For each of the following pairs of elements, state whether the binary compound they form is likely to be ionic or covalent. Write the empirical formula and name of the compound: (a) \(\mathrm{B}\) and \(\mathrm{F}\), (b) \(\mathrm{K}\) and \(\mathrm{Br}\).

Short Answer

Expert verified
(a) \(\mathrm{B}\) and \(\mathrm{F}\) form a covalent compound named boron trifluoride (\(\mathrm{BF}_3\)). (b) \(\mathrm{K}\) and \(\mathrm{Br}\) form an ionic compound named potassium bromide (\(\mathrm{KBr}\)).

Step by step solution

01

Determine the type of bond

To determine the type of bond which will be formed by the two elements, look at their positions in the Periodic Table. Non-metals usually make covalent bonds with each other, while metals usually make ionic bonds with non-metals. (a) Both \(\mathrm{B}\) and \(\mathrm{F}\) are non-metals, hence they would form a covalent bond. (b) \(\mathrm{K}\) is a metal and \(\mathrm{Br}\) is a non-metal, hence they would form an ionic bond.
02

Write the empirical formulas

For covalently bonded elements, the empirical formula usually mirrors the molecule's structure. For ionic compounds, the empirical formula represents the smallest whole number ratio of ions necessary for electric charge balance. (a) \(\mathrm{BF}_3\) - this represents one boron atom sharing electrons with three fluorine atoms. (b) \(\mathrm{KBr}\) - one potassium ion and one bromide ion balance each other out electrically.
03

Name the compounds

The name of a covalent compound is typically composed of the names of the two atoms, with prefixes indicating the number of atoms if greater than one. For ionic compounds, the name of the positively charged ion comes first followed by the name of the negatively charged ion. (a) \(\mathrm{BF}_3\) - Boron trifluoride. (b) \(\mathrm{KBr}\) - Potassium bromide.

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