Three hybrid orbitals in a plane at 120 0 to each other. One perpendicular to the plane, a p orbital.
6 electrons totally
10
p orbitals are at right angles to each other, there are three.
If you mean CH4(methane), then the geometry is tetrahedral, with bond angles of 109.5o
It is formaldehyde in which carbon atom is sp2 hybridized so it is a triangular molecule with bond angles of 1200 .
This is a tetrahedral structure; a typical example is methane, CH4.
A triangle has three angles. The sum of these 3 angles = 180°. At least two of the 3 angles will be acute angles (less than 90°). The third angle can be acute, or a right angle (equal to 90°) or obtuse (between 90° and 180°). Triangles can be categorized by the angles (acute, right or obtuse).
The molecular geometry is tetrahedral. The orbitals are sp^3 hybridized. The molecule is polar. The bond angles are 109.47 degrees.
the angle is 120 degrees.
Oxygen atoms in water form sp3 hybridized orbitals. This configuration of bond angles and bond lengths between the electron pairs and hydrogen atoms on oxygen allow for the least strain.
Urea is sp2 hybridized, so the bond angles are ~120 degrees.
p orbitals are at right angles to each other, there are three.
It is formaldehyde in which carbon atom is sp2 hybridized so it is a triangular molecule with bond angles of 1200 .
If you mean CH4(methane), then the geometry is tetrahedral, with bond angles of 109.5o
Assuming you mean two sets of p orbitals on adjacent atoms only one sigma bond can be formed, by the p orbitals that point between the atoms to form an axial bond. The lobes that are at right angles , ( two unused p orbitals on each atom) could form pi bonds.
Those acute angles all the central angles are acute.
The extraordinary difference in melting points between cyclohexane and cyclohexene is due to the difference in shape. Cyclohexene has an awkward geometry to stack with sp2 hybridized bond angles. This lends to an extreme low melting point for cyclohexene.
OF2 gemometry: sp3 hybridized atoms adopt a tetrahedral geometry. Becasue of the sp3 orbitals contain lone pairs, the VSEPR model indicates that the molecule has an overall bent geometry. The bond angles should be less than 109.5 degrees because the lone pairs repel each other more than the bonding pairs.
To count how many different central angles a circle has, count how many different numbers there are between zero and 360. Include all of the possible fractions. You should discover that the number is very big.