5.1 Light and Quantized Energy - Weebly



Ch 5 Electrons in Atoms5.1 Light and Quantized EnergyReview Vocabulary________________ the rays and particles —alpha particles, beta particles, and gamma rays—that are emitted by radioactive material217805098755quantumPlanck's constantphotoelectric effectphotonatomic emission spectrum4000020000quantumPlanck's constantphotoelectric effectphotonatomic emission spectrumNew Vocabularyelectromagnetic radiationwavelengthfrequencyamplitudeelectromagnetic spectrumMain Idea Light, a form of electronic radiation, has characteristics of both a____________ and a _______________5.1 THE ATOM AND UNANSWERED QUESTIONSRecall that in Rutherford's model, the atom’s mass is concentrated in the nucleus and electrons move around it.Atom is mostly ____________ spaceThe model does not explain: _________the electrons were arranged around the nucleus._________negatively charged electrons aren’t pulled into the positively charged nucleus.the_______________ properties of the elements a better description of the __________________ was neededIn the early 1900s, scientists observed certain elements _____________________________ when heated in a flame.Analysis of the emitted light revealed that an element’s chemical ________________ is related to the _______________________ of the __________________in its atoms.5.1 THE WAVE NATURE OF LIGHTVisible light is a type of _______________________________, a form of energy that exhibits wave-like behavior as it travels through space.All waves can be described by ____________characteristics.The ___________________ is the wave’s height from the origin to a crest.The ______________________ (λ) is the shortest distance between equivalent points on a continuous wave.The ___________________(f) is the number of waves that pass a given point per second.Frequency is measured in units of Hertz (Hz).1 Hz = ___________33274777112000335712-381000Wavelength and Frequency are __________________related, so as one goes _____ the other goes ____________.The product of the wavelength and the frequency of any electromagnetic wave is he speed of light (3.00 108 m/s).The wave speed equation is _____________.C = ___________________λ = ___________________f = ___________________Different __________________ of light are different _______________ of light.This also means that each color has a certain wavelength.The whole range of frequencies and wavelengths is called the ________________________.Sunlight contains a ________________________ of wavelengths and frequencies.A_________________ separates sunlight into a continuous spectrum of colors.498792569215Long Wavelength=Low Frequency=Low ENERGY00Long Wavelength=Low Frequency=Low ENERGYThe electromagnetic spectrum includes _________ forms of electromagnetic radiation.3072130654050014605010985500485107099695Short Wavelength=High Frequency=High ENERGY0Short Wavelength=High Frequency=High ENERGYExample CalculationCalculate the wavelength of yellow light emitted by a sodium light if the frequency is 5.10 x 1014 Hz. 5.1 the particle nature of lightThe wave model of light cannot explain all of light’s characteristics.It does not explain all of light’s interactions with matter.Why do heated objects emit only certain frequencies of light?Why do some metals emit electrons when colored light of a specific frequency shines on them?In 1900, the German physicist ____________________ began searching for an explanation as he studied the light emitted from heated objects and made the following conclusions.Matter can gain or lose _____________ only in small, specific amounts called _______________.A ____________ is the ________________ amount of energy that can be gained or lost by an atom.Planck’s constant has a value of ________________________.The ____________________________ is when electrons are emitted from a metal’s surface when light of a certain frequency shines on it.The wave model of light could not explain this either.1008380127000_____________________________ proposed in 1905 that light has a _____________________. A beam of light has wavelike and particlelike properties.A ______________ is a ________________of electromagnetic radiation with ______________ that carries a __________________ of energy.Ephoton = hfEphoton represents energy.h is Planck's constant.f represents frequency. Atomic Spectra____________light is made up of_________ the colors of the ________________spectrum.Passing it through a prism _________________ it.Each________________ gives off its own characteristic colors.Can be used to __________________ the atom.This is how we know what ______________are made of.2099462196570These are called the _________________________Unique to each element, like___________________!Very useful for_________________ elements00These are called the _________________________Unique to each element, like___________________!Very useful for_________________ elements313690476250033528040957500334365419100025279357683500The atomic emission spectrum of an element is the __________________________ of the electromagnetic waves emitted by the atoms of the element.Each element’s atomic emission spectrum is unique.Light in a neon sign is produced when electricity is passed through a tube filled with neon gas and excites the neon atoms.The excited atoms ___________________ to _________________________.The Math in Chapter 5There are 2 equations: c = E = h________________!ExamplesWhat is the wavelength of blue light with a frequency of 8.3 x 1015 hz?What is the frequency of red light with a wavelength of 4.2 x 10-5 m?What is the energy of a photon of each of the above?5.2 Quantum Theory and the AtomReview Vocabularyatom: the smallest particle of an element that retains all the properties of that element, is composed of electrons, protons, and neutrons2581605140335atomic orbitalprincipal quantum numberprincipal energy levelenergy sublevel4000020000atomic orbitalprincipal quantum numberprincipal energy levelenergy sublevelNew Vocabularyground stateMain Idea - quantum numberde Broglie equationHeisenberg uncertainty principlequantum mechanical model of the atomBohr’s model of the atom (Planetary Model)Why do elements’ atomic emission spectra show only certain frequencies?In 1913 ________________, a Danish physicist, was working in Rutherford’s lab and proposed a _______________________ for the hydrogen atom that seemed to answer this question.Bohr’s model correctly predicted the frequency lines in hydrogen’s atomic emission spectrum.The lowest allowable energy state of an atom is called its _______________________.When an atom gains energy, it is in an _______________________.Bohr suggested that an electron moves around the nucleus only in certain allowed circular orbits.15709909652000BUT, Why don’t the electrons fall into the nucleus?Move like planets around the sun.In specific concentric circular paths, or orbits, at different levels.A ____________ (amount) of fixed energy separates one level