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As a student, you can use the most powerful software to edit and create images for your class. Here is a list of Photoshop tutorials and guides:
Best Photoshop tutorials: Learn how to edit and create images with Photoshop tutorials.
2. Google GIMP
GIMP (GNU Image Manipulation Program) is an open-source graphics editor that’s free to download and use. It’s considered the best alternative to Photoshop and has many similar features.
You can use GIMP to edit, filter, create and share images. GIMP is available for Windows, Mac, Android, iOS, Linux and Unix operating systems. It also supports many layers and formats that allow you to create complex images and edits.
GIMP is very similar to Photoshop. Some people prefer GIMP because it’s free, open-source software, while others use the software because of its interface. You can learn how to edit photos with GIMP step by step.
3. Pixlr
Pixlr is a web-based graphics editor that is very similar to Photoshop. You can use Pixlr to edit, crop, adjust, create or apply filters. It has some limited features for image editing.
Pixlr is a free online graphics editor that allows you to use filters and effects to create new images. It’s very simple to use and works on all desktop and mobile devices. You can even create Pixelart creations.
You can download and install the software on your phone. Pixlr has mobile apps for Android, iPhone and iPad. You can also create, edit and apply filters to your images.
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4. Paint.NET
Paint.NET is another web-based image editing software. It has a simple, intuitive and friendly user interface. You can use Paint.NET to edit, duplicate, crop, restore, transform and retouch images. It’s ideal for image editing.
Paint.NET is a desktop program that offers free online image editing and filters. The program has some unique features like a canvas and brushes. You can create or apply various filters to images using a layer or pen tool.
Paint.NET is a very advanced tool that comes with thousands of image filters. You can create a variety of effects and filters using this tool.
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This research investigated the extent of contamination of the top soil of a residential area of Antalya, Turkey by mercury (Hg) and the corresponding ecological risk (ER) through a pilot study in 2012. The total Hg (THg) concentration in the topsoil, including the top 2 cm, was 60.6 ± 12.8 mg kg(-1). The average ER value was estimated to be 1737.8 kg Hg ha(-1). Partitioning of Hg was analyzed using the sequential extraction method with Chelex 100 resin. The statistical correlation between the total soil Hg and the soil solution was 0.79. A significant correlation between soil THg and the total concentration of Hg in the house dust (r = 0.85, p Q:
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What is the correct way to include default style sheet in ASP.NET MVC 4 RC?
Here’s what I do now:
A:
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Understanding the position of a bond and the calculation of bond energy in $\ce{CH2CH2O}$
I’m having a hard time understanding how the Wikipedia article on $\ce{CH2CH2O}$ works and I need help.
How does the position of the a and b bond work here, i.e. why is the c bond more electronegative than the a and b bonds?
Also, why is the energy of the c bond -15 kcal/mol and a and b bonds -78 kcal/mol?
A:
The effect of electronegativity differences is the same as in any carbon-carbon bond. The carbon in CH2CCH2O is more electronegative than carbon in CCO by the factor of 4. That’s what the Wikipedia article indicates.
The difference in energy is due to changes of electron density around the C=C bond. The bond energy of the ethylene C=C bond can be described as a sum of two terms
$$\Delta E = \Delta E_{(sp^3 \to sp^2)} + \Delta E_{(sp^2 \to sp^3)}$$
The first term, a $\sigma$-bond change, is due to the electron spillover from carbon atom. The second term is a $\sigma$-bond change due to the change of electron distribution in the bonding system.
The C=C bond in $\ce{C3H4}$ has a bond energy of 182 kcal/mol, C=C bond in $\ce{C3H3}$ have 138 kcal/mol and C=C bond in $\ce{C2H4}$ have a bond energy of 193 kcal/mol. The energy difference between C=C bond in ethylene $\ce{C3H4}$ and ethylene $\ce{C2H4}$ is 36 kcal/mol.
The bond energy of double C=C bond is similar to that of a single C=C bond, but without the spillover electron.
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