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Atomic orbital

Atomic Structure

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Biology
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Atomic physics
Quantum chemistry
Chemical bonding
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Atomic orbital
electron
Energy level
Emission spectrum
Photoelectric effect
Spin quantum number
Wave–particle duality

Atomic Structure Atomic structure of an atom based on energy relative to size of an electron can be measured with Einstein?s formula of e=mc2. However, energy of an electron within an atom based on how long a wavelength takes to pass can be determined with the formula of constant= wavelength x frequency. Electromagnetic Radiation is described with wavelike energy with both magnetic and electrical properties. Waves of electrons (atoms) are within radiation additionally wave measurements can be made with the wavelength, frequency, and the speed of light (constant). Wavelength= Indicated with lambda, described as the length of a wave from one crest to another. Frequency= Measured in Hz (1/s), the number of waves that pass per second

AP Chemistry Zumdahl 7E Chapter 9 Notes

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Chemistry
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Chemical bonding
Orbital hybridisation
Molecular orbital
Covalent bond
Antibonding molecular orbital
Pi bond
Delocalized electron
Atomic orbital
Chemical bond
Double bond
Sigma bond
Unpaired electron

1 Chapter 9 - Covalent Bonding: Orbitals 9.1 Hybridization and the Localized Electron Model A. Hybridization 1. The mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies B. Hybrid Orbitals 1. Orbitals of equal energy produced by the combination of two or more orbitals on the same atom C. Evidence for hybridization of carbon - Methane and sp3 1. Four bonds of equal length and strength Carbon's isolated configuration Carbon's hybridized configuration 2. Four effective pairs of electrons surround the carbon 3. "Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, this model assumes that the atom adopts a set of sp3 orbitals; the atom becomes hybridized"

AP Chemistry Zumdahl 7E Chapter 7 Notes

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Chemistry
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Atomic physics
Quantum chemistry
Chemical bonding
Molecular physics
Theoretical chemistry
Atomic orbital
Energy level
electron
Aufbau principle
Principal quantum number
Ionization energy
Bohr model

AP Chemistry A. Allan Chapter 7 Notes - Atomic Structure and Periodicity 7.1 Electromagnetic Radiation A. Types of EM Radiation (wavelengths in meters) 10-12 10-10 10-8 4 to 7x10-7 10-4 10-2 1 102 104 Wavelength increases Frequency decreases Energy decreases Speed is constant = 2.9979 x 108 m/sec B. Properties of EM Waves 1. Wavelength (l) a. Distance between two consecutive peaks or troughs in a wave b. Measured in meters (SI system) 2. Frequency (n) a. Number of waves that pass a given point per second b. Measured in hertz (sec-1) 3. Speed ( c ) a. Measured in meters/sec 4. Relationship of properties a. c=nl gamma xrays UV visible IR micro Radio waves FM short AM 7.2 The Nature of Matter

Campbell9thEdChapter2ChemicalContextofLife

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Biology
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Chemical bonding
Chemical bond
Covalent bond
Valence electron
Valence
Ionic bonding
Chemistry
Lewis structure
Electronegativity
Atomic orbital
Hydrogen bond
ion

The Chemical Context of Life Chapter 2 Matter consists of chemical elements in pure form and in combinations called compounds Organisms are composed of matter Matter is anything that takes up space and has mass ? 2011 Pearson Education, Inc. Elements and Compounds Matter is made up of elements An element is a substance that cannot be broken down to other substances by chemical reactions A compound is a substance consisting of two or more elements in a fixed ratio A compound has characteristics different from those of its elements ? 2011 Pearson Education, Inc. Figure 2.3 Sodium Chlorine Sodium chloride The Elements of Life About 20?25% of the 92 elements are essential to life, but it varies among organisms Humans need 25 elements while plants only need 17 elements

Principles of Chemistry Chapter 6

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Chemistry
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Atomic physics
Quantum chemistry
Molecular physics
Chemical bonding
Chemical properties
Atomic orbital
Energy level
electron configuration
electron
Aufbau principle
Hund's rule of maximum multiplicity
Bohr model

Chapter 6: The Periodic Table & Atomic Structure Section 6.2: The Electromagnetic Spectrum Monday, September 15, 2014 3:06 PM Visible Light - portion of electromagnetic spectrum that we can see, typically with wavelengths between 400 / 700 nanometers ? Electromagnetic Spectrum - various forms of light, consisting of oscillating electric and magnetic fields ? ? ? The Wave Nature of Light ? Wavelength - distance between corresponding points on a wave Amplitude - height of the wave from equilibrium position Frequency - number of cycles of a wave passing a certain point per second (measured in Hz) **note: amplitude corresponds with brightness, wavelength and frequency correspond with color ? Speed of light ( c ) : c = lamda x v = wavelength x frequency ? The Particulate Nature of Light

