2.
“The properties of materials”
Ionic, Covalent and Metallic Bonds
SOLUBILITY IN WATER OR ACETONE DEPENDING ON THE TIPE OF BOND
Our data:
MG (metalic) is not soluble in water or acetone
Our data:
Calcium chloride anhydrous (ionic) is soluble in water but it is not soluble in acetone.
1 naphthol (organic) is soluble in water but it is not soluble in acetone.
IONIC BOND:
Ionic bonds are soluble in water because:
Water is what is described as a polar solvent. That means it has a positive end and a negative end. The water molecule is shaped like wide a "V", with the oxygen at the point. The point of the "V" is the negative end and the arms with the hydrogens on them are the positive end.
When you put the ionic solid in water, the water molecules surround the molecules and align the positive ends with the negative ions and the negative ends with the positive ions. This gives enough energy to separate the ionic bond because it has been replaced with a number of other bonds with ionic character.
Ionic bonds are not soluble in acetone because:
Acetone is not polar and ionic bonds are only soluble in polar solvents. In organic compounds (as in acetone) there is no hydrogen bonding no surrounding of different charges and ultimately no solubility.
COVALENT BONDS:
Dissolving in water:
There’s a saying that says: ‘Like dissolves like’ this means that compounds can be dissolve in other compounds, this means that they have some of the same properties. That’s what we can call, ‘particularly polarity’. Many covalent compounds don’t dissolve in water, but others yes.
Water is a polar solvent, and most covalent compounds are nonpolar, so the won’t dissolve because they don’t have non of the same characteristics.
Covalent bonds are not soluble in acetone because:
Acetone is a covalent compound. So, covalent bonds could easily dissolve. They have the same properties.
METALLIC BONDS:
Metallic bonds are not soluble in water because:
They are not soluble in water for this reasons:
They are held together by strong metallic bonds and so no solvent to solute attractions could be stronger than these, so these substances are insoluble also they don’t have the necessary intermolecular forces (namely hydrogen bonds) that are present in water.
Metallic bonds are not soluble in acetone because:
It’s very difficult to break the metallic bonds because there are a lot of attraction between the electrons.
PROPERTIES OF METALLIC BONDING:
PROPERTIES OF IONIC AND COVALENT BONDING:
WHY DO COVALENT BONDS NOT CONDUCT ELECTRICITY?
Conditions for conducting electricity is to have free electrons, that can move throughout the structure and carry charge. In covalent compounds, there are no free electrons (electrons are shared) so covalent compounds do not conduct electricity.
WHY DO METALLIC BONDS CONDUCT ELECTRICITY?
Metallic bonds conduct electricity because they have have unfilled space in the valence energy band. They also conduct electricity because they are soft and with a low melting point, and this contributes with it to react - (Also helps the reaction.)
WHY DO METALS HAVE SUCH HIGH BOILING POINTS?
Metals have such as high boiling points because they have metallic bonding where there are delocalised electrons and extend over the metal atoms. There are strong forces of attraction between these electrons and the positive nucleus of the atom, which are relatively difficult to overcome and this explains the high melting points.
WHY DO IONIC COMPOUNDS HAVE SUCH HIGH BOILING POINTS?
Ionic compounds form very strong bonds, and the energy required to break these bonds is much higher than seen in most other bonds. The energy required for an ionic solid to melt (temperature at melting point) is therefore high, and even higher for the boiling point of course.
Conductivity of a solid is due to localized electrons - which ionic compounds generally do not possess and therefor do not convey an electric current efficiently if at all.
Poned la tabla que dio Mr. Canning.
ResponderEliminarWhere is your table of results? Most of the explanations are good but one or two are incorrect. Always try to include an introduction to the page which explains what the page is about and why we are doing it. (The index on your first page was good.)
ResponderEliminar