3.3 Ionic Bonding Flashcards
Forming metal ions
-Metal atoms tend to lose all of their outer-shell electrons to get a full outer-shell.
-They become positively charged ions and they are more stable.
-Loss of electrons is also called oxidation.
-The ion has a 2+ charge because it lost two electrons.
Forming non-metal ions
-Non-metal atoms tend to gain electrons to fill their outer-shell.
-They become negatively charged ions and they are more stable.
-Gain of electrons is called reduction.
-The ion has a 1− charge because it gained one electron
What are the things to check when forming ionic compounds?
Check for full outer shells in ions, balance charges (+ and -).
Forming ionic compounds
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-Metals transfer electrons to non-metals during reaction, forming ions with stable outer shells.
-Example: Lithium (Li) loses 1 electron, oxygen (O) gains 2 electrons.
-Ratio: 2 Li atoms for every O atom.
-Li atoms oxidize (lose electrons), O atoms reduce (gain electrons).
-Resulting ions: Li ions have 1+ charge, O ion has 2- charge.
Ionic structure
-In an ionic compound, ions are arranged in a giant ionic lattice
-The ions alternate: + - + - etc.
Ionic bonding
-Ionic bonding is the electrostatic attraction between oppositely charged ions.
-Always a very strong attraction
Why do ionic compounds have high melting points?
- Ionic bonds are very strong
- In a giant ionic lattice there are lots of ionic bonds
- Breaking all the ionic bonds requires a large amount of energy
-Some ionic compounds have higher melting points because their ions have higher charges.
-This makes the attraction between the ions even stronger and harder to break:
Can solids conduct electricity?
Solids (s):
-No conductivity
-Ions can’t move freely
Can liquids conduct electricity?
Liquids (l) or dissolved (aq):
-High conductivity
-Ions can move freely
Why do the nobles gases (Group 0) not readily react?
The noble gases are inert (unreactive) because they have a full outer shell of electrons.
