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6.9 Polarity of Molecules and Intermolecular Forces -- Part 1
The bonds and lone pairs are drawn for the Lewis structure.
To minimize repul sion, arrange the electron groups around the central atom.
There are four electron groups around the central atom.
To determine the shape, use the atoms that are bonding to the central atom.
The SiCl4 molecule has a tetrahedral shape because the central Si atom is bonding to four atoms.
The shape of SCl2 can be predicted using the VSEPR theory.
The shape is bent.
The central S atom has electron groups.
The geometry is called the electron-group.
The central S atom has a number of atoms.
The molecule has a shape.
You can compare the Lewis structures.
The Lewis structures of CH4 and H2O are compared.
covalent bonds can be either polar or non polar.
Identifying polarity of Molecules is determined by the bonds in a molecule and its shape.
H2, Cl2, and CH4 are nonpolar because they only have nonpolar bonds.
CO2 has two equal polar covalent bonds that point in opposite directions.
The CO2 molecule is nonpolar because the dipoles cancel out.
The CCl4 molecule has four polar bonds that are symmetrically arranged around the central C atom.
The molecule of CCl4 is nonpolar.
CCl4 is nonpolar.
A single dipole does not cancel out.
HCl is a polar molecule because it has a single bond that is polar.
The shape of the molecule determines whether the dipoles cancel.
H2O has a bent shape.
The water molecule is polar because the individual dipoles don't cancel.
H2O is polar and the dipoles do not cancel out.
The NH3 molecule is a trigonal pyramidal shape because of its electron-group geometry.
H dipoles are not canceled.
NH3 is polar and the dipoles do not cancel out.
The CH does not cancel out.
There is only one dipole in CH 3F.
3F, CH3F is a polar molecule.
Determine if a molecule of OF2 is either polar or non polar.
Determine if the bonds are polar or non polar.
Draw the Lewis structure if the bonds are polar covalent.
F bonds are not canceled.
The OF2 molecule is polar.
OF2 is polar and the dipoles do not cancel out.
In gases, there are minimal interactions between particles, which allows gas to move far apart from each other.
There are enough interactions between the particles to hold them together.
The strongest of the attractive forces in compounds are ionized bonds.
Most ionic compounds are solid at room temperature.
Large amounts of energy are needed to overcome the strong attractive forces between positive and negative ion.
The strongest types of attractive forces are hydrogen bonds.
The electrons in a nonpolar covalent molecule are distributed symmetrically.
The negative end of another molecule attracts the F molecule.
The weak dispersion forces make it possible for nonpolar molecules to form liquids.
When they form temporary dipoles, nonpolar covalent molecules have weak attractions.
There are various types of attractions between particles.
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