* Atomic Mass: This refers to the total mass of an atom, primarily determined by the number of protons and neutrons in its nucleus.
* Charge: This refers to the overall electrical charge of an atom, determined by the balance between protons (positive charge) and electrons (negative charge).
Here's the breakdown:
* Protons: Located in the nucleus, they carry a positive charge and contribute to the atom's mass.
* Neutrons: Also located in the nucleus, they have no charge (they are neutral) and contribute to the atom's mass.
* Electrons: Orbiting the nucleus, they carry a negative charge and have a very small mass compared to protons and neutrons.
Example:
* Carbon-12 has 6 protons, 6 neutrons, and 6 electrons.
* Atomic Mass: Approximately 12 atomic mass units (amu).
* Charge: Neutral (6 protons = 6 electrons).
* Carbon-14 has 6 protons, 8 neutrons, and 6 electrons.
* Atomic Mass: Approximately 14 atomic mass units (amu).
* Charge: Neutral (6 protons = 6 electrons).
Key Points:
* Isotopes: Atoms of the same element can have different numbers of neutrons, resulting in different atomic masses (like Carbon-12 and Carbon-14). However, they will still have the same charge.
* Ions: An atom can gain or lose electrons, resulting in a net positive or negative charge (becoming an ion). This does not change the atomic mass.
In summary, the atomic mass is related to the number of protons and neutrons, while the charge is related to the balance between protons and electrons. These two properties are independent of each other.
