how do you compare the outermost electrons with the inner electronsof an atom in terms of energy.
It requires more energy to remove an inner electron than it does to remove an outer electron.
i don't know
No problem! I'm here to help. When comparing the energy levels of the outermost electrons (also called valence electrons) with the inner electrons of an atom, it's important to understand the concept of electron shells or energy levels.
In an atom, electrons are organized into different energy levels or orbitals. The innermost energy level is closest to the nucleus and contains the inner electrons, while the outermost energy level contains the valence electrons.
To compare the energy of the valence electrons with the inner electrons, you need to consider the concept of electron shielding. Electron shielding occurs because the inner electrons repel the outer electrons, reducing the overall attraction between the positively charged nucleus and the valence electrons.
As a result, it requires less energy to remove an outer electron than it does to remove an inner electron. This is because the valence electrons experience weaker electrostatic attraction to the nucleus due to the shielding effect of the inner electrons. Removing an outer electron disrupts fewer interactions and requires less energy input compared to removing an inner electron, which is surrounded by other electrons and experiences stronger electrostatic forces.
In terms of energy, the outermost electrons are higher in energy compared to the inner electrons. They are further away from the nucleus and experience weaker attractive forces.
To summarize, the outermost electrons (valence electrons) have higher energy levels and are more easily removed because they are shielded by the inner electrons. Whereas, the inner electrons are closer to the nucleus and experience stronger attractive forces, making them more difficult to remove and requiring more energy.