Figure: 02-02 Title: An image of the surface of the semiconductor GaAs (gallium arsenide). Caption: This image was obtained by a technique called scanning tunneling electron microscopy. The color was added to the image by computer to distinguish the gallium atoms (blue spheres) from the arsenic atoms (red spheres).
Figure: 02-03 Title: Cathode-ray tube. Caption: (a) In a cathode-ray tube, electrons move from the negative electrode (cathode) to the positive electrode (anode). (b) A photo of a cathode-ray tube containing a fluorescent screen to show the path of the cathode rays. (c) The path of the cathode rays is deflected by the presence of a magnet.
Figure: 02-04 Title: Cathode-ray tube with perpendicular magnetic and electric fields. Caption: The cathode rays (electrons) originate from the negative plate on the left and are accelerated toward the positive plate, which has a hole in its center A beam of electrons passes through the hole and is then deflected by the magnetic and electric fields. The three paths result from different strengths of the magnetic and electric fields. The charge-to-mass ratio of the electron can be determined by measuring the effects that the magnetic and electric fields have on the direction of the beam.
Figure: 02-05 Title: Millikan's oil-drop experiment. Caption: A representation of the apparatus Millikan used to measure the charge of the electron. Small drops of oil, which had picked up extra electrons, were allowed to fall between two electrically charged plates. Millikan monitored the drops, measuring how the voltage on the plates affected their rate of fall. From these data he calculated the charges on the drops. His experiment showed that the charges were always integral multiples of 1.60 x 1019 C, which he deduced was the charge of a single electron.
Figure: 02-08 Title: Behavior of alpha (), beta (), and gamma () rays in an electric field. Caption: The rays consist of positively charged particles and are therefore attracted to the negatively charged plate. The rays consist of negatively charged particles and are attracted to the positively charged plate. The rays, which carry no charge, are unaffected by the electric field.
Figure: 02-09 Title: J. J. Thompson's “plum-pudding” model of the atom. Caption: Thompson pictured the small electrons to be embedded in the atom much like raisins in a pudding or like seeds in a watermelon. Ernest Rutherford proved this model wrong.
Figure: 02-10 Title: Rutherford's experiment on the scattering of particles. Caption: The red lines represent the paths of the particles. When the incoming beam strikes the gold foil, most particles pass straight through the foil but some are scattered.
Figure: 02-11 Title: Rutherford's model explaining the scattering of particles. Caption: The gold foil is several thousand atoms thick. Because most of the volume of each atom is empty space, most particles pass through the foil without deflection. When an particle passes very close to a gold nucleus, however, it is repelled, causing its path to be altered.
Figure: 02-12 Title: The structure of the atom. Caption: The nucleus, which contains protons and neutrons, is the location of virtually all the mass of the atom. The rest of the atom is the space in which the light, negatively charged electrons reside.
Figure: 02-12-01un Title: Symbol of an element. Caption: Symbol of carbon showing the mass number and atomic number.
Figure: 02-13 Title: A mass spectrometer. Caption: Cl atoms are introduced on the left side of the spectrometer and are ionized to form Cl+ ions, which are then directed through a magnetic field. The paths of the two isotopes of Cl diverge as they pass through the magnetic field. As drawn, the spectrometer is tuned to detect 35Cl+ ions. The heavier 37Cl+ ions are not deflected enough for them to reach the detector.
Figure: 02-14 Title: Mass spectrum of atomic chlorine. Caption: The fractional abundances of the 35Cl and 37Cl isotopes of chlorine are indicated by the relative signal intensities of the beams reaching the detector of the mass spectrometer.
Figure: 02-15 Title: Arranging the elements by atomic number reveals a periodic pattern of properties. Caption: This periodic pattern is the basis of the periodic table.
Figure: 02-16 Title: Periodic table of the elements. Caption: Different colors are used to show the division of the elements into metals, metalloids, and nonmetals.
