19.9.18
26.5.17
29.9.10
How LED works ?
Light-Emitting Diodes: Diverse Applications
Light-emitting diodes (LEDs) (Figure 1) are found in many ordinary objects that we use on a daily basis. Common examples of LEDs include the digital display on your alarm clock, the tiny light that indicates whether your iron, computer, or electric razor is on, and the scanners on grocery-store checkout counters. Although they are now commonplace, LEDs that give off visible light were actually invented relatively recently. In 1962, Nick Holonyak, Jr., while working for General Electric, discovered that the chemical composition of earlier diodes could be changed to make them give off visible light for use in digital displays and indicators. LEDs operate by a completely different mechanism from other sources of light, such as light bulbs and the sun. Furthermore, LEDs release only one particular color of light, and they produce very little heat. In contrast, the "white" light produced by a light bulb or the sun is really a blend of many different colors, and these sources typically produce a large amount of heat. Hence, LEDs are much more efficient for producing small quantities of light of a particular color than other light sources. Because of this efficiency, scientists and engineers are hard at work to develop designs that will allow LEDs to be used for many new applications. For example, the new traffic lights are made out of arrays of LEDs It has been estimated that replacing all the incandescent traffic lights in the United States with LED traffic signals would save almost 2.5 billion kilowatt hours per year (roughly equivalent to $200 million, or 5 billion pounds of CO2 (from burning fossil fuels to make electricity) released into the atmosphere)! | Figure 1This diagram shows the principal components of a typical LED, such as the one used in the Chem 151 experiment to test conductivity. The plastic lens encapsulating the LED takes up most of the space in this device, while the actual LED chip is only about 0.25 mm2. |
Bonding in Elemental Solids
Metals are electrically conducting because their valence electrons (the outermost electrons of an atom) "swim" in an electron "sea". This picture is useful for imagining how metals have sufficiently mobile charged particles to conduct electricity, but it does not fully explain the difference in conductivity among the various elements. To explain the difference in the properties of metals, semimetals, and nonmetals, and hence to understand how LEDs work, we need to understand the bonding of solids in more detail. Throughout this course (and science, in general), different models (theories) are used to describe a phenomenon. It is important to remember that all models will fail at some point, but all have their own usefulness and advantages in describing a phenomenon of interest.
You have learned that electronegativity is the ability of an atom in a molecule to attract electrons to itself (away from its neighbor), and the electronegativity of elements increases from the left side of the periodic table (metallic elements) to the right side (nonmetallic elements). Because atoms with low electronegativity (i.e., metals) do not hold their valence electrons tightly, their valence-electron orbitals are diffuse and may extend to large distances away from the nucleus. Highly electronegative atoms (i.e., nonmetals) hold their electrons tightly, so their valence-electron orbitals are less diffuse and smaller. (To help visualize how high electronegative makes orbitals less diffuse and smaller, think of a dog on a leash: if you pull harder on the leash, you bring the dog closer to you so that its movement is restricted to a smaller area.) When atoms interact together, their valence orbitals "overlap" to form bonds between the atoms. Electronegativity differences are important in determining the types of bonds that form between atoms of different elements. Electronegativity also plays an important role in determining the properties of bonds between atoms of the same element in a solid (for which the difference in electronegativity is zero). How can electronegativity help us to understand the behavior of metals, semimetals, and nonmetals? Metals: Weak Covalent Bonding (Metallic Bonding)
Let us first consider the example of sodium. Sodium has one valence electron, which is in the 3s orbital. When two Na atoms bond to form a gaseous Na2 molecule, the two valence electrons (one from each Na atom) are found primarily between the two Na nuclei. However, in a crystalline sodium solid, the Na atoms adopt a "closest packed" configuration, in which the atoms are packed together in a regular pattern with equal spacing between atoms (Figure 2a). Typically, in a closest packed configuration, an atom has many “nearest neighbors” (up to 12). Since the valence electrons of the metal atoms are not tightly constrained to a small space, one sodium atom can interact weakly with all of its nearest neighbors. Even though the individual interactions between atoms are weak, there are many interactions between an atom and its many nearest neighbors, and the ag gregate effect is a well-bonded metallic solid . (To illustrate this point, think of how a woven cloth is held together. Although the individual threads may be quite weak, when many threads are woven together, they form a strong cloth.)
