Chapter 2 – Chemistry Answers – Flashcards
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| Atom |
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| the basic structural unit of an element The smallest unit of an element that retains the chemical properties of that element |
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| Atoms consist of three primary particles |
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| electrons protons neutrons |
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| Nucleus |
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| small, dense positively charged region in the center of the atom |
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| Electrons |
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| negatively charged particles located outside of the nucleus of an atom |
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| have charges that are equal in magnitude but opposite in sign |
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| protons and electrons |
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| Neutral Atom |
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| has no electrical charge has the same number of protons and electrons |
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| Atomic Number |
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| the number of protons in the atom |
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| Mass Number |
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| sum of the number of protons and neutrons |
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| Isotopes |
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| atoms of the same element having different masses contain same number of protons contain different numbers of neutrons |
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| Isotopes of the same element have |
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| identical chemical properties |
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| The atomic mass |
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| the weighted average of the masses of all the isotopes that make up chlorine |
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| Weighted Average |
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| an average corrected by the relative amounts of each isotope present in nature |
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| Dalton's Atomic Theory |
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| the first experimentally based theory of atomic structure of the atom. |
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| Electrons were the __________ subatomic particles to be discovered |
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| First |
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| ___________were the next particle to be discovered, by Goldstein |
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| Protons |
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| not demonstrated to exist until 1932 |
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| Neutrons |
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| not demonstrated to exist until 1932 |
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| Neutrons |
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| It was initially assumed that protons and neutrons were |
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| evenly distributed throughout atom |
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| Rutherford's Gold Foil Experiment demonstrated... |
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| Most of the atom is empty space The majority of the mass is located in a small, dense region |
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| Rutherford's Atom |
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| tiny, dense, positively charged nucleus of protons surrounded by electrons |
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| Spectroscopy |
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| absorption or emission of light by atoms. |
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| Bohr Theory |
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| Atoms can absorb and emit energy via promotion of electrons to higher energy levels and relaxation to lower levels |
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| Quantization of energy |
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| Electrons exist in fixed energy levels surrounding the nucleus |
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| Excited State |
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| Promotion of electron occurs as it absorbs energy |
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| Relaxation |
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| Energy is released as the electron travels back to lower levels |
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| Orbit |
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| what Bohr called the fixed energy levels |
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| Ground state |
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| the lowest possible energy state |
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| Atoms absorb energy |
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| by excitation of electrons to higher energy levels |
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| Atoms release energy |
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| by relaxation of electrons to lower energy levels |
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| Atomic Orbitals |
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| regions in space with a high probability of finding an electron |
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| Periodic Law |
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| the physical and chemical properties of the elements are periodic functions of their atomic numbers. |
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| horizontal row of elements in periodic table |
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| period |
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| also called families are columns of elements in the periodic table. |
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| group |
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| elements that tend to lose electrons during chemical change, forming positive ions. |
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| metals |
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| a substance whose atoms tend to gain electrons during chemical change, forming negative ions. |
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| non metals |
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| have properties intermediate between metals and nonmetals. |
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| metalloids |
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| describes the arrangement of electrons in atoms |
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| electron configuration |
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| Valence |
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| outermost electrons |
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| Schrodengers Equations |
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| Equations that determine the probability of finding an electron in specific region in space, quantum mechanics |
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| The electron capacity of a principal energy level |
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| 2(n)2 n = 1 can hold 2(1)2 = 2 electrons n = 2 can hold 2(2)2 = 8 electrons |
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| Sublevel |
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| a set of energy-equal orbitals within a principal |
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| Sublevels increase in energy |
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| s < p < d < f |
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| Orbital |
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| a specific region of a sublevel containing a maximum of two electrons |
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| Aufbau |
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| or building up principle helps determine the electron configuration |
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| Pauli Exclusion Principle |
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| each orbital can hold up to two electrons with their spins in opposite directions. |
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| Hund's Rule |
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| each orbital in a subshell is half-filled (with one electron) and prior to filling the orbitals (with two electrons.) |
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| Octet Rule |
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| elements usually react in such a way as to attain the electron configuration of the noble gas closest to them in the periodic table |
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| electrically charged particles that result from a gain or loss of one or more electrons by the parent atom |
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| ion |
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| positively charged result from the loss of electrons 23Na ? 23Na+ + 1e- |
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| cation |
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| negatively charged results from the gain of electrons 19F + 1 e- ? 19F- |
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| anion |
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| tend to form positively charged ions called cations |
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| Metals |
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| Size of element decreases |
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| moving down from top to bottom of a group |
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| smaller than their parent atom |
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| cation |
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| anions |
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| larger than their parent atom. |
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| Ionization energy |
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| The energy required to remove an electron |
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| Electron Affinity |
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| energy released when a single electron is added to an isolated atom |
