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user7951
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"Is there any chemical phenomenon responsible for its stickiness?" You mean compared to a supernatural one? Almost everything that matter does in the everyday world has a chemical basis. (Radioactivity, weight and movement are examples of physics which most would agree aren't "chemical".) 

Sugar is a polar organic compound. Actually, "sugar" is the name for several related polar organic compounds. "Table sugar" (in the USA) is the common name for sucrose. Sucrose can be chemically broken apart into glucose and fructose, both of which are also sugars, and are also sold commercially. The three dietary sugars are glucose, fructose, and galactose - and you'll note that sucrose isn't included although it is the most common! (Since the body naturally breaks it down into fructose and glucose, it's "included by implication"). 

The reason sugar is sticky is because of "hydrogen bonding" (H-bonding). In high school, you may have learned that there are two types of chemical solids (compounds): ionic and covalent. All chemistry is "caused" by electric charges. In ionic compounds, the charges behave without directional preference - charge density is spherically uniform while in covalent compounds charge density is confined and is usually shared between "bonded" atoms. (I am ignoring metal bonding here, which arguably is a third type of solid). Despite its name, H-bonding is not usually included when we're talking about chemical bonding (sometimes it is, usually it is not). H-bonding is weaker than the weakest covalent bond. Water is an example of a material which gets many of its physical properties because of its H-bonding. The size of rain drops, the ability of insects to walk on its surface, and its melting and boiling points all are greatly influenced by the H-bonding that naturally occurs in it. By far the most common H-bond is the one between an -OH group (part of a large molecule) and an -O- "group" (although we'd usually say O atom). Often you will see H-bonds drawn as -OH...O- or something similar. They are much stronger than the typical interactions between separate molecules (and, as I said, weaker than the bond interactions between covalently bonded atoms) (of course, these things aren't black/white yes/no questions, there is a scale of strength...) 

So, sugar! If you take a look at the structure of sucrose (see Wikipedia), you'll see that there are 8 -OH groups on each molecule and that there are 3 more O 'groups' (a total of 11 O atoms capable of forming H bonds). That's a whole lot! So in a concentrated solution of sucrose, you'll get a lot of H-bonding which acts to link the fairly small sucrose molecules into chains. In fact, one experiment you can do is to heat a concentrated solution of sugar and see if you can make strings or threads of it by putting a spoon into it and pulling it quickly out. Cotton candy is popular at fairs in the USA and is based on this (although has been improved by trial and error changes to the process and recipe). 

Plastics are polymers which exist as chains. Most glues also are polymers. Our skin is composed of polymers. As a matter of fact our skin is composed of polar polymers. And sugar, also being polar, will tend to "stick" to our skin. But not only are they polar, both are capable of H-bonding. So, you have two different chemical phenomena: concentrated sugar solutions have a cohesive strength (it sticks together) and it has an adhesive strength (to polar surfaces). These are what make it sticky. One

One thing I've not explained is what I mean by "polar". It has to do with electric charge. In the context of molecules, when the negative charge density is centered at the same point as the positive charge density, a molecule is nonpolar. When the centers don't coincide, the molecule is polar (or if the positive charge is on an entirely different atom than the negative charge AND its a whole number, then we'd call that an ionic molecule) In other words, polar molecules are molecules which have fractional separation of negative and positive charges. It is a bit more complicated than that: In CO2 there is more negative charge "on" the O atoms than on the central C atom. But because the molecule is linear (the 3 atoms fromform a straight line in space) the center of negative charge is on the central C atom, despite its being slightly positively charged. NO2 is a slightly 'bent' molecule, it's not straight so although the negative charge on both O atoms is equal, they don't "cancel out" and the molecule is polar. So, we have a "spectrum" of polarity from something like H2 which is non-polar (and no charge separation) to CO2 which is also non-polar but with charge separation to NO2 which with a central bond angle of 134.3° is polar, but only "slightly" to HCl (in the gasseousgaseous state) which is very polar (but still covalent) to H(+)Cl(-) in solutonsolution which is ionic. 

Polar molecules will interact more with other polar molecules than they will with non-polar molecules (everything else being equal). Nonpolar molecules will interact with other non-polar molecules only slightly (due to "dipole-dipole interactions"). They'd interact more with polar molecules (due to "induced dipole interactions") and once you get to polar-polar molecular interactions, you're talking significant effects on some properties. H-bonding is a very strong type of polar-polar interaction; and it is very specific to the H atom.

