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Chapter 7: Q10E (page 390)

From the labels of several commercial products, prepare a list of six ionic compounds in the products. For each compound, write the formula. (You may need to look up some formulas in a suitable reference.)

Short Answer

Expert verified

The six iconic compounds in the products with their formula are:

Calcium carbonate (Antacid) -\({\rm{CaC}}{{\rm{O}}_{\rm{3}}}\)

Sodium Chloride (Salt) - \({\rm{NaCl}}\)

Sodium hydrogen carbonate (Baking soda) - \({\rm{NaHC}}{{\rm{O}}_{\rm{3}}}\)

Sodium hydroxide - \({\rm{NaOH}}\)

Potassium chloride (Alternative of salt) - \({\rm{KCl}}\)

Tin fluoride (Toothpaste) - \({\rm{Sn}}{{\rm{F}}_{\rm{2}}}\)

Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Explanation

Calcium carbonate, sometimes known as antacid, has the chemical formula \({\rm{CaC}}{{\rm{O}}_{\rm{3}}}\).

Sodium chloride is also known as salt and has the chemical formula\({\rm{NaCl}}\).

The chemical formula of sodium hydrogen carbonate, often known as baking soda, is\({\rm{NaHC}}{{\rm{O}}_{\rm{3}}}\).

The chemical formula for sodium hydroxide is\({\rm{NaOH}}\).

Potassium chloride is a salt alternative with the chemical formula\({\rm{KCl}}\).

\({\rm{Sn}}{{\rm{F}}_{\rm{2}}}\)is the chemical formula for tin fluoride, which is often used in toothpaste.

Therefore, six compounds in the products with their formula are:

Calcium carbonate (Antacid) -\({\rm{CaC}}{{\rm{O}}_{\rm{3}}}\)

Sodium Chloride (Salt) - \({\rm{NaCl}}\)

Sodium hydrogen carbonate (Baking soda) - \({\rm{NaHC}}{{\rm{O}}_{\rm{3}}}\)

Sodium hydroxide - \({\rm{NaOH}}\)

Potassium chloride (Alternative of salt) - \({\rm{KCl}}\)

Tin fluoride (Toothpaste) - \({\rm{Sn}}{{\rm{F}}_{\rm{2}}}\)

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Most popular questions from this chapter

Write out the full electron configuration for each of the following atoms and for the monatomic ion found in binary ionic compounds containing the element: (a) \({\rm{Al}}\) (b) \({\rm{Br}}\) (c) \({\rm{Sr}}\) (d) \({\rm{Li}}\) (e) \({\rm{As}}\) (f) \({\rm{S}}\) .

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\) and \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) have similar radii; \({{\rm{O}}^{{\rm{2 - }}}}\) and \({{\rm{F}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({\rm{MgO}}\) or \({\rm{MgSe}}\)

(b) \({\rm{LiF}}\) or \({\rm{MgO}}\)

(c) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{O}}\) or \({\rm{LiCl}}\)

(d) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{Se}}\) or \({\rm{MgO}}\)

Explain the difference between electron-pair geometry and molecular structure.

Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.

(a) \(C{O_2}\)

(b) \(CO\)
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