8. atomic mass: the mass of the element and represents the. 9. Atomic number: on top of the atomic symbol; represents the.
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1 Intro To Chemistry Study online at quizlet.com/_2xw51k 1....: alkali metals: 8. atomic mass: the mass of the element and represents the number of protons plus the number of neutrons. 9. Atomic number: on top of the atomic symbol; represents the number of protons 10. Atomic Symbol: the letters on the periodic table that represent the name of the given element 11. beta particle: 3. alkaline earth metals: any metal in Group 1A of the periodic table 4. alpha particle: the elements in Group 2A of the periodic table a high-speed electron or positron emitted in the decay of a radioactive isotope 12. Bohr: said that all matter is composed of atoms that have different shells/orbitals. These orbitals have different energy levels and electrons "orbit" on these shells. The shells can only hold a limited amount of electrons 13. Catylist: speeds up a chemical reaction 14. Chain reaction (nuclear): a type of nuclear radiation consisting of two protons and two neutrons 5. amu: atomic mass units 6. Anion: the process during which fission of one nucleus triggers fission of others, which, in turn, induces fission in others, and so on A negatively charged ion 7. atom: smallest particle of an element
2 15. Characteristics of Alkali Metals: 19. chemical bond: -Very reactive -good conductors -end in s1 -need to lose 1e- to have a noble gas configuration -reactivity increases as you go down the family -not hydrogen 16. Characteristics of Alkaline Earth Metals: the attractive force that holds atoms or ions together 20. chemical characteristic: cannot be reversed as it changes chemical compositions 21. chemical energy: Energy stored in chemical bonds 22. chemical equation: -end in s2 -less reactive -need to lose 2e- to have noble gas configuration 17. Characteristics of Halogens: A short, easy way to show a chemical reaction, using symbols. 23. Coefficient (in a chemical equation): 24. Cold Fusion: number of molecules/molar ratio have seven valence electrons; highly reactive; nonmetals; react with most metals 18. Characteristics of Nobel Gases: Non reactive, full valence shell nuclear fusion occurring at or close to room temperature. Claims for its discovery in 1989 are generally held to have been mistaken.
3 25. combustion reaction: 34. electron configuration: describes the number of electrons in each shell/orbital and gives a location of the element on the periodic table 35. Electron dot diagram (aka Lewis structures): a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light 26. condensation: phase change from a gas to a liquid 27. conductivity: allows heat/electricity/energy to flow 28. covalent bond: A shorthand representation of the valence electrons in an atom. 36. element: only one TYPE of atom 37. endothermic reaction: A chemical bond formed when two atoms share electrons 29. critical mass: the smallest possible mass of a fissionable material that can sustain a chain reaction 30. decomposition reaction (catabolism): AB --> A + B. breaks chemical bonds 31. deposition: phase change from a gas to a solid 32. double replacement reaction: 38. Equilibrium: A reaction that ABSORBS energy in the form of heat a chemical reaction between two compounds where the positive ion of one compound is exchanged with the positive ion of another compound 33. Electron: 39. exothermic reaction: A state of balance A reaction that releases energy in the form of heat 40. filtration: separation of substances by particle size negatively charged particle
4 41. Fission: 49. Ion: The splitting of an atomic nucleus to release energy. 42. flammability: ability to burn in the presence of oxygen 43. freezing: phase change from a liquid to a solid 44. gamma rays: A charged atom 50. ionic bond: the attraction between oppositely charged ions. Formed when one or more electrons are transferred/taken from one atom to another 51. Location of the metalloids (periodic table): high-energy electromagnetic waves emitted from a nucleus as it changes from an excited state to a ground energy state 45. Group 8A; 18 is called: Nobel Gas 46. groups: vertical columns used to help organize the periodic table 47. half-life: stair-cased from group 3A starting with element Boron 52. Location of the metals (periodic table): length of time required for half of the radioactive atoms in a sample to decay 48. Halogens: 53. Location of the non-metals: elements left of the metalloids Group 7A elements right of the metalloids 54. Location of the "P" block: groups: 3A, 4A, 5A, 6A, 7A, and 8A 55. Location of the "S" block: groups 1A and 2A 56. malleability: able to be hammered/shaped without shattering 57. matter: something that takes up space and has mass 58. melting: phase change from a solid to a liquid
5 59. metalloids: characteristics of a metal and a non-metal 60. molar mass: the mass of one mole of a pure substance 61. mole: 65. nuclear decay: a process that occurs when an unstable atomic nucleus changes into another more stable nucleus by emitting radiation 66. nuclear radiation: the SI base unit used to measure the amount of a substance 62. Molecule: 63. Neutron: two or more atoms held together by covalent bonds the particles that are released from the nucleus during radioactive decay 67. patterns seen across a period (periodic table): 1) atomic mass increases from left to right; 2) atomic number increases from left to right; 3) number of electrons increase from left to right; 4) number of protons increase from left to right; 5) number of groups increase from left to right 68. patterns seen down a group (periodic table): 1) atomic mass increases from top to bottom; 2) atomic number increases from top to bottom; 3) number of electrons increase from top to bottom; 4) number of protons increase from top to bottom; 5) number of periods increase from top to bottom 69. Periodic table is organized by:: groups, periods, atomic number, atomic mass, physical characteristics, chemical characteristics, reactivity, number of protons, electron configurations 70. periods: horizontal rows used to help organize the periodic table 71. phase changes: physical change to another form (solid, liquid, gas, or plasma) 72. physical characteristics: can be reversed and chemical composition stays the same A small particle in the nucleus of the atom, with no electrical charge 64. noble gases: the elements in Group 8A of the periodic table
6 73. polar-covalent bonding: 78. Radioisotopes: Isotopes that have unstable nuclei and undergo radioactive decay. 79. Reactant: unequal sharing of electrons 74. Product (of a chemical reaction): a substance that takes part in and undergoes change during a reaction. 80. reaction rate: 75. Proton: element or compound produced by a chemical reaction the rate at which reactants change into products over time 81. reactivity: describes how substances combine/behave/act with other substances 82. reversible reaction: positively charged particle 76. pure substance: matter with the same chemical composition 77. Radioactivity: a chemical reaction in which the products reform the original reactants The spontaneous emission of radiation by an unstable atomic nucleus
7 83. single replacement reaction: a chemical reaction in which one element takes the place of another element in a compound 84. sublimation: phase change from a solid to a gas 85. synthesis reaction (composition reaction): 86. valence electrons: two or more substances combine to form a new compound 87. valence shell: Electrons on the outermost energy level of an atom 88. vaporization: phase change from a liquid to a gas 89. viscosity: resistance to flow outermost shell of an atom
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