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Hydrogen bonds in water are weak interactions that occur between the hydrogen atom of one molecule and the electronegative atom of another.
Review the structure of water, hydrogen bonding, and their importance in biological systems.
Water interacts differently with charged and polar substances than with nonpolar substances because of the polarity of its own molecules. Water molecules are polar, with partial positive charges on the hydrogens, a partial negative charge on the oxygen, and a bent overall structure.
The water cycle, powered by the sun, involves water moving in various forms between sources and sinks. It starts with evaporation from bodies of water, condensation into clouds, and precipitation back to the earth. This cycle also includes transpiration from plants and sublimation from ice to vapor.
A water molecule is considered polar because of electronegativity differences between the oxygen atom and the 2 hydrogen atoms. The oxygen atom "Hogs" the electrons from the covalent bond creating a partially negative side in the molecule while the other side becomes partially positive.
Practice problems on the structure of water and hydrogen bonding.
The fluid mosaic model describes the structure of cell membranes, highlighting the dynamic nature and diverse components that enable various cellular functions.
Even though molecules, proteins, viruses, and cells are all tiny, there are significant size differences between them. The diameter of a water molecule is roughly 0.28 nanometers. The diameter of the protein hemoglobin is roughly 5 nanometers. The diameter of the HIV virus is roughly 120 nanometers. A red blood cell is 6-8 micrometers.
Hydrogen bonds can form between different molecules (intermolecular hydrogen bonding) or between different parts of the same molecule (intramolecular hydrogen bonding).
Explanation of the Calvin cycle in photosynthesis, including its stages and importance in converting carbon dioxide into glucose.