- Is S or s2 bigger?
- Which has a larger atomic radius Al or al3+?
- Which is larger fe2+ or fe3+?
- Why is Na+ larger than mg2+?
- Which is larger Cl or Ar?
- Does ionic size increase down a group?
- Why is fe3 more reactive than fe2?
- Why is F bigger than Na+?
- Why is fe3+ more stable than fe2+?
- Which is larger k or k+?
- Is mg2+ bigger than o2?
- Are K and Cl Isoelectronic?
- Which is smaller Au+ or au3+?
- Which ion is expected to be the largest?
- What is ionization energy trend?
- Why is p3 larger than al3+?
- What is isoelectronic with al3+?
- Which is smaller mg2+ or al3+?
Is S or s2 bigger?
(ii) Explain why the radius of the S2- ion is larger than the radius of the S atom.
The nuclear charge is the same for both species, but the eight valence electrons in the sulfide ion experience a greater amount of electron-electron repulsion than do the six valence electrons in the neutral sulfur atom..
Which has a larger atomic radius Al or al3+?
(b) Al has the larger radius. Al3+ has lost 3 electrons / valence shell. This means that there is one less energy level than in Al. The remaining electrons are drawn closer by nuclear charge / nuclear attraction greater causing smaller size.
Which is larger fe2+ or fe3+?
Fe2+ is greater in size than Fe3+. … Fe3+ ionic radius is 63 pm, while Fe2+ has an ionic radius of 77 pm. (For comparison, the Fe atom has a radius of 140 pm). This is because the outermost electron in the Fe2+ ion is pulled off to form Fe3+ ion.
Why is Na+ larger than mg2+?
Hence, Na+ will be larger in size. Deduce which of Na+ and Mg2+ is thesmaller ion. … mg2+ would be the smaller ion this isbecause each ion has the same number of electrons however mg2+ has a greater number of protons and therefore is more charge dense and the outer electrons feel a greater pull from the nucleus.
Which is larger Cl or Ar?
Cl- has the same number of electrons as Ar, but it has less protons, so less of a positive charge pulling those electrons to the nucleus, so will has a larger radius.
Does ionic size increase down a group?
As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. Ionic radius decreases moving from left to right across a row or period. … While the atomic radius follows a similar trend, ions may be larger or smaller than neutral atoms.
Why is fe3 more reactive than fe2?
Fe3+ is more reactive since it has a higher valency state. It depends. In an oxidative solution, Fe2+ will be. … Fe3 is more stable than Fe2, so Fe2 is more reactive than Fe3.
Why is F bigger than Na+?
F atomic number is 9 having 9-electrons & 9-protons. … So in that cases of Na+, F-, Na+ is less in size due to electron-proton attraction but F- is greater in size due to electron-electron repulsion as compared to electron-proton attraction. .
Why is fe3+ more stable than fe2+?
Fe3+ ion is more stable due to its half-filled 3d5 electron configuration. As half filled and completely filled shells are more stable Fe3+ ion is more stable. While Fe2+ is not stable.
Which is larger k or k+?
The size of the potassium ion depends on the location of the single electron, present on fourth energy level which is the highest, from the nucleus. The K+ ion has its outermost electrons on the third energy level now and is size is smaller than that of K ion. Hence, K is larger than K+.
Is mg2+ bigger than o2?
O2- will have larger atomic size. O2- has 10 electrons and 8 protons, while Mg+ has 10 electrons and 12 protons. As in Mg+ number of protons is more that compared to O2- the attraction force between the nucleus and the electrons will increase and the atom of Mg2+ will get shrink and hence has smaller atomic size.
Are K and Cl Isoelectronic?
Potassium has an atomic number of 19 (Z = 19). … And we can see that the potassium ion, K+, has the same electronic configuration as the chloride ion, Cl-, and the same electronic configuration as an atom of argon, Ar. Therefore, Ar, Cl-, and K+ are said to be isoelectronic species.
Which is smaller Au+ or au3+?
Answer: Au+ or Au3+: Au3+ is smaller than Au+ for the same reason as part (b).
Which ion is expected to be the largest?
The periodic is arranged in the order of increasing proton number. Phosphorus comes the first among the four species and contains the least number of protons. Its ion would be the largest among the four.
What is ionization energy trend?
The general trend is for ionization energy to increase moving from left to right across an element period. Moving left to right across a period, atomic radius decreases, so electrons are more attracted to the (closer) nucleus.
Why is p3 larger than al3+?
All three ions have the same number of electrons, but P3- has the fewest number of protons, so it has the least positive nucleus out of the three atoms. Therefore, it will be the largest. Use that logic to determine the relative sizes of the remaining two anions.
What is isoelectronic with al3+?
6. Make life easier by first sorting them into Periodic Table order: N3- O2- F- Na+ Mg2+ Al3+ These are all isoelectronic with the structure 2,8. The smallest ion will be the one with the largest number of protons – Al3+; the biggest, the one with the least protons – N3-.
Which is smaller mg2+ or al3+?
As they have equal number of electrons the electrons are not involving in determination of atomic radius. Hence atomic radius is totally depended on effective nuclear charge. Therefore radius of Al3+ is less than Mg2+.