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24 Cards in this Set
- Front
- Back
Definition: Ground state |
The lowest energy state |
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Written format for electron configuration |
Atomic symbol, then the list of orbitals from lowest to highest n, with a superscript for the number of electrons in that orbital. Ex: O 1s^2 2s^2 2p^4 |
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Definition: Noble gas notation
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Replaces the part of an atom's electron configuration that is the same as its previous noble gas with the symbol of that gas in brackets. Ex: Na's notation is [Ne] 3s^1 |
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Definition: Orbital diagram |
A diagram that shows an element's electron configuration and symbolizes the electrons as arrows in boxes representing orbitals
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The Pauli exclusion principle |
No two electrons in an atom can have the same four quantum numbers |
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How many electrons can occupy a single orbital? |
Two, as long as they have opposite spins. Half arrow up for up and half arrow down for down |
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Sublevels by least to greatest energy
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E(s orbital) < E(p orbital) < E(d orbital) < E(f orbital) |
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Definition: Aufbau principle |
The pattern of orbital filling based on starting with the orbitals with the least energy and moving gradually to those with greater energy |
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Definition: Hund's Rule |
When filling degenerate orbitals, electrons fill them singly first, with parallel spins, before doubling up. |
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Chart for filling electron configurations |
Exceptions: Chromium (4s^1, 3d^5) and Copper (4s^1, 3d^10) |
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In the periodic table, the row number is equal to which quantum number? |
The highest principal quantum number (n) of the atom |
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Definition: Valence electrons |
For main-group elements: Electrons that are in the outermost principal energy level For transition metals: Electrons in the outermost principal energy level as well as the outermost d sublevel |
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Definition: Core electrons |
Non-valence electrons, i.e. electrons that are in complete principal energy levels and complete d and f sublevels |
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Electron configurations for monoatomic ions |
For cations: Subtract electrons equal to the charge number from the atom's electron configuration.
For anions: Add electrons equal to the charge number to the atom's electron configuration. For main group use reverse order of filling. For transition metals always take from the highest n level first. |
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Definition: Isoelectronic |
Having the same electronic configuration |
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When atoms react they exchange electrons to become isoelectronic with _____ |
Their nearest noble gas |
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Definition: Periodic property |
A property of an atom that is predictable by its place in the periodic table |
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Three periodic properties to know |
Atomic size/radius, ionization energy, and electronegativity |
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Periodic trend of atomic size/radius
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Across a period size decreases, down a group size increases |
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Definition: Ionization energy |
The energy required to remove an electron from an atom in its gaseous state |
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Periodic trend of ionization energy |
Across a period energy increases (more negative), down a group energy decreases (less negative)
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Definition: Electronegativity |
The attraction an atom has for electrons in a covalent bond |
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Periodic trend of electronegativity |
Across a period increases, down a group decreases |
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Label blocks of the Periodic table |
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