General Chemistry Stuff
Sulfuric Acid Charge
-2
2 H2 + O2 -> 2 H2O If the reaction above releases 483.6kJ, then the standard enthalpy of formation of H2O is
-241.8kJ/mole
Phosphoric Acid charge
-3
Value of l for s orbital
0
Determine the oxidation number (oxidation state) for the indicated element in each of the following compounds: Br in HBrO
+1
Determine the oxidation number (oxidation state) for the indicated element in each of the following compounds: C in COCl2
+4
Determine the oxidation number (oxidation state) for the indicated element in each of the following compounds: S in SO2
+4
Determine the oxidation number (oxidation state) for the indicated element in each of the following compounds: Mn in KMnO4
+7
Nitric Acid Charge
-1
Carbonic Acid Charge
-2
Planck's constant
6.626 x 10^-34
A - B (with a chemical bond) What is not shown in this representation that we may forget?
Adding in attractive nuclear to electron forces and nuclear to nuclear repulsive forces
Formula for: aluminum hydroxide
Al(OH)3
Formula for: Bromide
Br
Formula for: Hypobromite
BrO-
Formula for: Bromite
BrO2-
Formula for: Bromate
BrO3-
Formula for: Perbromate
BrO4-
Specify what ions are present in solution upon dissolving each of the following substances in water: Ca(OH)2
Ca 2+ and OH-
Write the formula and classify it as either a strong, weak or non-electrolyte: Sucrose
C12H22O11, Non-electrolyte
Write the formula and classify it as either a strong, weak or non-electrolyte: Octante
C8H18, Non-electrolyte
Write the formula and classify it as either a strong, weak or non-electrolyte: Acetic Acid
CH3COOH, Weak
Formula for: Carbonate
CO3 2-
Formula for: Chlorite
ClO2-
Formula for: Chlorate
ClO3-
Formula for: Perchlorate
ClO4-
Formula for: copper oxide
CuO
Why is line spectra important?
Each element has a unique line spectrum
Specify what ions are present in solution upon dissolving each of the following substances in water: FeCl2
Fe 2+ and Cl -
Formula for: Iron (III) Carbonate
Fe2(CO3)3
Specify what ions are present in solution upon dissolving each of the following substances in water: HNO3
H + and NO3-
Carbonic Acid Formula
H2CO3
Sulfuric Acid Formula
H2SO4
Phosphoric Acid Formula
H3PO4
Formula for: Hydrogen carbonate
HCO3-
Define Isoelectronic
Having the same amount of electrons
Nitric Acid formula
HNO3
Formula for: Mercury(II) bromide
HgBr2
Why did Bohr's model fail?
It failed to explain the spectrum for elements other than hydrogen
Formula for: potassium sulfate
K2SO4
Write the formula and classify it as either a strong, weak or non-electrolyte: Potassium hydroxide
KOH, Strong
Formula for: Nitride
N 3-
Specify what ions are present in solution upon dissolving each of the following substances in water: (NH4)2SO4
NH4 + and SO2 2-
Formula for: Nitrite
NO2-
Formula for: Nitrate
NO3-
Formula for: Sodium hypobromite
NaBrO
Write the formula and classify it as either a strong, weak or non-electrolyte: Sodium chloride
NaCl, Strong
Formula for: Phosphite
PO3 3-
Formula for: Phosphate
PO4 3-
Formula for: Sulfite
SO3 2-
Formula for: Sulfate
SO4 2-
Formation enthalpy
The energy of forming or breaking bonds
Why is a 3s orbital larger than a 2s orbital?
The number of electrons. They repel each other
True or false: Sulfuric acid is a diprotic acid
True. It has two ionizable hydrogen atoms
Formula for: Zinc nitrate
Zn(NO3)2
Average bond enthalpies are
always positive, bond breaking is an endothermic process
What is a valence electron?
electrons in the outermost shell
The sum of all the kinetic and potential energies of a system is called the
internal energy
identify the n, l, ml, and ms for a 3p orbital
n=3 l=1 ml=-1,0,1 ms = +1/2 and -1/2
Sign of exothermic process
negative
Sign of endothermic process
positive
Shape of s orbital
spherical
Electron affinity
the energy change accompanying the addition of an electron to a gaseous atom
bond enthalpy
the enthalpy change required to break a particular bond in 1 mole of gaseous molecules
Define: Standard Enthalpy of Formation
the enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions
Size of s orbital increases with
the value of n