Consider the elements: Na, Mg, Al, Si, P a. Which element has the highest second ionization ener

step 1 We're considering the elements that are outlined in red. The highest second ionization energy is

Consider the elements: Na, Mg, Al, Si, P a. Which element...

Consider the elements: $\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{P}$
a. Which element has the highest second ionization energy?
b. Which element has the smallest atomic radius?
c. Which element is least metallic?
d. Which element is diamagnetic?

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in the gaseous state. The second ionization energy specifically refers to the energy needed to remove a second electron after the first has already been removed. This energy is influenced by the electron configuration and effective nuclear charge, and there is typically a substantial increase when the removal of a second electron disrupts a stable electron configuration.

Atomic Radius

Atomic radius is a measure of the size of an atom, usually defined as the distance from the nucleus to the outer boundary of the electron cloud. The atomic radius generally decreases across a period due to the increased effective nuclear charge pulling electrons closer to the nucleus, and increases down a group as additional electron shells are added.

Metallicity

Metallicity refers to the tendency of an element to exhibit properties characteristic of metals, such as good electrical conductivity, malleability, ductility, and lower ionization energies. In the periodic table, metallic character generally decreases from left to right across a period as atoms become smaller and ionization energies increase, indicating a shift towards non-metallic behavior.

Diamagnetism

Diamagnetism is a form of magnetism observed in materials in which all the electrons are paired. In diamagnetic substances, the induced magnetic field produced by these paired electrons is opposite to an externally applied magnetic field, causing a weak repulsion. This property is an indicator of the electron configuration and the absence of unpaired electrons.

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