how do i write the complete electron configuration for Ga3+ and Mg2+????????????
Ga3+
The atomic number of neutral Ga is 31. Atomic number is equal to the number of electrons if the atom is neutral. Since it has a charge of 3+, it means it lost 3 electrons. Therefore, 31 - 3 = 28. Writing the e config: (recall aufbau principle)
Ga : 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1
Ga 3+ : 1s2 2s2 2p6 3s2 3p6 4s0 3d10
or in Noble Gas core notation,
Ga3+ : [Ar]4s0 3d10
Note that 4s electrons are lost before 3d electrons thus, the electrons are deducted first to the 4s rather than 3d.
Mg2+
Atomic number of Mg is 12. Since the charge is 2+, 2 electrons are lost. Thus, 12 - 2 = 10:
Mg : 1s2 2s2 2p6 3s2
Mg2+ : 1s2 2s2 2p6
Hope this helps~ :)
To determine the electron configuration for Ga3+ and Mg2+, we need to follow a few steps.
Step 1: Identify the element's atomic number
The atomic number for Ga (Gallium) is 31, and for Mg (Magnesium) is 12.
Step 2: Determine the neutral atom's electron configuration
The electron configuration for Ga (neutral atom) is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^1.
The electron configuration for Mg (neutral atom) is 1s^2 2s^2 2p^6 3s^2.
Step 3: Determine the number of electrons lost or gained
Ga3+ means that the neutral Ga atom loses 3 electrons (since it has a positive charge).
Mg2+ means that the neutral Mg atom loses 2 electrons.
Step 4: Write the electron configuration for the ion
3 electrons are removed from the Ga atom, starting from the highest energy level (4s), followed by the 3d and 4p orbitals.
The electron configuration for Ga3+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10.
2 electrons are removed from the Mg atom, starting from the highest energy level (3s).
The electron configuration for Mg2+ is: 1s^2 2s^2 2p^6.
So, the complete electron configuration for Ga3+ is 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10, and for Mg2+ is 1s^2 2s^2 2p^6.
To determine the complete electron configuration for Ga³⁺ and Mg²⁺, we need to locate their positions in the periodic table and understand the rules for filling electron orbitals.
1. Ga³⁺ (Gallium ion):
Gallium (Ga) is a neutral atom with an atomic number of 31. We need to remove three electrons to form Ga³⁺.
To determine the electron configuration, we start by writing the electron configuration of the neutral Ga atom: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p¹.
Since we're removing three electrons, we remove them from the highest energy level, which is the 4th energy level (4s² 3d¹⁰ 4p¹).
As a result, the electron configuration of Ga³⁺ is: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰.
2. Mg²⁺ (Magnesium ion):
Magnesium (Mg) is a neutral atom with an atomic number of 12. To form Mg²⁺, we need to remove two electrons.
The electron configuration for the neutral Mg atom is: 1s² 2s² 2p⁶ 3s².
We remove two electrons from the 3s sublevel.
As a result, the electron configuration for Mg²⁺ is: 1s² 2s² 2p⁶.
Remember, when writing electron configurations for ions, indicate the charge of the ion by adding a superscript after the electron configuration.