chemistry final vocab review

ionization energy

the energy required to remove an electron from an atom

increases

Ionization energy _______ when you go left to right across the period

decreases

Ionization energy _________ when you go down the group/family

electron affinity

the attraction of an atom for an additional electron

1st ionization energy

the energy required to remove the most loosely bound electron from a neutral atom

shielding effect

Along with the increased distance of the outer electrons from the nucleus, the shielding effect of the inner electrons causes ionization energy to decrease going down a column on the periodic table

metal

a low ionization energy is a characteristic of a _______

non-metal

an element with a high ionization energy is classified as a ______

electronegativity

the attraction an atom has for shared electrons is called _______

atomic radius

the distance from the nucleus to the outer most electron is known as the ______

noble gases

The ________ do not have measured electronegativities since they do not commonly form compounds

zeff

pull between nucleus and electrons

shielding

attraction between nucleus and electrons

increases

electronegativity ______ when you go left to right across the period

decreases

electronegativity ________ when you go down the group

decrease

atomic radius _______ when you go left to right across the period

increases

atomic radius ______ when you go down the the group

alkali metals

elements located in group 1

alkaline earth metals

elements located in group 2

halogens

elements located in group 17

noble gases

elements located in group 18

thermochemistry

a branch of chemistry that studies the heat energy involved in various reactions

energy

the capacity to do work or produce heat, often stored within the structural, atomic, or molecular bonds of substances

chemical potential energy

the energy stored within the chemical bonds and structural arrangement of atoms and molecules

law of conservation of energy

states that energy cannot be created or destroyed, only converted from one form to another

endothermic process

a reaction that absorbs heat from its surroundings, resulting in a decrease in temperature of the environment.

heat

the transfer of thermal energy between systems or surroundings due to a difference in temperature

universe

refers to the total system of matter and energy, encompassing all that exists, including all physical and chemical processes.

system

a specific portion of the universe chosen for analysis, often separated from its surroundings by a boundary.

exothermic process

a chemical reaction that releases heat, causing the surrounding temperature to rise.

calorie

a unit of energy equivalent to the amount needed to raise the temperature of one gram of water by one degree Celsius.

heat capacity

the amount of heat required to raise the temperature of a substance by one degree Celsius.

specific heat capacity

the amount of heat per unit mass required to raise the temperature by one degree Celsius.

surroundings

the part of the universe outside the system being studied, which can exchange energy or matter with the system.

joule

a unit of energy in the International System of Units (SI), defined as the amount of work done when a force of one newton displaces an object by one meter.

specific heat

the amount of heat needed to change the temperature of a unit mass of a substance by one degree Celsius.

solution

A homogeneous mixture of two or more substances, where a solute is uniformly distributed within a solvent.

solvent

substance doing dissolving the solute.

solute

the substance being dissolved in a solution.

aqueous solution

A solution in which water is the solvent.

gas solutions

A solution where a gas is dissolved in a solvent.

liquid solutions

A solution in which a liquid is the solvent.

miscible

Refers to two liquids that can mix in any proportion without separating.

immiscible

Refers to two liquids that cannot mix in any proportion, resulting in separation.

solubility

The ability of a substance to dissolve in a solvent at a given temperature and pressure.

solubility curves

Graphs that show the relationship between the solubility of a substance and temperature, indicating how much solute can dissolve in a solvent.

soluble

Refers to a substance that can dissolve in a solvent to form a homogeneous solution.

saturated

A solution that contains the maximum amount of solute that can dissolve at a given temperature and pressure.

unsaturated

A solution that contains less solute than can be dissolved at a given temperature and pressure.

supersaturated

A solution that temporarily contains more solute than can ordinarily dissolve at a given temperature and pressure.

dilute

A solution that has a relatively small amount of solute compared to solvent, resulting in a lower concentration.

concentrated

A solution that has a relatively large amount of solute compared to solvent, resulting in a higher concentration.

molarity

A measure of the concentration of a solute in a solution, defined as the number of moles of solute per liter of solution.

molality

A measure of the concentration of a solute in a solution, defined as the number of moles of solute per kilogram of solvent.

mass percent

A way to express concentration, defined as the mass of solute divided by the total mass of the solution, multiplied by 100.

volume percent

A way to express concentration, defined as the volume of solute divided by the total volume of the solution, multiplied by 100.

boiling point elevation

The increase in the boiling point of a solvent when a non-volatile solute is added, proportional to the molality of the solution.

freezing point depression

The decrease in the freezing point of a solvent when a non-volatile solute is added, proportional to the molality of the solution.

colligative properties

Properties that depend on the number of solute particles in a solution, such as boiling point elevation and freezing point depression.

neutralization reaction

A chemical reaction in which an acid and a base react to form water and a salt, typically resulting in a solution with a pH closer to neutral.

dilution

The process of reducing the concentration of a solute in a solution, usually by adding more solvent. This increases the volume of the solution while keeping the amount of solute constant.

standard solution

A solution of known concentration used as a reference in titrations and chemical reactions.

nonelectrolyte

A substance that does not dissociate into ions when dissolved in water, thus not conducting electricity.

electrolyte

A substance that dissociates into ions when dissolved in water, allowing the solution to conduct electricity.

salt

A compound formed by the reaction of an acid and a base, typically consisting of cations and anions.