# 4.2: Covalent Compounds: Formulas and Names

Skills to Develop

• Determine the chemical formula of a simple covalent compound from its name.
• Determine the name of a simple covalent compound from its chemical formula.

What elements make covalent bonds? Covalent bonds form when two or more nonmetals combine. For example, both hydrogen and oxygen are nonmetals, and when they combine to make water, they do so by forming covalent bonds. Nonmetal atoms in polyatomic ions are joined by covalent bonds, but the ion as a whole participates in ionic bonding. For example, ammonium chloride has ionic bonds between a polyatomic ion, $$NH_4^+$$, and $$Cl^−$$ ions, but within the ammonium ion, the nitrogen and hydrogen atoms are connected by covalent bonds:

Example $$\PageIndex{1}$$

Is each compound formed from ionic bonds, covalent bonds, or both?

1. $$Na_2O$$
2. $$Na_3PO_4$$
3. $$N_2O_4$$

SOLUTION

1. The elements in $$Na_2O$$ are a metal and a nonmetal, which form ionic bonds.
2. Because sodium is a metal and we recognize the formula for the phosphate ion (see Table 3.1), we know that this compound is ionic. However, polyatomic ions are held together by covalent bonds, so this compound contains both ionic and covalent bonds.
3. The elements in $$N_2O_4$$ are both nonmetals, rather than a metal and a nonmetal. Therefore, the atoms form covalent bonds.

Exercise $$\PageIndex{1}$$

Is each compound are formed from ionic bonds, covalent bonds, or both?

1. $$Ba(OH)_2$$
2. $$F_2$$
3. $$PCl_3$$

The chemical formulas for covalent compounds are referred to as molecular formulas because these compounds exist as separate, discrete molecules. Typically, a molecular formula begins with the nonmetal that is closest to the lower left corner of the periodic table, except that hydrogen is almost never written first (H2O is the prominent exception). Then the other nonmetal symbols are listed. Numerical subscripts are used if there is more than one of a particular atom. For example, we have already seen CH4, the molecular formula for methane.

Naming binary (two-element) covalent compounds is similar to naming simple ionic compounds. The first element in the formula is simply listed using the name of the element. The second element is named by taking the stem of the element name and adding the suffix -ide. A system of numerical prefixes is used to specify the number of atoms in a molecule. Table $$\PageIndex{1}$$ lists these numerical prefixes. Normally, no prefix is added to the first element’s name if there is only one atom of the first element in a molecule. If the second element is oxygen, the trailing vowel is usually omitted from the end of a polysyllabic prefix but not a monosyllabic one (that is, we would say “monoxide” rather than “monooxide” and “trioxide” rather than “troxide”).

Table $$\PageIndex{1}$$ Numerical Prefixes for Naming Binary Covalent Compounds
Number of Atoms in Compound Prefix on the Name of the Element
1 mono-*
2 di-
3 tri-
4 tetra-
5 penta-
6 hexa-
7 hepta-
8 octa-
9 nona-
10 deca-
*This prefix is not used for the first element’s name.

Let us practice by naming the compound whose molecular formula is CCl4. The name begins with the name of the first element—carbon. The second element, chlorine, becomes chloride, and we attach the correct numerical prefix (“tetra-”) to indicate that the molecule contains four chlorine atoms. Putting these pieces together gives the name carbon tetrachloride for this compound.

Example $$\PageIndex{2}$$

Write the molecular formula for each compound.

1. chlorine trifluoride
2. phosphorus pentachloride
3. sulfur dioxide
4. dinitrogen pentoxide

SOLUTION

If there is no numerical prefix on the first element’s name, we can assume that there is only one atom of that element in a molecule.

1. ClF3
2. PCl5
3. SO2
4. N2O5 (The di- prefix on nitrogen indicates that two nitrogen atoms are present.)

Exercise $$\PageIndex{2}$$

Write the molecular formula for each compound.

1. nitrogen dioxide
2. dioxygen difluoride
3. sulfur hexafluoride
4. selenium monoxide

Note

Because it is so unreactive, sulfur hexafluoride is used as a spark suppressant in electrical devices such as transformers.

Example $$\PageIndex{3}$$

Write the name for each compound.

1. BrF5
2. S2F2
3. CO

SOLUTION

1. bromine pentafluoride
2. disulfur difluoride
3. carbon monoxide

Exercise $$\PageIndex{3}$$

Write the name for each compound.

1. CF4
2. SeCl2
3. SO3

For some simple covalent compounds, we use common names rather than systematic names. We have already encountered these compounds, but we list them here explicitly:

• H2O: water
• NH3: ammonia
• CH4: methane

Methane is the simplest organic compound. Organic compounds are compounds with carbon atoms and are named by a separate nomenclature system that we will introduce in Section 4.6 "Introduction to Organic Chemistry".

## Concept Review Exercises

1. How do you recognize a covalent compound?
2. What are the rules for writing the molecular formula of a simple covalent compound?
3. What are the rules for naming a simple covalent compound?

1. A covalent compound is usually composed of two or more nonmetal elements.
2. It is just like an ionic compound except that the element further down and to the left on the periodic table is listed first and is named with the element name.
3. Name the first element first and then the second element by using the stem of the element name plus the suffix -ide. Use numerical prefixes if there is more than one atom of the first element; always use numerical prefixes for the number of atoms of the second element.

## Key Takeaways

• The chemical formula of a simple covalent compound can be determined from its name.
• The name of a simple covalent compound can be determined from its chemical formula.

## Exercises

1. Identify whether each compound has covalent bonds.

1. NaI
2. Na2CO3
3. N2O
4. SiO2
2. Identify whether each compound has covalent bonds.

1. C2H6
2. C6H5Cl
3. KC2H3O2
4. Ca(OH)2
3. Identify whether each compound has ionic bonds, covalent bonds, or both.

1. Na3PO4
2. K2O
3. COCl2
4. CoCl2
4. Identify whether each compound has ionic bonds, covalent bonds, or both.

1. FeCl3
2. Fe(NO3)3
3. (NH2)2CO
4. SO3
5. Which is the correct molecular formula—H4Si or SiH4? Explain.

6. Which is the correct molecular formula—SF6 or F6S? Explain.

7. Write the name for each covalent compound.

1. SiF4
2. NO2
3. CS2
4. P2O5
8. Write the name for each covalent compound.

1. CO
2. S2O3
3. BF3
4. GeS2
9. Write the formula for each covalent compound.

1. iodine trichloride
2. disulfur dibromide
3. arsenic trioxide
4. xenon hexafluoride
10. Write the formula for each covalent compound.

1. boron trichloride
2. carbon dioxide
3. tetraphosphorus decoxide
4. germanium dichloride
11. Write two covalent compounds that have common rather than systematic names.

12. What is the name of the simplest organic compound? What would its name be if it followed the nomenclature for binary covalent compounds?

1. no
2. yes
3. yes
4. yes
1. both
2. ionic
3. covalent
4. ionic
1. SiH4; except for water, hydrogen is almost never listed first in a covalent compound.

1. silicon tetrafluoride
2. nitrogen dioxide
3. carbon disulfide
4. diphosphorus pentoxide
1. ICl3
2. S2Br2
3. AsO3
4. XeF6
1. H2O and NH3 (water and ammonia) (answers will vary)

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