Which of the following characterizes an ionic bond? *The electrons in the bond are shared between two atoms. *The electrons in the bond are shared between two ions. *The bond results from the attractive forces of two similar charges. *The bond results from the attractive forces of two opposite charges.
Hey! The answer is: “The bond results from the attractive forces of two opposite charges”. They occur between METALS and NON-METALS. E.g. Sodium Chloride, NaCl. The metal sodium, Na has 11 electrons in its elemental form, and so to form a stable compound, or ionic lattice, it will donate 1 e- (electron) to a non-metal, (giving it the same electronic configuration as the stable noble gas, Ne). A common non-metal recipient is Cl (Chlorine), which has 17 electrons (when gaining from Na, will have 18e- and therefore have the same stable configuration as Ar, another noble gas.) Once ‘donating’ and ‘receiving’ has taken place, and under the right conditions, an ionic lattice will result, Na+Cl-. For every Na+ there is one Cl-, and within the lattice itself, for every Na+, 4 Cl- will be attracted to it, and for every Cl-, 4 neighboring Na+ ions will be attracted to it. Note that the metal and non-metal are now ions (have a charge), therefore the term ionic bond is used (although technically ionic doesn’t exist where covalent character can be applied due to difference in polar properties). Furthermore, each ‘donated’ electron isn’t technically ‘received’ either, but forms part of a “sea of delocalized electrons”. Effectively, this acts as a glue between the two ions that were once elements with mutually convenient electronic configurations to form a new compound. NaCl is also referred to as regular table salt, and the ions themselves also play a major role in the nervous system, again, due to their useful ability to form ions in aqueous solution.
What Characterizes An Ionic Bond
The bond results from the attractive forces of two opposite charges.
*The bond results from the attractive forces of two similar
It is the last one.
the last statement is true; the rest are false