Explain the lack of reactivity of nitrogen gas, $$$\mathrm{N}_{2}(\mathrm{~g})$$$. ....................................................................................................................................... . ....................................................................................................................................... . ................................................................................................................................. (ii) Covalent bonds can be $$$\sigma$$$ bonds or $$$\pi$$$ bonds. Complete Table 1.1 to show the number of $$$\sigma$$$ and $$$\pi$$$ bonds in a molecule of $$$\mathrm{N}_{2}$$$ and to describe how the orbitals overlap to form $$$\sigma$$$ and $$$\pi$$$ bonds.

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_s24_qp_23 Year：2024 Question No：1(a)

Answer:

Knowledge points:

3.4.1.1.1 hydrogen,

3.4.1.1.10 ethene,

3.4.1.1.2 oxygen,

3.4.1.1.3 nitrogen,

3.4.1.1.4 chlorine

3.4.1.1.5 hydrogen chloride, HCl

3.4.1.1.6 carbon dioxide,

3.4.1.1.7 ammonia,

3.4.1.1.8 methane,

3.4.1.1.9 ethane,

3.4.1.2 understand that elements in period 3 can expand their octet including in the compounds sulfur dioxide, , phosphorus pentachloride, , and sulfur hexafluoride,

3.4.1.3 describe coordinate (dative covalent) bonding, including in the reaction between ammonia and hydrogen chloride gases to form the ammonium ion, , and in the molecule

3.4.2.1.1 $\sigma $ bonds are formed by direct overlap of orbitals between the bonding atoms

3.4.2.1.2 π bonds are formed by the sideways overlap of adjacent p orbitals above and below the σ bond

3.4.2.2 describe how the σ and π bonds form in molecules including

3.4.2.3 use the concept of hybridisation to describe sp, $\mathrm{sp}^{2}$ and $\mathrm{sp}^{3}$ orbitals

3.4.3.1.1 bond energy as the energy required to break one mole of a particular covalent bond in the gaseous state

3.4.3.1.2 bond length as the internuclear distance of two covalently bonded atoms

3.4.3.2 use bond energy values and the concept of bond length to compare the reactivity of covalent molecules

Answer:

Knowledge points:

Solution:

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