The statement "a nonmetal atom is more electronegative than metal" is generally not true. Metals tend to have lower electronegativity values compared to nonmetals. Electronegativity is a measure of the ability of an atom to attract electrons in a chemical bond.

Metals, such as those in Group 1 (alkali metals) and Group 2 (alkaline earth metals), have low electronegativity values because they have loosely bound valence electrons, which they can easily give up, making them electropositive. On the other hand, nonmetals have higher electronegativity values because they have a greater ability to attract electrons due to their strong nuclear charge and effective nuclear charge experienced by the valence electrons.

Here are some specific examples:

- Cesium (Cs), a metal, has an electronegativity value of 0.79, while Fluorine (F), a nonmetal, has an electronegativity value of 3.98.

- Sodium (Na), another metal, has an electronegativity value of 0.93, while Chlorine (Cl), a nonmetal, has an electronegativity value of 3.16.

Overall, nonmetals have higher electronegativity values than metals, with some exceptions in the periodic table where neighboring elements might have comparable electronegativity values.