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Domain 3 Structure and Properties of Matter I. Matter-any substance that occupies space and has mass A. States of matter State Shape Solid Definite shape Liquid Assumes shape of container Gas Fills container Volume Definite volume Definite volume Indefinite volume Video Clip B. Element 1. simplest form of matter; cannot be broken down into a simpler substance 2. made of atoms 3. represented by a symbol made of one or two letters. Example Na, C, Au, Ne C. Compound 1. a substance made of two or more elements that are chemically combined 2. represented by a chemical formula. ExampleNaCl, H2O, C6H12O6 3. the properties of the compound are different from the properties of the elements that make up the compound 4. can be separated only by a chemical reaction 5. two types of compounds a. ionic i. formed by the attraction between two or more elements that transfer electrons known as ions ii. example - NaCl (one metal ion and one nonmetal ion) b. Covalent (molecular) i. formed when two or more elements share electrons ii. example - H2O Video Clip D. Mixtures 1. different substances that are simply mixed together 2. can be separated by physical means (such as filtration, distillation, and chromatography) 3. Two types i. heterogeneous-does not have uniform composition; individual substances remain distinct. Examples are colloids and suspensions such as muddy water ii. homogeneous-has a uniform composition throughout. Example is a solution which is made up of a solvent and a solute such as koolaid or salt water E. Ions 1. Ions are atoms which have gained or lost electrons. 2. examples include Na+, Cl-, Mg2+, O2Try this online quiz on the organization of matter II. Physical and Chemical Properties A. Physical properties 1. properties that are determined by observation, either looking or measuring 2. examples include color, mass, density, odor, luster, malleable, ductile B. Chemical Properties 1. can only be found through testing 2. example includes flammability III. Chemical and Physical Changes Video Clip A. In a physical change, the original substance still exists. 1. Any change in size, shape, or phase is a physical change. It has only changed form. 2. There are six phase changes. Phase change What happens Melting Solid becomes liquid Vaporization Liquid (boiling or becomes gas evaporation) Sublimation Solid become gas Freezing Liquid becomes solid Condensation Gas becomes liquid Deposition Gas becomes a solid 3. Energy change Absorbs Endothermic heat Absorbs Endothermic heat Absorbs heat Releases heat Releases heat Releases heat Endothermic Exothermic Exothermic Exothermic 4. Other examples of physical changes include dissolving, crushing, mixing. B. In a chemical change, a new substance is produced. 1. Energy changes always accompany chemical changes. 2. Chemical changes can be accompanied by physical changes. 3. Identification of a chemical change involve careful examination of the original reactants to see if new substances (products) are produced. i. a gas is formed ii. temperature change iii. precipitate forms iv. appearance of a new color or odor 4. Examples of chemical changes include fermentation, metabolism, electrolysis. IV. Atomic Structure A. Atom 1. the smallest particle of an element that retains the properties of that element 2. Models of the atom through history a. Dalton’s model-solid and indivisible b. Thomson-plum pudding model c. Rutherford-gold foil experiment-the electrons orbit around the dense nucleus Click here for animation of the gold foil experiment d. Bohr model In the Bohr model there were distinct energy levels where electrons could exist. •1st energy level holds 2 electrons •2nd energy level holds 8 electrons •3rd energy level holds 8 then 18 after 4th level gets 2 electrons. Which element is this? e. Modern View of the Atom The atom is mostly empty space. Two regions •Nucleus- center region; positively charged, contains most of the atom’s mass •Electron cloud- region where you might find an electron. 3. Subatomic particles a. nucleus-center region; positively charged; contains most of the atom’s mass Video Clip i. proton –positive particle ii. neutron-neutral particle (no charge) b. electron cloud i. outer region of the atom; mostly empty space ii. electron-the negative particle located in energy levels in the electron cloud; involved in bonding electron neutron proton Video Clip 4. Neutral atoms have the same number of protons and electrons. 5. Isotopes are atoms that have the same number of protons but different numbers of neutrons. They have the same atomic number but different masses. Click here for video clip Click here for tutorial on isotopes 6. The atomic number of an element is the number of protons it has in the nucleus. Video Clip 7. The mass number is the number of protons plus the number of neutrons. 8. Atomic mass is the average mass of an atom of a particular element. Summary Click here to practice calculating protons, neutrons, and electrons Subatomic Charge Particle Proton, p+ positive Nucleus Neutron, no neutral Nucleus Electron, e- Electron cloud negative Location Mass (amu) 1 Number in atom Same as atomic number 1 Mass number – atomic number 1/1840 Same as number of protons II. Periodic Table (remember there is of one in your test booklet) A. Organization 1. The periodic table is organized by increasing atomic number and is read from left to right. 2. Each vertical column is called a group or family. All the elements in a family have the same number of valence electrons 3. Each horizontal row is called a period. All elements in the same period have the same ending energy level (where electrons are found). Video Clip B. Get to know the arrangement 1 2 3 4 5 6 1. 2. 3. 4. 5. 6. 7. 8. 8 7 metals nonmetals metalloids Alkali metals (most reactive metals) Alkaline Earth metals Transition metals Halogens (most reactive nonmetals) Noble gases (most unreactive elements) C. Valence electrons are the electrons in the outermost energy level of an atom. III. Solutions A. Solutions are homogeneous mixtures of two or more elements and/or compounds. The major component is called solvent, and the minor components are called solute. 1. A solute is the dissolved substance in a solution. There is less of it. salt in salt water sugar in soda carbon dioxide in soda 2. A solvent is the dissolving medium. You have more of it. water in salt water water in sodas Solutions Video Clip 3. Soluble – describes any substance that will dissolve in a solvent 4. Insoluble – any substance that will not dissolve in a solvent Solubility video clip B. Concentration-amount of solute dissolved in the solvent 1. Concentrated vs. dilute 2. Saturation of solutions a. Saturated – contains the maximum amount of dissolved solute in a given amount of solvent at a specific temperature and pressure b. Unsaturated – contains less than the maximum amount of dissolved solute in a given amount of solvent at a specific temperature and pressure c. Supersaturated – contains more than the maximum amount of dissolved solute in a given amount of solvent at a specific temperature and pressure C. Conductivity refers to the ability of a solution to conduct electricity. 1. Electrolytes are substances that dissolve in water to produce ions. These ions carry the electrical current through the solution. a. Strong electrolytes ionize completely in aqueous (water) solutions. b. Weak electrolytes are only partially converted to ions in aqueous solution. c. Examples of electrolytes ionic compounds such as NaCl (sodium chloride) acids and bases such as HCl (hydrochloric acid) and NaOH (sodium hydroxide) 2. Nonelectrolytes are substance whose aqueous solutions do not contain ions and do not conduct an electrical current. Click here to see NaCl dissolve