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A period refers to a horizontal row in the periodic table where elements have the same number of electron shells. As you move across a period, the atomic number increases, and properties such as ionization energy and electronegativity change. A group, on the other hand, refers to a vertical column where elements share similar chemical … Read more
Periodicity refers to the recurring trends or patterns in the properties of elements when arranged in order of increasing atomic number. These trends include atomic radius, ionization energy, electron affinity, and electronegativity. The periodic repetition of these properties is due to the regular arrangement of electrons in energy levels or shells as you move across … Read more
Alkali metals are highly reactive because they have only one electron in their outermost shell, which they can easily lose to achieve a stable noble gas configuration. This makes alkali metals very eager to react with other elements, especially halogens, to form stable compounds. The reactivity increases down the group because the outer electron is … Read more
Noble gases have high ionization energies because they possess a stable electron configuration with a full outer shell. This stability makes it difficult to remove an electron from the outermost energy level. The strong attraction between the positively charged nucleus and the tightly bound electrons requires a considerable amount of energy to overcome, thus giving … Read more
The atomic radius decreases across a period from left to right due to the increasing nuclear charge (the number of protons in the nucleus). As more protons are added, the positive charge of the nucleus attracts the electrons more strongly, pulling them closer to the nucleus. Although electrons are added to the same energy level, … Read more
(a) Li, Na, KOrder: K < Na < Li.Ionization energy decreases as you move down the group because atomic size increases, and the outermost electron is farther from the nucleus, experiencing less attraction. (b) Cl, Br, IOrder: I < Br < Cl.Ionization energy decreases as you go down the group because the atomic size increases, … Read more
Alkali metals are found in the S-block of the periodic table because they have their valence electron in an s orbital. These elements, such as lithium (Li), sodium (Na), and potassium (K), have a single electron in their outermost s orbital, making them highly reactive. Related Questions: Write the valence shell electronic configuration of an … Read more
Sodium (Na) has a higher ionization energy than potassium (K) because sodium has a smaller atomic radius and its valence electron is closer to the nucleus. Potassium, being in the 4th period, has a larger atomic radius, and its valence electron is farther from the nucleus. This makes it easier for potassium to lose its … Read more
Sodium (Na) has a higher shielding effect than lithium (Li). This is because sodium has more electron shells (3 shells) compared to lithium (2 shells), and the inner electron shells shield the outermost electron from the pull of the nucleus more effectively, reducing the effective nuclear charge experienced by the outer electron. Related Questions: Write … Read more
Halogens are elements found in Group VIIA (17) of the periodic table. These elements include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). Halogens are highly reactive, especially with alkali metals and alkaline earth metals, and readily form salts such as sodium chloride (NaCl). Related Questions: Write the valence shell electronic configuration … Read more