Cuprous copper and/or silver halophosphate glasses

BACKGROUND OF THE INVENTION
Most inorganic glasses at room temperature typically demonstrate values of electrical resistivity well in excess of 10.sup.8 ohm cm. However, it has long been recognized that a transparent membrane with high ionic conductivity would have considerable value. Thus, glasses with low electrical resistivities can have utility in electrochemical devices which demand high ionic conductivity.
The high ionic conductivity of copper and silver ions is well-known and glasses containing those ions have been formulated. Nevertheless, this prior research has not fully exploited the full capability of such glasses. For example, such glasses may exhibit an electrochromic phenomenon due to the electrochemical reduction of the copper and/or silver ions to the respective metal.
SUMMARY OF THE INVENTION
The present invention is founded in the discovery that glasses having compositions within the copper and/or silver-halide-phosphate system, wherein at least one halide is selected from the group of fluoride, bromide, chloride, and iodide, can be produced which have low softening points, high coefficients of thermal expansion, and which may have high conductivity and exhibit electrochromic behavior. The copper-containing glasses may also demonstrate thermochromic characteristics. Thus, such glasses have softening points below 400.degree. C. and, in some instances, below 150.degree. C. The coefficients of thermal expansion (25.degree.-300.degree. C.) are generally in excess of 180.times.10.sup.-7 /.degree. C. and, hence, approximate those of certain metals. The glasses demonstrate electrical resistivities less than 10.sup.8 ohm cm. at room temperature (.about.25.degree. C.), preferably less than 10.sup.7 ohm cm, with certain compositions ranging down to less than 10.sup.3 ohm cm. Finally, the glasses can exhibit electrochromism based upon their high ionic conductivity.
Electrochromism is the change in color of an electrode due to the passage of electric current. Color is typically produced electrochemically via the reduction of an ion to the metal at the cathode or a change in oxidation state of a colorless ion to a colored ion at the cathode or anode. In the darkened state the charge is stored electrochemically, i.e., the system is the charged state of a battery. Fading of the color is promoted by shorting the electrodes or by reversing the d.c. field. If the electrodes are shorted, the driving force for fading is the internal EMF of the battery and, consequently, will typically be slow. However, if a reverse field of the same magnitude as that utilized to cause darkening is applied, then fading will be more rapid than darkening since the internal EMF of the system adds to the applied EMF.
FIGS. 1, 2, and 3 constitute ternary composition diagrams illustrating the areas of stable glasses which have been produced in the Cu.sub.2 O-CuCl-P.sub.2 O.sub.5, the Cu.sub.2 O-CuBr-P.sub.2 O.sub.5, and the Cu.sub.2 O-CuI-P.sub.2 O.sub.5 system, respectively. Hence, in each diagram, transparent, stable glasses exhibiting a light yellow to amber color and demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm are depicted within the area delimited ABCD expressed in weight percent as calculated from the batch.
In FIG. 1, points A, B, C, and D have the approximate values recited below:
A=0% Cu.sub.2 O, 70% CuCl, 30% P.sub.2 O.sub.5
B=40% Cu.sub.2 O, 30% CuCl, 30% P.sub.2 O.sub.5
C=20% Cu.sub.2 O, 30% CuCl, 50% P.sub.2 O.sub.5
D=0% Cu.sub.2 O, 50% CuCl, 50% P.sub.2 O.sub.5
Glass compositions containing less than 30% CuCl were quite dark in color and showed electrical resistivities in excess of 10.sup.8 ohm cm. Compositions wherein the P.sub.2 O.sub.5 content exceeded 50% were poorly durable and also exhibited electrical resistivities greater than 10.sup.8 ohms. Compositions having less than 30% P.sub.2 O.sub.5 proved to be unstable with regard to devitrification. As can be seen, good stable glasses of high conductivity can be formed on the CuCl-P.sub.2 O.sub.5 binary.
In FIG. 2, points A, B, C, and D have the approximate concentrations reported below in weight percent:
A=0% Cu.sub.2 O, 70% CuBr, 30% P.sub.2 O.sub.5
B=50% Cu.sub.2 O, 20% CuBr, 30% P.sub.2 O.sub.5
C=40% Cu.sub.2 O, 10% CuBr, 50% P.sub.2 O.sub.5
D=0% Cu.sub.2 O, 50% CuBr, 50% P.sub.2 O.sub.5
Most of these glasses appeared to be somewhat lighter in color than the corresponding glasses containng CuCl. This phenomenon is believed to indicate less sensitivity to redox conditions in the melt. The same parameters were used to judge satisfactory glasses as were used with the CuCl-containing glasses. Acceptable glasses were found at higher Cu.sub.2 O levels than were seen in the Cu.sub.2 O-CuCl-P.sub.2 O.sub.5 system.
In the FIG. 3, points A, B, C, and D have the following approximate compositions in weight percent:
A=0% Cu.sub.2 O, 70% CuI, 30% P.sub.2 O.sub.5
B=50% Cu.sub.2 O, 20% CuI, 30% P.sub.2 O.sub.5
C=40% Cu.sub.2 O, 10% CuI, 50% P.sub.2 O.sub.5
D=0% Cu.sub.2 O, 50% CuI, 50% P.sub.2 O.sub.5
The composition ranges of suitable glasses were found to be essentially identical to those of the CuBr-containing glasses. Again, the same parameters were utilized to judge acceptable glasses as were used with the CuCl-containing glasses. In like manner to the CuBr and CuCl-containing glasses, good stable glasses demonstrating low electrical resistivities were found on the CuI-P.sub.2 O.sub.5 binary.
It will be appreciated, of course, that a combination of two or three halides, may be present in the glass compositions.
FIG. 4 illustrates that feature in that it constitutes a ternary composition diagram setting forth an area of stable glasses, expressed in terms of mole percent, demonstrating electrical resitivities at 25.degree. C. of less than 10.sup.8 ohm cm which have been formed in the Cu.sub.2 O-P.sub.2 O.sub.5 -X system wherein X is at least one halide selected from the group of Cl, Br, and I. Points A, B, and C have the following approximate compositions in mole percent:
A=35% Cu.sub.2 O, 50% P.sub.2 O.sub.5, 15% X
B=55% Cu.sub.2 O, 30% P.sub.2 O.sub.5, 15% X
C=35% Cu.sub.2 O, 30% P.sub.2 O.sub.5, 35% X
The center of the scribed triangle is a point having the molecular formula Cu.sub.2 O.multidot.P.sub.2 O.sub.5 .multidot.1/2X, where X is one or more of the group Cl, Br, and I.
