(a)
Interpretation:
The elements, sulfur, chlorine and silicon has to be arranged in the decreasing order of atomic radius.
Concept Introduction:
Atomic radius is the distance between the atomic nucleus and outermost shell having electrons of an atom. From the atomic radius, the size of atoms can be visualized
Down the group, the principal quantum number increases and thus the size of orbital also increases which results in the increase in atomic radii.
Along the period, the valence electron is added to the same shell and thus attraction by the nucleus gets stronger. Therefore, atomic radii reduces from left to right in the periodic table.
(b)
Interpretation:
The elements, cobalt, titanium and chromium has to be arranged in the decreasing order of atomic radius.
Concept Introduction:
Refer to (a).
(c)
Interpretation:
The elements, zinc, mercury and cadmium has to be arranged in the decreasing order of atomic radius.
Concept Introduction:
Refer to (a).
(d)
Interpretation:
The elements, antimony, bismuth and phosphorus has to be arranged in the decreasing order of atomic radius.
Concept Introduction:
Refer to (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Chemical Principles: The Quest for Insight
- Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forwardWhen a nonmetal oxide reacts with water, it forms an oxoacid with the same oxidation number as the nonmetal. Give the name and formula of the oxide used to prepare each of these oxoacids: (a) hypochlorous acid; (b) chlorous acid; (c) chloric acid; (d) perchloric acid; (e) sulfuric acid; (f ) sulfurous acid; (g) nitric acid; (h) nitrous acid; (i) carbonic acid; ( j) phosphoric acid.arrow_forward(a) Rank elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (b) Explain why atomic size decreases from left to right, but increases from top to bottom; (c) Explain why ionization energy increases from left to right, but decreases from top to bottom; (d) Explain why the reactivity of alkali metals (Group-1) increases from top to bottom, where as the reactivity of halogen (Group-17) decreases from top to bottom.arrow_forward
- Using only the periodic table, rank the elements in each set in order of decreasing size: (a) As, Cs, S; (b) F, P, K.arrow_forwardb) For each pair indicate which Ion you would expect to have the largest Radius: (a) 02 and O; (b) N³ and Mg2+ (c) Al3* and Alarrow_forwardPlace the following elements in order of increasing covalent radius (i.e., from smallest to largest): Aluminum (Al) Boron (B) Fluorine (F) Helium (He) Potassium (K)arrow_forward
- Place the following elements in order of decreasing atomic size: bismuth, bromine, neon, cesium, barium, and arsenic. Rank from largest to smallest. To rank items as equivalent, overlap them.arrow_forwardUsing only their location in the periodic table, rank the atoms in each set by decreasing atomic size. Explain your answers. (a) Mg, Be, Ba (b) Se, Br, Cl (c) Ca, Se, Gaarrow_forwardClassify each of the following elements as a main-group or transition element. Also,specify whether they are metals, metalloids, or nonmetals: Na, Re, S, I, Kr, Mg, U, Si, B, Al, As, H.arrow_forward
- (a) Among the nonmetallic elements, the change in atomic radius in moving one place left or right in a row is smaller than the change in moving one row up or down. Explain these observations. (b) Arrange the following atoms in order of increasing atomic radius: Si, Al, Ge, Ga.arrow_forward(a) Why do successive IEs of a given element always increase? (b) When the difference between successive IEs of a given element is exceptionally large (for example, between IE1 and IE2 of K), what do we learn about its electron configuration? (c) The bars represent the relative magnitudes of the first five ionization energies of an atom: Identify the element and write its complete electron config uration, assuming it comes from (a) Period 2; (b) Period 3; (c) Period 4.arrow_forwardElements can be classified into groups based on their electron configurations. The representative elements are those that have s and p orbitals. The transition elements are elements that fill the d orbitals (groups 3–11 on the periodic table), and the inner transition metals are elements that fill the f orbitals. (a) Like first member of other groups, boron also differs from rest of the members of its group. Give two (2) properties that were only own by boron, and not the other members of its group. (b) Give two (2) similar properties shared by the diagonal effect pair of lithium and magnesiumarrow_forward
- Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHERGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningIntroductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co