Chapter 1: Matter and Changes PDF

# Chapter 1: Matter and Changes ## Batterjee Medical College - For Science and Technology ## Edited By: - Dr. Nazar Abdulaziz Elnasri - Chemistry department - BMC asser-2024/2025 ## Content: - **Description of Matter** - **Classification of Matter** - **Properties of Matter** - **States (Ph...

# Chapter 1: Matter and Changes ## Batterjee Medical College - For Science and Technology ## Edited By: - Dr. Nazar Abdulaziz Elnasri - Chemistry department - BMC asser-2024/2025 ## Content: - **Description of Matter** - **Classification of Matter** - **Properties of Matter** - **States (Phases) of Matter** - **Physical Processes for Matter** - **Solutions** ## 1.1. Description of Matter - Matter is the term for any type of material that has mass and volume. - Matter is everything around you. - Atoms, molecules, wood, and metals are all classified as matter. - There are three basic states of matter: solid, liquid, and gas. ## States of Matter: Solids - Particles of solids are tightly packed, vibrating about a fixed position. - Solids have a definite shape and a definite volume. ### Examples of solids: - Wood - Metals ## 1.4. States (Phases) of Matter: Solids - Solids can be crystalline or amorphous. ### **Crystalline**: - Rigid and lattice structure. - Composed of one or more crystals. - Has a well-defined ordered structure. - **Example**: ice, table sugar, table salt, most metals. **Crystalline structure diagram**: A 2D representation of a crystalline solid. ### **Amorphous**: - No particular structure. - Has a disordered structure. - Lacks the well-defined arrangement of basic units. - **Example**: glass, porcelain, plastic. **Amorphous structure diagram**: A 2D representation of an amorphous solid. ## States of Matter: Gases - Particles of gases are very far apart and move freely. - Gases have an indefinite shape and an indefinite volume. ### **Examples of Gas**: - Air - Helium - Neon ## States of Matter: Liquids - Particles of liquids are tightly packed, but are far enough apart to slide over one another. - Liquids have an indefinite shape and a definite volume. ### **Examples of Liquids**: - Water - Juice - Honey ## Classification of Matter - **Matter:** Has mass and takes up space. - **Substance:** - **Element**: One kind of atom. - **Compound**: Two or more kinds of atoms. - **Mixture**: - **Homogeneous**: Evenly mixed. - **Heterogeneous**: Unevenly mixed. ## Elements and Compounds - **Elements** are substances that are made of one kind of atoms. - **Examples**: hydrogen (H2), carbon (C), oxygen (O2), and nitrogen (N2). - **Compounds** are substances made of two or more different atoms chemically combined together. - **Compounds** can be broken down into simpler substances only by chemical methods, **example**: pure water (H2O), salt (NaCl), and methane (CH4). ## Substance and Mixture - **Mixtures** are two or more substances that are mixed together without chemical reaction and can be separated by physical means into their original components. ### Types of Mixtures: - **Homogeneous mixtures** are mixtures whose components cannot be distinguished by naked eyes. - **Examples**: blood plasma, rainwater, tap water, air, juice, tea... - **Heterogeneous mixtures** are mixtures whose components can be distinguished by naked eyes. - **Examples**: sand in water, human skin.... ## Separation Techniques - Some methods of separation. - Separation techniques are used to separate mixtures into its constituent elements and/or compounds. - Old methods for separation. - Modern methods for separation. ### Diagram of Separation Techniques - Shows three different separation techniques: filtration, evaporation, and magnetic separation. Each has a labeled diagram of the technique. ## Physical Processes for Matter - Matter can often change from one physical state to another in a process called a physical change. For example, liquid water can be heated to form a gas called steam ### Diagram of Physical Processes - Shows a cycle of different physical processes, including melting, freezing, boiling, condensation, deposition, and sublimation. ## Key Definitions - **Phase Transition**: is the transformation of a system from one state of matter (phase) to another one by either change in the system heat or pressure. Phase transition occurs via the following physical processes. ### Diagram of Phase Transitions - Shows a cycle of different phase transitions, including freezing, melting, sublimation, deposition, condensation, and evaporation. ## Physical Processes for Matter: Detailed - **Melting** is a process (phase transition) in which the substance changes from a solid to a liquid by heating. - The temperature at which solid melts and changes to liquid is termed melting point (m.p). - **Boiling or Vaporization** is a process in which the substance changes from liquid to gas by heating. - The temperature at which liquid boils or the temperature at which liquid changes to gas is termed boiling point (b.p). - **Sublimation** is a process in which the substance changes from solid to gas by heating without becoming a liquid. ## Solutions - The solution is a homogeneous mixture of two or more substances, consisting of ions or molecules. ### Solute and Solvent - The terms solute and solvent refer to the components of a solution. - **Solute**: is the component of a solution in smaller amount. - **Solvent**: is the component of a solution in greater amount. - **Example**: Sodium chloride is dissolved in water. Sodium chloride is the solute and water is the solvent ### Diagram of Solute and Solvent - Shows a beaker with water as the solvent and sugar as the solute. ## Solutions - **When water is a solvent, the solution is aqueous.