"Is there any chemical phenomenon responsible for its stickiness?" You mean compared to a supernatural one? Almost everything that matter does in the everyday world has a chemical basis. (Radioactivity, weight and movement are examples of physics which most would agree aren't "chemical".) Sugar is a polar organic compound. Actually, "sugar" is the name for several related polar organic compounds. "Table sugar" (in the USA) is the common name for sucrose. Sucrose can be chemically broken apart into glucose and fructose, both of which are also sugars, and are also sold commercially. The three dietary sugars are glucose, fructose, and galactose - and you'll note that sucrose isn't included although it is the most common! (Since the body naturally breaks it down into fructose and glucose, it's "included by implication"). The reason sugar is sticky is because of "hydrogen bonding" (H-bonding). In high school, you may have learned that there are two types of chemical solids (compounds): ionic and covalent. All chemistry is "caused" by electric charges. In ionic compounds, the charges behave without directional preference - charge density is spherically uniform while in covalent compounds charge density is confined and is usually shared between "bonded" atoms. (I am ignoring metal bonding here, which arguably is a third type of solid). Despite its name, H-bonding is not usually included when we're talking about chemical bonding (sometimes it is, usually it is not). H-bonding is weaker than the weakest covalent bond. Water is an example of a material which gets many of its physical properties because of its H-bonding. The size of rain drops, the ability of insects to walk on its surface, and its melting and boiling points all are greatly influenced by the H-bonding that naturally occurs in it. By far the most common H-bond is the one between an -OH group (part of a large molecule) and an -O- "group" (although we'd usually say O atom). Often you will see H-bonds drawn as -OH...O- or something similar. They are much stronger than the typical interactions between separate molecules (and, as I said, weaker than the bond interactions between covalently bonded atoms) (of course, these things aren't black/white yes/no questions, there is a scale of strength...) So, sugar! If you take a look at the structure of sucrose (see Wikipedia), you'll see that there are 8 -OH groups on each molecule and that there are 3 more O 'groups' (a total of 11 O atoms capable of forming H bonds). That's a whole lot! So in a concentrated solution of sucrose, you'll get a lot of H-bonding which acts to link the fairly small sucrose molecules into chains. In fact, one experiment you can do is to heat a concentrated solution of sugar and see if you can make strings or threads of it by putting a spoon into it and pulling it quickly out. Cotton candy is popular at fairs in the USA and is based on this (although has been improved by trial and error changes to the process and recipe). Plastics are polymers which exist as chains. Most glues also are polymers. Our skin is composed of polymers. As a matter of fact our skin is composed of polar polymers. And sugar, also being polar, will tend to "stick" to our skin. But not only are they polar, both are capable of H-bonding. So, you have two different chemical phenomena: concentrated sugar solutions have a cohesive strength (it sticks together) and it has an adhesive strength (to polar surfaces). These are what make it sticky. One thing I've not explained is what I mean by "polar". It has to do with electric charge. In the context of molecules, when the negative charge density is centered at the same point as the positive charge density, a molecule is nonpolar. When the centers don't coincide, the molecule is polar (or if the positive charge is on an entirely different atom than the negative charge AND its a whole number, then we'd call that an ionic molecule) In other words, polar molecules are molecules which have fractional separation of negative and positive charges. It is a bit more complicated than that: In CO2 there is more negative charge "on" the O atoms than on the central C atom. But because the molecule is linear (the 3 atoms from a straight line in space) the center of negative charge is on the central C atom, despite its being slightly positively charged. NO2 is a slightly 'bent' molecule, it's not straight so although the negative charge on both O atoms is equal, they don't "cancel out" and the molecule is polar. So, we have a "spectrum" of polarity from something like H2 which is non-polar (and no charge separation) to CO2 which is also non-polar but with charge separation to NO2 which with a central bond angle of 134.3° is polar, but only "slightly" to HCl (in the gasseous state) which is very polar (but still covalent) to H(+)Cl(-) in soluton which is ionic. Polar molecules will interact more with other polar molecules than they will with non-polar molecules (everything else being equal). Nonpolar molecules will interact with other non-polar molecules only slightly (due to "dipole-dipole interactions"). They'd interact more with polar molecules (due to "induced dipole interactions") and once you get to polar-polar molecular interactions, you're talking significant effects on some properties. H-bonding is a very strong type of polar-polar interaction; and it is very specific to the H atom.

