The atomic radius is not determined by a specific formula because it is not a fixed value. It can change depending on the atom's state and the atoms around it. However, it is generally determined using the following methods:

1. Covalent Radius: This is half the distance between the nuclei of two like atoms joined by a covalent bond in a molecule.

2. Van der Waals Radius: This is half the distance between the closest approach of two non-bonded atoms of a given element.

3. Metallic Radius: This is half the distance between the nuclei of two adjacent atoms in a metallic crystal.

4. Ionic Radius: This is the radius of an atom's ion.

In general, atomic radius decreases across a period from left to right and increases down a group. This is due to the increase in positive charge in the nucleus which pulls the electrons closer to the nucleus across a period, and the addition of energy levels/shells down a group.

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The atomic radius is not determined by a specific formula because it is not a fixed value. It can change depending on the atom's state and the atoms around it. However, it is generally determined using the following methods:

1. Covalent Radius: This is half the distance between the nuclei of two like atoms joined by a covalent bond in a molecule.

2. Van der Waals Radius: This is half the distance between the closest approach of two non-bonded atoms of a given element.

3. Metallic Radius: This is half the distance between the nuclei of two adjacent atoms in a metallic crystal.

4. Ionic Radius: This is the radius of an atom's ion.

In general, atomic radius decreases across a period from left to right and increases down a group. This is due to the increase in positive charge in the nucleus which pulls the electrons closer to the nucleus across a period, and the addition of energy levels/shells down a group.

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The atomic radius is not determined by a specific formula because it is not a fixed value. It can change depending on the atom's state and the atoms around it. However, it is generally determined using the following methods:

1. Covalent Radius: This is half the distance between the nuclei of two like atoms joined by a covalent bond in a molecule.

2. Van der Waals Radius: This is half the distance between the closest approach of two non-bonded atoms of a given element.

3. Metallic Radius: This is half the distance between the nuclei of two adjacent atoms in a metallic crystal.

4. Ionic Radius: This is the radius of an atom's ion.

In general, atomic radius decreases across a period from left to right and increases down a group. This is due to the increase in positive charge in the nucleus which pulls the electrons closer to the nucleus across a period, and the addition of energy levels/shells down a group.

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