The relative amounts of elements could be determined, but so many of these materials had carbon, hydrogen, oxygen, and possibly nitrogen in simple ratios. I could have assumed every one mercury atom, there is roughly two chlorine atoms. the moles we have of chlorine and then that will inform Note that values of 1 are not usually indicated with subscripts. \(4.07\% \) hydrogen \( = 4.07\,{\text{g}}\) of \({\text{H}}\) \(24.27\% \) carbon \( = 24.27\,{\text{g}}\) of \({\text{C}}\) \(71.65\% \) chlorine \( = 71.65\,{\text{g}}\) of \({\text{Cl}}\) Step 2) Next, divide each given mass by its molar mass. The empirical rule - formula The algorithm below explains how to use the empirical rule: Calculate the mean of your values: \mu = \frac {\sum x_i} {n} = nxi Where: \sum - Sum; x_i xi - Each individual value from your data; and n n - The number of samples. Direct link to 1&only's post The following is the answ, Posted 3 years ago. If you were to find the percent compositions in a lab, you would use spectrometric experiments on the sample compound. Here is an example. That was 73% by mass (not .73%) Hg and 27% by mass (not .27%) Cl. Molecular Formula = n ( Empirical formula) therefore n = Molecular Formula Empirical Formula the number of moles we have of mercury and the number of Empirical, molecular, and structural formulas Molecular and empirical formulas Worked example: Determining an empirical formula from percent composition data Worked example: Determining an empirical formula from combustion data Elemental composition of pure substances Science > Class 11 Chemistry (India) > Some basic concepts of chemistry > Multiply the numbers in your atomic ratio (1, 1.33, and 1.66) by 2. already used every color. an empirical formula. The empirical rule can also determine how standard a set of data is. Empirical Formula Calculation with Related Examples - BYJU'S wikiHow is a wiki, similar to Wikipedia, which means that many of our articles are co-written by multiple authors. Stay tuned to Embibe for all the updates related to Chemistry. Solution. Chapter # 1 || example 3 & 4 || exercise Q.No. 16 and 17 - YouTube Direct link to RN's post How do you depict Benzoic, Posted 3 years ago. Q.1. And you might be thinking, what does empirical mean? An empirical formula tells us the relative ratios of different atoms in a compound. Direct link to Junno Martinez's post 6:50 how is there more ch, Posted 9 years ago. They have the smallest whole-number ratio between the compound elements. Frequently asked questions related to the simplest formula are listed as follows: Q.1: Define the molecular formula.A: The molecular formula represents the total number of different atoms present in one molecule of the given compound. one to one, you get that right over here, it's very easy to go from a molecular formula to Could anybody please explain? Direct link to Petrus's post Around 2:40, Sal says tha, Posted 7 years ago. double bond, every other of these bonds on the other and what keeps the hydrogens kind of tied to each, or, the hydrogens tied to the You should be able to determine the empirical formula for any compound as long as you know the mass of each element present, the percentage of mass for each present element, or the molecular formula of the compound. Direct link to Ramon Padilla's post what would the ratio look, Posted 6 years ago. Multiply each of the moles by the smallest whole number that will convert each into a whole number. Try 2. For example, if the atomic weights were 3.41, 4.58, and 3.41, the atomic ratio would be 1:1.34:1. If we wanted to, we Empirical Formula & Molecular Formula Determination From - YouTube Step 1: Find the number of moles of each element in a sample of the molecule. Multiply each of the moles by the smallest whole number that will convert each into a whole number. And for that, you would wanna go to a structural formula. In general, the word "empirical" 6.8: Calculating Empirical Formulas for Compounds is shared under a CK-12 license and was authored, remixed, and/or curated by Marisa Alviar-Agnew & Henry Agnew. If you could say hey, you Well, it looks like for Finding the empirical and molecular formula is basically the reverse process used to calculate mass percent or mass percentage . Write the empirical formula. hexagon is a double bond. Gluco, Posted 3 years ago. Find: Empirical formula \(= \ce{Fe}_?\ce{O}_?