Question

For which of these elements would the first ionization energy of the atom be higher than that of the diatomic molecule? helium oxygen carbon lithium please explain why and thanks

Answer 1

The first ionization energy for helium (He) will be higher than that of the diatomic molecule.

FURTHER EXPLANATION

Ionization energy is the amount of energy needed to remove a valence electron from a gaseous atom.

Ionization energy depends on the strength of attraction between the valence electron and the nucleus and the stability of the atom.

Strength of Attraction between Valence Electron and Nucleus

The more attracted the valence electron is to the nucleus, the more difficult it would be to remove it. It would require more energy, therefore, making the ionization energy higher.

• Bigger atoms tend to have lower ionization energies since their valence electrons are farther from the nucleus which decreases the attraction.

• When atoms have the same number of electron shells, the atom with more electrons are smaller because of the increased attraction of the valence electrons to the nucleus . The ionization energy becomes higher.

Stability of the Atom

A stable atom is unreactive. It is in a state which allows it to exist on its own and does not require any further addition or loss of electrons. Its electron shells are filled to capacity. To remove a valence electron will destabilize the atom. This would require a lot of energy as it opposes the nature of atoms - they tend to lose or gain electrons to have a fully filled valence shell. Losing an electron from a filled shell will be unfavorable and result in  a high ionization energy.

Examples of stable atoms are the noble gases (Group 18).

Helium, therefore, will have the greatest ionization energy since it is much smaller than all the other given atoms  and it is a noble gas. Lithium is biggest atom among the choices, hence, it will gave the lowest ionization energy.

LEARN MORE

1. Electron Affinity brainly.com/question/11302894
2. Electronegativity brainly.com/question/2552510
3. Atomic Radius brainly.com/question/862779

Keywords: ionization energy, periodic trends

Answer 2

The first ionization energy of the element will be highest for$\boxed{{\mathbf{helium}}}$ atom than it’s diatomic${\text{H}}{{\text{e}}_2}$.

Further explanation:

Ionization energy:

Ionization energy is defined as the amount of energy that is required to remove the most loosely bound valence electrons from the isolated neutral gaseous atom. It is denoted by IE. The value of IE is related to the ease of removing the outermost valence electrons.

The elements whose electronic configuration contains one or more electrons more than the valence shell of a noble gas can easily remove their valence electrons by even a small amount of energy. Hence the ionization energy associated with such element is least.  

The numbers of electrons present in the valence shell determine whether the ionization energy will be low or high. The electronic configuration of helium is  .it has already fully filled electronic configuration. All the electrons are paired. So it cannot remove any electron howsoever high energy is provided.

The electronic configuration of lithium is${\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^1}$. It has one additional electron that can be removed so its first ionization energy is low. The lithium-ion thus formed can readily combine with lithium cation and form dilithium.

The electronic configuration of carbon is ${\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{p}}^2}$.It can also lose electron as the electrons present in 2s are relatively loosely held compared to the electrons in 2s subshell. It has been found that energy of nearly $1086.4{\text{ kJ/mol}}$is required to ionize the first electron out of carbon.

The electronic configuration of oxygen is ${\mathbf{1}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{2}}{{\mathbf{p}}^4}$.It can also lose electron as the electrons present in 2s are relatively loosely held compared to the electrons in 2s subshell. It has been found that energy of nearly $1313.9{\text{ kJ/mol}}$is required to ionize the first electron out of carbon.

Therefore the electron that is removed with most difficulty is helium.

Learn more:

1. The subatomic particle with the least mass: brainly.com/question/2224691

2. Oxidation and reduction reaction: brainly.com/question/2973661

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Periodic classification of elements

Keywords: Periodic properties atomic structure groups, periods, periodic law chemical properties ionization enthalpy, electronegativity,atomic radii, effective nuclear charge, valence shell, electronic configuration.