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| 4745024289 | Biology | A multidisciplinary science | 0 | |
| 4745027086 | Element | A substance that cannot be broken down to other substances by chemical reactions | 1 | |
| 4745029221 | Compound | a substance consisting of 2 or more elements in a fixed ratio | 2 | |
| 4745034771 | C.O.H.N | Carbon, Oxygen, Hydrogen, and Nitrogen make up 96% of living matter | 3 | |
| 4745038067 | Salts (Calcium, Phosphorus, Potassium, and Sulfur) | The remaining 4% is comprised of these | 4 | |
| 4745043178 | Trace elements | Elements that are required by an organism but only in trace amounts | 5 | |
| 4745046255 | Daltons | The measurement of Neutron mass and Proton mass | 6 | |
| 4745049215 | Atomic number | The number of Protons/Electrons | 7 | |
| 4745053979 | Mass number | The sum of the Protons and Neutrons | 8 | |
| 4745056686 | Atomic mass | The atom's total mass (can be approximated by the mass number) | 9 | |
| 4745060518 | Isotopes | Two atoms of an element that differ in the number of electrons | 10 | |
| 4745063508 | Radioactive Isotopes | Decay spontaneously, giving off particles and energy | 11 | |
| 4745067516 | Applications of radioactive isotopes | Dating fossils, Tracing atoms through metabolic processes, and Diagnosing medical disorders | 12 | |
| 4745069679 | Energy | The capacity to cause change | 13 | |
| 4745070403 | Potential energy | The energy that matter has because of its location or structure | 14 | |
| 4745074899 | Electrons of an atom | differ in the amounts of potential energy | 15 | |
| 4745076503 | Electron shell/energy level | an electrons state of potential energy depends on | 16 | |
| 4745085281 | Chemical behavior | the distribution of electrons in electron shells determines | 17 | |
| 4745092483 | Valence electrons | Determines the chemical behavior | 18 | |
| 4745104837 | Orbital | A three-dimensional space where an electron is found 90% of the time | 19 | |
| 4745111597 | Chemical bonds | Attractions between atoms with full valence electrons | 20 | |
| 4745113745 | Covalent bond | 2 atoms that equally share a pair of valence electrons | 21 | |
| 4745118491 | Structural formula | The notation used to represent atoms and bonding H-H | 22 | |
| 4745120486 | Molecular formula | An abbreviated version of the structural formula H2 | 23 | |
| 4745123206 | Molecule | 2 or more atoms that are held together by covalent bonds | 24 | |
| 4745124925 | Valence | the bonding capacity of an atom | 25 | |
| 4745125984 | Electronegativity | An atom's attraction for the electrons in a covalent bond | 26 | |
| 4745129606 | Non-polar covalent bonds | The atoms share the electron equally | 27 | |
| 4745131043 | Polar covalent bonds | One atom is more electronegative, and the atoms do not share the electron equally | 28 | |
| 4745133655 | Ionic bonds | Stripping/giving an electron instead of sharing | 29 | |
| 4745135935 | Ion | A charged atom | 30 | |
| 4745136215 | Cation | A positively charged ion | 31 | |
| 4745136872 | Anion | A negatively charged ion | 32 | |
| 4745137929 | Ionic bond | The attraction between an anion and a cation | 33 | |
| 4745139286 | Ionic compounds/salts | Compounds formed by ionic bonds | 34 | |
| 4745144176 | Covalent bonds | The stronger bond | 35 | |
| 4745146783 | Ionic/Hydrogen bonds | The weaker bonds | 36 | |
| 4745149011 | Weak chemical bonds | Help reinforce shapes of large molecules and help molecules adhere to each other | 37 | |
| 4745151223 | Hydrogen bonds | When a hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom (usually oxygen and hydrogen atoms) | 38 | |
| 4745162273 | Van Der Waals interactions | Attractions between molecules that are close together as a result of these charges | 39 | |
| 4745165698 | S/P orbitals | The orbitals that hybridize in covalent bonds which creates a specific molecular shape | 40 | |
| 4745174221 | Chemical Equilibrium | When the forward and reverse reaction rates are equal | 41 |
