Use the periodic table to answer the following questions.- Identify an element with five electrons in the outer subshell.
- Identify an element that would tend to lose two electrons.
- Identify an element that would tend to gain two electrons.
- Identify the group having metal, non-metal, liquid as well as gas at the room temperature.
- Identify an element with five electrons in the outer subshell.
- Identify an element that would tend to lose two electrons.
- Identify an element that would tend to gain two electrons.
- Identify the group having metal, non-metal, liquid as well as gas at the room temperature.
Solution and Explanation
(a) The electronic configuration of an element having \(5\) electrons in its outermost subshell should be \(ns ^2 np^ 5\) . This is the electronic configuration of the halogen group.
Thus, the element can be \(F, CL, Br, I\), or \(At\).
(b) An element having two valence electrons will lose two electrons easily to attain the stable noble gas configuration. The general electronic configuration of such an element will be \(ns ^2\) . This is the electronic configuration of group \(2\) elements.
The elements present in group \(2\) are \(Be, Mg, Ca, Sr, Ba\).
(c) An element is likely to gain two electrons if it needs only two electrons to attain the stable noble gas configuration. Thus, the general electronic configuration of such an element should be \(ns^ 2 np^ 4\) . This is the electronic configuration of the oxygen family.
(d) Group \(17\) has metal, non-metal, liquid as well as gas at room temperature.
Top Questions on Periodic Trends In Properties Of Elements
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Concepts Used:
Trends in Periodic Table
The following trend in periodic properties of elements is observed:
Atomic size Trends:
The distance between the centre of the nucleus and the outermost shell of an atom is known as the atomic radius. In a group the atomic size increases due to the addition of shells as we move from one period to another. Across a period the atomic size decreases as the number of shells remain the same while the nuclear charge increases.
Metallic character Trends:
The elements which lose electrons to form cations are known as metals. Metallic character increases as we move down the group because the atomic size increases which lead to easy loss of electrons. On the other hand, it decreases across a period as we move from left to right.
Non-metallic character Trends:
The elements which have a tendency to gain electrons are known as non-metals. The tendency to gain electrons increases on moving across a period due to an increase in the nuclear charge and decrease in the atomic size. Hence, non-metallic character increases across a period.
Ionization potential Trends:
Ionization potential is defined as the amount of energy required to remove an electron from the outermost shell of a gaseous atom and convert it into a positively charged gaseous ion. The periodic properties in terms of ionization potential increase because the atomic size decreases across a period due to increase in the nuclear charge.
Melting Point Trends:
The melting point of an element is basically the energy required to change the state of an element from its solid state to its liquid state. Which essentially implies breaking a few bonds. Thus, higher the stronger the bond between the atoms, higher will be the melting point.