Respuesta :
You can use the periodic table to help you determine the charge of an element when it becomes an ion. You base this on the group 8 elements called the noble gases. You can determine the charge by finding the difference of the atomic numbers of the given element to their nearest noble gas. It is made easier for elements on the left side. You can take their charge to be their group number. Since calcium is in group 2A, it will have a charge of 2+. Since Na is in group 1A, it will have a charge of 1+. Since Phosphorus is a nonmetal, it will have a negative charge because it needs to gain electrons to achieve their nearest noble gas. Since the nearest noble gas is Argon having an atomic number of 18, while Phosphorus has an atomic number of 15:
Charge = 15 - 18 = -3
The charge of Phosphorus is -3.
Charge = 15 - 18 = -3
The charge of Phosphorus is -3.
If Ca was to form ions, its expectant charge will be [tex]\boxed{ + 2}[/tex].
If Na was to form ions, its expectant charge will be [tex]\boxed{ + 1}[/tex].
If P was to form ions, its expectant charge will be [tex]\boxed{ - 3}[/tex].
Further explanation:
The distribution of electrons in atomic orbitals of an atom is called electronic configuration. It is done in accordance with the following principles and rules:
1. Aufbau principle
According to this principle, the electrons are filled in various orbitals in the increasing order of their energies. The increasing order of energies of orbitals is,
[tex]1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p[/tex]
2. Hund’s rule
The pairing of the electron cannot occur unless each orbital is singly occupied.
3. Pauli’s exclusion principle
This states that no two electrons in the same orbital can have the same values for all the quantum numbers. The value of spin quantum number for both electrons in the same orbital must always be different.
Ions are produced either by gain or loss of electrons. Those formed by the gain of electrons are termed as anions while those formed by loss of electrons are cations.
The atomic number of Ca is 20 and it has a configuration of [tex]1{s^2}2{s^2}2{p^6}3{s^1}[/tex]. It can remove two electrons from 4s orbital to achieve the stable noble gas configuration of Ar and [tex]{\text{C}}{{\text{a}}^{2 + }}[/tex] is formed. Therefore Ca forms an ion with a charge of +2.
The atomic number of Na is 11 and it has a configuration of [tex]{\text{N}}{{\text{a}}^ + }[/tex]. It can remove one electron from 3s orbital to attain the stable configuration of Ne and [tex]{\text{N}}{{\text{a}}^ + }[/tex] is formed. Therefore Na forms an ion with a charge of +1.
The atomic number of P is 15 and it has a configuration of [tex]1{s^2}2{s^2}2{p^6}3{s^2}3{p^3}[/tex]. It can gain three electrons and acquire a stable noble gas configuration of Ar and [tex]{{\text{P}}^{3 - }}[/tex] is formed. Therefore P forms an ion with a charge of -3.
Learn more:
- Determine the ion with configuration : https://brainly.com/question/7599542
- Identification of element which has electron configuration :https://brainly.com/question/9616334
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Electronic configuration of the elements
Keywords: Ca, Na, P, +2, +1, -3, atomic number, 20, 11, 15, configuration, Aufbau principle, Hund’s rule, Pauli’s exclusion principle, distribution of electrons.
