Physical and Chemical Properties of Water
Physical
Water is the most cohesive non-metallic liquid. Hydrogen has a positive charge and Oxygen has a negative charge, so they attract each other and form a bond. Capillary action happens because of waters cohesiveness and stickiness. Capillary action occurs when the adhesion of water to the sides of the vessel it is in are stronger than the forces between the molecules. Another physical property of water is its color, water is actually not colorless, despite popular belief, but is actually slightly blue tinted. Waters color comes from its molecules absorbing the red end of the spectrum of light.
Chemical
Water acts as an insulator when it dissolves substances. If water holds a large amount of solutes
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The hydrogen and oxygen atoms share electrons, but the oxygen has more of the electrons than the hydrogens. Oxygen has more electrons, so it has a slightly negative charge, and hydrogen has less electrons, so it has slightly positive charge.
Water Molecules Geometric Shape and its Effects on Water Properties
Waters hydrogen and oxygen bond is on an angle of 104.5o, so the molecule is bent. The bent geometric shape and the increase of electrons on the oxygen side and the lack of electrons of the hydrogen side make water have very unique properties.
Water is a Universal Solvent
Water can dissolve more substances than any other liquid, which is why it is known as the universal solvent. Water is the universal solvent because of its physical and chemical properties. The polarity of a water molecule, one side being positive and the other being negative, allows many different molecules to attract to either the positive or negative side. The strong attraction makes water a great solvent.
The High Boiling Point of Water in its Molecular
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The intermolecular forces between water molecules cause surface tension. Molecules on the surface of a liquid are attracted to the molecules inside and to each other. Molecules inside the liquid have no force of attraction because other molecules surround them.
Water’s Phase Change and the Specific Properties of Each Phase
Water has the very unique physical property of being the only natural substance found as a solid, liquid, or gas. To change water from one phase to another you must have a great amount of energy. Water at or below 0oC is a solid (ice). Water at 0oC or above is a liquid. Water at 100oC is a gas (water vapor).
Gas
Water vapor is compressible, expandable, and takes up a lot more space than the other phases. It is free moving and has no definite shape or volume.
Liquid
Liquid water is not as easily expanded as gases. It will take the shape of the container it is put in and the motion of the particles is more restricted than those in gases, but less than those in solids.
Solid
Solid water is hard and less dense than its liquid form, which is rare. The particles do not change shape or expand/contract with the container it is put
In this lab, lab 4.3 Comparing the Concentrations of Saturated Solutions, we set out to find and compare the solubilities of two solids in water. In addition, we tested if solubility is a characteristic property of a solid in a given liquid. This lab allowed us to test and use a reliable way to measure the solubility of a solid. This lab can be replicated for any solid with the same procedure, thus it gives us a method to calculate solubility. The two solids we tested in this experiment were NaCl (Sodium Chloride) and NaNO3 (Sodium Nitrate).
...ns. This is related to Gay –Lussac’s Law. This is because temperature is the same thing as kinetic energy, and as the energy rises, the particles within the substance start to rapidly collide with one another, and they exert increased pressure. This law is written out as: .
Solubility should not be confused with the ability to dissolve a substance.The solution might occur not just because of dissolution, but of chemical reaction.For most solids dissolved in liquid water, the solubility increases up to 100 degrees celsius.Solubility is commonly expressed as a concentration.The solubility of a substance is determined by using water, and mixing it with the solute.
The reason why the gummy bear expanded and swelled in water is because of diffusion and going through osmosis. The molecules did diffusion by going from high concentration (the water) to the low concentration (the gummy bear). The diffusion of the water molecules went through a selectively permeable membrane to perform osmosis. By performing diffusion and osmosis, the molecules were at an equilibrium, which is when the concentration of molecules are equal on either side of the selectively permeable membrane. Although the membrane lets certain molecules through, some larger molecules cannot pass which is how basic living things perform life processes such as transporting water in a
The answer to why this works can be found in the physics of crystallization. To form a crystal you need something that the crystals can grow around a, nucleus of regularly arranged atoms (Science in school). Crystallization occurs most often when a liquid touches a solid surface or when the liquid contains crystalline impurities. It is kind of like the liquid copies the ordered structure of the solid. This is also know as heterogenous nucleation. In the liquid state, the neighboring atoms touch each other as if they were a solid, the single atoms move around making the perfect regular pattern of a crystal (Science In School). The density of a liquid is not so different from the density of a solid.
