Place the following pairs of elements in order from smallest to largest difference in electronegativity: K and F, S and O, Br and I, Ca and Se, Li and Cl.

Name: Chemistry: The Central Science
Author: Brown
ISBN: 9780137542970

Verified step by step guidance

Step 1: Understand the concept of electronegativity. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

Step 2: Identify the electronegativity values for each element using the Pauling scale. For example, F (Fluorine) has an electronegativity of 3.98, K (Potassium) has 0.82, etc.

Step 3: Calculate the difference in electronegativity for each pair of elements. For instance, for K and F, subtract the electronegativity of K from that of F.

Step 4: Compare the calculated differences for each pair to determine the order from smallest to largest difference.

Step 5: Arrange the pairs in order based on the differences calculated in Step 4.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It is a key factor in determining the nature of bonds between atoms, influencing whether they will form ionic or covalent bonds. The Pauling scale is commonly used to quantify electronegativity values, with higher values indicating a stronger attraction for electrons.

Difference in Electronegativity

The difference in electronegativity between two atoms can help predict the type of bond they will form. A larger difference typically indicates an ionic bond, while a smaller difference suggests a covalent bond. By calculating the electronegativity differences for the given pairs, one can rank them from smallest to largest, providing insight into their bonding characteristics.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements across the periodic table. Electronegativity generally increases across a period from left to right and decreases down a group. Understanding these trends is essential for comparing the electronegativities of different elements and determining their relative differences.

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Related Practice

Textbook Question

Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Se, Te, Br, I; (b) Be, Mg, C, Si (c) Al, Si, P, S (d) Zn, Ge, Ga, As.

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Textbook Question

Which of the following bonds are polar: a. B—F, b. Cl—Cl, c. Se—O, d. H—I? Which is the more electronegative atom in each polar bond?

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Textbook Question

(b) How many bonding electrons are in the structure?

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Textbook Question

Using Lewis symbols and Lewis structures, diagram the formation of PF₃ from P and F atoms, showing valence-shell electrons. (a) How many valence electrons does P have initially? (c) How many valence electrons surround the P in the PF₃ molecule? (d) How many valence electrons surround each P in the PF₃ molecule?

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Textbook Question

By referring only to the periodic table, select (d) the element in the group K, C, Zn, F that is most likely to form an ionic compound with Ba.

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Textbook Question

Which of the following statements about electronegativity is or are true? i. The alkali metals are the family with the largest electronegativity values. ii. The numerical values for electronegativity have no units. iii. Electronegativity is the ability of an atom in a molecule to attract electron density toward itself.

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