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Chapter 6: Problem 121

Classify each of the following as ionic or molecular, and give its name: (6.3,6.5) a. \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) b. \(\mathrm{NH}_{3}\) c. \(\mathrm{AlBr}_{3}\) d. \(\mathrm{CS}_{2}\) e. BN f. \(\mathrm{Ca}_{3} \mathrm{P}_{2}\)

Short Answer

Expert verified
a. Ionic, Sodium Carbonate; b. Molecular, Ammonia; c. Ionic, Aluminum Bromide; d. Molecular, Carbon Disulfide; e. Molecular, Boron Nitride; f. Ionic, Calcium Phosphide.

Step by step solution

01

- Identify Ionic or Molecular

Determine if each compound listed is ionic or molecular. Ionic compounds generally consist of metals combined with non-metals, while molecular (covalent) compounds consist of non-metals only.
02

- Classify and Name Compound a: \(\mathrm{Na}_{2} \mathrm{CO}_{3}\)

Compound \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is ionic because it is composed of a metal (sodium) and a polyatomic ion (carbonate). The name is Sodium Carbonate.
03

- Classify and Name Compound b: \(\mathrm{NH}_{3}\)

Compound \(\mathrm{NH}_{3}\) is molecular because it consists of only non-metals (nitrogen and hydrogen). The name is Ammonia.
04

- Classify and Name Compound c: \(\mathrm{AlBr}_{3}\)

Compound \(\mathrm{AlBr}_{3}\) is ionic because it is composed of a metal (aluminum) and a non-metal (bromine). The name is Aluminum Bromide.
05

- Classify and Name Compound d: \(\mathrm{CS}_{2}\)

Compound \(\mathrm{CS}_{2}\) is molecular because it consists of only non-metals (carbon and sulfur). The name is Carbon Disulfide.
06

- Classify and Name Compound e: BN

Compound BN is molecular because it consists of only non-metals (boron and nitrogen). The name is Boron Nitride.
07

- Classify and Name Compound f: \(\mathrm{Ca}_{3} \mathrm{P}_{2}\)

Compound \(\mathrm{Ca}_{3} \mathrm{P}_{2}\) is ionic because it is composed of a metal (calcium) and a non-metal (phosphorus). The name is Calcium Phosphide.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Ionic Compounds
Ionic compounds are formed when metals combine with non-metals. In an ionic bond, one atom donates an electron to another, creating charged ions that attract each other. Here鈥檚 how to recognize and name them:

Ionic compounds often consist of:
  • A positive ion (cation), usually a metal.
  • A negative ion (anion), which can be a non-metal or a polyatomic ion.
For example, in \(\text{Na}_2\text{CO}_3\), sodium (\(\text{Na}\)) is a metal, and carbonate (\(\text{CO}_3\)) is a polyatomic ion. This makes sodium carbonate an ionic compound.

Another example is \(\text{Ca}_3\text{P}_2\), which combines calcium (metal) and phosphorus (non-metal) to form calcium phosphide (ionic).

To name ionic compounds:
  • Name the metal (cation) first.
  • Then name the non-metal (anion), changing its ending to 鈥�-ide,鈥� or name the polyatomic ion directly.
This makes \(\text{AlBr}_3\) aluminum bromide, where aluminum (metal) bonds with bromine (non-metal).
Molecular Compounds
Molecular compounds form when non-metals share electrons through covalent bonds. Here鈥檚 how to recognize and name them:

Molecular compounds generally consist of:
  • Non-metal elements only.
For example, \(\text{NH}_3\) (ammonia) consists solely of nitrogen and hydrogen, both non-metals. Likewise, \(\text{CS}_2\) (carbon disulfide) contains only carbon and sulfur, which are also non-metals.

To name molecular compounds:
  • Use prefixes to indicate the number of each type of atom (mono-, di-, tri-, etc.), except the prefix 鈥渕ono-鈥� is often omitted for the first element.
  • Name the first element as it appears on the periodic table.
  • Name the second element, changing its ending to 鈥�-ide.鈥�
For example, in \(\text{BN}\), boron (non-metal) and nitrogen (non-metal) form boron nitride. The absence of metals indicates it's molecular.

When naming, 鈥渄initrogen tetroxide鈥� means two nitrogen atoms and four oxygen atoms. Precision is key in molecular naming.
Chemical Nomenclature
Chemical nomenclature is the systemic method of naming chemical substances. Accurate naming is vital for clear communication. Here鈥檚 how to apply it:

The rules differ for ionic and molecular compounds:
  • For ionic compounds, name the cation first, followed by the anion. Adjust the anion鈥檚 name to end in 鈥�-ide,鈥� unless involving polyatomic ions (e.g., sulfate, phosphate).
  • For molecular compounds, use numerical prefixes to indicate the quantity of each element. The second element鈥檚 name ends in 鈥�-ide.鈥�
Contextual Example:

For \(\text{Na}_2\text{CO}_3\): 鈥淪odium Carbonate.鈥� Sodium is the metal cation, and carbonate is the polyatomic anion.

For \(\text{NH}_3\): 鈥淎mmonia.鈥� No prefix for a single nitrogen; three hydrogens do not require prefixes.

Leveraging nomenclature rules helps in easily identifying and naming compounds accurately in chemistry. This systematic approach is crucial for clarity in scientific discourse.

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Most popular questions from this chapter

State the number of protons and electrons in each of the following ions: a. \(\mathrm{P}^{3-},\) needed for bones and teeth b. \(\mathrm{F}^{-},\) used to strengthen tooth enamel c. \(\mathrm{Mg}^{2+}\), needed for bones and teeth d. \(\mathrm{Ca}^{2+}\), needed for bones and teeth

Write the correct formula for the following ionic compounds: a. aluminum chlorate b. ammonium oxide c. magnesium bicarbonate d. sodium nitrite e. copper(I) sulfate

Classify each of the following as ionic or molecular, and name each: (6.2,6.3,6.4,6.5) a. \(\mathrm{FePO}_{3}\) b. \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) c. \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) d. \(\mathrm{PCl}_{3}\) e. \(\mathrm{Al}\left(\mathrm{ClO}_{2}\right)_{3}\) f. \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) g. \(\mathrm{MgCO}_{3}\)

Name each of the following molecular compounds: (6.5) a. \(\mathrm{B}_{2} \mathrm{H}_{6}\) b. \(\mathrm{ClF}_{3}\) c. \(\mathrm{NO}_{2}\) d. \(\mathrm{CCl}_{4}\) e. \(\mathrm{PCl}_{3}\) f. \(\mathrm{N}_{2} \mathrm{O}_{5}\)

Write the formula for each of the following ionic compounds: a. nickel(III) oxide b. barium fluoride c. tin(IV) chloride d. silver sulfide e. bismuth(V) chloride f. potassium nitride
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