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How is the concept of effective nuclear charge used to simplify the numerous electron- electron repulsions in a many electron atom?
Wiki User
∙ 10y ago
a) How is the concept of effective nuclear charge used to simplify the numerous electron-electron repulsions in a many-electron atom?
Effective Nuclear Charge- the (net) positive charge experienced by an electron in a many electron atom. This charge is not the full nuclear charge. It accounts for the shielding of the nucleus by other electrons in the atom.
The nucleus is surrounded by electrons. These electrons are shielded from the nucleus by electron repulsions. The effective nuclear charge is less than the actual nuclear charge because the repulsions of the electrons needs to be taken into account.
This is done in the equation
Zeff = Z (protons) - S (screening constant, the inner core amount of electrons)
b) Which experiences a greater effective nuclear charge in a Be atom, the 1s electrons or the 2s electrons?
The 1s electrons would have a greater nuclear charge. The number of electrons between the 1s electrons and the nucleus is less than the number of electrons between the 2s electrons and the nucleus. This means the screening constant is larger. When you subtract the larger amount of electrons from the amount of protons, 4, the difference will be less, meaning the value of the effective nuclear charge will be less.
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∙ 10y ago
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What is the region around the nucleus the electrons travel in?
Depending on the context of a situation, there are many answers to this.The atom's electrons are often referred to as the electron "cloud." This is because electrons do not seem to orbit the nucleus of an atom with perfect, "well-behaved" circular motion - in fact, electrons are so tiny, and moving so fast (VERY close to the speed of light), that the best anyone can do is represent them as an erratic, localized smear of probability in the space around the nucleus. (Well, some people do a bit better than that... people far cleverer than myself.)In elementary physics and chemistry, we often simplify this model back to nice, circular electron "orbits" or "shells," as their actual positions in space are of relatively little concern in these studies.Even more specifically, chemistry eventually delves into the study of what are called electron "configurations," which are much more specific: they describe the three-dimensional shapes adopted by electron cloud and the pattern in which its shape changes as more and more electrons are added. These are also sometimes referred to as "orbitals."To recap:"Electron cloud" conjures a visual image of what we imagine the outside of an atom to look like."Electron orbit" conjures an image of a perfect (simplified), circular motion about the nucleus. Useful for early education of atomic theory."Electron shells" is often used in the context of valence (the outer-most) electrons involved in the exchanges that constitute chemical reactions."Electron orbitals/configurations" usually refer to the shape of the "cloud" that a given number of electrons will adopt and the pattern of these shapes as the number of electrons increases.
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