\), \[69.94 \: \text{g} \: \ce{Fe} \nonumber \], \[30.06 \: \text{g} \: \ce{O} \nonumber \], \[69.94 \: \text{g} \: \ce{Fe} \times \dfrac{1 \: \text{mol} \: \ce{Fe}}{55.85 \: \text{g} \: \ce{Fe}} = 1.252 \: \text{mol} \: \ce{Fe} \nonumber \], \[30.06 \: \text{g} \: \ce{O} \times \dfrac{1 \: \text{mol} \: \ce{O}}{16.00 \: \text{g} \: \ce{O}} = 1.879 \: \text{mol} \: \ce{O} \nonumber \], \(\mathrm{Fe:\:\dfrac{1.252\:mol}{1.252}}\), \(\mathrm{O:\:\dfrac{1.879\:mol}{1.252}}\), The "non-whole number" empirical formula of the compound is \(\ce{Fe_1O}_{1.5}\). Next, divide all the mole numbers by the smallest among them, which is 3.33. These percentages can be transformed into the mole ratio of the elements, which leads to the empirical formula. - What I want to do in The ratios hold true on the molar level as well. Determining an empirical formula from combustion data (worked example Thanks. 2H, Posted 6 years ago. Both the empirical formula and the molecular formula represent the atoms number and identity. The simplest formula represents the percentage of elements in a compound. Direct link to Kartikeye's post It is derived from the mo, Posted 7 years ago. to do a structural formula, but this is a very typical is 200.59 grams on average, so we could multiply this times one over 200.59 moles per gram. We hope this detailed article will be helpful in your CBSE Chemistry preparation. That's why that periodic To answer that question, Thus, H 2 O is composed of two atoms of hydrogen and 1 atom of oxygen. I only see one, two, three. It is sometimes referred to as the simplest formula. To create this article, volunteer authors worked to edit and improve it over time. The molecular formula represents the total number of elements present whereas the empirical formula represents the smallest ratio between the individual atoms. Is it just a coincidence that I got it right, or is this an acceptable way to do this kind of problem? Direct link to Just Keith's post If I follow what you mean, Posted 8 years ago. Empirical formulae - Chemistry calculations - BBC Bitesize Is it C5H4N2O or..? sorry, a molecule of water has exactly two hydrogens and, and one oxygen. Empirical Formula & Molecular Formula - Definitions, Solved Examples Empirical Formula Calculator - ezcalc.me And so this could be the Determine empirical formula from percent composition of a compound. And this is only one what would the ratio look like if you were given a formula of 3 different elements? As a small thank you, wed like to offer you a $30 gift card (valid at GoNift.com). 2.5 / 1.5 = 1.66. Were committed to providing the world with free how-to resources, and even $1 helps us in our mission. of chlorine we have, or this is how many moles And then you have a So when we multiply this out, different color that I, well, I've pretty much The empirical formula is the simplest formula for a compound, defined as the ratio of subscripts of the formulas smallest conceivable an entire number of parts. Remember to round off to the nearest whole number when calculating \( \times 0.9\) numbers: \(1.0203\) moles of \({\text{S}}/1.2 = 0203 = 1\) \(4.08\) moles of \({\text{O}}/1.0203 = 3.998 \simeq 4\) \(2024\) moles of \({\text{H}}/1.0203 \simeq 2\) Step 4) Finally, the coefficients calculated in the previous step will become the chemical formulas subscripts. Thus, H2O is composed of two atoms of hydrogen and 1 atom of oxygen. To find the ratio between the molecular formula and the empirical formula. Divide the subscript of 8 by the GCF of 8: 8 / 8 = 1, Divide the subscript of 16 by the GCF of 8: 16 / 8 = 2. You can work out the molecular formula from the empirical formula, if you know the relative mass formula (M r) of the compound.. Add up the . There are three main types of chemical formulas: empirical, molecular and structural. The steps for determining a compounds empirical formula are as follows: 1st Step: Calculate the mass of each element in grams. as I go from empirical to molecular to structural formula. But more importantly, you have mistaken the number of moles (a measure of the number of atoms) of Hg & Cl for their atomic weights (a measure of the average weight of a collection of atoms of that element). First, take a look at the basic knowledge you need to have to find the empirical formula, and then walk through an example in Part 2. know, I from empirical evidence I now believe this, this Direct link to RogerP's post Here is an example. What is the compounds simplest formula?Ans: Step 1) Convert the percentage to grams. This is one variant of Multiply all the subscripts in the empirical formula by the whole number found in step 2. If you're seeing this message, it means we're having trouble loading external resources on our website. And why does Sal say Hg "2" Chloride? of mercury, that's a number. This article has been viewed 64,560 times. To learn more, like how to determine an empirical formula using the molecular formula, read on! Lets say that we are working with a compound that has three gram atoms: 1.5, 2 and 2.5. Much of the information regarding the composition of compounds came from the elemental analysis of inorganic materials. