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Polar Covalent Compounds

Why should a ...

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Why should a cation like Na+ should act as a Lewis acid and tend to accept an electron although it has already attained stability by having a Nobel gas configuration?

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Q. ________ element has one electron in the outermost shell and attains duplet configuration after accepting one more electron and attains stability.

Q. Chemical compounds in which anions and cations are held together by electrostatic force of attraction are known as ionic compounds. Cations and anions are charged species which are formed by losing and gaining electron(s) respectively to attain the nearest noble gas configuration or stability. Usually metals lose their valence electrons to form cations while non-metals accept electrons and form anions. Being held by a strong electrostatic force of attraction between ions, ionic compounds have high melting and boiling points.

(i) Which of the following electronic configuration is correct for the given elements?

Q. Chemical compounds in which anions and cations are held together by electrostatic force of attraction are known as ionic compounds. Cations and anions are charged species which are formed by losing and gaining electron(s) respectively to attain the nearest noble gas configuration or stability. Usually metals lose their valence electrons to form cations while non-metals accept electrons and form anions. Being held by a strong electrostatic force of attraction between ions, ionic compounds have high melting and boiling points.

(iii) To form an ionic compound Z, element Y accepts two electrons from X. Which of the following properties is not shown by Z?

Assertion: Between

N a^{+}

A g^{+}

A g^{+}

is a stronger Lewis acid.

Reason: Larger the size of a cation, greater is its tendency to accept electrons.

Q. ____________ element has one electron in its outermost shell and attains duplet configuration after one more electron and attains stability.

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