FIGS. 5, 6, 7, 8, 9, 10, and 11 represent ternary composition diagrams illustrating the areas of stable glasses demonstrating electrical resistivities at 25.degree. C. of less than 10.sup.8 ohm cm which have been formed in the Ag.sub.2 O-AgCl-P.sub.2 O.sub.5, the Ag.sub.2 O-AgBr-P.sub.2 O.sub.5, the Ag.sub.2 O-AgI-P.sub.2 O.sub.5, the Cu.sub.2 O-P.sub.2 O.sub.5 -F, the Cu.sub.2 O-P.sub.2 O.sub.5 -Cl/F, the Cu.sub.2 O-P.sub.2 O.sub.5 -Br/F, and the Cu.sub.2 O-P.sub.2 O.sub.5 -I/F system, respectively.
In FIG. 5, points A, B, C, and D have the approximate values set out below in weight percent:
A=42% Ag.sub.2 O, 46% AgCl, 12% P.sub.2 O.sub.5
B=73% Ag.sub.2 O, 3% AgCl, 24% P.sub.2 O.sub.5
C=52% Ag.sub.2 O, 3% AgCl, 45% P.sub.2 O.sub.5
D=30% Ag.sub.2 O, 46% AgCl, 24% P.sub.2 O.sub.5
Although glasses free from chloride can be prepared which are ionic conducting and electrochromic, the durability and electrical conductivity thereof are significantly improved through the addition of chloride to the composition. Accordingly, a finite amount of chloride will be incorporated into the glass composition effective to improve those properties. In general, chloride in an amount of at least 1% will be included in the composition (1% Cl.ident.3% AgCl) with at least 5% being preferred.
Glasses within the area ABCD vary in color from colorless to a pale yellow, are quite fluid, can exhibit electrochromic behavior, and soften at temperatures between about 200.degree.-400.degree. C. Rather rapid cooling of the individual melts was necessitated since several thereof tended to devitrify upon slow cooling. Compositions containing excessive amounts of P.sub.2 O.sub.5 formed glasses which were poorly durable and demonstrated electrical resistivities greater than 10.sup.8 ohm cm. The presence of Ag.sub.2 O and/or AgCl in high quantities reduces the stability of the glass against devitrification.
In FIG. 6, points A, B, C, and D have the approximate values reported below in weight percent:
A=36% Ag.sub.2 O, 56% AgBr, 8% P.sub.2 O.sub.5 ps
B=74% Ag.sub.2 O, 2% AgBr, 24% P.sub.2 O.sub.5
C=54% Ag.sub.2 O, 2% AgBr, 44% P.sub.2 O.sub.5
D=24% Ag.sub.2 O, 56% AgBr, 20% P.sub.2 O.sub.5
Similarly to the AgCl-containing glasses discussed above, bromide is incorporated into the composition in an effective amount, usually at least about 1% (1% Br.ident.2% AgBr) with a minimum of 5% being preferred, to improve the durability and electrical conductivity of the glass. The glasses within area ABCD were pale yellow in color and, like the AgCl-containing glasses above, can exhibit electrochromic behavior, are quite fluid, and soften at temperatures below about 400.degree. C. The same parameters were used to judge acceptable glasses as were used with the AgCl-containing glasses. Higher Ag.sub.2 O levels were found operable than were seen in the Ag.sub.2 O-AgCl-P.sub.2 O.sub.5 system glasses.
In FIG. 7, points A, B, C, D, and E have the following approximate compositions in weight percent:
A=16% Ag.sub.2 O, 70% AgI, 14% P.sub.2 O.sub.5
B=35% Ag.sub.2 O, 60% AgI, 5% P.sub.2 O.sub.5
C=74.5% Ag.sub.2 O, 1.5% AgI, 24% P.sub.2 O.sub.5
D=53.5% Ag.sub.2 O, 1.5% AgI, 45% P.sub.2 O.sub.5
E=16% Ag.sub.2 O, 40% AgI, 44% P.sub.2 O.sub.5
In like manner to the AgCl-containing glasses, iodide is included in the composition in an effective amount, typically at least about 1% (1% I.ident.1.5% AgI) with at least 5% being preferred, to enchance the durability and electrical conductivity of the glass. The glasses within area ABCDE were a darker yellow than the AgBr-containing compositions. Glasses still higher in AgI content were found to exhibit good ionic conductivity but were very dark brown in color and/or darkened in visible light. The same parameters were employed to judge satisfactory glasses as were used with the AgCl-containing glasses. Concentrations of AgI higher than either AgCl or AgBr are operable in the invention.
In FIG. 8, points A, B, C, D, and E have the following approximate compositions in weight percent:
A=90% P.sub.2 O.sub.5, 9% Cu.sub.2 O, and 1% F
B=69% P.sub.2 O.sub.5, 30% Cu.sub.2 O, and 1% F
C=50% P.sub.2 O.sub.5, 30% Cu.sub.2 O, and 20% F
D=50% P.sub.2 O.sub.5, 15% Cu.sub.2 O, and 35% F
E=62% P.sub.2 O.sub.5, 3% Cu.sub.2 O, and 35% F
F=90% P.sub.2 O.sub.5, 3% Cu.sub.2 O, and 7% F
Glass compositions containing more than 90% P.sub.2 O.sub.5 were so poorly durable as to be essentially useless from a practical point of view, whereas when less than 50% P.sub.2 O.sub.5 was utilized the glasses were difficult to melt and/or unstable with respect to devitrification. The presence of fluoride improves the electrical conductivity of the simple Cu.sub.2 O-P.sub.2 O.sub.5 glasses. However, the glasses exhibited a very dark green color.
It will be recognized that a combination of two or three halides may be present in the glass compositions. This is evidenced in FIGS. 9, 10, and 11.
FIG. 9 sets forth the operable composition area of the system P.sub.2 O.sub.5 -Cu.sub.2 O-F/Cl in weight percent wherein the total F/Cl represents the sum of equal molar amounts of F and Cl. In FIG. 8, points A, B, C, D, E, and F have the following approximate compositions in weight percent:
A=40% P.sub.2 O.sub.5, 55% Cu.sub.2 O, 5% F/Cl
B=20% P.sub.2 O.sub.5, 75% Cu.sub.2 O, 5% F/Cl
C=15% P.sub.2 O.sub.5, 75% Cu.sub.2 O, 10% F/Cl
D=15% P.sub.2 O.sub.5, 45% Cu.sub.2 O, 40% F/Cl
E=25% P.sub.2 O.sub.5, 35% Cu.sub.2 O, 40% F/Cl
F=40% P.sub.2 O.sub.5, 35% Cu.sub.2 O, 25% F/Cl
Less than about 15% P.sub.2 O.sub.5 hazards glass instability. The glasses demonstrated colors ranging from light yellow, through amber, to a red amber appearance. The mixture of halide displays a very positive effect in lowering electrical resistivity when compared with any one alone. Thus, resistivities of less than 10.sup.4 ohm cm have been measured at room temperature.
