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40 Cards in this Set

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