T he smallest first ionization energyis for lithium.
Within the alkali metals, or group 1, the ionization energy trend is that ionization energy decreases as you move down the group from top to bottom. This is because with each step down, you add an energy level, therefore the one valence electron is farther and farther from the atom's nucleus. So, the attraction between the nucleus and that electron (its electronegativity) decreases. This makes it easier (requires less energy), making the element more reactive. For example, cesium is more reactive than rubidium, which is more reactive than potassium, which is more reactive than sodium...
Barium has more energy levels. So it has lesser ionization energy.
There is no relation ship. They have the lowest ionization energies.
Yes. If the units are eV (electron volts) this is called ionization potential, if the units are kJ/mol then this ionization energy. The conversion between the units is:- 96.485 kJ/mol = 1 eV/particle) Historically it was always called ionization potential as that reflected the method of measurement.
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.
Potassium has the smallest first ionization energy among those elements listed. This is because potassium has the largest atomic size and the weakest attraction between its nucleus and outermost electron, making it easier to remove that electron.
No, cesium has a lower ionization energy than potassium. This is because cesium has a larger atomic size and a weaker attraction between the nucleus and the outermost electron compared to potassium.
Yes, rubidium and chlorine can bond together to form rubidium chloride. Rubidium will donate its valence electron to chlorine, resulting in the formation of an ionic bond between them.
The chemical formula for the compound formed between rubidium and oxygen is rubidium oxide - Rb2O.
Ionic bond is formed between rubidium and iodine, where rubidium donates its electron to iodine to complete its valence shell. Rubidium becomes a positively charged ion (cation) and iodine becomes a negatively charged ion (anion), resulting in the formation of an ionic compound, rubidium iodide.
A ionic bond forms between rubidium and iodine. Rubidium, a metal, donates its electron to iodine, a nonmetal, resulting in the formation of positively charged rubidium ions and negatively charged iodine ions that are then attracted to each other.
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.
The compound formed between rubidium and chlorine has the formula RbCl.
If you mean "What is the difference between rubidium and cesium?" then Rubidium and cesium are two different elements.They have similar properties but cesium is denser and has a higher atomic mass.Cesium also reacts more vigorously with water and air.
RbI (rubidium iodide) is an ionic compound because it is formed between a metal (rubidium) and a nonmetal (iodine). The attraction between the positively charged rubidium ion and the negatively charged iodide ion results in an ionic bond.
The relationship between radium and its ionization energy is that radium has a high ionization energy. This means that it requires a lot of energy to remove an electron from a radium atom.
Rubidium and oxygen typically form an ionic bond, where rubidium loses an electron to oxygen, resulting in the formation of rubidium cations and oxygen anions that are attracted to each other due to their opposite charges.