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Chapter 5: Problem 83

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

Short Answer

Expert verified
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

01

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.
02

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.
03

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.
04

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:
05

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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Valence Electrons
Valence electrons hold a crucial role in an atom's ability to form chemical bonds. They are the electrons located in the outermost shell of an atom, and their number corresponds to the atom's group number in the periodic table.
For example, group VA elements such as nitrogen and phosphorus possess 5 valence electrons. These electrons are particularly important because they determine how an atom can interact with other atoms.

Understanding valence electrons is essential because they are often involved in sharing or transferring processes, enabling elements to achieve more stable structures.
Covalent Bonds
Covalent bonds are a type of chemical bond where atoms share valence electrons. This sharing allows each atom to attain a full outer shell, resulting in a more stable state.
Group VA elements, which include nitrogen and phosphorus, are known to typically form covalent bonds due to their need to fill their valence shells with 3 additional electrons.
  • Covalent bonding involves the mutual sharing of electrons.
  • It is commonly seen in non-metal atoms that have a tendency to share rather than fully transfer electrons.
  • An example is the formation of a nitrogen molecule (N2), where each nitrogen atom shares three electrons.
This type of bonding is essential for the formation of stable molecular compounds.
Octet Rule
The octet rule is a guiding principle in chemistry that refers to the tendency of atoms to prefer a complete set of eight electrons in their valence shell. This configuration is typically associated with stability.
Atoms achieve this by gaining, losing, or sharing electrons through different types of bonds, primarily covalent bonds for group VA elements.

For example, group VA elements like nitrogen need 3 more electrons to reach the octet configuration. Thus, they often share electrons with other atoms to achieve this goal, leading to the formation of three covalent bonds.
By attaining a complete octet, atoms minimize their energy and gain stability, which is why the octet rule is such a vital concept in understanding chemical bonding and molecular structures.

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Most popular questions from this chapter

Does \(\mathrm{BeH}_{2}\) have all of its atoms obeying the octet rule? If not, indicate which atom or atoms violate the octet rule and why it is OK.

\(\mathrm{N}_{2} \mathrm{O}\) is called dinitrogen monoxide, whereas, \(\mathrm{Na}_{2} \mathrm{O}\) is called sodium oxide, not disodium oxide. Explain why, and also explain how the name sodium oxide still lets us know that there are two sodium atoms in the formula.

The oxide ion is \(\mathrm{O}^{2-}\). How does this ion differ from the peroxide ion, \(\mathrm{O}_{2}^{2-} ?\) Draw dot diagrams for both.

It is convenient to classify substances as ionic or covalent. How would you classify sodium sulfate? Explain fully.

Draw a dot diagram for the molecule \(\mathrm{SO}_{2}\), sulfur dioxide, a gas that comes from burning coal and is responsible for acid rain. (Hint: Sulfur is in the mid?le.)
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