Unit-5 Chemical Bonding
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Unit-5 Chemical Bonding
Answer: Sodium, a metal with one valence electron, loses it readily to become Na+.
Answer: Ca (2,8,8,2) loses two electrons to form the Ca2+ ion.
Answer: Two non-metals usually share electrons to form covalent bonds.
Answer: Nitrogen atoms are joined by a triple bond consisting of three shared pairs of electrons.
Answer: Oxygen donates one of its lone pairs to bond with a hydrogen ion.
Answer: The electron sea model describes metallic bonding in metals.
Answer: Delocalized electrons move freely through the metal and carry the electric charge.
Answer: Hydrogen, with one electron, needs one more electron to reach the duplet of two.
Answer: Carbon forms four single covalent bonds, one with each of the four hydrogen atoms.
Answer: Fluorine is more electronegative than chlorine, so the H-F bond is more polar.
Answer: Identical atoms have equal electronegativity, so the electrons are shared equally.
Answer: Ionic compounds form a repeating three-dimensional crystal lattice.
Answer: Valence electrons decide how and with what an element will bond.
Answer: Na loses one electron and Cl gains it, forming Na+ and Cl- ions.
Answer: Sigma bonds result from head-on overlap of orbitals along the bond axis.
Answer: Their first shell is complete with just two electrons.
Answer: Hydrogen and chlorine differ in electronegativity, making the HCl bond polar.
Answer: Delocalized electrons transfer both heat energy and electric charge.
Answer: Identical atoms such as N and N share electrons equally, giving a non-polar bond.
Answer: The large electronegativity difference causes complete electron transfer, forming an ionic bond.