AP Biology Basic Chemistry

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Biology
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Chemistry
Physics
Chemical bonding
Chemical bond
Valence electron
Covalent bond
electron
Lewis structure
ion
Atomic orbital
Chemical polarity
Atomic theory
Technology

Resch/Stuart AP Biology Basic Chemistry Basic Chemistry Review Directions: Since this will be handed in digitally, please type all response in bold directly below the question. ?Once you are done, please submit this document via google drive. ?Remember that this is due by Aug. 18th. Review: J.J. Thomson?s Plum Pudding model and ionic vs. molecular bonding

Chapter 8

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Chemistry
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Chemistry
Physics
Atomic physics
Quantum chemistry
Chemical bonding
Molecular physics
Chemical properties
Atomic orbital
electron configuration
Aufbau principle
Quantum number
Energy level
Technology
behavior
Human development
Interpersonal relationships
Love
Psychoanalysis
Human behavior
Attachment theory
Evolutionary biology
Personal life

Chemistry 1210: Introduction to General Chemistry Dr. Gina M. Florio 05 November 2012 Jespersen, Brady & Hyslop Chapter 8 The Quantum Mechanical Atom Quantum Mechanics Ch. 8.1 The physics that describes objects with wave-particle duality is called quantum mechanics or quantum theory. In the late 1800?s, scientists discovered that electrons acted like tiny charged particles in some experiments and waves in others. Quantum mechanics accurately describes the structure and reactivity of atoms and molecules. Electromagnetic Radiation Ch. 8.1 Energy can be transferred as heat or as light. Electromagnetic radiation can be carried energy through space in the form of electromagnetic waves.

Atomic Structure

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Chemistry
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Physics
Chemistry
Atomic physics
Quantum chemistry
Rotational symmetry
Introductory physics
Quantum electrodynamics
Bohr model
Introduction to quantum mechanics
Atomic orbital
electron
Principal quantum number
Technology

The Wave Nature of Light All forms of NRG/Light have characteristic wavelengths (?) and frequency (?). Inversely related ? ? = c (the speed of light) Light visible to the naked eye exists as a tiny portion of the electromagnetic spectrum Max Planck Transfer of energy was not continuous Only came in certain values (quantized) ?E = h? h = Planck?s constant = 6.626 x 10-34 Js Packets of energy (quantum Albert Einstein Proposed that electromagnetic radiation was quantized and made up of a stream of particles Photons The dual nature of light ? = h/mv (deBroglie equation) Electrons as Waves Louis de Broglie (1924) Applied wave-particle theory to electrons electrons exhibit wave properties QUANTIZED WAVELENGTHS

Bob Jones PPT Notes -- Chapter 4b

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Chemistry
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Chemistry
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Atomic physics
Quantum chemistry
Chemical bonding
Periodic Table
electron configuration
Theoretical chemistry
Atomic orbital
Block
Aufbau principle
Quantum number
Technology

The Electron Structure of the Atom The quantum model emphasizes the wave nature of electrons. The Quantum Model Quantum numbers are solutions to the wave equations of electrons. Scientists use a set of 4 quantum numbers to determine an electron?s location around an atom. Quantum Numbers Electrons exist in principal energy levels that correspond to Bohr?s orbits: 1, 2, 3, 4, 5, ? Principal energy levels are divided into 4 types of sublevels: s, p, d, and f. Where are the Electrons? The sublevels contain orbitals. Each orbital can hold up to two electrons. Where are the Electrons? Identifies the principal energy level Correlates to Bohr?s orbits n = 1, 2, 3, 4, 5, 6, or 7 for the ground state e?. The total number of e? in a level is 2n2. Principal Quantum Number (n) Level Total # e? 1

Chemistry The central science Summary Chapter 6

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Chemistry
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Chemistry
Physics
Atomic physics
Quantum chemistry
Chemical bonding
Molecular physics
Theoretical chemistry
Atomic orbital
electron configuration
electron
Bohr model
Energy level
Technology

Hot Objects and the Quantization of Energy Heated solids emit radiation (blackbody radiation) The wavelength distribution depends on the temperature (i.e., ?red hot? objects are cooler than ?white hot? objects). In 1900 Max Planck solved the problem He investigated black body radiation. He proposed that energy can only be absorbed or released from atoms in ?chucks? of some minimum size . These amounts are called quanta. A quantum (meaning ?fixed amount?) is the smallest amount of energy that can be emitted or absorbed as electromagnetic radiation. The relationship between energy and frequency is: . The Photoelectric Effect and Photons The photoelectric effect provides evidence for the particle nature of light and for quantization.

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