Update: Pictures are working!
There are a few basic chemistry concepts that are essential to understand. For starters, understanding what an atom is and its basic properties.
Atoms are the building block of all matter. They have a positive nucleus, with positive protons, and neutral neutrons. In a large area surrounding the nucleus, is the electron cloud, made of negatively charged electrons.
An atom in its elemental state is always neutral.
When an element has a charge, it is because it has an unequal number of protons an electrons, making it an ion. Sometimes an element’s nucleus has an unequal number of neutrons and protons, making it an isotope. Carbon-14, for example, has 8 neutrons, instead of the 6 that Carbon-12 has. Carbon-14 is also a radioisotope, meaning it emits particles and decays at a rate called a half-life, making it useful for fossil dating. Along with that, radioactive carbon can be used as a tracer. This means it is incorporated in CO2 molecules and used to track metabolic pathways.
The location of the electron affects how the atom will react with other elements. When electrons are in the lowest available energy level, they are in the ground state. When they absorb energy, they move to a higher energy level, entering the excited state. For instance, when chlorophyll absorbs light energy, electrons within it are boosted to higher energy levels. This provides the energy necessary to produce sugar when they return to their ground state level as they release the energy they absorbed.
Elements bond when two nuclei are attracted to each other. Energy is released when a bond is formed. All atoms want to either get rid of all their electrons on their outer shell or fill their outer shell with 8 (or in hydrogen’s case, 2) electrons, which makes them stable. There are 3 kinds of bonds, but for biochemistry, Ionic and covalent bonds are what is relevant.
Ionic bonds form ions (hence the name.) They occur when electrons are transferred. The atom that gains electrons becomes a negatively charged anion. The atom that loses electrons becomes a positively charged cation.
Covalent bonds are made when electrons are shared. This occurs when the two atoms have electronegativities that are closer together than in an ionic bond. Electronegativity is the tendency of an atom to pull electrons towards it. These bonds can be polar if the electronegativity is high enough. A polar molecule is a molecule with a partial charge. For example, water is a polar molecule, as oxygen is extremely electronegative, and water is partially electronegative.
Hydrogen bonding is a specific kind of intermolecular force that is essential to life. It is what keeps the 2 strands of DNA bonded together, and gives water its unique characteristics. Since oxygen has a partial negative charge, and hydrogen has a partial positive charge, they are naturally drawn to each other.
Hydrophobic vs Hydrophilic
Polar molecules are hydrophilic. This is because they are attracted to the partially charged ends of water. Hydrophilic means they are attracted to water. (Not in that way… sick) NaCl or table salt is hydrophilic. This is why salt dissolves in water.
Non-polar molecules are hydrophobic. This means they are repelled by water. (They’re filthy water haters.) Lipids are hydrophobic, which is why fats and oils do not dissolve in water.
The cell membrane is a phospholipid bilayer, only allowing nonpolar substances to dissolve through it. Large polar molecules have to use specific hydrophilic channels.
Water is a unique molecule, and without its unique properties, life on earth would not exist as it does, or even at all.
Water has a high specific heat: Because hydrogen bonds are so strong, it requires a lot of heat energy to break them. This is why large bodies of water remain the same temperature, and why coastal cities have a consistent temperature because the water absorbs all the heat energy before it can warm up.
Water has a high heat of vaporisation: A large amount of energy is needed for water to vaporise, which is why sweating is such an effective cooling method.
Water has high adhesion properties: Adhesion is when one substance clings to another. Adhesion causes capillary action, which occurs in the xylem of plants, and is used to bring water up from the roots without expending energy.
Water is a universal solvent: Due to its high polarity, water makes an excellent solvent.
Water is extremely cohesive: Molecules of water tend to stick to each other. This is observed in surface tension and allows for small insects to run across the surface of the water. Cohesion is also necessary to bring water up from the roots, by transpirational-pull cohesion tension.
Ice is less dense than water: Instead of freezing all the way through, ice crystallises, leaving large amounts of space, causing ice to float. This is essential for the survival of marine life during the winter, as they can live beneath the ice.
pH is calculated by taking the -log of the chance of finding hydronium (H30+) ions within a certain amount of water. Hydronium is made in rare circumstances, where a hydrogen ion breaks off from a water molecule. Normally, there is a 1 in 10 million chance of there being a hydronium ion. This is the equivalent of 1x10^-7. The -log of this number is 7, the neutral pH.