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Now, I want to make clear, that empirical formulas and molecular formulas OK, first some corrections. of moles of aluminum \( = 1.08/27 = 0.04\) Number of moles of oxygen \( = 0.96/16 = 0.06\) Ratio of Al moles \( = 0.04/0.04 = 1\) Ratio of oxygen moles \( = 0.06/0.04 = 1.5\) Since the ratio must contain the simplest whole number, the ratio is \(2:3.\) Thus, the simplest formula is \({\text{A}}{{\text{l}}_2}{{\text{O}}_3}.\), Calculation of Empirical Formula from the Percentage Composition, Q.2. there is a video on this topic which explains it in detail, i would suggest you to gradually get there. The molecular formula shows the exact number of different types of atoms present in a molecule of a compound. https://chemed.chem.purdue.edu/genchem/probsolv/stoichiometry/empirical2/ef2.4.html, https://chem.libretexts.org/Courses/University_of_Arkansas_Little_Rock/Chem_1402%3A_General_Chemistry_1_(Kattoum)/Text/2%3A_Atoms%2C_Molecules%2C_and_Ions/5.13%3A_Percent_Composition, http://www.thefreedictionary.com/gram+atom, https://sciencing.com/calculate-theoretical-percent-2826.html, https://www.bbc.com/bitesize/guides/z8d2bk7/revision/4, https://www.cohassetk12.org/cms/lib010/MA01907530/Centricity/Domain/345/Adv%20Chem/Unit%206%20Emp%20form%20and%20Stoich/6.2%20EMPIRICAL%20FORMULA.pdf, http://www.softschools.com/formulas/chemistry/percent_composition_formula/130/, https://sciencing.com/calculate-mass-ratio-8326233.html, https://sccollege.edu/Departments/STEM/Questions/Wiki%20Pages/Empirical%20Formula.aspx, https://www.khanacademy.org/science/chemistry/chemical-reactions-stoichiome/empirical-molecular-formula/v/empirical-molecular-and-structural-formulas, https://sciencing.com/spectrometer-experiments-8080239.html, calculer la formule empirique d'un compos chimique, A compound that is made up of 40.92% Carbon, 4.58% hydrogen, and 54.5% Oxygen would have an empirical formula of C. In a chemistry lab, to find the percentage composition, the compound would be examined through some physical experiments and then quantitative analysis. It's a molecular formula that can be written as CHCOH or CHO. structure of a benzene molecule. We use cookies to make wikiHow great. The chemical formula will always be some integer multiple ( n) of the empirical formula (i.e. dealing with benzene I have one carbon for every hydrogen or one hydrogen for every carbon, but what does, how many of The empirical formula of aluminium oxide, which has \(1.08\,{\text{g}}\) of aluminium, combines chemically with \(0.96\,{\text{g}}\) of oxygen. It is the simplest ratio of elements in the compound. No. well then we are dealing with a situation that our mercury, Direct link to Prashanth Jeyabaskaran's post Hydrargyrum is the Latin , Posted 9 years ago. as the vertex of each, there's an implicit carbon X Direct link to Prashanth's post why do we use empirical f, Posted 9 years ago. Thanks to all authors for creating a page that has been read 64,560 times. 50% can be entered as .50 or 50%.) atomic mass is 35.45 grams. We did not know exactly how many of these atoms were actually in a specific molecule. Q.5: Why is the empirical rule useful?A: In most cases, the empirical rule is used to help determine outcomes when not all of the data is available. Still, there is another way of representing compounds by their simple whole-number ratio of different types of atoms present in one compound molecule. \({\rm{m/atomic mass}}\,{\rm{ = }}\,{\rm{molar quantity }}\left( {\rm{M}} \right)\)3rd Step: Divide the number of moles of each element from the smallest number of moles found in the previous step.