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Chapter 9: Problem 72

The formulas for the fluorides of the third-period elements are \(\mathrm{NaF}, \mathrm{MgF}_{2}, \mathrm{AlF}_{3}, \mathrm{SiF}_{4}, \mathrm{PF}_{5}, \mathrm{SF}_{6},\) and \(\mathrm{ClF}_{3}\). Classify these compounds as covalent or ionic.

Short Answer

Expert verified
NaF, MgF2, and AlF3 are ionic compounds. SiF4, PF5, SF6, and ClF3 are covalent compounds.

Step by step solution

01

Identify the Ionic Compounds

Sodium (Na), Magnesium (Mg), and Aluminium (Al) are metals and they typically form ionic bonds with nonmetals. Hence, NaF, MgF2, and AlF3 are ionic compounds.
02

Identify the Covalent Compounds

Silicon (Si), Phosphorus (P), Sulfur (S) and Chlorine (Cl) are non-metals and they typically form covalent bonds with other non-metals. Therefore, SiF4, PF5, SF6, and ClF3 are covalent compounds.

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Most popular questions from this chapter

Write Lewis dot symbols for the following ions: (a) \(\mathrm{Li}^{+},(\mathrm{b}) \mathrm{Cl}^{-},(\mathrm{c}) \mathrm{S}^{2-},(\mathrm{d}) \mathrm{Sr}^{2+}\) (e) \(\mathrm{N}^{3+}\).

Four atoms are arbitrarily labeled \(\mathrm{D}, \mathrm{E}, \mathrm{F},\) and \(\mathrm{G}\). Their electronegativities are: \(\mathrm{D}=3.8, \mathrm{E}=3.3, \mathrm{~F}=\) \(2.8,\) and \(\mathrm{G}=1.3\). If the atoms of these elements form the molecules DE, DG, EG, and DF, how would you arrange these molecules in order of increasing covalent bond character?

Draw four reasonable resonance structures for the \(\mathrm{PO}_{3} \mathrm{~F}^{2-}\) ion. The central \(\mathrm{P}\) atom is bonded to the three \(\mathrm{O}\) atoms and to the \(\mathrm{F}\) atom. Show formal charges.

These species have been detected in interstellar space: (a) \(\mathrm{CH},\) (b) \(\mathrm{OH},\) (c) \(\mathrm{C}_{2},\) (d) \(\mathrm{HNC}\), (e) HCO. Draw Lewis structures of these species and indicate whether they are diamagnetic or paramagnetic.

Write three resonance structures for the isocyanate ion (CNO \(^{-}\) ). Rank them in importance.
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