Matter. Properties and Changes
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1 Matter Properties and Changes
2 Objectives Differentiate between forms of matter including elements, compounds, and mixtures. Explain the difference between a physical and chemical change. Explain the parts of a phase diagram and what is occuring at each part.
3 Bookwork 3-MATTER AND CHANGE Chapter 2 and 17.1 Problems: Chap. 2: 14, 16, 24, 26, 29, 30, 35, 38, 41, 43, 54, 56
4 Core Content Terms Matter Mass Physical Property Chemical Property Phase Solid Liquid Gas Extensive Property Heterogeneous Mix. Homogeneous Mix. Element Compound Chemical Reaction Reactants Products Law of Conservation of Mass Intensive Property
5 Matter Anything that has mass and takes up space. 2 Categories: 1. Pure Substances 2. Mixtures
6 Pure Substances Matter that has a uniform unchanging composition Cannot be separated by physical means Example: Sugar or Water Have identical physical properties (Color, Odor, density )
7 Types of Substances Elements Cannot be separated even by chemical means One type of atom Examples: Gold, Au Carbon, C Compounds Can be separated by chemical means Composed of 2 or more different elements in whole number ratios Examples: Water, H 2 O Salt, NaCl
8 What makes up Substances? Atom: The smallest particle of an element that retains all the properties of that element Comprised of protons, neutrons and electrons
9 Mixtures Combination of two or more substances Can be separated by physical means Example: Saltwater or Trail mix
10 Types of Mixtures Homogeneous A mixture with no physically distinct parts in the solution Examples: Kool Aid Air Heterogeneous A mixture with distinct physical parts Examples: Italian dressing Orange juice
11 Separating Mixtures of Matter Filtration-solid component trapped by filter paper Decant- pour liquid off solid (which has settled to the bottom) Centrifuge- centripetal force used to separate liquid and solid components Chromatography- separates mixtures based on solubility, boiling point, and other properties Paper chromatography, gas chromatography, liquid chromatography
12 Changes Physical Change: Change that does not alter the chemical composition of the substance. Examples: Phase Changes (Ice melting) Chemical Change: One or more substances are changed into other substances Ex: Metal Rusting or Batteries corroding
13 Physical Properties Properties that do not involve or describe a substance changing into another substance (Same after change) Characteristic that can be observed or measured without changing the sample s composition. Ex: Melting Point, Boiling Point, Hardness, and Luster
14 Physical Properties Extensive Properties: Depends on the amount of a substance Ex: Mass, Length, Volume Intensive Properties: Does not depend on the amount of the substance present Ex: Density, Solubility
15 Chemical Properties The ability of a substance to combine with or change into one or more other substances. Ex: Methane reacts with oxygen to form carbon dioxide and water Represented by a chemical equation: CH 4 + O 2 CO 2 + H 2 O Reactants change to Products
16 Start Up Identify each as an element, compound, heterogeneous, or homogeneous mixture 1. Air 2. Coffee 3. Cookie dough blizzard 4. Hydrogen gas 5. Carbon dioxide
17
18 Colligative Properties Can change certain properties of a substance by adding particles of another substance Number of particles are the only thing that is important not the composition of the added substance Examples: Boiling point elevation Freezing point depression
19 Energy and Matter Energy (heat or light) always involved in physical or chemical changes of matter The matter (mass) is never created or destroyed only assumes a different form. Law of conservation of mass The energy is never created or destroyed only assumes a different form. Law of conservation of energy
20 States of Matter Atoms are in constant motion The rate at which atoms or molecules in a substance move determines its state
21 Solids Intermolecular forces are very strong Particles remain relatively fixed Particles are closely packed and travel a distance equal to only a fraction of their diameter. (Don t move much) Solids have definite shape and volume
22 Liquids Particles are limited in their motion because of intermolecular forces Particles travel in a straight-line by slipping past each other (stay in contact and are dependent on each other) have a definite volume but assume the shape of their containers
23 Gases Particles are independent of each other Travel randomly in straight lines Assume the shape and volume of their container Have very weak intermolecular forces except in cases of extreme temperature and pressure
24 Plasma Matter is heated to extreme temperatures Electrons are knocked away from atoms Most of the universe is made of plasma including stars Many lasers are made of compounds in a plasma state
25 Solids, Liquids, Gases and Molecular Movement Given the same substance As phases change from a solid the average kinetic energy (molecular movement/ Temp) of particles increases Temperature of the solid, liquid, and gas is limited because of the maximum molecular speed
26 Heat Curve for Water
27 Phase Diagram
28 Phase Diagram Activity Change_Diagram_WSv103.pdf
29 Start Up 1. Sketch a heat diagram for water. 2. Explain why the temperature levels off instead of increasing with heat in certain points. 3. Identify each as a chemical or physical change: Water Boiling Leaves changing color in the fall Milk spoiling after two weeks in the fridge Shredding a cancelled check Burning a cancelled check
Intensive Properties are Independent.
Chapter 3: Matter- Properties and Changes Section 3.1: Properties of Matter SUBSTANCE: matter that has an uniform and unchanging composition EXAMPLES: gold, pure water, iron, aluminum PHYSICAL PROPERTIES:
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