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Will a substance with a higher specific heat value likely have more or less hydrogen bonding?
Wiki User
∙ 13y ago
more because high specific heat is based on the substances hydrogen bonding
Wiki User
∙ 13y ago
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Why do hydrogen bonds matter?
Hydrogen bonds are the strongest of the intermolecular forces that hold molecules together. They are important because the presence or absence of hydrogen bonds determines many physical and chemical characteristics of the compound in question. For example, a molecule with significant hydrogen bonding will have a much higher boiling point than one with no hydrogen bonding.
Why does ethanol have higher boiling point than butane although the latter has higher relative molecular mass?
Ethanol has a higher boiling point because of chemical bonding. Ethanol is an alcohol. Specifically hydrogen bonding. Ethanol is an alcohol, Butane does not have anything except Carbon and Hydrogen. I found this on google:Hydrogen bonding in alcohols An alcohol is an organic molecule containing an -O-H group. Any molecule which has a hydrogen atom attached directly to an oxygen or a nitrogen is capable of hydrogen bonding. Such molecules will always have higher boiling points than similarly sized molecules which don't have an -O-H or an -N-H group. The hydrogen bonding makes the molecules "stickier", and more heat is necessary to separate them. Ethanol, CH3CH2-O-H, and methoxymethane, CH3-O-CH3, both have the same molecular formula, C2H6O.---- Note: If you haven't done any organic chemistry yet, don't worry about the names.----They have the same number of electrons, and a similar length to the molecule. The van der Waals attractions (both dispersion forces and dipole-dipole attractions) in each will be much the same. However, ethanol has a hydrogen atom attached directly to an oxygen - and that oxygen still has exactly the same two lone pairs as in a water molecule. Hydrogen bonding can occur between ethanol molecules, although not as effectively as in water. The hydrogen bonding is limited by the fact that there is only one hydrogen in each ethanol molecule with sufficient + charge. In methoxymethane, the lone pairs on the oxygen are still there, but the hydrogens aren't sufficiently + for hydrogen bonds to form. Except in some rather unusual cases, the hydrogen atom has to be attached directly to the very electronegative element for hydrogen bonding to occur. The boiling points of ethanol and methoxymethane show the dramatic effect that the hydrogen bonding has on the stickiness of the ethanol molecules: ethanol (with hydrogen bonding) 78.5°C methoxymethane (without hydrogen bonding) -24.8°C The hydrogen bonding in the ethanol has lifted its boiling point about 100°C.
How do you find the relative melting point of a group of substance?
You have to look at the actual structures of each substance in the group. For each individual substance, think of it being multiplied many times, until you have a little "sea" of all one type of molecule. There are three forces that are possibly at work between these identical molecules: Van Der Waals, dipole-dipole, and hydrogen bonding. (You can find definitions for these terms with an online search if you're not sure what they are.) If a substance can participate in hydrogen bonding between two of its molecules (draw a picture of the structure, and then a copy of that structure oriented in such a way that the H of an H-F, H-O, or H-N bond can line up with a non-bonding electron pair on the second molecule) then it will have strong intermolecular forces, needing a lot of energy to break, and by extension a higher melting point. Dipole-Diploe forces, in the absence of hydrogen bonding, are next in line. The lowest melting points of substances occur when there are only Van Der Waals forces at work between the molecules of a substance.
Why do substances with higher density have a higher boling and freezing point?
Um... who says they do? Lead has a significantly higher density than aluminum but a considerably lower melting point.
Why methanol boil at high temperature than dimethyl ether?
bcoz of the intermolecular hydrogen bonding in methyl alcohol the vapour pressure of the molecule equalises the atmospheric pressure at higher temperatures. there is no hydrogen bonding in dimethyl ether and hence the molecule escapes at relatively lower temperatures.
Why c2h5oh has higher boiling point?
due to intermolecular hydrogen bonding
Why is the boilig point of water is higher than that H2S AND H2SE?
hydrogen bonding
Why is the boiling point of H2O much higher than h2se?
Hydrogen bonding
Which substance having high specific heat capacity?
A common substance with a high specific heat is water. There are a few substances that have a higher heat capacity than water, though, such as lithium and ammonia.
Does hydrogen or water has high specific heat capacity?
