Covalent compounds chlorine

Both boron and aluminium chlorides can be prepared by the direct combination of the elements. Boron trichloride can also be prepared by passing chlorine gas over a strongly heated mixture of boron trioxide and carbon. Like boron trifluoride, this is a covalent compound and a gas at ordinary temperature and pressure (boiling point 285 K). It reacts vigorously with water, the mechanism probably involving initial co-ordination of a water molecule (p, 152). and hydrochloric acid is obtained ... 

Many of the reactions of halogens can be considered as either oxidation or displacement reactions the redox potentials (Table 11.2) give a clear indication of their relative oxidising power in aqueous solution. Fluorine, chlorine and bromine have the ability to displace hydrogen from hydrocarbons, but in addition each halogen is able to displace other elements which are less electronegative than itself. Thus fluorine can displace all the other halogens from both ionic and covalent compounds, for example... 

Phosphorus forms two covalent compounds with chlorine, PCI, and PCI,. Discuss these compounds in terms of the octet rule. 

Elementary fluorine or chlorine may act drastically on a number of covalent compounds, forming products in which the only bonds remaining are eiement-to-halogen bonds. Such reactions are called halogenolyses the chlorinolysis of carbon diselenide and the fluorinolysis of ethane are typical ... 

This difference ist due mainly to experimental difficulties nitrogen resonances fall within the low-frequency range, 1 to 5 MHz, while most of the chlorine resonances, especially in covalent compounds, are located in the 30-40 MHz band.Thus the Boltzmann factor hv/kT for nitrogen is seven times smaller and the line intensity is accordingly reduced, Moreover, the splitting of the nitrogen resonance line by the asymmetry of the electric field gradient tensor reduces the line intensity by a factor of more than 2. 

For example, hydrogen chloride, also known as hydrochloric acid, has a low melting point and a low boiling point. (It is a gas at room temperature.) These properties might lead you to believe that hydrogen chloride is a covalent compound. Hydrogen chloride, however, is extremely soluble in water, and the water solution conducts electricity. These properties are characteristic of an ionic compound. Is there a clear, theoretical way to decide whether the bond between hydrogen and chlorine is ionic or covalent The answer lies in a periodic trend. 

Finally, consider hydrogen chloride, or hydrochloric acid. Hydrogen has an electronegativity of 2.20, and chlorine has an electronegativity of 3.16. Therefore, the electronegativity difference for the chemical bond in hydrochloric acid, HC1, is 0.96. Hydrogen chloride is a gas at room temperature, but its water solution conducts electricity. Is hydrogen chloride a covalent compound or an ionic compound Its AEN can help you decide, as you will see below. 

The main uses of chlorine are the following (l)the production of chloro-organic compounds, snch as vinyl chloride and ethylene dichloride for the plastics indnstry, as solvents, refrigerants, insecticides, and dyes (abont 70%) (2) as a bleaching agent of paper, pnlp, and textiles, and the disinfection of water snpplies (abont 20%) and (3) for the production of a large variety of inorganic chemicals, particularly covalent compounds. 

Pure perchloric acid is a colorless, hygroscopic, and shock-sensitive liquid. Although the anhydrous acid is a covalent compound, HOCIO3, the hydrates are considered to be ionic [H(H20) ]+ [C104] (n = 1, 2, and 3). Hydration does not increase the coordination number of the chlorine atom above four, which is in contrast to a periodic acid having a coordination number of six (discussed later). 

To do this we must draw the salt as a covalent compound or transfer one electron fr> chloride ion to the diazonium ion. The other product would be a chlorine radical. Addition alkene gives the more stable radical, which abstracts chlorine from the diazocompound and. the chain going. 

The Lewis model for covalent bonding starts with the recognition that electrons are not transferred from one atom to another in a nonionic compound, but rather are shared between atoms to form covalent bonds. Hydrogen and chlorine combine, for example, to form the covalent compound hydrogen chloride. This result can be indicated with a Lewis diagram for the molecule of the product, in which the valence electrons from each atom are redistributed so that one electron from the hydrogen atom and one from the chlorine atom are now shared by the two atoms. The two dots that represent this electron pair are placed between the symbols for the two elements ... 

The unshared electron pairs around the chlorine atom in the Lewis diagram are called lone pairs, and they make no contribution to the bond between the atoms. Lewis diagrams of some simple covalent compounds are... 

The oxidation number of the elements in a covalent compound can be deduced by considering the shared electrons to belong exclusively to the more electronegative atom (see Box 3.2). Where both atoms have the same electronegativity the electrons are considered to be shared equally. Thus the oxidation numbers of carbon and chloride in CCI4 are +4 and -1 respectively and the oxidation number of chlorine in Cl2 is 0. 

What are the formulas of the covalent compounds involving (a) one carbon atom and as much chlorine as needed, (b) one silicon atom and chlorine, and (c) one sulfur atom and chlorine ... 

In Group 7A(17), fluorine and chlorine have the condensed electron configuration [noble gas] ns np, as do the other halogens (Br, I, At). Little is known about rare, radioactive astatine (At), but all the others are reactive nonmetals that occur as diatomic molecules, X2 (where X represents the halogen). All form ionic compounds with metals (KX, MgX2), covalent compounds with hydrogen (HX) that yield acidic solutions in water, and covalent compounds with carbon (CX4). 

A metal and a nonmetal—elements from opposite sides of the periodic table— have a relatively large AEN and typically interact by electron transfer to form an ionic compound. Two nonmetals—elements from the same side of the table— have a small AEN and interact by electron sharing to form a covalent compound. When we combine the nonmetal chlorine with each of the other elements in Period 3, starting with sodium, we should observe a steady decrease in AEN and a gradation in bond type from ionic through polar covalent to nonpolar covalent. 

Halogens form a variety of covalent compounds with each other. For example, chlorine and fluorine form the compounds GIF, CIF3, and CIF5. Predict the molecular structure (including bond angles) for each of these three compounds. Would you expect FCI3 to be a stable compound Explain. 

For convenience, shared electrons in covalent compounds are assigned to the element having the greater electronegativity. For example, the oxidation number for phosphorus in PCI3 is -1-3 (chlorine is —1), since phosphorus is less electronegative than chlorine. 

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