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Chapter 2: Problem 40

Explain why the chemical formulas of ionic compounds are usually the same as their empirical formulas.

Short Answer

Expert verified
The chemical formulas of ionic compounds are the same as their empirical formulas because both represent the simplest whole-number ratio of ions or atoms in the compound that results in a charge balance.

Step by step solution

01

Understand Ionic Compounds

Firstly, it needs to be understood that ionic compounds are formed between metals and non-metals. In these compounds, electrons are transferred from the metal atoms to the non-metal atoms to achieve stable electron configurations for both. The result of these electron transfers is the formation of ions. Ions are simply atoms (or groupings of atoms) that carry a charge because they've lost or gained electrons. The cations and anions are attracted to each other due to the opposite charges they carry.
02

Understand Empirical Formulas

An empirical formula refers to the simplest whole number ratio of elements in a compound. It gives the simplest ratio of the atoms of each element involved. This doesn't tell you the actual number of atoms. Rather, it informs you about the ratio in which the atoms are present.
03

Relate Ionic Compounds and Empirical Formulas

When ionic compounds form, they do so in a way that achieves charge balance. This means the charge on the cations and anions must add up to zero within the compound. Therefore, the formula for the ionic compound is also the simplest, whole number ratio of ions that achieves this charge balance. This aligns with the concept of the empirical formula, which is the simplest, whole number ratio of atoms or ions.

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Most popular questions from this chapter

Write the names and symbols for four elements in each of these categories: (a) nonmetal, (b) metal, (c) metalloid.

For each of these species, determine the number of protons and the number of neutrons in the nucleus: \({ }_{2}^{3} \mathrm{He},{ }_{2}^{4} \mathrm{He},{ }_{12}^{24} \mathrm{Mg},{ }_{12}^{25} \mathrm{Mg},{ }_{22}^{48} \mathrm{Ti},{ }_{35}^{79} \mathrm{Br},{ }_{78}^{195} \mathrm{Pt}\)

Write the appropriate symbol for each of these isotopes: (a) \(Z=74, A=186 ;\) (b) \(Z=80 ; A=201\).

(a) Describe Rutherford's experiment and how it led to the structure of the atom. How was he able to estimate the number of protons in a nucleus from the scattering of the \(\alpha\) particles? (b) Consider the \({ }^{23} \mathrm{Na}\) atom. Given that the radius and mass of the nucleus are \(3.04 \times 10^{-15} \mathrm{~m}\) and \(3.82 \times 10^{-23} \mathrm{~g},\) respectively, calculate the density of the nucleus in \(\mathrm{g} / \mathrm{cm}^{3}\). The radius of a \({ }^{23}\) Na atom is \(186 \mathrm{pm}\). Calculate the density of the space occupied by the electrons in the sodium atom. Do your results support Rutherford's model of an atom? [The volume of a sphere is \((4 / 3) \pi r^{3},\) where \(r\) is the radius. \(]\)

In which one of these pairs do the two species resemble each other most closely in chemical properties? (a) \({ }_{1}^{1} \mathrm{H}\) and \({ }^{1} \mathrm{H}^{+},(\mathrm{b}){ }_{7}^{14} \mathrm{~N}\) and \({ }^{14} \mathrm{~N}^{3-},(\mathrm{c}){ }_{6}^{12} \mathrm{C}\) and \({ }_{6}^{13} \mathrm{C} .\)
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