Chapter 18: Problem 49
Arrange the following in order of increasing electronegativity: \(\mathbf{F} ; \mathrm{Cl} ; \mathrm{O} ;\) and \(\mathrm{S}.\)
Short Answer
Expert verified
S < Cl < O < F
Step by step solution
01
Understand Electronegativity
Electronegativity is the measure of the tendency of an atom to attract a bonding pair of electrons. Generally, electronegativity increases across a period from left to right in the periodic table and decreases down a given group. The elements given belong to the second and third periods of the periodic table.
02
Locate Elements in the Periodic Table
Find the position of F (Fluorine), Cl (Chlorine), O (Oxygen), and S (Sulfur) in the periodic table to determine their relative electronegativities based on their positions and trends.
03
Apply Periodic Trends
Since F and Cl are in the same group with F being above Cl, F is more electronegative. O and S are also in the same group with O being above S, hence O is more electronegative than S. Among nonmetals in periods, the electronegativity decreases from right to left, so F is more electronegative than O, and Cl is more electronegative than S.
04
Arrange in Order of Increasing Electronegativity
Based on the above steps, order the elements from least to the most electronegative: S < Cl < O < F.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Periodic Trends
Understanding periodic trends is essential for studying chemical properties of elements, including electronegativity. Electronegativity varies in a predictable pattern across the periodic table, which highlights the essence of these trends. As you move from left to right across a period, elements become more electronegative. This is because atoms generally gain more protons and electrons without significantly increasing in size, hence the increased pull on the shared electrons.
Contrastingly, as you navigate down a group, electronegativity tends to decrease. The reason for this is the addition of more electron shells, which places the outer electrons farther from the nucleus and weakens the pull on bonding pairs of electrons. It is this trend that lets us predict that sulfur (S) is less electronegative than oxygen (O), and chlorine (Cl) is less electronegative than fluorine (F), as described in the exercise solution provided.
Contrastingly, as you navigate down a group, electronegativity tends to decrease. The reason for this is the addition of more electron shells, which places the outer electrons farther from the nucleus and weakens the pull on bonding pairs of electrons. It is this trend that lets us predict that sulfur (S) is less electronegative than oxygen (O), and chlorine (Cl) is less electronegative than fluorine (F), as described in the exercise solution provided.
Periodic Table
The periodic table is more than just a tabulation of chemical elements; it's a roadmap of chemical properties and behaviors. Elements are arranged in order of increasing atomic number, which naturally brings about patterns in element properties. These patterns are not arbitrary; they are a result of the electronic structures of atoms and the way they interact to form chemical bonds.
A Guide to Electronegativity
When looking at electronegativity, the periodic table's structure becomes quite handy. As observed, elements in the top right corner, except for noble gases, typically exhibit the highest electronegativity. This phenomenon makes sense considering these elements are nearest to filling their valence, or outermost, electron shells and are thus more 'desperate' to attract electrons. Similarly, a deeper understanding of the positions and properties of elements like fluorine (F), chlorine (Cl), oxygen (O), and sulfur (S) provides an excellent foundation for predicting chemical properties and how these atoms will bond with others.Chemical Bonding
Chemical bonding, the mechanism by which atoms combine to form compounds, is deeply influenced by electronegativity. Atoms with similar electronegativities tend to form covalent bonds, where they share electrons more or less equally. On the other hand, if there's a significant difference in electronegativity between two atoms, the bond is ionic. In an ionic bond, one atom donates an electron and the other atom accepts it, leading to the formation of ions.