I was out sick & am copying a friends notes from class. My question is what does e- stand for?
it easier to form a positive ion with a low ionization energy because a positive ion is formed by removing an e-(I think maybe electron)
and the other one is e-s?
The trend in ionization as you go down decreases because the shielding effect makes it easier to remove outer e-s from atoms with more e-s ( I think maybe electron shield) Thanks in advance
e- simpley stands for electron,
and e-s for electrons (plural)
Thank you!
In the context of your question, "e-" stands for electrons. Let me explain further.
Electrons are negatively charged particles that orbit around the nucleus of an atom. They play a vital role in various chemical processes, including the formation of ions.
When an atom gains or loses electrons, it becomes an ion. Positively charged ions (cations) are formed by losing electrons, while negatively charged ions (anions) are formed by gaining electrons.
In your first question, you mentioned that it is easier to form a positive ion with a low ionization energy. Ionization energy refers to the amount of energy required to remove an electron from an atom or ion. So, if an atom has a low ionization energy, it means that it takes less energy to remove an electron from that atom, making it easier to form a positive ion by removing an electron.
In your second question, you mentioned the trend of ionization decreasing as you go down the periodic table. This trend is attributed to the shielding effect. The shielding effect occurs because, as you move down the periodic table, there is an increase in the number of electron shells (energy levels) in an atom. The outermost electrons are shielded or partially protected by the inner electron shells, making it easier to remove the outer electrons since they experience less attraction from the positively charged nucleus. This, in turn, leads to a decrease in ionization energy as you move down the periodic table.
So, in summary, in both cases, "e-" refers to electrons. It's important to understand the role of electrons in ion formation and how factors like ionization energy and shielding affect the behavior of electrons in atoms.