Why does the electron in a hydrogen atom remain close to the proton in the nucleus?

• A. Because the electron is chemically bonded to the proton by a covalent bond.
• B. Because the electron has a larger mass than the proton and is therefore less likely to move away.
• C. Because the electrostatic attraction between the negatively charged electron and the positively charged proton holds the electron near the nucleus.
• D. Because the electron is repelled by the proton due to their opposite charges.

Answer: (C)

Verified step by step guidance

1. Understand the nature of charges: The proton carries a positive charge, and the electron carries a negative charge.
2. Recall Coulomb's Law, which describes the electrostatic force between two charged particles: \(F = \dfrac{k \cdot |q_1 \cdot q_2|}{r^2}\), where \(F\) is the force, \(k\) is Coulomb's constant, \(q_1\) and \(q_2\) are the charges, and \(r\) is the distance between them.
3. Recognize that opposite charges attract each other, so the negatively charged electron is attracted to the positively charged proton.
4. This electrostatic attraction acts as a force that keeps the electron close to the proton, preventing it from drifting away.
5. Note that this attraction is not a covalent bond (which involves sharing electrons between atoms), and the electron's mass is much smaller than the proton's, so mass does not explain the electron's proximity.