write the mass number and atomic number for each of the following neutral atoms an atom that contains 22 protons and 21 neutrons
The correct answer and explanation is:
Correct Answer:
- Atomic Number: 22
- Mass Number: 43
Explanation (300 words):
To determine the atomic number and the mass number of an atom, start by understanding what these numbers represent. The atomic number is defined as the number of protons in the nucleus of an atom. This number also determines the identity of the element. In a neutral atom, the number of protons is equal to the number of electrons. The mass number, on the other hand, is the total number of protons and neutrons found in the nucleus.
In this problem, the atom contains 22 protons and 21 neutrons. Since the atomic number is equal to the number of protons, the atomic number of this atom is 22. This corresponds to the element titanium on the periodic table, which always has 22 protons.
To calculate the mass number, simply add the number of protons and neutrons together:
Mass number = Protons + Neutrons = 22 + 21 = 43
So the mass number of this atom is 43. This means the atom is a neutral isotope of titanium. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. In this case, the typical and most stable isotopes of titanium have mass numbers such as 46, 47, 48, 49, and 50, but here the isotope has a mass number of 43, which would be a less common and likely unstable isotope.
This understanding of atomic structure is crucial in chemistry and physics because it helps in identifying elements and their isotopes, predicting atomic behavior, and understanding nuclear reactions. The atomic number never changes for an element, but the mass number can vary due to different numbers of neutrons, which is the basis of isotopic variation.