Chemical Bonding and Solution Chemistry Concepts
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Intermolecular Forces (IMFs)
IMFs include: Covalent, Hydrogen, Metallic, Dipole, London, and Ion interactions.
Solution Chemistry Formulas
- pH (Acidic Solutions): $\text{pH} = -\log[\text{H}^+] = -\log N = \text{p}H_A = \sqrt{K_a M}$ (where $K_a = x^2/M$ and $-\log x = \text{p}OH$ is incorrect in this context, use $\text{pH} = 14 - \text{pOH}$)
- pOH (Basic Solutions): $\text{pOH} = -\log[\text{OH}^-] = -\log N$. For weak bases (WB): $K_b = x^2/M$ and $-\log x = \text{pOH}$, leading to $\text{pH} = 14 - \text{pOH}$.
Strong Acids
Common strong acids include: $\text{HNO}_3$, $\text{H}_2\text{SO}_4$, $\text{HBr}$, $\text{HI}$, $\text{HClO}_4$, and $\text{HClO}_3$.
Lewis Acid
A compound or ionic species that can accept an electron pair from a donor compound.
Lewis Base
A compound or ionic species that can donate an electron pair to an acceptor compound.
Gas Properties
Lighter the gas, the faster it moves.
Writing Ionic and Net Ionic Equations
Ionic equations and net ionic equations are usually written only for reactions that occur in solution and attempt to show how the ions present are reacting. While ionic equations show all of the substances present in solution, a net ionic equation shows only those that are changed during the course of the reaction.
To write ionic equations, follow the steps below. Each step is demonstrated using the reaction of magnesium metal with hydrochloric acid as an example.
| 1. | Write the molecular equation and balance it. |
$\text{Mg} + 2 \text{HCl} \longrightarrow \text{MgCl}_2 + \text{H}_2$ | |
| 2. | Determine the state of each substance (gas, liquid, solid, aqueous). Use the solubility rules to determine which of the ionic compounds are soluble in water. Soluble ionics are identified with an (aq), insoluble ones with an (s). Most elements and covalent compounds (covalent compounds are formed when two or more nonmetallic elements are bonded to each other) are insoluble in water and should be shown with an (s), (l) or (g). |
$\text{Mg}(s) + 2 \text{HCl}(aq) \longrightarrow \text{MgCl}_2(aq) + \text{H}_2(g)$ | |
| 3. | Write the ionic equation by breaking all the soluble ionic compounds (those marked with an (aq)) into their respective ions. Each ion should be shown with its charge and an (aq) to show that it is present in solution. Use coefficients to show the number of each ion present. Rewrite the elements and covalent compounds as they appeared in the preceding step. |
$\text{Mg}(s) + 2 \text{H}^+(aq) + 2 \text{Cl}^-(aq) \longrightarrow \text{Mg}^{+2}(aq) + 2 \text{Cl}^-(aq) + \text{H}_2(g)$ | |
| 4. | Write the net ionic equation by removing the spectator ions. Spectator ions are those ions that appear exactly the same on each side of the ionic equation. |
$\text{Mg}(s) + 2 \text{H}^+(aq) \longrightarrow \text{Mg}^{+2}(aq) + \text{H}_2(g)$ |