Table of Contents
- 1 Why does Na+ have a smaller radius?
- 2 Why is the ionic radius of K+ greater than that of Na+?
- 3 Why does the atomic radius get smaller?
- 4 Why is the radius of an Na atom larger than the radius of an Na+ ion?
- 5 Why does ionic radius decrease across a period?
- 6 Does K+ have a small radius?
- 7 Does NA 1 or K 1 have a larger radius?
- 8 Why does the atomic radius get larger as we move down a group but smaller as we move across a period?
- 9 Why is the atomic radius of Krypton smaller than potassium?
- 10 Why does potassium have a greater atomic radius than calcium?
Why does Na+ have a smaller radius?
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. Each one has 11 protons.
Why is the ionic radius of K+ greater than that of Na+?
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.
Which element has the largest atomic radius Na or K?
Answer: Potassium (K) with an atomic number of 19 has the largest atomic radius. This is because sodium and potassium are elements of group 1. On moving from top to bottom in a group, the atomic radius increases.
Why does the atomic radius get smaller?
In general, atomic radius decreases across a period and increases down a group. A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius.
Why is the radius of an Na atom larger than the radius of an Na+ ion?
HIGHLIGHT TO SEE THE ANSWER The ion has 1 less energy level than the atom. A sodium atom loses the electron in its outer shell, causing the radius of the ion to be smaller than the radius of the atom. An Na atom has three electron shells, but an Na+
Does Na+ have a larger radius?
And since they accept electrons, the ionic radius of the ANION, should be LARGER than the parent atom. And in fact many Periodic properties may be rationalized on this contest between nucular charge, and shielding by other electrons. And so to your question, finally! Na+ is smaller than Na ; and Cl− is larger than Cl .
Why does ionic radius decrease across a period?
Ionic radius decreases moving from left to right across a row or period. More protons are added, but the outer valence shell remains the same, so the positively charged nucleus draws in the electrons more tightly. While the atomic radius follows a similar trend, ions may be larger or smaller than neutral atoms.
Does K+ have a small radius?
K+ has a bigger effective nuclear charge than Cl−, which translates to a bigger net positive charge felt by the outermost electrons. This will compress the energy levels a bit and make the ionic radius smaller for the potassium cation.
Which is smaller Na or K?
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.
Does NA 1 or K 1 have a larger radius?
If you look at elements that are located in the same group, potassium will have a larger atomic radius when compared with sodium.
Why does the atomic radius get larger as we move down a group but smaller as we move across a period?
On the periodic table, atomic radius generally decreases as you move from left to right across a period (due to increasing nuclear charge) and increases as you move down a group (due to the increasing number of electron shells). …
Why does the K + ion have a smaller radius than Na +?
It actually does not. K+ has a larger atomic radius than Na+. The Periodic Table is accompanied by many trends. One such trend involves the atomic radius for these elements. As you go down the periodic table, the atomic radius increases which is why K+ has a larger radius… it’s below Na+.
Why is the atomic radius of Krypton smaller than potassium?
Consequently, there is more Coulomb force attracting the valence electrons of krypton than there is attracting the valence electron of potassium; accordingly, the atomic radius of krypton is smaller than the atomic radius of potassium. Is that correct? Your concept is close to the real answer.
Why does potassium have a greater atomic radius than calcium?
Potassium (K) has a greater atomic radius than that of Calcium (Ca) because when we move down a group, the atomic radius increases and when we move from left to right in a period, the atomic radius decreases. Both potassium and calcium belong to the 4th period in the periodic table of chemical elements.
Why is the radius of d orbital greater than kr?
Due to the poor shielding effect, of “d” orbital of” Kr” so the “z”effect is increase and radius is decrease but in “K” no poor shielding effect so it’s radius is greater than “Kr” Thanks for contributing an answer to Chemistry Stack Exchange!