In one sentence, describe what the following article is about: If you have guests over to the house, you don't want them crawling over furniture to get around. There should be enough space between each piece for them to walk through. And your furniture should not block any entrances into or exits out of the room. This might sometimes mean that you have furniture set away from the wall. That's okay! You should put two to four pieces together in each room so they face each other. This way, if you have guests over, they feel like you want them to talk to you! For example, arrange a couch parallel to a wall, but set away from it, so people can walk behind if necessary. Then set up two arm chairs next to each other, across from the couch. If you're not sure if the space looks too cluttered, take out one piece of furniture. You want the space to look cozy and inviting, but not stuffed. Try not to use just one texture or fabric in each room. Using one fabric can make the room all blend together and feel sterile. Using one material for your tables, one for your chairs, and another for throw pillows will help make the room feel cozy.  For example, in your living room, you could have a wooden coffee table paired with linen-covered arm chairs and plush, silky throw pillows. You can also break up your kitchen by using different textures for your accessories, storage, and countertop. Try metal shelving, glass storage containers, and a granite or quartz countertop. There’s nothing cozier than a comfy piece of furniture that you can sink into. When you’re choosing furniture, choose pieces that are plush or upholstered. If your rooms are small, upholstered is best because it won’t look too big for the room.  You can reupholster existing furniture. You'll need to remove the old fabric and batting (the fluffy stuff that makes a chair comfy to sit on). Cut out the furniture patterns, then reattach the new fabric by stapling it on the underside of the furniture. If you really love the pieces of furniture you have, but don't want to reupholster them, you can take them to a specialist and have it done. If you have a small home, you don’t want to cram your rooms with giant pieces of furniture. It will make your house look small and cramped, as opposed to cozy and inviting.  Your furniture doesn’t have to match to have similar scale. Use pieces that have a similar height and weight. This strategy is great for redecorating your home on a budget - look for things in resale shops or discount stores that are similar scale, and they don't have to match! A lot of scale is just using your eye to see if the furniture in the room looks proportionate. Start by placing your largest piece and work from there – don’t add other pieces that look too large or too small in comparison. Furniture that looks well-loved (distressed) can help make your home feel more lived in and cozy. You can achieve the distressed look by buying furniture that already looks this way, or using sandpaper to scrape off some of the paint on new furniture.
Summary: Arrange your furniture so it's easy to move around the room. Gather your furniture to facilitate conversation. Use less furniture when in doubt. Mix up your textures and fabrics. Use plush or upholstered furniture. Scale your furniture to fit the room you’re in. Use distressed furniture.

Problem: Article: There are many tables that have information on the average bond energies for a specific bond. These tables can be found online or in a chemistry book. It is important to note that these bond energies are always for molecules in a gaseous state.  For our example, you need to find the bond energy for an H-H bond, a Br-Br bond, and an H-Br bond. H-H = 436 kJ/mol; Br-Br = 193 kJ/mol; H-Br = 366 kJ/mol.  To calculate bond energy for molecules in a liquid state, you need to also look up the enthalpy change of vaporization for the liquid molecule. This is the amount of energy needed to convert the liquid into a gas. This number is added to the total bond energy. For example: If you were given liquid water, you would need to add the enthalpy change of vaporization of water (+41 kJ) to the equation. In some equations, you may have the same bond broken multiple times. For example, if 4 atoms of hydrogen are in the molecule, then the bond energy of hydrogen must be counted 4 times, or multiplied by 4.  In our example, there is only 1 bond of each molecule, so the bond energies are simply multiplied by 1. H-H = 436 x 1 = 436 kJ/mol Br-Br = 193 x 1 = 193 kJ/mol Once you have multiplied the bond energies by the number of the individual bonds, you need to then sum all of the bonds on the reactant side. For our example, the sum of the bonds broken is H-H + Br-Br = 436 + 193 = 629 kJ/mol. Just as you did for the bonds broken on the reactant side, you will multiply the number of bonds formed by its respective bond energy. If you have 4 hydrogen bonds formed, you would need to multiply that bond energy by 4. For our example we have 2 H-Br bonds formed, so the bond energy of H-Br (366 kJ/mol) will be multiplied by 2: 366 x 2 = 732 kJ/mol. Again, like you did with the bonds broken, you will add up all of the bonds formed on the product side. Sometimes you will only have 1 product formed and can skip this step. In our example, there is only 1 product formed, so the energy of the bonds formed is simply the energy of the 2 H-Br bonds or 732 kJ/mol. Once you have summed all of the bond energies for both sides, simply subtract the formed bonds from the broken bonds. Remember the equation: ΔH = ∑H(bonds broken) - ∑H(bonds formed). Plug in the calculated values and subtract. For our example: ΔH = ∑H(bonds broken) - ∑H(bonds formed) = 629 kJ/mol - 732 kJ/mol = -103 kJ/mol. The final step to calculating bond energy is to determine whether the reaction releases energy or consumes energy. An endothermic (one that consumes energy) will have a final bond energy that is positive, while an exothermic reaction (one that releases energy) will have a negative bond energy. In our example, the final bond energy is negative, therefore, the reaction is exothermic.
Summary:
Look up the bond energies of the bonds in question. Multiply the bond energies by the number of bonds broken. Add up all of the bond energies of the broken bonds. Multiply the bond energies by the number of bonds formed. Add up all of the formed bond energies. Subtract the formed bonds from the broken bonds. Determine whether the entire reaction was endothermic or exothermic.