Chemistry 3: Mixtures and Solutions
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This document discusses the differences between pure substances, elements, compounds, and mixtures. It defines a pure substance as having all particles being the same, an element as having all atoms being the same, and a compound as having elements chemically combined in a repeating pattern. A mixture can be physically separated into its components without a chemical change and includes solutions, suspensions, and colloids. The document provides examples of each and discusses concepts like cohesion, adhesion, solubility, concentration, and techniques for separating mixtures like filtration, evaporation, distillation, and centrifugation.
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This document defines and provides examples of mixtures, solutions, suspensions, and colloids. It explains that mixtures can be physically separated into their original substances, while solutions appear homogeneous but are mixtures of a solute dissolved in a solvent on a molecular level. Suspensions and colloids are heterogeneous mixtures where particles settle out or scatter light differently. The document also defines elements as pure substances that cannot be broken down further, and compounds as pure substances formed by a chemical combination of elements in fixed ratios that have properties distinct from the original elements.
Mixtures, solutions, elements, compounds
This document defines and provides examples of mixtures, solutions, suspensions, colloids, and gas mixtures. It explains that mixtures can be separated physically but their compositions are not fixed, while solutions appear homogeneous but are mixtures that dissolve. Suspensions and colloids are mixtures where particles settle or scatter light differently. The document also defines elements as pure substances that cannot be broken down, and compounds as pure substances formed by chemical combination of elements in specific ratios producing new properties.
Mixtures, solutions, elements, compounds
This document defines and provides examples of mixtures, solutions, suspensions, colloids, and gas mixtures. It explains that mixtures can be physically separated into their original substances, while solutions appear homogeneous. Suspensions can settle out but colloids cannot. It also defines elements as pure substances that cannot be broken down further, and compounds as pure substances formed by a chemical combination of elements in fixed ratios that have unique properties.
MixturesandPureSubstances.ppt
An atom is to an element as a single unit is to a pure substance.
An atom is to a molecule as a single unit is to multiple units bound together.
An atom is to a compound molecule as a single unit is to multiple different units bound together.
Elements are pure substances made of single types of atoms. Molecules are multiple atoms of one or more elements bound together, such as in compounds. Compounds are made of two or more different elements chemically bonded together at the molecular level. Atoms are the fundamental unit that make up elements, and atoms can bond together to form molecules, such as in compounds.
MixturesandPureSubstances.ppt
An atom is to an element as a single unit is to a pure substance.
An atom is to a molecule as a single unit is to multiple units bound together.
An atom is to a compound molecule as a single unit is to multiple different units bound together.
Atoms are the basic building blocks that make up all matter. An element is a pure substance made of only one type of atom. A molecule is formed when two or more atoms of one or more elements are chemically bonded together. A compound is a pure substance composed of molecules made of two or more different elements chemically bonded together.
Matter and its Properties Part 2
Pure substances are made of only one type of atom or molecule, and can be elements or compounds. Mixtures contain two or more substances mixed but not chemically combined. Mixtures can be homogeneous, containing a uniform composition, or heterogeneous, where the composition varies. Separation techniques like filtration, evaporation, distillation, and decantation are used to separate mixtures based on differences in their physical properties.
Mixtures, solutions, elements, compounds
Mixtures and pure substances can be categorized and separated in different ways. Mixtures are combinations of substances that are not chemically combined and can be physically separated. Pure substances include elements, which consist of only one type of atom, and compounds, which are formed by chemical combination of two or more elements. Mixtures include heterogeneous mixtures where the parts can be easily distinguished, like mixtures, and homogeneous mixtures where the parts are evenly distributed and appear uniform, like solutions.
Matter.pptx
This document provides an introduction to chemistry and the properties of matter. It discusses the three common states of matter - solids, liquids, and gases. All matter is made up of either pure substances or mixtures of substances. Pure substances have a definite composition while mixtures maintain their individual identities. Common techniques for separating mixtures include filtration, evaporation, distillation, and chromatography. Consumer products contain various pure substances and mixtures tailored for different applications like household cleaning or personal care.
chapter_13.ppt
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Physical_ Chemistry_ Lecture_ 1111 .ppt
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MixturesandPureSubstances.ppt
Here are the key differences between pure substances and mixtures:
- Pure substances are either elements or compounds, which have a definite composition and properties. Mixtures can be composed of any substances.
