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Chapter 2: Q30E (page 121)

Write the molecular and empirical formulas of the following compounds:

a)

(b)

(c)

(d)

Short Answer

Expert verified

a) Molecular formula: C4H8

Empirical formula: CH2

b) Molecular formula: C4H6

Empirical formula: C2H3

c) Molecular formula: H2Si2Cl4

Empirical formula: HSiCl2

d) Molecular formula: H3PO4

Empirical formula: H3PO4

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.Molecular formula for the compounds is

a) Molecular formula: C4H8

b) Molecular formula: C4H6

c) Molecular formula: H2Si2Cl4

d) Molecular formula: H3PO4

02

– Determine the definition of empirical formula

Empirical formula indicates the types of atoms present and the simplest whole-number ratio of the number of atoms (or ions) in the compound. Empirical formula for the compound is

a) Empirical formula: CH2

b) Empirical formula: C2H3

c) Empirical formula: HSiCl2

d) Empirical formula: H3PO4

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Most popular questions from this chapter

Using the periodic table, classify each of the following elements as a metal or a nonmetal, and then further classify each as a main-group (representative) element, transition metal, or inner transition metal:

  1. Uranium
  2. Bromine
  3. Strontium
  4. Neon
  5. Gold
  6. Americium
  7. Rhodium
  8. Sulfur
  9. Carbon
  10. Potassium

Question : Name the following compounds:

  1. NaF
  2. Rb2O
  3. BCl3
  4. H2Se
  5. P4O6
  6. ICl3

A sample of magnesium is found to contain 78.70% of 24Mg atoms (mass 23.98 amu), 10.13% of 25Mg atoms (mass 24.99 amu), and 11.17% of 26Mg atoms (mass 25.98 amu). Calculate the average mass of a Mg atom.

Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the 鈥淢ix Isotopes鈥� tab, hide the 鈥淧ercent Composition鈥� and 鈥淎verage Atomic Mass鈥� 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 鈥淢ore鈥� and then move the sliders to the appropriate amounts.

(d) Reveal the 鈥淧ercent Composition鈥� and 鈥淎verage Atomic Mass鈥� boxes. How well does your mixture match withyour prediction? If necessary, adjust the isotope amounts to match your prediction.

(e) Select 鈥淣ature鈥檚鈥� 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 鈥淣ature鈥檚鈥漚mounts as closely as possible.

An ion of platinum has a mass number of 195 and contains 74 electrons. How many protons and neutrons does it contain and what is it鈥檚 charge ?
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