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21 Cards in this Set
- Front
- Back
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Chemical Bond |
a force of attraction that holds two or more atoms together. Changes identifying properties of that material. |
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Properties |
Characteristics used to identify. |
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Electrostatic attraction |
attraction between opposite charges. |
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Ionic Bonds |
result from transfer of electrons |
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Covalent Bonds |
A force of attraction that results from sharing pairs of electrons between two atoms. |
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Metallic Bonds |
result from sharing electrons among many atoms. |
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Octet |
a group of 8 electrons in the outer level |
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Octet Rule |
all atoms of all elements will do whatever they can to make an octet. Metals will lose electrons and nonmetals will gain. |
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Isoelectronic |
having the same number of valence electrons as a noble gas. |
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Properties of Ionic Compounds |
1. Solid 2. Brittle, not malleable 3. High melting point 4. Crystalline 5. Form ionic lattice |
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Covalent substances |
1. Can be any phase (solid, liquid, gas) Solids have a low melting point and can sublime (solid to gas) |
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Diatomic Gases |
two atoms of elements bonded to one another covalently. |
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Isomers |
Compounds having the same formula but different structures |
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Resonance Structure |
When there are two or more equivalent structures for the same molecule |
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VSEPR Concept |
valence shell electron pair repulsion |
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polarity |
if symmetrical, nonpolar if non symmetrical, polar |
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Electronegativity |
the measure of an atoms ability to attract electrons. |
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Electronegativity |
the measure of an atoms ability to attract electrons. |
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bond measurement |
single bonds > double bonds > triple bonds |
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exceptions to octet rule |
1. if total # of electrons is an odd number 2. An atom that has less than an octet 3. An atom that has more than an octet |
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Formal Charge |
1. All unshared non bonding electrons are assigned to the atom in which they are found 2. Half of the bonding electrons are assigned to each atom that shared the bond formal charge= (# Val electrons in an isolated atom) - (# Val electrons assigned in Lewis structure atom) a. Atoms have the lowest formal charge b. Any negative formal charge reside in more electronegative atoms c. for a neutral molecule the most preferable Lewis structure is one where there are no formal charges d. Lewis structures w small formal charges are preferable to those w large formal charges |
