Water: 104.45° Ozone: 116.8° Difference: 12.4°
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.
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The bond angle for selenium hydride is likely to be around 90 degrees. This is because selenium has a lone pair that repels the bonding pairs, making the H-Se-H bond angle less than the ideal 109.5 degrees for a tetrahedral arrangement. Consequently, the bond angle is smaller due to the lone pair's influence.
The angle between the two Hydrogen atoms, ie the bond angle, is 104.45 degrees. This differs from the normal 109.5 degrees because the two lone electron pairs repel and are trying to distance themselves.
The bond angle of BF2 is 120 degrees.
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.
Ozone (O₃) has a bond angle of approximately 117 degrees, which is larger than water's bond angle of about 104.5 degrees. This difference is primarily due to the presence of resonance structures in ozone, which allows for a more spread-out electron distribution and reduces the repulsion between bonding pairs. In contrast, water has two lone pairs that exert greater repulsive forces on the bonding pairs, resulting in a smaller bond angle. Additionally, the molecular geometry of ozone is bent, but it experiences less steric hindrance compared to water.
The approximate H-O-H bond angle in water is 104.5 degrees.
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.
in ammonia as N has mre e.n. than H,bond pair of electrons are more towards it which causes repulsion with lone pair of electrons,and they tend o move away but in nf3 bond pair of electrons are away from flourine so they can have lesser bond angle
in water the electrons will be towards the oxygen since it is more electronegative than hydrogen so the repulsion between bp-bp will oppose the repulsion between lp-bp but in oxygenfluoride electrons will be towards fluorine so repulsion will be less so bond angle is less than water
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.