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Final Exam Terms 1
Final Exam Terms
| Question | Answer |
|---|---|
| Diatomic Elements | H2, N2, O2, F2, Cl2, Br2, I2 |
| Law of Conservation of Mass | Matter is neither created nor destroyed. Total mass stays the same during a chemical reaction. |
| Law of Conservation of Energy | Energy is neither created nor destroyed |
| kilo | Symbol K. Factor 10^3. Ex: 1 km = 1000m or 1m = 0.001 km. |
| Centi | Symbol C. Factor 10^-2. Ex: 1 cm = 0.01 m or 1 m = 100 cm. |
| Milli | Symbol M. Factor 10^-3. Ex: 1 mm = 0.001 m or 1 m = 1000 mm. |
| Memorize | 1 mL = 1 cm^3 |
| Temp (K) = | Temp (°C) + 273.15 |
| Kilograms To Grams | 1 kg = 1000 g |
| Inches To Feet | 12 in = 1 ft |
| Feet To Meters | 3.2808 ft = 1 m |
| Centimeters To Meters | 100 cm = 1 m |
| Millimeters to Meters | 1000 mm = 1 m |
| Kilometers To Meters | 1 km = 1000 m |
| Inches To Centimeters | 1 in = 2.54 cm |
| Grams To Milligrams | 1 g = 1000 mg |
| Liters To Milliliters | 1 L = 1000 mL |
| Avogadro's # | 1 mole = 6.022 x 10^23 things |
| Grams To Moles | Use Molar Mass |
| Moles To # Of Things | Use Avogadro's # |
| Grams To Milliliters | Use Density |
| Democritus | Greek philosopher who said matter is made of tiny, indivisible particles called atoms. |
| Atom (Atomos) | Means “indivisible”; the smallest piece of matter according to Democritus. |
| Aristotle | Greek philosopher who believed matter was made of fire, water, earth, and air and could be divided infinitely. |
| Law of Definite Proportions | A compound always contains the same elements in the same fixed ratio by mass. |
| Dalton’s Atomic Theory | Theory stating that matter is made of atoms, elements have one type of atom, and compounds form in fixed whole-number ratios. |
| J.J. Thomson - Cathode Ray Tube Experiment (1897) | The experiment determined that the particles: are negatively charged, weigh much less than atoms, are the same regardless of source material, we call these particles e^- (electrons). |
| Millikan Oil Drop Experiment (1909) | The experiment determined: the charge of electron (magnitude) & mass of the electron. |
| Thompson - Plum Pudding Model (1904) | Atom is a positive mass with negatively charged electrons embedded in it. |
| Hantaro Nagaoka - Saturn Like Model (1903) | Positively charged sphere with ring of electrons around it. |
| Rutherford - Gold Foil Experiment (1911) | The experiment determined that atoms: are largely empty space, have a dense, positively charged nucleus, surrounded by electrons. (Later discovered the proton). |
| Fredrick Soddy - Discovered Isotopes (1913) | Atoms with the same chemical properties, but different masses. |
| James Chadwick - Discovered The Neutron (1932) | Happened later because neutrons are neutral and don't interact with electronic and magnetic fields. |
| Proton | Symbol P. Relative Charge +1. Mass ~1 amu. |
| Neutron | Symbol N. Relative Charge 0. Mass ~1 amu. |
| Electron | Symbol E. Relative Charger -1. Mass 5.5 x 10^-4 amu. |
| Atomic Number | Number of protons in an atom. |
| Mass Number | Number of protons + number of nuetrons. |
| Ex: 15 N 7 | Protons: 7. Neutrons: 8 (15-7). Electrons: 7. |
| Isotopes | Atoms of an element that have different numbers of neutrons. Ex: ^12C, ^13C, ^14C. |
| Atomic Mass Equation = | (mass isotope 1 × fractional abundance 1) + (mass isotope 2 × fractional abundance 2) or (m₁ × %₁) + (m₂ × %₂) |
| Dual Nature of Light | Light acts as both a wave and a particle. |
| Wavelength (λ – lambda) | The distance between two crests or two troughs of a wave; measured in meters (m) or nanometers (nm). |
| Amplitude | The height of a wave from the center line to the crest; shows the wave’s energy. |
| Frequency (ν – nu) | Number of complete waves passing a point each second; measured in 1/s, s⁻¹, or Hz. |
| Speed of Light (c) | A constant value: 3.00 × 10⁸ m/s. |
| The relationship between wavelength, frequency, and speed: | c = λν |
| Electron Behavior | Electrons move in a large region outside the nucleus, and their behavior is closely linked to the behavior of light. |
| Electromagnetic Spectrum | Different types of EM radiation have different λ. |
| Refraction | Light changes path when it enters a new material. |
| Diffraction | Light bends when it passes through a slit around the size of the wavelength. |
| Interference | When waves collide, overlapping crests make brighter (or bigger) crests, and colliding crests and troughs cancel each other. |
| Particle Nature of Light | Idea that light behaves like particles (not just waves) to explain certain phenomena that classical physics could not. |
| Blackbody Radiation | Hot materials glow and change color with temperature; classical wave physics could not explain this behavior. |
| Photoelectric Effect | Light of a certain minimum frequency knocks electrons off a metal; higher frequency → higher energy electrons. |
| Threshold Frequency | The minimum frequency needed for light to eject electrons from a metal; brightness cannot substitute for this. |
| Photon | A particle or “packet” of light with a specific amount of energy. |
| Photon Energy Equation | E = hν. Where E = energy (Joules), h = Planck’s constant (6.626 × 10⁻³⁴ J·s), ν = frequency of light. |
| Key Finding of Photoelectric Effect | Energy of light depends on frequency, not brightness; brightness only increases the number of photons/electrons. |
| Ephoton = | hv |
| Etotal = | # photons x Ephoton |
| Photoelectric Effect | Minimum-energy photons knock electrons off a metal; higher frequency → more energetic electrons; brighter light → more electrons emitted. |
| Atomic Spectra | Atoms emit light at specific wavelengths (line spectra); each element has a unique pattern. |
| Bohr Model | Electrons move around nucleus in quantized energy levels; absorb energy → move up, release energy → move down, emitting photons. |
| Energy Level | Allowed region of electron energy. |
| Absorption | Electron gains energy → moves to higher level. |
| Emission | Electron loses energy → moves to lower level. |
| Ground State | Lowest energy level. |
| Excited State | Higher energy level. |
| Bohr Equation for Wavelength | 1/λ=1.10 x 10^7 m^-1 (1/n^2final − 1/n^1initial). n = energy level number. |
| Density Equation = | Mass/Volume |
Created by:
LaurenMaue
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