Chapter 5: Problem 83

How many bonds will an atom from group VA generally form? Explain why this is so.

Short Answer

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An atom from Group VA will generally form 3 bonds, as these elements have 5 valence electrons and need to share or gain 3 electrons to achieve a stable electronic configuration according to the octet rule. Group VA elements typically form covalent bonds, where they share electrons with other atoms to reach stability.

Step by step solution

Understanding Group VA Elements

Group VA elements in the periodic table have 5 valence electrons. The elements in this group include: nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi) among others. In a neutral atom, the number of valence electrons corresponds to the element's group number in the periodic table.

Valence Electrons and Bonding

Valence electrons are the electrons found in the outermost energy level of an atom. These electrons play a key role in forming chemical bonds, as they are involved in interactions with other atoms. Elements generally form bonds to achieve lower energy states, which are usually more stable. One way to achieve this stability is by achieving a complete (filled) outer energy level - a state known as the octet rule. For main group elements, the octet rule states that atoms are most stable when they have eight valence electrons. Therefore, atoms from group VA elements with 5 valence electrons will need to gain or share 3 electrons to achieve a complete outermost energy level.

Formation of Chemical Bonds

In order to gain, lose, or share electrons and form bonds, atoms can participate in three types of chemical bonds: ionic, covalent, and metallic. Group VA elements typically form covalent bonds, where the atoms share electrons with other atoms. Group VA elements can generally form three covalent bonds with other elements. This is because, as mentioned earlier, they have 5 valence electrons and need to gain or share 3 electrons to achieve a complete outer shell of 8 electrons.

Example: Nitrogen Molecule (N2)

A common example of a covalent bond formed by a group VA element is the nitrogen molecule - N2. In this case, two nitrogen atoms (each with 5 valence electrons) share 3 electrons with each other, forming a stable triple covalent bond. Each nitrogen atom in the molecule essentially ends up with 8 electrons in their outermost energy level, fulfilling the octet rule. In conclusion:

Number of Bonds for Group VA Elements

An atom from Group VA will generally form 3 bonds. This is because Group VA elements have 5 valence electrons and need to share or gain 3 electrons in order to achieve a stable electronic configuration according to the octet rule. Group VA elements typically form covalent bonds, where they share electrons with other atoms to reach stability.

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How many bonds will an atom from group VA generally form? Explain why this is so.

Short Answer

Step by step solution

Understanding Group VA Elements

Valence Electrons and Bonding

Formation of Chemical Bonds

Example: Nitrogen Molecule (N2)

Number of Bonds for Group VA Elements

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