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KMHS_Chemistry
Chapter 14/15 Vocabulary and Practice
| Question | Answer |
|---|---|
| How many valence electrons does S have? | 6 |
| How many valence electrons does O-2 have? | 8 |
| Electron Dot Structure | a notation that depicts balence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus |
| Ionic Bond | the electrostatic attraction that binds oppositely charged ions together |
| Octet Rule | atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas. there are usually eight electrons (two for hydrogen) |
| Valence Electron | an electron in the highest occupied energy level of an atom |
| Covalent Bonds | A molecule is composed of one or more chemical bonds |
| Dipole | a molecule that has two electrically charged regions, or poles |
| Dipole Interaction | a weak intermolecular force resultion from the attraction of oppositely charged regions of polar molecules |
| Hydrogen Bond | a relatively strong intermolecular force in which a hydrogen atom that is covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of an electronegative atom in the same molecule or one nearby |
| Nonpolar Covalent Bond | a bond formed when the atoms in a molecule ar alike and the bonding electrons ar shared equally |
| Polar Covalent Bond | a bond formed when two differentatoms are joined by a covalent bond and the bonding electrons are shared unequally |
| Polar molecule | a molecule in which one or more atoms is slightly negative, and one or more is slightly positive in such a way that the polarities do not cancel; water is a polar molecule |
| Resonance | a phenomenon taht occures when two or more equally valid electron dot structures can be written for aa molecule; the actual bonding is believed to be ahybrid or mixture of the extremes represented by the resonance forms |
| Structural Formula | a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion; each dash between two atoms indicates a pair of shared electrons |
| Tetrahedral Angle | a bond angle of 109.5 degrees created when a central atom forms four bonds directedtoward the corners of a regular tetrahedron |
| Unshared Pair of Electrons | a pair of balence electrons that is not involved in bonding |
| VSEPR Theory | (valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence-electron pairs are as far apart as possible. |
| Lewis Structure | prediction of the molecular shape |
| Electronegativity | the tendency for an atom to attract electrons to itself when it is chemically combined whith another element |
| Valence Shell | where the valence electrons are found |
| Numer of valence electrons in HCl | 8 |
| Number of valence electrons in P | 5 |
| Number of valence electrons in He | 2 |
| Number of valence electrons in Ar-3 | 11 |
| Number of valence electrons in Si+2 | 2 |
| Number of valence electrons in P | 5 |
| Number of valence electrons in PF5 | 40 |
| Number of valence electrons in I3 -1 | 22 |
| Number of valence electrons in CaCl2 | 16 |
| Number of valence electrons in OCS | 16 |
| Number of valence electrons in HNO3 | 24 |
Created by:
KellyBeck
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