Chemistry Chapter: Balancing Chemical Equations

A number placed in front of a chemical formula in a balanced chemical equation that indicates the relative number of moles of the substance involved in the reaction.

A law stating that mass is neither created nor destroyed in ordinary chemical or physical changes. The total mass of the reactants equals the total mass of the products.

A representation of a chemical reaction using chemical formulas and symbols. It shows the reactants on the left side and the products on the right side, with arrows indicating the direction of the reaction.

The substances that react in a chemical change.

The substances formed in a chemical change.

A chemical equation in which the number of atoms of each element on the reactants' side equals the number of atoms of that element on the products' side. It obeys the law of conservation of mass.

A chemical equation that does not have the same number of atoms of each element on both sides of the equation, violating the law of conservation of mass.

The rearranging of atoms in a chemical reaction, where atoms are neither created nor destroyed, but simply bonded differently.

A technique used for balancing chemical equations by ensuring that the number of atoms for each element on both sides of the equation is equal.

Balancing an equation means making sure the number of atoms of each element on the reactants side equals the number of atoms on the products side.

The process of converting reactants into products.

A number placed in front of a chemical formula in a balanced chemical equation that indicates the relative number of moles of the substance involved in the reaction.

A representation of a chemical reaction using chemical formulas and symbols. It shows the reactants on the left side and the products on the right side, with arrows indicating the direction of the reaction.

A chemical equation where the number of atoms of each element on the reactants' side equals the number of atoms of that element on the products' side.

A group of atoms that act as a single unit in chemical reactions. They often appear in both reactants and products without changing.

A chemical equation that does not have the same number of atoms of each element on both sides of the equation, violating the law of conservation of mass.

The substances that react in a chemical change.

The substances formed in a chemical change.

A chemical law stating that mass is neither created nor destroyed in ordinary chemical or physical changes. The total mass of the reactants equals the total mass of the products.

A chemical reaction in which a substance reacts rapidly with oxygen, producing heat and light.

A chemical reaction that involves the transfer of electrons between reactants. It can involve the gain of oxygen or the loss of hydrogen.

A type of chemical reaction used to generate energy. It often involves burning fuels like gasoline or coal.

Compounds made up of only carbon and hydrogen atoms.

A chemical reaction where reactants break down into simpler products.

A chemical reaction where two or more reactants combine to form a single product.

A chemical reaction where a more reactive element replaces a less reactive element in a compound.

These reactions involve the exchange of ions between two reactants, resulting in the formation of new products.

A chemical reaction is a process where chemical bonds are broken and formed between atoms and molecules, resulting in the transformation of reactants into products.

A balanced chemical equation ensures that the number of atoms of each element on the reactants' side equals the number of atoms of that element on the products' side, obeying the law of conservation of mass.

The coefficients in a balanced chemical equation represent the relative number of moles of each reactant and product involved in the reaction.

A chemical reaction in which there is energy released to the surroundings in the form of heat, light, or sound. The heat of reaction is negative.

A chemical reaction that absorbs energy from the surroundings, typically requiring heat input to proceed. The heat of reaction is positive.

Balancing chemical equations involves adjusting the coefficients in front of each chemical formula so that the number of atoms of each element is the same on both sides of the equation.

A compound formed from two elements, often with a metal losing electrons to a nonmetal. The charges of the ions determine the compound's formula.

A compound containing three different elements, often formed by combining water with a metal oxide or a nonmetal oxide.

When a metal reacts with a nonmetal, the metal typically loses electrons (positive charge), and the nonmetal gains electrons (negative charge), forming an ionic compound.

A compound formed when a metal reacts with a nonmetal, where the metal loses electrons and the nonmetal gains them.

Reactions with two elements forming a binary compound, often with electron transfer (ionic bonding), can be understood by analyzing the charges on the ions involved.

Water reacts with metal oxides (like calcium oxide) to form metal hydroxides (like calcium hydroxide or slaked lime).

Nonmetal oxides can react with water to form acids, like carbon dioxide reacting with water to form carbonic acid.