K+
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.
The order is: O, Cl, Sb, Rb, Ar.
To balance the equation Rb(s) + Cl2(g) → RbCl(s), you need to ensure that the number of atoms of each element is the same on both sides. Since Cl2 has two chlorine atoms, you need two rubidium chloride (RbCl) units to balance the chlorine. Therefore, the balanced equation is 2 Rb(s) + Cl2(g) → 2 RbCl(s), making the coefficient for rubidium (Rb) 2.
To balance the equation Rb(s) + Cl2(g) → RbCl(s), we need to ensure that the number of atoms for each element is the same on both sides. Since one molecule of Cl2 contains two chlorine atoms, we need two rubidium atoms to react with it. Therefore, the balanced equation is 2 Rb(s) + Cl2(g) → 2 RbCl(s), making the coefficient for rubidium (Rb) equal to 2.
The oxidation number of Rb is 1.
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.
Potassium's atomic radius is smaller than rubidium's because potassium has fewer energy levels of electrons.
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.
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.
Rb
c. Rb plus. Kr has 36 electrons, the same as Se2-, As3+, Sr2+, and Br-. Rb plus has 35 electrons, which is not isoelectronic with Kr.
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.
Smallest to largest is going down the group 1. I.e. Li is smallest<Rb<Cs
Rubidium has an atomic radius of 248 picometers.
Xe has a larger atomic radius than Rb because atomic radius generally increases from top to bottom within a group in the periodic table. Xe is located below Rb in the periodic table, so it has more electron shells, resulting in a larger atomic radius.
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.
A potassium atom has 19 protons and 19 electrons, plus 20-22 neutrons. A rubidium atom has 37 protons and 37 electrons, plus 46-50 neutrons and so is bigger.