{"appState":{"pageLoadApiCallsStatus":true},"authorState":{"author":{"headers":{"timestamp":"2024-11-22T08:49:31+00:00"},"authorId":35209,"data":{"name":"Christopher R. Hren","slug":"christopher-r-hren","description":" Christopher R. Hren has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. John T. Moore, EdD, has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. Peter J. Mikulecky, PhD, teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. ","photo":{"src":null,"width":0,"height":0}}},"authorLoadedStatus":"success"},"listState":{"list":{"count":1,"total":1,"items":[{"headers":{"creationTime":"2022-11-07T16:40:29+00:00","modifiedTime":"2022-11-08T14:15:33+00:00","timestamp":"2022-11-08T15:01:02+00:00"},"data":{"breadcrumbs":[{"name":"Academics & The Arts","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33662"},"slug":"academics-the-arts","categoryId":33662},{"name":"Science","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33756"},"slug":"science","categoryId":33756},{"name":"Chemistry","_links":{"self":"https://dummies-api.dummies.com/v2/categories/33762"},"slug":"chemistry","categoryId":33762}],"title":"Chemistry All-in-One For Dummies Cheat Sheet","strippedTitle":"chemistry all-in-one for dummies cheat sheet","slug":"chemistry-all-in-one-for-dummies-cheat-sheet","canonicalUrl":"","seo":{"metaDescription":"Chemistry covers all kinds of stuff. Sometimes you might not be sure where to start when you are first given a set of problems and told to go forth and succeed.","noIndex":0,"noFollow":0},"content":"Chemistry covers all kinds of stuff. Sometimes you might not be sure where to start when you are first given a set of problems and told to go forth and succeed. Sometimes it’s converting metric units, writing ionic formulas, naming covalent compounds, balancing reactions, or dealing with extensive and intensive properties.\r\n\r\nThis Cheat Sheet is designed to give you some help on a few of the trickier things you might encounter so that when you are done looking it over you can go forth and succeed!","description":"Chemistry covers all kinds of stuff. Sometimes you might not be sure where to start when you are first given a set of problems and told to go forth and succeed. Sometimes it’s converting metric units, writing ionic formulas, naming covalent compounds, balancing reactions, or dealing with extensive and intensive properties.\r\n\r\nThis Cheat Sheet is designed to give you some help on a few of the trickier things you might encounter so that when you are done looking it over you can go forth and succeed!","blurb":"","authors":[{"authorId":35209,"name":"Christopher R. Hren","slug":"christopher-r-hren","description":" <p><b>Christopher R. Hren </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b>John T. Moore, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b>Peter J. Mikulecky, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. 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Hren</b> </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b>John T. Moore, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b>Peter J. Mikulecky, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. <p><b>Christopher R. Hren </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b><b data-author-id=\"9159\">John T. Moore</b>, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b>Peter J. Mikulecky, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. <p><b>Christopher R. Hren </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b>John T. Moore, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b><b data-author-id=\"9161\">Peter J. Mikulecky</b>, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer.