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Water is less dense as a solid than as a liquid. This unusual property of water is due to hydrogen bonds. As water freezes, each molecule forms stable hydrogen bonds with its neighbors, holding them at "arm's length" and creating a three dimensional crystal.
In Ice Hydrogen bonds are stable
In liquid water hydrogen bonds constantly break and reform.
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What is hydrogen bonding and what effect does it have on water?
Hydrogen bonding is a weak electrostatic attraction between a covalently bonded H on one atom with an electronegative atom in another molecule. In water this is a bond between the H of one H2O molecule and the O of another. The effects are remarkable. Boiling point and melting point are much higher than you'd expect (compare H2S) the density of ice is lower than that of liquid water.
What characteristic of water is not a result of hydrogen bonding?
Liquid water is denser than ice. Hence, Ice floats on top of liquid water. It has a relatively high boiling point. It is a good solvent.
What property of water is NOT attributable to hydrogen bonding between water molecules A heat storage B ice formation C polarity D cohesion?
Transparency and wetness.
How do water's relative densities as a solid and a liquid from that of most other substances?
In most substances, as you solidify the product by cooling, its density rises (that is - it gets heavier). Water has a density inversion point, so ice is actually lighter than water - this is due to the way the molecules rearrange within the ice relative to the way they are packed together in the water. Hydrogen bonding in water molecules is quite strong (in the liquid phase) so the water is sort of "compacted" by this force - pulled together more tightly.
What are some properties of water that are determine by its polarity?
Water's polarity helps make it an excellent solvent. Polar substances dissolve well in water as "like dissolves like," but nonpolar substances do not dissolve as readily. Hydrogen bonding gives water its cohesion and surface tension, allowing it to cling to itself. It also greatly affects water's freezing behavior and density. Hydrogen bonds are responsible for the characteristic crystal lattice structure of ice.
What best explains why ice floats?
Hydrogen bonding makes ice less dense then liquid water
In what temperature range does density of water increases with temperature?
Density of water in solid state i.e. ice increases from 0oC to 4oC, where it has maximum density.Ice has a cage-liked structure with lots of vacant spaces in between because of extensive hydrogen bonding between the water molecules. When the temperature increases, this structure collapses as the hydrogen bonding starts to break and as such the water molecules occupy the void spaces thereby increasing the density.Beyond 4oC, the ice melts completely.
What type of bonds form water and ice?
hydrogen bonds Sincerely, #43 <3 :))
Compared to water ice has a lower?
"Density" water is heaver than ice so the ice floats on it.Added:There is a Calvin and Hobbes cartoon in which Calvin poses the question to Dad:"Why does ice float?"Dad responds:"Because it's cold. Ice wants to get warm, so it goes to the top of liquids in order to be nearer to the Sun."See the related question below for an in-depth explanation.
Why density of ice is less than water density?
Water has an unusual property that it expands as it freezes. This is due to the crystalline formation in conjunction with its hydrogen bonding. Since it expands, volume is larger. Density = mass / volume. Dividing by a larger number gives a smaller answer for the density. Water is most dense at 4 degrees Celsius.
Why are the hydrogen bonds in liquid water are less stable than in ice?
Because in water hydrogen bonding is not permanent due to random motion where as in ice it is permanent also in ice k.e.is also lower
Why does ice have a high melting point compared to other substances?
Hydrogen bonding between molecules, and bonding angle (H-O-H) of 105o
When ice melts does it expand?
yes it does. one of the consequences of water due to hydrogen bonding.
What electron behavior in compounds are found in hydrogen?
Hydrogen has the electron configuration of 1s1 meaning that Hydrogen has only one electron. Because of this, Hydrogen is a moderately reactive substance and behaves atypically both in intermolecular and atomic bonding. The most notable behaviour of Hydrogen is Hydrogen bonding. When hydrogen is bonded to a highly electronegative element, such as Fluorine in HF, the electron density is pulled away from the weak hydrogen atom, leaving the hydrogen almost completely deprived of electrons and a δ+ charge. This induces nearby atoms in other molecules to share their lone pair electrons with the hydrogen, effectively producing a bond similar to a covalent bond, however between molecules. Hydrogen bonding is the strongest intermolecular force and is present in compounds such as water, where the Hδ+ Effectively 'bonds' with the lone pairs of the oxygen atoms in neighbouring molecules, which is why water and ice show unusual properties.
What is hydrogen bonding and what effect does it have on water?
Hydrogen bonding is a weak electrostatic attraction between a covalently bonded H on one atom with an electronegative atom in another molecule. In water this is a bond between the H of one H2O molecule and the O of another. The effects are remarkable. Boiling point and melting point are much higher than you'd expect (compare H2S) the density of ice is lower than that of liquid water.
How many different shapes of snowflakes do scientists think exist?
due to strong hydrogen bonding between water as compare to ice form
Why does ice have a higher density than water?
Water is more dense because the hydrogen within the water molecule will interact with the oxygen in a different water molecule to form a "hydrogen-bond". These will occur between all the water molecules and hold them together through these bonds, making it denser. In ice the water molecules cannot move so the hydrogen bonding cannot occur to hold molecules tightly. The structure actually becomes more spaced and open, and thus less dense.
