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Rubidium has one valence electron in the 5th energy level, while strontium has two valence electrons in the 5th energy level. Since rubidium has only one valence electron compared to strontium's two, the valence electron in rubidium is further from the nucleus. This is due to the increasing number of electron shells as you move down a group in the Periodic Table.
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Why does rubidium have a smaller ionization energy than iodine?
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.
Why is it easier for strontium to lose valence electrons than calcium?
Strontium is larger in size compared to calcium due to more electron shells, making it easier for strontium to lose valence electrons farther from the nucleus. This results in weaker attraction between the valence electrons and the nucleus, leading to easier electron loss in strontium compared to calcium.
Where is the lowest electronegativity barium calcium magnesium or strontium?
Both are ions and we should consider the ionic radius, not the atomic radius. Rubidium ion (Rb+) will have a larger IONIC radius than strontium ion (Sr2+). Both ions have the same electronic configuration. But strontium ion has more number of protons in the nucleus. Hence it will have greater force of attraction between the nucleus and the valence electrons, resulting in smaller size.
In an atom an electron that is close to the nucleus is on the highest enegry level?
No. The greater distance from the nucleus the more energy an electron has.
Who said that the further an electron was from the nucleus the higher its energy?
The statement that an electron's energy increases with its distance from the nucleus is associated with Niels Bohr, who developed the Bohr model of the atom in 1913. In this model, electrons occupy quantized energy levels, and as an electron moves further from the nucleus, it occupies higher energy states. This concept is fundamental to understanding atomic structure and electron behavior in quantum mechanics.
What particle is emitted when rubidium-87 converts to strontium-87?
When rubidium-87 (Rb-87) converts to strontium-87 (Sr-87), it undergoes beta decay. In this process, a neutron in the rubidium nucleus is transformed into a proton, resulting in the emission of an electron, known as a beta particle, and an antineutrino. This transformation increases the atomic number from 37 (rubidium) to 38 (strontium) while the mass number remains the same at 87.
How does electron shielding explain why it is easier to remove an electron from rubidium than from lithium?
In rubidium, having a larger atomic radius, the attraction force between the atomic nucleus and and the electron from outermost shell is lower.
Why does rubidium have a smaller ionization energy than iodine?
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.
Why is it easier for strontium to lose valence electrons than calcium?
Strontium is larger in size compared to calcium due to more electron shells, making it easier for strontium to lose valence electrons farther from the nucleus. This results in weaker attraction between the valence electrons and the nucleus, leading to easier electron loss in strontium compared to calcium.
Why cesium has a lower first ionization energy then rubidium?
Caesium 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. But that's not just the answer. There is also a thing called electron shielding, the negative charges, of the electrons in the energy levels closer to the nucleus, sort of repel the outer electrons so they can't get closer to the nucleus. Since the electrons are further away and have the attraction from the positively charged nucleus reduced, it takes less energy to break the attraction for caesium than rubidium.
Which electron is on average further from the nucleus an electron in a 3p orbital or an electron in a 4p orbital?
An electron in a 2s orbital is on average closer to the nucleus.
What is the atomic radius of Rb?
Rubidium has an atomic radius of 248 picometers.
Will an electron feel a greater force when it is close to the nucleus or when it is further away?
further away :)
Where is the lowest electronegativity barium calcium magnesium or strontium?
Both are ions and we should consider the ionic radius, not the atomic radius. Rubidium ion (Rb+) will have a larger IONIC radius than strontium ion (Sr2+). Both ions have the same electronic configuration. But strontium ion has more number of protons in the nucleus. Hence it will have greater force of attraction between the nucleus and the valence electrons, resulting in smaller size.
Is a rubidium larger or smaller than a neutral atom?
A rubidium atom is larger than a neutral atom because, when it loses an electron to become an ion, it loses an electron from the outermost shell, increasing the effective nuclear charge which attracts the remaining electrons closer to the nucleus, reducing the size of the ion compared to the atom.
Would rubidium be reactive and lose one electron to form an ionic bond?
yes because rubidium has only 1 electron on the outer shell so is not stable and because is far away from the nucleus the attraction is weaker therefore is more likely to react faster with another atom and get stable
How does rubidium form an ion?
Rubidium forms a +1 cation (Rb+) by losing one electron to achieve a stable electron configuration. Rubidium has one valence electron in its outermost shell, so by losing this electron, it becomes a cation.
