Question

Determine the charge of each ion. (a) tungsten ion with 68 electrons (b) tellurium ion with 54 electrons (c) nitrogen ion with 10 electrons (d) barium ion with 54 electrons

Short answer

The charges are: (a) tungsten ion (W) +6, (b) tellurium ion (Te) -2, (c) nitrogen ion (N) -3, and (d) barium ion (Ba) +2.

Step-by-step solution

- Determine the atomic numbers

Find the atomic numbers of tungsten (W), tellurium (Te), nitrogen (N), and barium (Ba) from the periodic table. Atomic numbers represent the number of protons in an atom: tungsten (W) has 74, tellurium (Te) has 52, nitrogen (N) has 7, and barium (Ba) has 56.

- Calculate the charge for each ion

The charge of an ion is the difference between the number of protons and electrons. The charge can be calculated with the formula Charge = Protons - Electrons. For tungsten (W) with 68 electrons, the charge is 74 - 68 = +6. For tellurium (Te) with 54 electrons, the charge is 52 - 54 = -2. For nitrogen (N) with 10 electrons, the charge is 7 - 10 = -3. For barium (Ba) with 54 electrons, the charge is 56 - 54 = +2.

Key concepts

Ionic Charge Calculation

Ionic charge calculation is fundamental when studying chemistry, particularly in understanding how atoms interact to form compounds. The charge of an ion is determined by the difference between the number of protons, carry a positive charge, and electrons, which are negatively charged. When an atom loses electrons, it becomes a positively charged ion, or cation, whereas an atom that gains electrons becomes a negatively charged ion, or anion.

To calculate the ionic charge, use the formula:
\(\text{Ionic Charge} = \text{Number of Protons} - \text{Number of Electrons}\).

For example, a tungsten ion (W) with 68 electrons, having 74 protons inherently (based on its atomic number), will have an ionic charge of \(74 - 68 = +6\). It's vital to understand that the overall charge of an ion reflects its ability to combine with other ions to form stable compounds. Such calculations are not just academic; they are essential for predicting the behavior of substances in real-world applications.

Periodic Table

The periodic table is an organized chart of elements arranged by increasing atomic number, which is the number of protons in the nucleus of an atom. The table is designed to showcase patterns in elemental properties, including their size, electronegativity, and, crucially for our discussion, their tendency to form ions with particular charges.

Each element's position on the table—as well as the table's groupings into columns (groups) and rows (periods)—gives us information about that element's characteristics. For example, elements in the same group typically have similar ionic charges when they become ions. This predictive power makes the periodic table an invaluable tool for scientists and students alike in understanding how elements will behave and interact.

Atomic Number

The atomic number of an element, a fundamental concept in chemistry, is the total count of protons present in the nucleus of its atoms. It is represented by the symbol 'Z'. The atomic number uniquely identifies a chemical element and determines its position within the periodic table. Because each element has a different number of protons, the atomic number lets us differentiate between, say, nitrogen (N) with an atomic number of 7 and tellurium (Te) with an atomic number of 52.

In the context of determining ion charges, the atomic number is used to figure out the number of protons in an ion. Since the overall charge of an ion is the difference between protons and electrons, knowing the atomic number is crucial when calculating the ionic charge.

Subatomic Particles

Atoms are composed of subatomic particles, notably protons, neutrons, and electrons. Protons have a positive charge and reside in the atom's nucleus along with neutrons, which have no charge. Electrons, which have a negative charge, orbit the nucleus and are involved in chemical reactions and bonding.

Understanding the properties of these subatomic particles is crucial when it comes to determining the charge of an ion. Since ions are atoms that have lost or gained electrons, it's the balance—or imbalance—between protons and electrons that defines the charge of the ion. Each element’s electron configuration, which is also guided by its position on the periodic table, plays a role in its tendency to lose or gain electrons to form ions.