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# Which one has greater size potassium or sodium?

## Which one has greater size potassium or sodium?

K+ is larger than Na+ because the ionic radius increases in a particular group on moving from top to bottom due to increase in the principle energy shell though the number or electrons in the valence shell remain the same.

## How does the atomic radius of potassium?

Potassium, K Its atomic radius is 0.235 nm and the (+1) ionic radius is 0.133 nm. In the solid state Potassium has a body-centered cubic crystal structure with a = 0.533 nm and a nearest neighbor distance of 0.277 nm.

Which is larger sodium or potassium why?

Potassium is placed below sodium in group 1. It therefore has one more electron shell. So potassium atom is bigger than sodium atom.

What is the atomic radius of sodium?

227 pm

### Why is the atomic radius of potassium larger than sodium?

As an example, potassium (K) has a larger average atomic radius (220 pm)than sodium (Na) does (180 pm). The potassium atom has an extra electron shell compared to the sodium atom, which means its valence electrons are further from the nucleus, giving potassium a larger atomic radius.

### Why Na is greater in atomic size than Na +?

Na+ is smaller than Na atom because: Sodium is a Group 1 element, so its only ionic state is Na+. Cations of a given element have a smaller radius than the neutral atom so that Na+ will decrease in size compared with the Na atom. Sodium atoms and sodium ions have the same number of protons.

Which statement best compares the atomic radius of a potassium atom with the atomic radius of a calcium atom?

Which statement best compares the atomic radius of a potassium atom and the atomic radius of a calcium atom? The radius of the potassium atom is bigger because of its larger nuclear charge.

Why does potassium have a larger atomic radius than sodium?

#### Why does the atomic radius increase down a group?

In general, atomic radius decreases across a period and increases down a group. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

How do you determine the atomic radius?

The radius of an atom can only be found by measuring the distance between the nuclei of two touching atoms, and then halving that distance. As you can see from the diagrams, the same atom could be found to have a different radius depending on what was around it.

Why is the atomic radius of hydrogen smaller than the atomic radius of potassium?

Across a period, atomic radius decreases from left to right. Explain why the atomic radius of hydrogen is so much smaller that the atomic radius for potassium. K^+ is smaller in size than K because it has one less electron. Cl^- is larger than Cl because it has one additional electron.

## Which is larger in atomic radius sodium or potassium?

As we can see, only Potassium has four electron shells, therefore Potassium has the largest atomic size. Interestingly enough, Sodium has a larger atomic radius then magnesium, despite having less electrons and protons. Why does manganese have a larger atomic radius?

## What’s the difference between the density of potassium and sodium?

It has a bright silvery luster. One surprising fact is that though density of substances increase with an increase in their atomic number, Sodium is denser than Potassium even though the atomic number of sodium is only 11 while that of potassium is 19. Alkali metals are known to be reactive,…

Why is the ionization potential of sodium higher than potassium?

The correct option is iii) Higher ionization potential. The potential energy of Sodium is higher than Potassium because of the smaller atomic size. Sodium has three orbits, and potassium has four orbits. Lesser the distance of orbits from the nucleus, the higher the energy is required to remove the outermost electron, and vice versa.

Which is more affected by shielding potassium or sodium?

Hence, the ionization energy of sodium is higher. The electron in Potassium is also more affected by shielding due to more shells, further weakening this attraction. This means that less energy is needed to remove the outermost electron, and therefore, the ionisation energy is lower.