Introductory Chemistry, Books a la Carte Edition (6th Edition)
6th Edition
ISBN: 9780134564074
Author: Nivaldo J. Tro
Publisher: PEARSON
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Question
Chapter 9, Problem 72E
Interpretation Introduction
Interpretation: The number of elements present in periods 3 and 4 of the periodic table is to be listed. The difference that lies in these numbers is to be explained.
Concept Introduction: Elements are arranged in the order of increasing
From the periodic table, physical, chemical properties, electronic configuration of
the elements can be determined.
The principal quantum number
As the value of principal quantum number increases, the energy of the orbital also
increases.
The possible values of principal quantum number are 1, 2, 3….
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The periodic table is the most important organizing principle in chemistry. There is a regular progression in the periodic table that reflects a similar regularity in the structures and properties of the different elements. If you know the properties of any one element in a group, you can make a good guess at the properties
of every other element in the same group and even the elements in neighboring groups. Familiarizing yourself with the structure and arrangement of the periodic table early on will help you later on in chemistry.
Part A
Classify the following elements as main group elements, transition metals, or inner transition metals.
Drag the appropriate elements to their respective bins.
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Main group elements
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Ca Sn Fm Pd Zn S
Transition metals
Inner transition metals
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Two main-group elements are highlighted in the outline of the Periodic Table below:
What can you say about these elements without knowing exactly which they are? Use that knowledge to answer the questions in the following table, if possible.
Important: do not try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't need
to. You will also be marked wrong for any answer, correct or not, that can't be determined from the rough location of each marked element in the Periodic Table.
Element X
Element Y
Which element in the gas phase is
more likely to glow green or yellow in
a flame?
X 5
O Can't say without more information.
O Element X
Which element is more likely to form
an ionic compound with chlorine?
O Element Y
O Can't say without more information.
O Element X
Which element in the solid state is
probably brittle, so that it breaks
before bending?
Element Y
Can't say without more information.
Explanation
Check
Four main-group elements a, b, c and d are highlighted in the outline of the Periodic Table below:
List these elements below in order of decreasing atomic radius. For example, if an atom of a is the biggest, and b the next biggest, then your list should start
b, ...
a
d
X
a
с
Important: don't try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't need
to. You will also be marked wrong for any answer, correct or not, that can't be determined from only the rough location of each marked element in the Periodic
Table.
0.000
b
S
Chapter 9 Solutions
Introductory Chemistry, Books a la Carte Edition (6th Edition)
Ch. 9 - Q1. Which set of wavelengths for light are...Ch. 9 - Which of the listed types of electromagnetic...Ch. 9 - Q3. Which electron transition in the Bohr model...Ch. 9 - What is the electron configuration of arsenic...Ch. 9 - Which orbital diagram corresponds to phosphorus...Ch. 9 - Q6. How many valence electrons does tellurium (Te)...Ch. 9 - Q7. The element sulfur forms an ion with what...Ch. 9 - Order the elements Sr, Ca, and Se in order of...Ch. 9 - Which of the listed elements has the highest...Ch. 9 - Q10. Which of the listed elements is most...
Ch. 9 - Which property decreases as you move down a column...Ch. 9 - Q12. When aluminum forms an ion, it loses...Ch. 9 - 1. When were the Bohr model the quantum-mechanical...Ch. 9 - 2. What is light? How fast does light travel?
Ch. 9 - 3. What is white light? Colored light?
Ch. 9 - Explain in terms of absorbed and reflected light,...Ch. 9 - What is the relationship between the wavelength of...Ch. 9 - 6. List some sources of gamma rays.
