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Chapter 2: Problem 35

What does a chemical formula represent? What is the ratio of the atoms in the following molecular formulas? (a) NO, (b) \(\mathrm{NCl}_{3}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{4},\) (d) \(\mathrm{P}_{4} \mathrm{O}_{6}\)

Short Answer

Expert verified
A chemical formula represents the number and types of atoms present in a molecule. The ratio of atoms in the given formulas are - (a) NO - 1:1, (b) \(\mathrm{NCl}_{3}\) - 1:3, (c) \(\mathrm{N}_{2} \mathrm{O}_{4}\) - 1:2, (d) \(\mathrm{P}_{4} \mathrm{O}_{6}\) - 2:3.

Step by step solution

01

What Does a Chemical Formula Represent

A chemical formula represents the number and type of atoms present in a molecule of a substance.
02

Finding Ratio in (a) NO

The formula NO is composed of Nitrogen (N) and Oxygen (O). Since there are no numerical subscripts present, it means there's one atom each of Nitrogen and Oxygen. Therefore, the ratio of Nitrogen to Oxygen is 1:1.
03

Finding Ratio in (b) \(\mathrm{NCl}_{3}\)

In the formula \(\mathrm{NCl}_{3}\), there is one atom of Nitrogen and three atoms of Chlorine. Therefore, the ratio of Nitrogen to Chlorine is 1:3.
04

Finding Ratio in (c) \(\mathrm{N}_{2} \mathrm{O}_{4}\)

In the formula \(\mathrm{N}_{2} \mathrm{O}_{4}\), there are two atoms of Nitrogen and four atoms of Oxygen. Thus, the ratio of Nitrogen to Oxygen is 1:2.
05

Finding Ratio in (d) \(\mathrm{P}_{4} \mathrm{O}_{6}\)

In the formula \(\mathrm{P}_{4} \mathrm{O}_{6}\), there are four atoms of Phosphorus and six atoms of Oxygen. Hence, the ratio of Phosphorus to Oxygen is 2:3.

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Most popular questions from this chapter

Fluorine reacts with hydrogen \((\mathrm{H})\) and with deuterium (D) to form hydrogen fluoride (HF) and deuterium fluoride (DF) [deuterium \(\left({ }_{1}^{2} \mathrm{H}\right.\) ) is an isotope of hydrogen]. Would a given amount of fluorine react with different masses of the two hydrogen isotopes? Does this violate the law of definite proportions? Explain.

(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. \(]\)

Which of these are elements, which are molecules but not compounds, which are compounds but not molecules, and which are both compounds and molecules? (a) \(\mathrm{SO}_{2},\) (b) \(\mathrm{S}_{8},\) (c) \(\mathrm{Cs},\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5},\) (e) O, (f) \(\mathrm{O}_{2},(\mathrm{~g}) \mathrm{O}_{3},(\mathrm{~h}) \mathrm{CH}_{4},\) (i) \(\mathrm{KBr},(\mathrm{j}) \mathrm{S},(\mathrm{k}) \mathrm{P}_{4},(\mathrm{l}) \mathrm{LiF}\)

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

Identify the following as elements or compounds: \(\mathrm{NH}_{3}, \mathrm{~N}_{2}, \mathrm{~S}_{8}, \mathrm{NO}, \mathrm{CO}, \mathrm{CO}_{2}, \mathrm{H}_{2}, \mathrm{SO}_{2}\)
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