Unit-5 Chemical Bonding
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Unit-5 Chemical Bonding
Answer: Two shared pairs of electrons form a double bond.
Answer: O2 shares two pairs of electrons, written as O=O.
Answer: N2 shares three pairs of electrons, written as N identical to N with three lines.
Answer: N2 has a triple covalent bond formed by three shared pairs of electrons.
Answer: A double bond is made up of one sigma and one pi bond.
Answer: In metals, mobile (delocalized) electrons hold the positive metal ions together.
Answer: Unequal electronegativity causes unequal sharing of the electron pair, producing polarity.
Answer: Electronegativity measures an atom's power to attract the bonding electrons.
Answer: Fluorine is the most electronegative element in the periodic table.
Answer: Pi bonds result from the lateral (sideways) overlap of p orbitals.
Answer: H2 is made of identical atoms of equal electronegativity, so its bond is non-polar.
Answer: Oxygen is more electronegative than hydrogen, so the O-H bond is polar covalent.
Answer: The dative bond is another name for the coordinate covalent bond.
Answer: In a dative bond, one atom donates both electrons of the shared pair.
Answer: One of the four bonds in NH4+ is a coordinate covalent bond in which nitrogen donates the pair.
Answer: Hydrogen bonds are weak intermolecular forces, for example between water molecules.
Answer: Water molecules are linked to one another by hydrogen bonds.
Answer: Lewis structures use dots to represent the valence electrons of atoms.
Answer: Cl (2,8,7) has seven electrons in its outermost shell.
Answer: Chlorine attracts the shared electron pair more strongly, so it becomes partially negative.