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Interpretation:
The formulas of potassium nitride and cobalt(III) oxide are to be written.
Concept introduction:
When atom accepts or loses electrons it is termed as ion. If the ion is formed from a single atom, it is referred as monatomic ion. But, in nature, many compounds are found as polyatomic ions (poly = many). Polyatomic ions are electronically neutral, for example, ammonium ion will not exist without its counter negative ion. In general, formulas of ionic compounds depict the ratio of positive and negative ions found in a substance. Moreover, the formulas of compounds are made up of lowest whole number ratio of ions i.e., formula unit. Notably, the number of positive units and the number of negative units will be equal in a chemical formula. The polyatomic ion when used in more than once, parentheses is used, and the parentheses is applied only for polyatomic ions.
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Chapter 6 Solutions
Introductory Chemistry: An Active Learning Approach
- Write the formulas of the following compounds. (a) ammonia (b) laughing gas (c) hydrogen peroxide (d) sulfur trioxidearrow_forwardCobalt(II) sulfate heptahydrate has pink-colored crystals. When heated carefully, it produces cobalt(II) sulfate monohydrate, which has red crystals. What are the formulas of these hydrates? If 3.548 g of the heptahydrate yields 2.184 g of the monohydrate, how many grams of the anhydrous cobalt(II) sulfate could be obtained?arrow_forwardA platinum-containing compound, known as Magnuss green salt, has the formula [Pt(NH3)4][PtCl4] (in which both platinum ions are Pt2+). Name the cation and the anion.arrow_forward
- Write the formula for copper(II) nitrate. Give complete steps in explaining the steps you used to name the compound.arrow_forwardWrite the formula for a compound composed of Ammonium and sulfur.arrow_forwardGive the formulas of the compounds in each set: (a) lead(II)oxide and lead(IV) oxide; (b) lithium nitride, lithium nitrite, and lithium nitrate; (c) strontium hydride and strontium hydroxide;(d) magnesium oxide and manganese(II) oxide.arrow_forward
- Give the chemical formula of the acid. Your answer will be marked incorrect if you did not spelled the compound's name correctly. Please remember to include (aq) to your answer. Nitric acid Sulfuric acidarrow_forwardWrite the formula for each of the following compounds and indicate which ones are best described as ionic: sodium hypochlorite boron triiodide aluminum perchlorate calcium acetate potassium permanganate ammonium sulfite potassium dihydrogen phosphate disulfur dichloride chlorine trifluoride phosphorus trifluoride 2.A drop of water has a volume of about 0.050 mL. How many molecules of water are in a drop of water? (Assume water has a density of 1.00 g/cm3.) 3.Capsaicin, the compound that gives the hot taste to chili peppers, has the formula C18H27NO3. (a) Calculate its molar mass. If you eat 55 mg of capsaicin, what amount (moles) have you consumed? Calculate the mass percent of each element in the compound. What mass of carbon (in milligrams) is there in 55 mg of capsaicin? 4.Malic acid, an organic acid found in apples, contains C, H, and O in the following ratios: C1H50O1.25. What is the empirical formula of…arrow_forward2. Give the formula and name of an ionic compound containing (a) the sulfate ion, (b) the nitrite ion.arrow_forward
- Express your answer as a chemical formula. Calcium acetate Tin(II) nitrite Calcium chlorite Chromium(III) sulfate Aluminum sulfitearrow_forwardWhen looking at a compound's formula, they can become rather complicated. A simple compound might be CO2. The two capital letters tell us there are two elements. The carbon has no subscript directly to the right of it which means that, in this compound, there is only one carbon atom. The oxygen atom has a subscript of 2 which means that, in this compound, there are two oxygen atoms. How many atoms of sulfur are present in H2SO4?arrow_forwardThe element X has two naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is amu. Isotope | Abundance (%) | Mass (amu) 31x 35.16 31.16 34x 64.84 34.30 O 35.22 O 30.20 O 32.73 O 33.20 О 34.02arrow_forward
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