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CHEM 3
Chemistry Unit 3 Review
| Term | Definition |
|---|---|
| Molecular Compounds | form covalent bonds by sharing electrons |
| Ionic compounds | form by giviing up or recieving electrons |
| electron dot notation | a diagram that shows an element with its valence electrons surrounding it |
| Molecule | a group of atoms with a neutral charge held together by covalent bonds |
| Molecular Geometry | The three-dimensional arrangement of the atoms in a molecule |
| Cation | a positively charged ion formed when a neutral atom loses electrons |
| Metallic Bonding | A type of chemical bonding that is caused by the electrostatic attraction of electrons in the electron sea for the nuclei of metal atoms |
| Metalloid | An element that is not as malleable as a metal but not as brittle as a nonmetal, and which will conduct electricity under certain conditions |
| Electron Affinity | The amount of energy released when a neutral atom gains an electron to become an anion |
| Lewis structure | a chemical formula that uses element symbols to represent nuclei and inner shell electrons, dot pairs or dashes to represent electron pairs in covalent bonds and single or paired dots arranged around the symbol to represent unshared electrons. |
| Polyatomic ions | Covalently bonded atoms that function as a whole and have either a surplus or deficit of electrons, giving them a positive or negative charge |
| Nonpolar Bond | a covalent bond in which the force of attraction for the shared pair of electrons is exerted equally by all of the atoms in the molecule |
| London Dispersion Forces | intermolecular forces created by temporary dipoles that result from the movement of electrons in the atoms within molecules |
| Hydrogen Bond | force that forms between an unshared pair of electrons on one molecule and a hydrogen atom bonded to a strongly electronegative atom on another molecule |
| dipole-dipole forces | intermolecular forces resulting from the attraction of the negative portion of the dipole of a polar molecule to the positive portion of the dipole of an adjacent polar molecule |
| hybridization | the mixing of two or more orbitals of different energy levels on the same atom to produce new hybrid orbitals |
| Bond energy | The energy required to break a chemical bond and form neutral atoms |
| Valence electrons | electrons that occupy the highest energy level of an atom of a particular element and determine its chemical properties |
| luster | the name of the ability of a substance to shine by reflecting light |
| ductility | the ability of a substance to be drawn, pulled, stretched, or extruded into a wire |
| octet | a full s and p sublevel (eight electrons) that completes the outer electron shell of an atom and makes the element very stable and chemically nonreactive |
| malleability | the ability of a substance to be hammered, shaped, or beaten into thin sheets |
| ionization | The amount of energy required to remove one electron from a neutral atom of an element |
| Dmitri Mendeleev | Russian chemist and teacher who is given credit for compiling the Periodic Table of Elements |
| Periodicity | the repetition of chemical properties among elements when they are arranged according to their atomic numbers |
| Henry Moseley | the English physicist who discovered that periodicity is based on atomic numbers |
| Ionic Bond | A type of chemical bond in which positively charged cations and negatively charged anions are held together by electrostatic attraction |
| Resonance | The property of certain molecules or ions that exhibit the characteristics of more than one bond structure at the same time and cannot be represented by a single Lewis structure |
| VSEPR | a theory that states that repulsion between valence-level electron pairs surrounding the central atom in a molecule causes them to be oriented as far apart as possible |
| Polar covalent bond | a covalent bond in which the force of attraction for the shared pair of electrons is more strongly exerted by the atom with the greater electronegativity |
| electronegativity | The measure of the ability of an atom of one element to attract electrons from an atom of another element to form a compound |
| The real basis of periodicity of elements is the electron ___ of their atoms. | Configuration |
| Ionic Radius | The measure of the size of an ion |
| Monoatomic Ions | Positive or negative ions consisting of only one atom |
| octahedral | molecule with 6 atoms bonded to a central atom with no unshared electrons which form an octahedron, such as SF6 |
| tetrahedral | molecule with 4 atoms bonded to a central atom with no unshared pairs of electrons, such as CH4 |
| T-shaped | molecule with 3 atoms bonded to a central atom with 2 unshared pairs of electrons, such as CIF3 |
| Linear | molecule with 2 atoms bonded to a central atom with no unshared electrons, such as BeF2 |
| trigonal bipyramidal | molecule with 5 atoms bonded to a central atom with no unshared electrons that form the vertices of a bipyramid, such as PCl5 |
| trigonal pyramidal | molecule with 3 atoms bonded to a central atom with 1 pair of unshared electrons, such as NH3 |
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