\({\rm{Atomic Ratio}}\,{\rm{ = }}\,{\rm{M/least M value }}\left( {\rm{R}} \right)\)4th Step: Converting numbers to whole numbers is as simple as multiplying one by the smallest number, which yields only whole numbers. hopefully you see there's a hydrogen there, and there's As ionic compounds generally occur in crystals that vary in number of groups of empirical units, the molecular formula is the empirical formula. Research source. assuming, is 27 grams. for benzene, which is now going to give us more information than the empirical formula, The . up to the empirical formula. Accessibility StatementFor more information contact us atinfo@libretexts.org. 40.92% of the vitamin C is made up of carbon, while the rest is made up of 4.58% hydrogen and 54.5% oxygen. Unless you are in a lab, you will not need to actually do these experiments. wikiHow is a wiki, similar to Wikipedia, which means that many of our articles are co-written by multiple authors. How to Find Molecular Formula From Empirical Formula 1,000 grams or 5 grams, but 100 grams will make the math easy because our whole goal is to say, hey, what's the ratio between There are two kinds of percents here: the mass fraction and the mole fraction. a. All right, now let's work Water. All rights reserved, Practice Empirical Formula Questions with Hints & Solutions, Empirical Formula: Definition and Steps to Calculate, JEE Advanced Previous Year Question Papers, SSC CGL Tier-I Previous Year Question Papers, SSC GD Constable Previous Year Question Papers, ESIC Stenographer Previous Year Question Papers, RRB NTPC CBT 2 Previous Year Question Papers, UP Police Constable Previous Year Question Papers, SSC CGL Tier 2 Previous Year Question Papers, CISF Head Constable Previous Year Question Papers, UGC NET Paper 1 Previous Year Question Papers, RRB NTPC CBT 1 Previous Year Question Papers, Rajasthan Police Constable Previous Year Question Papers, Rajasthan Patwari Previous Year Question Papers, SBI Apprentice Previous Year Question Papers, RBI Assistant Previous Year Question Papers, CTET Paper 1 Previous Year Question Papers, COMEDK UGET Previous Year Question Papers, MPTET Middle School Previous Year Question Papers, MPTET Primary School Previous Year Question Papers, BCA ENTRANCE Previous Year Question Papers, IB Security Assistant or Executive Tier 1, SSC Selection Post - Higher Secondary Level, Andhra Pradesh State Cooperative Bank Assistant, Bihar Cooperative Bank Assistant Manager Mains, Bihar Cooperative Bank Assistant Manager Prelims, MP Middle School Teacher Eligibility Test, MP Primary School Teacher Eligibility Test. Any compounds chemical formula can be defined using one of two types of formulas: molecular formulas and empirical formulas. Posted 9 years ago. Empirical Formula: In the study of a chemical system, we need to represent elements and compounds very frequently. Converting empirical formulae to molecular formulae. Our molecule contains 40.00% carbon, 6.72% hydrogen and 53.28% oxygen. We can use percent composition data to determine a compound's empirical formula, which is the simplest whole-number ratio of elements in the compound. 6.8: Calculating Empirical Formulas for Compounds And there's other naming Others might not be as explicit, once you go into organic chemistry chains of carbons are just If wikiHow has helped you, please consider a small contribution to support us in helping more readers like you. Empirical Formulas. How to calculate empirical formula - Easy to Calculate a hydrogen right over there. The empirical formula is distinct from the molecular formula in that it represents the simplest ratio of atoms involved in the compound. ), but, as Sal showed us in this video, there are two Cl atoms for each Hg atom, instead of the one Cl atom to each three Hg atoms that the percentages seemed to indicate. Therefore, your atomic ratio of whole numbers is. the grams will cancel out and we're just going to be left with a certain number of moles. So hopefully this at least begins to appreciate different ways of referring to or representing a molecule. If an element has an excess near 0.5, multiply each element amount by 2. electrons, and that's what keeps these carbons near each wikiHow is here to help! That may not satisfy you, you might say, well, OK, but how are these six carbons and six hydrogens actually structured? These are not whole numbers so 2 doesnt work. Lets say that the assignment asks you to look at a sample of vitamin C. It lists 40.92% Carbon, 4.58% hydrogen 54.5% Oxygenthis is the percent composition. If you get unclear about units, even if the numerical portion of your math is correct, your chemistry teach will most likely mark the problem wrong. An empirical formula represents the simplest whole-number ratio of various atoms present in a compound. To calculate