The requirements of atoms to be able to participate in hydrogen bonding with a hydrogen atom include all of the following except a. atoms must not be able to closely approach the hydrogen. b. atoms must be electronegative. c. atoms must have one lone pair of electrons. d. atoms must be small.

B. atoms must be electro negative.

The answer is A.

Explanation:

This is a specific type of polar interaction that is established between two atoms with high electronegativity, usually between O or N, and an atom of H. In the case of oxygen, with a total of 8 electrons, two pairs of solitary electrons are presented and can act as acceptors of two hydrogen bridges. Nitrogen has one less electron and therefore has only one pair of solitary electrons to form a hydrogen bridge. These orbitals have a high negative charge density, and can, therefore, bind to the positive charge of hydrogen.

The interatomic distance between the hydrogen and the acceptor is less than the sum of its Van der Waals radius. The atomic radius of N and O are relatively small.

Have a nice day!

oh it is true if thats what you are asking

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."