Length of hydrocarbon chain increases ---> BP increases Hydrogen bonding increases-----> BP increases Hydrocarbon branching increase ----> BP decreases Halogen size increases ----> BP increases Molecular weight increases ----> BP increases Dipole moment increases -----> BP increases
Strong bounds raise boiling point temperatures. The thermal energy is necessary to break these bonds for boiling to occur.
Simple molecular structures like H2O and CO2 have the following properties: 1) Physical state: usually liquids and gases at room temperature due to weak intermolecular forces 2) Melting and boiling points: low (below 2000 C) melting and boiling points due to weak intermolecular forces 3) Electrical conductivity: cannot conduct electricity because there are no free electrons 4) Solubility: insoluble in water, but soluble in organic substances such as petrol Macromolecular structures such as diamond and SiO2 have the following properties: 1) Physical state: hard solids at room temperature due to the many strong covalent bonds holding the atoms together 2) Melting and boiling points: high melting and boiling points due to the many strong covalent bonds that must be broken before the substance can change state 3) Electrical conductivity: cannot conduct electricity because there are no free electrons 4) Solubility: insoluble
No. "A lot of energy is needed to separate the atoms in diamond. This is because covalent bonds are strong, and diamond contains very many covalent bonds. This makes diamond's melting point and boiling point very high. There are no free electrons or ions in diamond, so it does not conduct electricity"(BBC).
No. Water stays on a penny because of its cohesiveness due to water's strong intermolecular forces. These forces are due to its shape and properties as a polar molecule that is able to form Hydrogen bonds. The effect of the hydrogen bonds on a molecule this relatively small is very significant.
Strong hydrogen bonds as the Oxygen is really electronegative and the hydrogen is really unelectronegative. The hydrogen bonds to the oxygen of another molecule.
hydrogen bonds
When the water freezes, the molecules within it start to expand. When the water boils, hydrogen bonding allows for a higher boiling point.
If you have a ond that is connected to many other bond,s then obviously it will hae ahigher boiling, and lower melting point. It will aslo be hard
Crystalline structure at room temperature High melting and boiling points Exist as solids due to strong intermolecular force of attraction
color, size, shape, melting pint, boiling point
- covalent bonds involve electrons sharing- covalent bond is not so strong as ionic bond
i think it's because there are strong covalent bonds needed to be broken.
Because the metallic bonds between their particles are very strong.
madd strong bonds, yo
Compared to ionic compounds, covalent compounds have relatively low melting and boiling points because covalent bonds are not as strong as ionic bonds, and it is the bonds which hold materials together in the solid, or more solid phases.
The attraction forces or the attraction between the bonds is relatively high as opposed to H2O or water which the bonds aren't as strong giving it a relatively low boiling point (: I feel like that helped :D
These are melting point, boiling point, hardness.
Due to the fact that they have metallic bonds. This is the attraction between the delocalised( or free) electrons and positive ions and are strong so require a lot of energy to break (heat). So they can withstand a lot of heat before the bond starts to break and metals being to melt.