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| 4928470420 | Matter | Anything that has mass and takes up space | 0 | |
| 4928470421 | Element | A pure substance that cannot be broken down into other substances by ordinary chemical means. | 1 | |
| 4928474287 | Four Elements that make up 96% living organisms | CHON - Carbon, Hydrogen, Oxygen, Nitrogen | 2 | |
| 4928476293 | Four Elements that make up 4% of living organisms | Calcium, Phosphorus, Potassium, Sulfur | 3 | |
| 4928482306 | Two important trace elements | Iron and Iodine | 4 | |
| 4928488184 | Compound | A substance containing two or more different elements that are chemically combined in a fixed ratio | 5 | |
| 4928489244 | Molecule | Two or more atoms held together by covalent bonds. They do not have to be different atoms. | 6 | |
| 4928498342 | Chemicial Formula | Tells the number and types of atoms in a compound/molecule H2O | 7 | |
| 4928498343 | Structural Formula | Gives the way the atoms are bonded H-O-H | 8 | |
| 4928501367 | Atom | The smallest particle that an element can come in and still be that element | 9 | |
| 4928503907 | Sub Atomic Particles and their charges | Proton +, Electron -, Neutron 0 | 10 | |
| 4929579130 | Proton | Positively charged particle, located inside nucleus of an atom | 11 | |
| 4929582357 | Neutron | Particle with no charge, located inside the nucleus of an atom | 12 | |
| 4929587926 | Electron | Negatively charged particle, located outside the nucleus. | 13 | |
| 4949014628 | Nucleus | Protons and Neutrons in the central core. Contains nearly all of the mass of the atom. | 14 | |
| 4949019533 | Atomic Mass | The sum of the protons and the neutrons in an atom | 15 | |
| 4949027233 | Atomic Number | Is the same as the number of protons Each element has a different number of protons It is the way we identify each element | 16 | |
| 4949096844 | How do you calculate the number of neutrons in an atom? | N = AM - P (Neutrons equals Atomic Mass - Protons | 17 | |
| 4949113237 | Where are Electrons found | In the electron cloud | 18 | |
| 4949118025 | Valence Electrons | The Electrons in the outer energy levels | 19 | |
| 4957994825 | How many bonds can an atom make? | It can make as many as it needs to get 8 electrons in its outermost shell (except H and He which can only have 2 in its outer shell) ex. Oxygen has 6 electron in its outer orbit so it can make 2 bonds. | 20 | |
| 4958015093 | Isotope | An atom with a different number of neutrons, but the same number or protons. The atomic number is the same. The atomic mass (mass number) is different. | 21 | |
| 4958070388 | Radioisotopes | Radioactive isotopes. Atoms with an unstable nucleus. When an atom loses an neutron it gives off energy (radiation). | 22 | |
| 4958087007 | Radioactivity | The release of energy and matter that results from changes int he nucleus of an atom. | 23 | |
| 4958111531 | Uses for radioisotopes | 1. Determine the age of fossils 2. Treat cancer 3. Kill bacteria than cause food to spoil 4. Labels or "tracers" to follow the movement of substances within an organism. | 24 | |
| 4958175555 | Half life | The time required for one half of the atoms in a sample to degrade to a more stable material. It is always the same for a given material It is different from isotope to isotope. | 25 | |
| 4980547945 | Ionic Bond | A bond in which electrons are transferred from one element to another. Ionic bonds make charged particles. Ionic bonds are caused by the attraction between the positive and negative charges. Ionic bonds form salts. | 26 | |
| 4980613150 | Ion | a charged particle | 27 | |
| 4980553712 | Cation | Loses electrons and has a positive charge | 28 | |
| 4980562383 | Anion | Gains electrons and has a negative charge | 29 | |
| 4980629587 | Electron donors | Atoms with only 1 or 2 outer shell electrons | 30 | |
| 4980632299 | Electron acceptors | Atoms with 6 or 7 outer shell electrons | 31 | |
| 4980661647 | Hydrogen Bond | When hydrogen is bonded to a highly electronegative atom the bonding pair is drawn towards the electronegative atom. | 32 | |
| 4980670479 | Electronegativity | The measure of the tendency of an atom to attract a bonding pair of electrons. Flourine has the highest electronegativity value. | 33 | |
| 4980684199 | Van der Waals forces | The slight attraction that can develop between the oppositely charged regions of nearby molecules. These bonds are very weak but can hold molecules together especially when the molecules are large. | 34 | |
