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Is isotopes have same ionisation enthalpy?
yes, it is correct.
Would you expect the first ionisation enthalpy for two isotopes of the same element to be same or different?
This value is identical for isotopes.
What is 1st ionisation enthalpy?
it is the energy required for a mole of atom to loose a mole of electron.
Ionisation energy of noble gases?
Noble gases have high ionization energies due to their stable electron configurations and full outer electron shells. This makes it difficult to remove an electron from them compared to other elements. The ionization energy generally increases from helium to radon within the noble gas group due to increasing nuclear charge.
Is the ionization energy of alkali metals larger or smaller than the alkaline earth metals in the same period?
It is about first ionization energy. It is less than alkaline earth metals.
Is isotopes have same ionisation enthalpy?
yes, it is correct.
Would you expect the first ionisation enthalpy for two isotopes of the same element to be same or different?
This value is identical for isotopes.
How can you relate ionisation potential and ionisation energy?
Ionisation potential and ionisation energy are essentially the same concept - they both refer to the amount of energy required to remove an electron from an atom or molecule. The terms are often used interchangeably in practice.
How does the ionisation energy change down the groups in the periodic table?
Ionisation energy decreases down the group. It is easy to remove an electron.
What is ionisation energy What is first ionisation energy?
The first ionization energy of an atom or molecule describes the amount of energy required to remove an electron from the atom or molecule in the gaseous state.
First ionisation energy?
the first ionisation energy is the energy required to remove the first most loosely bound elecctron from a neutral gaseous atom in its ground state.
When does ionisation energy increases?
when we go from left to right
Who ionisation energy differs?
Ionisation energy differs between elements due to variations in the number of protons in their nucleus, which affects the strength of the attraction between the electrons and the nucleus. Elements with higher atomic numbers typically have higher ionisation energies due to increased nuclear charge. Additionally, ionisation energy generally increases across a period and decreases down a group on the periodic table.
What is the energy required to move an electron up an energy level called?
Ionisation energy, or alternatively quantum energy.
Why is the first ionisation energy of strontium larger than the first ionisation energy of rubidium?
Because, as we know that when we go across the period of the periodic table, the number of shells remain the same but the number of electrons and protons increases. So, Rb having its atomic number as 37 and Sr as 38, Strontium has got more nuclear charge as well as more electrons. As a result the first ionisation energy required to remove one electron is more in Strontium than Rubidium.
What is 1st ionisation enthalpy?
it is the energy required for a mole of atom to loose a mole of electron.
How are isotopes the same?
How isotopes same as element alike?
