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Examples are: Be, Al, Ti, V, Mn, Co, Ni etc.
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What element has a smaller ionic radius than magnesium?
Examples are: Be, Al, Ti, V, Mn, Co, Ni etc.
What happens to an atomic radius when an electrons is lost?
The positive ionic radius is smaller than the neutral atomic radius
Why is the ionic radius of a group 2 elemnt smaller than its atomic radius?
The ionic radius of a Group 2 element is smaller than its atomic radius because, when these elements form cations (specifically, (M^{2+}) ions), they lose two electrons from their outermost shell. This loss of electrons results in a reduced electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus, thus decreasing the size of the ion compared to the neutral atom. Additionally, the effective nuclear charge experienced by the remaining electrons increases, further contributing to the smaller ionic radius.
What element has a larger ionic radius than sulfur (S)?
Chlorine (Cl) has a larger ionic radius than sulfur (S) when comparing their anions, specifically the chloride ion (Cl⁻) and the sulfide ion (S²⁻). The ionic radius of Cl⁻ is approximately 181 picometers, while the ionic radius of S²⁻ is about 184 picometers. Additionally, phosphorus (P) in its anionic form (P³⁻) also has a larger ionic radius than sulfur.
What is smaller than the atomic radius of beryllium (Be)?
Generally, any element with a lower atomic number.
What element has a larger ionic radius than sulfur?
Potassium has a larger ionic radius than sulfur.
What element has a smaller ionic radius than magnesium?
Examples are: Be, Al, Ti, V, Mn, Co, Ni etc.
Which element has a larger ionic radius than sulfur?
Phosphorus has larger ionic radius than sulfur. There is more nuclear attraction in sulfur.
What happens to the atomic radius when an electron is lost?
the positive ionic radius is smaller than the neutral atomic radius
What happens to an atomic radius when an electrons is lost?
The positive ionic radius is smaller than the neutral atomic radius
Why is the ionic radius of a group 2 elemnt smaller than its atomic radius?
The ionic radius of a Group 2 element is smaller than its atomic radius because, when these elements form cations (specifically, (M^{2+}) ions), they lose two electrons from their outermost shell. This loss of electrons results in a reduced electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus, thus decreasing the size of the ion compared to the neutral atom. Additionally, the effective nuclear charge experienced by the remaining electrons increases, further contributing to the smaller ionic radius.
What element has a larger ionic radius than sulfur (S)?
Chlorine (Cl) has a larger ionic radius than sulfur (S) when comparing their anions, specifically the chloride ion (Cl⁻) and the sulfide ion (S²⁻). The ionic radius of Cl⁻ is approximately 181 picometers, while the ionic radius of S²⁻ is about 184 picometers. Additionally, phosphorus (P) in its anionic form (P³⁻) also has a larger ionic radius than sulfur.
Is the atomic radius generally smaller than the ionic radius of a non metal?
yeshttp://answers.yahoo.com/question/index?qid=20071116151305AAT0Lz3
Which element has a larger ionic radius than calcium?
An element that has a larger ionic radius than calcium is strontium. Strontium is located below calcium in the same group of the periodic table, which means it has an extra energy level and therefore a larger ionic radius.
What is the ionic radius of Mg2 and how does it compare to other ions in the same group on the periodic table?
The ionic radius of Mg2 is smaller than that of other ions in the same group on the periodic table.
What elements have an ionic radius equal to the atomic radius?
a) Sc,Ti,V,Crb) Na,K,Rb,Csc) B,Si,As,Ted) F,Cl,Br,Ie) Na,Mg,Al,SiThe correct answer of these options is a) Sc,Ti,V,Cr because they are the closest elements to each other in the periodic table.
Is Li have the smallest ionic radius?
No, H+ ions are the smallest (proton size), hydrogen atoms and even Li+ ions are smaller than Li atoms.
