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What is a consequence of electron-pair repulsion around the atom?
Electron-pair repulsion around an atom leads to the arrangement of electron pairs in specific geometries to minimize repulsive forces. This phenomenon is described by the VSEPR (Valence Shell Electron Pair Repulsion) theory, which predicts molecular shapes based on the spatial distribution of electron pairs. As a result, the geometry of a molecule, such as linear, trigonal planar, or tetrahedral, is determined by the number of bonding and non-bonding electron pairs around the central atom. This arrangement affects the molecule's physical and chemical properties.
Can acids donate an electron pair?
No, acids cannot donate an electron pair. Acids are substances that tend to donate a proton (H+) in a chemical reaction, while bases are substances that can donate an electron pair.
What makes atoms spread out around a centralatom?
Atoms spread out around a central atom primarily due to the repulsive forces between their electron clouds and the arrangement dictated by valence shell electron pair repulsion (VSEPR) theory. This theory posits that electrons in the outer shell of atoms repel each other, leading to a spatial arrangement that minimizes this repulsion. Additionally, the presence of different bonding and non-bonding electron pairs influences the geometry, ensuring that atoms adopt a configuration that optimizes stability.
What effect does a lone electron pair have a molecular shape?
The lone pair pushes bonding electron pairs away.
What kind of substance accepts an electron pair hydroxide ion alkali base acid?
A Lewis acid accepts an electron pair.
What effect does a lone electron pair have on molecular shape?
The lone pair pushes bonding electron pairs away.
What is a cobalent bond?
A covalent bond is a chemical bond between atoms that share electrons. It is the stable balance of the attractive and repulsive forces and the result of sharing of electron pairs between the atoms.
Why NO2 is bent in shape?
NO2 is an odd electron molecule - it has 17 valence electrons. There is one unpaired electron which "sits" on the nitrogen. The VSEPR model deals specifically with electron pair repulsion so strictly you can't use it to predict the shape. However what you do is assume that the lone pair orbital is only half filled and is not as repulsive as a true lone pair. So treat it as AX2E compound and therefore bent, but as E is not so repulsive the ONO angle opens out to be greater than 1200, which is in fact true, its 134 0
What is the difference between lone pair and bonding pair electron?
they are the same. Lone pair is unshared pair of electrons and bond pair is shared pair of electron.
What is the electron pair geometry for CS2?
The electron pair geometry for CS2 is Linear.
What is the electron pair geometry of C2H2?
The electron pair geometry of C2H2 is linear.
What is the electron pair geometry for SO2?
The electron pair geometry for SO2 is trigonal planar.
Diffirences of bonded and lone pair electron?
The difference between bonded and lone pair is that a bond pair is composed of two electron that are in a bond whereas lone pair is composed of two electron that is not a bond.
How does a lone pair distort a molecular pair?
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.
Can acids donate an electron pair?
No, acids cannot donate an electron pair. Acids are substances that tend to donate a proton (H+) in a chemical reaction, while bases are substances that can donate an electron pair.
What makes atoms spread out around a centralatom?
Atoms spread out around a central atom primarily due to the repulsive forces between their electron clouds and the arrangement dictated by valence shell electron pair repulsion (VSEPR) theory. This theory posits that electrons in the outer shell of atoms repel each other, leading to a spatial arrangement that minimizes this repulsion. Additionally, the presence of different bonding and non-bonding electron pairs influences the geometry, ensuring that atoms adopt a configuration that optimizes stability.
How does a lone pair distort the molecular shape?
A lone pair of electrons takes up space despite being very small. Lone pairs have a greater repulsive effect than bonding pairs. This is because there are already other forces needing to be taken into consideration with bond pairs. So to summarize: Lone pair-lone pair repulsion > lone pair-bond pair repulsion > bond pair-bond pair repulsion. This makes the molecular geometry different.