"Is there any chemical phenomenon responsible for its stickiness?" You mean compared to a supernatural one? Almost everything that matter does in the everyday world has a chemical basis. (Radioactivity, weight and movement are examples of physics which most would agree aren't "chemical".) 

Sugar is a polar organic compound. Actually, "sugar" is the name for several related polar organic compounds. "Table sugar" (in the USA) is the common name for sucrose. Sucrose can be chemically broken apart into glucose and fructose, both of which are also sugars, and are also sold commercially. The three dietary sugars are glucose, fructose, and galactose - and you'll note that sucrose isn't included although it is the most common! (Since the body naturally breaks it down into fructose and glucose, it's "included by implication"). 

The reason sugar is sticky is because of "hydrogen bonding" (H-bonding). In high school, you may have learned that there are two types of chemical solids (compounds): ionic and covalent. All chemistry is "caused" by electric charges. In ionic compounds, the charges behave without directional preference - charge density is spherically uniform while in covalent compounds charge density is confined and is usually shared between "bonded" atoms. (I am ignoring metal bonding here, which arguably is a third type of solid). Despite its name, H-bonding is not usually included when we're talking about chemical bonding (sometimes it is, usually it is not). H-bonding is weaker than the weakest covalent bond. Water is an example of a material which gets many of its physical properties because of its H-bonding. The size of rain drops, the ability of insects to walk on its surface, and its melting and boiling points all are greatly influenced by the H-bonding that naturally occurs in it. By far the most common H-bond is the one between an -OH group (part of a large molecule) and an -O- "group" (although we'd usually say O atom). Often you will see H-bonds drawn as -OH...O- or something similar. They are much stronger than the typical interactions between separate molecules (and, as I said, weaker than the bond interactions between covalently bonded atoms) (of course, these things aren't black/white yes/no questions, there is a scale of strength...) 

So, sugar! If you take a look at the structure of sucrose (see Wikipedia), you'll see that there are 8 -OH groups on each molecule and that there are 3 more O 'groups' (a total of 11 O atoms capable of forming H bonds). That's a whole lot! So in a concentrated solution of sucrose, you'll get a lot of H-bonding which acts to link the fairly small sucrose molecules into chains. In fact, one experiment you can do is to heat a concentrated solution of sugar and see if you can make strings or threads of it by putting a spoon into it and pulling it quickly out. Cotton candy is popular at fairs in the USA and is based on this (although has been improved by trial and error changes to the process and recipe). 

Plastics are polymers which exist as chains. Most glues also are polymers. Our skin is composed of polymers. As a matter of fact our skin is composed of polar polymers. And sugar, also being polar, will tend to "stick" to our skin. But not only are they polar, both are capable of H-bonding. So, you have two different chemical phenomena: concentrated sugar solutions have a cohesive strength (it sticks together) and it has an adhesive strength (to polar surfaces). These are what make it sticky.

One thing I've not explained is what I mean by "polar". It has to do with electric charge. In the context of molecules, when the negative charge density is centered at the same point as the positive charge density, a molecule is nonpolar. When the centers don't coincide, the molecule is polar (or if the positive charge is on an entirely different atom than the negative charge AND its a whole number, then we'd call that an ionic molecule) In other words, polar molecules are molecules which have fractional separation of negative and positive charges. It is a bit more complicated than that: In CO2 there is more negative charge "on" the O atoms than on the central C atom. But because the molecule is linear (the 3 atoms form a straight line in space) the center of negative charge is on the central C atom, despite its being slightly positively charged. NO2 is a slightly 'bent' molecule, it's not straight so although the negative charge on both O atoms is equal, they don't "cancel out" and the molecule is polar. So, we have a "spectrum" of polarity from something like H2 which is non-polar (and no charge separation) to CO2 which is also non-polar but with charge separation to NO2 which with a central bond angle of 134.3° is polar, but only "slightly" to HCl (in the gaseous state) which is very polar (but still covalent) to H(+)Cl(-) in solution which is ionic. 

Polar molecules will interact more with other polar molecules than they will with non-polar molecules (everything else being equal). Nonpolar molecules will interact with other non-polar molecules only slightly (due to "dipole-dipole interactions"). They'd interact more with polar molecules (due to "induced dipole interactions") and once you get to polar-polar molecular interactions, you're talking significant effects on some properties. H-bonding is a very strong type of polar-polar interaction; and it is very specific to the H atom.