from another.Electrons can _______________from one level to anotherEach____________ was given a number, called the ___________________.An _____________________ of an electron is analogous to the rungs of a ladderThe electron_________________ exist between energy levels, just like you can’t stand between rungs on a ladderA____________________ of energy is the amount of energy required to move an electron from one energy level to another394906516129000-185420158115003662680-56578500619125-15748000Hydrogen’s single electron is in the n = 1 orbit in the ground state.When ___________________________, the electron moves to a higher energy state such as the n = 2 orbit or n = 5 orbit._________________________________ can move the electron up to different energy levels. The electron is now said to be ___________________.As the electron falls back to the ground state, it gives the energy back as _____________.Bohr’s model explained the hydrogen’s spectral lines, but _____________ to explain any other element’s lines.The behavior of electrons is still not fully understood, but it is known they do not move around the nucleus in circular orbits.The Quantum Mechanical Model_________________ __________________explains how very small particles behaveQuantum mechanics is an explanation for_____________________ particles and atoms as waves _____________________________ describes the motions of bodies much larger than atomsIn 1924 _______________________, a French graduate student in physics, proposed an idea that eventually accounted for the fixed energy levels of Bohr’s model._____________ is still _________________ in his model. It comes in chunks.Louis de Broglie (1892–1987) hypothesized that particles, including electrons, could also have wavelike behaviors.The de Broglie equation predicts that all moving particles have wave characteristics.45354223825 represents wavelengthsh is Planck's constant.m represents mass of the particle. f represents frequency.The figure illustrates that electrons orbit the nucleus only in whole-number wavelengths.10236203683000___________________________, a German theoretical physicist and a contemporary of de Broglie proposed an idea that had profound implications on atomic theory.Heisenberg showed it is impossible to take any measurement of an object without disturbing it.It is more obvious with the very small objectsTo measure where a electron is, we use light.But the light energy moves the electronAnd hitting the electron changes the frequency of the light.The ___________________________________________states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.In 1926, Austrian physicist _____________________________ furthered the wave-particle duality theory proposed by de Broglie.Schr?dinger treated electrons as waves in a model called the _________________________________________________ of the atom.Schr?dinger’s equation applied equally well to elements other than hydrogen.The quantum mechanical model is a mathematical solutionIt is not like anything you can see (like plum pudding!)The atom is found inside a blurry “electron ___________”Schr?dinger’s wave function predicts a three-dimensional region around the nucleus called the _____________________.17938752603500Atomic orbitalsThe Quantum Mechanical Model:Has energy levels for electrons.Orbits are not circular.It can only tell us the probability of finding an electron a certain distance from the nucleus.Principal quantum number (n) indicates the relative size and energy of atomic orbitals.n specifies the atom’s major energy levels, called the principal energy levels. ______________________ are contained within the principal energy levels like theater seats arranged in sections: letters s, p, d, and f _________________ number of electrons that can fit in an energy level is ________.179133515748000Each energy _________________ relates to orbitals of ________________________.8915409779000 606425508000Orbital Shapess - sphericalp - dumbbelld – cloverleaff - just wild5.3 Electron ConfigurationReview Vocablularyelectron: a negatively charged, fast-moving particle with an extremely small mass that is found in all forms of matter and moves through the empty space surrounding an atom's nucleusNew Vocabularyelectron configurationaufbau principlePauli exclusion principleHund's rulevalence electronselectron-dot structureMain Idea - A set of __________________ determines the arrangement in an atom.5.3 ground state electron configurationThe arrangement of electrons in the atom is called the ____________________________________.The _________________________ states that each electron occupies the lowest energy orbital available.2522982775004012431038900The ________________________________________ states that a maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins.__________________________ states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same energy level orbitals.When electrons occupy orbitals of _________energy, they don’t __________ up until they have to.20628863886007385051174750019616434239200_______________________________ uses noble gas symbols in brackets to shorten inner electron configurations of other elements.332676513652500Orbital DiagramsShows the ___________ associated with a particular electronShows the _________________ of electrons in an atom36131508128000Explains bonding and various properties Can be called an ________________________ – Aufbau is German for “building up”Let’s write the orbital diagram for _______________ We need to account for all ____ electrons in phosphorusThe first two electrons go into the ____ orbitalNotice the _______________direction of the spinsonly 13 more to go...The next electrons go into the ____ orbitalonly 11 more...The next electrons go into the ____ orbitalonly 5 more...The next electrons go into the ____ orbitalonly 3 more...The last three electrons go into the ____ orbitals.They each go into separate shapes (Hund’s)3 unpaired electronsElectron configuration = ______________________ Example Electron configurations Calcium ___________________ Chromium ____________________144145139700035147255364500Orbitals fill in an order ______________energy to higher energy.Adding electrons can change the energy of the orbital. ________orbitals are the most__________.However, ________________ orbitals have a lower energy, and are next bestMakes them more stable.Changes the filling orderThe electron configurations (for chromium, copper, and several other elements) reflect the increased stability of half-filled and filled sets of s and d orbitals.____________________________ are defined as electrons in the atom’s outermost orbitals—those associated with the atom’s highest principal energy level._____________________________ consists of the element’s symbol representing the nucleus, surrounded by dots representing the element’s valence electrons.233354914935200 ................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download