Final Exam Flashcards
What are the three laws of thermodynamics?
Energy never created or destroyed
Entropy of the universe increases in spontaneous, unchanged in equilibrium
Entropy of a perfect crystalline substance is zero at the absolute zero of temperature
What is the atomic number equal to?
Number of protons
What is the mass number equal to?
Number of protons and neutrons
What are the two types of ions?
Cation - positive charge
Anion - negative charge
How many nanometers are in one meter?
1 X 10^9
What is the unit for frequency?
Hertz
1/s
What does heisenburgs uncertainty principle state?
Can not know position and momentum of a particle at the same time
What are the quantum numbers?
n - energy or distance from nucleus (1,2,3…..)
L - Shape (0,1,2 … n-1)
ML - Orientation in space ( -L to L)
Ms - Electron spin ( + .5 or - .5)
What are the shapes of the orbitals based on the L numbers?
0 = S-orbital 1 = P-orbital 2 = D-orbital 3 = F-orbital 4 = G-orbital
What happens in an excited state?
An electron gets bumped up a level
Always add or subtract from the orbital with the largest n followed by highest L
What does isoelectronic mean?
Any atom/ion with the same electronic configurations
What is the ionization energy?
Energy required to remove an electron
Why does ionization energy increase from left to right?
The force holding the electrons increases, closer to full orbital
Why does ionization energy decrease from top to bottom?
As you go down n increases, therefore so does the radius
Force on electrons is decreased as R goes up
Why does atomic radius increase from top to bottom?
There are more orbitals
Why does atomic radius decrease from left to right?
Elements with more protons in a period will have more attraction making the radius smaller
What is electronegativity?
The ability to attract electrons in a chemical bond
What is formal charge and how do you calculate it?
Mechanism that compares valence electrons in an atom
FC = (number of valence electrons) - (number of lone pair electrons) - .5(number of bonding electrons)
What is a resonance structure?
The location of the double bonds can change and the resonance structure is like a hybrid
What is the steric number?
Number of bonded atoms and lone pairs on a central atom
What are isotopes?
Same number of protons, different number of neutrons
What are paramagnetic?
Has at least one unpaired electron
What is diamagnetic?
No unpaired electrons
What are the bonding electron pairs, arrangement, angle, and shape?
2 - Linear - 180 - Linear
3 - Trigonal Planar - 120 - trigonal planar
4 - Tetrahedral - 109.5 - Tetrahedral
5 - Trigonal bipyramidal-120 or 90-trigonal bipyramid
6 - Octahedral - 90 - octahedral
What are the bonding electrons, lone pair electrons, arrangement, angle and shape?
2 - 1 - Trigonal planar - <109.5 - Trigonal Pyramidal
3 - 2 - Trigonal bipyr - 120, 90 - TShaped
4 - 1 - Trig bipyr - 120,90 - See saw
4 -2 - Octahedral - 90 -Square Planar
5 - 1 - Octahedral - 90 - square pyramidal
What is the hybridizarion based on the steric number?
2 - sp
3 - sp2
4 - sp3
5 - sp3d
What is the bond order?
.5(electrons in bonding pair) - .5(electrons in antibonding)
What are the two exceptions for molecular orbitals?
O2, ne2 and F2 have r2p before the pi2p
What is the triple point?
Intersection of three phase boundries, all three exist simultaneously
What is the critical point?
Where the gas and liquid line terminate
What is the order of strengths with internolecular forces?
Hydrogen Dipole - dipole Polar Dipole induced Dispersion
What are the atoms that hydrogen bonds can form with?
Oxygen
Nitrogen
Fluorine
According to simple collision theory what three things must happen for a reaction to occur?
Collision between reactant particles
Correct oroentation of collision particles
Minimum energy must be met to get it activated
What must a molecule have to be dipole?
Must be polar
How do you tell if a molecule is polar?
A molecule is polar if there are lone pairs on central atom or the centeal atom is bonded to different atoms
How are intramolecular forces related to boiling and melting point?
The stronger the intramolecular forces the higher the melting point and lower the boiling point
What is a buffer system?
A solution that resists change in pH
Consists of a weak acid and a weak base
What is a system?
Substance of interest
What are the surroundings?
All matter around the system
