Bonding

    Cards (79)

    • Ionic bonding
      Charged ions held together by strong electrostatic attractions
    • Formation of ionic bond
      1. Atom gives up electron to another atom
      2. Oppositely charged ions are attracted to each other
    • Molecular ions
      Hydroxide (OH-), Nitrate (NO3-), Ammonium (NH4+), Sulfate (SO4 2-), Carbonate (CO3 2-)
    • Determining formula of ionic compound
      1. Write the two ions
      2. Swap the charges over
      3. Drop the charges to get the subscripts
      4. Simplify the formula
    • Giant ionic structures
      • Cubic arrangement of ions
      • High melting points due to strong electrostatic forces
    • Covalent bonding
      Sharing of electrons between atoms to achieve stable electron configurations
    • Types of covalent bonds
      • Single
      • Double
      • Triple
    • Dative covalent (coordinate) bond

      One atom donates a pair of electrons to another atom
    • Giant covalent structures
      • Graphite: Layers of hexagons with delocalized electrons, can conduct electricity
      • Diamond: Tetrahedral structure with strong covalent bonds, does not conduct electricity
    • Molecular shape

      Determined by number of bond pairs and lone pairs of electrons around central atom
    • Molecular shapes with no lone pairs
      • Linear (2 bond pairs)
      • Trigonal planar (3 bond pairs)
      • Tetrahedral (4 bond pairs)
      • Trigonal bipyramidal (5 bond pairs)
      • Octahedral (6 bond pairs)
    • Molecular shapes with lone pairs
      • Pyramidal (3 bond pairs, 1 lone pair)
      • Bent/Angular (2 bond pairs, 2 lone pairs)
      • Trigonal planar (3 bond pairs, 2 lone pairs)
    • Octahedral
      Molecular shape with 6 bond pairs or lone pairs arranged in an octahedral geometry
    • Pyramidal
      • Molecular shape with 3 bond pairs and 1 lone pair
      • Example: ammonia
    • Bent/Nonlinear
      • Molecular shape with 2 bond pairs and 2 lone pairs
      • Bond angle shrinks from 107 to 104.5 degrees
    • Trigonal planar
      • Molecular shape with 3 bond pairs and 2 lone pairs
      • Bond angle remains at 120 degrees
    • Tetrahedral
      • Molecular shape with 4 bond pairs and 2 lone pairs
      • Bond angle remains at 90 degrees
    • Electronegativity
      The ability for an atom to attract electrons towards itself in a covalent bond
    • The further up and right you go in the periodic table, the more electronegative the element is (excluding noble gases)
    • Polar bond

      Covalent bond where there is a difference in electronegativity between the atoms, resulting in an uneven distribution of electrons
    • Polar bonds

      • H-Cl
      • H2O
    • Non-polar bonds

      • Cl2
      • Hydrocarbons
    • Intermolecular forces
      Weak forces between molecules, not within covalent bonds
    • Van der Waals forces
      • Weakest intermolecular force, induced dipole-dipole interactions
      • Larger molecules have stronger van der Waals forces
    • Dipole-dipole forces
      • Stronger than van der Waals, occur between permanent dipoles
    • Hydrogen bonding
      • Strongest intermolecular force, occurs between H and highly electronegative N, O, or F
    • Ice expands when cooled due to hydrogen bonding pushing molecules apart
    • Metallic bonding
      Giant lattice of positive metal ions with delocalized electrons in between
    • Metallic properties
      • High melting points
      • Good thermal and electrical conductors
      • Insoluble in water
    • Particle model
      Describes the arrangement and motion of particles in solids, liquids and gases
    • Bond types

      • Giant covalent
      • Simple molecular
      • Giant ionic
      • Metallic
    • Polar molecules dissolve in polar solvents like water, non-polar molecules dissolve in non-polar solvents
    • Cubic Arrangement
      In a cubic arrangement, ions are arranged in a three-dimensional grid where each ion is surrounded by eight counter-ions in the shape of a cube. This arrangement is highly symmetrical and efficient, which leads to strong electrostatic forces between oppositely charged ions.
    • Non-cubic Arrangement
      In a non-cubic arrangement, ions are arranged in a three-dimensional grid that is not in the shape of a cube. This can take many forms, such as hexagonal or tetragonal. In these arrangements, the ions are not as efficiently packed as in a cubic arrangement, which can lead to weaker electrostatic forces between oppositely charged ions.
    • High Melting Points
      Giant ionic structures with cubic arrangements of ions have high melting points due to the strong electrostatic forces between oppositely charged ions.
    • Low Melting Points
      Giant ionic structures with non-cubic arrangements of ions have lower melting points due to the weaker electrostatic forces between oppositely charged ions.
    • Symmetrical Arrangement
      Cubic arrangements of ions in giant ionic structures are highly symmetrical, which allows for a more uniform distribution of charges and a more efficient packing of ions.
    • Efficient Packing
      Cubic arrangements of ions in giant ionic structures allow for efficient packing of ions, which maximizes the number of attractive electrostatic interactions between oppositely charged ions.
    • Uniform Distribution of Charges
      Cubic arrangements of ions in giant ionic structures allow for a more uniform distribution of charges, which leads to stronger electrostatic forces between oppositely charged ions.
    • Weak Electrostatic Forces
      Non-cubic arrangements of ions in giant ionic structures can lead to a less uniform distribution of charges and weaker electrostatic forces between oppositely charged ions.