—B unit. It binds all three atoms together with bond order of 4 for each of the B—H bridging bonds. The molecule has two such bridging three-center bonds (9). 

The empirical formula is C4Hy the molecular formula might be C jHlg, which matches the formula for alkanes (C H, +,). It is not likely an alkene or alkyne, because there is no reasonable Lewis structure for a compound having the empirical formula C4II9 and multiple bonds. 

C09-0020. Tin tetrachloride (S11CI4) is an important starting material for the preparation of a variety of tin compounds. Build the Lewis structure for SnCl4 and determine its shape. 

Collecting and Interpreting Data Compare the appearance of the Lewis structure for a compound with a ball and stick model of the compound. 

A The Lewis structure for the cation, the anion, and the compound follows the explanation. 

B Below each explanation are the Lewis structures for the cation, for the anion, and for the compound. 

Ca— 0 is improperly written as a covalent Lewis structure, although CaO is an ionic compound. In addition, there are only two electrons around the Ca atom. [Ca]2+[ 0 ]2" is a more plausible Lewis structure for CaO. 

Which of the following is the correct Lewis structure for the ionic compound Ca(C102)2... 

Dichlorofluoroethane, CH3CFCI2, has been proposed as a replacement for chlorofluorocarbons (CFCs). The presence of hydrogen in CH3CFCI2 markedly reduces the ozone-depleting ability of the compound. Draw a Lewis structure for this molecule. 

How does the arrangement of electrons around the central atom differ in PI3 and CII3 Draw the Lewis structures for these compounds to answer this question. 

Problem 1.24 Write Lewis structures for the isomers of C,H N. Name the compound and classify the functional group in each case. 

This problem is in the nature of review of elementary inorganic chemistry and may require reference to a general chemistry book.) Write Lewis structures for each of the following compounds. Use distinct, correctly placed dots for the electrons. Mark all atoms that are not neutral with charges of the proper sign. 

An ionic compound is indicated by writing the Lewis structures for the two ions. 

Some compounds exhibit resonance. That is, there is more than one acceptable Lewis structure for a compound. Another way to say this is that no single Lewis structure fully describes the actual structure. Resonance structures differ only in how the electrons are distributed among the atoms. If the atom connectivity is different, the two structures are isomers, which can be isolated and observed separately. 

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