FIG. 10 reports the operable composition area of the system P.sub.2 O.sub.5 -Cu.sub.2 O-F/Br in weight percent. In like manner to F/Cl in FIG. 9, the expression F/Br represents the sum of equal molar amounts of F and Br. Points A, B, C, D, E, and F have the following approximate compositions in weight percent:
A=50% P.sub.2 O.sub.5, 45% Cu.sub.2 O, 5% F/Br
B=20% P.sub.2 O.sub.5, 75% Cu.sub.2 O, 5% F/Br
C=15% P.sub.2 O.sub.5, 75% Cu.sub.2 O, 10% F/Br
D=15% P.sub.2 O.sub.5, 45% Cu.sub.2 O, 40% F/Br
E=40% P.sub.2 O.sub.5, 20% Cu.sub.2 O, 40% F/Br
F=50% P.sub.2 O.sub.5, 20% Cu.sub.2 O, 30% F/Br
As was the case with the F/Cl compositions, glasses containing less than about 15% P.sub.2 O.sub.5 are unstable with regard to devitrification. Also, the glasses exhibited coloration ranging from light yellow to red amber and electrical resistivities approaching 10.sup.3 ohm cm have been measured at room temperature.
FIG. 11 diagrams the operable composition area of the system P.sub.2 O.sub.5 -Cu.sub.2 O-F/I in weight percent. Similarly to F/Cl in FIG. 9 and F/Br in FIG. 10, the term F/I represents the sum of equal molar amounts of F and I. Points A, B, C, D, E, and F have the following approximate compositions in weight percent:
A=50% P.sub.2 O.sub.5, 45% Cu.sub.2 O, 5% F/I
B=20% P.sub.2 O.sub.5, 75% Cu.sub.2 O, 5% F/I
C=15% P.sub.2 O.sub.5, 75% Cu.sub.2 O, 10% F/I
D=15% P.sub.2 O.sub.5, 40% Cu.sub.2 O, 45% F/I
E=35% P.sub.2 O.sub.5, 20% Cu.sub.2 O, 45% F/I
F=50% P.sub.2 O.sub.5, 20% Cu.sub.2 O, 30% F/I
Yet again, at least about 15% P.sub.2 O.sub.5 is necessary to provide against glass instability. The glasses were generally somewhat darker than the Cl and Br containing glasses, the colors varying from a light amber to dark brown. Also, the electrical resistivities measured at room temperature were not quite as low as the Cl and Br containing glasses. However, the values were generally less than where only one halide was incorporated into the glass compositions.
Furthermore, substitutions in part of copper for silver and vice versa can be made in each of the above groups of compositions outlined in FIGS. 1-11.
The electrochromic systems which appear to be of great present interest utilize a solid electrolyte and darken by the electrochemical reduction of an ion to the metal at the cathode or produce a transition metal ion that is colored in the reduced state. Those systems based upon the electrochemical reduction of an ion to the corresponding metal are more efficient because of the large optical absorption coefficient of metals.
In order to measure the properties of an electrochromic system, two transparent electrodes were placed on opposite sides of the electrochemical cell. This could be accomplished via R.F. sputtering of Sn-In.sub.2 O.sub.3 or Sb-SnO.sub.2 films. However, a more rapid and convenient system was devised wherein the electrochemical cell was sandwiched between two pieces of glass coated with Sb-SnO.sub.2 films by chemical vapor deposition. This process has been described in such literature as U.S. Pat. Nos. 2,564,707 and 3,331,702. Such a system limits the capability of electrochromic measurements to solid electrolytes having low softening points but that is precisely the type of materials resulting from the present invention.
Optical transmission measurements are customarily made with a photodiode using white light. However, the visible spectrum of each system was studied spectrophotometrically.
The resistivities reported for solid ionic conductors are normally measured with a.c. current to preclude the occurrence of polarization. For an electrochromic system, however, darkening takes place via an electrochemical reaction, i.e., in the region of polarization. A typical current-voltage relationship existing for an electrochemical reaction is set forth in FIG. 12.
In region A of that FIGURE, little current is passed through the cell and no irreversible reactions take place. In region B, electrochemical oxidation and reduction commence. Region C denotes the electrochemical reactions taking place at the maximum rate for the system. Hence, it is in region C where the electrochromic system should be operated for maximum speed. Unfortunately, the current in region C is too great for the Ag.sub.2 O and/or Cu.sub.2 O-halide-P.sub.2 O.sub.5 system, thereby leading to degradation. Consequently, the glasses of the instant invention require operation in region B.
By the very nature of the system, i.e., alternating from the discharged to the charged and back to the discharged state of a battery, the resistivity of the cell is voltage dependent. Therefore, the system is best characterized by the current-voltage representation rather than by a single resistivity value.
The darkening due to the electrochemical reduction of Ag.sup.+ Ag.degree. is fundamentally a very efficient reaction because of the large absorption coefficient of copper and silver. The transmission of an electrochromic system is represented by ##EQU1## where k is the absorption coefficient of the absorbing layer of thickness d at a wavelength .lambda..
Utilizing silver as the example, .lambda.=5600A and k=3.75. In this manner, Equation 1 becomes
1n(T/T.sub.o)=0.0084d (Equation 2)
where d is the thickness of silver in A. If the current efficiency of the system is assumed to be 100%, then the transmission can be calculated in terms of the amount of charge passed through the cell. Based upon that assumption, Equation 1 becomes
1n(T/T.sub.o)=89.6Q (Equation 3)
where Q is delineated in coulombs. To achieve a transmission of 50%, less than 0.008 coulomb/cm.sup.2 is required. This value corresponds to 8 seconds at a current of 1 ma/cm.sup.2. FIG. 13 depicts the transmission-time relationship calculated for the silver system at a constant current of 1 ma/cm.sup.2. Whereas Equations 1-3 were calculated at a wavelength of 5600 A, actual spectra obtained of electrochromic cells of Ag-containing glasses in the darkened state manifest that the transmission is generally uniform across the visible spectrum within about 5%.
To reduce the transmission of the Ag-containing system to 50% requires 8.65 .mu.g of Ag/cm.sup.2. This amount of Ag is equivalent to depleting silver from the glass to a depth of about 235 A. It is conjectured, however, that the Ag comes from a depth of several thousand angstroms within the glass and not just from an interface layer. Even reducing the transmission to 25% demands only about 17 .mu.g of Ag/cm.sup.2. This quantity of silver is less than 2.4% of that present in a 2 micron film of Ag.sub.2 O.multidot.AgCl..multidot.P.sub.2 O.sub.5 glass. The thickness of the typical laminate structure used for measurements is greater than 1000 microns.
