Figure: 01-01 Title: Molecular models. Caption: The white, dark gray, and red spheres represent atoms of hydrogen, carbon, and oxygen, respectively.

Figure: 01-04 Title: The three physical states of water–water vapor, liquid water, and ice. Caption: The three physical states of water are common and familiar to us: water vapor, liquid water, and ice. We cannot see water vapor. What we see when we look at steam or clouds is tiny droplets of liquid water dispersed in the atmosphere. In this photo we see both the liquid and solid states of water. The molecular views show that the molecules in the solid are arranged in a more orderly way than in the liquid. The molecules in the gas are much farther apart than those in the liquid or the solid.

Figure: 01-05 Title: Molecular comparison of element, compounds, and mixtures. Caption: Each element contains a unique kind of atom. Elements might consist of individual atoms, as in (a), or molecules, as in (b). Compounds contain two or more different atoms connected, or bonded together, as in (c). A mixture contains the individual units of its components, shown in (d) as both atoms and molecules.

Figure: 01-06 Title: Relative abundances of elements. Caption: Elements in percent by mass in (a) Earth's crust (including oceans and atmosphere) and (b) the human body.

Figure: 01-07 Title: Electrolysis of water. Caption: Water decomposes into its component elements, hydrogen and oxygen, when a direct electrical current is passed through it. The volume of hydrogen (tube on the right) is twice the volume of oxygen, which is collected in the left tube.

Figure: 01-09 Title: Classification of matter. Caption: Classification scheme for matter. At the chemical level all matter is classified ultimately as either elements or compounds.

Figure: 01-10 Title: A chemical reaction. Caption: In chemical reactions the chemical identities of substances change. Here, a mixture of hydrogen and oxygen undergoes chemical change to form water.

Figure: 01-11 Title: The chemical reaction between a copper penny and nitric acid. Caption: The dissolved copper produces the blue-green solution; the reddish brown gas produced is nitrogen dioxide.

Figure: 01-12 Title: Separation by filtration. Caption: A mixture of a solid and a liquid is poured through a porous medium, in this case filter paper. The liquid passes through the paper while the solid remains on the paper.

Figure: 01-13 Title: Distillation. Caption: A simple apparatus for the separation of a sodium chloride solution (salt water) into its components. Boiling the solution evaporates the water, which is condensed, then collected in the receiving flask. After all the water has boiled away, pure sodium chloride remains in the boiling flask.

Figure: 01-14 Title: Separation of ink into components by paper chromatography. Caption: Separation of ink into components by paper chromatography. (a) Water begins to move up the paper. (b) Water moves past the ink spot, dissolving different components of the ink at different rates. (c) Water has separated the ink into its several different components.

Figure: 01-15 Title: The scientific method. Caption: The scientific method is a general approach to problems that involves making observations, seeking patterns in the observations, formulating hypotheses to explain the observations, and testing these hypotheses by further experiments. Those hypotheses that withstand such tests and prove themselves useful in explaining and predicting behavior become known as theories.

Figure: 01-18 Title: Comparison of the Kelvin, Celsius, and Fahrenheit temperature scales. Caption: The freezing point and boiling point of water as well as normal human body temperature is indicated on each of the scales.

Figure: 01-19 Title: Volume relationships. Caption: The volume occupied by a cube that is 1 m on each edge is a cubic meter, 1 m3 (top). Each cubic meter contains 1000 dm3 (middle). A liter is the same volume as a cubic decimeter, 1 L = 1 dm3. Each cubic decimeter contains 1000 cubic centimeters, 1 dm3 = 1000 cm3. Each cubic centimeter equals a millimeter, 1 cm3 = 1 mL (bottom).

Figure: 01-20 Title: Common volumetric glassware. Caption: The graduated cylinder, syringe, and buret are used in laboratories to deliver variable volumes of liquid; the pipet is used to deliver a specific volume of liquid. The volumetric flask contains a specific volume of liquid when filled to the mark.

Figure: 01-22 Title: A section of carbon nanotube. Caption: Each intersection in the network represents a carbon atom bonded to three others.

Figure: 01-24 Title: Precision and accuracy. Caption: The distribution of darts on a target illustrates the distinction between accuracy and precision.

Figure: 01-25 Title: Significant figures in measurements. Caption: The thermometer has markings every 5ºC. The temperature is between 25ºC and 30ºC and is approximately 27ºC. The two significant figures in the measurement include the second digit, which is estimated by reading between the scale marks.

Figure: 01-25-02UN Title: Conversion of pounds to grams. Caption: Flow chart for the conversion of pounds to grams.

Figure: 01-25-03UN Title: Conversion of m to in. Caption: Flow chart for the conversion of meters to inches.

Figure: 01-25-04UN Title: Conversion of in.3 to g. Caption: Cubic inches are converted to cubic centimeters and the density of gold is used as a conversion factor to find the number of grams of gold in a given volume.

Figure: 01-25-05UNE01.01 Title: Exercise 1.1 Caption: Elements, compounds, and mixtures.

Figure: 01-25-06UNE01.02 Title: Exercise 1.2 Caption: Chemical and physical change.

Figure: 01-25-07UNE01.04 Title: Exercise 1.4 Caption: Precision and accuracy.

Figure: 01-25-08UNE01.05a Title: Exercise 1.5 Caption: Measurements and significant figures.

Figure: 01-25-09UNE01.05b Title: Exercise 1.5 Caption: Measurements and significant figures.

Figure: 01-T01 Title: Table 1.1 Caption: The Top Ten Chemicals Produced by the Chemical Industry in 2003

Figure: 01-T02 Title: Table 1.2 Caption: Some Common Elements and Their Symbols

Figure: 01-T03 Title: Table 1.3 Caption: Comparison of Water, Hydrogen, and Oxygen

Figure: 01-T04 Title: Table 1.4 Caption: SI Base Units

Figure: 01-T05 Title: Table 1.5 Caption: Selected Prefixes Used in the Metric System

Figure: 01-T06 Title: Table 1.6 Caption: Densities of Some Selected Substances at 25ºC