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| 6841907016 | Matter | Anything that takes up space and has mass | 0 | |
| 6841907017 | Element | A substance that cannot be broken down to another substance by chemical reaction | 1 | |
| 6841907018 | Compound | A substance made of two or more DIFFERENT elements combined in a fixed ratio (NaCl, H2O) | 2 | |
| 6841907019 | Essential elements | Elements that an organism requires for survival | 3 | |
| 6841907020 | Examples of essential elements | Carbon, oxygen, hydrogen, nitrogen, calcium, potassium, sulfur, ect.. | 4 | |
| 6841907021 | Trace elements | Elements that are required by an organism in only minute quantaties | 5 | |
| 6841907022 | Name two trace elements | Iron, iodine | 6 | |
| 6841907023 | Atom | The smallest unit of matter that still retains the properties of an element | 7 | |
| 6841907024 | What are the three subatomic particles? | Protons, neutrons, and electrons | 8 | |
| 6841907026 | Atomic number | a subscript identifying the number of protons in an atom by writing the number to the left of the symbol for the element (ex: 2He) | 9 | |
| 6841907027 | Mass number | The sum of protons plus neutrons in the nucleus of an atom, also written in superscript to the left of the atoms symbol | 10 | |
| 6841907028 | Atomic mass | The mass number is an approximation of the total mass of an atom | 11 | |
| 6841907029 | Isotopes | Different atomic forms of the same element, created when the same element has a different number of neutrons (Number of protons MUST remain the constant to consider the element the same) | 12 | |
| 6841907030 | Radioactive isotopes | An isotope in which the nucleus decays spontaneously, giving off particles and energy. When a decay leads to a change in protons, the element changes. | 13 | |
| 6841907031 | Energy | the capacity to cause change (ex. doing work) | 14 | |
| 6841907032 | Potential energy | the energy that matter possesses because of its location or structure. It takes work to move an electron farther away from its nucleus, so the more distant an electron is from it, the greater the potential energy. | 15 | |
| 6841907033 | Electron Shells | Electrons can be found here, and each shell has an average distance and energy level. The lower the electron shell, the lower the energy level, and thus lower potential energy to an electron in that electron shell | 16 | |
| 6841907034 | Valence electrons | Outermost electrons | 17 | |
| 6841907035 | Valence shell | Outermost electron shell | 18 | |
| 6841907036 | Chemical bond | The process of two or more atoms transferring or sharing electrons | 19 | |
| 6841907037 | What are the strongest types of chemical bonds? | Covalent and ionic bonds | 20 | |
| 6841907038 | Covalent bond | The sharing of a pair of valence electrons by two atoms. | 21 | |
| 6841907040 | Single bond | one pair of shared electrons | 22 | |
| 6841907041 | Double bond | Two pairs of shared electrons | 23 | |
| 6841907042 | Valence | the bonding capacity of two atoms and usually equals the number of electrons required to complete the atoms outermost valence shell | 24 | |
| 6841907043 | Electronegativity | The attraction of a particular atom for the electrons of a covalent bond. The more electronegative an atom is, the more strongly it pulls shared electrons toward itself. | 25 | |
| 6841907044 | Nonpolar covalent bond | Between two or more atoms of a common element, where the charges of the molecule are balanced and equal. | 26 | |
| 6841907045 | Polar covalent bond | Between two or more atoms of different elements, where they are not balanced and thus polar | 27 | |
| 6841907046 | Ion | A charged atom/molecule | 28 | |
| 6841907047 | Cation | A positively charged ion | 29 | |
| 6841907048 | Anion | A negatively charge ion | 30 | |
| 6841907049 | Ionic Bond | The attraction between cation and anion, where electrons are transfered. | 31 | |
| 6841907050 | Ionic Compounds/Salts | Compounds formed by ionic bonds. | 32 | |
| 6841907051 | Hydrogen bonds | The noncovalent attraction between a hydrogen and an electronegative atom | 33 | |
| 6841907052 | van der Waals interactions | Individually weak and occur only when atoms and molecules are very close together. This is what gives certain organisms the ability to stick to things. | 34 | |
| 6841907053 | Chemical reaction | The making and breaking of chemical bonds, leading to a change in the composition of matter | 35 | |
| 6841907054 | What is the chemical equation of photosynthesis? | 6 CO2 + 6 H2O --> C6H12O6 + 6 O2 | 36 | |
| 6841907055 | Chemical equilibrium | The point at which the reactions offset one another exactly. Reactions are still going on, but with no net effect on the concentrations of reactants and products. Does NOT mean the ^ and the ^ are equal in concentration. | 37 | |
| 6841907056 | Cohesion | Hydrogen bonds holding a substance together | 38 | |
| 6841907057 | Adhesion | The clinging of one substance to another | 39 | |
| 6841907058 | Surface tension | A measure of how difficult it is to stretch or break the surface of a liquid. | 40 | |
| 6841907059 | Kinetic energy | Anything that moves, the energy of motion | 41 | |
| 6841907060 | Thermal energy | The kinetic energy associated with the random movement of atoms or molecules, and depends on the matter's volume | 42 | |
| 6841907061 | Temperature | Represents the average kinetic energy of molecules, regardless of volume | 43 | |
| 6841907062 | Heat | Thermal energy transferred from one body of matter to another | 44 | |
| 6841907063 | Calorie | Unit of heat. Is the amount of heat it takes to raise the temperature of 1 g of water by 1 degree Celsius. | 45 | |
| 6841907064 | Kilocalroie | 1,000 calories, is the quantity of heat required to raise the temp of 1 kilogram of water by 1 degree Celsius | 46 | |
| 6841907065 | Joule | Another energy unit, equals 0.239 cal. One cal equals 4.184 j | 47 | |
| 6841907066 | Specific heat | the amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1*C | 48 | |
| 6841907067 | Heat of vaporization | The quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gaseous state | 49 | |
| 6841907068 | Evaporation cooling | Occurs because the hottest molecules (those with the greatest kinetic energy) are the ones most likely to leave as gas. | 50 | |
| 6841907069 | Solution | A liquid that is a completely homogeneous mixture of two or more substances | 51 | |
| 6841907070 | Solvent | The dissolving agent of a solution | 52 | |
| 6841907071 | Solute | The substance that is being dissolved | 53 | |
| 6841907074 | Hydrophilic | Any substance with an affinity for water (water-loving) | 54 | |
| 6841907075 | Hydrophobic | Substances that are nonionic/nonpolar and can't for hydrogen bonds repel water. Ex: oils and water | 55 | |
| 6841907081 | Acid | Is a substance that increases the hydrogen ion concentration of a solution | 56 | |
| 6841907082 | Base | A substance that reduces the hydrogen ion concentration of a solution | 57 | |
| 6841907085 | pH | What | 58 | |
| 6841907086 | Buffers | A substance that minimizes changes in the concentration of H+ and OH- in a solution. | 59 |
