Electronic transition – Flashcards
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| Electronic translation |
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| The movement of an electron from one energy level to another |
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| Electronic translation |
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| represented by means of an arrow |
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| Why was Bohr's model accepted? |
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| It was the FIRST model of them atom that could explain the hydrogen spectrum |
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| What is given off when an electron goes to a lower energy level? |
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| A proton of electromagnetic radiation |
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| How can an electron go to a higher energy level? |
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| Only by absorbing energy from an outside source |
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| When is an atom in an excited state? |
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| When one of its electrons has been promoted to a higher energy level |
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| When an atom is in the ground state, where are the electrons? |
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| In the lowest possible energy levels |
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| Emission spectrum of hydrogen atoms |
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| 1. Lymon Series 2. Balmen Series 3. Paschen Series |
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| Emission Spectrum of Hydrogen atoms |
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| Consists of thre series of lines |
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| Lymon Series |
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| - Produced by Uv photons - Due to transition of electrons from higher energy levels to n=1 |
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| Balmen series |
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| - Produced by visible photons - Due to the transitions of electrns from higher energy levels to n=2 |
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| Paschen Series |
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| - Produced by i.n. photons - Due to the transition of electrons from higher energy levels to n=3 |
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| What could Bohr's model of the atom explain? |
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| The spectra of single atoms with one electron |
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| The wavelike properties of electrons are useful for what? |
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| Magnifying objects |
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| Why was Rutherford's model replaced? |
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| 1. It couldn't explain why metals of compounds give off characteristic colors when heated 2. The chemical properties of the elements |
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| In Bohr's model, electrons are arranged in what? |
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| Specific, concentric, circular paths or orbits around the nucleus |
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| In Bohr's model, electrons in a particular circular path have a what? |
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| Fixed energy |
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| In Bohr's model, electrons in the cuircularpath closest to the nucles have the? |
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| Lowest energy |
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| In Bohr's model, electrons in the circular path furthest away from the nucles have? |
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| The highest energy |
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| In Bohr's model, electrons can? |
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| They can jump from one energy levels to another |
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| In Bohr's model, the amount of energy needed to move an electron from its present energy level to the next higher one is called? |
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| A quantum of energy |
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| In Bohr's Model, what gets closer the higher you go? |
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| Energy levels |
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| In Bohr's model, the elecgtron goes up the ladder and gets further away from the nuclus, what happens to the energy level? |
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| Increases |
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| Quantum Mechanical model |
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| Change Cloud model |
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| Quantum mechanical model |
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| Named after an area of physics which uses advanced math to study atoms and subatomic particles |
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| Who was one of the main people who developed the quantum mechanical model? |
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| Schrodinger |
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| The quantum mechanical model tells us atoms have: |
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| - Prinicipal energy levels - Sublevels - Orbitals |
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| What is similar to Bohr's energy levels? |
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| Principal energy levels |
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| 1, 2, 3, etc. What are these numbers called that are associated with principal energy levels? |
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| Principal quantum numbers; These numbers are represented by the letter m |
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| Principal energy levels conatin? |
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| One or more sublevels |
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| Each principal energy level has: |
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| - N sublevels - N squared orbitals - 2 N squared electrons when completely filled |
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| Sublevels of a prinipal energy level have: |
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| - Equal energies when the atom contains only 1 electron - Differen energies when the atom has more than 1 electron |
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| Are not the same as orbits |
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| Orbitals |
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| Region in space in which it is most likely to find an electron |
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| Orbital |
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| Each orbital can have a maximum of? |
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| 2 electrons (Called an orbital pair) |
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| Used to describe the placement of electrons in orbitals |
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| Orbital diagrams |
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| What is a half filled orbital represented by? |
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| A box or circle containing a single arrow pointed either up or down |
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| What is a filled orbital represented by? |
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| A box or circle containing 2 arrows, one pointing up and the other pointing down |
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| A shorthand notation describing the arrangement of electron in an atom |
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| Electron configuration |
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| Principle energy level |
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| Coefficent |
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| Type of orbital or sublevel |
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| Letter |
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| Orientation of orbital (optional) |
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| Subscript |
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| Number of electrons in an electron configuration |
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| Superscript |
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| Equals the total number of electrons in the atom |
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| Superscript Total of the Electron configuration |
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| Equals Z, the atomic number (total number of protons), when the atom is neutral |
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| Superscript total of the Electron Configuration |
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| How to simplify Electron configurations: |
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| 1. Do not use subscripts 2. Use mobile gas symbols |
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| Electrons enter orbitals of lowest energy first |
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| Aufbou principal |
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| An atomic orbital may have at most 2 electrons and they must have opposite spins |
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| Pauli exclusion principal |
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| When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with the same spin |
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| Hund's Rule |
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| Ground state Electron configuration Rules |
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| 1. Aufbou principle 2. Pauli exclusion principal 3. Hund's rule |
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| Filled sublevels are more stable than what? |
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| partially filled sublevels |
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| Half filled sublevels are not as stable as filled sublevels, but are more stable than? |
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| Other configurations |
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| The quantu mechanical model grew out of the study of what? |
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| Light |
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| Who thought of light as consisting of particles? |
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| Isaac Newton (1642-1727) |
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| By 1900, most scientists believed light was a? |
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| Wave |
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| A ____ is a wiggle (vibration) in time through space |
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| Wave |
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| The distance between 2 neighboring crests |
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| Wavelength (lambda) |
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| Number of wave cycles to pass a given point per unit of time |
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| Frequency (v, nu) |
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| The waves height from its origin (zero point) to the crest |
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| Amplitude (A) |
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| An arrangement of different types of waves acording to wavelength and frequency |
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| Spectrum |
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| Very well known spectrum |
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| Electromagnetic spectrum |
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| Inversely related |
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| Frequency and wavelength |
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| As wavelength increases- |
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| Frequency decreases |
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| The product of any 2 variables that are inversely related is equal to: |
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| A constant |
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| What are the two things that the modern theory of light says that light has? |
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| A wave of nature and a particle of nature |
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| The modern thoery of light says that light is composed of what? |
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| Photons |
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| A particle of ligh which has a frequency and wavelength |
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| Photon |
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| Bundle of energy |
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| Photon |
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| Producedf by electrons |
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| Photon |
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| Can travel billions of miles thrugh space and tell us the atoms that are present in the stars |
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| Photons |
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| Light is often composed of many different types of light each having a different? |
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| Wavelength and frequency |
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| Different types of light can often seperated by what? |
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| Using a prism |
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| When does every element emit light? |
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| When it is excited by the passage of an elctric discharge through its gas or vapor |
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| When light from excited elements pass through a prism, you get a? |
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| Atomic emission spectrum |
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| What does each element of light have? |
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| Its own, unique emission spectrum |
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| Each line in the emission spectrum is produced by an: |
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| Electronic transition |
