The reason electrons do not spin into the center of the nucleus is due to the principle of quantum mechanics, specifically the Heisenberg Uncertainty Principle. This principle states that it is impossible to know both the exact position and momentum of a particle at the same time. Therefore, the electrons have a probability of being found within a certain distance from the nucleus, but they do not have a defined path or orbit like planets around the sun.
Electrons stay in orbit around the nucleus due to the force of attraction between the positively charged nucleus and the negatively charged electrons. This force is known as the electromagnetic force and it is responsible for keeping the electrons in their orbit around the nucleus.
Electrons do not collide with the nucleus because they have a negative charge and the nucleus has a positive charge. Like charges repel each other, so the electrons are repelled by the positively charged nucleus and are therefore unable to collide with it.
Yes, electrons can change their orbit around the nucleus. This is known as electron excitation, where the electron absorbs energy and jumps to a higher energy level, or electron relaxation, where the electron releases energy and drops to a lower energy level. These changes in orbit are what allow atoms to emit and absorb light at specific wavelengths.
No, the orbit of an electron around the nucleus is not perfectly circular. As mentioned before, electrons do not have a defined path or orbit like planets around the sun. Instead, they have a probability of being found within a certain distance from the nucleus, which can be represented as an electron cloud. However, certain elements and molecules can have more circular electron orbits, known as s-orbitals, due to their symmetrical shape.