(a) What is the collective name for the group 18 elements? (b) Write down, in order, the names and symbols of these elements; check your answer by reference to the first page of this chapter. (c) What common feature does the ground state electronic configuration of each element possess?
(a)
Interpretation:
The collective name of the group 18 elements must be interpreted.
Concept introduction: All known elements are arranged in the form of the periodic table. Here, the elements are arranged in the increasing order of their atomic number.
The table is divided into 18 groups and 7 rows which are called periods. The elements of the same group show a periodic trend in their chemical and physical properties.
Answer to Problem 1P
The collective name of the group-18 elements is noble gases or inert elements.
Explanation of Solution
The elements of group-18 have the general electronic configuration as
(b)
Interpretation:
The name and symbols of the elements of the group 18 elements must be interpreted.
Concept introduction: All known elements are arranged in the form of the periodic table. Here the elements are arranged in the increasing order of their atomic number.
The table is divided into 18 groups and 7 rows which are called periods. The elements of the same group show a periodic trend in their chemical and physical properties.
Answer to Problem 1P
Element | Name of the element |
Helium | |
Neon | |
Argon | |
Krypton | |
Xenon | |
Radon |
Explanation of Solution
The elements of group-18 have the general electronic configuration as
Element | Name of the element |
Helium | |
Neon | |
Argon | |
Krypton | |
Xenon | |
Radon |
(c)
Interpretation:
The common feature of the ground state electronic configuration of each element of the group 18 elements must be interpreted.
Concept introduction: All known elements are arranged in the form of the periodic table. Here, the elements are arranged in the increasing order of their atomic number.
The table is divided into 18 groups and 7 rows which are called periods. The elements of the same group show a periodic trend in their chemical and physical properties.
Answer to Problem 1P
The common feature for these elements is the octet configuration of all elements in their valence shell excluding Helium that has duplet configuration.
Explanation of Solution
The elements of group-18 have the general electronic configuration as
Element | Name of the element | Valence Electronic configuration |
Helium | ||
Neon | ||
Argon | ||
Krypton | ||
Xenon | ||
Radon |
The common feature for these elements is the octet configuration of all elements in their valence shell excluding Helium, which has a duplet configuration.
This configuration makes them stable and least reactive compare to other elements.
Want to see more full solutions like this?
Chapter 18 Solutions
Inorganic Chemistry
Additional Science Textbook Solutions
Organic Chemistry
Organic Chemistry
Chemistry
The Organic Chem Lab Survival Manual: A Student's Guide to Techniques
Chemistry by OpenStax (2015-05-04)
Organic Chemistry As a Second Language: Second Semester Topics
- 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) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction 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_forwardBoron, 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_forward(a) The electronic configuration of a certain element known as element A, is 1s22s22p3. Write a balanced equation to represent the first (1st) ionization energy of element A. Use “A” as the symbol of the element. Include the physical states used. Either: Sketch and insert a graph showing the general form which you would expect for the seven ionization energies of element A, labelling the axes. Or Describe the graph that could be drawn, which should include the following: What is the label on the vertical axis of the graph, include units? What is the label on the horizontal axis of the graph? Describe the pattern expected in the graph Describe the shape of the amide ion (NH2-), using Valence Shell Electron Pair Repulsion (VSEPR) theory. State the bond angles and the shape of the amide ion. You may sketch and insert a suitable diagram to aid your description if…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_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(a) The electronic configuration of a certain element known as element E, is 1s22s22p4. Write a balanced equation to represent the first (1st) ionization energy of element E. Use “E” as the symbol of the element. Include the physical states.arrow_forward
- 9(a) Describe the Bohr model of the atom, including quantization and emission spectra. (b) Discuss the successes and failures of the Bohr modelarrow_forwardWrite the predicted electron configuration for each of the following elements. (a) He (b)Be (c) Co. (d) Cdarrow_forward(a) Write the electron configuration for silicon, element 14,in its ground state. (b) How many unpaired electrons does aground-state silicon atom possess?arrow_forward
- (a) Predict the atomic number of the (as yet undiscovered) alkali-metal element in the eighth period. (b) Suppose the eighth-period alkali-metal atom turned out to have atomic number 137. What explanation would you give for such a high atomic number (recall that the atomic number of francium is only 87)?arrow_forward1. An element has the following electronic configuration: [Kr]4d105s25p4(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? 3. (a) Which of the following atoms or ions is diamagnetic?Li+ Ni2+ Al Fe2+ Mn3+(b) Which of the following atoms or ions is paramagnetic?C4- S4+ V4+ Se2- Ge4+arrow_forward(a) Describe the trends of atomic size and ionization energy, respectively, in the Periodic Table: (1) from left to right across a period, and (ii) from top to bottom down a group. (b) Rank the following elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (c) Rank the following elements: F, CI, Br and I, in increasing order of: (i) atomic size; (ii) electron affinity, (iii) electronegativity, and (iv) reactivity.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co