Chem 1 Final Vocab
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148 terms
Terms | Definitions |
|---|---|
 Matter | that which has mass and occupies space |
| Crystal lattice | a repeating three-dimensional pattern of ions |
| Translational motion | Motion from one point to another which does not involve repeatedly passing the same point in space |
| Rotational motion | Motion when an object moves aroud its centre of mass |
| Vibrational motion | atoms in the molecule move periodically toward and away from one another |
| Fluid | any substance that can flow |
| Compressible | can be made to occupy a smaller volume |
| Density | the amount of matter in a given space, mass/volume |
| Temperature | the average kinetic energy of the individual particles |
| Maxwell-Boltzman distribution | An increase in temp spreads out the distribution and the mean speed shifts upward |
| Absolute Zero | The coldest temperature, 0 Kelvin, that can be reached. It is the hypothetical temperature at which all molecular motion stops. |
| Kelvin | SI unit for temperature |
| Condensation | gas to liquid |
| Evaporation | Liquid to Gas, the process by which water changes from liquid form to an atmospheric gas |
| Vaporization | liquid to gas |
| Sublimation | solid to gas |
| Deposition | gas to solid |
| Endothermic | describes a process in which heat is absorbed from the environment |
| Exothermic | chemical reaction in which energy is primarily given off in the form of heat |
| Kinetic Energy | the energy an object has due to its motion |
| Potential energy | energy stored due to an object's position or arrangement |
| Phase Change | the reversible physical change that occurs when a substance changes from one state of matter to another |
| Physical Change | a change in a substance that does not involve a change in the identity of the substance |
| Boiling point | The temperature at which a liquid boils |
| Melting/Freezing point | the temperature at which a substance changes from a solid to a liquid or a liquid to a solid |
| Heating/cooling curve | graph showing the increase of temp and energy for a substance |
| Pure substance | a sample of matter, either a single element or a single compound, that has definite chemical and physical properties |
| Mixture | a substance consisting of two or more substances mixed together (not in fixed proportions and not with chemical bonding) |
| Scientific law | a concise statement that summarizes the results of many observations and experiments |
| Scientific Theory | a well-tested concept that explains a wide range of observations |
| Pressure | the force applied to a unit area of surface |
| Torr(mmHg) | Ways to measure pressure. One atmosphere = 760 torr or mmHg |
| Atmosphere | A type of unit to measure pressure |
| Directly proportional | a term used to describe the relationship between two variables whose graph is a straight line passing through the point (0,0) |
| Inversely proportional | a term used to describe the relationship between two variables whose product is constant |
| Boyle's Law | The relationship between the pressure and volume of a gas at constant temperture; when volume increase, pressure decreases, P1V1=P2V2 |
| Charles' Law | the law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the gas decreases, V1/T1=V2/T2 |
| Kinetic Theory of Gasses | The model states that the movement of molecules in a gas is random and that no energy is lost when they collide with each other or their surroundings. |
| Elastic collisions | encounters between gas particles in which kinetic energy is transferred without loss from one particle to another |
| Cathode Ray | a beam of electrons emitted by the cathode of an electrical discharge tube |
| Subatomic Particles | protons, neutrons, and electrons |
| Atomic Number | the number of protons in the nucleus of an atom |
| Mass Number | the sum of the numbers of protons and neutrons in the nucleus of an atom |
| Atomic Mass | total mass of the protons and neutrons in an atom, measured in atomic mass units |
| Isotope | atoms of the same element that have different numbers of neutrons |
| Frequency | The number of waves that have passed through a specific point in a certain amount of time units. |
| Wavelength | The distance between crests of waves, such as those of the electromagnetic spectrum. |
| Photon | a tiny particle or packet of light energy |
| Electromagnetic Spectrum | arrangement of electromagnetic radiation--including radio waves, visible light from the Sun, gamma rays, X rays, ultraviolet waves, infrared waves, and microwaves--according to their wavelengths |
| Radiation | energy that is radiated or transmitted in the form of rays or waves or particles |
| Quantization | process of measuring the amplitude or energy of each sample at that point in the waveform-also increases dynamic range |
| Line Emission Spectra | when light from excited atoms of an element is passed through a prism, distinct colored lines are produced which can be used to identify the element. |
| Energy Level | a region of an atom in which electrons of the same energy are likely to be found |
| Sublevel | One part of a level, each of which can hold different numbers of electrons |
| Orbital | a region in an atom where there is a high probability of finding electrons |
| Electron Configuration | the ways in which electrons are arranged in various orbitals around the nuclei of atoms |
| Uncertainty Principle | The idea that we do know no anything for certain and all we know is possibilities, probabilities, and tendencies. Put forth by German physicist Heisenberg. |
| Pauli Exclusion Principle | no two electrons in the same atom can have the same set of four quantum numbers |
| Absorption | The Process of when and atom takes in Light and converts it into energy. Opposite of Reflection |
| Emission | something sent out; putting into circulation |
| J.J Thomson's Model | Thomson's model described the atom as a positively charged sphere, in which negatively charged particles were scattered. (Like raisins in bread pudding.) |
| Dalton's Model | described atoms as the smallest particle of matter ; indivisible; developed the Atomic Theory |
| Rutherford's Model | atoms possitively charged particles were contained in the nucleus, the negatively charged electrons were scattered outside the nucleus around the edge |
| Bohr Model | model of the atom in which electrons move rapidly around the nucleus in paths called orbits |
| Quantum Mechanical Model | determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus |
| Ground State | the lowest energy state of an atom |
| Excited State | a state in which an atom has a higher potential energy than it has in its ground state |
| Excitation | The process of an electron jumping to a higher energy level in its atom. |
| Relaxation | The process of an electron coming back to its original energy level in its atom. |
