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26 Cards in this Set
- Front
- Back
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Equation to show Frequency (v) and Wavelength (lamda) relationship.
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Frequency - v = speed of light - c/wavelength - lamda
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Speed of Light - c
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3.00 x 10^8 m/s
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What equation did Planck develop?
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Energy - E = (Planck's Constant - h)(Frequency - v)
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Planck's Constant?
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6.626 x 10^-34 Js
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What's the photoelectric effect?
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Its when electrons are ejected from the metal's surface after being exposed to certain frequencies of light. More electrons being ejected = more intense light or pure light.
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How are line spectras produced?
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Electrons are returning to ground state, from excited state, releasing energy in the form of light. Electrons do not give off a full rainbow, only the sun can do that (white light)
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What idea did the photoelectric effect and line spectra help support?
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Shows that electrons only absorb and emit certain energies and therefore only exist in certain orbits around the nucleus.
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Sublevels?
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S (1 orbital, 2 electrons) P (3 orbitals, 6 electrons) D (5 orbitals, 10 electrons) F (7 orbitals, 14 electrons)
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Energy Levels (n)?
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7 of them. Bigger - more space. Broken up into sublevels.
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Heisenberg Uncertainty Model?
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Specific velocity and location of electrons cannot both be known simultaneously. We can know the general location of where it was, but we can't know both.
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Photon?
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Bundle of Energy
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Aufbau Principle?
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Electrons are always added to lowest energy levels first.
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Hund's Rule?
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Electrons fill orbits of equal energy to have as many unpaired electrons as possible (spread out)
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Pauli Exclusion Principle?
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Each orbital can hold only 2 electrons with opposite spins.
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Order of Orbitals?
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1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p...
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Atomic Radius trends?
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Number of energy levels - more levels - bigger
Same energy level - more electrons - smaller. This is due to the stronger nuclear force making the atom smaller. |
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Ionic Radius trends?
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Gained an electron means it becomes larger.
Loses an electrons means the atom becomes smaller. |
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Ionization Energy Trends?
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- The energy needed to remove 1 valence electron.
- Increases going right across a period. - Decreases going down a group due to shielding effect |
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Shielding Effect?
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Valence electrons are further away from the nucleus and blocked by inner layers of electrons. Therefore they're easier to remove due to less pull.
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Electronegativity Trends?
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- Ability of an atom to attract an electron.
- Increases going right due to increasing nuclear charge. - Decreases going down due to increased shielding. The nucleus can't pull electrons in. |
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Where are metals found?
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Left of staircase.
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Where are nonmetals found?
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Right of staircase.
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Noble Gases (Group 18)
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Halogens (Group 17)
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Alkali Metals (Group 1)
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Alkaline Earth Metals (Group 2)
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