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Chemistry test 3 (2)
Chapters 7-9
| Term | Definition |
|---|---|
| electronegativity | the tendency for an atom to attract an electron pair toward itself - the higher, the greater its tendency to gain electrons |
| electronegativity trends | increases from left to right, decreases down |
| polar molecule | a molecule with a positive pole and a negative pole |
| polar covalent bond | one atom is partially positive and the other is partially negative - difference in electronegativities is >0.5, <1.2 |
| nonpolar molecule | a molecule with a symmetrical distribution of electrons |
| nonpolar covalent bond | the electrons are distributed symmetrically between the bonded atoms - difference in electronegativities is 0.4 or less |
| ionic bond | the difference in electronegativities of the two atoms bonding is greater than or equal to 1.2 |
| valence bond theory | a model of bonding in which a bond arises from the overlap of atomic orbitals on two atoms to give a bonding orbital with electrons localized between the atoms |
| 3 tenets of valence bond theory | valence atomic orbitals of adjacent atoms overlap, each pair of overlapping valence orbitals is occupied by 2 valence electrons to form a chemical bond, valence electrons are either involved in bonding b/w 2 atoms or reside on a single atom |
| molecular orbital theory | a model of bonding in which pure atomic orbitals combine to produce molecular orbitals that are delocalized over two or more atoms |
| orbital overlap | the partial occupation of the same region of space by orbitals on adjacent atoms |
| sigma bond | a bond formed by the overlap of orbitals head to head and with bonding electron density concentrated along the axis of the bond |
| hybrid orbitals | equal-energy orbitals that are the combination of an atom’s atomic orbitals |
| sp | linear |
| sp2 | triangular planar |
| sp3 | tetrahedron |
| sp3d | trigonal bipyramid |
| sp3d2 | octahedron |
| pi bond | the two orbitals overlap to form a bond where the bonding region is above and below the internuclear axis |
| bond energy | reactants - products |
| cis-trans isomer | the central atoms must have two different atoms bonded to them |
| atomic radii trend | decreases from left to right, increases down |
| ionization energy trend | increases from left to right, decreases down |
| linear bond angle | 180 |
| trigonal planar bond angle | 120 |
| tetrahedral bond angle | 109.5 |
| trigonal bipyramid bond angle | equatorial 120, axial 90 |
| octahedral bond angle | 90 |
| double bond | 1 sigma bonds and 1 pi bond |
| triple bond | 1 sigma bond and 2 pi bonds |
| formal charge | valence electrons - lone pair electrons - number of lines = |
| bond order | number of lines/number of places |
| transition metals lose | s electrons 1st to make a cation |
| atomic radii in cations/anions | smallest radii = most protons, biggest radii = least protons |
Created by:
imr36093
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