0! forms 4 sigma bonds
2
FOUR!
The molecular geometry is tetrahedral. The orbitals are sp^3 hybridized. The molecule is polar. The bond angles are 109.47 degrees.
Simply it is SP3 Hypridization three P orbitals + one S orbital formed the 4 sp3 orbitals and it is logic experimentally u can see that Methane Molecule is tetrahedral so it has 4 corners which means 4 bonds
The central B atom min BF4- is sp3 hybridised- BF4-is tetrahedral - B has s and p orbitals available for bonding.
sp3d. The ion is see-saw shaped (VSEPR thepry- AX4E geometry)
Butane : CH3CH2CH2CH3. You have got four orbitals to use in bonding with carbon; 2s, and 3 x 2p. They blend together to form four equal orbitals, called hybrids. Hybridisation isn't covered on UK Chemistry syllabuses at school, but it's not too hard to visualise. Each of your four sp3 hybrid orbitals wants to be as far apart from the others as possible, so they move to a tetrahedral shape. Then along the length of the butane C-C chain they are just overlapping end on, exactly like any other sigma bond. The hydrogens are overlapping their s orbitals with the rest of the sp3 hybrids. If you don't have chemistry models to hand, try making a set of blobs of plasticene with four pencils stuck in at tetrahedral angles, then connect them together - you should see the zig zag shape of the C-C chain.
mixture of one s and 3p orbitals forming a tetrahedral geometry
Methane has tetrahedral geometry. In methane carbon undergoes sp3 hybridisation. The four sp3 hybrid orbitals form four sigma bonds with four 1s orbitals of hydrogen atoms.
The molecular geometry is tetrahedral. The orbitals are sp^3 hybridized. The molecule is polar. The bond angles are 109.47 degrees.
In a tetrahedral molecule eg methane (CH4), hybridisation occurs between the 2s orbital and three p orbitals to form four sp3 hybrid orbitals. See: http://www.chem1.com/acad/webtext/chembond/cb06.html and: http://www.mikeblaber.org/oldwine/chm1045/notes/Geometry/Hybrid/Geom05.htm
Simply it is SP3 Hypridization three P orbitals + one S orbital formed the 4 sp3 orbitals and it is logic experimentally u can see that Methane Molecule is tetrahedral so it has 4 corners which means 4 bonds
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.
As the CCl4 molecule has a regular tetrahedral shape the hybridisation is sp3
of course!
In chemical bonding hybridisation is a mathematial device used in valence bond theory to devise new orbitals from the base atomic orbitals - the aim being to achieve new obitals that "point" in the right direction- so tetrahedral methane - use sp3 hybrid orbitals as these hybrid orbitals point tetrahedrally.
That is related to the relative positions of the orbitals involved.
Hybridization in brief can be said as inter mixing of orbitals. But you may have questions such as why? where ? when it happens and what exactly it is? Its very simple for example as in your question consider methane. The carbon atom has 2 electrons in 1s orbital and; 2 electrons in 2s orbital and; 1 electron in 2px orbital and; 1 electron in 2py orbital.In methane before carbon atom undergo bonding with hydrogen it undergoes hybridization ,that is 2s orbitals and 2p orbitals combines or hybridizes and for methane it is sp3 hybridization that means an s orbital had combined with 3 of the 2p orbitals (2px,2py,2pz). It has an tetrahedral arrangement (like four corners of a triangular pyramid) of four lobes of angles approx 109.5 degrees(The angle between H-C-H). After hybridization you cannot differentiate s orbital and p orbital.And in that sp3 hybrid each lobe has one electron and all the lobes bond with hydrogen atoms containing single electron.Note that all the lobes must be treated as an orbital such that they can maximum hold only of two electrons.Thus methane is formed as an result of head on collision of sp3 hybrids and hydrogen atoms.
The central B atom min BF4- is sp3 hybridised- BF4-is tetrahedral - B has s and p orbitals available for bonding.