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johncena
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How does atomic radii decrease when we move left to right in a periodic table? Though the nuclear charge increase as a result of increase in number of protons,the same increase is occurring in number of electrons.
Atomic radius is a measure of the size of an atom, specifically the distance from the nucleus to the outermost electron shell. It is typically measured in picometers (pm) or angstroms (Å).
Atomic radius is inversely proportional to nuclear charge. This means that as the number of protons in the nucleus increases, the atomic radius decreases. This is due to the increased attraction between the positively charged nucleus and the negatively charged electrons, causing the electron cloud to be pulled closer to the nucleus.
Atomic radius generally decreases from left to right across a period on the periodic table. This is because the number of protons and nuclear charge increases, while the number of electron shells remains the same. However, atomic radius increases from top to bottom down a group on the periodic table due to the addition of new electron shells.
Nuclear charge plays a major role in determining the chemical and physical properties of an element. As nuclear charge increases, the attraction between the nucleus and electrons increases, making the element more reactive. Additionally, elements with higher nuclear charge tend to have higher melting and boiling points, as well as higher densities.
Nuclear charge, or the number of protons in the nucleus, determines an element's position on the periodic table. As the number of protons increases, elements are placed in the next row or period on the periodic table. This also affects an element's properties and reactivity, as elements in the same period have similar characteristics.