A solid compound, which has high melting and boiling points, is highly soluble in water but shows poor solubility in non-polar solvents. This compound is formed by the transfer of electrons between the constituent atoms. Which of the following characteristic will be shown by this compound?
a. The compound will conduct electricity in the solid state. b. The compound will conduct electricity in the aqueous state. c. The compound will not conduct electricity in the molten form. d. The compound will conduct electricity due to the presence of free electrons.
Answers
Answer:
Two Classes of Compounds
Compounds are defined as substances containing two or more different chemical elements. They have distinct chemical structures characterized by a fixed ratio of atoms held together by chemical bonds. Here, we discuss two classes of compounds based on the bond type that holds the atoms together: ionic and covalent.
Covalent Compounds
Covalent bonds are characterized by the sharing of electrons between two or more atoms. These bonds mostly occur between nonmetals or between two of the same (or similar) elements. Two atoms with similar electronegativity will not exchange an electron from their outermost shell; the atoms instead share electrons so that their valence electron shell is filled.
Examples of compounds that contain only covalent bonds are methane (CH4), carbon monoxide (CO), and iodine monobromide (IBr).
Covalent bonding between hydrogen atoms Since each hydrogen atom has one electron, they are able to fill their outermost shells by sharing a pair of electrons through a covalent bond.
Ionic Compounds
Ionic bonding occurs when there is a large difference in electronegativity between two atoms. This large difference leads to the loss of an electron from the less electronegative atom and the gain of that electron by the more electronegative atom, resulting in two ions. These oppositely charged ions feel an attraction to each other, and this electrostatic attraction constitutes an ionic bond.
Ionic bonding occurs between a nonmetal, which acts as an electron acceptor, and a metal, which acts as an electron donor. Metals have few valence electrons, whereas nonmetals have closer to eight valence electrons; to easily satisfy the octet rule, the nonmetal will accept an electron donated by the metal. More than one electron can be donated and received in an ionic bond.
Some examples of compounds with ionic bonding include NaCl, KI, MgCl2.
Explanation:
b. The compound will conduct electricity in the aqueous state.
- The given properties are of Ionic compounds.
- Ionic compounds will conduct electricity in the aqueous state because their ions are free to travel from one location to another. After getting dissolved in water the strong electrostatic forces between ions weaken and they flow freely.
- Since the ions in ionic compounds are maintained in fixed places and cannot move, they cannot conduct electricity when solid.