Do Now: Bohr Diagram, Lewis Structures, Valence Electrons 1. What is the maximum number of electrons you can fit in each shell?
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1 Chemistry Ms. Ye Name Date Block Do Now: Bohr Diagram, Lewis Structures, Valence Electrons 1. What is the maximum number of electrons you can fit in each shell? 1 st shell 2 nd shell 3 rd shell 4 th shell 2. What are valence electrons? 3. What is the main difference between a Bohr diagram and a Lewis structure? 4. What is the maximum number of valence electrons an atom can have? Complete the Table Below: Element Subatomic Particles Bohr Diagram # Valence Electrons Lewis Structure Phosphorus-31 # protons= # neutrons= # electrons= Fluorine-19 # protons= # neutrons= # electrons=
2 Electromagnetic Radiation a form of that has wavelike properties all forms found in the spectrum The different forms of EMR arranged in order from lowest energy to highest energy Examples of Electromagnetic Radiation: Type of EMR Real-life example Radio waves Microwaves Infrared Visible light Ultraviolet (UV) light X-rays Properties of Waves i. and are two important properties of waves. ii. iii. iv. - The shortest distance between two equivalent points (meters) - How many waves pass a certain point per second (1/s or s - or Hz). - The height of a wave from crest to origin. v. What kind of relationship do frequency and wavelength have? vi. What kind of relationship do frequency and Energy have? vii. What kind of relationship do energy and wavelength have?
3 Energy, Wavelength, and Frequency: Qualitative Comparisons: 1. WAVE A WAVE B Wave B has a frequency than wave A. Wave B has a wavelength than wave A. Wave B has a energy than wave A. 2. When comparing the radio stations 96.7 MHz and 92.3 MHz a. Which one has a higher energy? How do you know? b. Which one has a longer wavelength? How do you know? 3. Red light has a longer wavelength than blue light a. Which color light has a higher energy associated with it? Why? b. Which color light is emitted at a higher frequency? How do you know?
4 Photons Released during. Tiny particles that have no All photons travel at the which carry a quantum of Can calculate wavelength if we know frequency and vice versa. in a vacuum (c = 3.00 x 10 8 m/s) Photons behave as particles o Quantum the amount of energy that can be absorbed or released from an atom. Cannot be any value but are in discrete energy levels ENERGY EQUATIONS = = E= energy h= Planck s Constant = x J*s c= speed of light = 3.00 x 10 8 m/s v= frequency (in Hz or 1/sec) λ=wavelength in meters EXAMPLES: 1. What is the frequency of green light, which has a wavelength of 4.9 x 10-7 m? = 2. A popular radio station broadcasts with a frequency of 94.6 MHz (= 94,600,000 Hz). What is the wavelength of the broadcast? 3. What is the energy of an infrared wave with the frequency of 2.56 x s -1? 4. What is the energy of an x-ray which has a wavelength of 2.4 x m? 5. The energy of a wave is 1.98 x J. What is the wavelength and the type of wave?
5 Electrons and Energy Levels Each electron has a distinct amount of related to the energy level (shell) it is in Electrons with the lowest energy are found in the shell Electrons with the highest energy are found in the shell How many electrons can each energy level (electron shell) hold? Electron Shell n=1 n=2 n=3 n=4 # of electrons The from the nucleus, the of the electron Ground State vs. Excited State Ground state=when the electrons occupy the Excited state=electrons are (even when a lower energy levels is not completely full) When an electron, it jumps to a energy level or shell o This is a very condition o We call this condition the Very rapidly, an electron in the excited state will and move back to a energy level or shell o When excited electrons fall from an excited state to a lower energy level, they release energy in the form of (which can be infrared, ultraviolet, or visible) (Energy: heat, light, electricity) Photon (Energy: light)
6 Summary: Ground State Excited State Energy is is produced Excited State Ground State Energy is is produced Bright Line Emission Spectrum (Visible Light Spectrum) Electrons falling from an down to the give off light Different elements produce different colors of light or The atomic emission spectrum is for (just like a human fingerprint is unique to each person) We use spectral lines to identify different elements. Demo: Substance Color 1. Which statement describes how an atom in the ground state becomes excited? a) The atom absorbs energy, and one or more electrons move to a higher electron shell b) The atom absorbs energy, and one or more electrons move to a lower electron shell c) The atom releases energy, and one or more electrons move to a higher electron shell d) The atom releases energy, and one or more electrons move to a lower electron shell 2. The light emitted from a flame is produced when electrons in an excited state a) Absorb energy as they move to lower energy states b) Absorb energy as they move to higher energy states c) Release energy as they move to lower energy states d) Release energy as they move to higher energy states
7 Waves & Energy HW: Describe the relationships between energy, frequency, and wavelength 1. What is the relationship between energy and frequency? 2. What is the relationship between energy and wavelength? 3. What is the relationship between frequency and wavelength? 4. In the diagrams below, which wave has the higher frequency? Higher wavelength? Higher energy? Wave A Wave B ENERGY EQUATIONS = = = E= energy h= Planck s Constant = x J*s c= speed of light = 3.00 x 10 8 m/s v= frequency (in Hz or 1/sec) λ=wavelength in meters 5. One of the lines in the emission spectrum of sodium has a wavelength of 5.9 x 10-7 m. What is the frequency of this line? 6. A radio station broadcasts at a frequency of Hz. What is the wavelength of this EM wave? 7. Calculate the energy of a gamma ray photon with a frequency of Hz. 8. When an electron in a hydrogen atom drops from the fifth to the second energy level, J of energy is released. Find the frequency of the photon that is produced. 9. Describe the energy changes that happen when an electron transitions between ground and excited state. During which transition to we see light given off?
Bohr Diagram, Lewis Structures, Valence Electrons Review 1. What is the maximum number of electrons you can fit in each energy level or shell?
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Atomic Spectra Objectives The objectives of this experiment are to: 1) Build and calibrate a simple spectroscope capable of measuring wavelengths of visible light. 2) Measure several wavelengths of light
Chapter 6 Electronic Structure of Atoms
Chapter 6. Electronic Structure of Atoms NOTE: Review your notes from Honors or regular Chemistry for the sequence of atomic models and the evidence that allowed scientists to change the model. If you