Chemistry Terms and Concepts: Oxidation, Reduction, Bonds, Gas Laws, and Atomic Structure, Quizzes of Chemistry

Download Chemistry Terms and Concepts: Oxidation, Reduction, Bonds, Gas Laws, and Atomic Structure and more Quizzes Chemistry in PDF only on Docsity! TERM 1 oxidation DEFINITION 1 loss of electrons in an oxidation reduction reaction TERM 2 reduction DEFINITION 2 gaining of electrons in an oxidation reaction TERM 3 ionic bond DEFINITION 3 metal and nonmetal transferred nonmetal = anion TERM 4 covalent bond DEFINITION 4 nonmetal and nonmetal shared, not always equally most stable lowest Potential Energy TERM 5 Boyle's Law DEFINITION 5 P1V1 = P2V2 TERM 6 Charles Law DEFINITION 6 V1 / T1 = V2 / T2 TERM 7 Avogadro's Law DEFINITION 7 V1 / N1 = V2 / N2 TERM 8 Gay-Lussacs Law DEFINITION 8 As temperature increases in a fixed of gas, the pressure increases. Aerosol can in fire = explode TERM 9 STP DEFINITION 9 standard temperature and pressure 1 mol = 22.4 L 273.15 Kelvin = 0 degrees Celcius TERM 10 Dalton's Law DEFINITION 10 Ptotal = Pa + Pb + Pc smaller particles travel faster TERM 21 speed of light DEFINITION 21 3.00 x 10^8 m/s = wavelength times frequency TERM 22 specific heat capacity DEFINITION 22 measure of a systems ability to absorb thermal energy without having a large temperature change. TERM 23 electromagnetic spectrum DEFINITION 23 radio - microwaves - infrarred - visible light - ultra violet - xrays - gamma radio - longest wavelengths and lowest energy gamma - shortest wavelengths and highest energy 750 - red - radio 400 - violet - gamma TERM 24 Bohr Model DEFINITION 24 model to explain the atomic spectra. electrons orbit around fixed distances - quantized orbits = stationary states. nothing can exist between these orbitals. only when an electron jumped or made a transition, from one stationary state to another that radiation was emitted or absorbed. TERM 25 Quantum Mechanical Model DEFINITION 25 explains how electrons exist in atoms and how those electrons determine the chemical and physical properties of elements. explains why. explains the modern periodic table and provides basis for our understanding of chemical bonding. TERM 26 de Brogile wavelength DEFINITION 26 wavelength = h/mv h = planck's constant = 6.626 x 10^-34 m = mass v = velocity TERM 27 Heisenburg's Uncertainty Principle DEFINITION 27 DX x MDV is greater than or equal to h/4pi DX = uncertainty of the position DV = uncertainty of the velocity TERM 28 Schrodinger Equation DEFINITION 28 HY = EY H = Hamiltonian Operator = represents the total energy of an electron of an atom Y1 = wave function E = actual energy at a given time. Y2 = plotted; gives probability distribution map. TERM 29 Spin quantum number DEFINITION 29 determines spin direction comes from Pauli exclusion principle TERM 30 Orbitals with the same principle quantum number (n)... DEFINITION 30 ... are in the same principle level (shell). TERM 31 Orbitals with the same value for n and l... DEFINITION 31 ... are in the same sublevel (shell). TERM 32 Pauli Exclusion Principle DEFINITION 32 no two electrons in an atom can have to same 4 quantum numbers. no more than two electrons can be in each orbital. TERM 33 Aufabau Principle DEFINITION 33 lowest energy levels will be filled first. TERM 34 Hund's Rule DEFINITION 34 when filling degenerate orbitals, first fill singly with parallel spins. TERM 35 Valence Bond Theory DEFINITION 35 based on overlap of orbitals. hybridizes. stays atomic.