Question 2 of b Incorrect Incorrect Sapling Learning Map d Classify each stateme
ID: 550502 • Letter: Q
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Question 2 of b Incorrect Incorrect Sapling Learning Map d Classify each statement about effective nuclear charge, Zeft, as true or false. True False Effective nuclear charge k Effective nuclear charge does not increases from left to right across a period on the periodic table. A 1s electron in a Be atom has a smaller Zeff than a 1s electron in a Li atom. depend on the number of Electrons in an s orbital electrons from the nuclear charge. electrons present in an atom. Across a period, as Zeff eases, atomic size increases. are more effective than those in other orbitals at shielding other In a N atom, a 1s electron s a greater Zem than a 2s electron. Hint O Previous Give Up & View Solution e Check Answer 0 Next a Exit !Explanation / Answer
True:
As the atomic number increases from left to right across a period on the periodic table. This is true because, the effective nuclear charge felt by the valence electrons also increases from left to right.
As, the order of electron penetration from greatest to least is s, p, d, f; the order of the amount of shielding done is also in the order s, p, d, f.
hence, statment "electrons in s orbital are more effective than those in other orbitals at shielding other electrons from the nuclear change" is true.
Zeff of 1s in N = 6.7 and Zeff of 2s in N = 3.9 hence statment : in a nitrogen atom, a 1s electron has a greater Zeff then a 2s electrons is true.
Flase:
Effective nuclear charge depend on both the nuclear charge and number of shielding electrons present in an atom. Hence statement : effective nuclear charge dose not depend on the number of electrons present in an atom" is false.
Zeff increases from left to right across a period, hence Li is on left to Be. Also, Li has Zeff = 2.7 and Be has Zeff = 3.7 for 1s electrons in each. Hence statement : "1s electron in Be atom has a smaller effective nuclear charge than a 1s electron in a Li atom" is false.
Effective nuclear charge increases from left to right across a period and therefore the atomic radius decreases as valancy electrons are added to same energy level, whereas number of protons increases which holds electrons more tightly. Hence statement: "across a period, as Zeff increases, atomic size increase" is false.
Atomic radius in 10-10 cm:
K = 243 (largest)
Rb = 265
Ca = 194
Mg = 145
Be = 112 (smallest)
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