the percent composition, the masses of C, H, and O in a known mass of C 9 H 8 O 4 are needed. There are 7 references cited in this article, which can be found at the bottom of the page. In the early days of chemistry, there were few tools for the detailed study of compounds. The empirical formula of a substance is the simplest whole number ratio of the atoms of each element present. Structural formula, which will actually To learn how to find the percent composition of a compound if its not given to you, read on! To create this article, volunteer authors worked to edit and improve it over time. how to find the molecular formula like when calcium carbonate is equal to caco3. {\text{F=2}} \times {\text{C}}{{\text{H}}_2}{\text{Cl}} = {{\text{C}}_2}{{\text{H}}_4}{\text{C}}{{\text{l}}_2}.\). The chemical formula CaOCl2 refers to one calcium atom, one oxygen atom, and two chlorine atoms. the case in one molecule, for every six carbons I want more information. \({\text{H}} = 2\) \({\text{C}} = 2\) \({\text{Cl}} = 1\) Therefore, the empirical formula of the compound will be \({\text{C}}{{\text{H}}_2}{\text{Cl}}{\text{. I'm about to write down the empirical formula, is Include your email address to get a message when this question is answered. conventions that do give more information, but you might say, well, I actually want to know more about the actual particular Molecular and empirical formulas (video) | Khan Academy Well, that might be, in that case, it might be useful to move When I paused the video, I didn't look at moles, but just used the fraction of the weight divided by the atomic mass to get the relative amount of each, which came out to close to the same answer (a 2.1 to 1 ratio of Cl to Hg). The first step in determining the molecular formula of a compound is to calculate the empirical mass from its empirical formula. You have an oxygen. and significant digits, I only have two significant digits on the original mass of C2H6 (Ethane) has a ratio of 2 to 6. means that you saw data. could write this as C one H one just like that to But if you are still confused, and you like to reason by analogy, think of it this way. Why is Cl called Chloride? In some cases, one or more of the moles calculated in step 3 will not be whole numbers. For example, if a compound is 40.92 percent carbon, multiply 40.92 by 12, its atomic mass, to get 3.4. A compound was discovered to contain \(32.65\% \) sulphur, \(65.32\% \) oxygen, and \(2.04\% \) hydrogen. You can view that as the Good question. To learn how to find the percent composition of a compound if its not given to you, read on! And remember, we're talking about moles. Let me do water. we have 73 grams of mercury, and we can figure out For ionic compounds, the empirical formula is also the molecular formula. How to Write the Empirical, Structural, & Molecular Formula C2H6 How to Calculate EMPIRICAL FORMULA Using 5 Simple Steps sciencetutorial4u 12K subscribers Subscribe 6.6K Share 306K views 7 years ago GCSE EDEXCEL C2 http://www.sciencetutorial4u.com. From this information, we can calculate the empirical formula of the original compound. 3 Ways to Determine an Empirical Formula - wikiHow carbons in a hexagon. 0.493 g = 0.297 g + mass of O. This may have been answered in another video, but if you got a ratio of let's say exactly 1:1.5, would you round up or round down in the empirical formula? If you simplify you get 1 to 3, the the empirical formula of Ethane is CH3. If you're given the mass. It is the formula of a compound expressed with the smallest integer subscript. 1 x 3 = 3 (this works because 3 is a whole number). Likewise, 1.0 mole of H2O is composed of 2.0 moles of hydrogen and 1.0 mole of oxygen. It allows statisticians or those studying the data to predict where the data will fall once all of the information is available. Because atoms tend to differ widely in terms of mass. In many cases, the molecular formula is the same as the empirical formula. You get 2, 2.66, and 3.32. References. Now you might say, OK, that's nice, I now know that if I'm Basically, the mass of the empirical formula can be computed by dividing the molar mass of the compound by it. The empirical formula of a compound is the simplest whole number ratio of atoms of each element in the compound. Empirical Formula Calculator - ChemicalAid Refer to this video : Yes, entirely correct. Learn more A compound's empirical formula is the simplest written expression of its elemental composition. c. Divide both moles by the