A tabela a seguir mostra algumas diferenças entre o diamante e a grafite, que são formas alotrópicas do carbono. }(c) Forma alotrópica & Dureza & Condução de calor & Condução de Diamante & Duro & Condutor & Isolante Grafite & Mole & Isolante & Conductor Essas propriedades são justificadas pelas e ruturas dos alótopos. Nessas estruturas, tomos de carbono do diamante e da grafi im, respectivamente, hibridização sp e mathrm(sp)^2 . d) mathrm(sp)^2 e mathrm(sp)^3 . mathrm(sp)^3 e mathrm(sp)^2 . e) mathrm(sp)^2 e sp. sp e mathrm(sp)^3 .

## Step 1: Understanding Allotropic Forms### The question involves two allotropic forms of carbon: diamond and graphite. Each form has distinct properties due to differences in atomic structure and bonding.## Step 2: Analyzing the Table Data### From the table, we see that diamond is hard, conducts heat but is an electrical insulator. Graphite, on the other hand, is soft, does not conduct heat well, but is a good conductor of electricity.## Step 3: Relating Properties to Hybridization### The hardness and insulating properties of diamond are due to its three-dimensional tetrahedral structure where each carbon atom is hybridized, forming strong covalent bonds with four other carbon atoms.### Graphite's softness and electrical conductivity arise from its planar structure where each carbon atom is hybridized, forming layers that can slide over each other. The delocalized electrons between these layers allow for electrical conduction.## Step 4: Matching Hybridization with Options### Based on the above analysis, diamond corresponds to hybridization, and graphite corresponds to hybridization.