Question

Assign suitable names to the compounds (a) \(\mathrm{CS}_{2}\) (b) \(\operatorname{SiF}_{4} ;\) (c) \(\operatorname{ClF}_{5} ;\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5} ;\) (e) \(\mathrm{SF}_{6} ;\) (f) \(\mathrm{I}_{2} \mathrm{Cl}_{6}\).

Short answer

The names of the compounds are: (a) Carbon disulfide, (b) Silicon tetrafluoride, (c) Chlorine pentafluoride, (d) Dinitrogen pentoxide, (e) Sulfur hexafluoride, (f) Diiodine hexachloride.

Step-by-step solution

Identify the chemical compound \(\mathrm{CS}_{2}\)

C is Carbon and S is Sulfur, and there are two atoms of sulfur. Therefore, the compound \(\mathrm{CS}_{2}\) is Carbon disulfide.

Identify the chemical compound \(\operatorname{SiF}_{4}\)

Si is Silicon and F is Fluorine, and there are four atoms of fluorine. Therefore, the compound \(\operatorname{SiF}_{4}\) is Silicon tetrafluoride.

Identify the chemical compound \(\operatorname{ClF}_{5}\)

Cl is Chlorine and F is Fluorine, and there are five atoms of fluorine. Therefore, the compound \(\operatorname{ClF}_{5}\) is Chlorine pentafluoride.

Identify the chemical compound \(\mathrm{N}_{2}\mathrm{O}_{5}\)

N is Nitrogen and O is Oxygen. There are two atoms of nitrogen and five atoms of oxygen. Therefore, the compound \(\mathrm{N}_{2}\mathrm{O}_{5}\) is Dinitrogen pentoxide.

Identify the chemical compound \(\mathrm{SF}_{6}\)

S is Sulfur and F is Fluorine, and there are six atoms of fluorine. Therefore, the compound \(\mathrm{SF}_{6}\) is Sulfur hexafluoride.

Identify the chemical compound \(\mathrm{I}_{2}\mathrm{Cl}_{6}\)

I is Iodine, Cl is Chlorine. There are two atoms of iodine and six atoms of chlorine. Therefore, the compound \(\mathrm{I}_{2}\mathrm{Cl}_{6}\) is Diiodine hexachloride.

Key concepts

Understanding Binary Compounds

Binary compounds are made up of two different elements. They are the simplest form of compounds, consisting of exactly two types of atoms.
These compounds can either be ionic or molecular, but in the context of molecular compounds, they often involve nonmetals.
In binary compounds, the chemical formula consists of the symbols of both elements, and numbers to indicate the number of atoms of each element. Examples from our exercise include

• Carbon disulfide (\( \mathrm{CS}_{2} \))
• Silicon tetrafluoride (\( \operatorname{SiF}_{4} \))
• Nitrogen dioxide (\( \mathrm{N}_{2}\mathrm{O}_{5} \))

These examples highlight how binary compounds involve two nonmetals, adhering to specific naming conventions that provide important information about the composition of the compound.

Exploring Molecular Compounds

Molecular compounds are formed from atoms sharing electrons, usually between nonmetals. These compounds rely on covalent bonds, making them different from ionic compounds which involve electron transfer.
Molecular compounds can include binary compounds but focus more on the sharing behavior of the involved elements.
In our example list, compounds like

• Chlorine pentafluoride (\( \operatorname{ClF}_{5} \))
• Sulfur hexafluoride (\( \mathrm{SF}_{6} \))
• Dinitrogen pentoxide (\( \mathrm{N}_{2}\mathrm{O}_{5} \))

demonstrate how multiple atoms bond covalently in a molecular structure. Understanding the principles of molecular compounds allows us to predict bonding patterns and its influence on compound properties.

Decoding Systematic Naming

Systematic naming in chemistry helps identify the number and types of atoms in a compound. This system utilizes prefixes and suffixes to clearly convey the compound's composition.
For binary molecular compounds, prefixes like mono-, di-, tri-, tetra-, penta-, and hexa- are used. They indicate the number of identical atoms in the compound.
In our solved exercise:

• "Di" in Dinitrogen pentoxide (\( \mathrm{N}_{2}\mathrm{O}_{5} \)) indicates two nitrogen atoms.
• "Penta" in Pentoxide represents five oxygen atoms.
• "Hexa" in Hexafluoride in Sulfur hexafluoride (\( \mathrm{SF}_{6} \)) signifies six fluorine atoms.

This naming helps avoid confusion and maintains consistency across chemical documentation and communication.

Interpreting Chemical Formulas

Chemical formulas are a shorthand way of presenting information about the elements making up a compound. They indicate the kinds and numbers of atoms present using element symbols and numerical subscripts.
In a chemical formula, the subscript refers directly to the number of atoms immediately preceding it. For example, in \( \mathrm{I}_{2}\mathrm{Cl}_{6} \), the subscript "2" means there are two iodine atoms, and "6" means there are six chlorine atoms.
More examples include:

• "\( \mathrm{CS}_{2} \): Two atoms of sulfur, one of carbon"
• "\( \operatorname{SiF}_{4} \): Four atoms of fluorine, one of silicon"

Understanding chemical formulas helps in writing them, balancing reactions, and predicting how compounds will react with others.