Using the Periodic Table

Complete the table below. If necessary, use the periodic table. 

Complete the table below. Use the periodic table if necessary. ... 

Reelity Check You can use the periodic table to check your answer. See Figure 6.9 and the accompanying discussion. 

The simple trend in the formulas shown by the third-row elements demonstrates the importance of the inert gas electron populations. The usefulness of the regularities is evident. Merely from the positions of two atoms in the periodic table, it is possible to predict the most likely empirical and molecular formulas. In Chapters 16 and 17 we shall see that the properties of a substance can often be predicted from its molecular formula. Thus, we shall use the periodic table continuously throughout the course as an aid in correlating and in predicting the properties of substances. 

Using the periodic table as a guide, predict which of the following compounds form ionic solutions in water silicon carbide, SiC magnesium bromide, MgBr2 carbon tetrabromide, CBr chromic chloride, CrCl3. 

Knowing the orbitals carbon uses for bonding, use the periodic table to predict the formula of the chloride of silicon. What orbitals does silicon use for bonding ... 

We are now at the point where we can begin to use the periodic table as chemists and materials scientists do—to predict the properties of elements and see how they can be used to create the materials around us and to design new materials for tomorrow s technologies. 

For this qualitative problem, use the periodic table to determine the order of orbital filling. Locate the element in a block and identify its row and column. Move along the ribbon of elements to establish the sequence of filled orbitals. 

The predictions made by Mendeleev provide an excellent example of how a scientific theory allows far-reaching predictions of as-yet-undiscovered phenomena. Today s chemists still use the periodic table as a predictive tool. For example, modem semiconductor materials such as gallium arsenide were developed in part by predicting that elements in the appropriate rows and columns of the periodic table should have the desired properties. At present, scientists seeking to develop new superconducting materials rely on the periodic table to identify elements that are most likely to confer superconductivity. 

C08-0031. Construct an orbital energy level diagram for all orbitals with < 8 and / < 4. Use the periodic table to help determine the correct order of the energy levels. 

C08-0088. Use the periodic table to find and list (a) all elements whose ground-state configurations indicate that the 4 5" and 3 d orbitals are nearly equal in energy (b) the elements in the column that has two elements with one valence configuration and two with another valence configuration and (c) a set of elements whose valence configurations indicate that the 6 of and 5 f orbitals are nearly equal in energy. 

Use the periodic table, without looking up electronegativity values, to rank each set of three bonds from least polar to most polar (a) S—Cl, Te—Cl, Se—Cl and (b) C—S, C—O, C— F. 

The larger the difference in electronegativity, the more polar the bond. Therefore, we can use periodic trends in electronegativities to arrange these bonds in order of polarity. Electronegativities decrease down most columns and increase from left to right across the s and p blocks. Use the periodic table to compare electronegativity values and rank the bond polarities. 

Use the periodic table to count valence electrons. Boron, in Group 13, has three valence electrons... 

Read over the entire laboratory activity. Use the periodic table in your textbook to answer the following questions. 

Using the periodic table if necessary, write formulas for the following compounds (a) hydrogen bromide, (b) magnesium chloride, (c) barium sulfide, (d) aluminum fluoride, (e) beryllium bromide, (/) barium selenide, and (g) sodium iodide. 

An effective way to determine the detailed electron configuration of any element is to use the periodic table to determine which subshell to fill next. Each s subshell holds a maximum of 2 electrons each p subshell holds a maximum of 6 electrons each d subshell holds a maximum of 10 electrons and each / subshell holds a maximum of 14 electrons (Table 17-5). These numbers match the numbers of elements in a given period in the various blocks. To get the electron configuration, start at hydrogen (atomic number = 1) and continue in order of atomic number, using the periodic table of Fig. 17-10. 

There are a number of ways that we can use the periodic table to classify the elements. One way is to divide all the elements into three groups metals, metalloids, and nonmetals. Look at the periodic table in this book. Notice the... 

Answer the following questions. You have 25 minutes. You may not use a calculator. You may use the periodic table in the back of the book. 

Use the periodic table and other information concerning bonding and electronic structure to explain the following observations. 

Since the start of high school science courses, you have used the periodic table to help you investigate the composition and behaviour of the elements. Your early experiences with the periodic table were limited largely to the first 20 elements, because you could explain their electron structure without the concepts of orbitals and electron configurations. 

This reference work uses the periodic table of the elements as the basis for organizing the presentations of the elements. Once you learn how this remarkable chart is organized, you will be able to relate the characteristics of many elements to each other based on the structure, which can be determined by their placement on the periodic table. 

Use the periodic table and your knowledge of atomic numbers and mass numbers to fill in the missing pieces in the following table. 

Write the formula mass of (a) BaF2 and (b) C6H404 with a reasonable number of digits. Use the periodic table inside the cover of this book to find atomic masses. 

You can use the periodic table as a quick reference when determining the type of ion an atom tends to form. As Figure 6.6 shows, each atom of any group 1 element, for example, has only one valence electron and so tends to form the 1+ ion. Each atom of any group 17 element has room for one additional electron in its valence shell and therefore tends to form the 1— ion. Atoms of the noble gas elements tend not to form any type of ion because their valence shells are already filled to capacity. 

J.9 Use the periodic table to determine which oxides form acidic solutions in water and which form basic solutions (a) CaO (b) S03 (c) N203 (d) T120. 

The 112 known elements—there may be more by the time you read this—combine to form millions of compounds. That is far more than we could study individually. Moreover just learning a string of isolated facts would not build the insight we need to devise new compounds. It is far more useful to study a select group of representative elements and their compounds. In this and the next two chapters, we use the periodic table as our guide in this highly selective journey. The topics of these chapters are commonly called descriptive chemistry—the description of the preparation, properties, and applications of elements and their compounds. 

KEY CONCEPT PROBLEM 1.4 The three so-called "coinage metals" are located near the middle of the periodic table. Use the periodic table to identify them. 

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