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22 Cards in this Set
- Front
- Back
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Wavelength
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Distance between identical adjacent points on a wave; lambda.
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Electromagnetic radiation
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All visible and invisible wavelengths; electromagnetic spectrum.
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Energy of electromagnetic radiation
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E = 6.626e-34 J(s) X 3e8 (m/s) / lambda
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Energy of radiation
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Energy of radiation increases as wavelength decreases.
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Electron's energy
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The closer the electron to nucleus, the lower its energy; more stable atom.
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Bohr Theoryof Atomic Structure
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Electrons can jump from one energy level to another.
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Shell
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Maximum Electron Capacity = 2n^2
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Valence Shell
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Outermost occupied shell.
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Valence Shell; Representative Elements
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Group Number = Number of valence shell electrons
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Ground State
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Arrangement of electrons with lowest total energy.
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Excited State
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1 or more electrons are located in high energy shells with room in lower energy shells.
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Relaxation
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When atom returns from excited to ground state, energy is released.
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Subshell
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n = number of subshells; n = 1 has 1 subshell.
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s Subshell
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2
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p Subshell
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6
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d Subshell
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10
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f Subshell
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14
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Octet Rule
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Elements react to form compounds to put 8 electrons in valence shell; valence shell configuration same as noble gas; most stable.
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Metals
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Tend to lose electrons.
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Nonmetals
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Tend to gain electrons.
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Decreasing Atom Size
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Atom size decreases as number of electrons increase, which increases the number of protons - a positive charge that attracts all electrons more tightly.
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When electrons are farther from nucleus...
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As n increases, electron gets farther from nucleus; increasing electron's energy.
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