Science 10 Summative 1: Chemical Reactions, Acids, and Bases

Comprehensive vocabulary flashcards covering chemical reaction indicators, acid-base properties, reaction types, and the law of conservation of mass based on the Science 10 reviewer.

Chemical Reaction

A process where one or more substances (reactants) change into new substances (products) with different properties.

Reactants

The starting substances in a chemical reaction, found before the arrow ($\rightarrow$) in a chemical equation.

Products

The new substances formed during a chemical reaction, found after the arrow ($\rightarrow$) in a chemical equation.

Precipitate

An insoluble solid formed when two solutions react.

Exothermic

A type of reaction where heat is released, often causing the temperature of the surroundings to rise.

Endothermic

A type of reaction where heat is absorbed from the surroundings.

Physical Change

A change that affects the size, shape, or state of a substance without forming a new substance; it is usually reversible.

Chemical Change

A change that results in the formation of a new substance and changes the chemical composition; it is usually irreversible.

Acid

A substance with a pH below $7$ that usually tastes sour, reacts with metals and carbonates, and turns blue litmus paper red.

Base

A substance with a pH above $7$ that has a bitter taste, slippery feel, and turns red litmus paper blue; also known as alkaline.

Neutral Solution

A solution with a pH of $7$, such as pure water.

Litmus Paper

An indicator where the blue version turns red in acids, and the red version turns blue in bases.

Phenolphthalein

An indicator solution that is colorless in acidic or neutral solutions and turns pink in basic solutions.

Universal Indicator

An indicator that shows a range of colors based on pH: red-orange-yellow for acids, green for neutral ($pH = 7$), and blue-purple for bases.

Methyl Orange

An indicator that is red in acidic solutions, yellow in basic solutions, and orange in neutral solutions.

Combination (Synthesis) Reaction

A reaction where two or more reactants combine to produce one product, following the general equation $A + B \rightarrow AB$.

Decomposition Reaction

A reaction in which a single compound breaks down into two or more simpler substances ($AB \rightarrow A + B$).

Single Replacement Reaction

A reaction in which one more reactive element replaces another element in a compound ($A + BC \rightarrow AC + B$).

Double Replacement Reaction

A reaction where two compounds exchange ions to form two new compounds ($AB + CD \rightarrow AD + CB$), often producing a precipitate, water, or gas.

Combustion Reaction

A reaction where a fuel (usually a hydrocarbon) reacts with oxygen ($O_2$) to release energy in the form of heat and light.

Neutralization Reaction

A specific type of double displacement reaction where an acid and a base react to produce salt and water ($\text{Acid} + \text{Base} \rightarrow \text{Salt} + \text{Water}$).

Law of Conservation of Mass

The scientific law stating that matter cannot be created or destroyed during a chemical reaction; the number of atoms on both sides of the equation must be equal.

Photosynthesis

The process by which plants make food using sunlight, represented by the equation $6CO_2 + 6H_2O \rightarrow C_6H_{12}O_6 + 6O_2$.

Respiration

The process where cells break down glucose and oxygen to release energy, producing carbon dioxide and water as byproducts.

Activity Series of Metals

A list of metals arranged from most reactive to least reactive; a metal can only displace another metal from a compound if it is located above it on this list.

Complete Combustion

Combustion that occurs with sufficient oxygen, producing carbon dioxide ($CO_2$) and water ($H_2O$).

Incomplete Combustion

Combustion that occurs when oxygen is limited, producing carbon monoxide ($CO$) or soot (carbon) and less energy.