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Transcript
Introduction to Atoms Lesson Objectives •Compare and contrast the atomic theories •Select a depiction for each atomic theory •Define vocabulary: atom, electron, nucleus, proton, energy level, and valence electron What’s in the box? 430 BC Democritus What is an atom ? atom the smallest particle that still can be considered an element The idea of atoms began to develop anew in the 1600s with research shaping ideas. Atomic theory grew as a series of models that developed from experimental evidence. As more evidence was collected, the theory and models were revised. Dalton Scientist Atomic Model Dalton atoms are smooth, hard balls electrons positive charge Thomson Scientist Atomic Model Dalton atoms are smooth, hard balls Thomson electrons scattered throughout a positive ball Rutherford space for electrons nucleus nucleus small region in the center of an atom electron negatively charged particles that orbit the nucleus Later research suggested that the nucleus was made up of one or more positively charged particles. Rutherford called the positively charged particles in an atom’s nucleus protons. proton positively charged particles in the nucleus of an atom Scientist Atomic Model Dalton atoms are smooth, hard balls Thomson electrons scattered throughout a positive ball Rutherford protons in nucleus surrounded by electrons Bohr Scientist Atomic Model Dalton atoms are smooth, hard balls Thomson electrons scattered throughout a positive ball Rutherford protons in nucleus surrounded by electrons Bohr electrons found only in specific orbits Electron Cloud Theory energy level the specific amount of energy of an electron Scientist Atomic Model Dalton atoms are smooth, hard balls Thomson electrons scattered throughout a positive ball Rutherford protons in nucleus surrounded by electrons Bohr electrons found only in specific orbits Electron Cloud electrons move rapidly in electron cloud Bohr Model Electron Energy Levels •Electrons in levels farther away from the nucleus have more energy. •Energy levels hold a specific amount of electrons. Electron Energy Levels st 1 The energy level holds up to 2 electrons. Electron Energy Levels nd 2 The energy level holds up to 8 electrons. Electron Energy Levels rd 3 The energy level holds up to 8 electrons. Valence Electrons •Located in the outer energy level •Have the highest energy valence electrons electrons in the atom’s outer energy level
