5171213
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Mapa Mental por Bee Brittain, atualizado more than 1 year ago
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Criado por Bee Brittain
mais de 8 anos atrás
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6.4 Hydrogen Bonding
- Hydrogen Bonds
- type of permanent dipole-dipole interaction found between molecules containing:
- an electronegative atom with alone pair
of electrons, for example, oxygen,
nitrogen or fluorine.
- a hydrogen atom attached to an
electronegative atom, for example, H-O,
H-N or H-F
- an electronegative atom with alone pair
of electrons, for example, oxygen,
nitrogen or fluorine.
- type of permanent dipole-dipole interaction found between molecules containing:
- Anomalous Properties of Water
- The solid form, Ice, is less dense than the liquid form, water.
- 1) Hydrogen bonds hold
water molecules apart in
an open lattice structure
- 2) The water molecules in ice are further apart than water
- 3) Solid ice is less
dense than liquid
water and floats
- With two lone pairs on the oxygen atom and two hydrogen atoms, each water molecule can form four hydrogen bonds.
- The hydrogen bonds extend outwards, holding water molecules slightly apart and forming an open tetrahedral lattice full of holes.
- The bond angle about the hydrogen atom involved in the hydrogen bond is close to 180 degrees.
- The bond angle about the hydrogen atom involved in the hydrogen bond is close to 180 degrees.
- The hydrogen bonds extend outwards, holding water molecules slightly apart and forming an open tetrahedral lattice full of holes.
- 1) Hydrogen bonds hold
water molecules apart in
an open lattice structure
- Water has a relatively high melting point and boiling point
- As with all molecules, water has London Forces
between molecules.
- Hydrogen bonds are extra forces, over and above the London forces
- An appreciable quantity of energy is needed to break the hydrogen bonds in water, so water has much higher
melting and boiling points than would be expected from just London Forces
- When water melts, the lattice breaks and the ridged arrangement of Hydrogen bonds is broken. When water boils, the hydrogen bonds break completely
- When water melts, the lattice breaks and the ridged arrangement of Hydrogen bonds is broken. When water boils, the hydrogen bonds break completely
- An appreciable quantity of energy is needed to break the hydrogen bonds in water, so water has much higher
melting and boiling points than would be expected from just London Forces
- As with all molecules, water has London Forces
between molecules.
- The solid form, Ice, is less dense than the liquid form, water.
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