</p>","authors":[{"authorId":35209,"name":"Christopher R. Hren","slug":"christopher-r-hren","description":" <p><b>Christopher R. Hren </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b>John T. Moore, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b>Peter J. Mikulecky, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/35209"}},{"authorId":9159,"name":"John T. Moore","slug":"john-t-moore","description":" <p><b>Christopher R. Hren </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b>John T. Moore, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b>Peter J. Mikulecky, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/9159"}},{"authorId":9161,"name":"Peter J. Mikulecky","slug":"peter-j-mikulecky","description":" <p><b>Christopher R. Hren </b>has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. <p><b>John T. Moore, EdD,</b> has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. <p><b>Peter J. Mikulecky, PhD,</b> teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer. ","hasArticle":false,"_links":{"self":"https://dummies-api.dummies.com/v2/authors/9161"}}],"_links":{"self":"https://dummies-api.dummies.com/v2/books/"}},"collections":[],"articleAds":{"footerAd":"<div class=\"du-ad-region row\" id=\"article_page_adhesion_ad\"><div class=\"du-ad-unit col-md-12\" data-slot-id=\"article_page_adhesion_ad\" data-refreshed=\"false\" \r\n data-target = \"[{"key":"cat","values":["academics-the-arts","science","chemistry"]},{"key":"isbn","values":["9781119908319"]}]\" id=\"du-slot-636a6f2eb4b65\"></div></div>","rightAd":"<div class=\"du-ad-region row\" id=\"article_page_right_ad\"><div class=\"du-ad-unit col-md-12\" data-slot-id=\"article_page_right_ad\" data-refreshed=\"false\" \r\n data-target = \"[{"key":"cat","values":["academics-the-arts","science","chemistry"]},{"key":"isbn","values":["9781119908319"]}]\" id=\"du-slot-636a6f2eb5a50\"></div></div>"},"articleType":{"articleType":"Cheat Sheet","articleList":[{"articleId":0,"title":"","slug":null,"categoryList":[],"_links":{"self":"https://dummies-api.dummies.com/v2/articles/"}}],"content":[{"title":"Converting metric units","thumb":null,"image":null,"content":"<p>Because chemists must be able to communicate their measurements to other chemists all over the world, they need to speak the same measurement language. This language is the SI system of measurement, related to the metric system.</p>\n<p>Below is a chart of the most commonly used metric prefixes, their abbreviations, and how they relate to a metric base unit. Remember, the metric system is based on 10s, so each time you are converting from one unit to another you can just count the number of jumps between prefixes to have an idea of what your conversion should be.</p>\n<table>\n<tbody>\n<tr>\n<td><strong>Prefix</strong></td>\n<td><strong>Abbreviation</strong></td>\n<td><strong>Meaning</strong></td>\n</tr>\n<tr>\n<td>kilo-</td>\n<td>k</td>\n<td>1,000 or 10<sup>3</sup></td>\n</tr>\n<tr>\n<td>hecto-</td>\n<td>h</td>\n<td>100 or 10<sup>2</sup></td>\n</tr>\n<tr>\n<td>deka- or deca-</td>\n<td>da</td>\n<td>10 or 10<sup>1</sup></td>\n</tr>\n<tr>\n<td>deci-</td>\n<td>d</td>\n<td>0.1 or 10<sup>–1</sup></td>\n</tr>\n<tr>\n<td>centi-</td>\n<td>c</td>\n<td>0.01 or 10<sup>–2</sup></td>\n</tr>\n<tr>\n<td>milli-</td>\n<td>m</td>\n<td>0.001 or 10<sup>–3</sup></td>\n</tr>\n</tbody>\n</table>\n<p>For example, if you want to convert 500 ml to liters, all you have to do is multiply that by the conversion shown in the chart for milli as shown below. Be sure to cancel out your units!</p>\n<p><img loading=\"lazy\" class=\"alignnone size-full wp-image-295577\" src=\"https://www.dummies.com/wp-content/uploads/chem-formula.png\" alt=\"equation to convert 500 ml to liters\" width=\"220\" height=\"78\" /></p>\n<p><strong>Writing the formulas of ionic compounds</strong></p>\n<p>A quick way to determine the formula of an ionic compound (remember ionic compounds are metals bonded to nonmetals) is to use the <em>crisscross rule</em>. The crisscross rule uses the ionic charges of the ions to predict the formula of the ionic compound. It doesn’t work every time but it is a very useful method for writing many ionic formulas. Check it out as shown here:</p>\n<p><img loading=\"lazy\" class=\"alignnone size-full wp-image-295578\" src=\"https://www.dummies.com/wp-content/uploads/9781119908319-fgcs01.jpg\" alt=\"Diagram of crisscross rule in chemistry\" width=\"250\" height=\"108\" /></p>\n<p>Take the numerical value of the metal ion’s superscript (forget about the charge symbol) and move it to the bottom right-hand side of the nonmetal’s symbol — as a subscript. Then take the numerical value of the nonmetal’s superscript and make it the subscript of the metal. (Note that if the numerical value is 1, it’s just understood and not shown.)