Draw Lewis structures for each of the following:
(A) nitrate ion $({[{N O}_{3}]}^{-})$
(B) phosphoric acid $(H_{3} P O_{4})$
(C) aluminum chloride $(A l {C l}_{3})$
(D) sodium phosphate $({N a}_{3} P O_{4})$

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Solution

(A) Nitrate ion ${[{N O}_{3}]}^{-}$
(B) Phosphoric Acid $H_{3} {P O}_{4}$
(C) Aluminum chloride ${A l C l}_{3}$
(D) Sodium Phosphate ${N a}_{3} {P O}_{4}$

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Similar questions

Q. Formula of phosphoric acid is

H_{3} P O_{4}

? A metal M forms chloride of the formula

M C l_{2}

. What is the formula of its phosphate?

Identify the odd one out and justify.

(a) Chloride, nitrate, hydride, ammonium

(b) Hydrogen chloride, sodium hydroxide, calcium oxide, ammonia

(d) Ammonium chloride, sodium chloride, potassium nitrate, sodium sulphate

(e) Sodium nitrate, sodium carbonate, sodium sulphate, sodium chloride

(f) Calcium oxide, magnesium oxide, zinc oxide, sodium oxide.

(g) Crystalline blue vitriol, crystalline common salt, crystalline ferrous sulphate, crystalline sodium carbonate.

(h) Sodium chloride, potassium hydroxide, acetic acid, sodium acetate.

Assertion: Aluminium chloride

(A l C l_{3})

is a Lewis acid.

Reason: Lewis acids donate electrons to an acceptor.

Question 12
Write the molecular formulae for the following compounds

(a) Copper (II) bromide
(b) Aluminium (III) nitrate
(c) Calcium (II) phosphate
(d) Iron (III) sulphide
(e) Mercury (II) chloride
(f) Magnesium (II) acetate

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Draw Lewis structures for each of the following:(A) nitrate ion ([NO3]−)(B) phosphoric acid (H3PO4)(C) aluminum chloride (AlCl3)(D) sodium phosphate (Na3PO4)

(A) Nitrate ion [NO3]−(B) Phosphoric Acid H3PO4(C) Aluminum chloride AlCl3(D) Sodium Phosphate Na3PO4

Draw Lewis structures for each of the following:
(A) nitrate ion $({[{N O}_{3}]}^{-})$
(B) phosphoric acid $(H_{3} P O_{4})$
(C) aluminum chloride $(A l {C l}_{3})$
(D) sodium phosphate $({N a}_{3} P O_{4})$

(A) Nitrate ion ${[{N O}_{3}]}^{-}$
(B) Phosphoric Acid $H_{3} {P O}_{4}$
(C) Aluminum chloride ${A l C l}_{3}$
(D) Sodium Phosphate ${N a}_{3} {P O}_{4}$