Unit-5 Chemical Bonding
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Unit-5 Chemical Bonding
Answer: Na (2,8,1) has one electron in its outermost shell.
Answer: Strong electrostatic forces in the ionic lattice require a large amount of energy to overcome.
Answer: In the molten or aqueous state, ions become free to move and carry the electric current.
Answer: In the solid state, ions are locked in the crystal lattice and cannot move freely.
Answer: The two equal C=O bond dipoles point in opposite directions and cancel each other out.
Answer: Weak intermolecular forces between covalent molecules require little energy to overcome.
Answer: Covalent molecules are electrically neutral and lack free-moving ions or electrons.
Answer: CO2 is formed by two non-metals sharing electrons.
Answer: Oxygen shares one electron with each hydrogen and keeps two lone pairs, giving eight electrons around it.
Answer: A triple bond has the most shared electron pairs and is the strongest and shortest.
Answer: Metals have a sea of delocalized electrons that move freely throughout the lattice.
Answer: Delocalized electrons allow layers of metal ions to slide without breaking the metal.
Answer: Group 2 elements such as magnesium and calcium have two valence electrons.
Answer: Eight valence electrons give a stable octet configuration.
Answer: With complete octets, noble gases have no tendency to form bonds.
Answer: Neon (2,8) has a complete octet of eight valence electrons.
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Answer: Nitrogen uses its lone pair of electrons to form the fourth bond in NH4+.
Answer: One atom donates both electrons of the pair to form the dative bond.
Answer: Molten ionic compounds have free ions, while covalent compounds exist as neutral molecules.
Answer: Increasing nuclear charge attracts the bonding electrons more strongly across a period.