Question: Consider an atom with an atomic number of 23 and a mass number of 51.

(a) Determine the number of protons, neutrons, and electrons in this atom. (b) Calculate the charge of this atom. (c) Identify the element represented by this atom.

Answer:

(a) To determine the number of protons, neutrons, and electrons in this atom, we use the atomic number and mass number.

The atomic number of an element represents the number of protons in its nucleus. Since the atomic number is given as 23, this atom contains 23 protons.

The mass number is the total number of protons and neutrons in an atom. Subtracting the atomic number from the mass number gives the number of neutrons. Therefore, the number of neutrons in this atom is 51 - 23 = 28.

In a neutral atom, the number of electrons is equal to the number of protons. Therefore, this atom contains 23 electrons.

(b) To calculate the charge of this atom, we need to compare the number of protons and electrons. Since the atom has 23 protons (positive charge) and 23 electrons (negative charge), the total charge is zero. Thus, the charge of this atom is neutral.

(c) To identify the element represented by this atom, we need to determine its atomic number. From part (a), we have the atomic number as 23.

By referring to the periodic table, we can see that the element with an atomic number of 23 is vanadium (V). Therefore, the atom in question represents the element vanadium.

In summary, the atom with an atomic number of 23 and a mass number of 51 contains 23 protons, 28 neutrons, and 23 electrons. It has a neutral charge and represents the element vanadium (V).