Learning Materials
Features
Discover
Chapter 4: Problem 39
The elements present in d-block are (a) metals and non-metals (b) only metals (c) only non-metals (d) metals, metalloids and non-metals
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
Which of the following sequence of explanation is appropriate for explaining the reason for the periodicity of reducing property in a period or group? (1) Tendency to undergo oxidation decreases in a period and increases in a group. (2) In a period ionization energy increases and in a group it decreases. (3) In a period the atomic size decreases and in a group it increases. (4) The elements present in the left side of the periodic table have strong reducing property. (a) 3214 (b) 3421 (c) 4312 (d) 4213
Assertion (A): First ionization energy of beryllium is greater than that of boron. Reason (R): Boron has larger size than beryllium. (a) Both \(\mathrm{A}\) and \(\mathrm{R}\) are true and \(\mathrm{R}\) is the correct explanation of \(\mathrm{A}\). (b) Both \(\mathrm{A}\) and \(\mathrm{R}\) are true and \(\mathrm{R}\) is not the correct explanation of \(A\). (c) \(\mathrm{A}\) is true, \(\mathrm{R}\) is false (d) \(\mathrm{A}\) is false, \(\mathrm{R}\) is true
The general electronic configuration of representative elements is (a) \(\mathrm{ns}^{1-2} \mathrm{np}^{1-6}\) (b) \(\mathrm{ns}^{1-2} \mathrm{np}^{1-5}\) (c) \(\mathrm{ns}^{1-2}(\mathrm{n}-1) \mathrm{p}^{1-5}\) (d) \(\mathrm{ns}^{1-2}(\mathrm{n}-1) \mathrm{p}^{1-6}\)
The energy released when an electron is added to the valence shell of a neutral, gaseous, isolated atom is called (a) electronegativity (b) ionization potential (c) electron affinity (d) lattice energy
In a period, from the left to right the electron affinity increases, but alkaline earth metals have lower electron affinity than alkali metals because (a) alkaline earth metals have lesser atomic radius than alkali metals. (b) alkaline earth have higher electronegativity than alkali metals. (c) alkaline earth metals have completely filled "s-" orbitals. (d) alkaline earth metals have lesser electronegativity than alkali metals.
What do you think about this solution?
We value your feedback to improve our textbook solutions.
Explanations 
Textbooks 
Exams 
GCSE 
IGCSE 
AS 
A Level 
International A Level 
University Admissions Tests 
Flashcards 
Vaia AI 
Notes 
Study Plans 
Study Sets 
Find a job 
Find a degree 
Student Deals 
Magazine 
Mobile App