Chemistry 9

Write the valence shell electronic configuration for the following groups:

(a) Alkali metals: ns¹(b) Alkaline earth metals: ns²(c) Noble gases: ns² np⁶(d) Halogens: ns² np⁵ Related Questions: Write the valence shell electronic configuration of the atoms of the following elements: Write the valence shell electronic configuration of an element present in the 3rd period and Group IIA. Arrange the elements in each of the following … Read more

For normal elements, the number of valence electrons of an element is equal to the group number. Find the group number of the following elements:

H: Group 1 Al: Group 3 S: Group 6 K: Group 1 O: Group 6 Related Questions: Arrange the elements in each of the following in order of decreasing shielding effect: Specify which of the following elements you would expect to have the greatest electron affinity: S, P, Cl Electronic configurations of some elements are … Read more

Arrange the elements in groups and periods from Q. No. 6:

Groups: IIA: B IVA: None VA: E, G VIA: C, H VIIA: None Periods: Period 1: A, D Period 2: B, C, F Period 3: E, G, H Related Questions: Arrange the elements in each of the following in order of decreasing shielding effect: Specify which of the following elements you would expect to have … Read more

Electronic configurations of some elements are given below. Group the elements in pairs that would represent similar chemical properties:

A = 1s², 2s¹B = 1s², 2s², 2p⁶C = 1s², 2s², 2p³D = 1s¹E = 1s², 2s², 2p⁶, 3s², 3p³F = 1s², 2s²G = 1s², 2s², 2p⁶, 3s¹H = 1s², 2s², 2p⁴, 3s² Pairs representing similar chemical properties: A and D (Both are in Group I, alkali metals) B and F (Both are noble gases) … Read more

Specify which of the following elements you would expect to have the greatest electron affinity: S, P, Cl

Chlorine (Cl) has the greatest electron affinity. This is because chlorine has a high tendency to gain an electron to complete its valence shell, as it is only one electron away from achieving a stable noble gas configuration. Related Questions: Arrange the elements in each of the following in order of decreasing shielding effect: Write … Read more

Arrange the elements in each of the following in order of decreasing shielding effect:

(a) Li, Na, KOrder: K > Na > Li.The shielding effect increases as you move down the group because there are more electron shells, leading to more shielding. (b) Cl, Br, IOrder: I > Br > Cl.The shielding effect increases as you move down the group due to additional electron shells. (c) Cl, BrOrder: Br … Read more

Arrange the elements in each of the following groups in order of increasing ionization energy:

(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 belong to the S-block in the periodic table. Why?

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

Explain why Na has higher ionization energy than K.

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

Which atom has a higher shielding effect, Li or Na?

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