1s², 2s², 2p⁴
Electronic configuration is the distribution of electrons of an atom in atomic orbitals. As we know Oxygen is a non metal and is present in group 6 and period 2 with atomic number 8. The atomic number in fact specifies the number of protons. Hence, for a neutral oxygen atom there must be 8 electrons to balance the charges of protons.
These 8 electrons are distributed in two main energy levels i.e. n = 1 and 2 and sub energy levels i.e. s and p. According to certain rules like Aufbau Principle, Pauli's Exclusion Principle and Hund's Rule the electronic configuration for eight electrons is as,
1s², 2s², 2px², 2p¹, 2p¹
The electronic configuration for oxygen is 1s2 2s2 2p4.
The electron configuration for oxygen is 1s2 2s2 2p4.
In the electron configuration, the numbers represent the energy levels (1s, 2s, 2p), and the superscripts represent the number of electrons in each orbital. The electron configuration follows the Aufbau principle, which states that electrons fill the lowest energy levels first.
In the case of oxygen, there are 8 electrons in total. The first two electrons fill the 1s orbital, the next two fill the 2s orbital, and the remaining four fill the 2p orbital (with two electrons each in the three 2p orbitals).
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Heavy metals are located on the lower part of the periodic table, specifically in the d-block and f-block elements.
In the periodic table, heavy metalsare found in the d-block and f-block, at the bottom. Elements in the d-block, or transition metals, span groups 3 through 12 in the periodic table. Metals like iron, copper, and zinc are included in this category.
The f-block elements, which comprise the lanthanides and actinides, may be found at the very end of the periodic table and are referred to as the inner transition metals. Due to their large atomic weights and high densities, elements like uranium and plutonium are classified as heavy metals.
Learn more about heavy metals, here:
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