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The molecule's function and chemical and physical properties
The factors affecting the shape of the molecules are the bonded e and the lone pairs of electrons
Without given a specific molecule there is not any way to determine the shape. Beryllium chloride consists of beryllium in the middle and a chlorine on each side, and is in the shape of a straight line.
when the molecule contains polar bonds
when the molecule contains polar bonds
Lone pairs do not affect the shape of diatomic molecules, and Lone pairs are electrons that are not in bonds. Lone pairs do not affect the shape if they are not on the central atom.
The molecule's function and chemical and physical properties
In a water molecule, there are two lone pairs of electrons connected to the oxygen. The lone pairs push the hydrogen atoms, creating a bent shape. In CO2, however, there are two double bonds and no lone electrons on the central atom, hence the molecule has a linear shape.
Four atoms bound to a central atom with no lone pairs
Four atoms bound to a central atom with no lone pairs
Four atoms bound to a central atom with no lone pairs
hydrogen bonding between base pairs
The shape of a molecule only describes the arrangement of bonds around a central atom. The arrangement of electron pairs describes how both the bonding and nonbonding electron pair are arranged. For example, in its molecular shape, a water molecule is describes as bent, with two hydrogen atoms bonded to an oxygen atom. However, the arrangement of electron pairs around the oxygen atom is tetrahedral as there are two bonding pairs (shared with the hydrogen) and also two nonbonding pairs.
how to draw a 105 degree angle this is an elaboration to what the previous user said: a v-shaped molecule that has a 105 degree angle is called a bent/angular molecule. It is a modified version of the tetrahedral because it has two lone pairs and two bonds around the central atom instead of the typical tetrahedron which has 4 bonds. an example of a bent molecule would be water (H20) the oxygen has 2 lone pairs and two bonds, slightly bending the shape of the molecule from linear (180) to angular (around 105). This happens because the oxygen is a little more negative (delta negative) than the hydrogens, and so the oxygen's electrons pushes themselves away from the hydrogens, creating a more bent shape (use the VSEPR theory to determine molecular shape for the future) hope this helps!! tip: to find the shape of a molecule, ignore the atoms involved, just focus on the electron pairs surrounding the central atom. if it has 4 bonds, it is tetrahedral, if it has one bond, it is linear, 2 bonds is also linear (JUST 2 BONDS AND NOTHING ELSE), and three bonds is trigonal planar. those were just dealing with bonds, if there are lone pairs around the central atom as well, this is how you would deal with it: 2 bonds and 2 lone pairs is bent; 3 bonds and one lone pair is pyramidal, and one bond and 3 lone pairs is linear, (if the molecule has only one bond, it will always be linear, no matter how many lone pairs) I know this was a lot i just wrote down whatever was on my mind haha.. but these ideas helped me out on my chem test dealing with covalent bond and shapes, hopefully it'll help u too
The central atom of this molecule has two lone pairs and four bonded pairs of electrons. Therefore it has the 'square planar' shape.
The factors affecting the shape of the molecules are the bonded e and the lone pairs of electrons
when the molecule contains polar bonds