Ch. 9 - How are X-rays used?Ch. 9 - Why should excess exposure to gamma rays and...Ch. 9 - Why should excess exposure to ultraviolet light be...Ch. 9 - What objects emit infrared light? What technology...Ch. 9 - Why do microwave ovens heat food but tend not to...Ch. 9 - 12 .What type of electromagnetic radiation is used...Ch. 9 - Describe the Bohr model for the hydrogen atom.Ch. 9 - 14. What is an emission spectrum? Use the Bohr...Ch. 9 - 15. Explain the difference between a Bohr orbit...Ch. 9 - 16. What is the difference between the ground...Ch. 9 - 17. Explain how the motion of an electron is...Ch. 9 - 18. Why do quantum-mechanical orbital have “fuzzy”...Ch. 9 - 19. List the four possible subshells in the...Ch. 9 - 20. List the quantum-mechanical orbitals through...Ch. 9 - Prob. 21ECh. 9 - Prob. 22ECh. 9 - Within an electron configuration. What do symbols...Ch. 9 - Explain the difference between valence electrons...Ch. 9 - Identify each block in the blank periodic table....Ch. 9 - Prob. 26ECh. 9 - Prob. 27ECh. 9 - Prob. 28ECh. 9 - Prob. 29ECh. 9 - How far does light travel in each time period? a....Ch. 9 - 31. Which type of electromagnetic radiation has...Ch. 9 - 32. Which type of electromagnetic radiation has...Ch. 9 - List the types of electromagnetic radiation in...Ch. 9 - List the types of electromagnetic radiation in...Ch. 9 - List two types of electromagnetic radiation with...Ch. 9 - List two types of electromagnetic radiation with...Ch. 9 - List these three types of radiationinfrared,...Ch. 9 - List these three types of electromagnetic...Ch. 9 - Prob. 39ECh. 9 - 40. In the Bohr model, what happens when an...Ch. 9 - 41. Two of the emission wavelengths in the...Ch. 9 - 42. Two of the emission wavelengths in the...Ch. 9 - 43. Sketch the 1s and 2p orbitals. How do the 2s...Ch. 9 - Sketch the 3d orbitals. How do the 4d orbitals...Ch. 9 - Which electron is, on average closer to the...Ch. 9 - 46. Which electron is, on average, farther from...Ch. 9 - 47. According to the quantum-mechanical model for...Ch. 9 - Prob. 48ECh. 9 - 49. Write full electron configuration for each...Ch. 9 - 50. Write full electron configurations for each...Ch. 9 - 51. Write full orbital diagrams and indicate the...Ch. 9 - Write full orbital diagrams and indicate the...Ch. 9 - Write electron configurations for each element....Ch. 9 - Write electron configurations for each element....Ch. 9 - Prob. 55ECh. 9 - Prob. 56ECh. 9 - Write full electron configurations and indicate...Ch. 9 - 58. Write full electron configurations and...Ch. 9 - Write orbital diagrams for the valence electrons...Ch. 9 - 60. Write orbital diagrams for the valence...Ch. 9 - How many valence electrons are in each element? a....Ch. 9 - 62. How many valence electrons are in each...Ch. 9 - 63. List the outer electron configuration for each...Ch. 9 - Prob. 64ECh. 9 - Prob. 65ECh. 9 - Use the periodic table to write electron...Ch. 9 - Use the periodic table to write electron...Ch. 9 - 68. Use the periodic table to write electron...Ch. 9 - Prob. 69ECh. 9 - How many 3d electrons are in an atom of each...Ch. 9 - Prob. 71ECh. 9 - Prob. 72ECh. 9 - Name the element in the third period (row) of the...Ch. 9 - 74. Name the element in the fourth period of the...Ch. 9 - 75. Use the periodic table to identify the element...Ch. 9 - 76. Use the periodic table to identify the element...Ch. 9 - 77. Choose the element with the higher ionization...Ch. 9 - Choose the element with the higher ionization...Ch. 9 - Arrange the elements in order of increasing...Ch. 9 - 80. Arrange the elements in order of increasing...Ch. 9 - 81. Choose the element with the larger atoms from...Ch. 9 - Choose the element with the larger atoms from each...Ch. 9 - Prob. 83ECh. 9 - Prob. 84ECh. 9 - 85. Choose the more metallic element from each...Ch. 9 - Choose the more metallic element from each pair....Ch. 9 - 87. Arrange these elements in order of increasing...Ch. 9 - Arrange these elements in order of increasing...Ch. 9 - What is the maximum number of electrons that can...Ch. 9 - 90. What is the maximum number of electrons that...Ch. 9 - Use the electron configurations of the alkaline...Ch. 9 - Prob. 92ECh. 9 - Write the electron configuration for each ion....Ch. 9 - Write the electron configuration for each ion....Ch. 9 - Prob. 95ECh. 9 - 96. Examine Figure 4.14, which shows the elements...Ch. 9 - Prob. 97ECh. 9 - Identify what is wrong with each electron...Ch. 9 - Prob. 99ECh. 9 - Prob. 100ECh. 9 - Prob. 101ECh. 9 - Based on periodic trends, which one of these...Ch. 9 - When an electron makes a transition from n=3 to...Ch. 9 - Prob. 104ECh. 9 - The distance from the sun to Earth is 1.496108 km....Ch. 9 - Prob. 106ECh. 9 - 107. The wave nature of matter was first proposed...Ch. 9 - 108. The particle nature of light was first...Ch. 9 - Prob. 109ECh. 9 - When atoms lose more than one electron, the...Ch. 9 - 111. Excessive exposure to sunlight increases the...Ch. 9 - 112. The quantum-mechanical model, besides...Ch. 9 - Prob. 113QGWCh. 9 - 116. Using grammatically correct sentences,...Ch. 9 - 117. The first graph shown here is of the first...
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