Each of the following elements is capable of forming an ion in chemical reactions. By referring to the periodic table, predict the charge of the most stable ion of each: (a) Be (b) Rb (c) As (d) In (e) At.

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Identify the group number of arsenic (As) in the periodic table. Arsenic is in group 15.

Determine the number of valence electrons for arsenic. Elements in group 15 have 5 valence electrons.

Consider the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a full set of 8 valence electrons.

Calculate how many electrons arsenic needs to gain to achieve a full octet. Arsenic needs 3 more electrons to reach 8 valence electrons.

Predict the charge of the arsenic ion. Since arsenic gains 3 electrons, it will have a charge of -3, forming the As^{3-} ion.

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Key Concepts

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

Ion Formation

Ion formation occurs when an atom gains or loses electrons, resulting in a charged particle. Metals typically lose electrons to form cations, while nonmetals gain electrons to form anions. The charge of the ion is determined by the number of electrons lost or gained relative to the neutral atom.

Periodic Table Trends

The periodic table displays trends in atomic properties, including electronegativity, ionization energy, and atomic radius. Elements in the same group often exhibit similar behaviors in ion formation. For example, elements on the right side of the table tend to gain electrons, while those on the left tend to lose them, influencing the charge of the ions they form.

Group 15 Elements

Arsenic (As) is a Group 15 element, which typically has five valence electrons. To achieve a stable electron configuration, arsenic can either gain three electrons to form a -3 anion or lose five electrons to form a +5 cation. However, the most stable ion for arsenic is usually the -3 anion, as it aligns with the tendency of nonmetals to gain electrons.

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