physical and chemical changes

Chemical Changes

• Chemical changes involve one or more substances transforming into new substances with different properties.
• Chemical reactions are examples of chemical changes.
• These changes involve breaking and forming chemical bonds.
• Energy is often released or absorbed during chemical changes.
• Chemical equations represent chemical changes.

Crystallisation

• Crystallisation is a process where a solid substance forms a crystal structure from a solution.
• It often involves slow evaporation of the solvent.
• It's a significant purification method in various industries.
• Factors like temperature, concentration, and evaporation rate influence crystal size and shape.
• Different substances have varying solubilities, affecting their crystallisation.
• Crystallisation has applications in drug, food additive, and chemical production.

Physical Changes

• Physical changes alter a substance's appearance or structure without changing its composition.
• Physical changes include changes in state, shape, size, and phase.
• Examples include melting, freezing, boiling, condensation, and sublimation.
• These changes are either reversible or irreversible.
• No new substance is formed during a physical change.

Reversible and Irreversible Changes

• Reversible changes can be undone, returning the substance to its original state.
• Melting ice and boiling water are examples of reversible changes.
• Irreversible changes cannot be reversed. Burning paper is an irreversible change.

Rusting of Iron

• Rusting is a chemical process where iron deteriorates due to exposure to oxygen and moisture.
• This process creates iron oxide.
• Rusting is an oxidation reaction, where iron atoms lose electrons to oxygen atoms.
• Water acts as an electrolyte, speeding up electron flow and rust formation.
• Rust weakens iron structures over time.
• Coating iron surfaces with protective barriers prevents rusting.

Types of Chemical Reactions

• Chemical reactions can be categorized into five main types:
• synthesis, decomposition, single displacement, double displacement, and combustion.
• Synthesis combines substances to form a new compound.
• Decomposition breaks down a compound into simpler compounds or elements.
• Single displacement involves one element replacing another in a compound.
• Double displacement involves exchanging ions between two compounds.
• Combustion involves a fuel reacting with oxygen to produce heat and light energy.

Combination Reaction

• This occurs when two or more substances combine to form a single product, often a more complex compound.
• It's also known as a synthesis reaction.
• The reaction often involves the transfer or sharing of electrons.
• Energy (often heat or light) is typically released during a combination reaction.

Chemical Properties

• Chemical properties describe how a substance interacts with other substances to form new ones.
• These properties include flammability, reactivity, and toxicity.
• They relate to the composition of atoms and molecule arrangements within a substance, determining its behavior in various reactions.
• Helps identify and classify substances.

Chemical Reaction

• A chemical reaction involves reactants transforming into new products.
• Bonds break and new ones form during this process.
• Reaction rate is affected by temperature, concentration, and catalysts.
• The balanced chemical equation shows atom conservation.

Decomposition Reaction

• A decomposition reaction is where a compound breaks down into simpler substances.
• Decomposition can be initiated by heat, light, or electricity.
• Often involves a single compound as the reactant.
• Types of decomposition reactions include thermal, electrolytic, and photolytic.

Displacement Reaction

• A displacement reaction occurs when a more reactive element displaces a less reactive element in a compound.
• Redox reactions or single replacement reactions are also examples
• The reactivity series shows the order of displacement reactions.
• Metals are often involved in displacement reactions.

Endothermic Reactions

• Endothermic reactions absorb heat from the surroundings, decreasing the temperature.
• These reactions require an energy input.
• Reactants have lower energy than the products in endothermic reactions.
• Enthalpy change (ΔH) is positive for endothermic reactions.
• Photosynthesis and a reaction between baking soda and vinegar are examples of endothermic reactions.

Exothermic Reactions

• Exothermic reactions release heat to the surroundings, increasing the temperature of surrounding areas.
• These reactions are often spontaneous and don't need an external energy source.
• Common examples include combustion reactions such as burning wood or hydrogen reacting with oxygen.
• Enthalpy change (ΔH) is negative for exothermic reactions.
• Galvanization is the process of coating Iron or steel with zinc to prevent corrosion.

Hydrated Iron Oxide

• Hydrated Iron oxide is a compound formed when iron reacts with oxygen and water (moisture).
• It's also known as rust.
• Has the chemical formula Fe2O3.nH2O.
• Rust formation is important to prevent on iron-based structures.

Irreversible Change

• Irreversible changes cannot be undone.
• The transformation of substances during these changes is permanent.
• Examples include burning something or rusting iron.
• Often involve the creation of new substances and a change in energy.

Physical Properties

• These properties are observable or measurable without changing the substance's composition.
• Examples include color, odor, density, melting point, and boiling point.
• Used for identifying and classifying substances.
• Influenced by factors like temperature, pressure, and impurities.
• These properties are important in various scientific instruments and calculations for measurements.

Precipitate

• A precipitate is a solid that forms in a solution during a chemical reaction.
• Often the result of a double-displacement reaction or a metathesis reaction.
• Can be observed by identifying changes in color, texture, or state of the solution.
• Common methods for isolating the solid precipitate from the solution include filtration and centrifugation.
• Observing a precipitate helps determine the presence of certain ions or substances.

Products

• Products are the substances formed as a result of a chemical reaction.
• The reactants change to form products.
• Products often have different properties than the reactants.
• The ratio of reactants to products is shown in a balanced chemical equation.

Reactants

• Reactants are substances that undergo a chemical change in a reaction to form a new substance or substances.
• Present at the start of a reaction and are consumed during the reaction.
• They can be elements, compounds, or mixtures.
• Reactants determine the type and nature of products in a reaction.

Reversible Change

• Reversible change is when a substance can return to its original state from the changed state.
• Typical reversible processes are physical changes such as melting or dissolving.
• Properties of the substance retain after the reversible change is reversed.
• Processes involve breaking and forming chemical bonds in a reversible manner.

Rust

• Rust is a reddish-brown discoloration or coating formed on iron or steel due to oxidation.
• It's a type of iron oxide.
• Rusting occurs through a reaction between iron, oxygen, and moisture.
• Rusting can be accelerated by factors like salt and acidic conditions.

Silver Nitrate

• Silver nitrate is a compound frequently used in photography and laboratories.
• It's a white crystalline solid.
• Silver nitrate is soluble in water, forming a clear colorless solution.
• It can decompose when exposed to light.
• Corrosive, causing burns on skin contact.
• Used in organic chemistry for identifying certain chemical compounds.

Explore the fascinating world of chemical changes and crystallisation processes. This quiz covers the principles of chemical reactions, the formation of crystals, and the distinctions between physical and chemical changes. Perfect for students looking to solidify their understanding of chemistry concepts.