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Chapter 5: Problem 2

What is a binary chemical compound? What are the two major types of binary chemical compounds? Give three examples of each type of binary compound.

Short Answer

Expert verified
A binary chemical compound is a compound formed by the combination of two different elements, which can be categorized into two major types: ionic and covalent. Ionic compounds are formed by the electrostatic force of attraction between oppositely charged ions, usually formed from a metal and a nonmetal element, such as sodium chloride (\(NaCl\)), magnesium oxide (\(MgO\)), and calcium fluoride (\(CaF_2\)). Covalent compounds are formed when atoms share electrons to achieve a stable electron configuration, usually formed between nonmetal elements, such as hydrogen chloride (\(HCl\)), water (\(H_2O\)), and carbon dioxide (\(CO_2\)).

Step by step solution

01

Definition of Binary Chemical Compound

A binary chemical compound is a compound formed by the combination of two different elements. These compounds can be categorized into two major types: ionic and covalent.
02

Types of Binary Chemical Compounds

The two major types of binary chemical compounds are: 1. Ionic Compounds: These are compounds formed by the electrostatic force of attraction between oppositely charged ions, usually formed from a metal and a nonmetal element. 2. Covalent Compounds: These are compounds formed when atoms share electrons to achieve a stable electron configuration, usually formed between nonmetal elements.
03

Ionic Binary Compounds: Examples

Here are three examples of ionic binary compounds: 1. Sodium chloride (\(NaCl\)): Sodium chloride is formed by the electrostatic force of attraction between a positively charged sodium ion (\(Na^{+}\)) and a negatively charged chloride ion (\(Cl^{-}\)). 2. Magnesium oxide (\(MgO\)): Magnesium oxide is formed by the electrostatic force of attraction between a positively charged magnesium ion (\(Mg^{2+}\)) and a negatively charged oxide ion (\(O^{2-}\)). 3. Calcium fluoride (\(CaF_2\)): Calcium fluoride is formed by the electrostatic force of attraction between a positively charged calcium ion (\(Ca^{2+}\)) and two negatively charged fluoride ions (\(F^{-}\)).
04

Covalent Binary Compounds: Examples

Here are three examples of covalent binary compounds: 1. Hydrogen chloride (\(HCl\)): Hydrogen chloride is formed when a hydrogen atom shares an electron with a chlorine atom to create a single covalent bond. 2. Water (\(H_2O\)): Water is formed when two hydrogen atoms each share an electron with an oxygen atom, creating two single covalent bonds. 3. Carbon dioxide (\(CO_2\)): Carbon dioxide is formed when a carbon atom shares two electrons with each oxygen atom, creating two double covalent bonds.

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Most popular questions from this chapter

Write the formula for each of the following chlorinecontaining ions, including the overall charge of the ion. a. chloride b. hypochlorite c. chlorate d. perchlorate

What is an oxyanion? How is a series of oxyanions named? (Give an example.)

For each of the negative ions listed in column \(1,\) use the periodic table to find in column 2 the total number of electrons the ion contains. A given answer may be used more than once. Column 1 \(\left[\begin{array}{l}1\end{array}\right] \mathrm{Se}^{2-}\) \(\left[\begin{array}{l}2\end{array}\right] S^{2-}\) \(\left[\begin{array}{l}3\end{array}\right] \mathrm{P}^{3-}\) [4] \(\mathrm{O}^{2-}\) \(\left[\begin{array}{lll}5 & \mathrm{N}^{3-}\end{array}\right.\) \(\left[\begin{array}{lll}6\end{array}\right] \mathrm{I}^{-}\) \(\left[\begin{array}{l}7\end{array}\right] \mathbf{F}^{-}\) [8] \(\mathrm{Cl}^{-}\) \(\left[\begin{array}{l}9\end{array}\right] \mathbf{B} \mathbf{r}^{-}\) [10] \(\mathrm{At}^{-}\) Column 2 [a] 18 \([b] 35\) \([\mathrm{cl}] \mathrm{s} 2\) \(\left[\begin{array}{ll}1 & 34\end{array}\right.\) [e] 36 \([\mathrm{f}] 54\) \([g] 10\) \([\mathrm{h}] 9\) \([\mathrm{i}] 53\) \([j] 86\)

Name each of the following compounds, which contain polyatomic ions. a. \(\mathrm{LiH}_{2} \mathrm{PO}_{4}\) b. \(\mathrm{Cu}(\mathrm{CN})_{2}\) c. \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) d. \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\) e. \(\mathrm{NaClO}_{2}\) f. \(\mathrm{Co}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)

Write the formula for each of the following binary compounds of nonmetallic elements. a. phosphorus triiodide b. silicon tetrachloride c. dinitrogen pentoxide d. iodine monobromide e. diboron trioxide f. nitrogen trichloride g. carbon monoxide
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