![]() The atom which loses electrons becomes a positively charged ion or cation whereas the atom which gains electrons becomes a negatively charged ion or anion.Įlements with extremely high ionization energies can’t lose electrons, and those with extremely low electron affinity can’t accept them. First, I will explain the types of bonds.Īn ionic bond formation takes place due to the permanent transfer of valence (outermost) electrons of one atom to another atom.Įlectrostatic attraction between positively and negatively charged ions causes these bonds to form. Now let me discuss the covalent nature of CCl4 in detail.īefore we dig into the details of covalent bonds in methane, let’s start from the basics. This makes CCl4 a covalent compound.Īs chlorine and carbon atoms share their outer electrons, chlorine attains the electronic configuration of argon and carbon attains that of neon.Īs a result, while forming covalent bonds both the chlorine and carbon atoms essentially have outer shells with 8 electrons. The bond so formed between carbon and chlorine is a covalent bond since it is formed by sharing electrons. ![]() Since each chlorine atom is one electron short of an octet configuration (complete shell) and carbon is 4 electrons short of a complete valence shell of eight, four chlorine atoms share electrons with the four valence electrons of carbon, resulting in full outer shells for all five atoms. Is CCl4 (carbon tetrachloride) a covalent compound? In the next part, we’ll find out.įour chlorine atoms and one carbon atom make up a CCl4 molecule. The following is the reaction:ĬH4 (Methane) + 4Cl2 (chlorine) -> CCl4 + 4 HCl (acid) These days, tetrachloromethane is manufactured by treating methane with chlorine. Chloroform and chlorine were combined to make it. Henri Victor Regnault, a French chemist, first produced tetrachloromethane in the year 1839. It was a popular solvent in organic chemistry, but, it is rarely used today because of its adverse health effects. Its boiling point is 76 degrees Celcius.ĬCl4 is a poisonous gas that depletes the ozone layer and is often known as a greenhouse gas. It has a melting point of about -23 degrees Celcius. At room temperature, CCl4 exists as a liquid. When reading about smog production or ozone depletion, consider the bond strengths of the chemicals involved in this environmental problems.Carbon tetrachloride (CCl4), is a colorless liquid with a sweet odor. For example, the triple bond found in carbon monoxide is harder to break than one of the double bonds found in carbon dioxide. For this reason, it is more difficult to break or cleave a multiple bond than it would be a single bond or a bond of a lower order (when comparing the same connected atoms). Multiple bonds involve more that one type of connection. If an octet can be achieved with a single bond, do not incorporate multiple bonds into the structure. Let's look at a few molecules that utilize multiple bonds:Ītoms that could employ multiple bonds would be oxygen, nitrogen, sulfur, phosphorus, and carbon. Although it is mathematically feasible, halogens will not use multiple bonds to become stable either. Please note the rules above on which atoms will never achieve octets (hydrogen and boron). ![]() If a single bond does not work, then you may incorporate a multiple bond. In covalent bonding, using double (four total electrons) or triple (six total electrons) is an option in order to achieve a stable octet. In our class, we do not use multiple bonds for halogens.
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