Figure: 02-19 Title: Diatomic molecules. Caption: Seven common elements exist as diatomic molecules at room temperature.
Figure: 02-20 Title: Molecular models of some simple molecules. Caption: Notice how the chemical formulas of these substances correspond to their composition.
Figure: 02-21 Title: Different representations of the methane (CH4) molecule. Caption: Structural formulas, perspective drawings, ball-and-stick models, and space-filling models each help us visualize the ways atoms are attached to each other in molecules. In the perspective drawing, solid lines represent bonds in the plane of the paper, the solid wedge represents a bond that extends out from the plane of the paper, and dashed lines represent bonds behind the paper.
Figure: 02-21-02UN Title: Ionization of sodium. Caption: A sodium atom loses an electron to form a sodium ion.
Figure: 02-21-03UN Title: Formation of a chloride ion. Caption: A chlorine atom gains an electron to form a chloride ion.
Figure: 02-22 Title: Charges of some common ions. Caption: Notice that the steplike line that divides metals from nonmetals also separates cations from anions.
Figure: 02-23 Title: The formation of an ionic compound. Caption: (a) The transfer of an electron from a neutral Na atom to a neutral Cl atom leads to the formation of an Na+ and a Cl ion. (b) Arrangement of these ions in solid sodium chloride (NaCl). (c) A sample of sodium chloride crystals.
Figure: 02-24 Title: Biologically essential elements. Caption: The elements that are essential for life are indicated by colors. Red denotes the six most abundant elements in living systems (hydrogen, carbon, nitrogen, oxygen, phosphorus, and sulfur). Blue indicates the five next most abundant elements. Green indicates the elements needed in only trace amounts.
Figure: 02-26 Title: Summary of the procedure for naming anions. Caption: The root of the name (such as "chlor" for chlorine) goes in the blank.
Figure: 02-27 Title: Common oxyanions. Caption: The composition and charges of common oxyanions are related to their location in the periodic table.
Figure: 02-28 Title: Relationship between anion and acid names. Caption: Summary of the way in which anion names and acid names are related. Notice that the prefixes per- and hypo- are retained in going from the anion to the acid.
Figure: 02-29 Title: The two forms of propanol (C3H7OH). Caption: (a) 1-Propanol, in which the OH group is attached to one of the end carbon atoms, and (b) 2-propanol, in which the OH group is attached to the middle carbon atom.
Figure: 02-29-01UNE02.01 Title: Exercise 2.1 Caption: Path of a charged particle.
Figure: 02-29-02UNE02.02 Title: Exercise 2.2 Caption: Metals and nonmetals.
Figure: 02-29-03UNE02.03 Title: Exercise 2.3 Caption: Atom or ion.
Figure: 02-29-04UNE02.04 Title: Exercise 2.4 Caption: Ionic or molecular compound.
Figure: 02-29-05UNE02.05 Title: Exercise 2.5 Caption: IF5
Figure: 02-29-06UNE02.06 Title: Exercise 2.6 Caption: An ionic compound.
Figure: 02-29-07UNE02.45 Title: Exercise 2.45 Caption: Molecular models.
Figure: 02-29-08UNE02.46 Title: Exercise 2.46 Caption: Molecular models.
Figure: 02-29-09UNE02.80 Title: Exercise 2.80 Caption: Rb atoms.
Figure: 02-29-10UN02.91 Title: Exercise 2.91 Caption: Molecular structures.
Figure: 02-T01 Title: Table 2.1 Caption: Comparison of the Proton, Neutron, and Electron
Figure: 02-T02 Title: Table 2.2 Caption: Some Isotopes of Carbon
Figure: 02-T03 Title: Table 2.3 Caption: Names of Some Groups in the Periodic Table
Figure: 02-T04 Title: Table 2.4 Caption: Common Cations
Figure: 02-T05 Title: Table 2.5 Caption: Common Anions
Figure: 02-T06 Title: Table 2.6 Caption: Prefixes Used in Naming Binary Compounds Formed Between Nonmetals