Arrange these elements in order of increasing atomic size: Ca, Rb, P, Ge, Sr. (Try arranging the

step 1 So the periodic table is a tabular display of chemical elements that are arranged by atomic numb

Arrange these elements in order of increasing atomic size:...

Arrange these elements in order of increasing atomic size: $\mathrm{Ca}, \mathrm{Rb}, \mathrm{P}, \mathrm{Ge}, \mathrm{Sr}$. (Try arranging these without looking at Figure 5.25 and then check yourself by looking up the necessary atomic radii.)

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Key Concepts

Periodic Trends

Periodic trends describe the patterns observed in the properties of elements as you move across periods or down groups in the periodic table. Atomic radius, for example, generally decreases across a period due to increasing nuclear charge drawing electrons closer, and increases down a group as additional electron shells are added.

Shielding Effect

The shielding effect describes how inner electrons partially block the attractive force of the nucleus on the outer electrons. This phenomenon reduces the effective nuclear charge on the valence electrons, allowing the atomic radius to increase, particularly noticeable in elements lower down a group.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by electrons in an atom. It takes into account the total nuclear charge reduced by the shielding effect of inner electrons, and it significantly influences the atomic radius by determining how strongly electrons are attracted to the nucleus.

Atomic Radius

Atomic radius refers to the distance from the center of an atom's nucleus to the outer boundary of its electron cloud. It is a key measure of an atom's size and is influenced by the number of electron shells as well as the effective nuclear charge experienced by the electrons.

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