Alkanes Lewis structures

Draw Lewis structures of the following molecules and identify each as an alkane, alkene, or alkyne (a) CH3CCCH3 ... 

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. 

C09-0075. Draw Lewis structures of all possible stmctural isomers of the alkanes with formula Cg H14. ... 

The Lewis structures for the alkane having one carbon atom are as follows. 

The cycloalkanes are a special class of alkanes in the form of a ring. Figure 2-30 shows the Lewis structures and line-angle formulas of cyclopentane and cyclohexane, the cycloalkanes containing five and six carbons, respectively. 

Multiple carbon-carbon bonds result when hydrogen atoms are removed from alkanes. Hydrocarbons that contain at least one carbon-carbon double bond are called alkenes and have the general formula C H2 . The simplest alkene (C2H4), commonly known as ethylene, has the Lewis structure... 

The three-dimensional representations and the ball-and-stick models for these alkanes indicate the tetrahedral geometry around each carbon atom. In contrast, the Lewis structures are not meant to imply any three-dimensional arrangement. Moreover, in propane and higher molecular weight alkanes, the carbon skeleton can be drawn in a variety of different ways and still represent the same molecule. 

Given a Lewis structure, a condensed formula, or a line drawing for an organic compound, identify it as representing an alkane, alkene, alkyne, arene (aromatic), alcohol, carboxylic acid, ether, aldehyde, ketone, ester, amine, or amide. 

I) The alkanes are covalent compounds. Write Lewis structures for ethane and propane. 

Although Lewis structures can be used to describe bonding in alkenes, they do not really explain why alkenes are so much more chemically reactive than alkanes. In order to explain the reactivity of alkenes, a more sophisticated model of bonding must be used. 

Plan To determine the condensed structural formula of the product, we must first write the condensed structural formula or Lewis structure of the reactant In the hydrogenation of the alkene, H2 adds to the double hond, producing an alkane. 

As will be seen over and over again, carbon has a tendency to form four bonds. In alkanes these four bonds will be either single bonds to H or single bonds to G. Another simple alkane is propane, CjHg, which is represented by the following Lewis structure. 

Methane (CH4) and ethane (C2He) are the first two members of the alkane family. Figure 3.2 shows molecular formulas, Lewis structures, and ball-and-stick models for these molecules. The shape of methane is tetrahedral, and all H—C—H bond angles are 109.5°. Each carbon atom in ethane is also tetrahedral, and all bond angles are... 

The formulas for the alkanes given in Table 25.1 are written in a notation called condensed structural formulas. This notation reveals the way in which atoms are bonded to one another but does not require drawing in all the bonds. For example, the Lewis structure and the condensed structural formulas for butane (C4H10) are... 

We will frequently use either Lewis structures or condensed structural formulas to represent organic compounds. Notice that each carbon atom in an alkane has four single bonds, whereas each hydrogen atom forms one single bond. Notice also that each succeeding compound in the series listed in Table 25.1 has an additional CH2 unit. 

Analyze We are asked to predict the compound formed when a particular alkene undergoes hydrogenation (reaction with H2). Plan To determine the structural formula of the reaction product, we must first write the structural formula or Lewis structure of the reactant. In the hydrogenation of the alkene, H2 adds to the double bond, p rodudng an alkane. (That is, each carbon atom of the double bond forms a bond to an H atom and the double bond is converted to a single bond.)... 

Alkanes are hydrocarbons in which all carbon atoms are connected by single bonds. They have the general molecular formula C H2 +2> where n represents the number of carbon atoms in the molecule. The simplest alkane is methane (CHJ, the major component in natural gas. Since methane is a prototype for all hydrocarbons, many of the properties of hydrocarbons can be understood by understanding methane. Let s use some of what we have learned in Chapter 5 to determine the structure and properties of methane. We begin with the Lewis structure of methane. 

Computational chemists will readily attest that it is nowadays hard to compute metal clusters but trivial to compute ground state closed-shell organic molecules. On the other hand, we have seen that it is equally hard to understand the electronic structures of metals and alkanes. The MOVE formulas for methane and derivatives differ from the Lewis structure ip a fundamental way ... 

Straight-chain alkane, 80 Strecker synthesis, 972 Structure, condensed, 22 electron-dot, 9 Kekule, 9 Lewis, 9 line-bond, 9 skeletal, 23... 

From eqns. 4.50 and 4.51 it can be seen that complex 1 is converted into complex 2 by a stronger base 2 or into complex 3 by a stronger acid 2 in other words, complexes 2 and 3 are much more stable than complex 1. Whereas reactions 4.48 and 4.49 are addition reactions, reactions 4.50 and 4.51 are exchange reactions often Lewis titrations must be carried out in completely inert solvents such as alkanes or benzene because of instability of the titrants and titrands in other media. Examples of potentiometric Lewis titration curves are given in Fig. 4.9 for CS2 and C0220, where one of their resonance structures can react as a Lewis acid with OH as a Lewis base ... 

---