a.  | b.  |
Figure 21a. This is a representation of the three-dimensional structure of a crystalline metal, in which each atom has 12 nearest neighbors (closest-packed configuration). Weak covalent bonds are formed between metal atoms.b. This is a representation of the three-dimensional structure of a crystalline nonmetal, in which each atom has only 4 nearest neighbors. Strong covalent bonds are formed between nonmetal atoms. | |
The low-electronegative metal atoms "give up" their valence electrons, allowing them to be found throughout the "mixed" orbitals of the valence band. Hence, the band of orbitals is filled according to the number of valence electrons provided by all of the Na atoms in the solid. Because electrons are shared among atoms in these "mixed" orbitals, they form covalent bonds between the atoms in the solid. Each atom shares electrons with all its many neighbors in all directions; the bonds formed are not confined between two atoms. Another term frequently used to describe this type of bonding is "metallic bonding." Solids with this type of bonding exhibit metallic properties and are therefore categorized as metals. As we shall see later in the tutorial, elements with metallic bonding are very good conductors of electricity because of the nondirectionality of the orbitals (i.e., electrons can easily move in any direction). Metallic elements are not used in LEDs, although they are important components of the circuits used to power LEDs.
 |
| Figure 3 When metal atoms interact together to form a solid, their atomic orbitals mix to form a continuous band of orbitals. In the representation of 1 Na atom (left-hand side of diagram), the blue dot represents an electron in the 3s orbital; in the representation of many Na atoms (center of diagram), the blue dots again represent electrons in the "mixed" orbitals that are formed when many atoms interact. This "mixing" of orbitals is better represented by a "band" of orbitals (right-hand side of diagram), in which the blue area represents orbitals that are filled with electrons. |
Now consider the example of carbon (C), a nonmetal. Its electronegativity is high relative to that of sodium. Therefore, the valence orbitals of a C atom are not diffuse and are smaller than those of Na. When C atoms are packed together to make a solid, the valence orbitals overlap within a small volume, thus causing the electrons in these orbitals to be constrained to a small space. Some of the C atoms are drawn closer together, pulling them further away from others. This severely distorts the closest-packed structure (Figure 2a) and causes it to become a nonmetallic crystalline solid structure (Figure 2b). In order to form the nonmetallic solid structure, the highly electronegative atoms interact with only a few (usually four or less) nearest neighbors, and each valence orbital is oriented in the direction of the atom with whose valence orbital it overlaps. Hence, the interactions between those atoms that are drawn close together are strong. As in metal solids, the valence atomic orbitals lose their individual identity in the aggregate of C atoms, and these orbitals "mix" to form a band of orbitals that are close in energy.
Electrons are shared between atoms in these "mixed" orbitals, but the bonds are directional. Therefore, the bonds formed in nonmetal elemental solids are stronger and are called strong covalent bonds. In strong covalent bonds, a large energy gap arises between the orbitals that are formed, as you will see later in Chem 111. When many strong covalent bonds are present, as in the nonmetallic solid, two bands of "mixed orbitals" form, separated by an energy gap called the band gap (Figure 4). The lower-energy band consists of filled orbitals (i.e., orbitals containing electrons) and is known as the valence band; the higher-energy band consists of unfilled orbitals and is known as the conduction band. As you go across the periodic table, the band gap increases (as the electronegativity increases). Semimetals (Figure 5), which lie between metals and nonmetals on the periodic table, have an energy gap between the valence and conduction bands (band gap) similar to nonmetals (not a continuous band like metals), but the band gap for semimetals is smaller than for nonmetals.
