Imagine that you create the tetrahedron by joining opposite vertices on the faces of a cube as in the diagram below. To simplify the arithmetic assume that the cube has sides of length 2.
Let O be the point at the center of the cube (equidistant from the eight vertices) as in the diagram below. Construct the triangle OPQ.
Consider the triangle OPQ. Let R be the midpoint of PQ.
Since the sided of the cube are of length 2, a use of Pythagoras' Theorem gives |PQ| = . Also, since O is at the center of the cube, |OR| = 1. From the diagram the tangent of the angle ROP is . Thusangle QOP = 2 x angle ROP = 2 x arctan() = 109.5o
The central atom of a methane molecule is the carbon atom. Four hydrogen atoms are directly bonded to it and there is no lone pairs located in the central atom. Having a tetrahedral shape, every bond angle in methane is equal to 109.5 degrees.
The bond angle of singlet methylene is 120°. This is because it has a steric number of 3 and no lone electron pairs, and thus its molecular geometry is trigonal planar.
arccos(-1/3), which is approximately 109.5 degrees
Methane has a tetrahedral geometry. Thus, the bond angles in methane are all equal to 109o.
since the lewis dot structure of this compound is a tetrahedral (around the C atom that is) and all four electron pairs are bonding pairs, the ideal angles should be 109.5 degrees
The question is nonsense. WHICH bond angle? There are many of them in a molecule the size of estradiol.
The value of the bond angle in XeF2 is 180 degrees.
90 degrees is the value of the smallest bond angle in IF4.
The bond length is equal to the linear distance between the nuclei of the bonding atoms. The bond angle is equal to the angle between any two consecutive bonds in a molecule or ion. Bond angles of molecules and ions are usually determined by using the VSEPR theory.
The bond angle is 180 because ICl2- has three Lone Pairs attached to it making it Linear.
The methylene radical CH2 has just 6 electrons around the central carbon. The lowest energy methylene is "triplet" methylene with two unpaired electrons. Simple VSEPR cannot predict the bond angle which is measured as being 133 0. A slightly higher energy form has no unpaired electrons and the angle is measured at 102 0. This is in accord with simple VSEPR theory which would predict a decrease in bond angle from 120 0 due to repulsion of the lone pair.In compounds the -CH2- unit in alkanes such as propane the bond angles are close to 109 0 the tetrahedral angle (sp3 hybridisation). When =CH2 terminates an alkene such as ethene (ethylene) the bond angle is close to 120 0, (sp2 hybridisation)
Increases
Bond angle is 109.5 degrees.It is equal in every bond
NH4+ is tetrahedral, with bond angle of 109.5o
the f-p-f bond angle is 120the cl -p-cl bond angle is 180and the f - p - cl bond angle is 90
Bond Angle (:
The bond angle for H2S is 92.1­°.
The water molecule's bond angle is about 104.45 degrees.
the shape is bent and the bond angle is approximately 120
No, the bond angle for linear structure is 180 degrees.
The answer would be bond angle, for number 19#
The question is nonsense. WHICH bond angle? There are many of them in a molecule the size of estradiol.