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Yes, because an electron is negatively charged, and opposite charges repel.
Wiki User
∙ 12y ago
Wiki User
∙ 14y agoNo, electrons are not repelled by nucleus.
Nucleus is positively charged while electrons are negatively charged.
Therefore electrons are attracted by nucleus.
Wiki User
∙ 11y agoNo. Electrons are negatively charged particles, except in the case of positrons which are positively charged electrons ( see positron emission - Nuclear Decay)
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What is the principal reason for using neutrons to bombard nucleus?
They are not repelled by the nucleus.
Where are the protons neutrons and electron located in the atom?
Protons and neutrons are located within the nucleus. Electrons are revolving around the nucleus.
Where is the subatomic particles located?
Protons and neutrons are in the center of an atom in the nucleus. Electrons are dispersed around the nucleus.
Which parts of the atom move around the nucleous?
Electrons. They have a negative charge.
Is electrons found inside the nucleus?
They are not in the nucleaus, they orbit around the nucleus.
What particles might be found in shells around a nucleus?
The particles found in the area surrounding the nucleus are called electrons. Electrons are attracted to the protons in the nucleus, but are repelled from other electrons. This is why they can be found orbiting the nucleus.
How do you know that atom is mostly empty space?
The electrons are repelled by the protons, which causes then to be farther away. If the nucleus was the size of a marble, then the atom would be the size of a football stadium. Correction: Electrons are not repelled by the protons but are attracted to them. Opposite charges attract.
What is the principal reason for using neutrons to bombard nucleus?
They are not repelled by the nucleus.
Why d orbital show poor shielding effect?
the electrons in d orbital push the electrons of s and p orbitals more away from themselves i.e push them inward (towards the nucleus) thereby making the nucleus to exert more pull on these repelled electron which in turn cause the other electrons of outer shells to come more closer to the nucleus; thus the size of the atom as a whole start shrinking. the electrons in d orbital push the electrons of s and p orbitals more away from themselves i.e push them inward (towards the nucleus) thereby making the nucleus to exert more pull on these repelled electron which in turn cause the other electrons of outer shells to come more closer to the nucleus; thus the size of the atom as a whole start shrinking.
What is the factor that affects the atomic number in an element?
More shielding of the outer electrons by the inner electrons is the most important factor that affects the atomic number in an element. A valence electron in an atom is attracted to the nucleus of an atom and is repelled by the other electrons in the atom. The inner electrons shield the outer electrons from the attraction of the nucleus and cause the atomic radius to be larger.
Does electrons make up an atom nucleus?
No, the electrons are around the nucleus, not in the nucleus.
Where are the protons neutrons and electron located in the atom?
Protons and neutrons are located within the nucleus. Electrons are revolving around the nucleus.
Where is the subatomic particles located?
Protons and neutrons are in the center of an atom in the nucleus. Electrons are dispersed around the nucleus.
Why is it easier to split a Uranium 235 nucleus using neutrons than using alpha particles?
they wont be repelled by the electromagnetic fields of the electron shell or the nucleus
Why do electrons stick together so well?
In general, electrons do not stick together well at all. In fact each electron repels every other electron. Electrons pack into high densities in atoms because each electron is attracted to the positive charge of the atom's nucleus more strongly than it is repelled by the other electrons in the atom.
Are electrons next to the nucleus?
No, electrons are around nucleus but at a great distance.
Do all atom nucleus have electrons?
All atoms have electrons, but not in the nucleus.
