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What is the electronic configuration of (i) a sodium atom, and (ii) an oxygen atom?

What is the electronic configuration of (i) a sodium atom, and (ii) an oxygen atom?

(a) a sodium atom, and (ii) an oxygen atom

(C) Show the formation of Na^2O by the transfer of electrons between the combining atoms.

(d) Why are ionic compounds usually hard ?

(e) How is it that ionic compounds in the solid state do not conduct electricity but they do so when in

molten state ?​

The answer is :

a) When we write the configuration we'll put all 11 electrons in orbitals around the nucleus of the Sodium atom. ... Therefore the sodium electron configuration will be 1s22s22p63s1.

b) So now you have Na2O. When sodium (Na) atoms bond with one oxygen (O) atom, there have to be two sodium atoms, each with an extra electron. Each of these sodium atoms gives oxygen one electron, allowing oxygen to have a full shell with eight electrons

c) Metals and Non-metals. (a) Show the formation of Na2O by the transfer of electrons between the combining atoms. ... Thus it requires two sodium atoms to lose one electron each. In this case the doubly negative charge of oxide anion is balanced exactly by two single positively charged sodium cations.

d) The ionic compounds are usually hard because the ions are held by strong force of attraction as the positive and negative ions are strongly attracted to each other and difficult to separate.

e) Answer. In molten state or dissolved state ionic compounds conduct electricity because they contain charged particles called cations and anions. These ions are free to move to conduct electricity. Thus ionic compounds conduct electricity in molten state or solution but in solid state they do not conduct electricity.

Explanation:

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