Untitled Flashcards Set

Chemical Reactions

Processes where substances (reactants) transform into different substances (products).

Valency

The measure of an element's bonding capacity, indicating how many atoms can combine.

Chemical Equations

Representations of chemical reactions showing relationships between reactants and products.

Physical Change

A change in the state or appearance of a substance without altering its chemical composition.

Chemical Change

A change resulting in the formation of new substances with different chemical compositions.

Acids

Substances that release hydrogen ions (H⁺) in solutions.

Bases

Substances that release hydroxide ions (OH⁻) in solutions.

Neutralization Reaction

A reaction between an acid and a base to form salt and water.

Synthesis Reaction

A reaction where two or more substances combine to form a new compound.

Decomposition Reaction

A reaction where a compound breaks down into simpler substances.

Single Displacement Reaction

A reaction where one element replaces another in a compound.

Double Displacement Reaction

A reaction where two compounds exchange ions to form new compounds.

Combustion Reaction

A reaction that typically involves oxygen and produces energy, carbon dioxide, and water.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Criss-Cross Rule

A method used to write chemical formulas for ionic compounds by crossing valencies.

Balancing Chemical Equations

Ensuring that the number of atoms for each element is the same on both sides of a chemical equation.

Law of Conservation of Mass

The principle stating that mass is neither created nor destroyed in a chemical reaction.

Empirical Formula

A chemical formula that shows the simplest whole-number ratio of elements in a compound.

Molar Mass

The mass of one mole of a substance, usually expressed in grams per mole.

Periodicity

The recurring trends that are seen in the properties of elements across different periods in the periodic table.

Acidic Solution

A solution that has a pH less than 7, indicating a higher concentration of hydrogen ions.

Basic Solution

A solution that has a pH greater than 7, indicating a higher concentration of hydroxide ions.

Redox Reaction

A reaction involving the transfer of electrons between two species, combining reduction and oxidation.

Catalysts

Substances that increase the rate of a chemical reaction without being consumed.

Inhibitors

Substances that decrease the rate of a chemical reaction.

Electrolytes

Substances that dissociate into ions in solution, conducting electricity.

pH Scale

A scale used to specify how acidic or basic a water-based solution is.

Salt

An ionic compound formed from the neutralization reaction between an acid and a base.

Hydrogen Ion (H⁺)

A positively charged ion formed when an acid donates a proton.

Hydroxide Ion (OH⁻)

A negatively charged ion formed when a base donates a hydroxide group.

Polyatomic Ion

An ion composed of two or more atoms that functions as a single ion.

Ionization Energy

The energy required to remove an electron from an atom or ion.

Electronegativity

The tendency of an atom to attract electrons towards itself in a chemical bond.

Mass Number

The total number of protons and neutrons in an atomic nucleus.

Atomic Number

The number of protons in the nucleus of an atom, which determines the element.

Isotope

Atoms of the same element with different numbers of neutrons and thus different mass numbers.

Sustainable Solutions

Chemistry practices aimed at minimizing waste and using renewable resources.

Chemical Kinetics

The study of the speeds or rates at which chemical reactions occur.

Thermodynamics

The study of energy changes during chemical reactions.

Endothermic Reaction

A reaction that absorbs heat from its surroundings.

Exothermic Reaction

A reaction that releases heat to its surroundings.

Bio-Chemicals

Chemicals derived from biological sources used for sustainable chemical processes.

Fermentation

A metabolic process converting sugar to acids, gases, or alcohol, typically occurring in anaerobic conditions.

Photosynthesis

The process by which green plants and some other organisms use sunlight to synthesize foods from carbon dioxide and water.

Rusting

A chemical reaction where iron reacts with oxygen and moisture, forming iron oxide.

Chemical Inventory

A list of all chemicals and substances available in the lab or institution.

Environmental Chemistry

The study of chemical processes occurring in the environment and the effects of human activities.

Acid Rain

Rainfall that has a low pH due to the presence of sulfur dioxide and nitrogen oxides in the atmosphere.

Green Chemistry

The design of chemical products and processes that reduce or eliminate hazardous substances.

Phytoremediation

The use of plants to absorb or filter out pollutants from the soil and water.

Electrolysis

A chemical process that uses electricity to drive a non-spontaneous reaction.