An atom of an element has 13 electrons. Its nucleus has 14 neutrons. Find out atomic no. and approximate atomic weight. Indicate the arrangement of electrons and the electrovalency of the element.

Understanding the fundamentals of atomic structure is crucial, and atomic number determination is the key to unlocking the identity of an element. The atomic number, typically symbolized as 'Z', is the number of protons found in the nucleus of an atom. In any neutral atom, the number of electrons orbiting the nucleus is equal to the number of protons inside the nucleus. This balance ensures the atom remains electrically neutral.

For instance, if an atom has 13 electrons, it must also have 13 protons. Therefore, the atomic number for this atom is 13. An element's position in the periodic table is defined by its atomic number, making it an essential aspect when classifying and studying elements. In practice problems, the atomic number can often be deduced from given information about the electrons in a neutral atom.

The atomic weight, also referred to as the atomic mass, is a crucial piece of information about an element's characteristics. It is approximately equivalent to the mass number 'A', which is the sum of protons and neutrons in the atom's nucleus. To calculate the atomic weight, we must recognize that protons and neutrons carry nearly equal mass, much larger than the mass of electrons.

For an atom with an atomic number of 13 (number of protons) and 14 neutrons, the atomic weight can be calculated as follows: \[ \text{Atomic weight} = \text{Number of protons} + \text{Number of neutrons} = 13 + 14 = 27 \]
This sum gives us an approximate mass number, which helps us compare the relative masses of different atoms. This calculation is fundamental in understanding the composition and potential reactions involving the chemical element.

Electron arrangement in atoms is a systematic process, with electrons occupying shells or energy levels around the nucleus. Understanding this structure helps us predict the chemical properties of an element. The electron configuration follows a set of principles, including the Pauli exclusion principle and Hund's rule, to determine the distribution across different shells.

The first shell accommodates up to two electrons, the second takes up to eight, and subsequent shells follow similar patterns as defined by the quantum mechanical model of the atom. Taking a 13-electron atom as an example, the arrangement would be 2 electrons in the first shell, 8 in the second, and the remaining 3 in the third shell, often written as 2, 8, 3. This configuration is pivotal to understanding chemical bonding and reactivity.

Electrovalency is a concept that relates to an atom's ability to gain or lose electrons during chemical reactions, thus forming ions. The valency of an element is typically determined by the number of electrons in its outermost shell; this predicts the charge that the ion of this element will carry. Elements tend to react in ways that allow them to achieve a stable electronic configuration, usually the noble gas structure.

In our example, the element has 3 electrons in the outer shell; by losing these, it strives for a full outer shell and, therefore, stability. Thus, the element exhibits an electrovalency of +3, indicating it can form an ion with a charge of +3. This predictive tool is essential for understanding how elements will combine to form ionic compounds.