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You can tell when it is a carbon double bond in a diagram by a show of two lines between two carbon atoms; however, you can tell when a carbon is double-bonded when you look at what the carbon is paired with. If one carbon is bonded with 4 hydrogens, then you know it only contains a single covalent bond between each hydrogen atom. But if there are two carbon atoms and 4 hydrogen atoms, you know that for that molecule to be stable, two more of those electrons need to be paired. So it is clear that the carbon must double bond to become stable.

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A molecule is two or more atoms held together by covalent bonds. An atom is the smallest unit of matter that has properties of an element, whereas a compound is a substance made of two or more combined elements in a fixed ratio. A particle is what makes up atoms.

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Particles are the small inner workings that make up an Atom. Particles are things like protons, neutrons, and electrons.

An Atom is the smallest form of matter made up of these particles, where the weight and name of the atom are determined by these protons and neutrons; an example of an atom is oxygen.

A molecule is the combination of atoms when you put them together. These molecules are connected through bonds, like a covalent bond, for example, water.

A compound is when you take different elements and put them together an example, sugar.

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The types of bonds covered in this module are covalent, ionic and hydrogen. There are also different classifications within these bonds such as single/ double bonds and polar/non polar bonds.

- Covalent bonds are when two atoms share one or more pairs of valence electrons (electrons in outermost shell of an atom).

- Covalent bonds can be polar, which is when the shared electron in the covalent bond are pulled to an electronegative atoms, making it slightly positive and slightly negative (like water). Non polar covalent bonds are when the electron is shared equally between two atoms of similar electronegativity.

- Ionic bonds are different because they don't share electrons, but rather cations and anions attract in a compound and bonds are formed that way.

- Hydrogen bonds exist between two polar covalent bonds molecules. The slightly positive Hydrogen atom of the polar bond and the slightly negative hydrogen atom of another molecule come together to make hydrogen bonds.

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ATP (which is adenosine triphosphate) is when free energy is released after water is added to phosphate bonds, this gives cells the energy to complete important processes in our bodies. ADP is the product of the reaction between ATP and water. When ATP reacts with water it loses a phosphate, becoming ADP (adenosine diphosphate). Energy is released as a result of the triphosphate bond being broken.

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Covalent bonds are the strongest bonds an atom can have. This is when two atoms share the same electron, and it orbits both nuclei. A covalent bond is polar when two atoms share an electron unfairly, but the atoms are oppositely charged. For example, in water, the oxygen is partially negative, which attracts the electron in the hydrogen, making it partially positive. A covalent bond can also be non-polar, which is when the atoms share an electron, but fairly and equally, and there is no partial opposite charge, for example, when two hydrogen atoms are bonded.

Hydrogen bonds are the weakest bonds made by molecules. It can only occur between two polar covalently bonded molecules. It does not occur between atoms.

Ionic bonds are not truly bonds; they are attractions between ions (that are now bound to a molecule) that have lost or gained an electron. For example, Na⁺(a cation) is attracted to OH⁻ (an anion) because they are both oppositely charged and bound as a molecule.

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ATP, also known as Adenosine triphosphate, is the thing that all organisms use in their cells as energy. When ATP goes through the cells and reacts with water it loses one of its three phospates and becomes ADP, Adenosine diphospate. So ADP is the product of the reaction between ATP and Water.

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Carbon atoms are very diverse in how they appear and their functions. Different types of isomers show how differently structured carbon atoms may seem the same but that the differences result in varied outcomes. For example, enantiomers (mirror image isomers) seem exactly the same but only one of those mirror image isomers are biologically active which means only that one can bond to a specific molecule in an organism.

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All carbon molecules have four electrons that need to be bonded to other molecules (such as hydrogen) to be stable. Since hydrogen has only electron and carbon requires four to be stable it looks to another carbon that has the two available electron it needs. Carbon's sharing of their two electrons results in a double bond.

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All living organisms are built from carbon skeletons. However, these carbon skeletons can form in many different ways, like branching, rings, and chains, as well as carbon being able to bond with nitrogen, hydrogen, and oxygen. This wide range of options for carbon to bond with causes a diversity in the organism. Leading to things like isomers, which are the same molecular formulas but with different structures and properties, and these differences are what lead to the differences in organisms.