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| 7553236031 | Atom | The basic unit of an element that retains the properties of the element. |  | 0 |
| 7553236032 | Proton | Positively charged subatomic particle found in the nucleus of an atom; equal to the number of electrons in an electrically neutral atom. |  | 1 |
| 7553236033 | Neutron | A neutrally charged subatomic particle found in the nucleus of an atom. |  | 2 |
| 7553236034 | Electron | A negatively charged subatomic particle found orbiting the nucleus of an atom; equal to the number of protons in an electrically neutral atom. | | 3 |
| 7553236035 | Atomic Weight | Measured in daltons, and consists of the weight of protons and neutrons together, each of which weighs about one dalton. |  | 4 |
| 7553236036 | Atomic Nucleus | The portion of an atom which contains protons and neutrons. |  | 5 |
| 7553236037 | Orbital | The volume of space an electron occupies. |  | 6 |
| 7553236038 | Energy Shells | Represent the state of potential energy of an electron. Those closer to the nucleus have the least amount of energy. |  | 7 |
| 7553236039 | Valence Shell | The outermost shell of an atom which has the most potential energy. |  | 8 |
| 7553236040 | Valence electrons | Electrons in the valence, or outermost, energy shell of an atom, which have the most potential energy and which can form bonds with other atoms. |  | 9 |
| 7553236041 | Isotopes | Varying atomic forms of an element which vary from an electrically neutral atom in the number of neutrons, causing the atomic weight to vary. Radioactive isotopes have medical imaging and other applications. |  | 10 |
| 7553236042 | Chemical Bonds | Attractions between atoms resulting from a sharing of valence electrons or the presence of opposite charges on the atoms. The bonded atoms gain complete valence shells. |  | 11 |
| 7553236043 | Covalent Bond | The sharing of a pair of valence electrons by two atoms. |  | 12 |
| 7553236044 | Molecule | Two or more atoms held together by covalent bonds. |  | 13 |
| 7553236045 | Single Bond | One pair of shared electrons. Example: hydrogen. |  | 14 |
| 7553236046 | Double Bond | Two pairs of shared electrons. Example: Oxygen has 6 electrons in its valence shell, which can hold 8. Each atom shares 2 electrons for a total of 4. | 15 | |
| 7553236047 | Valence | An atom's bonding capacity, or the number of covalent bonds the atom can form to give the atom a full complement of electrons in the valence shell. Usually equals the number of unpaired electrons required to complete the valence shell. |  | 16 |
| 7553236048 | Electronegativity | The attraction of a particular atom for the electrons of a covalent bond. Atoms in a molecule attract shared bonding electrons to varying degrees. This degree is _________. |  | 17 |
| 7553236049 | Nonpolar Covalent Bond | A covalent bond between 2 atoms of the same element in which the electrons are shared equally because the two atoms have the same electronegativity. |  | 18 |
| 7553236050 | Polar Covalent Bond | An atom bonded to a more electronegative atom. |  | 19 |
| 7553236051 | Ionic Bonds | Bonds between two atoms so unequal in their attraction for valence electrons that the more electronegative atom strips an electron completely away from its partner. |  | 20 |
| 7553236052 | Ion | One of two charged atoms resulting from an ionic bond. |  | 21 |
| 7553236053 | Cation | A positively charged ion |  | 22 |
| 7553236054 | Anion | A negatively charged ion |  | 23 |
| 7553236055 | Ionic compounds | Compounds formed by ionic bonds. |  | 24 |
| 7553236056 | Salts | Another name for ionic compounds; formed by ionic bonds. |  | 25 |
| 7553236057 | Stable or Inert Atom | An atom with a full valence shell |  | 26 |
| 7553236058 | Hydrogen Bonds | Relatively weak bonds formed due to the mutual attraction of two electronegative atoms to hydrogen. |  | 27 |
| 7553236059 | Compound | A substance consisting of two or more elements in a fixed ratio. |  | 28 |
