This is an impossible formula. Pretend it is real.
1 answer:
There are eight moles of oxygen atoms in 1 mole of .
We know that a compound is composed of atoms. The atoms that make up the molecule are chemically combined. It is usual that the number of atoms in the compound would correspond with the chemical formula.
Now we have the compound . In one mole of the compound we have;
- 9 Moles of manganese atom
- 2 moles of chlorine atom
- 8 moles of oxygen atom
Thus, there are eight moles of oxygen atoms in 1 mole of .
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The arrangement of the electrons on the orbitals is governed by the principles of quantum energy. To be able to draw the correct electronic configuration of an element, they should follow these three principles.
1. Aufbau's Principle. The electrons of an element should be filled up from the highest energy level. You can use the periodic table as a guide for this. In decreasing order, the energy of the orbitals are 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d and 7p. Each 'box' of these orbital must be filled with two electrons from 1s before moving on to the next.
2. Hund's rule. This states that you must fill all boxes of one orbital with one electron first. For example, 2p has 3 boxes. You fill one electron for each box first before going back to fill it to two electrons if there are still excess.
3. Pauli's Exclusion Principle. This states that no electrons of the same element should have the same quantum numbers. To achieve this, the two electrons in each box should have opposite spins, one facing up, and the other facing down.
Using these three rules, you will be able to draw the electronic configuration of Fluorine with 9 electrons as shown in the picture.
1. Aufbau's Principle. The electrons of an element should be filled up from the highest energy level. You can use the periodic table as a guide for this. In decreasing order, the energy of the orbitals are 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d and 7p. Each 'box' of these orbital must be filled with two electrons from 1s before moving on to the next.
2. Hund's rule. This states that you must fill all boxes of one orbital with one electron first. For example, 2p has 3 boxes. You fill one electron for each box first before going back to fill it to two electrons if there are still excess.
3. Pauli's Exclusion Principle. This states that no electrons of the same element should have the same quantum numbers. To achieve this, the two electrons in each box should have opposite spins, one facing up, and the other facing down.
Using these three rules, you will be able to draw the electronic configuration of Fluorine with 9 electrons as shown in the picture.