nucleus
Electrons surround the nucleus of an atom in patterns called electron shells.
The nucleus, consisting of protons and neutrons, is much more massive than the electrons.
The electron cloud becomes larger as the value of n increases because electrons in higher energy levels are on average farther from the nucleus. These higher energy levels have more sublevels and orbitals, resulting in a larger spatial distribution of the electron cloud. This increased distance from the nucleus leads to a larger orbital size.
No, it is not. Almost all of the mass of an atom is located in the nucleus. The proton, that carrier of the positive electrical charge, is some 1836 times more massive that the negatively charged electron that it attracts to "build" an atom. If we take a look, we'll find that in a simple hydrogen-1 atom, a single proton is in the nucleus and a lone electron makes up the electron cloud. And the nucleus is about 1836 times more massive than the "rest" of the atom. In a helium-4 atom, two protons and two neutrons form the nucleus and a pair of electrons form the electron cloud. In this case, the nucleus is about 7,444 times as massive as the electrons. As we move up the periodic table, the figure gets even more lopsided.
The denser areas of an electron cloud represent regions of higher electron probability density, where electrons are more likely to be found. These regions correspond to the most stable electron configurations around the nucleus of an atom.
The nucleus by far.
The nucleus is far more massive than the electron cloud. The mass of the electron cloud is almost negligible compared to that of the nucleus.
The distance of the electron cloud from the nucleus affects the atom's stability. When the electron cloud is closer to the nucleus, the atom is more stable. This is because the positively charged nucleus and negatively charged electrons are closer together, creating a stronger attraction. Conversely, if the electron cloud is further from the nucleus, the atom is less stable as the attraction between the nucleus and electrons is weaker.
Electrons surround the nucleus of an atom in patterns called electron shells.
In atoms. More specifically, they orbit the nucleus of an atom, in the aptly name electron cloud. Or electron shell.
Not exactly. An electron is an actual physical particle with a negative charge. An electron cloud is (generally) a spherical area around the nucleus of an atom that predicts where the electrons might be located.
The nucleus, consisting of protons and neutrons, is much more massive than the electrons.
I think the word you're looking for is "electron cloud". That term already describes where electrons are found. It would be kind of silly to define "electron cloud" in such a way that it describes an area where electrons are not found, wouldn't it?
The electron cloud becomes larger as the value of n increases because electrons in higher energy levels are on average farther from the nucleus. These higher energy levels have more sublevels and orbitals, resulting in a larger spatial distribution of the electron cloud. This increased distance from the nucleus leads to a larger orbital size.
No, it is not. Almost all of the mass of an atom is located in the nucleus. The proton, that carrier of the positive electrical charge, is some 1836 times more massive that the negatively charged electron that it attracts to "build" an atom. If we take a look, we'll find that in a simple hydrogen-1 atom, a single proton is in the nucleus and a lone electron makes up the electron cloud. And the nucleus is about 1836 times more massive than the "rest" of the atom. In a helium-4 atom, two protons and two neutrons form the nucleus and a pair of electrons form the electron cloud. In this case, the nucleus is about 7,444 times as massive as the electrons. As we move up the periodic table, the figure gets even more lopsided.
Denser areas in the electron cloud represent regions where there is a higher probability of finding an electron. These areas correspond to regions of higher electron density and show where electrons are more likely to be located around the nucleus.
The denser areas of an electron cloud represent regions of higher electron probability density, where electrons are more likely to be found. These regions correspond to the most stable electron configurations around the nucleus of an atom.