Made of protons and neutrons
Surrounded by cloud of electrons
Size of \(10^{-15}\) meters
| Proton (+) | Neutron ( ) | Electron (-) | |
|---|---|---|---|
| Mass | 1.67262×10⁻²⁴ grams | 1.674493×10⁻²⁴ grams | 9.10938356×10⁻³¹ grams |
| Mass ratio | 1837 | 1837 | 1 |
| Charge | 1.602×10⁻¹⁹ | 0 | -1.602×10⁻¹⁹ |
| Charge Ratio | 1 | 0 | -1 |
Energy it takes to remove an electron completely
Equal and opposite to Coulombic Potential Energy
Measured in kilojoules per molecules
Increases across a period and decreases across a group
Same number of protons but a different number of neutrons
Atoms that lose electrons to have a positive charge (metals do this more often)
Metals do this more often
Atom that gain electrons to have a negative charge (nonmetals do this more often)
Nonmetals do this more often
Lowest energy state(ie. # of protons is equal to # of electrons)
# of protons is equal to # of electrons
Photon makes an electron jump to an outside shell
Electron loses energy and falls down a shell
Energy change resulting from adding an electron to a gaseous atom
\(\Delta EN \leq 0.7\)
An equal amount of attraction occurs on both atoms
\(\Delta EN > 0.7\) and \(\leq 2\)
The attraction from an atom on another atom is greater than its reciprocal
\(\Delta EN > 2\)
The attraction from an atom on another atom is a lot greater than its reciprocal
It holds everything together
It is represented by \(\delta^{+}\) and \(\delta^{-}\)
The larger atom is labeled as \(\delta^{-}\)
The smaller atom is labeled as \(\delta^{+}\)
Bond made possible by the electronegative atoms nitrogen, oxygen, and fluorine to the atom hydrogen
The strongest intermolecular force
Pulling apart of an ionic structure in dissolving (ie. water dissociating sodium chloride into sodium and chlorine ions)
Only the seperation of molecules, not seperating atoms (ie. water dissolving glucose)
Minor component
Gets dissolved
Major component
Does the dissolving
Homogeneous mixture of solute and solvent
Uniform composition
| Solute | Solvent | Dominant intermolecular Force | Is solution formed? |
|---|---|---|---|
| Polar | Polar | Dipole-Dipole Force and/or Hydrogen Bond | Yes |
| Non-Polar | Non-Polar | Dispersion Force | Yes |
| Polar | Non-Polar | No | |
| Non-Polar | Polar | No | |
| Ionic | Polar | Ion-Dipole | Yes |
| Ionic | Non-Polar | No |
Increases the neutral concentration of \(\ H^{+}\)
Increases the neutral concentration of \(\ H^{-}\)
\(\ H_{2}O\) and salts
Show up as pairs in nature
Hydrogen
Oxygen
Fluorine
Bromine
Iodine
Nitrogen
Chlorine
All the particles are tightly attracted to each other and cannot freely move around.
All the particles are not so tightly bound and can slide past each other. However, the attractions is still not weak enough to turn it into a gas
All the particles have little to no attraction to each other due to some factor like heat and fills all avalible volume.
All particles of a compound is dissolved in water but the water is not part of the chemical reaction
\(q_{1}\) and \(q_{2}\) represents the masses of the atoms
\(k_{e}\) is a constant
\(r\) is the distance between the centers of the atoms
\(F_{12}\) and \(F_{21}\) is the force by \(q_{1}\) on \(q_{2}\) and \(q_{2}\) on \(q_{1}\) respectively
Particles correctly orientated
Collide with enough energy
Rate: Change in something per unit time
Rate of Reaction: \(\frac{\textrm{Amount of substance change}}{\Delta\textrm{(Unit Time)}}\)
Exothermic: Heat is a byproduct of the reaction
Endothermic: Heat is absorbed in the reaction
Activation Energy: Energy needed to start a reaction
Catalyst: Lowers the activation energy of a reaction
Particles: Refers to both molecules and atoms depending on context and reaction
Potential energy is equal to bond energy
Exothermic reaction
Endothermic reaction
Concentration
Temperature
Surface Area
Catalyst
Pressure