Complete the following tables. a. Cation # Protons in ion # Electrons in ion Formula

Complete the following tables. a. Cation # Protons in...

Complete the following tables. a. $$\begin{array}{|l|l|}\hline \text {Cation} & {\text {# Protons in ion}} & {\text {# Electrons in ion}} & {\text {Formula with $0^{2-}$}} \\ \hline \mathrm{K}^{+} & {} \\ \hline \mathrm{Co}^{2+} & {} \\ \hline \mathrm{Al}^{3+} & {} & {} \\ \hline\end{array}$$ b. $$\begin{array}{|l|l|}\hline \text {Anion} & {\text {# Protons in ion}} & {\text {# Electrons in ion}} & {\text {Formula with $\mathrm{Ca}^{2+}$}} \\ \hline \mathrm{Cl}^{-} & {} \\ \hline S^{2-} & {} \\ \hline P^{3-} & {} & {} \\ \hline\end{array}$$

Complete the following tables.
a. $$\begin{array}{|l|l|}\hline \text {Cation} & {\text {# Protons in ion}} & {\text {# Electrons in ion}} & {\text {Formula with $0^{2-}$}} \\ \hline \mathrm{K}^{+} & {} \\ \hline \mathrm{Co}^{2+} & {} \\ \hline \mathrm{Al}^{3+} & {} & {} \\ \hline\end{array}$$
b. $$\begin{array}{|l|l|}\hline \text {Anion} & {\text {# Protons in ion}} & {\text {# Electrons in ion}} & {\text {Formula with $\mathrm{Ca}^{2+}$}} \\ \hline \mathrm{Cl}^{-} & {} \\ \hline S^{2-} & {} \\ \hline P^{3-} & {} & {} \\ \hline\end{array}$$

Key Concepts

Ionic Compound Formulation

Formulating ionic compounds involves combining cations and anions in ratios that neutralize their overall charges. This requires an understanding of the stoichiometric balance between ions; for instance, determining the appropriate number of anions needed to balance the charge of a given cation so that the total positive and negative charges cancel each other out, resulting in a neutral compound.

Ionic Charges

This concept explains that ions are atoms or groups of atoms that have gained or lost electrons, resulting in an overall positive or negative charge. Cations form when electrons are lost, leaving a positive charge, while anions form when electrons are gained, imparting a negative charge. The magnitude of the ion’s charge indicates how many electrons have been lost or gained compared to the number of protons.

Atomic Structure

Atomic structure involves understanding that every atom is composed of protons, neutrons, and electrons. The number of protons, which defines the element, remains constant even when an atom becomes an ion. However, the number of electrons adjusts according to the ion's charge, which is crucial in determining the properties and behavior of the ion.

Electron-Proton Relationship in Ions

This concept focuses on the relationship between the number of protons and electrons in an ion. In a neutral atom, the number of electrons equals the number of protons. When an ion forms, electrons are either removed or added, resulting in an imbalance that corresponds to a positive or negative charge. Accurately determining the electron count in ions based on their charge is essential for constructing accurate ion tables.

Transcript

00:02 So when working with any ion, it doesn't matter what the charge is, positive, negative, positive charge of plus 25, whatever.

00:11 The number of protons will never change because that's the atomic number for the element.

00:16 So for potassium, its number of protons will always be 19.

00:22 For cobalt, the number of protons will always be 27.

00:26 For aluminum 13, for chlorine 17, sulfur will always be 16, phosphorus 15.

00:39 Number of electrons is a different story.

00:42 Since potassium has a positive charge, that means there's more protons than electrons, because protons are positively charged and electrons are negatively charged.

00:50 There's not a balance or an even number amount.

00:53 So since protons can't change, that means we have less electrons.

00:57 So it will be 19 minus 1 equals 18.

01:01 Same with cobalt, 27 minus 2.

01:06 We'll have 25 electrons.

01:08 Aluminum will be 13 minus 3, 10 electrons.

01:14 For the anions, it's the opposite.

01:16 Chlorine has a negative charge.

01:18 So that means we have more electrons than protons.

01:23 In fact, chlorine will have 18 electrons.

01:26 Sulfur will have 2 more electrons, so it will be 18, and phosphorus will have three electrons, three extra electrons...