(a)
Interpretation:
The similar chemical behaviors of chlorine, bromine, iodine and differences in between fluorine and other halogens have to be given.
Concept introduction:
Halogens: A group of non-metallic elements which are showing similar chemical properties in the periodic table (group 17).
(b)
Interpretation:
The similar chemical behaviors of chlorine, bromine, iodine and differences in between fluorine and other halogens have to be given.
Concept introduction:
Halogens: A group of non-metallic elements which are showing similar chemical properties in the periodic table (group 17).
(c)
Interpretation:
The similar chemical behaviors of chlorine, bromine, iodine and differences in between fluorine and other halogens have to be given.
Concept introduction:
Halogens: A group of non-metallic elements which are showing similar chemical properties in the periodic table (group 17).
(d)
Interpretation:
The similar chemical behaviors of chlorine, bromine, iodine and differences in between fluorine and other halogens have to be given.
Concept introduction:
Halogens: A group of non-metallic elements which are showing similar chemical properties in the periodic table (group 17).
(e)
Interpretation:
The similar chemical behaviors of chlorine, bromine, iodine and differences in between fluorine and other halogens have to be given.
Concept introduction:
Halogens: A group of non-metallic elements which are showing similar chemical properties in the periodic table (group 17).
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Chapter 22 Solutions
CHEMISTRY 4
- When 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_forwardUntil the early 1960s the group 8A elements were called the inert gases; before that they were called the rare gases. The term rare gases was dropped after it was discovered that argon accounts for roughly 1% of Earth’s atmosphere. (a) Why was the term inert gases dropped? (b) What discovery triggered this change in name? (c)What name is applied to the group now?arrow_forwardA certain element, M, is a main-group metal that reacts with chlorine to give a compound with the chemical formula MCl2 and with oxygen to give the compound MO.(a) To which group in the periodic table does element M belong?(b) The chloride contains 44.7% chlorine by mass. Name the element Marrow_forward
- Discuss each conclusion from a study of redox reactions:(a) The sulfide ion functions only as a reducing agent.(b) The sulfate ion functions only as an oxidizing agent.(c) Sulfur dioxide functions as an oxidizing or a reducing agentarrow_forward(a) The third row element with the largest first ionization energy. (b) The Group 3A element with the largest first ionization energy. (c) The Group 3A element with the largest atomic radius.arrow_forwardUse the data from Appendix F to graph the variation ofatomic radius with atomic number for the rare-earth elements from lanthanum to lutetium.(a) What is the general trend in these radii? How do you account for it?(b) Which two elements in the series present exceptions to the trend?arrow_forward
- Write a balanced equation for the reaction that occurs in each ofthe following cases: (a) Chlorine reacts with water. (b) Bariummetal is heated in an atmosphere of hydrogen gas. (c) Lithiumreacts with sulfur. (d) Fluorine reacts with magnesium metal.arrow_forward(a) Would you expect scandium oxide to be a solid, liquid, or gas at room temperature?arrow_forward(a) Why does xenon react with fluorine, whereas neon does not? (b) Using reference sources such as the CRC Handbook of Chemistry and Physics or online sources, look up the bond lengths of Xe—F bonds in several molecules. How do these numbers compare to the radii of the elements?arrow_forward
- 24. Which member of the following pairs has the larger radius? Provide your reasoning. (a) Al or S (b) Cl or Ca²+ (c) Ba or Sn (d) Na+ or Karrow_forwardSome versions of the periodic table show hydrogen at the topof Group 1A(1) and at the top of Group 7A(17). What properties of hydrogen justify each of these placements?arrow_forward(a) Briefly describe how the atomic radii and ionization energies of group 1A(1) elements compared with those of group 8A(18). Also, explain why the values of these properties are so different between these two groups. 2.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning