Question

rank the following atoms in order of decreasing size (i.e., largest to smallest): rb, f, mg, b, n. answer: a rb>mg>b>n>f b n>f>b>mg>rb c rb>mg>f>n>b d mg>rb>b>n>f e rb>mg>n>b>f

Explanation:

• Atomic radius trend: In the periodic table, atomic radius increases down a group (more electron shells) and decreases across a period (increasing nuclear charge pulls electrons closer).
• \(Rb\) (Rubidium) is in period 5, has the most electron shells among these atoms, so it is the largest.
• \(Mg\) (Magnesium) is in period 3.
• \(B\) (Boron), \(N\) (Nitrogen), and \(F\) (Fluorine) are in period 2. Among them, \(B\) has atomic number 5, \(N\) has atomic number 7, \(F\) has atomic number 9. As atomic number increases across a period, atomic radius decreases. So \(B > N > F\).

Answer:

A. \(Rb > Mg > B > N > F\)