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Chemistry - Final
Vocabulary
| Term | Definition |
|---|---|
| Coulomb's Law | like charges repel one another, and opposite charges attract one another |
| "Rays" | stream of negatively charged particles (electrons) |
| X-Rays | sufficiently energetic to penetrate matter and causes certain materials to fluoresce; doesn't have charged particles |
| Radioactivity | spontaneous emission of radiation |
| Alpha Rays | Positively charged |
| Beta Rays | Negatively charged |
| Gamma Rays | high energy; no charge |
| Atomic Radius | generally 100 picometers |
| Atomic Number | the number of protons in the nucleus of each atom in an element; also indicates number of electrons |
| Mass Number | Total number of protons and neutrons present in the nucleus of an atom |
| Isotopes | atoms that have the same atomic number, but different mass numbers |
| Atomic Mass | the mass of an atom in atomic mass units (amu) |
| Average Atomic Mass (atomic weight) | determines atomic mass of an element while finding and measuring the mixture of isotopes |
| Groups/Families | Vertical Columns |
| Periods | Horizontal rows |
| Mole | amount of a substance that contains as many elementary entities (atoms, particles, etc) as there are atoms in exactly 12 g of Carbon `12 |
| Avogadro's Number | the number of atoms in exactly 12 grams of carbon-12 (6.022x10^23) |
| Molar Mass | mass in grams of 1 mole of the substance (average atomic mass) |
| Energy | capacity to do work or transfer heat |
| Kinetic Energy | energy that results from motion |
| Thermal Energy | form of kinetic energy associated with random motion of atoms and molecules |
| Potential Energy | energy possessed by an object by virtue of its position |
| Chemical Energy | form of potential energy stored within the structural units of chemical substances |
| Electrostatic Energy | potential energy that results from the interaction of charged particles |
| Law of Conservation of Energy | energy can be neither created or destroyed; when 1 form disappears, the same amount of energy must appear in another form |
| Electromagnetic spectrum | consists of visible light, radio waves, microwaves, infrared, X-rays, and gamma rays |
| Electromagnetic Wave | has both electric field component and magnetic field component. |
| Interference | phenomenon that demonstrates the wave nature of light |
| Constructive Interference | two waves are "in phase" resulting in light lines |
| Destructive Interference | two waves are "out of phase" resulting in dark lines |
| Blackbody Radiation | Electromagnetic radiation emitted when a solid is heated (stove, lightbulb) |
| Quantum | smalles quantity of energy that can be emitted or absorbed in the form of electromagnetic radiation |
| Photoelectron effect | Electrons are ejected from the surface of a metal exposed to light; the light must be of a certain minimum frequency called the threshold frequency |
| Photon | light particles |
| Emission Spectra | the light emitted, either as a continuum or in discrete lines, by a substance in an excited electronic state |
| Line Spectra | The emission of light only at specific wavelengths |
| Electromagnetic Radiation | energy given off when electrons that were promoted to a higher level, returns to the lower levels |
| Ground State | the lowest energy state of an atom (n=1) |
| Excited State | each state where n>1; the higher this state the farther away the electron is from the nucleus |
| de Broglie Hypothesis | an electron in an atom behaves like a "standing wave" ; only certain wavelengths are possible/allowed; the wavelength must fit the circumference of the orbit exactly |
| Heisenberg Uncertainty Principle | It is impossible to know simultaneously both the momentum and position of a particle with certainty |
| The Schrodinger Equation | describes behavior and energies of subatomic particles |
| Electron Densities | probability that an electron will be found in a particular region of an atom |
| Atomic Orbittal | wave function of an electron in an atom |
| Principal Quantum Number (n) | designates size of orbital; the larger n is the greater the average distance of an electron in the orbital from the nucleus and therefore the larger the orbital |
| Angular Momentum Quantum Number (L) | describes shape of atomic orbital; depends on value of n |
| Magnetic Quantum Number (ML) | describes the orientation of the orbital in space; depends on value of L; indicates number of orbitals in a subshell |
| Electron Spin Number (Ms) | describes electron that occupies orbital; 2 possible directions) |
| Electron Configuration | how the electrons are distributed in the various atomic orbitals |
| Pauli Exclusion Principle | no two electrons in an atom can have the same 4 quantum numbers (2 electrons can't be in same place at same time) |
| Ground State | one in which all electrons occupy orbitals of the lowest possible energy |
| Aufbau Principle | electrons are added to orbital of lowest energy |
| Hund's Rule | most stable arrangement of atoms is the one with the number of electrons with the same spin that is maximized |
| Diamagnetic | atoms with all paired electrons; the noble gases (repelled by magnets) |
| Paramagnetic | atoms with one or more unpaired electrons (attracted to magnetic field) |
| Transition Metals | either have incompletely filled d subshells or give rise to cations with incompletely filled d subshells |
| Effective Nuclear Charge | the actual magnitude of the positive charge "experienced" by an electron in an atom (shielding) |
| Metallic Radius | half the distance between the nuclei of 2 adjacent, identical metal atoms |
| Covalent Radius | half the distance between, adjacent identical nuclei that are connected by a chemical bond |
| Ionization Energy | minimum energy required to remove an electron from an atom in the gas phase (forms cations) |
| Electron Affinity | energy released when an atom in the gas phase accepts an electron (forms anions) |
| Compound | substance composed of 2 or more elements combined in a specific ratio and held together by chemical bonds; cannot be physically separated into a simpler substance |
| Ionic Compound | when a compound consists of anions and cations |
| Ionic Bonding | electrostatic attraction between oppositely charged particles |
| Chemical Formula | part of ionic compound that denotes the constituent elements of a compound and the ratio in which they combine |
| Lattice | structure of an ionic compound that consists of a vast array of interspersed cations and anions; the arrangement is such that the compound is electrically neutral |
