Which statement best relates an empirical formula with a molecular formula?
1 answer:
You might be interested in
Answer:
Explanation:
Although the context is not clear, let's look at the oxidation and reduction processes that will take place in a Fe/Sn system.
The problem states that anode is a bar of thin. Anode is where the process of oxidation takes place. According to the abbreviation 'OILRIG', oxidation is loss, reduction is gain. Since oxidation occurs at anode, this is where loss of electrons takes place. That said, tin loses electrons to become tin cation:
Similarly, iron is cathode. Cathode is where reduction takes place. Reduction is gain of electrons, this means iron cations gain electrons and produce iron metal:
The net equation is then:
However, this is not the case, as this is not a spontaneous reaction, as iron metal is more reactive than tin metal, and this is how the coating takes place. This implies that actually anode is iron and cathode is tin:
Actual anode half-equation:
Actual cathode half-equation:
Actual net reaction:
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.