in water there are two bond pairs and two lone pairs where as in CH4 there are are four bond pairs nad no lone pair. in ch4 there is only bond pair to bond pair repulsion but in water there are three types of repulsions, lone to lone (greatest repulsion), lone to bond ( lesser repulsion ) and bond to bond ( the least repulsion) , therefore due to the presence of two lone pairs in water the bond pairs are repelled with greater force and they get compressed, reducing the ideal bond angle from 109.5 to 104.5 on the other hand, ch4 has only bond pairs and they dont repel each other that strongly so its angle is greater n its 109.5..
No, the bond angle for linear structure is 180 degrees.
ClO3 has the smaller bond angle than ClO4
Yes, water is a bend molecule with a bond angle of about 105 degrees. They are described as bent planar (or V shaped)
bond angle
Water: 104.45° Ozone: 116.8° Difference: 12.4°
The water molecule's bond angle is about 104.45 degrees.
Oxygen difluoride (OF2) has a larger bond angle than carbon dioxide (CO2). OF2 has a bond angle of around 103 degrees, while CO2 has a bond angle of 180 degrees due to its linear molecular geometry.
Oxygen difluoride (OF2) has a larger bond angle than carbon dioxide (CO2). OF2 has a bond angle of 103.3 degrees while CO2 has a bond angle of 180 degrees. This is because OF2 has two lone pairs of electrons on the central oxygen atom, causing the fluorine atoms to be pushed closer together, resulting in a smaller bond angle.
The approximate H-O-H bond angle in water is 104.5 degrees.
Ammonia (NH3) has a larger bond angle than NF3 because nitrogen is less electronegative than fluorine. Therefore, the lone pair-bond pair repulsion in ammonia is less significant than the lone pair-bond pair repulsion in NF3, resulting in a larger bond angle in ammonia.
The difference in bond angles between water (104.5°) and oxygen fluoride (102.7°) is due to the presence of different atoms bonded to the central oxygen atom. In water, two hydrogen atoms create a more electronegative environment around oxygen, causing a greater compression of the bond angle. In oxygen fluoride, the larger fluorine atoms reduce this compression, resulting in a slightly larger bond angle.
The bond angle in H2S (92 degrees) is less than in H2O (104.5 degrees) due to the larger size of sulfur compared to oxygen. The larger size of sulfur results in weaker repulsions between the electron pairs, causing the bond angle to be smaller in H2S compared to H2O.
Santa clause crawled into my bed and told me because he said so
In CH2F2, the bond angle between the carbon-hydrogen bonds will be greater than the bond angle between the carbon-fluorine bonds. This is because hydrogen atoms have a smaller size compared to fluorine atoms, causing repulsion between the larger fluorine atoms to decrease the carbon-hydrogen bond angle.
The lone pair - OH bond repulsion in water is greater than the OH bond- OH bond repulsion. In methane all of the bonds are the same so it has perfect tetrahedral symmetry. This is VSEPR theory
The approximate HOH bond angle in ice is around 109.5 degrees due to the tetrahedral arrangement of water molecules in the solid state. The hydrogen bonds in ice help hold the water molecules together in a regular pattern, contributing to the observed bond angle.