Question

For each of the following sets of elements, arrange the elements in order of increasing electronegativity. a.\(\mathrm {Li}\), \(\mathrm{F}\), \(\mathrm{C}\) b. \(\mathrm {I}\), \(\mathrm{Cl}\), \(\mathrm{F}\) c. \(\mathrm {L}\), \(\mathrm{R}\), \(\mathrm{C}\)

Short answer

Based on the periodic table trends of electronegativity: a. \(\mathrm{Li} < \mathrm{C} < \mathrm{F}\) b. \(\mathrm{I} < \mathrm{Cl} < \mathrm{F}\) c. Please provide the correct element symbols for set c.

Step-by-step solution

Recall the periodic table trends related to electronegativity

Electronegativity increases from left to right across a period and decreases down a group. Keep this trend in mind when comparing the given elements in each set.

Analyze the elements in set a (\(\mathrm {Li}\), \(\mathrm{F}\), \(\mathrm{C}\) )

Locate these elements in the periodic table: \(\mathrm {Li}\) is in Group 1 and Period 2, \(\mathrm{F}\) is in Group 17 and Period 2, and \(\mathrm{C}\) is in Group 14 and Period 2. Since all the elements are in the same Period (Period 2), the electronegativity will increase from left to right.

Order the elements in set a according to electronegativity

Based on the periodic table and electronegativity trends, set a should be ordered as follows: \(\mathrm {Li}\) < \(\mathrm{C}\) < \(\mathrm{F}\).

Analyze the elements in set b (\(\mathrm {I}\), \(\mathrm{Cl}\), \(\mathrm{F}\) )

Locate these elements in the periodic table: \(\mathrm {I}\) is in Group 17 and Period 5, \(\mathrm {Cl}\) is in Group 17 and Period 3, and \(\mathrm{F}\) is in Group 17 and Period 2. Since all the elements are in the same Group (Group 17), the electronegativity will decrease down the group.

Order the elements in set b according to electronegativity

Based on the periodic table and electronegativity trends, set b should be ordered as follows: \(\mathrm {I}\) < \(\mathrm{Cl}\) < \(\mathrm{F}\).

Analyze elements in set c (\(\mathrm {L}\), \(\mathrm{R}\), \(\mathrm{C}\) )

\(\mathrm {L}\) and \(\mathrm{R}\) are not valid element symbols. Please check and provide the correct element symbols for set c.

Key concepts

Periodic Table

The periodic table is a comprehensive chart that organizes chemical elements according to their atomic number, electron configuration, and recurring chemical properties. Elements are listed in rows called periods and columns known as groups.

Understanding the layout of the periodic table is crucial for studying electronegativity trends. For example, elements in the same group share similar electron configurations in their valence shell, which significantly affects their chemical behavior.

When solving problems related to element electronegativity, like the exercise with the elements Li, F, and C, you can refer to their positions on the periodic table to determine their electronegativity relationship.

Element Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons when it forms a chemical bond. A higher electronegativity value means an element is more effective at drawing electrons towards itself.

Electronegativity is a key factor in determining the polarity of bonds and the reactivity of an element. For instance, in the compound H₂O, oxygen has a higher electronegativity than hydrogen, which results in a polar molecule with a partial negative charge near the oxygen atom.

It's important to recognize that electronegativity is not a physical property with a direct measurement, but rather a relative scale. This can be seen in the exercise where elements Li, C, and F are arranged according to their electronegativity.

Chemical Elements Order

The order of chemical elements in the periodic table is not arbitrary; it reflects the elements' atomic number and overall trend in properties. From left to right in a period, the atomic number increases which leads to changes in properties such as electronegativity.

In the provided exercise, ordering elements like Li (Lithium), C (Carbon), and F (Fluorine) in terms of increasing electronegativity is simplified by understanding the layout of the periodic table. Li, being to the left of C and F in the same period, is least electronegative, while F, to the far right, is most electronegative.

Periodic Trends in Electronegativity

Electronegativity varies in a predictable way across the periodic table. Horizontally, it increases across a period from left to right due to the higher effective nuclear charge with increasing atomic number. Vertically, it decreases down a group as the farther valence electrons are from the nucleus, the less pull they experience.

These trends help explain the order of electronegativity for elements such as F, Cl, and I from the exercise, which are in the same group but different periods. The trend tells us that fluorine (F) has the highest and iodine (I) the least electronegativity of the three. Remembering these trends is pivotal for solving problems related to the arrangement of elements by electronegativity.