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| ionic compounds are formed by the transfer of electrons from one atom to another |
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| lose all valence electrons to form positive ions with stable outer octet of electrons (noble gas configuration) |
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| gain electrons to form negative ions with stable outer octet of electrons (noble gas configuration) |
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| how to spot ionic bonding |
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Definition
look at formula. For an ionic bond you will always see:
METALS (first) bonded to NONMETALS(second)
EX: CaCl2—> Ca=metal
Cl2=nonmetal |
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| electronegativity and ionic bonding |
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Definition
| The larger the difference in electronegativity between two atoms in a bond the more ionic the bond is. (Subtract the electronegativity value for one atom from the value for the second atom in the bond.) |
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Term
| Electronegativity difference is small (less than 1.7) |
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Definition
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| electronegativity difference is large (greater than 1.7) |
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| atoms with 8 electrons in the valence shell are stable (2 electrons formH, He, and Be.) |
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| atoms form a chemical bond by gaining, losing, or sharing electrons in order to form an octet in the valence shell |
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Definition
- metal/nonmetal bond is always ionic
- electronegativity greater than 1.7 is ionic. Less than 1.7 is covalent
- metals bonded to polyatomic ions (table E) contain both ionic and covalent bonds.
Ex: CaCO3 or Na2SO4 |
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| basis properties of ionic compounds |
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Definition
- ionic solids are poor conductors of heat and electricity but when liquid or in solution (electrolyte) they are good conductors
- ionic solids are giant crystals lattice structures
- formula units for ionic solids are empirical formulas (lowest whole number ratio)
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