In the context of atomic physics, the smallest radius for an atomic orbital is typically found in the hydrogen atom, where the radius is defined by the Bohr model. For the ground state (n=1), the Bohr radius is approximately 0.529 angstroms. In multi-electron atoms, the effective nuclear charge and electron-electron interactions can influence the size of the orbitals, but for a hydrogen-like atom (one electron), the smallest radius occurs at n=1.
K+
The atomic radius generally decreases across a period from left to right and increases down a group in the periodic table. Therefore, a sequence arranged in order of decreasing atomic radius might include elements like cesium (Cs), rubidium (Rb), and potassium (K). In this case, Cs would have the largest atomic radius, followed by Rb, and then K, illustrating the trend of increasing size down the group. Another example could be sodium (Na), magnesium (Mg), and aluminum (Al), where Na has the largest radius and Al the smallest.
When there is an anion (negative charge) the radius will be larger because it is more full whereas it will be smaller if it is a positive charge because of less electrons. ex largest to smallest radius (K-,K, K+)
Helium has the smallest covalent radius
Rubidium (Rb) is the largest element among lithium (Li), sodium (Na), and potassium (K). This is because, as you move down the alkali metal group in the periodic table, the atomic size increases due to the addition of electron shells. Therefore, Rb, being the heaviest and furthest down the group, has the largest atomic radius.
K+
Potassium's atomic radius is smaller than rubidium's because potassium has fewer energy levels of electrons.
Rb (rubidium) is the largest element among K (potassium), Rb (rubidium), Na (sodium), and Li (lithium). This is because as you move down a group in the periodic table, the atomic size increases due to the addition of more electron shells.
The species with the smallest atomic radius among K, Mg, Rb, and Ca is Rb (Rubidium). This is because atomic radius tends to decrease across a period from left to right in the periodic table, and Rb is located towards the right side of this group of elements.
Rb
Br is the atom with the smallest. K+ is the ion with the smallest radius. In general, the shape with the smallest radius has the smallest diameter
Rb > K > Na > Li. The order based on atomic size is Rb > K > Na > Li. Therefore, the size of the circles should reflect this order from largest to smallest.
The atomic radius generally decreases across a period from left to right and increases down a group in the periodic table. Therefore, a sequence arranged in order of decreasing atomic radius might include elements like cesium (Cs), rubidium (Rb), and potassium (K). In this case, Cs would have the largest atomic radius, followed by Rb, and then K, illustrating the trend of increasing size down the group. Another example could be sodium (Na), magnesium (Mg), and aluminum (Al), where Na has the largest radius and Al the smallest.
Ca, Mg, Be, Fr, Cs, Rb, K, Na, Li, H
The atomic radius of Sr (Strontium) is larger than that of Rb (Rubidium). This is because atomic radius generally increases down a group in the periodic table, and Sr is located below Rb in the same group.
The group of elements with members of the smallest atomic radii for a given period is the group of noble gases. Noble gases have the smallest atomic radii because they have a completely filled valence shell, which results in strong electron-electron repulsions and a smaller atomic size.
Smallest to largest is going down the group 1. I.e. Li is smallest<Rb<Cs