| 4980702510 | Covalent Bond | When electron pairs are shared between the outer shells of two atoms. | 35 | |
| 4980741306 | Nonpolar Covalent Bond | When two atoms of the same element share the electrons equally. No surface charge. | 36 | |
| 4980749290 | Polar Covalent Bond | When the electrons in a molecule are shared unequally. Creates a surface charge. | 37 | |
| 4980771969 | Polar Covalent Molecules | React readily with other polar substances React readily with ionic substances They are water soluble They are attracted to any polar, ionic or charged surface | 38 | |
| 5009124126 | Hydrophobic | "Water fearing" they will not dissolve in water. They are non-polar. They tend to self-associate. | 39 | |
| 5009182640 | Chemical Reaction | The breaking of old and the forming of new chemical bonds forming new substances | 40 | |
| 5009187139 | What happens when bonds are broken? | Energy is released. | 41 | |
| 5009189593 | What happens when bonds are made? | Energy is absorbed. | 42 | |
| 5009224043 | Reactants | Starting materials in a chemical reaction. | 43 | |
| 5009226154 | Products | Ending materials in a chemical reaction | 44 | |
| 5009231948 | Conservation of matter/energy | There must be the same number of atoms of each element on both sides of a chemical equation. | 45 | |
| 5009257175 | Properties of Water | 1. Water molecules contain polar covalent bonds. 2. Water forms hydrogen bonds between molecules. 3. Water molecules are very cohesive. 4. Water has a high surface tension. 5. Water is adhesive 6. Water a high specific heat. 7. Water is an excellent solvent | 46 | |
| 5009298251 | Cohesion | The tendency of like molecules to stick to one another. | 47 | |
| 5009322516 | Adhesion | The tendency of unlike molecules to stick to one another. | 48 | |
| 5009337920 | Specific heat | The amount of heat a substance can hold before its temperature increases 1 degree Celsius. | 49 | |
| 5009371083 | Solvent | A substance that dissolves other substances | 50 | |
| 5009373976 | Solute | A substance that is dissolved in another substance | 51 | |
| 5009378200 | Solution | A uniform mixture of two or more substances | 52 | |
| 5009383951 | Aqueous solution | Any solution where water is the solvent. | 53 | |
| 5009496031 | Hyrophilic | "Water Loving" molecules that are soluble in water | 54 | |
| 5009471408 | Are Ionic substances water soluble | Yes they are because they are hydrophilic | 55 | |
| 5011196795 | Are polar substances water soluble | Yes they are because they are hydrophilic | 56 | |
| 5009480542 | Are non-polar substance water soluble | No they are not because they are hydrophobic | 57 | |
| 5009506796 | Thermal Energy | The total amount of energy associated with the random movement of atoms and molecules in matter. | 58 | |
| 5009511285 | Temperature | The measure of the average energy of random motion of the particles in a substance | 59 | |
| 5009515933 | Density | mass per unit of volume g/ml | 60 | |
| 5009530858 | pH | Percent hydrogen in an aqueous solution. How acidic or basic a solution is. | 61 | |
| 5009549248 | Acid | A compound that donates a hydrogen ions to the solution. | 62 | |
| 5009557038 | Base | A compound that removes hydrogen ions from the solution. | 63 | |
| 5009576520 | pH scale | A rating scale from 1 to 14. It measures the hydrogen ions in solution. 7 is neutral. Below 7 has more hydrogen ions and is acidic. Above 7 has less hydrogen ions and is basic. The closer to the ends of the scale, the more acidic or basic the substance is. | 64 | |
| 5045564966 | what is the difference between a pH of 5 and a pH of 4 | a power of 10 | 65 | |
| 5045570463 | What are the Characteristics of Acids | 1. They taste sour 2. They sting the skin 3. They react with metals 4. Strong acids are dangerous and can burn the skin. 5. They are H+ donors. | 66 | |
| 5045592506 | What are the Characteristics of Bases | 1. They taste bitter 2. They feel slippery to the touch 3. They do not react with metals 4. Strong bases are dangerous and can burn the skin. 6. They are H+ acceptors | 67 | |
| 5045610885 | What is a Neutralization Reaction. | When you combine equal concentrations of a Base and an Acid, the resulting products are salt and water. HCL + NaOH --> NaCl + H2O | 68 | |
| 5045627081 | What are buffers? | Substances that cause a resistance to a change in pH. | 69 | |
| 5045634971 | What is Density? | Density is mass per unit volume. (g/ml) | 70 |
