Transcript Quiz review
Quiz review Lewis Structures, VSEPR shape, polarity, and IMFs Get started! Draw the Lewis Structure for…. Once you have drawn a Lewis Structure, click on the molecule to check your answer and complete the rest of the questions What is its shape? tetrahedral angular linear Try again!! Go back Angular…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Polar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back Dipole-Dipole…Very good! This molecule is angular because it has 4 e- pairs around the central atom, 2 atoms bonded to it, and 2 lone pairs. It is polar because it is angular with two lone pairs. Since it is polar, it will have a dipole-dipole IMF Back to Lewis Structures What is its shape? Trigonal planar Pyramidal Tetrahedral Try again!! Go back Trigonal Planar…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Nonpolar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back London Dispersion…Very good! This molecule is trigonal planar because it has 3 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is nonpolar and therefore will experience london dispersion intermolecular forces. Back to Lewis Structures What is its shape? tetrahedral octahedral pyramidal Try again!! Go back Octahedral…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Nonpolar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back London Dispersion…Very good! This molecule is octahedral because it has 6 e- pairs around the central atom, 6 atoms bonded to it, and 0 lone pairs. It is nonpolar so it will experience london dispersion intermolecular forces. Back to Lewis Structures What is its shape? tetrahedral angular square planar Try again!! Go back Tetrahedral…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Nonpolar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back London Dispersion…Very good! This molecule is angular because it has 4 e- pairs around the central atom, 4 atoms bonded to it, and 0 lone pairs. Since it is nonpolar it will experience london dispersion intermolecular forces. Back to Lewis Structures What is its shape? tetrahedral pyramidal see saw Try again!! Go back See Saw…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Polar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back Dipole-Dipole…Very good! This molecule is see saw shape because it has 5 e- pairs around the central atom, 4 atoms bonded to it, and 1 lone pairs. It is polar because it has one lone pair which will distort the shape. Since it is polar, it will have a dipoledipole IMF Back to Lewis Structures What is its shape? tetrahedral trigonal planar pyramidal Try again!! Go back Trigonal planar…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Nonpolar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back London Dispersion…Very good! This molecule is trigonal planar because it has 4 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is polar because it is angular with two lone pairs. Since it is polar, it will have a dipole-dipole IMF **It is also ok to determine shape by saying 3 electron regions, 3 atoms bonded to it, and 0 lone pairs. You get the same answer Back to Lewis Structures What is its shape? Square planar Pyramidal Octahedral Try again!! Go back Square Planar…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Nonpolar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back London Dispersion…Very good! This molecule is square planar because it has 6 e- pairs around the central atom, 4 atoms bonded to it, and 2 lone pairs. Although it has lone pairs, it is nonpolar because it is one of the exceptions. The fluorines cancel each other out, as do the lone pair in this specific shape. Since it is nonpolar it experiences london dispersion intermolecular forces. Back to Lewis Structures What is its shape? see saw angular linear Try again!! Go back Linear…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Nonpolar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back London Dispersion…Very good! This molecule is linear because it has 5 e- pairs around the central atom, 2 atoms bonded to it, and 3 lone pairs. Although it has lone pairs, this is one of the exceptions and is nonpolar since the lone pairs are on the same plane and cancel each other out. Since is it nonpolar, it will experience london dispersion intermolecular forces. Back to Lewis Structures What is its shape? angular trigonal planar linear Try again!! Go back Angular…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Polar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back Dipole-Dipole…Very good! This molecule is angular because it has 4 e- pairs around the central atom, 2 atoms bonded to it, and 1 lone pair. It is polar because it is angular with a lone pair. Since it is polar, it will have a dipole-dipole IMF Back to Lewis Structures Remember for any acid with an oxygen (starts with H and has an O), the hydrogen is bonded to one of the oxygen atoms What is its shape? tetrahedral angular trigonal planar Try again!! Go back Trigonal planar…Very good! What is the polarity? Polar Nonpolar Try again!! Go back Polar…Very good! What is its principal IMF? London Dispersion Dipole Dipole Hydrogen Bonding Try again!! Go back Hydrogen bonding…Very good! This molecule is trigonal planar because it has 4 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is polar because all of the electrons around the central atom are not pulled equally because of the -OH group. Since it is polar and there is an oxygen atom covalently bonded to a hydrogen atom, this molecule will experience hydrogen bonding **It is also ok to determine shape by saying 3 electron regions, 3 atoms bonded to it, and 0 lone pairs. You get the same answer Back to Lewis Structures