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In Figure 10-40, you see the result of opening the Properties palette with one line selected. To change either endpoint of the selected line, type new coordinates in the Properties palette and press Enter. Of course, this method of editing a line is useful only when you know the absolute coordinates that you want. When you select a geometric property, such as Start X, which is the X coordinate of the line s start point, you can also use the Pick a Point button that appears. You can click this button and then pick a new start point directly on your screen. The new point becomes the new start point of the line, changing both the X and Y coordinates of the start point if your pick point requires it. The information that you see in the Properties palette depends on the objects selected: If no object is selected, you see only properties that apply to the entire drawing, such as UCS, current layer, and viewport data. You can select an object while the window is open to display data on that object. If one object or one type of object (such as all lines) is selected, you see both general information and geometrical information on that object or object type. If more than one type of object is selected, you see general information, such as layer, color, and linetype data, but no geometry data. If more than one object is selected and you choose one type of object from the dropdown list at the top of the palette, you see information applying only to that type of object. This drop-down list provides a quick way to filter the type of objects that you can edit.

Tower . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Desktop/Rack Mount . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Cube . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . Laptop . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . All-In-One . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 18 19 20 21 22

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On the CD-ROM The drawing used in the following exercise on configuring a Microsoft Access database, ab20-a.dwg, is in the Drawings folder on the CD-ROM. This exercise requires that you have completed the steps in the previous exercises.

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combinations of devices that might be used with it. Thus the only feasible solution is to have each device in the system develop through the ve levels described above such that colorimetric, or color appearance, data (or the information necessary for obtaining it) can be handed off from one device to the next in the process known as device-independent color imaging.

the line, the gap is the space between the bottom of the text and the dimension line. The gap also controls the space between the box created for Basic tolerance dimensions and the text inside them. Basic tolerances are discussed in the Formatting tolerances section later in this chapter.

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40 Prevalence of overweight (%)

Covalent Bonding Covalent bonding is based on cooperative sharing of valence electrons. It can be described by orbital overlap. Covalent bonds are conspicuously directional: The bond is manifest in the direction of the greatest orbital overlap. The potential energy of a system of covalently interacting atoms depends not only on the type of atoms and the distances between atoms but also on the physical angles between bonds. The covalent bond model asserts that an atom can covalently bond with at most 8 n , where n is the number of valence electrons. Compounds that are formed due to covalent bonding of atoms are called covalent compounds. See Figure 3.2, middle. Covalent bonds are generally formed between nonmetals. Nitrogen gas (N2), hydrogen gas (H2), oxygen gas (O2), and hydrochloric acid (HCl) represent some of the examples of covalent bonded compounds. Most of the carbon bonds in organic materials (cells, sugar, etc.) are examples of covalent bonds. Since covalent bonds are directional in space, the molecules that arise have de nite shapes. The physical length of covalent bonds (distance between the atoms forming the respective bonds) is shorter than the length of an ionic bond. It follows that covalent bonds are harder to break compared with ionic bonds. Due to the absence of free ions, covalent compounds are not good conductors of heat and electricity. The characteristics

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