Final answer:
The statement is true; higher electronegativity indicates a stronger ability of an atom to attract and accept electrons, which is crucial for understanding bond polarity and chemical reactivity.
Step-by-step explanation:
True. Electronegativity is a measure of the tendency of an element to attract electrons towards itself. The higher the electronegativity, the stronger is the atom's ability to attract electrons, making it more likely for the element to accept electrons. This principle is essential in understanding chemical bonding and reactivity. Electronegativity values range from about 0.6 to 4.0, with fluorine being the most electronegative. Covalent bonds formed between atoms of different electronegativities will be polar, with the most electronegative atom attracting more electron density towards itself.
Increasing electronegativity is observed as we move from the lower left-hand corner to the upper right-hand corner of the periodic table. Elements with high electronegativity tend to gain electrons in chemical reactions, while elements with lower electronegativity values are more likely to lose electrons. For instance, elements found in periods 3-7 of the periodic table can sometimes accommodate more than eight electrons in their valence shell due to valence shell expansion, highlighting the complexity of electron interactions in molecules with such elements.