An electrochemical cell utilizing a cuprous halophosphate glass demonstrates a markedly different mechanism for electrochromic behavior. FIG. 14 illustrates the darkening in transmission exhibited by a glass consisting, by weight, of 40% P.sub.2 O.sub.5, 20% Cu.sub.2 O, and 40% CuI when a field of one volt is applied thereacross. With this glass the darkening occurs at the anode of the device instead of the cathode, thereby indicating that the electrochemical reaction is the result of an oxidation rather than a reduction mechanism. The color of the darkened film is black, the appearance thereof being similar to that typical of the mixed valency copper oxide black used as optically absorbing coatings.
Although the complete details of the mechanism are not known, the summation of the anode reaction is believed to be:
Cu.sup.+ .fwdarw.Cu.sup.+2 +e.sup.-
This produces a region of glass at the anode where both cupric and cuprous ions exist, in contrast to the original glass where substantially all the copper is present as cuprous ions.
It is well recognized that a strongly allowed optical transition exists between the two valence states of copper leading to the development of copper oxide black, the intensity thereof being proportional to the product of the concentrations of the cupric and cuprous ion species. Consequently, when an electric field of sufficient magnitude is applied to a cuprous halophosphate glass, an optically absorbing film is produced at the anode via a mixed valency mechanism. Measurements on such glasses as that described above, viz., 40% P.sub.2 O.sub.5, 20% Cu.sub.2 O, and 40% CuI, and 30% P.sub.2 O.sub.5, 40% Cu.sub.2 O, and 30% CuBr have demonstrated that the darkening mechanism is electrically efficient, requiring on the order of 0.01-0.05 coulombs/cm.sup.2 for significant darkening. FIG. 14 shows a darkening of about 50% after the application of one volt for about four minutes. That glass will fade back to its original transmission by simply removing the applied field. Thus, the glass will assume its original transmission at room temperature without requiring the application of a reverse field thereto. This fading can be expedited by exposure to slightly elevated temperatures.
It is believed that this same mechanism of mixed valency darkening is responsible for an additional phenomenon observed in the Cu.sub.2 O-P.sub.2 O.sub.5 -CuX glasses encompassed within the compositions defined in FIGS. 1-3, viz., thermochromic behavior. For example, a glass having a composition of 30% P.sub.2 O.sub.5, 40% Cu.sub.2 O, and 30% CuBr will change its optical transmission by 50% when it is subjected to a temperature change from 70.degree. C. to 25.degree. C. The glass is more absorbing, i.e., it is darker in color, at the higher temperature. It will be appreciated that under these conditions the oxidation of cuprous ions is effected thermally and occurs throughout the glass rather than solely at an interface, as is the case with the electrochromic mechanism.

BRIEF DESCRIPTION OF THE DRAWINGS
FIG. 1 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-CuCl-P.sub.2 O.sub.5 system.
FIG. 2 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-CuBr-P.sub.2 O.sub.5 system.
FIG. 3 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-CuI-P.sub.2 O.sub.5 system.
FIG. 4 constitutes a ternary composition diagram illustrating an area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-P.sub.2 O.sub.5 -X field, expressed in mole percent, wherein X is at least one halide selected from the group of Cl, Br, and I.
FIG. 5 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Ag.sub.2 O-AgCl-P.sub.2 O.sub.5 system.
FIG. 6 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Ag.sub.2 O-AgBr-P.sub.2 O.sub.5 system. FIG. 7 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Ag.sub.2 O-AgI-P.sub.2 O.sub.5 system.
FIG. 8 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-P.sub.2 O.sub.5 -F system.
FIG. 9 constitutes a tenary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-P.sub.2 O.sub.5 -F/C1 system.
FIG. 10 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-P.sub.2 O.sub.5 -F/Br system.
FIG. 11 constitutes a ternary composition diagram illustrating the area of stable glasses demonstrating an electrical resistivity at 25.degree. C. of less than 10.sup.8 ohm cm produced in the Cu.sub.2 O-P.sub.2 O.sub.5 -F/I system.
FIG. 12 sets forth a typical current-voltage relationship existing for an electrochemical reaction.
FIG. 13 represents the transmission-time relationship calculated for the silver system at a constant current of 1 ma/cm.sup.2.
FIG. 14 graphically depicts the typical relative transmission: time relationship which a glass having a composition in the P.sub.2 O.sub.5 -Cu.sub.2 O-CuI field exhibits when subjected to a constant applied potential of one volt. The optical transmission is plotted in terms of relative units.

DETAILED DESCRIPTION OF THE INVENTION
Table I recites several compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses coming within the quadrangle ABCD reported in FIG. 1. Table IA records the batch ingredients utilized, expressed in parts by weight.
Melting of the batch ingredients was conducted in covered crucibles, generally VYCOR.RTM. brand 96 percent silica crucibles, marketed by Corning Glass Works, Corning, New York, or glazed porcelain, at temperatures between about 70.degree.-1100.degree. C. for about 10-15 minutes. This melting practice, coupled with the character of the batch ingredients, provided a sufficiently reducing environment to insure that the copper was present in the glass in the cuprous state. The time for melting was kept short to avoid loss through volatilization. The molten batches were very fluid, even when cooled to 300.degree.-400.degree. C. The melts were poured onto a steel plate and a part thereof pressed to a thin plate having a thickness of 1 mm or less.
Table IB reports visual observations made on the glass specimens and electrical resistivity measurements made at room temperature by contacting the glass with probes from a Simpson 260 volt ohm milliammeter marketed by Simpson Electric Company, Elgin, Ill.
TABLE I______________________________________Example No. P.sub.2 O.sub.5 Cu.sub.2 O CuCl______________________________________1 35 32.5 32.52 30 35 353 40 30 304 40 20 405 40 10 506 40 5 557 40 -- 608 35 -- 65______________________________________
TABLE IA______________________________________Example No. NH.sub.4 H.sub.2 PO.sub.4 Cu.sub.2 O CuCl______________________________________1 5.67 3.25 3.252 4.86 3.5 3.53 6.48 3 34 6.48 2 45 6.48 1 56 6.48 0.5 5.67 6.48 -- 68 5.67 -- 6.5______________________________________
TABLE IB______________________________________ Surface ResistanceExample No. Appearance (ohms .times. 10.sup.4)______________________________________1 Clear if quenched, crystal- 300 line if not2 Clear dark amber glass 5003 Black glass 10004 Clear amber glass 4005 " 10006 " 10007 " 20008 " 40______________________________________
Table II lists several compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses coming within the quadrangle ABCD reported in FIG. 2. Table IIA reports the batch ingredients used, expressed in parts by weight.
Melting of the batch ingredients and forming of the molten batches were undertaken in like manner to the exemplary compositions of Table I. Table IIB recites visual observations noted on the glass samples along with electrical resistivity determinations made at room temperature utilizing a Simpson ohm-meter.
