CH 101 Final Flash Cards
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209 Terms
nuclear theory
the theory stating that most of an atom’s mass and all of its positive charge are contained in a small
law of definite proportions
the law stating that all samples of a given compound have the same proportions of their constituent elements
law of multiple proportions
the law stating that when two elements form different compounds
atomic theory
the theory that matter is composed of atoms
Electromagnetic radiation
energy transmitted through space by oscillating electric and magnetic fields
Amplitude
the height of a wave from its center line to its crest
Wavelength
the distance between adjacent crests or troughs of a wave
Frequency and electromagnetic spectrum
frequency is the number of wave cycles that pass a point per second; the electromagnetic spectrum is the range of all electromagnetic radiation organized by wavelength or frequency
Gamma ray
the highest-energy
Ultraviolet (UV) radiation
electromagnetic radiation with wavelengths shorter than visible light but longer than gamma rays
Visible light
electromagnetic radiation detectable by the human eye
Infrared (IR) radiation
electromagnetic radiation with wavelengths longer than visible light
Microwave
electromagnetic radiation with longer wavelengths than infrared
Radio wave
the longest-wavelength
Interference
the combination of waves when they overlap
Constructive interference
when overlapping waves add together to produce a wave of greater amplitude
Destructive interference
when overlapping waves cancel each other
Diffraction
the bending or spreading of waves when they encounter an obstacle or pass through a slit
Photoelectric effect
the emission of electrons from a metal surface when exposed to light of sufficient energy
Binding energy
the minimum energy required to remove an electron from an atom or from a metal surface
Photon (quantum)
a packet of light energy; the fundamental particle of electromagnetic radiation
Emission spectrum
the set of wavelengths of light emitted by atoms or molecules as excited electrons return to lower energy states
Absorption spectrum
the set of wavelengths of light absorbed by atoms or molecules as electrons move to higher energy states
De Broglie relation
the equation stating that a particle’s wavelength equals Planck’s constant divided by its momentum
Complementary properties
properties that cannot be observed or measured simultaneously
Heisenberg’s uncertainty principle
the principle that it is impossible to know both the exact position and exact momentum of a particle simultaneously
Deterministic
describing a system in which present conditions completely determine future behavior
Indeterminacy
the inherent quantum-level randomness that prevents precise prediction of a particle’s future position
Orbital
a region of space around the nucleus where an electron is likely to be found
Wave function
a mathematical function describing the behavior and probability distribution of an electron in an atom
Quantum number
a set of numbers that specify the properties and location of an electron in an atom
Principal quantum number
the quantum number (n) that indicates the energy level and size of an orbital
Angular momentum quantum number
the quantum number (l) that defines the shape of an orbital
Magnetic quantum number
the quantum number (mₗ) that specifies the orientation of an orbital in space
Spin quantum number
the quantum number (mₛ) that describes the intrinsic spin of an electron
Electron spin
the intrinsic angular momentum of an electron
Principal level (shell)
the group of orbitals with the same principal quantum number n
Sublevel (subshell)
the set of orbitals within a principal level that share the same angular momentum quantum number l
Probability density
the value of the wave function squared
Radial distribution function
a plot showing the probability of finding an electron at various distances from the nucleus
Node
a point or region in an orbital where the probability of finding an electron is zero
Phase
the sign (positive or negative) of a wave function
Pauli exclusion principle
the principle stating that no two electrons in an atom can have the same set of four quantum numbers
degenerate
describing orbitals within the same subshell that have the same energy
Coulomb’s law
the law describing the attraction between opposite charges and repulsion between like charges
shielding
the reduction of the full nuclear charge felt by an electron due to repulsion from other electrons
effective nuclear charge
the net positive charge experienced by an electron after accounting for shielding
penetration
the phenomenon in which an electron spends time closer to the nucleus
aufbau principle
the rule stating that electrons fill orbitals in order of increasing energy
Hund’s rule
the rule stating that electrons fill degenerate orbitals singly with parallel spins before pairing
ionization energy
the energy required to remove an electron from an atom or ion in the gas phase
electron affinity
the energy change associated with adding an electron to an atom or ion in the gas phase