Periodic Trends
These periodic trends increase up and to the right of the periodic table
Electronegativity, Electron Affinity, Ionization Energy
A bond between a metal and a non-metal
Ionic Bond
NO2- & NO3-
Nitrite & Nitrate
Maximum number of electrons in a subshell
4L+2
Name of the first column in the periodic table
The energy required to remove an electron from a gaseous species
Ionization Energy
Both electrons shared in this bond originate from one atom
Coordinate Covalent Bond
H2PO4-
Dihydrogen Phosphate
The ability to draw the same arrangement of atoms in multiple ways based on their electron locations
Resonance
A difference in polarity greater than 0.4
Polar bond
The number of valence electrons and number of electron shells determines
Atomic Radius
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, & Iodine
Naturally Occurring Diatomic Elements
Monoatomic anions have this suffix added to the end of their names
-ide
EX. H- is hydride
How many valence electrons are in HCN
10
This electrostatic attraction is the result of negatively charged valence electrons and the positively charged nucleus
A molecule that has such a separation of positive and negative charges
Dipole Moment
HCO3-
HSO4-
H2PO4-
Hydrogen Carbonate or Bicarbonate
Hydrogen Sulfate or Bisulfate
Dihydrogen Phosphate
The electron configuration of Cr
Expected: Cr = [Ar] 4s2 3d4
Actual: Cr = [Ar] 4s1 3d5
Why are the electron configurations for some transition metals different than their expected configurations
The atom is more stable with a half-full d-orbital and half-full s-orbital than a full s-orbital and the d-orbital only having 4 electrons
The highest energy orbital of elements with valence electrons in the n = 3 shell
d-orbital
C2H2 and HCN both contain triple bonds, but the length of these are not equal, why?
Nitrogen is more electronegative than carbon
These compounds form large arrays of ions in crystalline solids
Ionic compounds
The number of resonance structures for sulfur dioxide
3