Question

Boron differs from other members of III A because of its (1) small size, high ionization potential and absence of \(d\) -orbitals. (2) large size, low ionization potential and presence of \(d\) -orbitals. (3) small size, low ionization potential and absence of \(d\) -orbitals. (4) large size, high ionization potential and absence of \(d\) -orbitals.

Short answer

Option (1) is correct: small size, high ionization potential, and absence of d-orbitals.

Step-by-step solution

Understand Boron's Position in the Periodic Table

Boron is a member of Group III A (Group 13) in the periodic table. It is the first element in this group.

Identify the Properties of Boron

Boron has unique properties due to its small atomic size, high ionization energy, and absence of available d-orbitals for bonding.

Compare Boron's Properties to Other Group III A Elements

Other elements in Group III A, such as aluminum, gallium, indium, and thallium, have larger atomic sizes, lower ionization energies, and in some cases, accessible d-orbitals.

Match Boron's Properties with Given Options

Compare the unique properties of boron with the given options: 1) Small size, high ionization potential, and absence of d-orbitals 2) Large size, low ionization potential, and presence of d-orbitals 3) Small size, low ionization potential, and absence of d-orbitals 4) Large size, high ionization potential, and absence of d-orbitals The correct option is the one that fits the unique properties of boron.

Select the Correct Option

Option (1) matches the unique properties of boron: small size, high ionization potential, and absence of d-orbitals.

Key concepts

Periodic Table

The periodic table is a tabular arrangement of elements, organized by increasing atomic number. Each element is placed in a specific location based on its atomic structure and properties. Elements in the same column, known as a group, share similar chemical behaviors because they have the same number of valence electrons.

Boron is an element in Group III A (also known as Group 13) of the periodic table. This group includes boron (B), aluminum (Al), gallium (Ga), indium (In), and thallium (Tl). Boron is the first element in this group and is unique among its group members due to its small size and distinct chemical properties.

Understanding an element's position in the periodic table helps us predict its behavior, reactivity, and the type of bonds it forms.

Ionization Potential

The ionization potential (or ionization energy) is the energy required to remove an electron from an atom or ion in its gaseous state. It is a crucial factor that affects an element's chemical reactivity.

Elements with high ionization potential hold their electrons tightly and do not lose them easily. Conversely, a low ionization potential means that electrons can be removed more readily.

Boron has a high ionization potential compared to other members of Group III A. This is because boron has a smaller atomic size, leading to a stronger attraction between the nucleus and the valence electrons. This makes it more difficult to remove an electron from boron.

d-orbitals

Atomic orbitals are regions around the nucleus of an atom where electrons are likely to be found. They come in different shapes and energy levels, often categorized by the principal quantum number (n) and the type of orbital, such as s, p, d, and f.

The d-orbitals appear starting from the third energy level (n=3) and are higher in energy than the s and p orbitals of the same principal quantum number.

Boron is unique among its group members because it does not have available d-orbitals. Boron's electron configuration is simple, with only 2s and 2p orbitals available for bonding. This absence of d-orbitals plays a significant role in its chemistry. In contrast, elements like aluminum, gallium, indium, and thallium have readily accessible d-orbitals, influencing their bonding capabilities and reactivity.