Flashcards
Exam #3
Flashcards do conjunto (59)
- 1Amplitudeheight of the wave, measured from the centerline between peak and trough
- 2Angular-Momentum Quantum Numberdefines the three-dimensional shape of the orbital
If n=1, then l=0 If n=2, then l=0 or 1 If n=3, then l=0, 1, or 2… and so on - 3Principal Quantum Number is Represented by what Character of the Alphabetn
- 4Angular-Momentum Quantum Number is Represented by what Character of the Alphabetl
- 5Aufbau Principleguides the filling order of orbitals
(in general, each successive electron added to an atom occupies the lowest-energy orbital available) - 6Balmer–Rydberg Equationm and n represent integers with n> m.
- 7Balmer–Rydberg Equation: If m= ? then what? (m=1?, m=2?, m=3?)If m=1, then the ultraviolet series of lines results.
If m=2, then Balmer’s series of visible lines results.
If m=3, an infrared series is described, and so forth for still larger values of m. - 8d-block elementmiddle of the table result from the filling of d orbitals
- 9de Broglie equationallows calculation of a “wavelength” of an electron or of any other particle or object of mass m moving at velocity v:
λ=h/mv - 10degenerateOrbitals that have the same energy level are degenerate
- 11Rules of the Aufbau Principle:1. Lower-energy orbitals fill before higher-energy orbitals.
2. An orbital can hold only two electrons, which must have opposite spins.
3. If two or more degenerate orbitals are available, one electron goes into each until all are half-full - 12Hund's RuleIf two or more orbitals with the same energy are available, one electron goes in each until all are half full. The value of the spin quantum number of electrons in the half-filled orbitals will be the same.
- 13effective nuclear charge ZeffThe nuclear charge actually felt by an electron and is often substantially lower than the actual nuclear charge Z.
Zeff = Zactual− Electron shielding - 14Electromagnetic SpectrumThe spectrum consists of a continuous range of wavelengths and frequencies, from radio waves at the low-frequency end to gamma rays at the high-frequency end.
Electromagnetic energy is characterized by a frequency, a wavelength, and an amplitude. - 15Radiant EnergyAlthough they appear quite different to our senses, visible light, infrared radiation, microwaves, radio waves, X rays, and so on are all different forms of electromagnetic radiation
- 16electron configurationKnowing the relative energies of the various orbitals, we can predict for each element which orbitals are occupied by electrons—the element’s electron configuration
- 17f-block elementslanthanide/actinide f-block elements detached at the bottom of the table result from the filling of f orbitals.
- 18p-block elementsthe group 3A–8A elements on the right side of the table are the p-block elements because they result from the filling of p orbitals
- 19s-block elementsThe group 1A and group 2A elements on the left side of the table are called the s-block elements because they result from the filling of an s orbital
- 20Difference between: d-block f-block s-block p-block
- 21frequency (ν)a wave is simply the number of wave peaks that pass by a given point per unit time, usually expressed in units of reciprocal seconds, or hertz (Hz)
- 22wavelength (λ)the wave is the distance from one wave peak to the next
- 23Difference between.... Amplitude Wavelength Frequency
- 24How do you calculate speed?
- 25ground-state electron configurationlowest-energy configuration is called the ground-state electron configuration of the atom
- 26Heisenberg uncertainty principleIn 1927 by Werner Heisenberg (1901–1976) that it is impossible to know precisely where an electron is and what path it follows
Heisenberg uncertainty principle.
(Δx)(Δmv) ≥ h/4π - 27hertz (Hz)units of reciprocal seconds
- 28line spectrum(White Light) When passed first through a narrow slit and then through a prism, the light emitted by an excited atom is found to consist of only a few wavelengths rather than a full rainbow of colors, giving a series of discrete lines on an otherwise dark background
- 29Example of Line SpectrumIf hydrogen atoms are electrically excited in a discharge tube, they give off a pinkish light made of several different colors
- 30magnetic quantum number (ml)defines the spatial orientation of the orbital with respect to a standard set of coordinate axes.