TABLE II______________________________________Example No. P.sub.2 O.sub.5 Cu.sub.2 O CuBr______________________________________ 9 40 30 3010 40 20 4011 40 17.5 17.512 50 30 2013 40 40 2014 30 -- 7015 30 30 4016 30 50 2017 40 -- 6018 35 25 4019 45 35 2020 45 30 2521 45 25 3022 45 20 3523 40 15 4524 35 -- 65______________________________________
TABLE IIA______________________________________Example No. NH.sub.4 H.sub.2 PO.sub.4 Cu.sub.2 O CuBr H.sub.3 PO.sub.4 (85%)______________________________________ 9 6.48 3 3 --10 -- 2 4 6.5211 7.29 1.75 3.75 --12 8.10 3 2 --13 6.48 4 2 --14 4.86 -- 215 4.86 3 4 --16 4.86 5 2 --17 6.48 -- 6 --18 5.67 2.5 4 --19 7.29 3.5 2 --20 7.29 3 2.5 --21 7.29 2.5 3 --22 7.29 2 3.5 --23 6.48 1.5 4.5 --24 5.67 -- 6.5 --______________________________________
TABLE IIB______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________ 9 Clear amber glass 3010 Clear light amber glass 7011 Clear amber glass 200012 " --13 " 20014 " 7015 Clear dark amber if quenched, 10 crystalline if not16 Clear dark amber if quenched, 500 crystalline if not17 Clear dark amber glass 20018 Clear light amber glass 1019 Clear amber glass 100020 " 50021 " 40022 " 100023 " 10024 " 70______________________________________
Table III records several compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses encompassed within the quadrangle ABCD outlined in FIG. 3. Table IIIA lists the batch ingredients utilized, expressed in parts by weight.
Melting of the batch ingredients and forming of the molten batches were conducted in similar fashion to the exemplary compositions of Table I. Table IIIB reports visual observations made on the glass samples along with electrical resistivity measurements determined via a Simpson ohm-meter.
TABLE III______________________________________Example No. P.sub.2 O.sub.5 Cu.sub.2 O CuI______________________________________25 40 30 3026 30 -- 7027 40 -- 6028 50 -- 5029 40 5 5530 40 10 5031 40 15 4532 40 20 40______________________________________
TABLE IIIA______________________________________Example No. NH.sub.4 H.sub.2 PO.sub.4 Cu.sub.2 O CuI______________________________________25 6.48 3 326 4.86 -- 727 6.48 -- 628 8.10 -- 529 6.48 0.5 5.530 6.48 1 531 6.48 1.5 4.532 6.48 2 4______________________________________
TABLE IIIB______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________25 Clear amber glass 7026 Light amber clear if quenched, 2 crystalline if not27 Clear amber glass 15028 Dark amber glass --29 Clear amber glass 30030 " 5031 Clear light amber glass 5032 " 25______________________________________
Table IV reports two compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses consisting of more than three components. Table IVA recites the batch constituents employed, expressed in parts by weight. The glasses are stable and exhibit high electrical conductivity.
Melting of the batch ingredients and forming of the molten batches were carried out in accordance with the procedure outlined above for the exemplary compositions of Table I. Table IVB notes visual observations made on the glass specimens along with electrical resistivity measurements made with a Simpson ohm-meter.
TABLE IV______________________________________Example No. P.sub.2 O.sub.5 Cu.sub.2 O CuO CuBr______________________________________33 40 15 5 4034 30 15 15 40______________________________________
TABLE IVA______________________________________Example No. Cu.sub.2 O CuO CuBr NH.sub.4 H.sub.2 PO.sub.4______________________________________33 1.5 0.5 4 6.4834 1.5 1.5 4 4.86______________________________________
TABLE IVB______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________33 Clear amber glass 7034 Clear dark amber if quenched, 5 crystalline if not______________________________________
Chemical analyses were performed upon nine of the above glasses to determine the effect of volatilization. The analyses were reported in terms of Cu.sub.2 O, P.sub.2 O.sub.5, and halide. Table V compares the theoretical compositions as calculated from the batch with the analyzed values. The compositions are adjusted to 100% by weight.
TABLE V__________________________________________________________________________Example Theoretical AnalyzedNo. P.sub.2 O.sub.5 Cu.sub.2 O Cl Br I P.sub.2 O.sub.5 Cu.sub.2 O Cl Br I__________________________________________________________________________ 4 38.8 47.4 13.8 -- -- 42.8 51.7 5.5 -- -- 5 38.5 44.5 17.0 -- -- 49.5 46.1 4.4 -- -- 8 33.3 44.8 21.9 -- -- 41.1 52.8 6.1 -- --14 28.7 41.9 -- 29.4 -- 34.7 42.5 -- 22.8 --17 38.5 36.2 -- 25.3 -- 50.7 38.9 -- 10.4 --18 34.1 48.8 -- 17.1 -- 33.5 47.8 -- 18.7 --26 29.2 25.5 -- -- 45.3 35.3 38.1 -- -- 26.631 39.3 31.3 -- -- 29.4 45.2 37.1 -- -- 17.732 39.4 34.4 -- -- 26.2 40.1 38.3 ---- 21.6__________________________________________________________________________
One important finding resulting from the chemical analysis of the copper-containing glasses is that the analyzed concentration of cuprous copper is essentially equivalent to the total copper concentration. The level of Cu.sup.o was too low to analyze but this circumstance does not rule out the presence of colloidal copper in trace amounts to act as a colorant. The primary loss through volatilization was halide with the chloride loss being greater than that of bromide or iodide.
Table VI recites the analyzed values of the Examples listed in Table V approximated in terms of mole percent.
TABLE VI______________________________________Example No. P.sub.2 O.sub.5 Cu.sub.2 O Cl Br I______________________________________ 4 30.4 44.6 19.1 -- -- 5 44.0 40.6 15.6 -- -- 8 35.0 44.3 20.7 -- --14 29.6 36.0 -- 34.5 --17 47.2 36.0 -- 17.2 --18 29.3 41.7 -- 29.2 --26 34.2 36.7 -- -- 34.531 44.4 36.7 -- -- 19.632 39.2 37.2 -- -- 23.6______________________________________
Table VII records several compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses having electrical resistivities at room temperature less than about 10.sup.8 ohm cm coming within the quadrangle ABCD cited in FIG. 5. The batch materials consisted of AG.sub.2 O, AgC, and H.sub.3 PO.sub.4 (85% by weight).
The melting of the batch constituents and the forming of the resulting melt were undertaken in like manner to the description above with respect to the compositions of Table I. Table VIIA records visual observations noted on the glass specimens and electrical resistivity measurements conducted at room temperature via the probes of a Simpson ohm-meter.
