Which of the following pair of molecules contain odd electron molecule and an expanded octet molecule?
BCl3 and SF6
NO and H2SO4
SF6 and H2SO4
BCl3 and NO
The Correct Option is B
Approach Solution - 1
To determine which pair of molecules, contain an odd electron molecule and an expanded octet molecule, let's analyze each option:
- BCl3 and SF6:
- BCl3 (Boron Trichloride) is a compound in which boron has an incomplete octet. Boron has three valence electrons, bonding with three chlorine atoms without expanding its octet.
- SF6 (Sulfur Hexafluoride) has sulfur with six fluorine atoms bonded, leading to an expanded octet with 12 valence electrons around sulfur.
- This option does contain an expanded octet molecule (SF6), but BCl3 does not have an odd electron.
- NO and H2SO4:
- NO (Nitric Oxide) is a molecule with an odd number of electrons (15 in total), classifying it as an odd electron molecule.
- H2SO4 (Sulfuric Acid) has sulfur with an expanded octet due to the presence of more than 8 electrons in its valence shell.
- This option has both an odd electron molecule (NO) and an expanded octet molecule (H2SO4), making it the correct choice.
- SF6 and H2SO4:
- Both SF6 and H2SO4 have expanded octets, but neither has an odd electron molecule.
- BCl3 and NO:
- BCl3 does not have an odd electron or an expanded octet.
- NO has an odd electron; however, the combination does not have a molecule with an expanded octet.
Therefore, the pair of molecules that includes an odd electron molecule and an expanded octet molecule is: NO and H2SO4.
Approach Solution -2
NO is an odd electron species as N has 5 valence electrons and O has 6 valence electrons. Thus overall 1 electron on N remains unpaired.
S in H2SO4 has an expanded octet thus H2SO4 is expanded octet molecule.
So, the correct option is (B): NO and H2SO4
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Concepts Used:
Bond Parameters
Covalent bonds can be characterized on the basis of several bond parameters such as bond length, bond angle, bond order, and bond energy (also known as bond enthalpy). These bond parameters offer insight into the stability of a chemical compound and the strength of the chemical bonds holding its atoms together.
Bond parameters
- Bond length: it is an equilibrium distance between the centres of the nuclei of the two bonded atoms. It is expressed in terms of A.
- Bond Angle: It is characterized as the point between the orbitals consisting of holding electron sets around the focal iota in an atom/complex particle. Bond points are communicated in degrees which are tentatively controlled by spectroscopic strategies.
- Bond Enthalpy: the measure of energy needed to break one mole of obligations of a specific sort between two molecules in a vaporous state. The unit of bond enthalpy is kJ mol–1. The more the bond enthalpy, the more grounded the bond is.
For example, The H—H bond enthalpy in hydrogen is 435.8 kJ mol-1. \
- Bond Order: According to Lewis, Bond Order is given by the number of connections between the two atoms in a particle.
Bond order of H2 (H —H) =1
Bond order of 02 (O = O) =2
Bond order of N2 (N = N) =3
- Resonance Structures: It is observed that there are many molecules whose behaviour cannot be explained by a single Lewis structure.
Read More: Chemical Bonding and Molecular Structure