Draw the electronic diagrams for the bonding in O2 and H2O.

Here are the electronic diagrams showing the bonding in each molecule/compound: Key for diagrams: represents valence electrons from one atom. × represents valence electrons from another atom. For ionic compounds, × also represents electrons gained from another atom. --- a) Oxygen (O_2) Oxygen is a diatomic molecule with a double covalent bond. Each oxygen atom has 6 valence electrons and needs 2 more to achieve a stable octet. They share two pairs of electrons. Step 1: Identify valence electrons. Each Oxygen atom (O) has 6 valence electrons. Total valence electrons = 2 × 6 = 12. Step 2: Form a double bond and distribute remaining electrons. Two oxygen atoms share two pairs of electrons (a double bond). Each oxygen atom then has two lone pairs. c × × \\ × O × ×= O \\ × × Each oxygen atom has 4 shared electrons and 4 non-shared electrons (2 lone pairs), totaling 8 electrons in its valence shell. The bonding in oxygen is a double covalent bond. --- b) Water (H_2O) Water is a covalent molecule where oxygen shares electrons with two hydrogen atoms. Step 1: Identify valence electrons. Oxygen (O) has 6 valence electrons. Each Hydrogen (H) has 1 valence electron. Total valence electrons = 6 + (2 × 1) = 8. Step 2: Form single bonds and distribute remaining electrons. The oxygen atom forms a single covalent bond with each hydrogen atom. The remaining electrons on oxygen form two lone pairs. c × \\ H × O × H \\ \\ Each hydrogen atom achieves a stable duet (2 electrons), and the oxygen atom achieves a stable octet (8 electrons: 4 shared, 4 lone pair). The bonding in water consists of two single covalent bonds. --- c) Ammonia (NH_3) Ammonia is a covalent molecule where nitrogen shares electrons with three hydrogen atoms. Step 1: Identify valence electrons. Nitrogen (N) has 5 valence electrons. Each Hydrogen (H) has 1 valence electron. Total valence electrons = 5 + (3 × 1) = 8. Step 2: Form single bonds and distribute remaining electrons. The nitrogen atom forms a single covalent bond with each of the three hydrogen atoms. The remaining two electrons on nitrogen form one lone pair. c × \\ H × N × H \\ \\ × \\ H Each hydrogen atom achieves a stable duet (2 electrons), and the nitrogen atom achieves a stable octet (8 electrons: 6 shared, 2 lone pair). The bonding in ammonia consists of three single covalent bonds. --- d) Aluminium oxide (Al_2O_3) Aluminium oxide is an ionic compound formed by the transfer of electrons from aluminium (metal) to oxygen (non-metal). Step 1: Identify valence electrons and ion formation. Aluminium (Al) is in Group 13, has 3 valence electrons, and tends to lose them to form Al^3+ ions. Oxygen (O) is in Group 16, has 6 valence electrons, and tends to gain 2 electrons to form O^2- ions. Step 2: Show electron transfer and resulting ions. To balance the charges, two aluminium atoms will lose a total of 6 electrons (2 × 3 = 6), and three oxygen atoms will gain a total of 6 electrons (3 × 2 = 6). Initial atoms: Al · · · Al · · · · · O · · · · O · · · · O · · · · · · · · Electron transfer: Each Al atom transfers its 3 valence electrons. Each O atom accepts 2 electrons. Resulting ions: 2 × [Al]^3+ 3 × [ c × × \\ × O × \\ × × ]^2- The bonding in aluminium oxide is ionic bonding. --- e) Magnesium sulphide (MgS) Magnesium sulphide is an ionic compound formed by the transfer of electrons from magnesium (metal) to sulphur (non-metal). Step 1: Identify valence electrons and ion formation. Magnesium (Mg) is in Group 2, has 2 valence electrons, and tends to lose them to form Mg^2+ ions. Sulphur (S) is in Group 16, has 6 valence electrons, and tends to gain 2 electrons to form S^2- ions. Step 2: Show electron transfer and resulting ions. One magnesium atom transfers its 2 valence electrons to one sulphur atom. Initial atoms: Mg · · · · S · · · · Electron transfer: Mg · · + · · S · · [Mg]^2+ + [ c × × \\ × S × \\ × × ]^2- The bonding in magnesium sulphide is ionic bonding.