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Matter and Atomic Structure Chap. 3 • What are elements? • How atoms combine • States of matter What makes a gold atom different from a silver atom? What are elements? – 3.1 Objectives • Describe the particles within atoms and the structure of atoms • Relate the energy levels of atoms to the chemical properties of elements •Define the concept of isotopes I. Element Element Substance that cannot be broken down into simpler substance by physical or chemical means. I. Element A. Element names Carbon 6 C 12.011 I. Element A. Element names B. Element symbols Carbon 6 C 12.011 I. Element A. Element names B. Element symbols C. Elements are made of atoms II. Atoms Atom Smallest particle of an element. II. Atoms A. Composed of 3 particles II. Atoms A. Composed of 3 particles 1. Protons II. Atoms A. Composed of 3 particles 1. Protons 2. Neutrons II. Atoms A. Composed of 3 particles 1. Protons 2. Neutrons nucleus II. Atoms A. Composed of 3 particles 1. Protons 2. Neutrons 3. Electrons II. Atoms A. Composed of 3 particles B. Atomic number Atomic number Number of protons. proton neutron Atomic number Number of protons. proton neutron 5 II. Atoms A. Composed of 3 particles B. Atomic number C. Mass number Mass number Sum of the number of protons and neutrons proton neutron Mass number Sum of the number of protons and neutrons proton neutron 11 II. Atoms D. Electrons in Energy Levels Electron Energy Levels Energy level First Second Third Fourth Electron Capacity 2 8 18 32 Model of Oxygen Self Check – Ex. 1 Draw a model of the lithium-7 atom. Include protons, neutrons, and electrons. Self Check – Ex. 2 Draw a model of the chlorine-35 atom. Include protons, neutrons, and electrons. II. Atoms D. Electrons in Energy Levels 1. Core electrons II. Atoms D. Electrons in Energy Levels 1. Core electrons 2. Valence electrons Valence electron Outermost electron found in a shell. III. Isotopes Isotopes Atoms with the same number of protons, but different numbers of neutrons. III. Isotopes A. Isotopes have different masses III. Isotopes A. Isotopes have different masses B. Nature contains a variety of isotopes III. Isotopes A. Isotopes have different masses B. Nature contains a variety of isotopes C. Isotopes used to find atomic mass of element Atomic mass The average of the masses of each isotope present for a give element. III. Isotopes D. Radioactivity Radioactivity The spontaneous decay of an atom’s nucleus into a new nucleus. IV. Abundance A. In Universe Abundance in Universe IV. Abundance A. In Universe B. In Earth’s crust Abundance in Earth’s Crust The End How atoms combine – 3.2 Objectives • Describe the chemical bonds that unit atoms to form compounds • Relate the nature of chemical bonds that hold compounds together to the physical structures of compounds •Distinguish between different types of mixtures and solutions I. Compounds Compound More than one element chemically combined. I. Compounds A. Covalent compounds share electrons I. Compounds A. Covalent compounds share electrons 1. Sharing electrons helps atoms get full electron set I. Compounds A. Covalent compounds share electrons 1. Sharing electrons helps atoms get full electron set 2. Sharing may not be equal: this makes polar molecules I. Compounds B. Ionic compounds transfer electrons I. Compounds B. Ionic compounds transfer electrons 1. When an atom gains an electron it becomes _______ I. Compounds B. Ionic compounds transfer electrons 1. When an atom gains an electron it becomes _______ 2. When an atoms loses an electron it becomes _______ Ion An atom that has gained or lost an electron. I. Compounds B. Ionic compounds transfer electrons 1. When an atom gains an electron it becomes _______ 2. When an atoms loses an electron it becomes _______ 3. Opposites _______ I. Compounds C. Metallic bonds have a ‘sea of electrons' II. Reactions II. Reactions A. Bonds are broken and reformed II. Reactions A. Bonds are broken and reformed B. New substances are formed II. Reactions A. Bonds are broken and reformed B. New substances are formed C. Energy is exchanged III. Mixtures III. Mixtures A. Most mixtures are heterogeneous Heterogeneous A mixture with visibly different parts. III. Mixtures A. Most mixtures are heterogeneous B. Mixtures that are homogeneous are called solutions Homogeneous A mixture with the same makeup throughout. IV. Acids & Bases IV. Acids & Bases + A. An acid makes H ions IV. Acids & Bases + A. An acid makes H ions B. A base produces OH ions IV. Acids & Bases + A. An acid makes H ions B. A base produces OH ions C. The pH scale tells how acidic/basic something is The pH Scale 0 1 acidic 3 5 7 9 neutral 11 13 14 basic The End States of Matter – 3.3 Objectives •Describe the states of matter on Earth • Explain the reasons that matter exists in these states • Relate the role of thermal energy to changes of state in matter I. The Four Phases of Matter I. The Four Phases of Matter A. Solid I. The Four Phases of Matter A. Solid 1. solids with regular structure are described as crystalline. I. The Four Phases of Matter A. Solid 1. solids with regular structure are described as crystalline. 2. in some solids there is no organized pattern. These are amorphous. I. The Four Phases of Matter A. Solid B. Liquid I. The Four Phases of Matter A. Solid B. Liquid C. Gas I. The Four Phases of Matter A. Solid B. Liquid C. Gas 1. gases have undergone vaporization or sublimation Evaporation Changing from liquid to vapor Sublimation Changing from solid to vapor I. The Four Phases of Matter A. Solid B. Liquid C. Gas 1. gases have undergone vaporization or sublimation 2. gas particles are separated by large distances I. The Four Phases of Matter A. Solid B. Liquid C. Gas D. Plasma Plasma Hot, highly ionized, electrically conducting gas. II. Changes in State II. Changes in State A. When a liquid changes to a gas, heat is _______. II. Changes in State A. When a liquid changes to a gas, heat is _______. B. When a gas changes to a liquid, heat is _______. The End