linear
It depends upon number of bonds and lone pairs. 1.Number of bonds-2 lone pair-1 shape is Angular lone pairs-2 shape is Angular lone pairs-3 shape is Linear 2.Number of bonds-3 lone pairs-1 shape is Pyramid lone pairs-2 shape is T shape 3.Number of bonds-4 lone pairs-1 shape is See Saw lone pairs-2 shape is Square Planer 4.Number of bondsg-5 lone pairs1-1 shape is Square pyramidal
Pyramidal I believe, example being NH3 or ClP3
pyramidal has a charge cloud of 4 while BENT has a charge cloud of 3
trigonal [planer
Linear
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
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.
linear
It is a bent molecule because of Oxygen's lone pairs
linear
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
The lone pair pushes bonding electron pairs away.
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.
Electron pairs repelling each other push atoms apart.
PH3 has 3 bonding pairs and 1 non-bonding pair of electrons. Its electron pair geometry is Tetrahedral and its molecular geometry is Trigonal Pyramidal.
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.
Repulsion of the unshared electron pairs (2)and the bonded pairs (2) around the central oxygen atom. Repulsion of these 4 electron pairs attempts to form a tetrahedral shape. Describing the molecular shape, we ignore the unshared electrons and just describe the shape of the molecule based on the location of the atoms, thus bent.
The number of electron pairs around the central atom determines its shape by following the VSEPR theory, which states that electron pairs arrange themselves around the central atom to be as far apart from each other as possible. The arrangement of electron pairs gives rise to specific molecular geometries, which in turn determine the overall shape of the molecule.
The lone pair pushes bonding electron pairs away.