Bromine Lewis structure

Write the Lewis structure for BrF.. What is the hybridization of the bromine atom in the molecule ... 

The compound l-bromo-4-nitrobenzene (p-bromonitrobenzene) can be brominated. What do you expect to be the major product and why Draw appropriate Lewis structures to support your answer. 

B As was the case in 2A, we begin by drawing a plausible Lewis structure for the cation in question. This time the Lewis structure must contain 34 valence electrons. The skeletal structure has bromine, the least electronegative element present, as the central atom. Next, we join the four terminal fluorine atoms to the central bromine atom via single covalent bonds and complete the octets for all of the fluorine atoms. Placing the last two electrons on the central bromine atom completes the diagram. 

Show Lewis structures for the simplest neutral compounds formed from these elements a) Carbon and chlorine b) Hydrogen and bromine... 

You have used Lewis structures to demonstrate how ionic and covalent bonds form between atoms. When given two elements, you determined how many atoms of each element bond together to form a compound, according to the octet rule. For example, you used the periodic table and your understanding of the octet rule to determine how calcium and bromine bond to form an ionic compound. Using a Lewis structure, you determined that calcium and bromine form a compound that contains two bromine atoms for every calcium atom, as shown in Figure 3.39. 

Making Predictions Draw the electron-dot diagrams for the elements sulfur, carbon, bromine, oxygen, and hydrogen. Using Lewis structures, predict the number of covalent bonds formed when... 

Shortcut The shortcut to drawing Lewis structures described in Section 3.3 can often be used for uncharged molecules such as CH3Br. Carbon atoms usually have four bonds and no lone pairs, hydrogen atoms always have one bond, and bromine atoms most commonly have one bond and three lone pairs. The only way to give these atoms their most common bonding patterns is with the following Lewis structure, which is the same Lewis structure we arrived at with the stepwise procedure. 

Another way of depicting this reaction is to show all the outer-shell electrons, as in the following Lewis structures (oxygen is in Group VI and bromine in Group VII of the Periodic Table)... 

The Lewis structure of BrFs, is shown next. The central bromine atom has six electron groups (one lone pair and five bonding pairs). The electron geometry, due to the six electron groups, is octahedral. Since all six positions in the octahedral geometry are equivalent, the lone pair can be situated in any one of these positions. The resulting molecular geometry is square pyramidal. 

Consider, for example, hydrogen bromide. The shared electron pair supplies the hydrogen atom with a dnet, the bromine with an octet, because the bromine carries three lone electron pairs. Conversely, in methane, the four C-H bonds satisfy the requirement of the hydrogens and, at the same time, furnish the octet for carbon. Examples of correct and incorrect Lewis structures for HBr are shown below. 

We will often show the structure of benzene as a Lewis structure with a hexagon that contains three double bonds. However, the double bonds in the Lewis structure are misleading because the chemistry of benzene does not in the least resemble a triene. For example, benzene does not react with bromine, HBr, or aqueous acid, and does not react with the powerful oxidizing agent potassium permanganate. In short, benzene is remarkably unreactive. 

The O—Br bonds of (35) (1.98 A) are also longer than the sum of the covalent radii of oxygen and bromine atoms (1.81 A). The crystal structure of (35) reveals some interaction between adjacent molecules (Figure 2). The distance between the bromine atom of one molecule and its nearest oxygen atom of a neighboring molecule is only 2.97 A, well within the sum of the van der Waals radii (3.35 A) of bromine and oxygen. This suggests a measure of Lewis acidity at the bromine of such species. 

In sharp contrast, benzene is unreactive with bromine tinder these same conditions. Under more vigorous reaction conditions (the presence of a Lewis acid catalyst, such as aluminum tribromide, and higher temperature), benzene does react with bromine However, the product results from a substitution of a Br for a H, rather than addition of Br2 to one of the double bonds. The product retains the benzene structure of three conjugated double bonds in a six-membered ring ... 

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