Freezing is a big part of this experiment. When liquids freeze it becomes ice, the molecules begin to form a crystal lattice, which pushes them apart. However, when a liquid is frozen it has taken up to 9% more room than it did when it was a liquid. Another word for freezing is solidifying. But, the purity of a compound can influence at when the liquid to solid change takes place. Most substances freeze at the exact same temperature that they melt. But did you know that hot water freezes faster than cold water? As the water warms up it becomes less dense, the hydrogen bonds stretch and the molecules move farther apart when these hydrogen bonds stretch they allow the covalent bonds to shrink and release their energy. This is equivalent to cooling. So, hot
from solid to liquid, liquid to gas and vice versa. Phase changes arexreversible, and an equilibrium exists between phases atxcertain conditions. For example, the liquid-solid equlibriumxpoint for water is at 1 atm and under those conditions, an ice cubexfloating in a glassxof water would be constantly undergoing phase changes (some of the ice is absorbing heat and meltingxand some of the water isxreleasing heat and freezing), but the relative proportion of solid to liquid remains the same.
You are walking on the street by an auto repair shop and see a puddle of water. but it's not just water. There is some sort of black liquid in the water. You look around to find out what it might be. You see a bucket of oil. You obviously think that someone must have spilt oil. Oil and the water don't seem to mix. It might be a little confusing now but it's just a thing called density. A lot of people have no idea why helium balloons float or why oil floats on water. Well if you're one of those people then you are in luck, so read on to find out why.
When in solution, the hydronium and chloride ions formed will be partially surrounded by water molecules via ion-dipole bonds, an electrostatic force of attraction that exists between charges in the ions and the partial charges in the water molecules. Water molecules surrounding ions is called hydration.
Introduction: A phase change is a result from the kinetic energy (heat) either decreasing or increasing to change the state of matter (i.e. water, liquid, or gas.) Thus saying, freezing is the phase change from a liquid to a solid which results from less kinetic energy/heat. Also, melting is the phase change from a solid to a liquid which results from adding kinetic energy/heat. So, the freezing and melting point of something is the temperature at which these phase changes occur. Therefore, a phase change will occur when a vial of 10 mL of water is placed into a cup of crushed ice mixed with four spoonfuls with 5 mL of sodium chloride for 30 minutes. If 10 mL of water is placed in an ice bath, it will then freeze at 5 degrees Celsius because the kinetic energy will leave quicker with the ice involved. The purpose of this lab is to observe what temperature the water must be to undergo a phase change.
When a liquid phase and dry granular material are added to each other, then different forms of liquid distribution can be noted:
The water molecule is a very small one but because of its unique properties it behaves like
The Biological Importance of Water as a Solvent and as a Medium for Living Organisms
Capillary action can only occur when the adhesive forces are stronger than the cohesive forces, which creates surface tension in liquid. The kinetic energy produced when the liquid is heated, allows the attractive forces between the molecules to weaken and this causes them to move past each other more freely. This results in the liquid flowing more easily. Therefore temperature increases capillary action and capillary flow because of the decrease in cohesive force. The intermolecular forces between the molecules are less packed due to the increase in temperature and the surface tension in the liquid will decrease as the temperature increases and this will help the flow of the liquid through the capillary tube.
Water is an essential part of life. It is always available and inexpensive. Water is nontoxic and do not give rise to the toxic products. It has a very high heat absorption capability due to the high heat of vaporization and a high specific heat for both liquid and gas phases. The heat absorption of water is the same as when the sponges absorb water. The longer the water is exposed to the heat source, the more the heat that the water absorbs. The heat of vaporization is the quantity of heat that must be absorb if the certain quantity of liquid is vaporized at the constant temperature while the specific heat is the amount of heat required to change the substance by one degree of temperature.