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Why are electrons usually found near the nucleus?
Electrons are usually found near the nucleus due to the attractive force of the positively charged protons in the nucleus. This force keeps the electrons in orbit around the nucleus rather than floating away. The balance between the attractive force of the protons and the repulsive force of the electrons determines the electron's energy level and distance from the nucleus.
What is charge effect?
the nuclear charge experienced by valence or outer-shell electrons, diminished by the shielding effect of inner-shell electrons and also by the distance from the nucleus
Why do force of attraction between nucleus and electrons decrease in alkali metal as increase in size?
As alkali metals increase in size, the distance of the outermost electrons from the nucleus increases. The attraction between the electrons and the nucleus is electrostatic, and it is a fundamental property of electrostatic attractions that the attraction decreases with increasing distance between the attracting charges. Another way of describing this is that the attractive force is partially "screened" by the inner electrons between the outermost electrons and the nucleus.
What two forces act in the nucleus to create a nuclear tug of war?
The two forces are the strong nuclear force and the electromagnetic force. The strong nuclear force acts to hold the nucleus together by overcoming the repulsive electromagnetic force between positively charged protons. This creates a delicate balance between the attractive strong nuclear force and the repulsive electromagnetic force, resulting in a "nuclear tug of war" within the nucleus.
What is closer to nucleus the stronger the attractive force?
When it is close to the nucleus because the postively charged protons attract the negatively charged electrons
Why are electrons usually found near the nucleus?
Electrons are usually found near the nucleus due to the attractive force of the positively charged protons in the nucleus. This force keeps the electrons in orbit around the nucleus rather than floating away. The balance between the attractive force of the protons and the repulsive force of the electrons determines the electron's energy level and distance from the nucleus.
How does the interference of inner electrons affect the attraction of outer electrons in an atom?
The interference of inner electrons in an atom can shield the attraction of outer electrons to the nucleus. This is because the inner electrons create a repulsive force that counteracts the attractive force between the outer electrons and the nucleus. As a result, the outer electrons may not be held as tightly to the nucleus, leading to weaker bonding and reactivity in the atom.
What are the relative strength strengths of attractive and repulsive forces in a stable nucleus?
In a stable nucleus, the attractive nuclear forces (such as the strong nuclear force) are stronger than the repulsive forces (such as the electromagnetic force) between protons. This balance of forces keeps the nucleus stable and prevents it from breaking apart.
Why do electrons stay mostly between the two nuclei?
Electrons stay mostly between two nuclei due to the attractive forces from the positive nucleus and the repulsive forces between electrons. This balance minimizes the total energy of the electron in the system, leading to a stable configuration with the electrons located in the space between nuclei.
When an atom is stable what is happening with the attractive and repulsive forces in the nucleus?
Inside an atom's nucleus there is a neutron, which has no charge, therefore no attractive or repulsive forces. The proton carries a positive charge, though, and repels the negative charge of the electron particle which exists somewhere outside of the nucleus.I'm yet of the old technology which thinks that protons and electron attract. Of course, that doesn't explain why the electron don't crash into the proton, but that's another story.
What keeps electrons moving around the nucleus?
Electrons move around the nucleus due to the attractive force between the positively charged protons in the nucleus and the negatively charged electrons. This force, called electrostatic attraction, keeps the electrons in orbit around the nucleus.
What is it called when electrons in the inner energy levels block the attraction between the nucleus and the valence electrons?
It is called shielding or screening effect. Inner electrons shield the valence electrons from the positive charge of the nucleus, reducing the attractive force between them.
What has a strong hold on electrons?
Nucleus of an atom has a strong hold on electrons because of the attractive force between the positively charged nucleus and negatively charged electrons. This attraction keeps the electrons in orbit around the nucleus, forming the structure of the atom.
What is the attraction and repulsion forces between subatomic particles?
attraction forces between the electrons of one atom and the nucleus of the other atom are balanced by the repulsive force caused by the two + charged nuclei as they are forced together~attractive forces have a little attraction for the atoms.
Why not electron collapse into the nucleus?
Electrons inhabit a probability cloud around the nucleus, which is related to their possible velocities. The closer the cloud is to the nucleus, the higher the kinetic energy, which allows it to overcome the electromagnetic attraction of the protons.
The five thousand billion billion freely moving electrons in a penny repel one another why dont they fly out of the penny?
The electrons in a penny are bound to the atoms within the penny's structure, which prevents them from flying out. The attractive force between the electrons and the positively charged nucleus of the atoms balances out the repulsive force between the electrons themselves. This equilibrium allows the electrons to move freely within the penny without escaping.
Do attractive forces have less hold on electrons farther from the nucleus?
Yes, as electrons get farther from the atomic nucleus they are less attracted to that nucleus, which is exactly what you would expect on the basis of Coulomb's Law, F=q1q2/r2 as the radius of the orbit increases the attractive force becomes decreased.
