0
Strontium(Sr) lies to the right of rubidium(Rb) in the 5th period on the Periodic Table. Ionization energy (IE) increases as you go from left to right so Sr would have a higher IE than Rb. The actual reason for this is that both of them have their valence electrons in the 5th shell, so they are the same distance from the nucleus, however, Sr has more protons in the nucleus, and thus the attraction of these electrons is greater. Greater attraction means it takes more energy to remove them.
Wiki User
∙ 7y ago
Wiki User
∙ 7y agoBoth electrons being removed are in the 5s subshell so they experience the same amount of shielding from the nuclear pull. The strontium electron is being pulled away from a nuclear charge of +38 whereas the rubidium is being pulled away from a charge of =37, so less energy is required.
Wiki User
∙ 10y agothere are more protons in strontium therefore there is a greater attraction between the nucleus and the electrons resulting in a smaller atomic radius compared torubidium
Wiki User
∙ 11y agoCesium has more electron levels than rubidium, because the electrons are further away the attraction between the outer electrons and protons in the nucleus is less.
Wiki User
∙ 7y agoThe atomic radius of strontium is lower, the attraction between the nucleus and electrons is higher.
Add your answer:
Earn +20 pts
Does an atom of fluorine have larger or smaller radius than an atom of iodine?
Smaller
How might the size of the membrane pore compare to the size of the starch molecules?
In other words this question asks if the pores are bigger or smaller than the iodine molecules. So.... the answer is that the iodine are smaller than the pores and the pores are bigger, because the iodine molecules need room to pass through, and the pores are not selectively permeable because they let the iodine through.
How much energy is needed to melt 25.4grams of l2?
Iodine sublimes - it does not melt
Why is the radius of an atom of iodine greater than the radius of bromine atom?
An iodine atom has one more principal energy level than a bromine atom. Therefore the radius of an iodine atom is greater than the latter.
How much energy does iodine need to lose an electron?
1008.4 kJ mol-1
Which element in each pair has the greatest ionization energy fluorine or iodine?
The ionization energy of fluorine is 1681 kJ/mol (the first) and the ionization energy of iodine is 1008,4 kJ/mol.
Why does boron have a higher ionization energy than fluorine?
Because fluorine's size is lower than that of iodine, it has a greater ionization energy than iodine. Fluorine, on the other hand, appears to have a smaller shielding effect. As a result, fluorine's nucleus attracts more valence electrons than iodine's.
Balanced equation for rubidium and iodine?
what is the balanced equation for Rubidium metal reacting with halogen iodine
Can rubidium react with iodine?
Yes. Rubidium is an alkali metal in the sodium group. It will react with iodine to form rubidium iodide:- 2Rb+ I2 -> 2RbI
What is the empirical formula for iodine and rubidium?
The rubidium iodide is RbI.
Which element has a higher electronegativity value Rubidium or Iodine?
Iodine
When rubidium react with iodine which compound will make?
Rubidium metal would react with iodine to make rubidium iodide , according to the equation: 2 Ru + I2 -> 2 RuI
What is the compound name for Rbl?
Rubidium iodine
Is the ionization energy of chlorine higher than that of fluorine?
In the periodic table of elements, fluorine and iodine are in the same column, but fluorine is in the second, iodine in the fifth row. That means fluorine has only nine electrons flying around in orbitals while iodine has 53 of them. Ionization is the called a process during which a single electron is abstracted - we're now talking about the 1st ionization energy, which is much higher for fluorine. Well, as it only has nine electrons scattered in the orbitals (but according laws, of course), they do not really influence the repelling - attracting actions between the positive center and the other electrons beside them. For iodine with 53 electrons, they really do interfere with the attraction of other electrons AND as the outmost electrons (which are the ones taken away by ionization) are in those orbitals which are at the biggest distance to the center - for 53 electrons the outmost orbitals is at a much bigger distance... both results in a smaller attraction of the electrions at max distance from the center... so for iodine you need less energy to perform ionization.
Write equations that show the process for the first two ionization energies of tin?
The first ionization of tin is given as , Sn becomes Sn+1 and 1 e- . The amount of energy released is 708.6 kJ/mol . The second ionization reaction is Sn+1 becomes Sn+2 and 1 e- with 1411.8 kJ/mol energy released.
Does an atom of fluorine have larger or smaller radius than an atom of iodine?
Smaller
Could negative ion is formed when ionization occur in potassium iodine?
Question makes no sense.
