Question

Write the charge and full ground-state electron configuration of the monatomic ion most likely to be formed by p. charge: ground-state electron configuration:

Answer 1

Answer: The charge on Phosphorus will be -3 and its electronic configuration is given below.

Explanation:

Phosphorous is the 15th element of the periodic table. The number of electrons this element contain are 15.

Ground state electron configuration is defined as the arrangement of electrons around the nucleus of an atom present in lower energy levels.

Ground state electronic configuration of phosphorous = $1s^22s^22p^63s^33p^3$

As, this element is short of 3 electrons, thus, it requires 3 electrons to attain stable electronic configuration.

When an element gains electrons, it attains a negative charge.

Hence, the charge on phosphorous element is -3 and its electronic configuration is given above.

Answer 2

The charge on the monoatomic ion formed by P is $\boxed{{\text{-3}}}$ and its full ground-state electronic configuration is $\boxed{1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}}$.

Further explanation:

The electronic configuration is the distribution of electrons of an atom in the atomic orbitals. There are two states for an electron: ground as well as the excited state. The configuration of the atom in the lowest possible energy levels is called the ground-state electronic configuration. When an electron jumps from the stable ground state to some higher level, that state is called the excited state and the electronic configuration corresponding to this state is known as the excited-state electronic configuration.

The filling of electrons in different energy levels or orbitals is done in accordance with the following three rules.

1. Aufbau principle: The principle states that the electrons are filled in various orbitals in the increasing order of their energies.

2. Hund’s rule: Electron pairing will not start until each orbital is singly occupied.

3. Pauli’s exclusion principle: According to this principle, all the four quantum numbers $\left({n,\;l,\;{m_l},\;{m_s}}\right)$ for any two electrons can never be the same. In an orbital, the spin of two electrons has to be different. If one electron has the clockwise spin, the other would have the anticlockwise spin and vice-versa.

The atomic number of P is 15 so its full ground-state electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^2}3{p^3}$. It is three electrons short of the stable noble gas configuration of Ar. So the monoatomic ion formed by gain of 3 electrons will have a charge of -3 and its full ground-state electronic configuration is ${\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{p}}^{\mathbf{6}}}{\mathbf{3}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{3}}{{\mathbf{p}}^{\mathbf{6}}}$.

Learn more:

1. Determine the ion with configuration $\left[{{\text{Ar}}}\right]\;3{d^2}$: brainly.com/question/7599542

2. Identification of element which has electron configuration $1{s^2}2{s^2}2{p^2}3{s^1}$:brainly.com/question/9616334

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Electronic configuration of the elements.

Keywords: monoatomic ion, P, 15, Ar, electronic configuration, condensed electronic configuration, noble gas, Aufbau principle, Hund’s rule, Pauli’s exclusion principle, charge, -3.