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The reason the second ionization energy is higher than the first relates to the attraction between the electrons and the nucleus. When one electron is removed from an atom, the neutral atom becomes positive. When one attempts to remove a second electron from a positive ion, there is more attraction between the electrons and the nucleus due to the extra proton. Thus, the second electron is harder to remove and the ionization requires more energy.
What else can I help you with?
When one object causes a second object to resonate and the second object has absorbed from the first?
Resonance occurs when an object vibrates at the same frequency as another object, causing the second object to absorb energy from the first. This transfer of energy can lead to increased amplitude of vibrations in the second object, creating a phenomenon known as resonance.
How does energy efficiency relate to the first and second law of thermodynamics?
By the first law of thermodynamics, energy is conserved - i.e. the sum of the useful work and the energy lost to heat will equal the energy you started with. The second law states that you will never get 100% energy efficiency.
Why does helium has a higher first ionization energy than argon?
The ionisation energy depends on the orbital from which the electron is removed and also the distance of the orbital from the nucleus. In the case of Helium, the electron is removed from 1s orbital whereas in the case of argon it is from 3p orbital. As 1s is closer to the nucleus, the force of attraction experience by these electrons is higher and hence helium will have higher 1st ionisation energy.
First ionisation energy equation?
The equation for first ionization energy is the equation for the energy required to remove an electron from one mole of gaseous atoms to produce a mole of gaseous ions. It is as follows: X(g) ---> X^+1(g) + e^-1.
What are the laws of energy conversion?
Those would basically be the First and Second Laws of Thermodynamics. The First Law (energy conservation) states that the total energy can not be increased or decreased. The Second Law imposes some limitations about what conversions are possible.
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.
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.
Why ismthe second ionisation energy greater than first for lithium?
The second ionization energy for lithium is greater than the first because removing the second electron requires breaking a stronger bond due to the higher effective nuclear charge after the first electron is removed. This leads to a greater energy input to remove the second electron compared to the first.
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.
What happens to the first ionisation energy of the elements as a period is crossed?
tinger tinger tales
Which Lewis structure represent an atom x in period 4 with the highest first ionisation energy?
. .x ..
What is the energy needed to remove electrons from an atom called?
ionization potential energy. but remember the atom must be neutral .
Why are the ionisation energy of isotopes the same?
The ionization energy of isotopes is the same because isotopes have the same number of protons in their nucleus, which determines the ionization energy. Isotopes differ in the number of neutrons they possess, but neutrons do not contribute significantly to the ionization energy compared to protons.
Why does Be have a much larger second ionization energy than the first?
The energy to remove 1 electron is the first ionization energy. To remove a second electron requires more energy. This is because the electron being removed now has to overcome the +1 positive charge introduced after the 1st electron was removed.
What is the relationship between ionization energy and the alkali metals?
There is no relation ship. They have the lowest ionization energies.
Why boron has a lower first-ionization energy than beryllium?
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
