Question

Which set has strongest tendency to form anions? (1) \(\mathrm{Ga}, \mathrm{In}, \mathrm{Te}\) (2) \(\mathrm{Na}, \mathrm{Mg}, \mathrm{A} 1\) (3) \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) (4) V, Cr, Mn

Short answer

Set 3: \(\mathrm{N}, \mathrm{O}, \mathrm{F}\).

Step-by-step solution

- Identify Groups and Periods

Look at the periodic table and identify which groups and periods each element belongs to. Elements in the same group have similar chemical properties.

- Determine Electron Affinity

Consider each element's electron affinity. Higher electron affinity indicates a stronger tendency to form anions. Elements in the top right of the periodic table (excluding noble gases) have higher electron affinities.

- Analyze Set 1: \(\mathrm{Ga}, \mathrm{In}, \mathrm{Te}\)

\(\mathrm{Ga}\) and \(\mathrm{In}\) are in group 13 and have lower tendencies to form anions. \(\mathrm{Te}\) is in group 16 and is more likely to form anions.

- Analyze Set 2: \(\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}\)

\(\mathrm{Na}\), \(\mathrm{Mg}\), and \(\mathrm{Al}\) are group 1, 2, and 13 elements respectively, which do not have a strong tendency to form anions.

- Analyze Set 3: \(\mathrm{N}, \mathrm{O}, \mathrm{F}\)

\(\mathrm{N}\), \(\mathrm{O}\), and \(\mathrm{F}\) are group 15, 16, and 17 elements, respectively. They are located in the top right of the periodic table and have high electron affinities, thus a strong tendency to form anions.

- Analyze Set 4: \(\mathrm{V}, \mathrm{Cr}, \mathrm{Mn}\)

\(\mathrm{V}\), \(\mathrm{Cr}\), and \(\mathrm{Mn}\) are transition metals and typically have a lower tendency to form anions compared to non-metals.

- Conclusion

Compare the sets and determine which set contains elements with the strongest tendency to form anions.

Key concepts

Periodic Table Groups

Understanding the periodic table groups can help identify elements' chemical properties. Each group on the periodic table consists of elements that share similar characteristics. Groups are the vertical columns in the periodic table, numbered from 1 to 18. Elements within the same group have the same number of valence electrons, leading to similar chemical behaviors. For instance, Group 1 elements (alkali metals) have one valence electron, making them highly reactive. Similarly, Group 17 elements (halogens) have seven valence electrons, making them eager to gain one more electron to achieve a stable electron configuration. Knowing the group can thus hint at how readily an element might form an anion. Elements in groups 15, 16, and 17 are more likely to form anions as they gain electrons easily to complete their outer shell.

Electron Affinity

Electron affinity is the amount of energy released when an atom gains an electron. It is a crucial factor in determining an element's tendency to form anions. Higher electron affinity means the element releases more energy upon gaining an electron, making it more likely to become negatively charged (anion). Elements with high electron affinities are generally found in the top right region of the periodic table, excluding noble gases. For example, fluorine (F) has one of the highest electron affinities, making it highly reactive and prone to forming anions. In contrast, elements in the lower left of the periodic table have lower electron affinities, showing less tendency to gain electrons. Group 16 and 17 elements usually have higher electron affinities, indicating their strong inclination to form anions.

Chemical Properties

Chemical properties of elements define how they react with other substances. These properties are influenced by atomic structure, particularly the number and arrangement of electrons. Elements within the same group typically exhibit similar chemical properties due to their having identical valence electron configurations. For instance, elements in Group 1 (alkali metals) react vigorously with water. The behavior of an element to form an anion is a key chemical property. Non-metals, found on the right side of the periodic table, especially those in groups 15, 16, and 17, tend to form anions readily. This is because they need to gain electrons to achieve a stable electronic configuration similar to noble gases. In contrast, metals, particularly transition metals and elements on the left side of the periodic table, tend to lose electrons and form cations instead of anions. Understanding these properties is essential in predicting the outcomes of chemical reactions and the formation of compounds.