 |  |
| Figure 4 When nonmetal atoms interact to form a solid, their atomic orbitals mix to form two bands of orbitals that are separated by a large band gap. | Figure 5 When semimetal atoms interact to form a solid, their atomic orbitals mix to form two bands of orbitals that are separated by a small band gap. |
 |
Figure 6This is a representation of the periodic table showing the trends in the bonding properties, molecular interactions, and conductivity of solids from the left-hand side to the right-hand side. |
Bands and the Conductivity Properties of the Elements
Recall from the introduction to the experiment that substances conduct electricity if they contain mobile charged particles (i.e., ions or electrons). In a solid, electrons can become mobile if the electrons can be promoted to unfilled orbitals in the conduction band of the solid. How can we account for the electrical conductivity of metals? Think again about an individual Na atom, containing only one valence electron in the 3s orbital (recall Figure 3). This atom has a half-filled 3s orbital (because the 3s orbital can hold up to 2 electrons) and three unfilled 3p orbitals, as you will learn later in Chem 111. All of these are valence orbitals and combine with those from other atoms in the solid to form the band of "mixed" orbitals described above. However, the number of electrons contained in the valence band is much smaller than the number the band is capable of containing. The reason the band is filled much less than its capacity is that each atom contributes only one electron to the band, but contributes four orbitals to the band; hence, the band is capable of holding up to eight electrons per atom. The filled and unfilled portions of the band are continuous (recall Figure 3); no band gap is present like in carbon and other nonmetal solids. Therefore, electrons can easily (i.e. with very little energy input) be promoted from filled orbitals in the band to unfilled orbitals in the band, and hence move throughout the metal solid. Therefore, metals conduct electricitybecause the partially-filled band of orbitals allows electrons to move easily throughout the sample.What about nonmetals? We know that nonmetallic solids form two distinct bands. The lower-energy band, known as the valence band, contains all of the valence electrons (the band is filled with electrons), while the higher-energy band, the conduction band, contains no electrons (recall Figure 4). Electrons in the filled valence band cannot move to other orbitals within the band because all of the orbitals are already filled. No motion of electrons occurs in the conduction band because it is empty. Now, recall that these bands are separated by a large band gap. Therefore, a large amount of input energy is required to promote an electron from the filled lower-energy (valence) band to the unfilled higher-energy (conduction) band. Thus, without the high-energy input to promote an electron from the lower-energy band to the higher-energy band, there are no mobile charge carriers, and the nonmetallic solid cannot conduct electricity.
As you should observe in lab, semimetalssuch as silicon (Si) have intermediate properties between those of metals and nonmetals. The band gap in semimetals is small enough (recall Figure 5) that an electron can be promoted from the filled lower-energy band to the unfilled higher-energy band with a moderate input of energy (such as the thermal energy that dissipates in the solid when electrical current is passed through it). Then, the lower-energy (valence) band is no longer completely filled and the higher-energy (conduction) band is no longer completely empty; i.e., both bands are partially filled (Figure 7). In the valence band, electrons can move between orbitals (and thus throughout the solid) once some of the orbitals have become vacant. Promotion of electrons to the conduction band allows the electrons to move easily between the band's many empty orbitals. Hence, semimetals can conduct electricity with a moderate input of energy.
 |
| Figure 7 In a semiconductor, the band gap is small enough that electrons can be moved from the orbitals in the valence band to the orbitals in the conduction band. This leaves both bands partially filled, so the material can conduct electricity. |
Doping to Enhance Conductivity of Semiconductors
LEDs are made of semiconductors, but the conductivity of the semiconductors in LEDs has been specially enhanced to allow for the unique properties of LEDs. Adding small, controlled amounts of "impurities" that have roughly the same atomic size, but more or fewer valence electrons than the semimetal can increase the conductivity of semiconductors like Si. This process is known as doping. An impurity with fewer valence electrons (such as Al; see the periodic table) takes up space in the solid structure, but it contributes fewer electrons to the valence band, thus generating an electron deficit (Figure 8). This type of dopant creates a space (or "hole") in the lower-energy (valence) band, making room for electrons to travel. Hence, the electrons in the valence band can move from one orbital to another within this band with only a small input of energy (smaller than required for the semiconductor without the doping). In this way, the electrons can move throughout the solid. Alternately, an impurity with more valence electrons (such as P; see the periodic table) contributes extra electrons to the band (Figure 9). Since the valence band is already filled by the semimetal, the extra electrons must go into the higher-energy (conduction) band. These electrons now occupy a partially-filled band (the conduction band) and can move easily between the orbitals of this band. This allows the electrons to move easily throughout the solid. Semiconductors whose conductivity has been enhanced with valence-electron-deficient dopants are known as p-type semiconductors (p for "positive" because it is deficient in negatively-charged electrons). Semiconductors whose conductivity has been enhanced with valence-electron-enriched dopants are known as n-type semiconductors (n for "negative" because it is enriched with negatively-charged electrons). Now we know that LEDs are doped semiconductors and hence conduct electricity with a small input of energy (i.e., LEDs are very efficient). However, we have not yet answered the questions, how does an LED give off light, and why does an LED give off only one specific color of light? |  |
| Figure 8 A schematic diagram showing the solid crystal-lattice structure and bands for silicon doped with aluminum, a p-type semiconductor. | Figure 9 A schematic diagram showing the solid crystal-lattice structure and bands for silicon doped with phosphorus, an n-type semiconductor. |
How Do LEDs Emit Light?
