Bonding and States of Matter
Review ionic, covalent, and metallic bonding and how structure explains properties.
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Questions Covered in This Set
10 cards to master
Why do atoms form chemical bonds?
To get closer to a full outer electron shell, which makes them more stable.
Ionic bonding forms between which types of elements, and how?
Between a metal and a non-metal: the metal transfers outer electrons, forming positive metal ions and negative non-metal ions held by strong electrostatic attraction in a giant lattice.
Why does solid NaCl not conduct electricity, but molten or dissolved NaCl does?
In the solid the ions are locked in the lattice; when molten or dissolved the ions are free to move and carry charge.
Why is the formula of magnesium chloride MgCl₂?
Charges must balance: one Mg²⁺ needs two Cl⁻ ions.
Why do simple molecular substances like CO₂ have low melting and boiling points?
Only the weak intermolecular forces between molecules are broken on melting/boiling — the strong covalent bonds inside molecules stay intact.
Compare diamond and graphite structures.
Diamond: each carbon bonded to 4 others in a rigid 3D network — very hard, non-conducting. Graphite: each carbon bonded to 3 others in layers with weak forces between layers — slippery, and conducts via one delocalised electron per atom.
Describe metallic bonding.
A lattice of positive metal ions attracted to a 'sea' of delocalised outer electrons.
Why are metals malleable but alloys harder?
Metal ion layers can slide past each other without breaking bonding; in alloys differently sized atoms distort the layers so they can't slide easily.
Why are ionic compounds brittle?
If layers are knocked out of alignment, like charges line up and repel, cracking the crystal.
How does bond strength relate to states of matter?
Stronger forces between particles mean more energy is needed to separate them, so higher melting and boiling points.