For an orbital whose angular-momentum quantum number is l, the magnetic quantum number ml can have any integral value from −l to +l. - 31nodea surface of zero electron probability separating regions of nonzero probability
- 32orbitalor wave functions
a solution to the Schrödinger wave equation, describing a region of space where an electron is likely to be found - 33Pauli exclusion principleNo two electrons in an atom can have the same four quantum numbers.
- 34phasea state of matter
- 35photonthe smallest possible amount of radiant energy; a quantum
- 36photoelectric effectthe ejection of electrons from metal on exposure to radiant energy
- 37Planck’s postulatethe energy of one quantum is related to the frequency of an electromagnetic wave
Planck’s postulate E = hν = hc/λ - 38quantumthe smallest possible amount of radiant energy
- 39quantizedmeaning that both matter and electromagnetic energy occur only in discrete amounts.
- 40quantum mechanical modela model of atomic structure that concentrates on an electron’s wavelike properties
The fundamental idea behind the model is that it’s best to abandon the notion of an electron as a small particle moving around the nucleus in a defined path and to concentrate instead on the electron’s wavelike properties. - 41quantum numberis a positive integer (n=1, 2, 3, 4,…) on which the size and energy level of the orbital primarily depends.
For hydrogen and other one-electron atoms, such as He+, the energy of an orbital depends only on n.
For atoms with more than one electron, the energy level of an orbital depends both on n and on the l quantum number. - 42Rutherford’s nuclear modelan atom must consist mostly of empty space, having a dense, positively charged nucleus at its center
- 43shella grouping of orbitals according to the principal quantum number
- 44spin quantum numberElectrons behave in some ways as if they were tiny charged spheres spinning around an axis. This spin (blue arrow) gives rise to a tiny magnetic field (green arrow) and to a fourth quantum number, ms, which can have a value of either +1/2 or −1/2.
- 45subshella grouping of orbitals by angular-momentum quantum number
- 46valence shellthe outermost electron shell
all the elements in a given group of the periodic table have similar valence-shell electron configurations - 47wave functionor orbitals
a solution to the Schrödinger wave equation - 48Born–Haber cyclea pictorial way of viewing the energy changes in the various steps during formation of an ionic solid from its elements
- 49core electroninner-shell electrons
- 50Coulomb’s lawThe force resulting from the interaction of two electric charges is equal to a constant k times the magnitude of the charges divided by the square of the distance between them.
- 51electron affinity (Eea)the energy change that occurs when an electron is added to an isolated atom in the gaseous state
- 52ground-state electron configurationthe lowest-energy electron configuration of an atom
- 53ionic bondoccurs when one atom transfers an electron to another, creating an electrostatic attraction between positively charged cations and negatively charged anions
A familiar example of an ionic compound is table salt, NaCl, consisting of Na+ and Cl− ions - 54ionic solida solid whose constituent particles are ions ordered into a regular three– dimensional arrangement held together by ionic bonds
- 55ionization energy (Ei)the amount of energy necessary to remove the outermost electron from an isolated neutral atom in the gaseous state
- 56isoelectronicAtoms or ions with same electron configuration
main group ions are isoelectronic to noble gases - 57lattice energy (U)the sum of the electrostatic interactions between ions in a solid that must be overcome to break a crystal into individual ions
amount of energy that must be added to break up an ionic solid into its individual gaseous ions, so it has a positive value - 58octet ruleMain-group elements tend to undergo reactions that leave them with eight outer-shell electrons. That is, main-group elements react so that they attain a noble-gas electron configuration with filled s and p sublevels in their valence electron shell.
- 59shieldedValence electrons are strongly shielded by inner-shell (core) electrons. They are less strongly shielded by other electrons in the same shell and the magnitude of shielding follows the order: s>p>d>f.
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- FlashCards sobre Exam #3, criado por Emma/Jace Wilson em 02-06-2019.
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