Cation are smaller & anions larger in radii than their parent atoms because there is a loss of electrons from valence shell in the case of cation ,so decreases the shell number and in the case of anion there is addition of electrons.
Q. Why is a positive ion smaller than an atom?
When an atom has its electrons attracted to another atom it becomes a positive ion. The positive ion is smaller than the original atom. This means that with fewer electrons but the same number of positive protons, the size of the ionic radius will decrease.
Table of Contents
- Q. Why is a positive ion smaller than an atom?
- Q. Why monovalent ions are smaller than parent atom?
- Q. How would you compare the sizes of anions and cations with their atoms?
- Q. How do you compare ion sizes?
- Q. Which element in each pair has a larger ionization energy?
- Q. Does Na or o have a larger ionization energy?
- Q. Why is there such a large jump in ionization energy between the second?
- Q. Which of the following has lowest ionization potential?
- Q. Which one of the following atoms has highest ionic potential?
Q. Why monovalent ions are smaller than parent atom?
Why monovalent ions (m+)are smaller than the parent atom ? 1. whereas,Radius of anion is greater than that of parent atom due to increase in no of shells and addition of electrons cause electron electron repulsion because of which size expands.
Q. How would you compare the sizes of anions and cations with their atoms?
Cations are always smaller than the neutral atom and anions are always larger.
Q. How do you compare ion sizes?
Ions aren’t the same size as the atoms they come from. Compare the sizes of sodium and chloride ions with the sizes of sodium and chlorine atoms. Positive ions are smaller than the atoms they come from. Sodium is 2,8,1; Na+ is 2,8.
Q. Which element in each pair has a larger ionization energy?
Which element in each pair has the larger first ionization energy? Sodium has the larger first ionization energy and in the second pair, Phosphorus has the largest first ionization energy.
Q. Does Na or o have a larger ionization energy?
Periodic Trends — Ionization Energy
1A | 6A | |
---|---|---|
1 | H 1312 | |
2 | Li 513 | O 1314 |
3 | Na 496 | S 1000 |
4 | K 419 | Se 941 |
Q. Why is there such a large jump in ionization energy between the second?
The third ionization energy is even higher than the second. Successive ionization energies increase in magnitude because the number of electrons, which cause repulsion, steadily decrease. This is not a smooth curve There is a big jump in ionization energy after the atom has lost its valence electrons.
Q. Which of the following has lowest ionization potential?
Down in a group ionization potential decreases so, the ionization potential of sulphur is lower than the oxygen. So, sulphur has the lowest ionization potential among all four. Therefore, option (C) sulphur is correct.
Q. Which one of the following atoms has highest ionic potential?
sodium