Q.1
When applying VSEPR theory to predict molecular shape, which of the following do we not need to take into account?
  • Valence electrons occupying sigma bonding orbitals
  • Valence electrons occupying pi bonding orbitals
  • Valence electrons occupying non-bonding orbitals
Q.2
Determine the molecular shape of carbon tetrafluoride.
  • linear
  • trigonal planar
  • bent
  • tetrahedral
Q.3
What shape would PH3 have?
  • Trigonal Planar
  • Trigonal pyramidal
  • Bent
  • Linear
Q.4
A molecule with a lone pair on the central atom would have the same electron and molecular geometry
  • True
  • False
Q.5
How many lone pairs of electrons are on the P atom in PF3?
  • 1
  • 2
  • 3
  • 0
Q.6
The Bohr model of the atom proposed that electrons move at fixed distances from the nucleus and that the energy of the electron is related to its orbit. What discovery contributed to the development of this atomic model?
  • Electrons can flow freely through metals making metals good conductors.
  • Elements have characteristic wavelengths of light emission and absorption
  • Noble gas elements are much less reactive than most other elements.
  • Electrons exhibit properties of both particles and waves.
Q.7
Which of the following correctly matches a compound with its molecular geometry?
  • Water (H2O) : linear
  • Carbon dioxide (CO2): tetrahedral
  • Ammonia (NH3): trigonal planar
  • Methane (CH4): tetrahedral
Q.8
The general formula for TETRAHEDRAL shape is __________
  • AB2
  • AB3
  • AB4
  • AB
Q.9
AB3 is a symbol for molecular shape __________________
  • Tetrahedral
  • Linear
  • Trigonal planar
  • Trigonal pyramidal
Q.10
Valence-Shell electrons pair repulsion theory is used to predict
  • physical properties of compound
  • type of chemical bonding
  • molecular shape
  • solubility
Q.11
Which of the following molecular shapes would have a bond angle ofDegrees?
  • Bent
  • Trigonal Planar
  • Tetrahedral
  • Linear
0 h : 0 m : 1 s