Term
| Metals tend to ____ electrons to acquire stable energy levels, while non-metals tend to ___ electrons to do so |
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Definition
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Term
| Name: the electron pairs around atoms which are not involved in bonding |
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Definition
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Term
| what is the rule that says atoms like 8 electrons around them? |
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Definition
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Term
| name: electron pairs around atoms which are not involved in bonding |
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Definition
| lone pairs or non-bonding pairs |
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Term
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Definition
-different atoms
-same # of valence electrons
-same Lewis structures |
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Term
| name: the situation resulting when more than 1 electron structure can represent a molecule or ion |
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Definition
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Term
| define: the ability of an atom to hold its electrons |
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Definition
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Term
a covalent bond between 2 atoms tends to shift towards the atom with...
what does this do? |
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Definition
the greater electronegativity
creates polarization |
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Term
| When molecules are THIS range in bond length, they are nonpolar covalent |
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Definition
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Term
| To determine the polarity of a non-symmetrical molecule, what must one do? |
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Definition
1. determine the polarity of each bond in the molecule
2. eliminate all bonds which cancel
3. Remaining bonds will determine molecular polarity |
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Term
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Definition
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Term
| What does VSEPR stand for? What does it mean? |
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Definition
Valence Structure Electron-Pair Repulsion [Theory]
states that because electron pairs repel, molecules adjust their shapes so that the valence electron pairs are as far apart as possible |
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Term
| What are the possible electron geometry shapes? |
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Definition
-linear (180)
-trigonal planar (120)
-tetrahedral (109.5)
-trigonal bipyramidal (120/90) |
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Term
| electron pair geometry is... |
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Definition
| the geometry taken up by ALL valence electron pairs in the central atom |
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Term
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Definition
| the arrangement in space of the central atom, and the atoms directly attached to it |
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Term
| Lone pairs of electrons on the central atoms occupy... |
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Definition
| spatial positions even though their locations are not included in the verbal description of the shape of the molecule or ion |
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Term
| Anything beyond the WHAT period can be hypervalent, and anything below WHAT period can be hypovalent? |
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Definition
3-hypervalent
2-hypovalent |
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Term
| WHAT DETERMINES MOLECULAR GEOMETRY? |
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Definition
| ELECTRON PAIR GEOMETRY!!! |
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Term
| In terms of resonance structure, what is going on in reality? |
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Definition
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Term
| Do bond and lone electron pairs in valence shells repel or attract one another? |
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Definition
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Term
| The strength of repulsion between electrons are strongest when what and what are bonded? |
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Definition
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Term
| The top pole of a molecule is called the ___ position |
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Definition
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Term
| The side pole of a molecule is called the ___ position |
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Definition
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Term
| 5 bonds and no valence electrons= |
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Definition
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Term
| 4 bonds and 1 lone pair = |
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Definition
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Term
| 3 bonds and 1 lone pair = |
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Definition
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Term
| 2 bonds and 3 lone pairs = |
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Definition
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Term
| six bonds and no lone pairs = |
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Definition
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Term
| 5 bonds and 1 lone pair = |
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Definition
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Term
V/F: Mult. bonds do not affect the overall molecular shape...
Why/not? |
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Definition
Verum
e- pairs in same region occupy same nuclei/region of space |
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Term
How do you calculate the formal charge of an atom?
Bond length? |
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Definition
group # of atom-dots &dashes
----
dashes/legs |
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Term
| What is pure covalent bonding? |
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Definition
| atoms share e- pairs equally (similar atoms) |
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Term
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Definition
| atoms share e- bonds unequally |
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Term
| Why are certain (polar) atoms more positive/negative? |
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Definition
| differing ionization energies mean that some atoms cannot hold on to their electrons as well, and this means that electrons are attracted to certain atoms more than others |
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Term
| Define: electronegativity |
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Definition
| ability of an atom to attract electrons to itself |
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Term
| When the electron pair geometry is tetrahedral, what are the three possible molecular shapes? (and the degrees of their angles) |
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Definition
-tetrahedral:109.5
-trigonal-pyramidal:107.5
-bent:104.5 |
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Term
| 4 bond pairs and 2 lone pairs = |
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Definition
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Term
| When the electron-pair geometry is a trigonal bipyramid, what are the possible molecular shapes? |
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Definition
-trigonal bipyramid
-seesaw
-t-shaped
-linear |
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Term
| When the electron-pair geometry is an octahedron, what are the possible molecular shapes? |
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Definition
-octahedron
-square pyramidal
-square-planar |
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Term
| What are the angle measurements for an octahedron? |
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Definition
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Term
| When molecules are THIS range in bond length, they are moderately polar covalent |
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Definition
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Term
| When atoms are more polar, what happens to bond length? |
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Definition
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Term
| Molecules that are symmetrical are ___ |
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Definition
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Term
| Electronegativity increases... |
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Definition
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Term
| When molecules are THIS range in bond length, they are very polar covalent |
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Definition
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Term
| When molecules are THIS range in bond length, they are ionic |
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Definition
| greater than or equal to 2 |
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