Term
| reactivity depends on ---- & is why----- |
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Definition
| valence electrons...why similar groups have similar properties. |
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Term
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Definition
force that holds two atoms together
attaction between + & - ions
'' between + nucleus to a - nucleus
types-
ionic
metallic
covelant |
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Definition
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Term
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Definition
lose electrons
end in -ide |
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Term
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Definition
| energy realeased when forming a negetive ion |
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Term
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Definition
| energy added when forming a positive ion |
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Term
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Definition
| electrostatic force holds opposite ions together |
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Definition
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Definition
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Term
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Definition
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Term
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Definition
+ and - ions are packed in a regularly repeating pattern
no singular units |
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Term
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Definition
structure:
positive and negative ions surround eachother |
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Term
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Definition
high melting points
brttle, hard, rigid
non conductor (tightly paked)
conduct in water (electrolyte) |
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Term
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Definition
putting off energy
forming ionic compounds is always exothermic |
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Term
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Definition
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Term
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Definition
energy required to seperate an ionic bond
endothermic
"put released energy back in bond to seperate ions"
more negetive lattice= stronger force
smaller ion-more negative
larger + or - charges = more negative lattice |
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Term
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Definition
| the simplest ratio of ions represented in an ionic compound |
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Term
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Definition
the charge of an ion (2-,+)
rep elements: # of valence electrons it will form= o #
trans switch sometimes |
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Term
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Definition
Symbol
Oxidation #
Cross it
charges=0
metal 1st
Lowest ratio possible |
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Term
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Definition
metal (cation)+
[nonmetal (anion)+ ide] |
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Term
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Definition
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Term
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Definition
ions made up of more than one ion
name= cation+polyatomic ion
Al2(CO3)2 |
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Term
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Definition
per---ate= most oxygen
-ate= 1 less |
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Term
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Definition
valence electrons are shared
delocalised-mobile elrctrons
cations |
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Term
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Definition
| cation atracted to delocalized electrons |
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Term
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Definition
incresed #= harder
outer s and inner d electrons |
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Term
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Definition
mixture of metals
form w/ similar size or much smaller |
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Term
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Definition
| no replacing but forming w/ ions in between |
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