![]() Now, ionization energy decreases down the group as the atomic size increases due to an increase in atomic size or energy shells. It tends to increase while moving across a period as the nuclear charge increases across a period that increases pull on electrons and thus more energy is required to remove an electron from an atom's valence shell. It is the minimum amount of energy required to remove an electron from an atom in its neutral or gaseous state. On the other hand, the valency of elements remains the same while moving down the group. The valency (the tendency to gain or lose electrons) first increases then decreases when we move from left to right in a period. However, there are few exceptions, such as in group 13, the electronegativity increases from Aluminium to Thallium and in the 14 th group tin is more electronegative than lead. Whereas, while moving down a group from top to bottom, the electronegativity decreases as the atomic size increases which reduce the nuclear pull on the electrons and thus the tendency of elements to gain electrons decreases. Electronegativity increases across a period from left to right as the atomic size decreases the pull on electrons increases which increases the element's tendency to gain electrons. It the tendency to gain or attract electrons. Non-metallic character or electronegativity: The reason is that the atomic size increases as the number of shells increase and thus the pull on electrons decreases that increases the tendency to lose an electron or metallic character or reactivity of elements. Whereas, while moving down the group the elements' electropositivity or tendency to lose electrons increases. The reason for this trend is that due to a decrease in atomic size the pull on the electrons increases, so, the atoms tend to gain electrons instead of losing. Now, as we move left to right in a period the metallic character as well as reactivity decreases. ![]() More is the metallic character, more is the reactivity of an element. The metallic character refers to the tendency to lose electrons or electropositivity. Metallic character or electropositivity or reactivity: An element with more number of shells will have more atomic size. However, the atomic size increases while moving down the group due to an increase in the number of shells. An increase in atomic number increases nuclear charge that increases pull on electrons, so, size of the atom tends to decrease. Now, the atomic size decreases across a period due to an increase in the atomic number or number of protons. Picometre is even smaller than a nanometre as 1 pm = 10 -12 metre, whereas, 1 nm = 10 -9 metre. The atomic radius is represented in picometre (pm) as it is very small. Whereas, the atomic radius refers to the shortest distance between the atom's nucleus and its outmost shell or the distance between atoms of the same element in a molecule. It refers to the distance between the centre of the nucleus of an atom and its outermost shell. Some of the most common periodic trends in the modern periodic table are described below Atomic size: Periodicity refers to the repetition of similar properties of elements when we move down a group or across a row after a specific interval or gaps between their atomic numbers. We can say that periodic trends occur in the periodic table due to the periodicity in the properties of elements. The periodic trends refer to the periodicity in properties of elements arranged in the periodic table. The valence electrons occupy higher levels due to the increasing quantum number (n).Next → ← prev Periodic Trends in the Periodic table \( \newcommand\): Periodic Table showing Atomic Radius Trendĭ own a group, atomic radius increases.
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