PS+3+-+Properties+and+Classification+of+Matter

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 * ====Standard PS-3:==== || ====[|The student will demonstrate an understanding of various properties and classifications of matter.]==== ||
 * Indicators:**
 * || PS-3.1 || [|Distinguish chemical properties of matter (including reactivity) from physical properties of matter (including boiling point, freezing/melting point, density [with density calculations, solubility, viscosity, and conductivity). ]] ||
 * || PS-3.2 || [|Infer the practical applications of organic and inorganic substances on the basis of their chemical and physical properties.] ||
 * || PS-3.3 || [|Illustrate the difference between a molecule and an atom.] ||
 * || PS-3.4 || [|Classify matter as a pure substance (either an element or a compound) or as a mixture (either homogeneous or heterogeneous) on the basis of its structure and/or composition.] ||
 * || PS-3.5 || [|Explain the effects of temperature, particle size, and agitation on the rate at which a solid dissolves in a liquid.] ||
 * || PS-3.6 || [|Compare the properties of the four states of matter-solid, liquid, gas, and plasma-in terms of the arrangement and movement of particles.] ||
 * || PS-3.7 || [|Explain the processes of phase change in terms of temperature, heat transfer, and particle arrangement.] ||
 * || PS-3.8 || [|Classify various solutions as acids or bases according to their physical properties, chemical properties (including neutralization and reaction with metals), generalized formulas, and pH (using pH meters, pH paper, and litmus paper).] ||
 * || PS-3.8 || [|Classify various solutions as acids or bases according to their physical properties, chemical properties (including neutralization and reaction with metals), generalized formulas, and pH (using pH meters, pH paper, and litmus paper).] ||

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• Substances which have unique, identifying properties are called pure substances. • There are two types of pure substances: – Elements – Compounds • An element is a pure substance which is composed of only one type of atom. All of the elements are listed on the periodic table. • A compound is a pure substance which is composed of more than one type of element. • Some examples of elements include oxygen (O), carbon (C), iron (Fe), gold (Au), and fluorine (F). • Some examples of compounds include water (H2O), sugar (C12H22O11), rust (Fe2O3), and salt (NaCl). • The properties of compounds are different from the properties of the elements which compose them. • When two or more component substances which retain their own identifying properties, the matter is classified as a mixture. • Mixtures do not have a definite composition. The components of a mixture may be in any ratio. – You can have sweet tea that has a lot of sugar or sweet tea with less sugar. • A mixture can be separated physically because the components of the mixtures have different physical properties. • Heterogeneous mixtures do not have the components distributed evenly throughout. The different components are easy to see in a heterogeneous mixture. • Homogeneous mixtures have components distributed evenly throughout.

§  A physical property of a substance can be observed directly or measured with a tool without changing the composition of the substance. o  Boiling point, freezing/melting point o  Density o  Solubility o  Viscosity o  Electrical Conductivity §  A chemical property involves the substance to undergo a change that will alter the composition of the substance. §  A substance is soluble in a solvent if it will dissolve in that solvent. §  Solute - the substance being dissolved §  Solvent - what the substance is being dissolved in   §   Solubility is the maximum amount of solute that can dissolve in a given volume of solvent at a particular temperature and pressure. §  Viscosity is a measure of the material’s resistance to flow. High-viscosity fluids take longer to pour than low-viscosity fluids. §  When oxidation occurs, a substance combines with oxygen to form a new substance with new properties. §  The new substance formed is a combination of the atoms of the original substance and oxygen §  The properties of a substance change during the process of oxidation

• The dissolving process involves the sugar molecules being pulled away from each other. • The three factors that affect the rate of solution are: • Agitation (Which means movement or stirring) • Particle size • Temperature • The more a solution is agitated (meaning stirred), the faster the rate of solution • When a solution is agitated the water particles hit the surface of the solute (sugar) faster and the sugar crystals are dissolved (separated by water) faster • The smaller the size of the particles, the faster they will dissolve. • Smaller particles have more surface area than larger ones • This means that the particles have more space to contact the water and dissolve • The higher the temperature, the faster the rate of dissolving is for a solid in a liquid. • Higher temperatures cause water molecules to move faster. • This means that water molecules collide with the surface of the solute (sugar) and separate the sugar crystals from one another.

[[image:tempvstime.jpg]]
1. Solid - KE is increasing as temperature increases. solids are low energy, particles close together 2. Freezing/Melting Point- PE is increasing KE is staying the same 3. Liquid - KE is increasing as temperature increases. liquids are medium in energy and medium distance apart 4. Boiling Point - KE is staying the same and PE is increasing 5. Gas - KE is increasing as temperature increases. gases are high in energy and the particles are far apart

• Kinetic Theory • All matter is composed of small particles (molecules, atoms, and ions) •  The particles are in constant random motion •  The particles are colliding with each other and the wall of their container • Solids • The particles of solids are closely packed together because there is an attractive force holding them together • The particles of solids are constantly vibrating but they do not slip past one another • Because the particles cannot slip past one another, a solid cannot be poured, and a solid has a definite shape • Liquids • The particles of liquids are in contact with each other because there is an attractive force holding them together • The particles of liquids are moving fast enough to partially overcome the attractive force of the surrounding particles. Liquid particles can slip past surrounding particles and slide over one another. • Because the particles slip past one another, a liquid can be poured. • Gases • The particles of gases are not in contact with each other because they are moving fast enough to completely overcome the attractive force between or among the particles • The particles of gases are moving randomly, in straight lines until they bump into other particles or into the wall of the container. When a particle hits another particle or the container, it bounces off and continues to move. • More About Gases • Because gas particles move independently, a gas takes the shape of the container. The forces between particles are not strong enough to prevent the particles from spreading into different shapes. • Plasma • Plasma is matter consisting of positively and negatively charged particles • A substance is converted to the plasma phase at very high temperatures, such as those on stars (such as the sun). High temperatures means that the particles of a substance are moving at high speeds. At these speeds, collisions between particles result in the electrons being stripped from the atom.