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Examples of the the word, hydrogen , in a Sentence Context

The word ( hydrogen ), is the 4573 most frequently used in English word vocabulary

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  1. To a carboxyl group (thus they are carboxylic acids),an amino group,a, hydrogen ,atom and a variable group. The variable group, also called the R group or side
  2. Conjugate base is more negatively charged. Although the subsequent loss of each, hydrogen ,ion is less favorable,all the conjugate bases are present in solution. The
  3. Ethane,C2H6 - two carbon and six hydrogen : propane,C3H8 - three carbon and 8, hydrogen , : butane,C4H10 - four carbon and 10 hydrogen : pentane,C5H12 - five carbon and
  4. Only one additional electron is required to fill in the outermost shell of the, hydrogen ,atom, so hydrogen can in some circumstances behave like a halogen, forming the
  5. Equal to half of the atom's atomic weight, expressed in numbers of, hydrogen ,atoms. This central charge would thus be approximately half the atomic weight (
  6. C4H10 - four carbon and 10 hydrogen : pentane,C5H12 - five carbon and 12, hydrogen , : humane,C6H14 - six carbon and 14 hydrogen These names were derived from
  7. Behave like a halogen, forming the negative hydride ion. Binary compounds of, hydrogen ,with the alkali metals and some transition metals have been produced in the
  8. Dissolved in water. Note that chemists often write H+ (a) and refer to the, hydrogen ,ion when describing acid-base reactions but the free hydrogen nucleus, a proton
  9. Hydrogen bonds and are insoluble in polar solvents such as water. Since the, hydrogen ,bonds between individual water molecules are aligned away from an alkane
  10. Three examples show, acids can be solutions, liquids,or solids. Gases such as, hydrogen ,chloride can be acids as well. Strong acids and some concentrated weak acids
  11. React with halogens in a so-called free radical alienation reaction. The, hydrogen ,atoms of the alkane are progressively replaced by halogen atoms. Free-radicals
  12. Usually placed at the top of Group 1 of the periodic table for convenience, but, hydrogen , is not counted as an alkali metal. Under typical conditions, pure hydrogen
  13. With water are as follows: Alkali metal + water → Alkali metal hydroxide +, hydrogen ,gas For a typical example (M represents an alkali metal): :2 M (s) + 2 H2O
  14. The Swedish chemist State Arrhenius attributed the properties of acidity to, hydrogen ,in 1884. An Arrhenius acid is a substance that increases the concentration of
  15. Chain reaction or Propagation then takes place—the halogen radical abstracts a, hydrogen ,from the alkane to give an alkyl radical. This reacts further. * Chain
  16. Does become metallic, and it behaves like an alkali metal. This type of, hydrogen ,is known as metallic hydrogen . Hydrogen is sometimes considered to be an alkali
  17. It exists only in small quantities due to its high radioactivity. Below, hydrogen ,is included for comparison. Hydrogen The element hydrogen , with its solitary
  18. Of a specific amino acid. In glycine, the simplest amino acid, the R group is a, hydrogen ,atom, but in all other amino acids it is contains one or more carbon atoms
  19. Properties Virtually all organic compounds contain carbon – carbon and carbon –, hydrogen ,bonds, and so show some features of alkanes in their spectra. Alkanes
  20. Or saturated hydrocarbons) are chemical compounds that consist only of, hydrogen ,and carbon atoms and are bonded exclusively by single bonds (i.e., they are
  21. Of 14. Each carbon atom must have 4 bonds (either C-H or C-C bonds),and each, hydrogen ,atom must be joined to a carbon atom (H-C bonds). A series of linked carbon
  22. The tetrahedron onto a flat plane. However, the torsion angle between a given, hydrogen ,atom attached to the front carbon and a given hydrogen atom attached to the
  23. Radioactivity. Below, hydrogen is included for comparison. Hydrogen The element, hydrogen , with its solitary one electron per atom, is usually placed at the top of Group
  24. Usually found at oh 0.5 – 1.5. The carbon-13 resonances depend on the number of, hydrogen ,atoms attached to the carbon: BC 8 – 30 (primary, methyl,-CH3),15 – 55 (
  25. The axis of the C – C bond, one will see the so-called Newman projection. The, hydrogen ,atoms on both the front and rear carbon atoms have an angle of 120° between