</p>\n<p>So, in this example, you make magnesium’s 2 a subscript of bromine and make bromine’s 1 a subscript of magnesium (but because it’s 1, you don’t show it), and you get the formula MgBr<sub>2</sub>.</p>\n"},{"title":"Naming covalent compounds","thumb":null,"image":null,"content":"<p>Covalent compounds are nonmetals to nonmetals. These differ from ionic compounds in that their names clearly specify how many of each type of atom participate in the compound. The table below shows you the prefixes used when naming covalent compounds.</p>\n<table>\n<tbody>\n<tr>\n<td><strong>Number of Atoms</strong></td>\n<td width=\"312\"><strong>Prefix</strong></td>\n</tr>\n<tr>\n<td>1</td>\n<td>mono-</td>\n</tr>\n<tr>\n<td>2</td>\n<td>di-</td>\n</tr>\n<tr>\n<td>3</td>\n<td>tri-</td>\n</tr>\n<tr>\n<td>4</td>\n<td>tetra-</td>\n</tr>\n<tr>\n<td>5</td>\n<td>penta-</td>\n</tr>\n<tr>\n<td>6</td>\n<td>hexa-</td>\n</tr>\n<tr>\n<td>7</td>\n<td>hepta-</td>\n</tr>\n<tr>\n<td>8</td>\n<td>octa-</td>\n</tr>\n<tr>\n<td>9</td>\n<td>nona-</td>\n</tr>\n<tr>\n<td>10</td>\n<td>deca-</td>\n</tr>\n</tbody>\n</table>\n<p>You can attach the prefixes in the table above to any of the elements in a covalent compound, as exemplified by SO<sub>3</sub> (sulfur trioxide) and N<sub>2</sub>O (dinitrogen monoxide). The second element in each compound receives the –<em>ide</em> suffix, as in ionic compounds (which we discuss earlier in this chapter).</p>\n<p>In the case of covalent compounds, where cations or anions aren’t involved, the more electronegative element (in other words, the element that’s closer to the upper right-hand corner of the periodic table) tends to be named second.</p>\n<p>Finally, if the compound only has 1 atom for the first element you can leave off mono as the prefix. For example, you don’t call CO<sub>2</sub> monocarbon dioxide. Instead, you just call it carbon dioxide.</p>\n"},{"title":"Balancing reactions","thumb":null,"image":null,"content":"<p>Balancing chemical reactions can be a real challenge for some people. Sometimes just getting started is a real challenge. The example below shows how to balance a combustion reaction. There is a good chance that if you are here reading this you might be stuck on a combustion reaction, so make sure to read on. Even if not, this example is going to give you a solid idea of how to go about balancing any reaction you encounter.</p>\n<ol>\n<li>\n<p><strong>Start with the unbalanced reaction written out</strong>.</p>\n<p>C<sub>4</sub>H<sub>10</sub>(<em>g</em>) + O<sub>2</sub>(<em>g</em>) ®CO<sub>2</sub>(<em>g</em>) + H<sub>2</sub>O(<em>g</em>)</p>\n</li>\n<li>\n<p><strong>Balance the carbon atoms first</strong>.</p>\n<p>Remember: You want to wait until the end to balance hydrogen and oxygen atoms. You have 4 carbon atoms on the left and 1 carbon atom on the right, so put a coefficient of 4 in front of the carbon dioxide:</p>\n<p>C<sub>4</sub>H<sub>10</sub>(<em>g</em>) + O<sub>2</sub>(<em>g</em>) ® 4 CO<sub>2</sub>(<em>g</em>) + H<sub>2</sub>O(<em>g</em>)</p>\n</li>\n<li>\n<p><strong><strong>When all non-hydrogen and non-oxygen atoms are balanced, balance the hydrogen atoms.</strong></p>\n<p>Carbon is the only other atom in this example, so you can move on to hydrogen now. You have 10 hydrogen atoms on the left and 2 hydrogen atoms on the right, so use a coefficient of 5 in front of the water on the right:C<sub>4</sub>H<sub>10</sub>(<em>g</em>) + O<sub>2</sub>(<em>g</em>) ®4 CO<sub>2</sub>(<em>g</em>) + <strong>5</strong> H<sub>2</sub>O(<em>g</em>)</p>\n</li>\n<li>\n<p><strong>Balance the oxygen atoms</strong>.</p>\n<p>You have 2 oxygen atoms on the left and a total of 13 oxygen atoms on the right [(4 × 2) + (5 × 1) = 13]. What can you multiply 2 with in order for it to equal 13? How about 6.5?</p>\n<p>C<sub>4</sub>H<sub>10</sub>(<em>g</em>) + <strong>6.5</strong> O<sub>2</sub>(<em>g</em>) ®4 CO<sub>2</sub>(<em>g</em>) + 5 H<sub>2</sub>O(<em>g</em>)</p>\n</li>\n<li>\n<p><strong>Multiply all coefficients in the equation to get the lowest <em>whole-number</em> ratio of coefficients</strong>.