Chem SI 12/2 Exam 2 Review

Hydrocarbons containing only single bonds.

Hydrocarbons containing one or more double bonds.

Hydrocarbons containing one or more triple bonds.

Hydrocarbons with a specific six-carbon ring with three double bonds.

A systematic method for naming organic compounds.

Specific groups of atoms that give molecules unique properties.

In chemical reactions, atoms are neither created nor destroyed.

Making the number of atoms of each elements equal on both sides of the equation

Quantitative relationship between reactants and products in a chemical reaction.

Solvents with a significant positive and negative end (e.g., water).

Solvents with no significant positive or negative ends (e.g., oil).

Attractive forces between an ion and a polar molecule.

Movement of solvent across a semipermeable membrane from low solute to high solute concentration.

Pressure applied to prevent osmosis.

Applying pressure to force solvent against the concentration gradient.

Describing the relative concentrations of solutes in solutions.

Higher solute concentration compared to another solution.

Lower solute concentration compared to another solution.

Same solute concentration as another solution.

Concentration expressed as moles of solute per liter of solution.

Substance that produces H3O+ ions in water.

The four classes of hydrocarbons are alkanes, alkenes, alkynes, and aromatics. Alkanes contain only single bonds, alkenes contain double bonds, alkynes contain triple bonds, and aromatics have a specific six-carbon ring with three double bonds.

The ending for an alkane is -ane.

The ending for an alkene is -ene.

The ending for an alkyne is -yne.

The prefix used to indicate the number of carbons in a chain is based on the number of carbons.

The root used to identify the type of hydrocarbon is based on the type of bond. It is '-ane' for alkanes, '-ene' for alkenes, and '-yne' for alkynes.

The Law of Conservation of Mass states that in all chemical reactions, atoms are neither created nor destroyed. It ensures that the number of atoms on the reactant side equals the number of atoms on the product side for each element, ensuring the equation is balanced.

Polar solutes dissolve in polar solvents due to hydrogen bonding. Polar solutes break their hydrogen bonds, form new hydrogen bonds with the solvent, leading to a lower potential energy.

Nonpolar solutes dissolve in nonpolar solvents through weaker forces like dispersion forces or dipole-dipole interactions.

Soluble ionic compounds dissolve in polar solvents because the ion-dipole forces are stronger than the ionic bonds. Ionic bonds between cations and anions are replaced by ion-dipole interactions with polar molecules, usually water.

Concentration can be expressed in various units, including mass/volume (m/v) or % mass/ volume (%m/v), molarity (moles solute/liters solution), parts per million (ppm), and parts per billion (ppb).

Dilute solutions contain less solute compared to concentrated solutions, meaning they are diluted. Concentrated solutions have a higher amount of solute.

Osmosis is the movement of solvent (usually water!) through a semipermeable membrane to equalize concentrations. It occurs when solutes cannot pass through the membrane, and the solvent moves to balance the solute concentrations on both sides.

Osmotic pressure is the amount of pressure needed to be applied to the more concentrated solution to prevent osmosis. It is a measure of the tendency of water to move across the membrane.

Reverse osmosis is the process where pressure greater than the osmotic pressure is applied to force water to flow against the concentration gradient, from a high solute concentration to a low solute concentration.

Hypertonic solutions have a higher solute concentration compared to another solution. Hypotonic solutions have a lower solute concentration compared to another solution. Isotonic solutions have the same solute concentration as another solution.

In hypertonic solutions, water flows out of the cell causing it to shrink or crenate. In hypotonic solutions, water flows into the cell causing it to swell and potentially burst (hemolysis). In isotonic solutions, there is no net movement of water, and the cell stays normal.

Brönsted-Lowry acids are proton donors. Protons are represented as H+.

Brönsted-Lowry bases are proton acceptors. Protons are represented as H+.

Strong acids and bases completely dissociate in water, meaning they donate/accept all their protons. Weak acids and bases only partially dissociate in water, meaning they donate/accept only some protons.

Le Chatelier's Principle states that if a change of conditions is applied to a system in equilibrium, the system will shift in a direction that relieves the stress. This applies to weak acid/base reactions.

If you remove a substance from a system in equilibrium, the reaction will shift towards making more of that substance to regain equilibrium. If you add a substance, the reaction will shift away from the substance to consume the excess.

pH is a measure of the hydronium ion (H3O+) concentration in a solution. The lower the pH, the higher the H3O+ concentration, and vice versa.

A buffer is a solution that resists changes in pH when small amounts of acid or base are added. It helps maintain a stable pH.

Buffers are made of a weak acid and its conjugate base or a weak base and its conjugate acid pair.

The pH range maintained by a buffer depends on the identity of the weak acid. The buffer capacity, which is the ability to resist pH changes, depends on the concentration of the buffer components.