Electronegativity. Ionization Energy & Electron Affinity. Ionization Energy & Electron Affinity. Electronegativity. Chapter 7: Periodic Properties of the Elements. There are a number of atomic characteristics that either increase or decrease along the periodic table. Atomic Radius:By misha
Combinations of Atoms. Chapter 8.2. Compounds. Compounds Elements are rarely found pure in the earth, they are generally found as compounds. A compound is a substance that results when the atoms of two or more elements are chemically combined. Compounds.By denali
Nomenclature. Naming Compounds. Ionic Compounds. Metal bonding with non-metal One atom gains electrons, one atom loses electrons Exist as ions with full highest energy levels. Are held together in a giant crystal by the electrostatic attraction of the opposite charges.By feng
Ionic and Metallic Bonding. And how!. 1/5/12. Objective: To review the fundamentals of ions and learn about ionic bonding Do now: Do the hokey pokey. Turn yourself around. Then write down what a valence electron is and how many aluminum and gold have. (4 minutes!) Le homework:By nerina
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Energy Levels. And Drawing Energy Level Diagrams. Energy Levels. Electrons travel within the Electron Cloud, but at different distances from the nucleus. Energy Level close to nucleus - Low Energy Electrons Energy Level farthest away - High Energy Electrons. Electrons in Energy Levels.
Energy Levels. Quantum Physics Lesson 4. Learning Objectives. Explain what is meant by the term energy level. Describe what happens when excited atoms de-excite. Calculate the energy of emitted photons using the equation hf = E 1 - E 2 . Explain how a fluorescent tube works HWK.
Energy Levels. Electrons. Nucleus . Sodium at room temperature . Who discovered Sodium and when?. Humphry Davy is credited with being the first to discover sodium as he was the first person to isolate the metal from caustic soda in 1807. What is sodium used for?.
Energy levels and sub-levels. Electron Configurations. Energy levels and sub-levels. Energy levels. These are broadly similar to the “shells” used in the Bohr Model.
Electron Energy Levels. Not all electrons in an atom have the same energy They exist in discreet energy levels These levels are arranged in shells (n = 1, n = 2…) Electrons closer to the nucleus have lower energy (stabilized by positively charged nucleus)
Hydrogen energy levels. Paschen. Lyman. Balmer. Hydrogen atomic energy levels. E=hf = hc/ λ. Paschen. Spectra produced by transitions of electrons from upper energy levels to n=3 level. These are in the Infra red region. n=infinity. n=5. -0.54eV -0.85eV -1.5eV -3.4eV -13.6eV.
ENERGY LEVELS AND SPECTRA. The Electromagnetic Spectrum. wavelength. frequency. Gamma 10 -11 – 10 -13 m. X-rays 10 -9 – 10 -11 m. 700 nm. 400 nm. Visible. Microwaves cms. Radio 1 - 2000 m. IR 10 -3 – 10 -7 m. UV 10 -7 – 10 -9 m. Line Spectrum, unique to the gas.
Lecture 9 Energy Levels. Translations, rotations, harmonic oscillator Independence of energy storage Many particle systems Independent distinguishable particles Independent indistinguishable particles. Energy levels from quantum mechanics.
Wavefunctions and Energy Levels. Since particles have wavelike properties cannot expect them to behave like point-like objects moving along precise trajectories.