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40 Cards in this Set
- Front
- Back
Energy Level
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n = 1,2,3,4...
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Sublevel
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Inside energy level
nS, nP, nD, nF |
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Orbital
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S - 1 orbitals
P - 3 orbitals D - 5 orbitals F - 7 orbitals Each orbital can only hold 2 electrons |
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Electrons per Sublevel
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2 electrons per orbital
S - 2 P - 6 D - 10 F - 14 |
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Electrons per Energy Level
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2n^2
Energy Level 1 - 2 2 - 8 3 - 18 4 - 32 |
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What does the Aufbau Principle state?
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Electrons will fill the lowest energy positions in an atom first
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What does the diagonal rule do?
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Arranges sublevels in order of energy levels from lowest to highest
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Lewis Dot Model
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Shows only valence electrons
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Orbital diagram:
Hund's rule |
Each orbital in a sublevel must have 1 electron before any orbital has 2 electrons
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Orbital diagram:
Pauli Exclusion Principle |
No 2 electrons in an atom have the same 4 quantum numbers
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He...
Made the 1st attempt to organize the known elements |
Lavoisier
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He...
Tried to organize approx. 30 known elements into trials |
Dobereiner
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He...
Arrange known elements in order of increasing atomic mass - Notices that chemical properties repeat w/ every 8th element - Organized in groups of 7 |
Newlands
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What is the Law of Octaves?
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Developed by Newlands
The chemical properties repeat every 8th element |
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He...
Arranges the known elements in order of increasing atomic mass and places the elements w/ similar chemical properties in the same column - Blanks spaces were left and the existence of undiscovered elements was correctly predicted |
Dmitri Mendeleev
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He...
Rearranged the periodic table in order of increasing atomic number |
Henry Moseley
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What is the Modern Period Law?
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The properties of elements is a function of their atomic numbers
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What are the 3 ways atoms "want" to be stable?
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1.) Have a full valence shell (8 outer shell electrons)
2.) Full sublevels: s^2, p^6, d^10, f^14 3.) Half-filled sublevels: s^1, p^3, d^5, f^7 |
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How are abbreviated electron configurations determined
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Based on the noble gas at the end of the preceding period
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What is a periodic trend?
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A repeating pattern that can be found on the periodic table
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What is atomic radius?
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The radius of an atom
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What is ionization?
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The energy needed to remove the most loosely held electrons
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Where is atomic radius the largest? The smallest?
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Largest - Fr: bottom, left
Smallest - He: top, right |
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Where is ionization energy the highest? The lowest?
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Highest - He: top, right
Lowest - Fr: bottom, left |
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Why does atomic radius decrease across a period?
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Because increasing nuclear charge has a greater attraction for electrons being added to the same energy level
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Why does atomic radius increase as it moves down a group?
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- With each period an additional energy level is added
- Electron shielding: Inner electrons block the force of attraction b/w the nucleus and outer electrons - Allows electrons to momentarily "drift away" |
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What is electronegativity?
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The tendency of an atom to attract electrons in a chemical bond
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How does electronegativity increase?
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It increases across the periodic table and up the periodic table
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What is the most chemically active nonmetal?
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Fluorine
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What are the most chemically active metals?
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Cesium and Francium
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What is an ionic bond?
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- Electrostatic force of attraction
- Solids @ room temp. - High melting/boiling point - Solid, well-defined crystal - Most are soluble in H2O - Electrolytes in solution or as a liquid |
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What is a covalent bond?
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- Shared electrons
- Lower melting/boiling points - Liquids/gases @ room temp. - Some solids --> Sugar - Some are soluble in H2O, most are not - Not electrolytes |
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What are van der waals forces?
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- Weak forces of attracting b/w molecules
- Caused by the protons in 1 molecule being attracted to the electrons in a neighboring molecule |
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What are the types of van der waals forces?
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1.) Dipole-dipole (strongest)
- Hydrogen bonds - a special type of dipole-dipole 2.) Dipole-induced dipole 3.) London dispersion forces (weakest) |
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What is a dipole?
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A polar molecule
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Dipole-dipole occurs between what?
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2 permanent dipoles
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Hydrogen bonding is...
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- A special type of dipole-dipole
- Strongest intermolecular force - Formed b/w molecules in which H is directly connected with N, O, or F |
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Covalent bonds are either...
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Polar or nonpolar
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What are nonpolar covalent bonds?
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Bond b/w 2 atoms w/ very close electronegativities
- electrons are shared equally |
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What are polar covalent bonds?
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Bonds b/w 2 atoms w/ a larger difference in electronegativity
- electrons are shared unequally |