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Chemistry Chapter 7
terms
Term | Definition |
---|---|
Wave | a periodic back and forth motion that transmits energy |
Crests | the high points of a series of waves |
Troughs | the low points of a series of waves |
Wavelength | the distance between any two corresponding points on successive waves |
Amplitude | a measure of the waves’ strength |
Frequency | the number of complete waves that pass by a point in a given time |
hertz | SI unit of frequency; one wave per second |
Speed | the rate at which the wave travels |
Particle theory of light | the idea that light can be pictured as streams of tiny particles emitted by light sources |
Wave theory of light | states that light consists of a series of waves rather than individual particles |
Electromagnetic wave | an electric field and a magnetic field vibrating at right angles to each other |
Electromagnetic spectrum | an arrangement of all forms of electromagnetic radiation in order of frequency and wavelength |
Wave particle duality | two sided nature of light |
Quantum theory of light | says that light consists of tiny bundles of energy |
Photons | tiny bundles of energy |
Light | electromagnetic waves traveling as photons |
spectrometer | separates colors |
Spectroscope | a prism separates light into its component wavelengths |
Line spectrum | a spectrum containing only certain colors |
Continuous spectrum | a spectrum with the complete array of colors |
Energy levels | specific orbits in which the electron moves about the nucleus |
Ground state | the lowest energy state of an electron |
Excited states | all states higher than the ground state |
Matter waves | particles that, when in motion, have properties of waves |
Wave mechanical model | combined the Bohr model with Broglie’s hypothesis |
Standing wave | a 3D matter wave with an integral number of wavelengths in an orbit |
Uncertainty principle | states that it is impossible to simultaneously determine the momentum and the position of an electron with precision |
Orbitals | regions of space in which there is a high probability of finding an electron |
Orbit | an electrons definite path in space |
Electron cloud model | Born's interpretation of the wave |
Probability contour | drawn around where 90% of the electrons are most likely to be found |
Electron configuration | the complete arrangement of electrons in an atom |
Quantum numbers | four numbers that describe the electron |
Principle quantum number | describes the electron shell of the electron |
Electron shell | main energy level of the electron |
subshells | make up each electron shell |
Subshell quantum number | indicates the shape or type of subshell |
Magnetic quantum number | describes the orientation of the orbital within the subshell |
Spin quantum number | describes the spin of the electron |
Pauli exclusion principle | states that no two electrons in the same atom can have the same set of four quantum numbers |
Aufbau principle | electrons occupy the lowest energy orbital available |
Hund’s rule | one electron will fill each orbital before pairing begins |
Valence electrons | the outermost electrons |
Lewis symbol | uses dots written around the element’s symbol to represent the valence electrons |
Stimulated emission | if an atom is struck by a photon of the correct frequency during its excited state, the electron instantly emits two identical photons |
Laser | narrow beams of high intensity light |