Bonding: Ionic Bonding Flashcards

1
Q

Definition of Ionic Bonding

A
  • Ionic bonding involves electrostatic attraction between oppositely charged ions in a lattice
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2
Q

Compound Ions: Ammonium, carbonate, hydroxide, nitrate, sulfate, hydrogensulfate, phosphate

A
  • Ammonium - NH4 +
  • Carbonate - CO3 2-
  • Hydroxide - OH -
  • Nitrate - NO3 -
  • Sulfate - SO4 2-
  • Hydrogensulfate - HSO4 -
  • Phosphate - PO4 3-
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3
Q

Giant Ionic Lattices

A

• Ionic crystals are giant lattices of ions

  • A lattice is a regular repeated three-dimensional arrangement of ions/molecules/atoms in a solid
  • The structure is ‘giant’ because it’s made of the same basic unit repeated over and over again
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4
Q

Properties of Ionic Compounds: Melting Point

A
  • Ionic compounds have high melting points
  • They have lots of strong electrostatic forces of attraction between oppositely charged ions
  • These require a lot of energy to break
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5
Q

Properties of Ionic Compounds: Electrical Conductivity

A
  • As solids, ionic compounds cannot conduct heat/electricity because their ions are bonded together in the lattice and can’t move
  • When liquid (molten) or in solution the ions can break free of the lattice and are able to move
  • The ions are charged particles and so can carry heat and an electric current
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6
Q

Properties of Ionic Compounds: Solubility

A
  • Ionic compounds are usually soluble in water because water molecules are polar and have delta-positive/negative charges that can attract the ions away from the lattice, causing the compound to dissolve
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7
Q

Factors which Affect the Strength of Ionic Bonds

A

• Charge on the ions
- The bigger the charge on the ion, the stronger the ionic bonding

• Size of the ions
- The smaller the ions, the stronger the ionic bonding

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