hydrogen-like

(adjective)

having a single electron

Related Terms

  • valence shell
  • electron shell

Examples of hydrogen-like in the following topics:

  • Energy of a Bohr Orbit

    • So, if a nucleus has $Z$ protons ($Z=1$ for hydrogen, $Z=2$ for helium, etc.) and only one electron, that atom is called a hydrogen-like atom.
    • The spectra of hydrogen-like ions are similar to hydrogen, but shifted to higher energy by the greater attractive force between the electron and nucleus.
    • Using this equation, the energy of a photon emitted by a hydrogen atom is given by the difference of two hydrogen energy levels:
    • Bohr's model predicted experimental hydrogen spectrum extremely well.
    • Apply proper equation to calculate energy levels and the energy of an emitted photon for a hydrogen-like atom
  • Problems

    • Derive the lifetime of the $n=2, l=1, m=0$ state of hydrogen to emit a photon and end up in the $n=1, l=0, m=0$ state.
    • Consider that the mass fraction of the different atoms are hydrogen (0.7), helium (0.27), carbon (0.008), oxygen (0.016) and iron (0.004).
  • Hydrogen Bonding and Van der Waals Forces

    • When polar covalent bonds containing hydrogen form, the hydrogen in that bond has a slightly positive charge because hydrogen’s one electron is pulled more strongly toward the other element and away from the hydrogen.
    • This interaction is called a hydrogen bond.
    • Hydrogen bonds are also responsible for zipping together the DNA double helix.
    • Like hydrogen bonds, van der Waals interactions are weak attractions or interactions between molecules.
    • The slightly negative oxygen side of the water molecule and the slightly positive hydrogen side of the water molecule are attracted to each other and form a hydrogen bond.
  • Water’s Polarity

    • The two hydrogen atoms and one oxygen atom within water molecules (H2O) form polar covalent bonds.
    • Water's charges are generated because oxygen is more electronegative, or electron loving, than hydrogen.
    • Thus, it is more likely that a shared electron would be found near the oxygen nucleus than the hydrogen nucleus.
    • Since water is a nonlinear, or bent, molecule, the difference in electronegativities between the oxygen and hydrogen atoms generates the partial negative charge near the oxygen and partial positive charges near both hydrogens.
    • This interactive shows the interaction of the hydrogen bonds among water molecules.
  • The Hydrogen Economy

    • The hydrogen economy refers to using hydrogen as the next important source of fuel.
    • Free hydrogen does not occur naturally in quantities of use, like other energy sources, but it can be generated by various methods.
    • Alternatively, liquid hydrogen or slush hydrogen (a combination of liquid and solid hydrogen) can be used.
    • Hydrogen can be stored as a chemical hydride or in some other hydrogen-containing compound.
    • This means that any leak of hydrogen from a hydrogen:air mixture will most likely lead to an explosion if it comes into contact with a spark or flame.
  • Water’s States: Gas, Liquid, and Solid

    • The formation of hydrogen bonds is an important quality of liquid water that is crucial to life as we know it.
    • In liquid water, hydrogen bonds are constantly formed and broken as the water molecules slide past each other.
    • On the other hand, when the temperature of water is reduced and water freezes, the water molecules form a crystalline structure maintained by hydrogen bonding (there is not enough energy to break the hydrogen bonds).
    • Cells can only survive freezing if the water in them is temporarily replaced by another liquid like glycerol.
    • Hydrogen bonding makes ice less dense than liquid water.
  • Covalent Bonds and Other Bonds and Interactions

    • The electron from the hydrogen splits its time between the incomplete outer shell of the hydrogen atom and the incomplete outer shell of the oxygen atom.
    • When polar covalent bonds containing hydrogen are formed, the hydrogen atom in that bond has a slightly positive charge (δ+) because the shared electrons are pulled more strongly toward the other element and away from the hydrogen atom.
    • The weak interaction between the δ+ charge of a hydrogen atom from one molecule and the δ- charge of a more electronegative atom is called a hydrogen bond.
    • For example, hydrogen bonds are responsible for zipping together the DNA double helix.
    • Like hydrogen bonds, van der Waals interactions are weak interactions between molecules.
  • Binary Hydrides

    • A hydride is the anion of hydrogen (H−), and it can form compounds in which one or more hydrogen centers have nucleophilic, reducing, or basic properties.
    • In such hydrides, hydrogen is bonded to a more electropositive element or group.
    • Even certain enzymes, like hydrogenase, operate via hydride intermediates.
    • Instead, many compounds have a hydrogen center with a hydridic character.
    • In these substances, the hydride bond, formally, is a covalent bond much like the bond that is made by a proton in a weak acid.
  • Chemiosmosis and Oxidative Phosphorylation

    • During chemiosmosis, electron carriers like NADH and FADH donate electrons to the electron transport chain.
    • This protein acts as a tiny generator turned by the force of the hydrogen ions diffusing through it, down their electrochemical gradient.
    • The overall result of these reactions is the production of ATP from the energy of the electrons removed from hydrogen atoms.
    • The extra electrons on the oxygen attract hydrogen ions (protons) from the surrounding medium and water is formed.
    • In oxidative phosphorylation, the hydrogen ion gradient formed by the electron transport chain is used by ATP synthase to form ATP.
  • Hydrogen Bonding

    • A hydrogen bond is a strong intermolecular force created by the relative positivity of hydrogen atoms.
    • A hydrogen atom attached to a relatively electronegative atom is a hydrogen bond donor.
    • This hydrogen atom is a hydrogen bond donor.
    • Greater electronegativity of the hydrogen bond acceptor will create a stronger hydrogen bond.
    • Where do hydrogen bonds form?
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