Which property of water allows living things to survive in ponds covered with ice?

Which property of water allows living things to survive in ponds covered with ice?

Water is less dense as a solid than as a liquid. This means that ice is less dense than liquid water, which is why it floats. This property is important, as it keeps ponds, lakes, and oceans from freezing solid and allows life to continue to thrive under the icy surface.

Which of the following properties of water is most responsible for the fact that lakes do not freeze from the bottom up?

Which of the following properties of water is most responsible for the fact that lakes do not freeze from the bottom up? Explanation: When water freezes, its density decreases (most substances do not exhibit this property). This means that ice will float on top of a lake, rather than sink to the bottom.

What does a high surface tension mean?

Surface Tension: “The property of the surface of a liquid that allows it to resist an external force, due to the cohesive nature of its molecules.” The high surface tension helps the paper clip – with much higher density – float on the water.

Which has a higher surface tension?

water

What causes high surface tension and low vapor pressure?

Water has high surface tension because of extensive hydrogen bonding. The vapor pressure of water is low due to hydrogen bonding. Vapor pressure increases as temperature increases.

How does this property make hydrogen bonds between water molecules possible?

Water molecules forming hydrogen bonds with one another. The partial negative charge on the O of one molecule can form a hydrogen bond with the partial positive charge on the hydrogens of other molecules. Water molecules are also attracted to other polar molecules and to ions.

Which answer helps to explain how many hydrogen bonds a water molecule can form?

four hydrogen bonds

How many bonds are in h2o?

Each water molecule can form two hydrogen bonds involving their hydrogen atoms plus two further hydrogen bonds utilizing the hydrogen atoms attached to neighboring water molecules. These four hydrogen bonds optimally arrange themselves tetrahedrally around each water molecule as found in ordinary ice (see right).