Hohmann transfer orbit

Examples of Hohmann transfer orbit in the following topics:

• Orbital Maneuvers

  • The rest of the flight, especially in a transfer orbit, is called coasting.
  • The Hohmann transfer orbit is an elliptical orbit used to transfer between two circular orbits of different altitudes in the same plane.
  • The orbital maneuver to perform the Hohmann transfer uses two engine impulses that move aspacecraft onto and off the transfer orbit, as diagramed in .
  • Hohmann transfer orbits are the most efficient with fuel.
  • Other non-Hohmann types of transfer orbits that are less efficient with fuel exist, but these may be more efficient with other resources (such as time).

• Satellites

  • Low Earth orbit is any orbit below 2000 km, and Medium Earth orbit is any orbit higher than that but still below the altitude for geosynchronous orbit at 35,786 km.
  • High Earth orbit is any orbit higher than the altitude for geosynchronous orbit.
  • Hohmann transfer orbit: An orbital maneuver that moves a spacecraft from one circular orbit to another using two engine impulses.
  • Geosynchronous transfer orbit: An elliptic orbit where the perigee is at the altitude of a Low Earth orbit (LEO) and the apogee at the altitude of a geosynchronous orbit.
  • Geostationary transfer orbit: An elliptic orbit where the perigee is at the altitude of a Low Earth orbit (LEO) and the apogee at the altitude of a geostationary orbit.

• Coloring Agents

  • Most transitions that are related to colored metal complexes are either d–d transitions or charge transfer bands.
  • In a d–d transition, an electron in a d orbital on the metal is excited by a photon to another d orbital of higher energy.
  • A charge transfer band entails promotion of an electron from a metal-based orbital into an empty ligand-based orbital (Metal-to-Ligand Charge Transfer or MLCT).
  • The converse will also occur: excitation of an electron in a ligand-based orbital into an empty metal-based orbital (Ligand to Metal Charge Transfer or LMCT).
  • Discuss the relationship between charge transfer and the color of a metal complex.

• Color

  • Most transitions that are related to colored metal complexes are either d–d transitions or charge band transfer.
  • In a d–d transition, an electron in a d orbital on the metal is excited by a photon to another d orbital of higher energy.
  • Electrons can also be transferred between the orbitals of the metal and the ligands.
  • In Metal-to-Ligand Charge Transfer (MLCT), electrons can be promoted from a metal-based orbital into an empty ligand-based orbital.
  • Conversely, an electron may jump from a predominantly ligand orbital to a predominantly metal orbital (Ligand-to-Metal Charge Transfer or LMCT).

• Reactions of Coordination Compounds

  • There are also organic ligands such as alkenes whose pi (π) bonds can coordinate to empty metal orbitals.
  • A common reaction between coordination complexes involving ligands are electron transfers.
  • There are two different mechanisms of electron transfer redox reactions: inner sphere or outer sphere electron transfer.
  • These substrates need an empty orbital to be able to react with a metal center.
  • Metals with half-filled orbitals have a tendency to react with such substrates.

• Physical Properties and Atomic Size

  • Color in transition-series metal compounds is generally due to electronic transitions of two principal types: charge-transfer transitions and d-d transitions.
  • An electron may jump from a predominantly ligand orbital to a predominantly metal orbital, giving rise to a ligand-to-metal charge-transfer (LMCT) transition.
  • A metal-to ligand charge transfer (MLCT) transition will be most likely when the metal is in a low oxidation state and the ligand is easily reduced.
  • In a d-d transition, an electron jumps from one d-orbital to another.
  • In complexes of the transition metals, the d orbitals do not all have the same energy.

• Transition Metals

  • Color in transition-series metal compounds is generally due to the electronic transitions of two principal types of charge transfer transitions.
  • An electron may jump from a predominantly ligand orbital to a predominantly metal orbital, giving rise to a ligand-to-metal charge transfer (LMCT) transition.
  • An electron jumps from one d-orbital to another.
  • In complexes of the transition metals, the d orbitals do not all have the same energy.
  • I2•PPh3 charge-transfer complexes in CH2Cl2.

• Percent Ionic Character and Bond Angle

  • When two elements form an ionic compound, is an electron really lost by one atom and transferred to the other?
  • The answer to the above question is both yes and no: yes, the electron that was now in the 2s orbital of Li is now within the grasp of a fluorine 2p orbital; but no, the electron is now even closer to the Li nucleus than before, so it is not truly "lost."
  • The emerging view of ionic bonding is one in which the electron orbitals of adjacent atom pairs are simply skewed, placing more electron density around the "negative" element than around the "positive" one.
  • The more covalent in nature the bond, the more likely the atoms will situate themselves along the predetermined vectors given by the orbitals that are involved in bonding (VSEPR theory).

• Rotational Kinetic Energy: Work, Energy, and Power

  • Due to conservation of angular momentum this process transfers angular momentum to the Moon's orbital motion, increasing its distance from Earth and its orbital period.

• Charge Separation

  • ., they can be transferred from atom to atom) it is possible for the phenomenon of "charge separation" (often referred to as static electricity) to occur.
  • In chemistry, this charge separation is illustrated simply by the transfer of an electron from one atom to another as an ionic bond is formed.
  • This is because electrons from one have transferred to the other, causing one to be positive and the other to be negative.
  • For example, a nearby negative charge can "push" electrons away from the nucleus around which they typically orbit.