1. The most important effect of hydrogen bonding on the properties of water is that it is a liquid at temperature. If it were not for strong hydrogen bonding, water would be a gas at room temperature. Other molecules that are larger and heavier are gases at room temperature (such as carbon dioxide (CO2), propane (C3H8), butane (C4H10), and others). The world would be a different place if water were a gas at room temperature!
2. Water is known for being cohesive. This means that if you drip water on a table, water droplets will 'stick' to one another rather than being spread out. This is due to the hydrogen bonding between molecules. A hydrogen bond is a tenth of a covalent bond, making it the strongest common intramolecular bonding.
Why is this important? Well, a good and common answer to that is found in plants. When plants absorb water from the ground, the water molecules are actually 'pulled' up. Water is lost through the leaves and thus causing a small vacuum within the plant's xylem, a small 'tube' in the plant that carries water. The vacuum then causes the 'pulling' up of water molecules.
2. Water has an extremely high specific heat capacity. This means that it takes a lot of energy to increase the temperature of water by 1 degree compared to other chemicals. This is also due to the hydrogen bondings. As hydrogen bondings are so strong, it takes a large amount of energy to break the bonds.
This is important to evaporation, boiling points etc. Why do you think it takes so long to boil water? Because an extremely large amount of energy is needed to break bonds. Also, we sweat to cool ourselves down. Water on the surface of our skin can absorb up a lot of heat before evaporating.
Really Short answer - The hydrgen bonds create a slightly positive side and and slightly negative side that allow the water to easily stick together and break apart
, this is called cohesion.
if you've ever heard of the octet rule, then you'll understand where the single proton from a hydrogen atom will most likely bond with an oxygen atom, this would make the molecule more stable. on to the effects... Water is denser when it's liquid than when it's in the solid phase. this is because of how, when frozen, the molecules are dispersed. I hope this helped. There's a lot more to it, but I've only completed one year of chemistry, I think some of it has to do with freezing point and why its such a great solvent. Hope I helped.
water is unique because its oxygen atom has two lone pairs and two hydrogen atoms, meaning that the total number of bonds of a water molecule is up to four.
It turns plain water into hydrogen peroxide, not sure about the bonding procedure.
chemical bonding
Hydrogen bonds between the Oxygen of one molecule and the hydrogen of another :)
hydrogen bonds
The polar covalent bonds that make up the structure of water are responsible for surface tension and adhesion characteristics found in water. The bonds are also responsible for the high heat of vaporization.
Water properties are also influenced by the hydrogen bonds formrd between water molecules.
hydrogen bonds
Hydrogen bonds.
Hydrogen bonds between the Oxygen of one molecule and the hydrogen of another :)
They are electrically attract each other and form hydrogen bonds. One of the strongest intermolecular forces.
A hydrogen bond does not dissolve, but it can be broken. Water molecules form hydrogen bonds with each other. This is why water has so many unique properties, such as its high heat capacity.
hydrogen bonds
Hydrogen Bonds
The polar covalent bonds that make up the structure of water are responsible for surface tension and adhesion characteristics found in water. The bonds are also responsible for the high heat of vaporization.
No ethane (C2H6) is a hydrocarbon and hydrocarbons can't form hydrogen bonds. Only molecules containing hydrogen (H) bonded with nitrogen (N), oxygen (O) or fluorine (F) can form hydrogen bonds.
Water properties are also influenced by the hydrogen bonds formrd between water molecules.
Hydrogen Bonds
hydrogen bonds
hydrogen bonds