In order to convert electrical current into light, an LED must have a p-type semiconductor in contact with an n-type semiconductor. This combination of the two types of semiconductors is known as a p-n junction, or a diode. When a p-n junction is placed in a circuit with an external power source (e.g., a 9 V battery), electrons from the power source flow to the diode and change the arrangement of electrons in the diode (Figure 10). How does this lead to the emission of light in the LEDs? Recall that the p-type semiconductor (Figure 8) has extra space for electrons in its valence band and no electrons in its conduction band. On the other hand, the n-type semiconductor (Figure 9) has a full valence band (no space) and extra electrons in its conduction band. If the circuit is constructed such that electrons flow into the n-type side of the p-n junction from the power source (Figure 10), the electrons will occupy the conduction band, since there is no space in the valence band of an n-type semiconductor. As electrons continue to come into the conduction band, they will be pushed to the p-type side of the p-n junction, which has more space to hold electrons (you can think of the "positive" side attracting the negatively-charged electrons). The electrons go into the empty conduction band of the p-type side, since they already occupy the higher-energy band in the n-type side. However, once the electrons are in the higher-energy band of the p-type side, they will fall to the lower-energy band if there is space available for the electrons to occupy in the valence band. Electrons falling from the higher-energy band of orbitals (conduction band) to the lower-energy band of orbitals (valence band) in the p-type semiconductor result in the atoms going from a higher-energy state to a lower-energy state (i.e., becoming more stable). As the electrons cross the band gap, energy related in magnitude to the size of the band gap is released in the form of light. |  |
Figure 10The diagram on the left depicts a circuit composed of an LED, a resistor, and a battery. The resistor in the circuit is necessary to limit the current so that the LED does not “burn out” by receiving too much current from the battery.The diagram on the right shows the path of electrons moving through a circuit containing a p-n junction. Electrons flow from the negative pole of the battery to the n-type semiconductor, where they occupy the conduction band. The electrons then move into the conduction band of the p-type semiconductor and fall into the empty orbitals of the valence band, which releases energy in the form of light. The electrons then move through the wire back to the positive pole of the battery, and they re-circulate. ( Note: This picture has been simplified to follow the discussion presented here. A more complete picture would show a potential energy barrier to electrons moving from the n-type to the p-type semiconductor must be overcome (using the voltage from the battery; known as "biasing"). For more information, see Elllis et. al in the References. Click on the pink buttons to view a QuickTime movie showing the flow of electrons through the circuit and the light emitted by the LED. Click the link to download QuickTime and click on the pink button to view a QuickTime movie showing the inflation of dual airbags when a head-on collision occurs.  | |
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| Figure 11 The color of light emitted by an LED depends on the size of the band gap in the doped semiconductors. For instance, LEDs that emit red light have a smaller band gap than LEDs that emit yellow light. |
Summary and a Look to the Future
In this tutorial, you learned that LEDs contain p-type and n-type semiconductors that are side-by-side. Semiconductors conduct electricity because of small band gaps between the valence and conduction bands, which allow electrons to move throughout the material with a moderate input of energy. The LED emits light when the electrons fall from the conduction band to the valence band. The color of the light emitted depends on the size of the band gap. Today's LEDs use inorganic material in the semiconductor. In 1990, the next generation of light-emitting material, the light-emitting polymer (LEP), was discovered. LEPs are organic (carbon-based) semiconducting materials. LEPs are based on the same chemical concepts taught in this tutorial. LEP's can be used in more diverse applications than LEDs because polymers are flexible and can be shaped to different forms, for example flat-panel color displays are made of LEP materials. At this time, technology and applications based on LEPs are still in developmental stage.2.9.10
IMPORTANT QUESTIONS FOR MID – 1
1. (a) Explain about the forward bias and reverse bias of PN junction.
(b) Distinguish between Avalanche and Zener breakdown mechanisms.
2. (a) Give the relation between voltage and current of PN junction and explain each term in detail.
(b) problem
3. (a) Derive the expression for transition capacitance of a diode.