| 7553236060 | Element | A substance that cannot be broken down into other substances by chemical reactions. |  | 29 |
| 7553236061 | Trace Elements | Elements required by organisms but only in minute quantities. |  | 30 |
| 7553236062 | Radioactive Isotopes | An unstable isotope with a nucleus that decays spontaneously, emitting particles and energy. Have many applications in biological research, including fossil dating (Carbon-14 or 14C), tracing atoms through metabolic processes, and diagnosing medical disorders. |  | 31 |
| 7553236063 | Electron configuration influences the ______ of an atom. | Chemical behavior |  | 32 |
| 7553236064 | Atoms are mostly _________. | Empty space. |  | 33 |
| 7553236065 | Atoms with the same number of ____________ have similar chemical behaviors. | Valence electrons |  | 34 |
| 7553236066 | Each orbital can hold a maximum ____ electrons. | 2 |  | 35 |
| 7553236067 | The reactivity of atoms arises from the presence _______ _____________ in one or more orbitals of their valence shells. | Unpaired electrons |  | 36 |
| 7553236068 | Electrons occupy ________ _________ within the valence shell until forced to share orbitals. | Separate orbitals |  | 37 |
| 7553236069 | The strongest chemical bonds are _______ bonds and _________ bonds. | Chemical and ionic |  | 38 |
| 7553236070 | Two or more atoms held together by a covalent bond consistute a _________. | Molecule |  | 39 |
| 7553236071 | True or False: Covalent bonds can form between atoms of the same element ONLY. | False. |  | 40 |
| 7553236072 | _____ chemical bonds play important roles in the chemistry of life. | Weak |  | 41 |
| 7553236073 | Octet Rule | An atom with more than 1 energy shell is most biologically stable with 8 electrons in the valence shell. |  | 42 |
| 7553236074 | Structural Formula | Uses bond symbols to show shared electrons between atoms. Example: H-H shows a hydrogen molecule sharing one pair of valence electrons. O=O shows two oxygen atoms sharing two pairs of valence electrons. |  | 43 |
| 7553236075 | Molecular Formula | A formula showing the type of element and number of atoms only. Example: H2O |  | 44 |
| 7553236076 | Cellular Respiration Equation | CR= C6H12O6 + 6O2 ---> 6CO2 + 6H2O + 30 - 32ATP |  | 45 |
| 7553236077 | Photosynthesis Equation | Photo = 6CO2 + 6H2O ---> C6H12O6 + 6O2 |  | 46 |
| 7553236078 | Enzymes | Proteins that catalyze chemical reactions |  | 47 |
| 7553236079 | Metabolic Pathways | Series of metabolic reactions that occur in specific sequences |  | 48 |
| 7553236080 | Anabolism | Conversion of small organic molecules by forming chemical bonds between the smaller molecules. |  | 49 |
| 7553236081 | Catabolism | Conversion of large molecules into smaller components. |  | 50 |
| 7553236082 | Metabolism | All the chemical conversions that occur within a cell. |  | 51 |
| 7553236083 | van der Waals interactions | Weak attractions between molecules or parts of molecules that result from transient local partial charges. |  | 52 |
| 7553236084 | Molecular shape is determined by the position of the atoms' _________. | Orbitals |  | 53 |
| 7553236085 | Biological molecules often bind temporarily to each other by forming weak bonds, but only if their _________ are complementary. | Shapes |  | 54 |
| 7553236086 | Chemical Reactions | The making and breaking of chemical bonds, leading to changes in the composition of matter. |  | 55 |
| 7553236087 | Reactants | The starting materials in a chemical reaction. |  | 56 |
| 7553236088 | Products | The ending materials in a chemical reaction. |  | 57 |
| 7553236089 | Reactions cannot create or destroy matter but can only _________ ____ _________ among them. | Rearrange the electrons |  | 58 |
| 7553236090 | True or False: All chemical reactions are reversible. | True |  | 59 |
| 7553236091 | Chemical Equilibrium | The point at which chemical reactions offset one another and the forward and reverse reaction rates are equal. |  | 60 |