| Lattice Energy | amount of energy required to convert a mole of ionic solid to its constituent ions in the gas phase |
| Lewis Theory of Bonding | electrons are shared between elements of similar properties |
| Covalent Bonding | when two atoms share a pair of electrons which makes a covalent bond |
| Molecule | a neutral combination of at least 2 atoms in a specific arrangement held together by chemical bonds |
| Law of Definite Proportions | Different samples of a given compound always contain the same elements in the same mass ratio |
| Law of Multiple Proportions | if 2 elements can combine with the other to form 2 or more different compounds the ratio of masses of one element that combine with the fixed mass of another element can be expressed in small whole numbers. |
| Diatomic molecule | contains 2 atoms |
| Polyatomic Molecules | contains more than 2 atoms |
| Chemical formula | can be used to denote the composition of any substance - ionic or molecular |
| Molecular formula | shows the exact number of atoms of each element in a molecule |
| Allotrope | one of 2 or more distinct forms of an element (O, O2, O3) |
| Structural Formula: | Shows not only the elemental composition but also the general arrangement of atoms within a molecule (water - HOH) |
| Empirical Formula | tells us what elements are present in a molecule and in what whole number ratio they are combined |
| Ionizable Hydrogen Atom | one that separates from the molecule upon dissolving and becomes a hydrogen ion (a proton) |
| Organic Compounds | contain carbon and hydrogen |
| Inorganic Compound | does NOT contain carbon |
| Hydrocarbons | those that only contain carbon and hydrogen |
| Polyatomic Ions | ions that consist of 2 or more atoms |
| Oxoanions | polyatomic ions that contain one or more O atoms and one "central atom" of another element |
| Oxoacids | when dissolved in H2O produces H+ ions and corresponding oxoanions |
| Hydrate | compound that has a specific number of water molecules within its solid structure |
| Molecular Mass | sum of atomic masses of the atoms that make up the molecule (multiply atomic masses of each element by the number of atoms present too) |
| Formula Mass | sum of atomic masses of the atoms that make up an ionic compound (multiply atomic masses of each element by the number of atoms present as well) |
| Percent Composition by Mass | a list of the percent by mass of each element in a compound; divide the mass of each element by the molecular/formula mass |
| Molar Mass | mass in grams of one mole of a substance (atomic mass) |
| Octet Rule | atoms will lose, gain, or share an electron in order to achieve noble gas electron configuration |
| lone pair | pairs of unbounded valence electrons |
| Bond Length | distance between nuclei of 2 covalently bonded atoms in a molecule; multiple bonds are SHORTER than single bonds |
| Bond Strength | quantity of energy required to break bond; the shorter the length the stronger the bond |
| Polar bonds | electrons are shared, but not equally |
| Pure Covalent Bond | neutral atoms held together by equally shared atoms |
| Polar Covalent bond | partially charged atoms held by unequally shared electrons |
| Ionic Bond | oppositely charged ions held by electrostatic attraction |
| Electronegativity | ability of an atom to draw shared electrons (in the bond) toward itself; determines electron density |
| High Electronegativity | greater tendency to attract electron density |
| dipole moment | quantative measure of the polarity of a bond; calculated as the product of the charge and the distance between the charges |
| Percent ionic Character | the ratio of observed dipole moment to calculated dipole moment |
| formal charge | can be used to determine most plausible Lewis Structures when more than 1 structure exists for a compound |
| Resonance Structure | one of two or more equally valid Lewis Structures for a single species |
| The Bigger the change in Electronegativity : | the bigger the dipole moment. |
| Coordinate Covalent bond | covalent bond in which one of the atoms donates both electrons |
| free radicals | molecules with an odd number of electrons; exception to the octet rule; adds an electron to central atom |
| VSEPR Theory | a model that accounts for electron pairs in the valence shell of an atom repelling one another |
| Electron Domain | a lone pair OR bond, regardless of whether bond is double, single, or triple |
| VESPR Theory | predicts electron domains will rearrange themselves to be as far apart as possible, minimizing repulsive interactions |
| Electron domain geometry | arrangement of electron domains (lone pairs and bonds) around central atom |
| molecular geometry | arrangement of bonded atoms |
| Linear Bond Angle | 180 degrees |
| Trigonal Planar Bond Angle | 120 degress |
| Tetrahedral Bond Angle | 109 degrees |
| Trigonal Bipyramidal Bond Angle | 120 and 90 degrees |
| Octahedral Bond Angle | 90 degrees |
| equitorial | bonds in trigonal plane |
| axial | bonds on axis perpendicular to trigonal plane |
| Structural Isomers | molecules with same chemical formula but different arrangements of atoms |
| Bond Energy | amount of energy required to break a mole of identical bonds |
| Valence Bond Theory | atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on another; each orbital must have an unpaired electron and must have opposite spins; formation of bond results in lower potential energy |
| hybridization | mixing of atomic orbitals |
| hybrid orbitals | neither s or p but have characteristics of both |
| Chemical reactions | neither creates/destorsy atoms, but rearranges them in chemical compounds; involves changes in energy |
| Combination Reactions | a reaction in which 2 or more reactants combine to form a single product |
| Decomposition Reaction | a reaction in which 2 or more products form a single reactant |
| Combustion Reaction | a reaction in which a substance burns in the presence of oxygen |
| Combustion Analysis | experimental determination of empirical formula |
| Hess's Law | change in enthalpy in a chemical reactions is the same, whether it takes place in 1 step or several |
| Enthalpy of Formation | the change in enthalpy to produce one mole of compound from its constituent elements at standard conditions (most stable form is zero) |
| Bond Enthalpy | Gives us a numerical value for the strength of a covalent bond |
Created by:
ebeneda
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