IB DP Chemistry Topic 14.2 Hybridization HL Paper 1

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Question

Identify the hybridization of carbon atoms in this molecule

▶️Answer/Explanation

Hybridization of carbon in any organic molecule can be easily determined.
Carbon with single bond has $s p^{3}$ , carbon with double bond has $s p^{2}$ hybridization, and carbon with triple bond has $s p$ hybridization.

C1 has 4 single bonds, it has sp³ hybridization. C2, C3 and C4 have 1 double bond and 2 single bonds, hence they have $s p^{2}$ hybridization.

Question

What is the hybridization of the carbon atom, and the number of $\sigma $ and $\pi $ bonds in the methanal molecule?

▶️Answer/Explanation

Here, carbon is double bonded, hence it is $s p^{2}$ hybridized. It is formaldehyde and it contains 3 $s i g m a$ and 1 $π$ bond so it’s hybridization will be $s p^{2}$ and geometry will be $t r i g o n a l$ $p l a n a r$ .

Question

What is the type of hybridization of the silicon and oxygen atoms in silicon dioxide?

▶️Answer/Explanation

Silicon dioxide is a covalent, three-dimensional network solid in which each silicon atom is bonded to four oxygen atoms which are arranged tetrahedrally around it and each oxygen atom is attached to two silicon atoms by covalent bonds. Each corner is further shared by another tetrahedron. The entire crystal may thus be considered as a giant molecule in which eight-membered rings are formed with alternate silicon and oxygen atoms. SiO2 is a giant covalent molecule in which each silicon is surrounded by four oxygen atoms in a tetrahedral fashion and hence Si is sp³ hybridized. Oxygen is also sp³ hybridized.

Question

In which compound are all the carbon atoms ${\text{s}}{{\text{p}}^{\text{2}}}$hybridized?

C. ${\text{C}}{{\text{H}}_{\text{2}}}{\text{CHC}}{{\text{H}}_{\text{3}}}$

D. ${\text{C}}{{\text{H}}_{\text{3}}}{\text{C}}{{\text{H}}_{\text{2}}}{\text{CHCHC}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{H}}_{\text{3}}}$

▶️Answer/Explanation

In the first compound, all C atoms have on double bond. Carbon in COOH forms C=O and all other carbons in the benzene ring have C=C bond. Hence, it has all carbons with sp² hybridization.

Question

Which statements about hybridization are correct?

I. The hybridization of carbon in diamond is ${\text{s}}{{\text{p}}^{\text{3}}}$.

II. The hybridization of carbon in graphite is ${\text{s}}{{\text{p}}^{\text{2}}}$.

III. The hybridization of carbon in ${{\text{C}}_{{\text{60}}}}$ fullerene is ${\text{s}}{{\text{p}}^{\text{3}}}$.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

▶️Answer/Explanation

In diamond, each carbon atom is linked to four other carbon atoms. Thus, each carbon atom forms four bonds. The carbon atoms in diamond have sp³ $s p^{3}$ hybridization.

Graphite has layer structure in which several layers are formed. In graphite, each carbon atom is linked to three carbon atoms present in the same layer via strong covalent bonds. There are some interactions between two carbon atoms present in two adjacent layers. The carbon atom in graphite is sp² hybridized.

Fullerenes have closed cage structure like a soccer ball or football. The hybridization of carbon in ${{\text{C}}_{{\text{60}}}}$ fullerene is ${\text{s}}{{\text{p}}^{\text{2}}}$.

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