The metallic character of the Boron family is less than that of alkaline earth metals.
The Boron family, also known as Group 13 elements, consists of boron (B), aluminum (Al), gallium (Ga), indium (In), and thallium (Tl). On the other hand, alkaline earth metals are found in Group 2 of the periodic table and include elements such as beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).

Explanation:

1. Definition of Metallic Character:
The metallic character refers to the tendency of an element to lose electrons and form positive ions (cations). It is a measure of how easily an element can donate electrons and exhibit metallic properties such as high thermal and electrical conductivity, luster, malleability, and ductility.

2. Factors Affecting Metallic Character:
The metallic character of an element is influenced by several factors, including:
- Atomic radius: Larger atoms have more loosely held electrons, making it easier for them to be lost, thus increasing metallic character.
- Ionization energy: The energy required to remove an electron from an atom. Lower ionization energy means it is easier for an atom to lose electrons, increasing metallic character.
- Electronegativity: The tendency of an atom to attract electrons towards itself. Lower electronegativity facilitates the donation of electrons, enhancing metallic character.

3. Comparison between Boron Family and Alkaline Earth Metals:
In the Boron family, the metallic character decreases from boron to thallium. This trend can be attributed to the following factors:
- Atomic size: As we move down the Boron family, the atomic size increases, resulting in a decrease in the effective nuclear charge. This decrease reduces the attraction between the nucleus and valence electrons, making it harder for the elements to lose electrons and exhibit metallic properties.
- Ionization energy: The ionization energy generally decreases down the group, indicating that the elements become more willing to lose electrons. However, the decrease in metallic character is primarily due to the larger atomic size.

In contrast, alkaline earth metals have a higher metallic character than the Boron family. This is because alkaline earth metals have larger atomic sizes, lower ionization energies, and lower electronegativities compared to the Boron family. These factors make it easier for alkaline earth metals to lose electrons and form positive ions, thereby exhibiting stronger metallic properties.

In conclusion, the metallic character of the Boron family is less than that of alkaline earth metals due to differences in atomic size, ionization energy, and electronegativity.