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Chapter 2: Q28 E (page 128)

Explain why the symbol for element sulfur and the formula for a molecule of sulfur differ.

Short Answer

Expert verified

The symbol for an element sulfur and the formula for a molecule of sulfur differ because sulfur molecules have 8 sulfur atoms. Therefore, it has different symbols. Although many elements consist of discrete, individual atoms, some exist as molecules made up of two or more atoms of the elements chemically bonded together.

Step by step solution

01

- Determine the definition of molecular formula

A molecular formula is a representation of a molecule that uses chemical symbols to indicate the type of atoms. It is also used as abbreviations for the names of compounds.

02

- Describe how symbol for S atom and S molecules are different.

The sulfur molecule formula is S8. The subscript 8 denotes the number of atoms bounded to form a molecule.

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Most popular questions from this chapter

For each of the following compounds, state whether it is ionic or covalent, and if it is ionic, write the symbols for the ions involved:

  1. \(KCl{O_4}\)
  2. \(Mg{\left( {{C_2}{H_3}{O_2}} \right)_2}\)
  3. \({H_2}S\)
  4. \(A{g_2}S\)
  5. \({N_2}C{l_4}\)
  6. \(Co{\left( {N{O_3}} \right)_2}\)

Give the group name for each of the following elements: (a) krypton (b) selenium (c) barium (d) lithium

Question: Write the formulas of the following compounds:

(a) rubidium bromide

(b) magnesium selenide

(c) sodium oxide

(d) calcium chloride

(e) hydrogen fluoride

(f) gallium phosphide

(g) aluminum bromide

(h) ammonium sulfate

Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the “Mix Isotopes” tab, hide the “Percent Composition” and “Average Atomic Mass” boxes, and then select the element boron.

(a) Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts.

(b) Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice.

(c) Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes fromtheir bins or click on “More” and then move the sliders to the appropriate amounts.

(d) Reveal the “Percent Composition” and “Average Atomic Mass” boxes. How well does your mixture match withyour prediction? If necessary, adjust the isotope amounts to match your prediction.

(e) Select “Nature’s” mix of isotopes and compare it to your prediction. How well does your prediction comparewith the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match “Nature’s”amounts as closely as possible.

Write the empirical formula for the following compounds:
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