TABLE VII______________________________________Example No. P.sub.2 O.sub.5 Ag.sub.2 O AgCl______________________________________33 34.2 55.8 1034 32.3 52.7 1535 30.4 49.6 2036 26.6 43.4 3037 24.7 40.3 3538 22.8 37.2 4039 25 45 3040 22.5 47.5 3041 20 50 3042 17.5 52.5 3043 15 55 3044 12.5 57.5 3045 25 10 6546 25 53 2247 25 50 2548 15 45 4049 20 40 40______________________________________
TABLE VIIA______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________33 Pale yellow clear if quenched, crystalline if not 200034 Pale yellow clear if quenched, crystalline if not 100035 Pale yellow clear if quenched, crystalline if not 50036 Pale yellow clear glass --37 Clear glass if quenched, crystalline if not38 Clear glass if quenched, crystalline if not 50039 Clear pale yellow if 300 quenched, hazy if not40 Clear pale yellow if quenched, hazy if not 30041 Clear yellow glass 20042 Clear amber glass 15043 Clear yellow if quenched, 70 crystalline if not44 Clear yellow if quenched, crystalline if not 15045 Clear if quenched, hazy -- crystalline if not46 Clear if quenched, hazy 500 if not, yellow47 Clear if quenched, hazy if not, yellow 50048 Clear if quenched, 40 crystaline if not, yellow49 Clear if quenched, crystalline if not, yellow 30______________________________________
Table VIII reports several compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses exhibiting electrical resistivities determined at room temperature of less than about 10.sup.8 ohm cm within the quadrangle ABCD represented in FIG. 6. Thebatch materials consisted of Ag.sub.2 O, AgBr, and 85% H.sub.3 PO.sub.4.
The melting of the batch components and the forming of the resulting molten mass were conducted in accordance with the description outlined above with regard to the compositions of Table I. Table VIIIA lists visual observations noted on the glass samples and electrical resistivity measurements made at room temperature utilizing a Simpson ohm-meter.
TABLE VIII______________________________________Example No. P.sub.2 O.sub.5 Ag.sub.2 O AgBr______________________________________50 23 67 1051 20.4 59.6 2052 17.8 52.2 3053 12.8 37.2 5054 17 53 3055 16 54 3056 15 55 3057 14 56 3058 22 68 1059 12 38 5060 11 39 5061 10 40 5062 14 45 4063 20 40 40______________________________________
TABLE VIIIA______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________50 Clear light yellow glass 50051 Clear yellow glass 20052 " 10053 " 1554 " 7055 Clear yellow is quenched, 50 crystalline if not56 Clear yellow is quenched, 50 hazy if not57 Clear yellow if quenched, 200 crystalline if not58 Clear yellow if quenched, crystalline if not 50059 Clear brown glass 2060 Clear yellow glass 2061 Clear yellow if quenched, 20 crystalline if not62 Clear yellow glass 5063 " 50______________________________________
Table IX lists a number of compositions, expressed in weight percent on the oxide basis as calculated from the batch, of stable glasses having electrical resistivities measured at room temperature of less than about 10.sup.8 ohm cm within the area ABCDE represented in FIG. 7. The batch materials consisted of Ag.sub.2 O, AgI, and 85% H.sub.3 PO.sub.4.
The melting of the batch constituents and the forming of the melts were undertaken in the same way as that described above with respect to the compositions of Table I. Table IXA reports the visual appearance observed on the glass specimens and electrical resistivity determinations conducted at room temperature employing a Simpson ohm-meter.
TABLE IX______________________________________Example No. P.sub.2 O.sub.5 Ag.sub.2 O AgI______________________________________64 20 40 4065 15 25 6066 15 35 5067 18 32 5068 26 44 3069 15 55 3070 24 26 5071 14 45 4072 25 35 4073 15 20 6074 10 30 6075 20 20 6076 20 60 2077 10 50 4078 30 20 5079 10 40 5080 35 25 4081 35 35 3082 45 25 30______________________________________
TABLE IXA______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________64 Clear orange glass 1065 Clear yellow glass 0.0266 Clear yellow if quenched, 0.1 crystalline if not67 Clear light amber glass 268 Clear yellow glass if quenched, 70 hazy if not69 Clear amber glass 3070 Clear yellow glass 0.171 Clear yellow glass if quenched, 0.4 translucent if not72 Clear yellow glass --73 Clear yellow glass if quenched, 0.01 crystalline if not74 Clear orange glass 0.0775 Clear orange glass if quenched, 0.02 crystalline if not76 Clear orange glass if quenched, 150 translucent if not77 Clear yellow glass if quenched, 0.05 crystalline if not78 Clear dark amber if quenched, 10 crystalline if not79 Clear orange glass 580 Clear light yellow if quenched, 10 hazy if not81 Clear yellow glass 20082 Pale yellow glass if quenched, 200 translucent if not______________________________________
Table X records several stable glasses in the Ag.sub.2 O-mixed halide-P.sub.2 O.sub.5 systems where the batches were precipitated in the known manner from aqueous solutions of NaPO.sub.3, AgNO.sub.3, NaCl, NaBr, and NaI, dried, and then melted to a glass. The values reported are expressed in weight percent on the oxide basis as calculated from the batch. Table XA recites the batch materials in terms of parts by weight.
The melting of the batch ingredients and the forming of the molten batches were carried out in the same fashion as described above with respect to the compositions of Table I. Table XB reports the visual appearance observed and the electrical resistivities measured at room temperature with a Simpson ohm-meter.
TABLE X______________________________________Example No. P.sub.2 O.sub.5 Ag.sub.2 O AgCl AgBr AgI______________________________________84 30.4 49.6 8.4 -- 11.684 12 58 12.6 -- 17.485 16 54 12.6 -- 17.486 27.6 42.4 -- 10 2087 28.5 46.5 15 10 --88 28.5 46.5 15 -- 1089 28.5 46.5 15 5 590 26.6 43.4 20 5 5______________________________________
TABLE XA______________________________________Example No. NaPO.sub.3 AgNO.sub.3 NaCl NaBr NaI______________________________________83 21.85 45.60 1.80 -- 3.6084 6.96 45.87 2.02 -- 4.4585 9.28 42.71 2.02 -- 4.4586 4.00 8.57 -- 0.55 1.2887 10.88 13.69 0.62 0.55 --88 10.88 13.51 0.62 -- 0.6489 10.88 13.60 0.62 0.28 0.3290 10.15 13.46 0.82 0.28 0.32______________________________________
TABLE XB______________________________________ ResistivityExample No. Appearance (ohms .times. 10.sup.4)______________________________________83 Clear glass --84 " --85 " --86 Hazy yellow glass 10087 Clear if quenched, 1000 crystalline if not88 Clear if quenched, crystalline if not 100089 Clear if quenched, crystalline if not 100090 Clear if quenched, crystaline if not 500______________________________________
Table XI lists several exemplary compositions, expressed in mole percent on the oxide basis as calculated from the batch, wherein various additives were included in the base P.sub.2 O.sub.5 -Ag.sub.2 O-X system, wherein X is selected from the group of Cl, Br, and I. The glasses were prepared in the following manner. Appropriate amounts of AgNO.sub.3 and H.sub.3 PO.sub.4 were blended together and the mixture heated to about 200.degree. C., at which time the AgNO.sub.3 melted and a clear, colorless, homogeneous solution resulted. Upon further heating, viz., up to 500.degree. C., water and nitrogen oxide fumes were evolved. The resultant melt was heated to about 700.degree. C. and held at that temperature for about one hour to insure removal of water and the nitrogen oxides. A AgPO.sub.3 glass was formed by pouring the melt onto a stainless steel block. The glass was annealed at 160.degree. C.