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Li Zhi
Li Zhi
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"Is there any chemical phenomenon responsible for its stickiness?" You mean compared to a supernatural one? Almost everything that matter does in the everyday world has a chemical basis. (Radioactivity, weight and movement are examples of physics which most would agree aren't "chemical".) Sugar is a polar organic compound. Actually, "sugar" is the name for several related polar organic compounds. "Table sugar" (in the USA) is the common name for sucrose. Sucrose can be chemically broken apart into glucose and fructose, both of which are also sugars, and are also sold commercially. The three dietary sugars are glucose, fructose, and galactose - and you'll note that sucrose isn't included although it is the most common! (Since the body naturally breaks it down into fructose and glucose, it's "included by implication"). The reason sugar is sticky is because of "hydrogen bonding" (H-bonding). In high school, you may have learned that there are two types of chemical solids (compounds): ionic and covalent. All chemistry is "caused" by electric charges. In ionic compounds, the charges behave without directional preference - charge density is spherically uniform while in covalent compounds charge density is confined and is usually shared between "bonded" atoms. (I am ignoring metal bonding here, which arguably is a third type of solid). Despite its name, H-bonding is not usually included when we're talking about chemical bonding (sometimes it is, usually it is not). H-bonding is weaker than the weakest covalent bond. Water is an example of a material which gets many of its physical properties because of its H-bonding. The size of rain drops, the ability of insects to walk on its surface, and its melting and boiling points all are greatly influenced by the H-bonding that naturally occurs in it. By far the most common H-bond is the one between an -OH group (part of a large molecule) and an -O- "group" (although we'd usually say O atom). Often you will see H-bonds drawn as -OH...O- or something similar. They are much stronger than the typical interactions between separate molecules (and, as I said, weaker than the bond interactions between covalently bonded atoms) (of course, these things aren't black/white yes/no questions, there is a scale of strength...) So, sugar! If you take a look at the structure of sucrose (see Wikipedia), you'll see that there are 8 -OH groups on each molecule and that there are 3 more O 'groups' (a total of 11 O atoms capable of forming H bonds). That's a whole lot! So in a concentrated solution of sucrose, you'll get a lot of H-bonding which acts to link the fairly small sucrose molecules into chains. In fact, one experiment you can do is to heat a concentrated solution of sugar and see if you can make strings or threads of it by putting a spoon into it and pulling it quickly out. Cotton candy is popular at fairs in the USA and is based on this (although has been improved by trial and error changes to the process and recipe). Plastics are polymers which exist as chains. Most glues also are polymers. Our skin is composed of polymers. As a matter of fact our skin is composed of polar polymers. And sugar, also being polar, will tend to "stick" to our skin. But not only are they polar, both are capable of H-bonding. So, you have two different chemical phenomena: concentrated sugar solutions have a cohesive strength (it sticks together) and it has an adhesive strength (to polar surfaces). These are what make it sticky. One thing I've not explained is what I mean by "polar". It has to do with electric charge. In the context of molecules, when the negative charge density is centered at the same point as the positive charge density, a molecule is nonpolar. When the centers don't coincide, the molecule is polar (or if the positive charge is on an entirely different atom than the negative charge AND its a whole number, then we'd call that an ionic molecule) In other words, polar molecules are molecules which have fractional separation of negative and positive charges. It is a bit more complicated than that: In CO2 there is more negative charge "on" the O atoms than on the central C atom. But because the molecule is linear (the 3 atoms from a straight line in space) the center of negative charge is on the central C atom, despite its being slightly positively charged. NO2 is a slightly 'bent' molecule, it's not straight so although the negative charge on both O atoms is equal, they don't "cancel out" and the molecule is polar. So, we have a "spectrum" of polarity from something like H2 which is non-polar (and no charge separation) to CO2 which is also non-polar but with charge separation to NO2 which with a central bond angle of 134.3° is polar, but only "slightly" to HCl (in the gasseous state) which is very polar (but still covalent) to H(+)Cl(-) in soluton which is ionic. Polar molecules will interact more with other polar molecules than they will with non-polar molecules (everything else being equal). Nonpolar molecules will interact with other non-polar molecules only slightly (due to "dipole-dipole interactions"). They'd interact more with polar molecules (due to "induced dipole interactions") and once you get to polar-polar molecular interactions, you're talking significant effects on some properties. H-bonding is a very strong type of polar-polar interaction; and it is very specific to the H atom.