(b) Derive the expression for Diffusion capacitance of a diode.
4. (a) What is a rectifier ? draw the circuit diagram of a HWR and explain its operation.
(b) Derive the expression for the ripple factor for a PI section filter when used with a FWR.
5. (a) Problem
(b) Derive the expression for ripple factor, efficiency, average value, rms value, form factor and peak factor for a HWR.
6. (a) Define ICBO and ICEO. Derive the following relations.
(i) 1-α = 1 / (1+ β) (ii) ICEO = (1+ β ) ICBO
(b) Explain the current components of a NPN transistor.
7. (a) Explain about CE transistor input and output characteristics interms of cutoff, active and saturation regions.
(b) Compare CB, CC and CE configurations.
8. (a) Explain the need of biasing a transistor.
(b) Explain the concept of dc operating point with the help of dc load line with neat sketches.
22.6.10
XILINX TUTORIALS
Tutorials
Current Software Tutorials
Previous Software Tutorials
- ISE Design Suite 11 Tutorials
- ISE 10 Software Tutorials
- PlanAhead 10 Tutorial
- ISE 9 Software Tutorials
- ISE 8 Software Tutorials
- ISE 7 Software Tutorials
- ISE 6 Software Tutorials
- ISE 5 Software Tutorials
- EDK BFM Simulation Tutorial
- MicroBlaze™ Tutorial (Requires ISE 4.2i)
- ISE/Foundation™ 4.1i Tutorials
18.6.10
Keil RealView Microcontroller Development Kit & RealView Real-Time Library v.4.1
The software development RealView Microcontroller Development Kit (MDK ARM) combines the company Keil compiler C / C + + ARM RealView IDE and Keil uVision.
Year: 2010
Version: 4.10
Developer: Keil ?, an ARM ® Company
Platform: Windows
Compatibility with Vista: Yes (set to Win7 x64 Ultimate build 7600 - no problems)
Medician: Yes
This product gives developers a multifunctional development environment optimized to work with a broad line of microcontrollers based on the core ARM. MDK ARM provides device support, based on the ARM7, ARM9 and Cortex M3 manufacturers such as Analog Devices, Atmel, Freescale, Luminary, OKI, NXP, Samsung, Sharp, STMicroelectronics and TI. Using the MDK ARM reduces the design cycle and significantly reduce time-to-market. MDK ARM - the ideal tool for standardized industrial projects with a developed system debugging and support for real-time.
Library RL ARM - RealView ® RealTime Library
? RTX Real Time Kernel - a full-featured operating system real-time RTX Keil, which manages the CPU time semaphores (resource allocation), events (for task synchronization), and mailboxes (for communication between tasks). RTX is easily configured using the configuration file.
? TCP / IP Networking Suite - a communication module based on the stack TCP / IP, specially adapted for embedded applications. It includes TCP and UDP-sockets, PPP and SLIP interfaces, DNS, Telnet, TFTP, SMTP, built-in Web server and CGI with password protection. The stack works with Ethernet, and serial (modem). Configured examples are intended to work on a few standard demonstration boards.
? Flash File System - a system that allows you to save files in Flash, ROM or RAM. This is useful in decisions that require a large amount of memory for data storage or systems with internet interfaces, HTTP or FTP.
? USB Device Interface - drivers for USB, which allows you to connect standard devices such as HID or Mass Storage.
? CAN Interface - in RTX Keil library includes CAN, which provide a powerful and simple interface for different controllers CAN.
Library RL-ARM is designed for typical problems that confront the developer, and allows you to:
? manage multiple tasks on one CPU;
? control the timing of the task;
? communicate and configure the interaction between different programs in the system;
? Provide access to the Internet via Ethernet or serial connection (modem);
? Implement a built-in web server which includes CGI-scripts;
? Implement a E-mail via Simple Mail Transfer Protocol (SMTP).
Changes in RV MDK ARM 4.10 compared with 4.03a
[ARM Processor Support]
MDK now includes the RealView Compilation Tools version 4.0.0.728 with Cortex-M4 and Cortex-R4 support.
[ARM Processor Support]
Added: simulation for Cortex-M4 Processor core including DSP and FPU extensions.
[New Device Support]
NXP LPC1759, and LPC1769 devices.
[Device Simulation]
Simulation support added for NXP LPC11xx, LPC13xx, and LPC17xx series.