  26. Of an acid to lose a proton is the strength of the bond between the acidic, hydrogen ,and the atom that bears it. This, in turn, is dependent on the size of the
  27. Its atomic radius is also much smaller, so it shares a stronger bond with, hydrogen , Moving down a column on the periodic table atoms become less electronegative
  28. Pentane,C5H12 - five carbon and 12 hydrogen : humane,C6H14 - six carbon and 14, hydrogen , These names were derived from methanol, ether,prop ionic acid and butyric acid
  29. Mixture produced, however,is not a statistical mixture: Secondary and tertiary, hydrogen ,atoms are preferentially replaced due to the greater stability of secondary and
  30. Of carbon atoms) are named as follows:: methane,CH4 - one carbon and four, hydrogen ,: ethane,C2H6 - two carbon and six hydrogen : propane,C3H8 - three carbon and 8
  31. Using renewable energy (such as by electrolysis) or if other sources of, hydrogen ,are not available to replace the Haber Process, in amounts sufficient to supply
  32. And it behaves like an alkali metal. This type of hydrogen is known as metallic, hydrogen , Hydrogen is sometimes considered to be an alkali metal, as it, like the other
  33. But hydrogen is not counted as an alkali metal. Under typical conditions, pure, hydrogen , exists as a diatomic gas consisting of two atoms per molecule. The removal of
  34. Or side-chain that, like an alkane, consists solely of single-bonded carbon and, hydrogen ,atoms, for example a methyl or ethyl group. The simplest possible alkane (the
  35. And the size of the atom tends to dominate its acidity when sharing a bond to, hydrogen , Hydrogen sulfide,H2S,is a stronger acid than water, even though oxygen is
  36. Substantially polarized by an electric field. For this reason they do not form, hydrogen ,bonds and are insoluble in polar solvents such as water. Since the hydrogen
  37. Acid with a strong base gives a weakly basic salt,e.g. sodium fluoride from, hydrogen ,fluoride and sodium hydroxide. Weak acid/weak base equilibrium In order to lose
  38. Result from the overlap of a SP³-orbital of carbon with the 1s-orbital of a, hydrogen ,; the latter by the overlap of two SP³-orbitals on different carbon atoms. The
  39. Propane,C3H8 - three carbon and 8 hydrogen : butane,C4H10 - four carbon and 10, hydrogen , : pentane,C5H12 - five carbon and 12 hydrogen : humane,C6H14 - six carbon and
  40. Such as those found at the cores of the planets Jupiter and Saturn, hydrogen ,does become metallic, and it behaves like an alkali metal. This type of
  41. Halogenation produces a mixture of all possible isomers, indicating that all, hydrogen ,atoms are susceptible to reaction. The mixture produced, however,is not a
  42. Is the weakly acidic ammonium chloride, which is produced from the strong acid, hydrogen ,chloride and the weak base ammonia. Conversely, neutralizing a weak acid with a
  43. Methane,CH4 - one carbon and four hydrogen : ethane,C2H6 - two carbon and six, hydrogen ,: propane,C3H8 - three carbon and 8 hydrogen : butane,C4H10 - four carbon and
  44. So scarce that natural gas is used as a partial stopgap replacement, and, hydrogen , use in transportation increases, natural gas will become much more expensive.
  45. And refer to the hydrogen ion when describing acid-base reactions but the free, hydrogen ,nucleus, a proton, does not exist alone in water, it exists as the hydronium
  46. Metal, as it, like the other alkali metals, has one valence electron; however, hydrogen ,rarely acts like an alkali metal, as can be seen from the data above. In fact
  47. Electron is required to fill in the outermost shell of the hydrogen atom, so, hydrogen , can in some circumstances behave like a halogen, forming the negative hydride
  48. Angle between a given hydrogen atom attached to the front carbon and a given, hydrogen ,atom attached to the rear carbon can vary freely between 0° and 360°. This is a
  49. Gas consisting of two atoms per molecule. The removal of the single electron of, hydrogen ,requires considerably more energy than removal of the outer electron from the
  50. Natural gas is used because it is the cheapest currently available source of, hydrogen , When oil production becomes so scarce that natural gas is used as a partial

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