Final Flashcards
How to find empirical formula
If given percent, the percent is grams (assume 100g)
Find miles of each through stoich
Divide each by smallest number of moles
How to find molecular formula
Find molar mass of empirical
If given real molar mass, divide by empirical mass
Take that number and multiply formula
Entropy
Disorder of a system
How to find what has greatest entropy
Largest molecules and highest states of matter have greatest entropy
Entropy change is measured in
Δs
In order for an endothermic reaction to be spontaneous under standard conditions and constant pressure…. what’s up with Δa and Δh/t
Δs must be positive and greater than Δh/t
What’s the difference between internal energy change Δu and enthalpy change Δh
Work
What is a spontaneous process
It occurs on its own
For quantum number stuff, what is L
N-1 or less (it’s the orbital) ex-2P
Spdf numbers
S-0
P=1
D=2
F=3
What is m sub l (quantum number)
Number of sub orbital
It can be + or - L
(Write out the written electron theory thing with the ups and downs) (the last electrons placement is the sub level )
What is VSEPR bro is same as electron pair geometry? Is it polar or non polar
Non polar
What dictates mass change in an atom
Number of neutrons
Isotopes
Same element with different mass number/number of neutrons
What is the identity of an atom determined by
Protons
Isomer
Two or more compounds with same formula but different arrangement of atoms
Also has different properties
Allotrope
Two or more physical forms which an element can exist in
What can be lost from nucleus that doesn’t result in charge of atomic number
Neutrons
What did Rutherford’s gold foil experiment show
Atoms were mostly empty space
Electromagnetic spectrum in terms of high to low
X rays If rays Visible Infrared Microwaves TV radio
What does the L quantum number determine
Angular momentum
Entropy measures
Energy going out in the universe
If surroundings are increasing, system is decreasing
Emission
When electron returns to ground state by releasing extra energy absorbed
Absorption
When atom changes from ground state to excited state
Isoelectric
Having no net charge or difference in electron potential
Think or noble gas configuration?
How does Mg differ from Mg2+
Ion has inert gas electron configuration
Atom does not
Which term best characterized relation of hydrogen to deutreium
Isotope
Deuterium
One of two stable isotopes of hydrogen
2h
Protium
Another stable isotope of hydrogen (1h)
Tritium
Hydrogen radioactive isotope (3h)
Alpha particle
2 protons and 2 neutrons released from an atom
Has a charge of +2 and interacts with matter greatly
Equation of wavelength if given speed
λ=h/mass x velocity
How to determine what the m sub s quantum number is
It will be + or - 1/2 depending on if last electron is an up or down arrow
(Down is -)
What are the two types of bonds that have expected conductivity when solid is FUSED
Ionic
Metallic
What is the only type of bond with a high expected conductivity when in a SOLID state?
Metallic
Melting point of a mixture is expected to be _____than melting point of a pure substance
Lower
Lower vapor pressures have ____ surface tension
Greater
Substances with a lower vapor pressure have ______ tendency to change from liquid to gas
Little
What mass of gases will escape most quickly through a pinhole leak
Light gasses
Partial pressure
Force exerted by gas
Heavier gassed have more partial pressure
Avogadro principle with gas
Equal volumes of any gas under the same temperature and pressure conditions will contain the same number of particles
Average kinetic energy is proportional to..
Temperature
When finding how much WATER needs to be added to a stock solution, what do you do?
Find difference between v1 and v2
What is a unit cell
the smallest group of atoms of a substance that has the overall symmetry of a crystal of that substance, and from which the entire lattice can be built up by repetition in three dimensions.
What effects vapor pressure of a liquid
Temperature
Work function
Energy needed to eject electrons from surface
Stuff below frequency won’t eject light
Exceptions to hunds rule
Cr
Cu
Ag
Mo
Lattice energy guidelines
Greater the difference in charge makesattice energy go up
Bigger diameter makes lattice energy go down
Intensive physical qualities
Not dependent on quantity
Extensive physical properties
Dependent on physical quantity
Ex-boiling point
How to get from Celsius to kelvin
C plus 273.15
