- Helium (He, element 2) – used in balloons, because it is lighter than air
- Carbon (C, element 6) – one of the key elements in living things
- Nitrogen (N, element 7) – makes up 78% of the atmosphere
- Oxygen (O, element 8) – makes up 21% of the atmosphere
- Aluminium (Al, element 13) – a light metal used to make saucepans and aeroplanes
- Silicon (Si, element 14) – used to make electronics
- Phosphorus (P, element 15) – used in elemental form on the side of matchboxes
- Sulfur (S, element 16) – a widely used element which occurs naturally in elemental form
- Titanium (Ti, element 22) – a light, strong metal
- Iron (Fe, element 26) – the most widely used metal (mixed with other elements it becomes steel)
- Copper (Cu, element 29) – a metal that has been used for about 10,000 years, named after the island of Cyprus
- Zinc (Zn, element 30) – used in batteries and to prevent corrosion
- Silver (Ag, element 47) – widely used in jewellery since ancient times (the symbol is from the Latin argentum)
- Tin (Sn, element 50) – about 5,000 years ago, tin (Latin stannum) was mixed with copper to produce bronze
- Iodine (I, element 53) – dissolved in alcohol, it is used as a disinfectant
- Gold (Au, element 79) – widely used in jewellery since ancient times (the symbol is from the Latin aurum)
Our previous kitchen chemistry post discussed soap. Soap consists of sodium salts (or potassium salts) of fatty acids. For example, sodium stearate soap consists of sodium (Na+) and stearate C17H35COO−) ions:
These ions do their soapy job because the charged oxygen end of the molecule is attracted to water (since the hydrogen side of a water molecule has a slight positive charge). The long hydrocarbon tail, on the other hand, is attracted to oil and grease. Mixing soap and water with oil or grease therefore produces little grease droplets surrounded by many, many stearate (or other fatty acid) ions, with their tails embedded in the grease droplet, and their oxygen heads poking out into the water. I’ve only had the patience to draw eight for this droplet:
Because these little droplets are surrounded by negative charges (on the oxygen atoms), the droplets repel each other. This means the droplets stay separate from each other, and cannot combine into larger oily blobs. Because the negatively charged oxygen atoms are attracted to water molecules, the droplets also remain dispersed within the water (so that they can later be rinsed away). In fact, what we have here is an emulsion (or sol) of oil or grease in water, stabilised by the soap. Recall the image with which we began this post series:
Other kinds of emulsion will likewise need some kind of molecule that keeps the droplets separate – usually also a molecule with a distinct head and tail. In mayonnaise, for example, the emulsion of oil in water is stabilised by phospholipid molecules from egg yolks. These molecules also have a “head” attracted to water and a “tail” attracted to oil.
This post brings our kitchen chemistry series to a close, at least for now.
Our previous kitchen chemistry post discussed fats and oils, which are “triple esters” of glycerol:
Apart from their role in diet, fats are also used to produce soap:
The soap-making process involves reacting fats with strongly alkaline substances, such as lye (sodium hydroxide, NaOH). This can be done at home, but since lye is dangerous, soap-making is not appropriate for children (see these precautions: 1, 2, 3).
In solution, the lye exists as sodium (Na+) and hydroxide (OH−) ions (indeed, the presence of hydroxide ions is what “alkaline” means). The hydroxide ions react with the fat to free the glycerol:
Fatty acid ions (such as stearate ions, C17H35COO−) are also produced:
Since the sodium ions from the lye still exist, soap is basically sodium stearate, sodium palmitate, or something similar. Because it is the result of reacting a very strongly alkaline substance (sodium hydroxide) with very weak acids (fatty acids), soap itself is also alkaline. This alkaline nature can be harsh on the skin, and especially on the hair. Shampoos are therefore usually made from synthetic detergents, and formulated to be mildly acidic (with a pH between 5 and 7).
Another problem with soap is that it reacts with dissolved calcium, iron, or magnesium ions in hard water, giving an insoluble soap scum of compounds such as magnesium stearate. This can be demonstrated at home by mixing soap solution with a solution of epsom salts (see here or here).
Our previous kitchen chemistry post discussed esters. Fats and oils (triglycerides) are an important special case of esters. The alcohol in triglycerides is glycerol, a “triple alcohol” with three OH groups:
The glycerol combines with “fatty acids” (like the one on the right) which resemble acetic acid (left), but with a much longer hydrocarbon chain hanging off the COOH group:
The resulting triglyceride esters have three COO groups:
Fatty acids have important dietary implications, and they can be classified in dietary terms, but the most common classifications are chemical. The three main chemical classifications all refer to the presence of carbon-carbon double bonds:
One important classification is in terms of the number of carbon-carbon double bonds:
- Saturated fatty acids have no carbon-carbon double bonds (they are “saturated” in the sense of containing as much hydrogen as possible). Fats made from saturated fatty acids (“saturated fats”) tend to be solid at room temperature, because the straight-line molecules stick to each other. Saturated fats are usually of animal origin (although coconut oil and palm oil are also mostly saturated).
- Monounsaturated fatty acids have exactly one carbon-carbon double bond per molecule. Oleic acid (in e.g. olive oil) is an example.