Water has a MUCH higher specific heat than hydrogen.
Does water has a high specific heat due to the hydrogen bonding between water molecules?
Because of these slightly polar bonds water molecules need the input of greater amounts of energy to separate molecule from molecule in the rapid motion defining heat and further on to vaporization. A molecule such as methane, CH4, has no hydrogen bonding and has a low specific heat capacity by comparison.
Why do hydrogen bonds matter?
Hydrogen bonds are the strongest of the intermolecular forces that hold molecules together. They are important because the presence or absence of hydrogen bonds determines many physical and chemical characteristics of the compound in question. For example, a molecule with significant hydrogen bonding will have a much higher boiling point than one with no hydrogen bonding.
Why ethanol has high boiling point than diethyl-ether?
Ethanol has intermolecular hydrogen bonding where as diethylether does not have this kind of bonding. So BP of ethanol is higher than diethylether.
Why the specific molar conductivity of 0.01 M KOH is much higher than the specific conducivity of 0.01M KCl?
This is true because KOH has a high concentration of hydrogen ions (H+) and this increases the conductivity of KOH to be significantly higher than that of KCl. KCl has a very highly electronegative ion Cl- Hydrogen bonding occurs at sites of electronegativity which will interfere conductivity at lower concentrations of these Ions
Why does ethanol have higher boiling point than butane although the latter has higher relative molecular mass?
Ethanol has a higher boiling point because of chemical bonding. Ethanol is an alcohol. Specifically hydrogen bonding. Ethanol is an alcohol, Butane does not have anything except Carbon and Hydrogen. I found this on google:Hydrogen bonding in alcohols An alcohol is an organic molecule containing an -O-H group. Any molecule which has a hydrogen atom attached directly to an oxygen or a nitrogen is capable of hydrogen bonding. Such molecules will always have higher boiling points than similarly sized molecules which don't have an -O-H or an -N-H group. The hydrogen bonding makes the molecules "stickier", and more heat is necessary to separate them. Ethanol, CH3CH2-O-H, and methoxymethane, CH3-O-CH3, both have the same molecular formula, C2H6O.---- Note: If you haven't done any organic chemistry yet, don't worry about the names.----They have the same number of electrons, and a similar length to the molecule. The van der Waals attractions (both dispersion forces and dipole-dipole attractions) in each will be much the same. However, ethanol has a hydrogen atom attached directly to an oxygen - and that oxygen still has exactly the same two lone pairs as in a water molecule. Hydrogen bonding can occur between ethanol molecules, although not as effectively as in water. The hydrogen bonding is limited by the fact that there is only one hydrogen in each ethanol molecule with sufficient + charge. In methoxymethane, the lone pairs on the oxygen are still there, but the hydrogens aren't sufficiently + for hydrogen bonds to form. Except in some rather unusual cases, the hydrogen atom has to be attached directly to the very electronegative element for hydrogen bonding to occur. The boiling points of ethanol and methoxymethane show the dramatic effect that the hydrogen bonding has on the stickiness of the ethanol molecules: ethanol (with hydrogen bonding) 78.5°C methoxymethane (without hydrogen bonding) -24.8°C The hydrogen bonding in the ethanol has lifted its boiling point about 100°C.
Why water is unusual?
It has much higher boiling and melting points than would be expected from its molecular size. This is a result of strong hydrogen bonding. Its solid form is less dense than the liquid, because the hydrogen bonding creates a very open structure.
How do you find the relative melting point of a group of substance?
You have to look at the actual structures of each substance in the group. For each individual substance, think of it being multiplied many times, until you have a little "sea" of all one type of molecule. There are three forces that are possibly at work between these identical molecules: Van Der Waals, dipole-dipole, and hydrogen bonding. (You can find definitions for these terms with an online search if you're not sure what they are.) If a substance can participate in hydrogen bonding between two of its molecules (draw a picture of the structure, and then a copy of that structure oriented in such a way that the H of an H-F, H-O, or H-N bond can line up with a non-bonding electron pair on the second molecule) then it will have strong intermolecular forces, needing a lot of energy to break, and by extension a higher melting point. Dipole-Diploe forces, in the absence of hydrogen bonding, are next in line. The lowest melting points of substances occur when there are only Van Der Waals forces at work between the molecules of a substance.