| Ion | atom that has a positive or negative charge |
| Cation | a positively charged ion |
| Anion | a negatively charged ion |
| Ionic bond | a chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion |
| Crystal Lattice | a 3-dimensional geometric arrangement of the atoms or molecules or ions composing a crystal |
| Atomic Radius | one-half the distance between the nuclei of identical atoms that are bonded together |
| Ionization Energy | the amount of energy required to remove an electron from an atom |
| Ionic Radius | Distance from the center of an ion's nucleus to its outermost electron |
| Ionic compound | a compound that consists of positive and negative ions |
| Binary Compound | chemical compound composed of only two elements |
| Formula Unit | the lowest whole-number ratio of ions in an ionic compound |
| Octet rule | States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons |
| isoelectronic | having the same number of electrons |
| Coulomb's Law | electric force between charged objects depends on the distance between the objects and the magnitude of the charges. |
| Shielding | The more electrons there are to hold on to, the more the strength of the nucleus gets diffused |
| Mole | the SI base unit used to measure the amount of a substance whose number of particles is the same as the number of atoms of carbon in exactly 12 g of carbon-12 |
| Avogadro's Number | number of representative particles in a mole, 6.02 X 10^23 |
| Molar Mass | the mass of one mole of a pure substance |
| Covalent Bond | a chemical bond that involves sharing a pair of electrons between atoms in a molecule |
| Lone pair | Pair of electrons associated with one atom in a molecule and not involved in bonding. |
| Molecule | two or more atoms held together by covalent bonds |
| Polyatomic Ion | a charged group of covalently bonded atoms |
| Covalent Compound | a chemical compound formed by the sharing of electrons |
| Lewis Structure | a structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds. |
| VSEPR model | Valence Shell Electron Pair Repulsion model, which is based on an arrangement that minimizes the repulsion of shared and unshared pairs of electrons around the central atom |
| Electron Geometry | the arrangement of electron domains about the central atom |
| Electron regions | electron cloud, the area of possibilities in which the electrons could be in a general region. |
| Bond Angle | the angle formed by two bonds to the same atoms |
| Electronegativity | a measure of the ability of an atom in a chemical compound to attract electrons |
| Polar covalent bond | a covalent bond in which electrons are not shared equally |
| non-polar covalent bond | A covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge |
| Bond Dipole | an indicator in a Lewis structure that shows which element is more electronegative |
| Lone Pair Dipole | no bond, just a lone pair, unshared |
| Symmetric Dipoles | there are equal forces on each side that cancel each other out, no net dipole because they fully cancel |
| Net dipole | the overall direction of partial negative charge in a molecule |
| Molecular Polarity | the uneven distribution of molecular charge |
| Polar Molecule | molecule with an unequal distribution of charge, resulting in the molecule having a positive end and a negative end |
| Intermolecular Forces | forces of attraction between molecules. The following types are: London Dispersion Forces, Dipole-Dipole Forces, and Hydrogen Bonds |
| Dipole-Dipole Forces | attractions between oppositely charged regions of polar molecules |
| Hydrogen Bonds | attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom |
| London Dispersion Forces | the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles |
| Temporary Dipole | An atom or molecule in which the spatial center of positive charge is momentarily different from the center of negative charge. |
| Percent Composition | the percent by mass of each element in a compound |
| Empirical Formula | a formula showing the lowest whole number ratio of atoms in a compound |
| Solution | A homogeneous mixture of two or more substances |
| Solute | the dissolved substance in a solution |
| Solvent | the substance in which the solute dissolves |
| Dissolving | the process of going into solution |
| Ion-Dipole Bonding | Attraction between an ion and a dipolar molecule |
| Homogeneous Mixture | a mixture in which substances are evenly distributed throughout the mixture |
| Heterogeneous Mixture | a mixture in which different materials can be distinguished easily |
| Saturated | being the most concentrated solution possible at a given temperature |
| Unsaturated | solution in which it is possible for more solute to be dissolved |
| Concentrated | a solution containing relatively large amounts of solute |
| Dilute | make (a liquid) less concentrated; reduce in strength; Ex. dilute the influence of the president |
| Soluble | capable of being dissolved |
| Insoluble | not able to dissolve |
| Electrical Conductivity | how well a substance allows electricity to flow through it. |
| Hydration Energy | the attraction between ions and water in the solution; the change in energy when gaseous ions dissolve in water |
| Lattice Energy | the energy released when one mole of an ionic crystalline compound is formed from gaseous ions |
| Entropy | a measure of the disorder of a system |
| Dynamic Equilibrium | result of diffusion where there is continuous movement of particles but no overall change in concentration |
| Concentration | the strength of a solution |
| Molarity | concentration measured by the number of moles of solute per liter of solvent |
| Dilution | the process of adding solvent to lower the concentration of solute in a solution |
| Volumetric Flask | used to make solutions of known concentration, accurate liq. vol. measurement |
| Graduated Pipet | Used to deliver precise volumes of liquids |
| Organic Molecule | carbon-based molecule |
| Structural Formula | an expanded molecular formula showing the arrangement of atoms within the molecule |
| Line-Angle Drawing | zig zag format of how many bonds are in the molecule double lines for double bonds etc. and draw in the bond angles for each one |
| HydroCarbon | an organic compound containing only carbon and hydrogen |
| Functional Group | the portion of a molecule that is active in a chemical reaction and that determines the properties of many organic compounds |
| Alcohol | -ol |
| Amine | -Amine, -Amino, -ine |
| Carboxylic Acid | -(o)ic Acid |
| Ester | -Oate |
| Amide | -Amide |
| Metallic Bonding | the chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
| Covalent Network | this solid consists of atoms held together throughout the entire sample of material in large networks or chains by covalent bonds, and has a high melting point |
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