Electronic Structure Of Atoms Test Questions – Flashcards
Unlock all answers in this set
Unlock answersquestion
| electronic structure |
answer
| the arrangement of electrons in an atom or molecule |
question
| electromagnetic radiation |
answer
| a form of energy that has awave characteristics and that propagates through a vacuum at the characteristic speed of 3.00*10^8 m/s |
question
| wavelength |
answer
| the distance between identical points on successive waves |
question
| frequency |
answer
| the number of times per second that one complete wavelength passes a given point |
question
| quatum |
answer
| the smallest increment of radiant energy that may be absorbed or emitted the magnitude of radiant energy is hv |
question
| Planck's constant |
answer
| the constant that relates the energy and frequency of a photon E = hv; equals 6.626*10^-34 J-s |
question
| photoelectric effect |
answer
| the emissions of electrons from a metal surface induced by light |
question
| spectrum |
answer
| the distribution among various wavelengths of the radiant energy emitted or absorbed by an object |
question
| continuous spectrum |
answer
| a spectrum that contains radiation distributed over all wavelengths |
question
| line spectrum |
answer
| a spectrum that contains radiation at only certain specific wavelengths |
question
| ground state |
answer
| the lowest energy, or most stable, state |
question
| excited states |
answer
| a higher energy state than the ground state |
question
| matter waves |
answer
| the term used to describe the wave characteristics of a moving particle |
question
| momentum |
answer
| the product of the mass and velocity of an object |
question
| uncertainty principle |
answer
| a principle stating there is an inherent uncertainty in the precision with which we can simultaneously specify the position and momentum of a particle this uncertainty is significant only for particles of extremely small mass, such as electrons |
question
| wave functions |
answer
| a mathematical description of an allowed energy state (an orbital) |
question
| probability density |
answer
| a value the represents the probability that an electron will be found at a given point in space |
question
| electron density |
answer
| the probability of finding tan electron at any particular point in an atom; this probability is equal to the square of the wave function |
question
| orbitals |
answer
| an allowed energy state of an electron in the quantum mechanical model of the atom; the term orbital is also used to describe the spatial distribution of the electron; an orbital is defind the the values of three quantum numbers: n, l, and ml |
question
| electron shell |
answer
| a collection of orbitals that have the same value of n |
question
| subshell |
answer
| one or more orbitals with the same set of quantum numbers n and l |
question
| radial probability function |
answer
| the probability that the electron will be found at a certain distance from the nucleus |
question
| nodes |
answer
| points in an atom at which the electron density is zero; for example the node in a 2s orbital is spherical surface |
question
| degenerate |
answer
| a situation in which two or more orbitals have the same energy |
question
| electron spin |
answer
| a property of the electron that makes it behave as though it were a tiny magnet; the electron behaves as if it were spinning on its axis; electron spin is quantized |
question
| spin magnetic quantum number |
answer
| a quantum number associated with the electron spin |
question
| Pauli exclusion principle |
answer
| a rule stating that no two electrons in an atom may have the same four quantum numbers; as a reflection of this principle, there can be no more than two electrons in any one atomic orbital |
question
| electron configuration |
answer
| the arrangement of electrons in the orbitals of an atom or molecule |
question
| Hund's rule |
answer
| a rule stating that electrons occupy degenerate orbitals in such a way as to maximize the number of electrons with the same spin; in other words, each orbital has one electron placed in it before pairing of electrons in orbitals occurs |
question
| valence electrons |
answer
| the outermost electrons of an atom; those that occupy orbitals not occupied in the nearest noble-gas element of lower atomic number; the valence electrons are the ones the atom uses in bonding |
question
| core electrons |
answer
| the electrons that are not in the outermost shell of an atom |
question
| representative elements |
answer
| an element from within the s and p blocks of the periodic table |
question
| main-group elements |
answer
| elements in the s and p blocks of the periodic table |
question
| transition elements |
answer
| elements in which the d orbitals are partially occupied |
question
| lanthanide (rare earth) elements |
answer
| element in which the 4f subshell is only partially occupied |
question
| actinide elements |
answer
| element in which the 5f orbitals are only partially occupied |
question
| f-block metals |
answer
| lanthanide and actinide elements in which the 4f and 5f orbitals are partially occupied |
