Final Exam Flashcards
Boyles Law
As pressure increases volume decreases
P1V1=P2V2
Inversely proportional
Charles Law
As temperature increases volume increases
Directly proportionate
V1/T1 = V2/T2
Degrees in Kelvin
Gay Lussac Law
As pressure increases temperature increases
P1/T1 = P2/V2
Units of pressure
1 atm= 101.3 kpa = 760 mm Hg = 760 Torr = 14.7 psi
Combined gas law
P1V1/T1 = P2V2/T2
Ideal gas law
PV=nRT P= pressure V= volume n= moles R= constant T= temperature in Kelvin
Kelvin Temperature
Degrees celsius + 273
Orbital
Area where an electron is most likely found
S p d f
Where is the electron
S - starts in energy level 1/ 1 orbital w 2 electrons/ sphere shape
P - energy level 2 orbital 3/ 6 electrons/ dumbell shape
D- energy level 3 orbital 5/ 10 electrons flower shape
F- energy level 4/ 7 orbitals 14 electrons
Electron configurations
Rules
Aufbau principle- electrons enter the lowest energy level
Hans rule- electrons enter different orbitals of the same energy level
Pauli Exclusion- max 2 electrons must have opposite spins
Wavelength
Length of the wave
Frequency
of waves per second
The periodic table
Patterns
Rows and Families
Electronegativity
Ability of an atom to attract electrons
Increase from left to right- atoms are smaller with greater nucleur charge (same electrons in level but more protons means they are pulles tighter together )
Decrease from top to bottom- more energy levels
Ionization Energy
Energy required to remove the electron of the outermost energy level
Increase from left to right- atoms are smaller with greater nucleur charge (same electrons in level but more protons means they are pulles tighter together )
Decrease from top to bottom- more energy levels
Atomic Radius
Half the diameter of an atom, found by the distance between the nuclei of 2 bonded atoms
Increase top to bottom bc more energy levels
Decrease left to right bc greater nucleur charge
Acid
Produces H3O when dissolved in water
Increases by 0s ( 2=10 4=1000)
Base
Produces OH- when dissolved in water
Strong vs Concentrated
Weak vs dilute
Strong - all or most electrons are ionizing
Concentrated- a lot of solute
Weak- few electrolytes are breaking apart
Dilute- little solute
Acid strength
0-7 acidic
7 neutral
7-14 basic
Lewis dot structure
Shows where the 8 valence electrons are located
Ionic chart
Ionic - the give and take of electrons between a metal and a nonmetal only conductive if dissolved in water High melting point Ex salt
Nonpolar covalent
The even sharing of electrons Between a metal and a nonmetal Not conductive Low melting pt Ex butter
Polar covalent
Uneven sharing of electrons Between a metal and a nonmetal Not conductive Medium melting point Ex sugar
Metalloids
Sea of electrons Between metals Conductive Pretty high melting pt Ex aluminum
Molarity
Moles of solvent / kg of solvent
VSPER
Valence Shell Electron Repulsion Theory
Single bond
Sharing of 2 electrons
Double bond
Sharing of 2 electrons
Triple bond
Sharing of 6 electrons
Bond length
Distance between 2 bonding atoms on picometers
In order single double triple
Bond order
Same as # of bonds
London dispersion theory
Used with nonpolar bonds
Weakest
Buildup of electrons temporarily on one side of the molecule
Ex traffic jam
Dipole forces
Polar bonds
Two opposite sided molecules that have a partial permanent separation of charge bc electrons are not evenly shared
Hydrogen bonding
Only with H - O N or F
Strongest bc Hydrogen can only bond with one thing so nothing counteracts it
Intermolecular forces
Forces between seperate molecules
The breakdown of IMFs is a physical change
Nonpolar vs polar
Nonpolar = even sharing Polar = uneven
Solution
Homozygous mixture too small to see the solute particles
Colloid
A solute thay reflects light but you cant really see with the human eye
Suspension
Solute that settles over time
Solute vs solvent
Solute- what is being dissolved
Solvent- what it is being dissolved kn
Electrolyte
Anything that produces free flowing charges when dissolved on water
Non electrolyte
When molecules separate from other molecules but free flowing charges are not produces
