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Answer :
Final answer:
The atom with the greater electronegativity acquires a partial negative charge. In the context of a bond between hydrogen and fluorine, the fluorine atom would have a partial negative charge (δ-) due to its higher electronegativity compared to hydrogen. so the correct option is B) Fluorine
Explanation:
Atoms in a molecule will have a partial negative charge, represented by the symbol δ-, if they are more electronegative than the atoms they are bonded to. Electronegativity is a measure of how strongly atoms attract the electrons in a chemical bond. In the molecule being discussed, which contains a bond between hydrogen and fluorine, we look at the relative electronegativities of the atoms involved to determine partial charges.
The fluorine atom is highly electronegative, more so than hydrogen, therefore it will attract the bonding electrons more strongly. As a result, the fluorine atom will have a partial negative charge (δ-). If nitrogen were involved in a similar comparison, it would also tend to take on a partial negative charge because nitrogen is more electronegative than hydrogen but less so than fluorine.
Conversely, the hydrogen atom has less electronegativity compared to fluorine and will thus adopt a partial positive charge (δ+). Thus, in a molecule of hydrogen fluoride (HF), which is a dipole, we designate the fluorine atom with δ- and the hydrogen atom with δ+.
In conclusion, based on the given information and understanding of electronegativity, the correct answer to which atom(s) have a partial negative charge (δ-) would be Fluorine, as it is the most electronegative atom in the bond, attracting electrons and gaining a partial negative charge.
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