Chemical laws + theories

• Avogadro's Law

  Equal volumes of gases under identical temperature and pressure will contain equal numbers of particles (atoms, ions, molecules, electrons, etc.)
• Boyle's Law

  At a constant temperature, the volume of a confined gas is inversely proportional to the pressure to which the gas is subjected: PV = k OR P=1/V OR T=1/P
• Charles' Law

  At a constant pressure, the volume of a confined gas is directly proportional to the absolute temperature in Kelvin: V = kT OR T1/V1 = T2/V2
• Conservation of Energy

  Energy can neither be created nor destroyed; the energy of the universe is constant. This is the First Law of Thermodynamics.
• Conservation of Mass

  Matter can neither be created nor destroyed, though it can be rearranged. Mass remains constant in an ordinary chemical change. This principle is also known as Conservation of Matter.
• Dalton's Law

  The pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases.
• Law of Definite Composition/Proportions

  A compound is composed of two or more elements chemically combined in a definite ratio by weight.
• Dulong-Petit Law

  Most metals require 6.2 calories of heat to raise the temperature of one gram-atomic mass of metal by one degree Celsius.
• Faraday's Law

  The weight of any element liberated during electrolysis is proportional to the quantity of electricity passing through the cell and also to the equivalent weight of the element.
• First Law of Thermodynamics

  The total energy of the universe is constant and can neither be created nor destroyed. This law is also known as Conservation of Energy.
• Gay-Lussac's Law

  When volume is constant, pressure is directly proportional to kinetic energy/temperature in Kelvin: T1P1=T2P2
• Graham's Law

  The rate of diffusion or effusion of a gas is inversely proportional to the square root of its molecular mass.
• Henry's Law

  The solubility of a gas (unless it is highly soluble) is directly proportional to the pressure applied to the gas.
• Ideal Gas Law

  The state of an ideal gas is determined by its pressure, volume, and temperature according to the equation: PV = nRT where P is the absolute pressure, V is the volume of the vessel, n is the number of moles of gas, R is the ideal gas constant, and T is the absolute temperature in Kelvin.
• Multiple Proportions

  When elements combine, they do so in the ratio of small whole numbers. The mass of one element combines with the fixed mass of another element according to certain ratios.
• Periodic Law

  The chemical properties of the elements vary periodically according to their atomic numbers.
• Second Law of Thermodynamics

  Entropy increases over time. Another way of stating this law is to say that heat cannot flow, on its own, from an area of cold to an area of hot.
• Gibbs Free energy is the maximum amount of work that can occur in a closed system under constant conditions
• Entropy is the degree of randomness in a system and its ability to put energy into work
• Combined gas law


  (P1 x V1)/T1 = (P2 x V2)/T2
• Hund's rule


  Each atomic orbital must be filled once (singularly) before being filled twice (doubly)
• Aufbac's Principle

  Electrons must fill lower energy levels first before moving outwards
• Pauli's exclusion Principle

  Each Atomic orbital may only hold 2 electrons and they must be of opposite spins
• Fehling's Reagent


  A solution of copper that detects glucose in urine to examine for diabetes
• Why does ionization energy double after losing all its valance electrons?

  After ionization, atom is positive so there is a higher nuclear charge and electrons are more attracted to the nucleus. Additionally the loss of all valance electrons means the atom now needs to lose electrons from a sub-level that is even closer to the nucleus, hence more attracted and hard to remove, requiring much more energy
• Absolute zero

  At 0 Kelvins, where all motion theoretically ceases to exist.
• Heisenberg Uncertainty principle

  It isn't possible to know the exact location or momentum of electrons at the same time but there are spaces in which there is a large probability of finding these electrons
• Order of sub-atomic orbitals

  1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f
• Holding all components of the atom together

  Effective nuclear charge that increases with greater mass that draws in electrons through electrostatic attraction and the momentum of electrons keep them from crashing into the nucleus
• Electromagnetic spectrum acronym

  Gay Xylophones united very interestingly, maybe rationally
• 5 assumptions for the Kinetic theory of Mass for ideal gases?

  • The volume of gas particles = 0
  • gas particles are in constant random motion
  • collisions between gas particles are elastic with no force being -exchanged
  • collisions of gas against the vessel cause pressure
  • average kinetic energy is proportional to temperature in Kelvins
• Kinetic theory of Mass

  A model of the thermodynamic behaviors of gases
• What is achieved due to non-directional electrons?

  Alloys, Malleability, ductility, good conduction
• Concentration

  [x]
• Law of electrostatic attraction

  like deflect, opposite attract
• Dalton's atomic theory


  atoms cannot be destroyed but can be changed through nuclear fission/fusion and contain protons, neutrons, and electrons
• Neils Bohr


  said that electrons don't crash into nucleus because of nuclear force with neutrons balancing charges and adding mass- more protons than neutrons=radioative