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Define the following terms: a. Neutral atom b. Element c. Molecule Give (3) examples of a. Element b. Molecule State the bond found in the following Compounds: (i) ZnO (ii) Al2O3 (iii) CaCl2 With the aid of a diagram explain the formation BeCl2.

Chemistry

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Step-by-step solution

2 steps

Step 1a: Definition of covalent bond

A covalent bond is a chemical bond formed when two atoms share one or more pairs of valence electrons to achieve stable electron configurations.

Step 1b: Definition of covalent compounds

Covalent compounds are substances composed of molecules formed by covalent bonds between non-metal atoms. They typically have low melting and boiling points and do not conduct electricity in any state.

Examples: H2OH_2O (water), CO2CO_2 (carbon dioxide), CH4CH_4 (methane).

Step 1c: Definition of ionic bond and compounds where found

An ionic bond is a chemical bond formed by the electrostatic attraction between oppositely charged ions, resulting from the complete transfer of electrons from a metal atom (forms cation) to a non-metal atom (forms anion).

Ionic bonds are found in the following compounds: NaCl\mathrm{NaCl} (sodium chloride), KCl\mathrm{KCl} (potassium chloride), MgO\mathrm{MgO} (magnesium oxide), CaCl2\mathrm{CaCl_2} (calcium chloride).

Step 2: Bond found in the following compounds (common examples)

Assuming typical examples like:

Part a

NaCl\mathrm{NaCl}: Ionic bond.

Part b

HClHCl: Covalent bond (polar).

Part c

H2OH_2O: Covalent bonds.

Part d· 2 steps

AlCl3\mathrm{AlCl_3}: Covalent bond (if listed).

  1. Formation of ionic bond with diagram (e.g., NaCl\mathrm{NaCl})

    Ionic bond formation in NaCl\mathrm{NaCl}:

    Sodium (Na, group 1, 1 valence electron) loses 1 electron to achieve stable octet.

    Na→Na++e−\mathrm{Na} \rightarrow \mathrm{Na}^{+} + e^{-}

    Chlorine (Cl, group 17, 7 valence electrons) gains 1 electron to achieve stable octet.

    Cl+e−→Cl−\mathrm{Cl} + e^{-} \rightarrow \mathrm{Cl}^{-}

    The Na+\mathrm{Na}^{+} and Cl−\mathrm{Cl}^{-} ions are held together by strong electrostatic attraction.

    Diagram description (Lewis structure):

    Na atom: [Na]⋅[\mathrm{Na}] \cdot (1 dot)

    loses dot → [Na+][\mathrm{Na}^{+}]

    Cl atom: :Cl¨⋅:\ddot{\mathrm{Cl}}\cdot (7 dots)

    gains dot → [:Cl¨:]−[:\ddot{\mathrm{Cl}}:]^{-}

    Ionic lattice: Na+Cl−Na+…\mathrm{Na}^{+} \mathrm{Cl}^{-} \mathrm{Na}^{+} \ldots

  2. Formation of covalent bond with diagram (e.g., H2H_2)

    Two hydrogen atoms each with 1 valence electron share a pair.

    H⋅+⋅H→H:H\mathrm{H} \cdot + \cdot \mathrm{H} \rightarrow \mathrm{H:H}

    Shared pair (single bond) allows both to have duet.

    For H2OH_2O:

    Oxygen shares 1 electron with each H.

    Lewis: Central O with two lone pairs, single bonds to two H.

    \chemfigH−O−H\chemfig{H-O-H}

    (Note: Simple text representation; actual diagram shows dots for shared pairs.)

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