Question

Group Elements and Molecular Shapes

U Print 10-043: E- Group Arrangements, Molecular Shapes, And Bond Angles From Formulas 1) O3 Draw Lewis structures for each of the following and use them to answer the next 3 questions. 2) NF3 3) NO2 4) SO2 5) CF 6) CH2Cl2 Match each molecule orion above to the correct electron-group arrangement from the list below. CCF A square planar B T shape О снус, C tetrahedral D bent E trigonal pyramidal C NF, F linear SOZ G trigonal planar NO, BurnAww Tries 0/5 Now match the sames molecules or lons above to the correct molecular shape. DNF A quare planar NO ronal pyramidal SO, C tetrahedral D trigonalplaner CF CHCI F bent GT shape Sobre Tries os Finally, match the same molecules and ions above to the correct ideal bond angles from the list below CNS A109.5" CF B 30° Do C90° SO D 45° E 60° CPNO, F 120° G 180° CH, A Tries 0/5 Send Feedback This discussion is closed.

Answer 1

Answer:

Lewis structure: (182) O Ö ONZE 5+243) : 2 (triangular pyramidal) (trigonal planov) I NORD 5+ (1) #1 10: :30] levaron sez: ©:3:8 6 +642 18e or bend) trigonal planner (6) CH₂ CL . I do :C1 —ė – 01: 4+2 +7x2 = 20e = 322 if: . (tetrahedral) (trigonal Pyramidal) matching 109.50 - CH2 421 - CF4 ,NFZ 120° - 802, 03, 0022 (SP2)

N:B:

Ozone has three electron groups about the central oxygen. One group is a lone pair. These groups have a trigonal planar arrangement.

The bond pairs arrange themselves in a trigonal planar way. In NF3 there are also three bond pairs, but the nitrogen has a lone pair as well. The four pairs of electrons arrange themselves tetrahedrally, but the description of the shape only takes account of the atoms. NF3 is a pyramidal.

As a result they will be pushed apart giving the NO2 - molecule a bent molecular geometry or shape. The NO2 - bond angle will be about 120 degrees since it has a trigonal pyramidal molecular geometry (it will be a bit less since the lone pair will push down – the actual value is 115.4t)

The electron geometry of SO2 is formed in the shape of a trigonal planner. The three pairs of bonding electrons arranged in the plane at the angle of 120-degree.

CF4, or tetrafluoromethane, is a tetrahedral molecule. As indicated by the "tetra" portion of the name, the molecule has four groups of electrons bonded around a central atom. As with many-electron bonds, there are several parts to a tetrahedral molecule.

As the hybridization is sp3, the molecular geometry of Dichloromethane becomes tetrahedral. The shape of the compound is a trigonal pyramidal.