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ADV CHEM
vocab for Unit 4 Test on 12/8.
| Question | Answer |
|---|---|
| chemical bonding | a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
| why do atoms bond | to create a more stable environment (become more stable) |
| significance of valence electrons | they show the atoms chemical bonding |
| octect rule | chemical compounds form by gaining, losing, or sharing electrons so each atom has a full octect (8) of electrons in the highest energy level |
| exceptions to the octect rule | group 13 can form bond with only 6 Hydrogen only needs 2 |
| types of atoms in ionic bond | nonmetals and metals |
| types of atoms in covalent bond | nonmetals and nonmetals |
| ionic | the complete TRANSFER of 1 or more electrons from one atom to another |
| covalent | some valence electrons are SHARED between atoms |
| metallic | hold atoms of a metal together |
| lewis dot structure | shows valence electrons in an element, valence electrons are shown by dots |
| cation | positively charged ion |
| anion | negatively charged ion |
| when do positive ions form in ionic bonds | when the number of electrons are less than the number of protons |
| crystalline lattice | repeated pattern of multiple IONS |
| properties of ionic compounds | strong attractions between ions high melting/boiling points hard and brittle on-volatile soluble conductivity |
| solid ions in lattice structure | ions are so close together with fixed position NO conductivity |
| liquid ions in lattice structure | ions are freely moving due to broken lattice structure |
| molecular compound | a chemical compound whose simplest units are molecules |
| molecular formula | shows the types and numbers of atoms combined in a single molecule of a molecular compound |
| bond pairs | shared electrons (form bonds) |
| lone pairs | unshared electrons (don't form bonds) |
| properties of covalent compounds | low melting/boiling point soft and waxy volatile insoluble poor conductivity |
| polyatomic ions | a charged group of covalently bonded atoms |
| diatomic elements def | always bonded with another element |
| what are the diatomic elements | hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine (the magnificent 7) |
| electronegativity | measure of ability of an atom in a bond to attract electrons |
| different types of electromagnetically (the ranges) | 1.70-4.00 = IONIC 0.40-1.69= POLAR COVALENT 0.00-0.39= COVALENT |
| bond polarity | a covalent bond in which the bonded atoms have unequal attraction |
| metallic bonds | a bond formed by a metal ion (cation) and the sea of electrons that surround it |
| properties of metallic bonds | good conductors malleable |
| VSEPR theory acronym | valence shell electron pair repulsion |
| VSPER theory | predicts the molecular shape of a bonded molecule electrons arrange themselves as far apart as possible unshared electrons repel the most !only look at the central atom! |
| shapes for only bonded electrons around the central atom | linear trigonal planer tetrahedral |
| linear | 2 atoms bonded no lone pairs |
| linear bond angle | 180 |
| linear structural formula | AB or AB2 |
| trigonal planer | 3 atoms attached no lone pairs |
| trigonal planer bond angle | 120 |
| trigonal planer structural formula | AB3 |
| tetrahedral | 4 atoms attached no lone pairs |
| tetrahedral bond angle | 109.5 |
| tetrahedral structural formula | AB4 |
| structures for only bonded and lone pairs | trigonal pyrimidal bent |
| trigonal pyramidal | 3 bonds 1 lone pair |
| trigonal pyramidal bond angle | 107 |
| trigonal pyramidal structural formula | AB3E |
| bent | 2 bonds 2 lone pairs |
| bent bond angle | 104.5 |
| bent structural formula | AB2E2 |
| symmetrical | non polar |
| unsymmetrical | polar |
| 2 types of attraction in molecules | INTRAmolecular INTERmolecular |
| intramolecular forces | the attraction between atoms in molecules |
| intermolecular forces | the attraction between molecules |
| intramolecular examples | ionic, covalent, polar covalent |
| intermolecular examples | dipole-dipole London dispersion forces hydrogen bonding |
| dipole-dipole forces | when molecules have a separation of charge on its poles POLAR |
| hydrogen bonding | the strongest attraction occurs when H is bonded with F, N, or O found withing important biological systems POLAR |
| london dispersion forces | very weak due to small dipoles in nonpolar molecules electrons are moving and there are instants where the charge around an atom are nonsymmetrical POLAR and NONPOLAR |
| instantaneous dipole | eventually electrons are situated ad tiny dipoles form |
| induced dipole | when an instantaneous dipole forms and attracts another molecule |
| resonance structures | bonding in molecules or ions that cannot be correctly represented by a singled Lewis Structure |
Created by:
stella_koe
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