(Jeremy Krug) AP Chem Unit 3 Review | Properties of Substances and Mixtures

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from his video https://youtu.be/a03QTLXKwzY?si=P_LU-5q25CLBzHlt

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25 Terms

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London dispersion forces

The weakest intermolecular forces found in all molecules; stronger in large molecules due to increased polarizability.

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Dipole-dipole forces

Intermolecular forces that occur between polar molecules, where the positive pole of one molecule attracts the negative pole of its neighbors.

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Hydrogen bonding

A strong type of intermolecular force that occurs when hydrogen is bonded to oxygen, fluorine, or nitrogen.

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Ion-dipole forces

Forces that occur between polar molecules and ions, crucial for solubility in ionic compounds.

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Ionic solids

Solids composed of ions, characterized by high melting points, brittleness, and conductivity when dissolved in water.

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Covalent network solids

Solids with strong covalent bonds extending in multiple directions, such as diamond and silicon dioxide.

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Molecular solids

Solids made up of molecules which have relatively weak intermolecular forces and low melting points.

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Metallic solids

Solids composed of metal atoms, known for malleability, ductility, and good electrical conductivity.

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Amorphous solids

Solids that lack a long-range crystalline structure.

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Ideal Gas Law

An equation of state for an ideal gas, given by PV=nRT, relating pressure, volume, temperature, and amount of gas.

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Molarity

A measure of concentration representing moles of solute per liter of solution.

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Distillation

A separation technique that relies on differences in boiling points to separate components of a mixture.

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Chromatography

A separation technique that involves the movement of a mixture through a stationary phase, separating components based on their affinities.

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Like dissolves like

A rule of thumb in chemistry stating that polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes.

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Electromagnetic spectrum

The range of all types of electromagnetic radiation, each affecting molecules in different ways.

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Photon

A packet of light energy that exhibits both wave and particle properties.

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Beer-Lambert Law

A relationship that relates absorbance to concentration, path length, and molar absorptivity, commonly used in spectrophotometry.

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Relationship between Temperature and Kinetic Energy

Temperature reflects the average kinetic energy of molecules; higher temperature indicates faster-moving molecules.

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Heterogeneous mixtures

Mixtures that consist of visibly different substances or phases, where the individual components can often be separated physically.

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Homogeneous mixtures

Mixtures that have a uniform composition throughout; the individual components are not visible and they cannot be easily separated.

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Outliers for Spectrophotometry

Possible contamination or dilution can lead to data points straying from the expected curve.

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UV/Visible Light

Causes electronic transitions.

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Infrared Radiation

Causes vibrational energy changes.

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Microwave Radiation

Induces rotational transitions.

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Crystalline solids

Solids that have a well-defined, ordered structure, with a repeating pattern of atoms or molecules.