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Chemistry Honors S1
Study guide for Mr. Feebeck’s semester 1 Chemistry Honors final.
| Term | Definition |
|---|---|
| Compound | Substance made from two or more DIFFERENT elements |
| Molecule | A group of two or more atoms |
| Heterogeneous Mixture | A mixture in which the composition differs throughout |
| Homogeneous Mixture | A mixture in which the composition stays the same throughout |
| Solution | A homogenous mixture composed of two or more substances |
| 1 inch | 2.54 centimeters |
| Intensive Property | Does not vary based on the amount of substance |
| Extensive Property | Varies based on the amount of substance |
| Four Clues of Chemical Change | Energy transfer, color change, production of gas, formation of precipitate |
| Reactant | Starting materials |
| Product | End result |
| Atomic Number | The number of protons in an atom |
| Mass Number | The number of protons and neutrons in an atom |
| Atomic Symbol | Mass number top left, atomic number bottom left, charge top right |
| Empirical Formula | A formula showing the ratio of atoms in a compound, but not the actual numbers |
| Molecular Formula | A formula showing the exact numbers in a compound |
| Covalent Compound | A compound consisting of two non-metal elements |
| Ionic Compound | A compound consisting of a metal and non-metal element |
| Erwin Schrodinger | Quantum mechanical waves |
| John Dalton | Theory that all matter is made up of atoms |
| Antoine Lavoisier | Conservation of mass |
| Robert Millikan | Oil drop + charge on an electron |
| J. J. Thompson | Cathode ray experiment + plum-pudding model of an atom |
| Ernest Rutherford | Gold-foil experiment + nucleus of an atom |
| Dmitri Mendeleev | Periodic table |
| James Chadwick | Neutron discovery |
| Periodic Table Electronegativity | Increases bottom to top, left to right |
| Periodic Table Atomic Radius | Increases top to bottom, right to left |
| Periodic Table Ionization Energy | Increases bottom to top, left to right |
| Periodic Table Ion Radius | Increases bottom to top, right to left |
| Visual Periodic Table Group Order | S, D, P, F |
| Hund’s Rule | All orbitals in a subsection should have one spin-up before any have a spin-up and a spin-down |
| Pauli Exclusion Principle | A spin-up can only be paired with a spin-down |
| Heisenberg Uncertainty Principle | One cannot determine the position and speed of a particle simultaneously |
| Cation | Positively charged ion |
| Anion | Negatively charged ion |
| Aufbau Principle | Order of orbital sub-levels (S, P, D, F) |
| Valence Electron | An electron in the outer-shell of an atom |
| Electrolyte | A medium containing ions that conducts electricity |
| Quantum Number (n) | The orbital number |
| Quantum Number (l) | The shape of the orbital |
| Quantum Number (ml) | The orientation in space of the orbital |
| Quantum Number (ms) | The orientation of the spin axis of an electron |
| Molecular Geometry | Geometry, including lone pairs |
| Electron Geometry | Geometry, excluding lone pairs |
| Sigma Bond | Any primary/initial bond |
| Pi Bond | Any bond following a sigma bond |
| Intermolecular Force | Forces between molecules |
| Intramolecular Force | Forces within molecules |
| Bond Order | Divide the total number of bonds by the number of sigma bonds |
| Resonance | Equivalent lewis dot structures of a molecule |
| Binary acids | Begin with hydro-, end with -ic acid |
| Oxyacids | End with -ous acid |
| Covalent Compound Naming | Use prefixes (di-, tri-, tetra-…) |
| Molarity | Number of moles of solute per liter of solution |
| Solute | Substance being dissolved |
| Solvent | Dissolving medium |
| Maximum Number of Electrons per Shell | 2n² |
Created by:
odebettencourt
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