Chemistry: electron 2

1. The answer is : 1s^2 2^2 2p^6

The electron configuration of Na 1s^2 2^2 2p^6 3s^1.
An Na atom loses on electron to give Na^+.
Hence, the electronic configuration of Na^+ is 1s^2 2^2 2p^6
Any atom/ion with electronic configuration of 1s^2 2^2 2p^6 is said to be isoelectronic with Na^+.


2. The answer is : s and p electrons

Group IA : The outermost shell is ns^1.
Group IIA : The outermost shell is ns^2.
Group IIIA : The outermost shell is ns^2 np^1.
Group IVA : The outermost shell is ns^2 np^2.
Group VA : The outermost shell is ns^2 np^3.
Group VIA : The outermost shell is ns^2 np^4.
Group VIIA : The outermost shell is ns^2 np^5.
Group VIIIA / Group 0 : The outermost shell is ns^2 np^6.


3. The answer is : acid oxides and neutral oxides

For example, nitrogen forms to oxides : NO and NO2.
NO is a neutral oxide.
NO2 is an acidic oxide.

However, most of the non-metal oxides are acidic.


4. The answer is : lose electrons and form cations.

For example, when sodium reacts with a non-metal, sodium (Na) will lose electrons to form sodium cations (Na^+).


5. The answer is : definitely a metal

In the Periodic Table :
Down a group, the metallic property is increasing.
Across a period, the metallic property is decreasing.

Therefore, the element in the lower left corner would have the highest metallic property.
This element is definitely a metal.


6. The answer is : ns^2 np^2

Group IVA elements are d-block elements with 4 outermost shell electrons (ns^2 np^2).

(1) 1s22s22p6

(2) s, p, and d electrons

(3) acid oxides

(4) lose electrons and form cations

(5) definitely a metal

(6) ns2np3