An appropriate amount of a silver halide was then mixed with a comminuted sample of th AgPO.sub.3 glass and the mixture fused at about 450.degree. C. The additive materials were then dissolved in the molten mass. To prepare glasses containing BaO, ZnO, La.sub.2 O.sub.3, desired amounts of the hydrated forms of the nitrates of those oxides were added slowly to the molten Ag.sub.2 O-P.sub.2 O.sub.5 -X. A vigorous reaction ensued with oxides of nitrogen as well as water being emitted. The addition of such constituents as B.sub.2 O.sub.3, Al.sub.2 O.sub.3, and LiF can be made by simply incorporating them in that form into the molten Ag.sub.2 O-P.sub.2 O.sub.5 -X. The resultant Ag.sub.2 O-P.sub.2 O.sub.5 -X additive oxide glasses are generally yellow in color.
TABLE XI______________________________________Example No. Ag.sub.2 O P.sub.2 O.sub.5 AgCl Additive Oxide______________________________________92 43.1 43.1 11.0 2.8 La.sub.2 O.sub.393 43.2 43.2 9.6 4.0 Y.sub.2 O.sub.394 40 40 10 10 ZnO95 40.7 40.7 14.3 7.3 BaO96 40.4 40.4 10 9.2 ZnO______________________________________
Table XII records electrical resistivity determinations measured at room temperature utilizing a Simpson ohm-meter. Finally, transition temperature determinations via differential thermal analysis, and refractive index measurements are recited.
TABLE XII______________________________________ ResistivityExample No. (ohms) T.sub.g n.sub.D______________________________________92 9.3 .times. 10.sup.5 -- --93 1.3 .times. 10.sup.8 -- --94 1.4 .times. 10.sup.8 -- --95 -- 178.degree. C. 1.72596 -- 170.degree. C. 1.720______________________________________
Table XIII sets forth a group of compositions, expressed in weight percent on the oxide basis as calulated from the batch, of stable glasses falling within area ABCDEF of FIG. 8 along with a visual description of the glass prepared. Melting of the batch ingredients and forming of the molten batches were carried out in a manner similar to that described above with respect to the working examples of Table I. That is, the batches were compounded, placed into 96 percent silica crucibles, and melted for about 10 minutes at 900.degree. C. The melts were poured onto a steel slab and quenched under the pressure of a graphite block into a thin plate of about 1 mm thickness. The batch materials employed were NH.sub.4 H.sub.2 PO.sub.4, CuF.sub.2, and NH.sub.4 F.HF.
Table XIIIA reports the compositions as calculated in terms of mole percent and also includes electrical resistivity measurements (ohm cm) conducted at room temperature (.about.25.degree. C.) at 120 Hz, 1 KHz, and 10 KHz utilizing painted silver electrodes.
TABLE XIII______________________________________Example No. Cu.sub.2 O P.sub.2 O.sub.5 F Visual Appearance______________________________________97 12 77 11 Dark glass98 16 37 47 Dark glass99 5 90 5 Dark, sticky glass100 7 83 10 Dark, sticky glass101 6 77 17 Dark, sticky glass102 18 76 6 Dark glass103 53 39 8 Dark, partly devi- trified glass______________________________________
TABLE XIIIA______________________________________ExampleNo. Cu.sub.2 O P.sub.2 O.sub.5 F 120Hz 1KHz 10KHz______________________________________97 7 45 48 7 .times. 10.sup.7 6.8 .times. 10.sup.7 5.8 .times. 10.sup.798 4 9 87 -- -- 2.6 .times. 10.sup.799 4 68 28 6.6 .times. 10.sup.5 6.3 .times. 10.sup.5 6.1 .times. 10.sup.5100 4 50 46 1.9 .times. 10.sup.6 1.9 .times. 10.sup.6 6.5 .times. 10.sup.5101 3 37 60 1.3 .times. 10.sup.7 1.3 .times. 10.sup.7 1.1 .times. 10.sup.7102 13 56 31 -- -- 4.9 .times. 10.sup.7103 34 25 41 -- -- 5.8 .times. 10.sup.7______________________________________
Table XIV lists a number of compositions, reported in terms of weight percent on the oxide basis as calculated from the batch, of relatively stable glasses encompassed within the area ABCDEF of FIG. 9 accompanied with a visual description of each glass prepared. The melting of the batch ingredients and the forming of the resultant melt were undertaken in like manner to that described immediately above with regard to Table XIII. The batch ingredients included NH.sub.4 H.sub.2 PO.sub.4, CuF, CuCl, and NH.sub.4 F.HF. The quantities of the batch components were adjusted such that equal molar amounts of fluoride and chloride were present in the batch.
Table XIVA recites the compositions as calculated in terms of mole percent and lists electrical resistivity determinations (reported in ohm cm) measured at room temperature (.about.25.degree. C.) at 120 Hz, 1 KHz, and 10 KHz utilizing painted silver electrodes.
TABLE XIV______________________________________Example No. Cu.sub.2 O P.sub.2 O.sub.5 F Cl Visual Appearance______________________________________104 55 34 3.8 7.2 Light amber glass105 62 19 6.5 12.5 Dark, partly devitrified glass106 41 25 11.5 21.5 Yellow glass107 74 18 2.8 5.2 Dark surface devitrified glass108 51 34 5.2 9.8 Amber, partly devitrified glass109 56 19 8.7 16.3 Dark glass______________________________________
TABLE XIVA______________________________________ExampleNo. Cu.sub.2 O P.sub.2 O.sub.5 F Cl 120Hz 1KHz 10KHz______________________________________104 37 23 20 20 3.7 .times. 10.sup.5 1.8 .times. 10.sup.5 4.4 .times. 10.sup.4105 36 8 28 28 2.0 .times. 10.sup.3 1.9 .times. 10.sup.3 1.1 .times. 10.sup.3106 17 11 36 36 3.4 .times. 10.sup.3 3.4 .times. 10.sup.3 2.7 .times. 10.sup.3107 54 14 16 16 8.6 .times. 10.sup.4 8.1 .times. 10.sup.4 7.7 .times.10.sup.4108 31 21 24 24 3.9 .times. 10.sup.4 3.2 .times. 10.sup.4 1.1 .times. 10.sup.4109 27 9 32 32 4.4 .times. 10.sup.4 4 .times. 10.sup.4 4 .times. 10.sup.4______________________________________
Table XV records exemplary glasses, stated in terms of weight percent on the oxide basis as calculated from the batch, of relatively stable glasses having compositions within the area ABCDEF of FIG. 10 and includes a visual description of each glass prepared. The melting of the batch materials and the forming of the molten batch into thin sheet were conducted in accordance with the method described with reference to Table XIII. NH.sub.4 H.sub.2 PO.sub.4, CuF.sub.2, CuBr, and NH.sub.4 F.HF comprised bath ingredients therefor. The quantities of chloride and fluoride were carefully controlled such that equal molar amounts of each were present in the batch.
