what is higher ionization enthalpy?
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Electrons removed from more highly charged ions of a particular element experience greater forces of electrostatic attraction; thus, their removal requires more energy. ... Ionization energy is also a periodic trend within the periodic table organization.
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Heya....❤❤❤
here is ur answer...
Ionization enthalpy of elements refers to the total quantity of energy essential for an isolated gaseous atom to lose an electron in its ground state.
Losing of electrons results in the formation of cations.
It is measured in units of electron volts (eV) per atom or kilocalorie per mole or kilojoules per mole.
1 electron volt is the energy obtained by an electron while moving under a potential difference of 1 volt.
The first ionization energy of an element (for example, element A) is defined as the energy required by an atom to form A+ ions. The unit of ionization energy is given as KJ mol-1.
A (g) → A+ (g) + e–
Correspondingly, the second ionization energy is illustrated as the energy which is needed to remove the second electron from its valence shell. It can be understood by the equation given below:
A+ (g) → A2+ (g) + e–
every time an electron is removed from an atom, a definite amount of energy is required to remove it, for this reason, the ionization enthalpies of chemical elements are constantly positive.
The second most outer electron will be more attracted to the nucleus than the first outer electron. As a result, the second ionization energy will be greater than the first ionization energy.
Correspondingly, the third ionization enthalpy will be greater than the second one.
hope it helps...
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here is ur answer...
Ionization enthalpy of elements refers to the total quantity of energy essential for an isolated gaseous atom to lose an electron in its ground state.
Losing of electrons results in the formation of cations.
It is measured in units of electron volts (eV) per atom or kilocalorie per mole or kilojoules per mole.
1 electron volt is the energy obtained by an electron while moving under a potential difference of 1 volt.
The first ionization energy of an element (for example, element A) is defined as the energy required by an atom to form A+ ions. The unit of ionization energy is given as KJ mol-1.
A (g) → A+ (g) + e–
Correspondingly, the second ionization energy is illustrated as the energy which is needed to remove the second electron from its valence shell. It can be understood by the equation given below:
A+ (g) → A2+ (g) + e–
every time an electron is removed from an atom, a definite amount of energy is required to remove it, for this reason, the ionization enthalpies of chemical elements are constantly positive.
The second most outer electron will be more attracted to the nucleus than the first outer electron. As a result, the second ionization energy will be greater than the first ionization energy.
Correspondingly, the third ionization enthalpy will be greater than the second one.
hope it helps...
plzz mark me as brainliest my dear !!!
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