</p>\n<p>For this example, multiply the entire equation by 2 (just the coefficients, please) in order to generate whole numbers:</p>\n<p>[C<sub>4</sub>H<sub>10</sub>(<em>g</em>) + 6.5 O<sub>2</sub>(<em>g</em>®4 CO<sub>2</sub>(<em>g</em>) + 5 H<sub>2</sub>O(<em>g</em>)] ×2</p>\n<p>Multiplying every coefficient by 2 (don’t touch the subscripts!) gives you</p>\n<p>2 C<sub>4</sub>H<sub>10</sub>(<em>g</em>) + 13 O<sub>2</sub>(<em>g</em>) ®8 CO<sub>2</sub>(<em>g</em>) + 10 H<sub>2</sub>O(<em>g</em>)</p>\n</li>\n<li>\n<p><strong>Check the atom count on both sides of the equation to ensure that the equation is balanced and the coefficients are in the lowest whole-number ratio</strong>.</p>\n</li>\n</ol>\n<p>This is a pretty complex example and hopefully it helps you out. Sometimes, though, all you might need to do is add a single coefficient of 2 or 3 in front of one compound. Just stay organized and keep things simple and you’ll be balancing reactions in no time!</p>\n"},{"title":"Extensive and intensive properties","thumb":null,"image":null,"content":"<p>There are all kinds of ways you can classify matter. One is to look at the different physical properties that that matter has. There are two major types of physical properties:</p>\n<ul>\n<li><strong>Extensive Properties:</strong> properties that depend on the amount of matter present\n<p>Examples: mass, volume, length, width or anything else that depends entirely on how much of the substance you have</li>\n<li><strong>Intensive Properties:</strong> properties that don’t depend on the amount of matter present\n<p>Examples: density, malleability, ductileness, hardness, melting point</li>\n</ul>\n<p>A helpful way to remember this is that intensive properties rely on what is “in”-side the matter, with the “in” signifying <em>intensive</em> and how it doesn’t matter how much of the matter is present.</p>\n<p>Extensive properties rely on the “ext”-erior of the matter, with the “ext” signifying <em>extensive</em> and the fact that now, the amount of what you see on the exterior of the matter does impact the property.</p>\n<p>Some physical properties are <em>extensive properties,</em> properties that depend on the amount of matter present. Mass and volume are extensive properties. A large chunk of gold has a larger mass and volume than a smaller chunk.</p>\n<p><em>Intensive properties,</em> however, don’t depend on the amount of matter present. Hardness is an intensive property. A large chunk of gold, for example, has the same hardness as a small chunk of gold. The mass and volume of these two chunks are different (extensive properties), but the hardness is the same.</p>\n<p>Intensive properties are especially useful to chemists because they can use intensive properties to identify a substance.</p>\n"}],"videoInfo":{"videoId":null,"name":null,"accountId":null,"playerId":null,"thumbnailUrl":null,"description":null,"uploadDate":null}},"sponsorship":{"sponsorshipPage":false,"backgroundImage":{"src":null,"width":0,"height":0},"brandingLine":"","brandingLink":"","brandingLogo":{"src":null,"width":0,"height":0},"sponsorAd":"","sponsorEbookTitle":"","sponsorEbookLink":"","sponsorEbookImage":{"src":null,"width":0,"height":0}},"primaryLearningPath":"Advance","lifeExpectancy":"Five 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Christopher R. Hren

Christopher R. Hren

Christopher R. Hren has taught high school chemistry, honors chemistry, and AP Chemistry for more than 15 years. John T. Moore, EdD, has taught chemistry at Stephen F. Austin State University in Nacogdoches, Texas, for more than 40 years. Peter J. Mikulecky, PhD, teaches science and math at Fusion Learning Center and Fusion Academy, and is a technical writer.

Articles From Christopher R. Hren

Chemistry Chemistry All-in-One For Dummies Cheat Sheet

Cheat Sheet / Updated 11-08-2022

Chemistry covers all kinds of stuff. Sometimes you might not be sure where to start when you are first given a set of problems and told to go forth and succeed. Sometimes it’s converting metric units, writing ionic formulas, naming covalent compounds, balancing reactions, or dealing with extensive and intensive properties. This Cheat Sheet is designed to give you some help on a few of the trickier things you might encounter so that when you are done looking it over you can go forth and succeed!

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