Chapter 3, Problem 13P

3-29 Answer true or false.

(a) According to the Lewis model of bonding, atoms bond together in such a way that each atom participating in the bond acquires an outer-shell electron configuration matching that of the noble gas nearest to it in atomic number.

(b) Atoms that lose electrons to achieve a filled valence shell become cations and form ionic bonds with anions.

(c) Atoms that gain electrons to achieve filled valence shells become anions and form ionic bonds with cations.

(d) Atoms that share electrons to achieve filled valence shells form covalent bonds.

(e) Ionic bonds tend to form between elements on the left side of the Periodic Table, and covalent bonds tend to form between elements on the right side of the Periodic Table.

(f) Ionic bonds tend to form between a metal and a nonmetal.

(g) When two nonmetals combine, the bond between them is usually covalent.

(h) Electronegativity is a measure of an atom’s at traction for the electrons it shares in a chemical bond with another atom.

(j) Electronegativity generally increases with atomic number.

(j) Electronegativity generally increases with atomic weight.

(k) Electronegativity is a periodic property.

(l) Fluorine, in the upper-right corner of the Periodic Table, is the most electronegative element; hydrogen, in the upper-left corner, is the least electronegative element.

(m)Electronegativity depends on both the nuclear charge and the distance of the valence electrons from the nucleus.

(n) Electronegativity generally increases from left to right across a period of the Periodic Table.

(o) Electronegativity generally increases from top to bottom in a column of the Periodic Table.