Table of Contents
- 1 Why does the bond angle of hydrides decrease down the group?
- 2 Why does the bond angle increase as the number of electron groups decrease?
- 3 Why does the hydrides decrease down the group 15?
- 4 On what factors does the bond angle depends?
- 5 Which hydrides of group 16 has the highest bond angle?
- 6 Why bond angle of hydrides of Group 15 decreases down group?
- 7 Why does the stability of hydrides decrease from ammonia to bismuthine?
Why does the bond angle of hydrides decrease down the group?
Dipole moment is proportional to electronegativity of the central atom. So it decreases down the group. These hydrides are pyramidal in shape with a lone pair of electrons in one of the orbits. The bond angle gradually decreases down the group due to the decrease in bond pair- bond pair repulsions.
Why does the bond angle increase as the number of electron groups decrease?
i) The bond angle decreases due to the presence of lone pairs, which cause more repulsion on the bond pairs and as a result the bond pairs tend to come closer. ii) The repulsion between electron pairs increases with increase in electronegativity of central atom and hence the bond angle increases.
Why does bond angle decrease down group 16?
On going down the group, electronegativity of central atom decreases, thus reducing its tendency to attract shared pair of electrons towards itself. So lone pair-bond pair repulsions become more efficient as against bond pair-bond pair repulsions thus reducing the bond angle.
What is the cause of change in bond angle?
(i) Repulsion between atoms or groups attached to the central atom may increase or decrease the bond angle. (ii) In hybridisation as the s character of the s hybrid bond increases, the bond angle increases. (iii) By increasing lone pair of electron, bond angle decreases approximately by 2.5\%.
Why does the hydrides decrease down the group 15?
The stability of hydrides decreases down the group from NH3 to BiH3. This is due to a decrease in their bond dissociation enthalpy. Stability decreases down the group as the bond dissociation energy decreases. Hence, the bond dissociation energy decreases down the group due to the increase in the central atom size.
On what factors does the bond angle depends?
Hybridization:- Bond angle depends on the state of hybridization of the central atom. Greater the s character, greater is the bond angle. 2.
What determines bond angle?
The bond angles depend on the number of lone electron pairs. Water, with two lone pairs of electrons, has a bent shape with 104.5-degree bond angles. The VSEPR theory assumes that each atom in a molecule will achieve a geometry that minimizes the repulsion between electrons in the valence shell of that atom.
Which has maximum bond angle among the hydrides of group 16?
(ii) H2O has maximum bond angle, because of small size and high electronegativity of oxygen, bond pair–bond pair repulsion is more.
Which hydrides of group 16 has the highest bond angle?
1 Answer
- Correct option (d) H2O.
- Explanation:
- As we move down the group, the bond angle decrease due to decrease in bond pair-bond pair repulsion.
- H2O H2S H2Se H2Te.
- Bond angle 104.5° 92.2° 91° 90°
Why bond angle of hydrides of Group 15 decreases down group?
Why bond angle of hydrides of group 15, decreases down the group? This is due to the decrease in electronegativity of the central atom of hydride. As the electronegativity decrease the electrons which were more close to central atom at lower hydrides tends to more far from it and bp-bp repulsion decreases.
Why does the electronegativity of a hydride decrease as it decreases?
This is due to the decrease in electronegativity of the central atom of hydride. As the electronegativity decrease the electrons which were more close to central atom at lower hydrides tends to more far from it and bp-bp repulsion decreases. Which is more basic N (CH3)3 or N (SiH3)3 , explain?
What is the bond angle of water in Group VI?
I noticed the fact that all the hydrides of the elements belonging to group IV has bond angle 109.5° while in group V it varies from 107.3° for $\\ce{NH3}$ to 91.3° for $\\ce{SbH3}$. Similarly we see in group VI that water has highest bond angle then it significantly decreases to 89.5° for $\\ce{H2Te}$.
Why does the stability of hydrides decrease from ammonia to bismuthine?
The stability of hydrides decreases from ammonia to bismuthine. This is because the central atom E increases in size down the group. With the increase in the size of the central atom, the E – H bond becomes weaker. where E is nitrogen ,phosphorus, arsenic,antimony , bismuth.