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  • What is the bond angle of hydrogen sulfide
    It is covalent due to the small electronegativity difference between hydrogen and sulfur.

  • why is the shape of hydrogen sulphide bent? Yahoo Answers
    The angle is 92 degrees, rather than the 105 degrees in water. Both are bent because there are four electron pairs, two of which are bonding, and two are lone

  • Why bond angle of water is more than hydrozen sulphide?
    In H2O with all the smaller sized O-atom on the opposite, this is the situation therefore the bonds are usually forced further separate to reduce energy. hydrogen sulphide physical properties.

  • Predicted bond angles
    This small difference between the predicted angle and the observed angle can be explained by proposing that the unshared pair of electrons on nitrogen repels the adjacent bonding pairs more strongly than the bonding pairs repel each other.

  • VSEPR - Nonideal Bond Angles
    The experimental HOH bond angle is only slightly smaller, but the effect is noticable.

  • How to calculate bond angle of simple molecules quantitatively?
    This is because the entire subject of predicting bond angles is a lot more tricky than it was displayed to you. Take phosphane and hydrogen sulphide, the heavy analogues to ammonia and water.

  • Why does H2S have a smaller bond angle than H2O? Forum
    The bond pair-bond pair is smaller in magnitude, still the bond pair-bond pair repulsion (steric effect) between the hydrogen in water is bigger than in hydrogen sulfide because oxygen is smaller.

  • Hydrogen bond - Wikipedia, the free encyclopedia
    A hydrogen bond is the electrostatic attraction between polar groups that occurs when a hydrogen (H) atom bound to a highly electronegative atom such as nitrogen (N), oxygen (O) or fluorine (F) experiences attraction to some other nearby highly electronegative atom.

  • Hydrogen sulphide - MOTM 2008 - HTML-only version
    The dipole moment of hydrogen sulphide is 0.97 Debye, less than that of H2O (1.84 D), meaning that it is a less polar molecule. This is due to the smaller

  • The angle between the oxygen-hydrogen bonds in water
    Generally, more lone pairs means a stronger "crowding" effect, and bond angles that deviate further from ideal values: The angle between the oxygen-hydrogen bonds in water is even smaller than the ideal value, because there are two lone pairs squeezing the bonding groups together.

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