** - **Solvents may be gases**: air is a solution of nitrogen, oxygen, argon, and other gases. - **Steel is an alloy**, solution of one solid dissolved in another solid are solutions of various metals. ## Solutions - Solutions may exist in any of the three states of matter; that is, they may be gases, liquids, or solids (according to the state of the solvent). ### Types of Solutions - **Gaseous solution**: Air (O2, N2, others) - **Liquid solution**: Ethanol in water, CO2 in water, NaCl in water. - **Solid solution**: Gold-silver alloy, Dental-filling alloy ## Solutions, Colloidal and Suspension - The solute particle in true solutions are molecules having diameter less than 1nm. The particle size in colloidal solution lies in the range 1nm to 100nm. The size of the particles in the case of suspension is greater than 100 nm. ### Diagram of Solutions, Colloids, and Suspensions - Shows three glasses with different mixtures: a true solution, a colloid, and a suspension. A **true solution** shows a clear liquid with dissolved particles. A **colloid** shows a cloudy liquid with visible particles. A **suspension** shows a heterogeneous mixture with visible solid particles sinking to the bottom. ## Solutions, Colloidal and Suspension ### Table of Solutions, Colloids, and Suspensions - **True Solution**: - The solute particles cannot be separated from the mixture by filtration. - **Ex**: A true solution of common salt, sugar, and alum. - **Colloids**: - Particles in a colloid cannot be separated from the mixture by the process of filtration. - **Ex**: A colloidal of starch in water, egg albumin in water. - **Suspensions**: - The solute in a suspension can be separated from the mixture by the process of filtration. - **Ex**: A suspension of soil, chalk powder in water. ## Solubility and Solubility Test - Solubility is the ability of a solid, liquid, or gaseous chemical substance (referred to as the solute) to dissolve in solvent (usually a liquid) and form a solution. The solubility of a substance fundamentally depends on the solvent used - Solubility is a very important physicochemical parameter of a compound. Solubility test is a type of test used to determine the ability of compounds to dissolve in a solvent — usually liquid — at equilibrium. ## Solubility Terms - **Miscible**: - Two liquids that are soluble in each other. - If they are soluble in any proportion, they are said to be completely miscible. - Liquids that are partially soluble are said to be partially miscible. - **Immiscible**: - Liquids that are not soluble when mixed. ### Diagram of Miscible and Immiscible Liquids - Shows two liquid columns: one with miscible liquids and the other with immiscible liquids. ## Solubility - Diagram of solubility showing a glass with salt and water, a glass with sand and water, and a glass with oil and water. - **The glass with salt and water** show that salt dissolves in water, forming a homogeneous mixture. - **The glass with sand and water** shows that sand does not dissolve in water, this forms a heterogeneous mixture. - **The glass with oil and water** shows two immiscible liquids with no mixing. ## Concentration - In chemistry, **concentration** refers to the amount of a substance in a defined space, either solvent. - Concentration is usually expressed in terms of **mass per unit volume**. ### Formula for Concentration - Concetration = (mass of solute in grams) / (volume in dm3 (L)) - If less than 1 to 10 then its dilute. ## Solubility Terms: Concentrated vs Dilute - **Insoluble**: When a substance does not appear to dissolve in a solvent. - **A concentrated solution** has a relatively large amount of solute for a given quantity of solution. - **A dilute solution** has a smaller amount of solute for a given quantity of solution. ### Diagram of Concentrated vs Dilute Solutions - Shows two beakers with water and sugar, one labeled as concentrated and the other labeled as dilute. ## Assignment - What is the role and importance of chemical solutions in health? - The assignment is being prepared and presented by 4 students, and it is displayed to everyone in the class in the form of a presentation(Microsoft PowerPoint). ## Class Work - What is the physical process in which the substance changes from a solid to a gas by heating? - **a. Sublimation** - b. Melting - c. Solidification - d. Boiling ## Class Work - Which of the following is a mixture - A-sodium chloride NaCl - **B-NaCl and water** - C-Water - If 8 g of aspirin is dissolved in 2.5 dm3 of water. Calculate the concentration of the aspirin solution formed. - A-32 - B.320 - **C.3.2** ## Thank You - End of presentation.