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Chapter 2: Discussion Questions (page 46)

Q.15. The formula of water is H2O. Which of the following is indicated by this formula? Explain your answer


a. the mass of hydrogen is twice that of oxygen in each molecule
b. there are two hydrogen atoms and one oxygen atom per water molecule
c. the mass of oxygen is twice that of hydrogen in each molecule
d. there are two oxygen atoms and one hydrogen atom per water molecule

Short Answer

Expert verified

Answer

There are two hydrogen atoms and one oxygen atom per water molecule. Option B is correct.

Step by step solution

01

Step-by-Step SolutionStep 1: Chemical Formula

The chemical formula of a compound shows the constituent atoms of each element in it. For example, the formula of carbon dioxide is CO2 . It is the short form representation of this molecule.

02

Water

The ratio of hydrogen atoms and oxygen atoms makes a water molecule. So, the chemical formula of it becomes .

Hence, among the given options, the correct answer is option c; that is, there are two hydrogen atoms and one oxygen atom per water molecule.

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Most popular questions from this chapter

Q.22 The three most stable oxides of carbon are carbon monoxide (CO), carbon dioxide (CO2 ), and carbon suboxide ( C3O2). The molecules can be represented as:

Explain how thesemolecules illustrate the law of multiple proportions.

What number of protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, what number of electrons are present?

a.U92235
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Q.3.How would you go about finding the number of “chalk molecules” it takes to write your name on the board? Explain what you would need to do and provide a sample calculation.

Compare and contrast the MO model with the L.E model. When is each useful?

You take three compounds, each consisting of two elements (X, Y, and /or Z) and decompose them to their respective elements. To determine the relative masses of X, Y, and Z, you collect and weigh the elements, obtaining the following data:

X and Y for (Elements in compound)

X=0.4g,Y=4.2g (Masses of Elements)

Y and Z for (Elements in compound)

Y=1.4g,Z=1.0g(Masses of Elements)

X and Y for (Elements in compound)

X=2.00g,Y=7.00g (Masses of Elements)

a. What are the assumptions needed to solve this problem?

b. What are the relative masses of X, Y, and Z?

c. What are the chemical formulas of the three compounds?

d. If you decompose 21g of compound XY, how much of each element is present?
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