Table XVA lists the glasses as calculated in terms of mole percent and also reports electrical resistivity data (expressed as ohm cm) measured at room temperature (.about.25.degree. C.) at 120Hz, 1KHz, and 10KHz utilizing painted silver electrodes.
TABLE XV______________________________________ExampleNo. Cu.sub.2 O P.sub.2 O.sub.5 F Br Visual Appearance______________________________________110 46 34 3.8 16.2 Yellow, sticky glass111 47 19 6.3 27.7 Amber glass112 24 46 5.4 24.6 Amber glass113 36 28 6.9 20.1 Yellow-green glass114 17 58 4.8 20.2 Dark glass115 74 18 1.5 6.5 Dark glass116 51 34 3 12 Yellow, amber sticky glass117 56 19 5 20 Red, amber glass118 31 48 4 17 Amber glass______________________________________
TABLE XVA______________________________________ExampleNo. Cu.sub.2 O P.sub.2 O.sub.5 F Br 120Hz 1KHz 10KHz______________________________________110 33 25 21 21 1.9 .times. 10.sup.4 1.5 .times. 10.sup.4 9.5 .times. 10.sup.3111 29 11 30 30 1.3 .times. 10.sup.3 2.6 .times. 10.sup.3 3.5 .times. 10.sup.3112 16 32 26 26 3.1 .times. 10.sup.7 2.7 .times. 10.sup.7 1.6 .times. 10.sup.7113 21 17 31 31 4.9 .times. 10.sup.3 2.5 .times. 10.sup.3 1.2 .times. 10.sup.3114 12 40 24 24 -- -- 1.4 .times. 10.sup.7115 64 16 10 10 4.1 .times. 10.sup.5 4.1 .times. 10.sup.5 4.0 .times. 10.sup.5116 40 27 17 17 6 .times. 10.sup.4 3.6 .times. 10.sup.4 2.7 .times. 10.sup.4117 40 14 23 23 2.2 .times. 10.sup.3 2.0 .times. 10.sup.3 1.7 .times. 10.sup.3118 17 37 23 23 1.0 .times. 10.sup.7 9.8 .times. 10.sup.6 7.7 .times. 10.sup.6______________________________________
Table XVI lists a number of working examples, recorded in terms of weight percent on the oxide basis as calculated from the batch, of relatively stable glasses having compositions included within the area ABCDEF of FIG. 11 along with a visual description of each glass body. The melting of the batch materials and the pressing of the melt into thin sheet were carried out in a manner similar to that described above with respect to Table XIII. The batch ingredients for the glasses included NH.sub.4 H.sub.2 PO.sub.4, CuF.sub.2, CuI, and NH.sub.4 F.HF. The contents of fluoride and iodide were so controlled as to incorporate equal molar amounts of each into the batch.
Table XVIA recites the glasses as calculated in terms of mole percent and also tabulates electrical resistivity determinations (reported in ohm cm) measured at room temperature (.about.25.degree. C.) at 120Hz, 1KHz, and 10KHz employing painted silver electrodes.
TABLE XVI______________________________________ExampleNo. Cu.sub.2 O P.sub.2 O.sub.5 F I Visual Appearance______________________________________119 74 18 1 7 Dark glass120 51 34 2 13 Red-brown, partly devitrified glass121 56 19 3.2 21.8 Dark amber glass122 31 47 2.7 19.3 Light amber glass123 26 32 5.4 36.6 Amber, surface devitrified glass124 13 76 1.5 9.5 Dark brown glass______________________________________
TABLE XVIA______________________________________ExampleNo. Cu.sub.2 O P.sub.2 O.sub.5 F I 120Hz 1KHz 10KHz______________________________________119 69 17 7 7 9.8 .times. 10.sup.5 9.2 .times. 10.sup.5 8.6 .times. 10.sup.5120 45 29 13 13 3.0 .times. 10.sup.5 1.7 .times. 10.sup.5 9.0 .times. 10.sup.4121 45 15 20 20 2.4 .times. 10.sup.4 2.2 .times. 10.sup.4 2.0 .times. 10.sup.4122 26 40 17 17 2.6 .times. 10.sup.5 2.1 .times. 10.sup.5 1.7 .times. 10.sup.5123 18 24 29 29 2.2 .times. 10.sup.6 1.3 .times. 10.sup.6 1 .times. 10.sup.6124 12 68 10 10 -- -- 1.4 .times. 10.sup.7______________________________________
Table XVII reports several other glasses, expressed in weight percent on the oxide basis as calculated from the batch, having compositions within the base P.sub.2 O.sub.5 -Ag.sub.2 O-X system, wherein X is selected from the group of Cl, Br, I, and equal molar amounts of Cl and I. The glasses were prepared in like manner to that described above with respect to the examples listed in Table XI except that no additive oxides were incorporated therein. Table XVII also records d.c. electrical resistivity measurements conducted at room temperature (.about.25.degree. C.) utilizing the three probe method.
TABLE XVII______________________________________ ResistivityExample (ohm cm .times.No. Ag.sub.2 O P.sub.2 O.sub.5 AgCl AgBr AgI 10.sup.4______________________________________125 59.7 36.5 3.8 -- -- 173126 57.2 35.1 7.7 -- -- 73127 54.8 33.5 11.7 -- -- 49128 52.1 31.9 16.0 -- -- 26129 46.5 28.5 25.0 -- -- 8.6130 41.1 25.2 33.7 -- -- 3.2131 58.9 26.1 -- 5.0 -- 152132 52.7 32.3 -- 15.0 -- 41133 37.1 22.8 -- 40.1 -- 2.7134 57.9 35.8 -- -- 6.3 81135 50.9 31.1 -- -- 18.0 27136 23.1 15.2 -- 25.0 2.7137 41.2 25.3 12.7 -- 20.8 2.2138 44.2 27.2 10.8 -- 17.8 8.6139 51.6 31.6 6.4 10.4 29.8______________________________________

Number	Name	Date
3853568	Chvatal	Dec 1974
3875321	Gliemeroth	Apr 1975
4038203	Takahashi	Jul 1977
4079022	Ferrarini et al.	Mar 1978

Cuprous copper and/or silver halophosphate glasses

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