Any pH below 7 is acidic. Any pH above 7 is basic. Stomach acid has a pH of 2, while bleach has a pH of 11. Human blood has a pH of around 7.4
Most living cells need to have an internal environment with a pH of around 7. Buffers exist to regulate pH by either absorbing excess hydrogen ions or donating missing hydrogen ions. In human blood, the bicarbonate ion (HCO3) is essential.
There are 4 types of macromolecules: carbohydrates, lipids, proteins, and nucleic acids.
Carbohydrates are made of carbon, hydrogen, and oxygen. They supply quick and easy energy. 1 gram of all carbohydrates will release 4 calories of energy. In our diet, they can be found almost everywhere in foods such as rice, pasta, bread, cookies, etc.
There are 3 kinds of carbohydrates: monosaccharides, disaccharides, and polysaccharides.
All monosaccharides have a chemical formula of C6H12O6. It is the placement of the carbon, oxygen, and hydrogen that determines its properties. Glucose, fructose, and galactose are all examples. They are isomers, meaning they have the same chemical formula, but a different structure.
When 2 monosaccharides join together, they create disaccharides. They all have the chemical formula C12H22O11. Dehydration synthesis is the process that creates them. This process releases 1 molecule of water, hence the name. Lactose, maltose, and sucrose are all examples.
Hydrolysis is the exact opposite of dehydration synthesis. It is used during digestion. One molecule of water is used to breakdown polymers into monomers.
Polysaccharides
Polysaccharides are long polymers of carbohydrates. Cellulose (plant cell wall), chitin (exoskeleton, fungi cell wall), glycogen (how animals store carbohydrates) and starch (how plants store carbohydrates) are all examples.
Lipids include fats, oils, and waxes. Most contain 1 glycerol and 3 fatty acids. Glycerol is alcohol.
Fatty acids are the building blocks of lipids and are hydrocarbon chains with carboxyl groups at the end. There are 2 varieties; saturated and unsaturated. (3 if you count trans-fats when extra hydrogen is added to the fat to make the lipid solid)
Saturated fats are solid at room temperature, and are famously unhealthy as they are linked to heart disease.
Unsaturated fats are liquid at room temperature and are good dietary fats.
Lipids store much more energy than carbohydrates. 1 gram of any lipid will release 9 calories of heat per gram. They can be structural, as in the phospholipids of the cell membrane, or they can be hormones.
Proteins are polymers of amino acids linked together by peptide bonds.
Amino acids are identifiable by their carboxyl group, amine group, and variable R, attached to a central carbon atom.
Proteins are complex and perform a vast array of duties, such as growth and repair, being enzymes, membrane channels, and hormones.
1 gram of protein releases 4 calories of heat.
Proteins contain the elements C H O N P S
There are only 20 amino acids coding for the thousands of proteins in the human body.
There are 4 levels to the structure of a protein.
The primary structure results from the sequence of amino acids making up the polypeptide
The secondary structure results from hydrogen bonding within the molecule. This causes a helical structure
The tertiary structure is an intricate 3-dimensional shape or conformation of a protein and most directly decides the function of the protein. Enzymes denature in high temperatures or in the wrong pH because the tertiary structure is compromised.
The quaternary structure is only found in proteins that have more than 1 polypeptide chain, such as in haemoglobin.
Enzymes are large proteins
Enzymes lower the energy of activation, speeding up the reaction, as it lowers the amount of energy needed to start the reaction.
The chemical an enzyme works on is known as a substrate
Enzymes are specifically designed for specific substrates. For example, lactase only works on lactose. Notice the naming pattern for enzymes and their substrates.
The induced fit model is an explanation for how they work. When the substrate enters the active site, it induces the enzyme to change its shape to fit the substrate.
Enzymes can be reused as they do not degrade during a reaction
Enzymes are assisted by cofactors (minerals) or coenzymes (vitamins)
Prions are proteins that cause diseases. Mad cow disease is an example. It is a misformed protein able to influence other proteins to fold in the same way.
There are 2 kinds of nucleic acids: RNA and DNA. They are necessary for carrying genetic information.
Nucleic acids are polymers of nucleotides
The nucleotides are the two purines: Adenine and Guanine, and the 3 pyrimidines, Thymine, Uracil, and Cytosine. Uracil is only found in RNA, and thymine is only found in DNA. Adenine connects with thymine/uracil, and guanine connects with cytosine.
