Question

Jodine monochloride molecule is formed by the overlap of (1) s-s orbitals (2) s-p orbitals (3) p-d orbitals (4) \(\mathrm{p}-\mathrm{p}\) orbitals

Short answer

The overlap is between \( \text{p}-\text{p} \) orbitals.

Step-by-step solution

Identify Atomic Orbitals Involved

Recognize that iodine (I) and chlorine (Cl) are both elements in the p-block of the periodic table and have valence electrons in p orbitals.

Determine the Type of Bonds

Understand that in the formation of the Jodine monochloride (ICl) molecule, the overlap occurs between the valence orbitals of the iodine and chlorine atoms.

Identify the Specific Orbitals

Since both iodine and chlorine use their outermost p orbitals to form bonds, the overlap that occurs during the formation of the ICl molecule is between their p orbitals.

Conclude the Overlap Type

Conclude that the bond formation involves the overlap of \( \text{p} \) orbitals from both iodine and chlorine.

Key concepts

Atomic Orbitals

Atomic orbitals are regions around an atom where electrons are likely to be found. These orbitals come in different shapes and sizes, which are designated as s, p, d, and f. Each type of orbital has a unique shape:

• s-orbitals are spherical
• p-orbitals are dumbbell-shaped
• d orbitals have more complex shapes

. The electrons in these orbitals play a crucial role in determining an element's ability to form bonds. When two atoms come close, their atomic orbitals can overlap to form molecular orbitals. This overlap is essential in bond formation. For instance, in the formation of the ICl molecule, the p orbitals of iodine and chlorine overlap to form a bond.

P-Block Elements

P-block elements are found on the right side of the periodic table and include groups 13 to 18. These elements have their valence electrons in p orbitals. Examples include oxygen, sulfur, chlorine, and iodine. P-block elements show a wide range of properties. They can form multiple types of bonds, such as covalent and ionic bonds. In the case of iodine and chlorine, both being p-block elements, they form a covalent bond where electrons are shared between the two atoms. Understanding the behavior of p-block elements is essential to comprehend their bonding patterns and reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in chemical bonding. These electrons reside in the outer s and p orbitals. For p-block elements, the valence electrons occupy the p orbitals. In the ICl molecule, the valence electrons of iodine and chlorine are found in the 5p and 3p orbitals, respectively. These electrons overlap when the two atoms form a bond. The number of valence electrons helps determine the bonding capacity of an atom. For instance, chlorine has 7 valence electrons and needs one more to complete its octet, leading it to form a single covalent bond with iodine.

Bond Formation

Bond formation occurs when atomic orbitals overlap. This overlap allows atoms to share or transfer electrons, stabilizing the resulting molecule. There are different types of bond overlap:

• s-s orbital overlap
• s-p orbital overlap
• p-d orbital overlap
• p-p orbital overlap

. In the case of iodine monochloride (ICl), the bond is formed by the overlapping of their p orbitals. Both iodine and chlorine use their outermost p orbitals to share electrons and form a covalent bond. This p-p overlap results in a stable molecule with a shared pair of electrons between the two atoms.