Question

Atoms react to achieve an octet in the outermost shell. This is achieved by :
A.Sharing electrons
B.Gaining electrons
C.Losing electrons
D.All of the above

Answer 1

Hint: To answer this question, you should recall the concept of octet rule. The octet rule refers to the tendency of atoms to like better to have eight electrons within the valence shell. This is considered as a stable arrangement.

Complete Step by step solution:
We know that octets are often made up of their own electrons and a few electrons which are shared. Thus, an atom continues to make bonds until an octet of electrons is formed. When atoms have electrons more or but eight electrons, they react with other atoms or ions to make more stable compounds. The d or f electrons aren't considered within the octet rule.
Only the s and p electrons are involved within the octet rule, making it useful for the representative elements. The following facts can be discussed for the elements:
Atoms of the representative elements achieve an inert gas configuration by gaining or losing electrons and becoming ions, or by sharing electrons.
• Helium, in Period 1, is the first noble gas with an exceptional electronic configuration. In Period 2, lithium atoms in Group 1 lose their single valence electron to become a positively charged 1+ ion, and beryllium atoms in Group 2 will lose their two valence electrons to become 2+ ions. After losing their valence electrons, lithium and beryllium ions will have the inert gas configuration of helium in Period 1.
• The atoms of the rest of the representative elements (Groups 13-17) in Period 2 will gain, lose, or share electrons to achieve the noble gas of Neon at the end of Period 2.
• the remainder of the representative elements (Groups 1, 2, 13-17), will follow an equivalent pattern because of the Period 3 elements.
• The s-block elements will lose their valence electrons to realize the electron configuration of the inert gas within the previous period, and therefore the p-block elements will lose, gain, or share electrons to understand the electron configuration of the noble gas at the highest of that period.
• The transition elements behave differently, and lots of form ions of quiet one charge, like iron, which may form 2+ and 3+ ions hence not considered a neighborhood of the octet rule. But they still lose electrons to form charged ions with stable electron configurations, but not noble gas configurations.
Therefore, we will conclude that the right answer to the present question is option D.


Note: There are 4 blocks within the periodic table: s-block, p-block, d-block and f-block. All of the s-block elements are metals. Usually, they're shiny, silvery, good conductors of warmth and electricity, and lose their valence electrons easily. The p-block has the foremost important kind of elements and is that the sole block that contains three kinds of elements: metals, nonmetals and metalloids. d-block elements have properties that are between s-block elements and p-block elements properties. It consists of transition metals. The f-block elements are mostly radioactive.