- Elements are made of only one type of atom. Compounds are made of two or more elements chemically combined in a fixed ratio. Mixtures may contain multiple elements without fixed ratios.
- Particles in pure substances are molecules or atoms of a single type. Particles in mixtures can be molecules, atoms, or even larger phases that have not undergone a chemical reaction with each other.
- Pure substances have a consistent melting and boiling point as well as other properties. Mixtures can have varying properties depending on the relative amounts
Water 3
Water is a polar molecule that can form hydrogen bonds with up to four neighboring water molecules. These hydrogen bonds give water unique properties including high surface tension and the ability to act as a universal solvent. Water's density peaks at 4°C, allowing it to moderate temperatures on Earth. The hydrogen bonds between water molecules also allow water to act as a solvent for biochemical reactions and transport substances inside organisms.
The chemistry of life chapter 2
The document discusses the basics of chemistry as it relates to life. It covers the following key points in 3 sentences:
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Introduction to objective, scope and outcome the subject
Chapter 2
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Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
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Chapter 5
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Chapter 6
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Chemistry 3: Mixtures and Solutions
- 1. Chemistry 3: Mixtures & Solutions ppt. by Robin D. Seamon 1
- 2. 2
- 3. Pure Substance: all of the particles are the same Element: all the atoms are the same • Lots of the same atom Compound: elements are the same and chemically combined- in a repeating pattern • Lots of the same molecule mixture Can be physically separated compound Chemically bound element Chemically bound 3
- 4. 4
- 5. S T I C K I N G T O G E T H E R : • Cohesion- force that holds molecules of a material together • Adhesion- force that holds different substances together Water drop and water drop Water drop and paper 5
- 6. D I S S O L V I N G • Water is a solvent- it dissolves solutes of solids, liquids & gases • Solute- substance that dissolves • Solution- mixture of solvent and solute http://www.chem4kids.com/files/matter_ solution.html 6
- 7. W A T E R • universal solvent- most substances will dissolve in it WHY? • Polar- have two areas that have opposite charges negative near the oxygen b/c of unshared electrons positive near hydrogens fully shared electrons 7
- 8. S O L U T I O N S Solubility: ability of a solute to dissolve in a solvent at a certain temperature -Looks like a single substance; particles spread out evenly until the point of saturation • Concentration: amount of solute dissolved in a solvent • Dilute: less solute • Concentrated: lots of solute • Saturation: no more solute can be dissolved in the solvent 8
- 9. Borax snowflakes or Rock candy 9
- 10. M I X T U R E S Combination of two or more substances that are NOT chemically combined • No chemical change • Can be separated 1. Filter: use a sieve to separate liquid from larger particles 10
- 11. 2. Evaporation: heat water; water evaporates, solute remains in the container 11
- 12. 3. Distillation: separates based upon boiling points (crude oil into gasoline & kerosene) 12
- 13. 4. Magnet: separates iron & aluminum 13
- 14. 5. Centrifuge: spinning machine separates parts of blood 14
- 15. S U S P E N S I O N S Suspension- Mixture in which particles of a material are dispersed throughout a liquid or gas but are large enough that they settle out muddy water 15
- 16. C O L L O I D Colloid- mixture in which particles are dispersed throughout but are not heavy enough to settle out milk, mayonaise, gelatin, whipped cream 16
- 17. Pure Substance Element Compound Mixture Homogeneous Mixture Heterogeneous Mixture Carbon C Oxygen O Salt NaCl Sugar C H O Water H O2 2 2 12 22 11 Solution Alloy Saltwater NaCl + H O Brass Cu + Zn Bronze Cu + Sn Steel Fe + C Salad Conglomerate CLASSIFICATION OF MATTER 2 17
- 18. 18
- 19. 19
- 20. 20