Chemistry MYP4 (2).docx

MYP4 EOSA

Matter

Anything that takes up space and has mass.

Pure substances

Elements & compounds. Mixtures:Homogeneous & heterogeneous.

Law of conservation of mass

Mass cannot be created or destroyed in an isolated system.

Element

A simple substance that cannot be broken down into smaller parts.

Compound

Combination of 2 or more elements in a definite ratio by mass.

Gases

Have weak intermolecular forces, high kinetic energy, low density, and no fixed shape or volume.

Liquids

Have medium intermolecular forces, density, and compression, with a fixed volume but no fixed shape.

Solids

Have strong intermolecular forces, no compressibility, fixed shape and volume, and slow diffusion.

Bose Einstein Condensate (BEC)

Fifth state of matter at near absolute zero, formed by cooling low-density gas.

Plasma

Consists of free electrons and cations, no fixed shape or volume, and can conduct electricity.

Interconversion of states of matter

Solid to liquid to gas with temperature changes.

Heating curves

Show temperature changes during state changes like melting and boiling.

Cooling curves

Show temperature changes as a substance is cooled down.

Kinetic Molecular Theory of Gas

Describes behavior of gases based on kinetic energy and motion of particles.

Gas Laws

Describe the relationship between pressure, volume, temperature, and amount of gas in a system.

Boyle's Law

Inversely proportional relationship between pressure and volume of a gas at constant temperature.

Charles Law

Describes the relationship between temperature and volume of a gas at constant pressure and number of particles. As temperature increases, the volume of the gas also increases.

Combined Gas Law

Shows the relationship between pressure, volume, and temperature of a gas. Expressed as PV/T = constant.

Gay Lussac Law

States that the ratio of the pressure and temperature of a gas remains constant if the volume is kept constant.

Ideal Gas Equation

Describes the behavior of ideal gases using the formula PV = nRT, where n is the number of particles and R is the constant.

Elements

Substances that cannot be broken down into simpler substances and are the building blocks of matter.

Compounds

Formed when two or more elements chemically combine to create a new substance with unique properties.

Solutions

Homogeneous mixtures where substances are evenly distributed at a molecular level.

pH Levels

Measure of the concentration of hydrogen ions in a solution, ranging from 0 to 14 with 7 being neutral.

Separation Techniques

Various methods used to separate mixtures based on their physical properties.

Diffusion

Movement of particles from an area of higher concentration to lower concentration due to kinetic energy.

Solvent

The component in a solution that dissolves the other substance, present in larger quantity.

Solute

The substance that is dissolved in the solvent, typically present in a smaller quantity.

Classification of Matter

Categorizes matter into atoms, elements, compounds, mixtures, and molecules based on their composition and properties.

Chemical Changes

Irreversible alterations in chemical composition resulting in the formation of new substances with different properties.

Rate of Reaction

Describes how quickly a reaction occurs and is influenced by factors like temperature, concentration, and surface area.

Catalyst

A chemical that speeds up a reaction by lowering the activation energy, increasing the rate of effective collisions, and hence the reaction rate.

Reversible reaction

A reaction where products can convert back to reactants, maintaining a dynamic equilibrium.

Chemical equilibrium

When the rate of the forward reaction equals the rate of the backward reaction, with constant concentrations of reactants and products.

Le Chatelier's principle

If a system at equilibrium faces a change in concentration, temperature, or pressure, it adjusts to counteract the change and restore equilibrium.

Collision theory

States that reactant particles must collide with proper orientation and sufficient energy for a successful reaction.

Stoichiometry

The calculation of reactants and products in chemical reactions based on the Law of Conservation of Mass.

pH

A measure of the acidity or alkalinity of a solution, ranging from 0 (most acidic) to 14 (most basic).

Arrhenius concept of acids and bases

Acids produce H+ ions in water, while bases produce OH- ions when dissolved in water.

Neutralization reaction

When an acid reacts with a base, forming water and a salt.

Indicators

Chemical compounds that change color based on the presence of an acid or a base, used to determine the pH of a solution.

Alkali

Bases soluble in water, such as sodium hydroxide and potassium hydroxide, are known as alkalis.

Strong acid/base

Acids or bases that completely ionize in an aqueous solution are termed strong acids or bases.

Weak acid/base

Acids or bases that partially ionize in an aqueous solution are referred to as weak acids or bases.

Concentration

The relative amount of solute to solvent in a solution, categorized as concentrated (more solute) or dilute (more solvent).

Chemical properties of acids

Acids react with metals, metal oxides, bases, carbonates, and bicarbonates to form salts and release hydrogen gas.

Neutralization reaction

When an acid reacts with a base, a neutralization reaction occurs, producing salt and water.

Chemical properties of alkalis

Alkalis heated with ammonium salts release ammonia gas, affecting soil acidity and mineral nutrient availability.

Oxides

Basic oxides react with water to form bases, while acidic oxides react with water to form acids.

Salts

Ionic compounds produced from the reaction of acids and bases, soluble salts like sodium hydroxide and insoluble salts like lead chloride can be formed.

Precipitation reaction

Mixing solutions of two soluble compounds to form an insoluble salt, following solubility rules to identify soluble and insoluble compounds.