Energy Changes

Flashcards covering key concepts related to energy changes, phase changes, and chemical reactions.

Sublimation

The phase change from solid to gas without passing through the liquid phase.

Melting

The phase change from solid to liquid.

Freezing

The phase change from liquid to solid.

Vaporization

The phase change from liquid to gas.

Condensation

The phase change from gas to liquid.

Deposition

The phase change from gas to solid without passing through the liquid phase.

(s)

Indicates the solid phase of a substance in chemical equations.

(l)

Indicates the liquid phase of a substance in chemical equations.

(g)

Indicates the gas phase of a substance in chemical equations.

(aq)

Indicates a substance that is aqueous, or mixed/dissolved in water.

Exothermic Reaction

A reaction that releases energy into its surroundings.

Endothermic Reaction

A reaction that absorbs energy from its surroundings.

Entropy

A measure of the disorder or randomness in a system.

Kinetic Energy

The energy of an object due to its motion.

Potential Energy

Stored energy that has the potential to do work.

Law of Conservation of Energy

The principle that energy cannot be created or destroyed, only transformed from one form to another.

Physical Change

A change in the form or appearance of a substance, but not its chemical composition. The substance's chemical identity remains the same.

Chemical Change

A change that results in the formation of new chemical substances with different properties and chemical composition from the original substances.

Carbon's Bonding Capacity

Carbon atoms have a valency of four, meaning they can form four covalent bonds with other atoms, enabling the creation of complex organic molecules.

Shared Electrons in a Carbon-Carbon Triple Bond

In a carbon-carbon triple bond (C ext{\equiv}C), two carbon atoms share a total of 6 electrons (3 pairs) to form a very strong and short bond.