- Polyunsaturated fatty acids have two or more carbon-carbon double bonds per molecule. Linoleic acid (in e.g. sunflower oil) is an example.
The position of carbon-carbon double bonds is also significant. A common classification counts the position of the first double bond, starting from the “omega” end of the molecule (the end furthest from the oxygen atoms). For example, there are omega-3, omega-6, and omega-9 fatty acids:
Finally, the orientation of double bonds is very important. In cis fatty acids, there are two hydrogen atoms on the same side of the double bond, giving a molecule with a “kink.” In trans fatty acids, the two hydrogen atoms are on the opposite sides of the double bond, giving a straight-line molecule (trans fats are usually synthetic, resulting from the partial hydrogenation of vegetable oils). Since the straight-line molecules tend to stick together, “trans fats” (made from trans fatty acids) tend to be solid at room temperature, while “cis fats” (made from cis fatty acids) tend to be liquid – that is, oils (such as olive oil) rather than fats:
Fatty acids can also be classified in dietary terms. The body needs fatty acids, but can manufacture most of them itself. Essential fatty acids are fatty acids that must be included in the diet. Both ALA and linoleic acid (found in vegetable oils) are essential. Adult men need about 13 grams of linoleic acid and 1.3 grams of ALA per day. Some omega-3 fatty acids from oily fish should also be included in the diet.
In contrast, trans fats are particularly unhealthy, and should be eliminated from the diet completely. This can be difficult in the USA, since pre-packaged foods there often contain trans fats (because of their long shelf life). Monounsaturated and polyunsaturated oils are also preferable to solid saturated fats.
Our previous kitchen chemistry post discussed acids, particularly the acetic acid in vinegar (and its reaction with sodium bicarbonate):
Acids like acetic acid, with a structure that looks like X–COOH, are also important because they react with alcohols (with a structure Y–OH) to form compounds called esters. The reaction is X–COOH + Y–OH → X–COO–Y + H2O. For example:
Industrially, strong acids are often used to make this reaction happen, but biologically, enzymes do the job. The combination of acetic acid and ethanol is ethyl acetate (used in some nail polish removers), and the image below also shows isoamyl acetate and geranyl acetate. Each ester has the same X–COO–Y structure:
Esters have a “fruity” smell, and indeed the odour of fruit is largely a result of a mix of various esters (go on, sniff some fruit, and celebrate the complex odours that you smell!). Synthetic fruit flavours likewise use esters, but typically in a simpler mix that never smells quite like the real thing.
James Kennedy has produced this wonderful infographic of esters and their smells (click on the thumbnail to zoom):
In previous kitchen chemistry posts, we discussed the fermentation processes which produce lactic acid and alcohol. A different fermentation process turns alcohol (at about wine strength) into vinegar (or, more precisely, into acetic acid). However, this process requires oxygen (C2H5OH + O2 → CH3COOH + H2O + energy):
This process usually takes place via a bacterial culture called “mother of vinegar” (photo below by “Zinnmann”), and producing gourmet vinegar by fermentation is something that can be done at home (see here, here, here, and here). It is important to remember that (unlike the bacteria producing yoghurt and wine), the “mother of vinegar” culture requires oxygen.
The acetic acid in vinegar is an acid, though not a strong one. Being an acid means that it splits into positively charged hydrogen ions and negatively charged acetate ions. Hydrogen ions are hydrogen atoms without electrons, usually written H+ (although in practice they hitch a ride with water molecules). As a reaction, CH3COOH → CH3COO− + H+:
The presence of hydrogen ions is the sign of an acid, and the stronger the acid, the more hydrogen ions. The strength of an acid is measured by the pH value, where 7 is neutral, 6 is a weak acid, and 1 is a very strong acid (numbers above 7 indicate alkaline substances). Indicator paper (photo below) is often used to determine the pH of a liquid:
However, an extract of red cabbage also does the job (photo below by “Supermartl” – acids with pH 1, 3, and 5 in the tubes on the left; neutral water with pH 7 in the fourth tube; and alkaline solutions on the right):
A common kitchen reaction is to mix vinegar with baking soda (sodium bicarbonate, NaHCO3), causing the bicarbonate to break up into carbon dioxide gas and water (photo by Kate Ter Haar):
The reaction is H+ + NaHCO3 → Na+ + CO2 + H2O:
Any other acid (citric acid, for example) would also do the job, of course, since hydrogen ions are doing the work. Sodium ions (sodium atoms with an electron missing, Na+) are left over, together with acetate ions from the vinegar, and these form sodium acetate (also the subject of a home experiment). Another common home experiment with vinegar is dissolving the shell of an egg.
My recent series of kitchen chemistry posts has included:
- A new post series (Introduction)
- Aerosols and explosions
- Burning propane
- Ethylene and ripening fruit
- Melting and boiling
- Carbohydrates and metabolism
- Metabolism and fermentation
As a brief change of pace, here are three books that might interest parents teaching children about science (links go to my reviews):
Under the Sea-Wind by Rachel Carson – a classic of nature-writing, written in 1941
The Elements by Theodore Gray – a beautifully illustrated picture-book on the elements, and a must-have reference
The Field Guide to Natural Phenomena [Wonders] by Keith Heidorn and Ian Whitelaw – a great book to keep in the family vehicle
More kitchen chemistry posts in a week or so…