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Chapter 6

Chemical Bond Mutual electrical attraction between nuclei and valence electrons of dif. atoms that bind together to make stable and happy atoms
Ionic Bonding Chemical bond that is caused by cats and onions combining to become neutral and with out stench
Covalent Bonding Chemical Bond in which electron pairs are shared between 2 unhappy atoms to make both happy (2 atoms of same element)
Polar covalent Unequal pull on electrons that are covalently bonded (.3 and 1.7), balanced distribution of the electrical charge
Non polar Covalent Each atom has equal attraction to the electrons (less than 3), unequal distribution of the electrical charge
Molecules Neutral group of atoms that are held together by covalent compounds
Molecular Compound Chemical compound whose simplest units are molecules
Formation of Covalent Bonds Nuclei and electrons attract each (decreasing the potential energy) while the 2 nucleus and electron clouds repel (increasing potential energy)
Ionic Compound Positive and negative ions that are combined so that the number of + and - charges are =
Formula Unit Simplest collection of atoms from which an ionic compound formula can be established
Lewis Structures formulas representing the atomic symbols of atoms bonding relationships
Lattice Energy Energy that is released when a separated ions come together in a crystal structure from a gas
Polyatomic Ions Charged group of covalently bonded atoms, that add or loose electrons to become one with the world
Metallic Bonding Chemical bonding that results from the attraction between metal atoms the surrounding sea of electrons
Metallic Properties Conductors/ reflector of light/ absorber of light/ Malleable/ Ductile
Metallic Bond Strength Depends on nuclear charge and number of electrons, effects the enthalpy of vaporization
Diatomic Molecules When atoms bond there is a specific shape created, it must be linear because there are only 2 atoms
Hybridization explains how orbitals of an atom become rearranged when the atom forms covalent bonds- produce a new hybrid atomic orbitals of equal energy
Intermolecular Forces Attractive forces that vary in strength, and are generally weaker than bonds that join atoms in molecules
Dipole Created by equal and opposite charges that are separated by a short distance
Dipole-Dipole created by unequal charges, separated by short distances, between polar molecules
Induced Dipole Induce a non-polar molecule to become temporarily polar by attracting its electrons
Hydrogen Bonding Intermolecular force in which the hydrogen atom (which is bonded to a highly electronegative atom) is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
London Dispersion Forces Intermolecular attractions resulting from the constant motion of electrons and the separation of induced dipoles/ increase with atomic mass
Created by: jenniferbauer



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