Practice NAT questions with answers and explanations.
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Carbon in methane has four bonding pairs and no lone pairs.
The molecular geometry is tetrahedral.
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Nitrogen has three bonds and one lone pair.
The lone pair changes the molecular shape from tetrahedral electron geometry.
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Oxygen has two bonding pairs and two lone pairs.
Lone-pair repulsion produces a bent molecule.
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Carbon has two electron domains from the two double bonds.
They arrange 180 degrees apart.
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Boron has three bonding regions and no lone pairs.
The molecule is planar with approximately 120-degree angles.
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Four equivalent bonding directions correspond to sp3 hybridization.
The ideal geometry is tetrahedral.
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Each carbon has three sigma-bonding regions.
The remaining p orbitals form the pi bond.
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Lone pairs influence shape and reactivity.
They repel bonding pairs strongly in VSEPR theory.
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Each carbon has two electron domains.
Sp hybridization gives linear geometry and leaves two p orbitals for pi bonds.
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Noble gases have filled valence shells in their common ground states.
They are generally unreactive.
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Increasing nuclear charge pulls electrons closer within the same main shell.
Effective nuclear attraction generally increases across a period.
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Additional electron shells are added down a group.
This outweighs the increased nuclear charge.
