Concept explainers
(a)
Interpretation:
The order of the increasing size of the elements
Concept Introduction:
Atomic size is half of the distance between the adjacent atoms in the molecule. Since the electron cloud has no fixed boundary so the size of the atom is measured with high difficulty.
(b)
Interpretation:
The order of the increasing size of the elements
Concept Introduction:
Atomic size is half of the distance between the adjacent atoms in the molecule. Since the electron cloud has no fixed boundary so the size of the atom is measured with high difficulty.
(c)
Interpretation:
The order of the increasing size of the elements
Concept Introduction:
Atomic size is half of the distance between the adjacent atoms in the molecule. Since the electron cloud has no fixed boundary so the size of the atom is measured with high difficulty.
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Chapter 8 Solutions
Chemistry: Principles and Practice
- Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends in ionization energy and atomic radius? Explain.arrow_forwardFor each of the following pairs of atoms or ions, state which you expect to have the larger radius. (a) Na or K (b) Cs or Cs+ (c) Rb+ or Kr (d) K or Ca (e) Cl or Ararrow_forwardTwo elements are in the same group, one following the other. One is a metalloid; the other is a metal. Both form oxides of the formula RO2. The first is acidic; the next is amphoteric. Identify the two elements.arrow_forward
- Rank the elements in each of the following sets in order of increasing atomic radius. (a) K, Na, Rb, Cs (b) Ne, O, B, Carrow_forwardWhich of the following statements is incorrect? (a) The second ionization energy of sulphur is greater than that of chlorine (b) The third ionization energy of phosphorus is greater than that of aluminium (c) The first ionization energy of aluminium is approximately the same as that of gallium (d) The second ionization energy of boron is greater than that of carbon a b O darrow_forwardArrange each set of atoms in order of increasing IE₁:(a) Sr, Ca, Ba(b) N, B, Ne(c) Br, Rb, Se (d) As, Sb, Snarrow_forward
- Arrange each set of atoms in order of increasing IE1: (a) Sr, Ca, Ba (b) N, B, Ne (c) Br, Rb, Se (d) As, Sb, Snarrow_forwardBe sure to answer all parts. On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs. (a) Na, Si: Si Na (b) Ba, Be: Ba Be (c) N, F: N F (d) Br, Cl: Br Cl (e) Ne, Kr: Kr Nearrow_forwardAn element has the following electronic configuration: [Kr]4d105s25p2(a) What period does it belong to?(b) What is its group number? (Use group numbers from 1 to 18)(c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?)(d) How many unpaired electrons are there in an atom of this element?arrow_forward
- Give the shell electron configuration for the following. (For example, the shell electron configuration of lithium is written 2,1.) (a) argon (b) magnesiumarrow_forwardArrange in order of increasing ionization energy. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Group 1A elements Na, H, and Li (b) the Period 4 elements Ga, Se, and Karrow_forwardWhich element in each of the following sets would you ex-pect to have the lowest IE₃?(a) Na, Mg, Al(b) K, Ca, Sc(c) Li, Al, Barrow_forward
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