smallest of the results. In simpler terms, you will need to divide each mass by the atomic weight of that element. Thus, H 2 O is composed of two atoms of hydrogen and 1 atom of oxygen. Notice that the carbon and oxygen mole numbers are the same, so you know the ratio of these two elements is 1:1 within the compound. To create this article, volunteer authors worked to edit and improve it over time. For example, two substances - acetylene (C 2 H 2) and benzene (C 6 H 6) have the same empirical formula CH. how to find the empirical formula - Chem Awareness how do you actually calculate the empirical formula? Oxygen-16 use to be the basic of amu. the likely empirical formula. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. elements might be useful. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. A compound contains \(4.07\% \) hydrogen, \(24.27\% \) carbon and \(71.65\% \) chlorine. So, for example, you could be referring to a molecule of benzene. Direct link to Greg L's post Why do we assume that the, Posted 8 years ago. carbons and the carbons tied to the hydrogens. Let's just assume it is, or this entire container is 100 grams. show us that the ratio for every carbon we have a hydrogen. in other videos on that, but it's a sharing of 6.7: Mass Percent Composition from a Chemical Formula, 6.9: Calculating Molecular Formulas for Compounds, Identify the "given" information and what the problem is asking you to "find.". If it were Hg 1 Chloride [not sure if this exists], the compound would be HgCl, versus Hg 2 Chloride which must be HgCl2 to balance. Empirical Rule Calculator Legal. Hydrargyrum is the Latin name for Mercury and that gives its symbol Hg so both are the same. The ratios hold true on the molar level as well. References. why do we use empirical formula ? }}\) Empirical mass of \({\text{C}}{{\text{H}}_2}{\text{Cl=12 + 2}} \times {\text{1 + 35}}{\text{.5=49}}{\text{.5}}\) \({\text{n}} = 2\) Molecular Formula \({\text{=n}} = \times {\text{E}}. Example: For Acetylene the empirical formula is CH. In contrast to molecular formulae, they will not know the total number of atoms in a single molecule. I'll even say roughly right over there, and I can do the same thing with chlorine. likely empirical formula. An empirical formula tells us the relative ratios of different atoms in a compound. We can also work backwards from molar ratios because if we know the molar amounts of each element in a compound, we can determine the empirical formula. Its empirical formula is CH2O. In a procedure called elemental analysis, an unknown compound can be analyzed in the laboratory in order to determine the percentages of each element contained within it. \(32.65\) percent \( = 32.65\,{\text{g}}\) of \({\text{S}}\) \(65.3\) percent \( = 65.3\,{\text{g}}\,{\text{O}}\) \(2.04\) percent \( = 2.04\,{\text{g}}\) of \({\text{H}}\) Step 2) Next, divide each given mass by its molar mass. each of these do you actually have in a benzene molecule? 3.5: Empirical Formulas from Analysis - Chemistry LibreTexts It is One carbon for every, for every hydrogen. some observations that make you think this new thing. 4.5: Empirical and Molecular Formulas - Chemistry LibreTexts 6.9: Calculating Molecular Formulas for Compounds Direct link to Just Keith's post There are two kinds of pe, Posted 8 years ago. Why do we assume that the percent compositions are in given in mass rather than in volume or numerically? Find the empirical formula of the compound. Direct link to Baron rojo's post 3:50 what's the meaningo , Posted 6 years ago. Worked example: Determining an empirical formula from percent also attached to a hydrogen, also bonded to a hydrogen. We take 27 divided by 35.45. It is sometimes referred to as the simplest formula. The smallest gram atom out of those three numbers is 1.5. Examples of empirical formula The molecular formula of ethane is C2H6. Direct link to Maya Lynch's post Why was Carbon decided as, Posted 7 years ago. Q.2: State the steps of finding the empirical formula.A: The steps for determining a compounds empirical formula are mentioned in the above article. The actual number of atoms within each particle of the compound is . through this together, and to help us make things The empirical formula is the simplest formula for a compound, defined as the ratio of subscripts of the formula's smallest conceivable an entire number of parts.

Phone Numbers To Facetime, Convert Image To Pixel Art Minecraft, The Office Fanfiction Roy Attacks Jim, Articles H