[Checksum Utility]
Added: ELFDWT utility creates boot checksum for NXP LPC11xx, LPC13xx, and LPC17xx device series. Usage is:
C: \ Keil \ ARM \ BIN \ ELFDWT elf_file.AXF
The checksum creation can be automated in µVision by entering in the dialog Project - Options for Target - User, Run User Programs After Build / Rebuild, Run # 1:
$ K \ ARM \ BIN \ ELFDWT.EXE # L
When this command is enabled µVision calls the ELFDWT utility and the required checksum gets inserted into the AXF linker output file. Note that this process is not needed when programs are downloaded using ULINK. ULINK automatically adds the checksum during Flash programming.
[Target Debugging]
Updated: support for ST-Link USB-JTAG debugger. The STLinkIIIUSBDriver.dll debug driver has been replaced by STLinkUSBDriver.dll in folder .. \ ARM \ STLink \. The flash file loader stm32f10xLoader.bin for STM32F10x devices has been added in folder .. \ ARM \ STLink \
[Target Debugging]
Updated: Luminary lmidk-agdi.dll to version 37.0.0.0.
[Target Debugging]
Updated: Segger's J-Link driver for ARM devices to version 4.11.9.0 that solves problems with Micrium µC / evaluation STM32FF-107 board.
[Target Debugging]
Added: support for Cortex-M0 devices when Segger's J-Link and J-Trace debugger is used.
[Board Support]
Added: USBHID and USBMem examples for Atmel's ATSAM3S device in folder .. \ ARM \ Boards \ Atmel \ ATSAM3S-EK \.
[Board Support]
Added: Blinky, BlinkyCAN, LCD_BLinky, RTX_Blinky, USBHID, and USBMem examples for NXP's LPC2929 device in folder .. \ ARM \ Boards \ Keil \ MCB2929 \.
The changes in the RL-ARM 4.10 compared with 4.05
[RTX - Problems Solved]
Corrected: potential wrong return value of os_mbx_send () function in Cortex-M library.
[TCPnet - Enhancements]
Added: support for Cortex-M1 devices. Free TCP_CM1.lib and debug TCPD_CM1.lib library have been added.
Added: a SNMP Agent implementation and SNMP_demo example for various evaluation boards. SNMP version 1 with trap messages is supported.
Added: a Gratuitous ARP implementation. If this feature is enabled, the embedded host broadcasts an ARP notification at startup or if local IP address changed.
Added: a new file type php-script, file extension php [text / html] to the Web server.
[TCPnet - Problems Solved]
Added: MSS option (maximum segment size) to SYN packet for outgoing TCP connections. Because this option was missing, PC used reduced segment size of 536 bytes in communication.
Corrected: auto disconnect problem in FTP Server during large file transfer.
Corrected: a problem in WEB Server. It failed to load pages from SPI or parallel flash.
Corrected: a Null Modem driver problem. It failed to connect in client mode, if connect request was issued delayed from application reset.
Corrected: a problem in PPP module which sometimes fails to connect.
[FlashFS - Enhancements]
Added: Support for SDHC Cards.
[CAN - Problems Solved]
Corrected: function CAN_set now returns error code.
[FCARM - Enhancements]
Added: a simple compression for Cascading Style Sheet files.
Improved: compression ratio for Java Script files.
[FCARM - Problems Solved]
Corrected: a problem in Java and CGI script compression.
Install crack:
In Keil:
1. File-> License Management, copy the contents of the CID
2. Run the crack, choose what generic license Target-> ARM, Prof.Devkit / RealView MDK
In the CID insert that copied in Keil
Click Generate
3. Copy the licensed paste in Keil in the field of New License ID Code (LIC), click Add LIC
4. Repeat pp.2-3 for all the required products
5. Glad result
Download:
http://hotfile.com/dl/41343113/364d079/MDK.RL.ARM.HLP_4.10.part1.rar.html
http://hotfile.com/dl/41343157/6eeb038/MDK.RL.ARM.HLP_4.10.part2.rar.html
http://hotfile.com/dl/41343163/9afe055/MDK.RL.ARM.HLP_4.10.part3.rar.html
http://hotfile.com/dl/41343157/6eeb038/MDK.RL.ARM.HLP_4.10.part2.rar.html
http://hotfile.com/dl/41343163/9afe055/MDK.RL.ARM.HLP_4.10.part3.rar.html
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