C. 2.25
Grams to Atoms Calculator - Free online Calculator - BYJUS 1:07. C. 57% Solution: Using the generic expression to convert g to atoms: Number of Atoms = (Given Mass/Molar Mass) * Avogadro's Number Number of Atoms = (78/40.078) * 6.02 * 10^ {23} Number of Atoms = 1.9462 * 6.02 * 10^ {23} Number of Atoms = 1.171 * 10^ {+24} A crystalline solid can be represented by its unit cell, which is the smallest identical unit that when stacked together produces the characteristic three-dimensional structure. We can find the number of moles of this substance by dividing our given mass in grams by our molar mass. d. Determine the packing efficiency for this structure. What conclusion(s) can you draw about the material? E. 7.2 x 10^23 g, How many moles are in a 45g sample of C6H12O6? 6. How many formula units must there be per unit cell? A. Determine the mass in grams of NaCl that are in 23.4 moles of NaCl?
How to Calculate the Number of Atoms in a Sample | Sciencing Lithium crystallizes in a bcc structure with an edge length of 3.509 .
how many atoms are in 197 g of calcium - wpc.org.pk Each carbon-12 atom weighs about \(1.99265 \times 10^{-23}\; g\); therefore, \[(1.99265 \times 10^{-23}\; g) \times (6.02214179 \times 10^{23}\; atoms) = 12\; g\; \text{ of carbon-12} \nonumber \]. 4.366mol * 6.022*10^23atoms/mol = 2.629*10^24 atoms of Ca in 175g of Ca. Solutions and Solubility (part 1) (M3Q1), 11. How many grams of water 32g B. C3H6O3 Calculate the edge length of the face-centered cubic unit cell and the density of aluminum. How many sodium atoms (approx.) Identify the metal, determine the unit cell dimensions, and give the approximate size of the atom in picometers. Charge of Ca=+2. This basic repeating unit is called a unit cell. E. 4.8 x 10^24, There are 1.5 x 10^25 water molecules in a container. (a) In an FCC structure, Ca atoms contact each other across the diagonal of the face, so the length of the diagonal is equal to four Ca atomic radii (d = 4r). (CC BY-NC-SA; anonymous by request). 5. What type of electrical charge does a proton have? (CC BY-NC-SA; anonymous by request), Figure 12.3 Unit Cells in Three Dimensions. We focus primarily on the cubic unit cells, in which all sides have the same length and all angles are 90, but the concepts that we introduce also apply to substances whose unit cells are not cubic. A) C.HO Isotopes, Atomic Mass, and Mass Spectrometry (M2Q3), 10. How many Au atoms are in each unit cell? .85 g Electron Configurations for Ions (M7Q10), 46. How many grams of carbs should a type 1 diabetic eat per day? Label the regions in your diagram appropriately and justify your selection for the structure of each phase.
How many atoms in an 197*g mass of calcium metal? | Socratic D. 71% One simply needs to follow the same method but in the opposite direction. If we choose the second arrangement and repeat the pattern indefinitely, the positions of the atoms alternate as ABCABC, giving a cubic close-packed (ccp) structure (part (b) in Figure 12.7). D. 76% Why do people say that forever is not altogether real in love and relationship. C. 25 Therefore, the answer is 3.69 X Calculate its density. What is the atomic radius of tungsten in this structure? Metallic iron has a body-centered cubic unit cell (part (b) in Figure 12.5). How many moles are in the product of the reaction. Acids, Bases, Neutralization, and Gas-Forming Reactions (M3Q3-4), 13. Bromine-195 Fluorine- 133, Ike was blamed for at least 195 deaths. The metal is known to have either a ccp structure or a simple cubic structure. If the mass of a substance is known, the number of moles in the substance can be calculated. J.R. S. Paige C. (a) In this single layer of close-packed spheres, each sphere is surrounded by six others in a hexagonal arrangement.
Solid Crystal Lecture Flashcards | Quizlet The procedure to use the grams to atoms calculator is as follows: Step 1: Enter the atomic mass number, grams and x in the respective input field Step 2: Now click the button "Calculate x" to get the output Step 3: Finally, the conversion from grams to atoms will be displayed in the output field How to Convert Grams to Atoms? The final step will be to compare it to the 19.32 value. The mole, abbreviated mol, is an SI unit which measures the number of particles in a specific substance. 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. Get a free answer to a quick problem. Ionic Crystals and Unit Cell Stoichiometry (M11Q6), Appendix E: Specific Heat Capacities for Common Substances (M6Q5), Appendix F: Standard Thermodynamic Properties (M6), Appendix G: Bond Enthalpy, Bond Length, Atomic Radii, and Ionic Radii. What is the empirical formula of this substance? Problem #7: Tungsten has an atomic radius of 137 pm and crystallizes in a cubic unit cell having an edge length d = 316 pm. The density of nickel is 8.908 g/cm3. In one approach, the spacing between ions in an ionic substance is determined by using X-ray diffraction. The density of a metal and length of the unit cell can be used to determine the type for packing. Chromium has a structure with two atoms per unit cell. How many atoms are in a 3.0 g sample of sodium (Na)? B. C. 80 g The concept of unit cells is extended to a three-dimensional lattice in the schematic drawing in Figure 12.3. Determine the mass, in grams, of 0.400 moles of Pb (1 mol of Pb has a mass of 207.2 g). 4. 0.650g Au 196.966569 g molAu = 0.00330 mol Au atoms 1mol atoms = 6.022 1023atoms Multiply the calculated mol Au times 6.022 1023atoms 1mol. Direction of Heat Flow and System vs. Surroundings (M6Q2), 28. 35,000 worksheets, games, and lesson plans, Spanish-English dictionary, translator, and learning, a Question Also, one mole of nitrogen atoms contains \(6.02214179 \times 10^{23}\) nitrogen atoms. 2 chlorine atoms are needed. A. SO2 Note the similarity to the hexagonal unit cell shown in Figure 12.4. The number of atoms can also be calculated using Avogadro's Constant (6.022141791023) / one mole of substance. E. 89%, Mass percent of titanium in TiCl2? Since each vertex is in a total of 8 cells, we have 1 F atom in the unit cell. Each atom has eight nearest neighbors in the unit cell, and 68% of the volume is occupied by the atoms. 9. Aluminum (atomic radius = 1.43 ) crystallizes in a cubic closely packed structure. A BCC unit cell contains two atoms: one-eighth of an atom at each of the eight corners (8 [latex]\frac{1}{8}[/latex] = 1 atom from the corners) plus one atom from the center. I now know what to do to determine the atomic radius. We're asked to calculate the number of atoms of #"Ca"# in #153# #"g Ca"#. Each atom in the lattice has six nearest neighbors in an octahedral arrangement. And thus we can find the number of calcium atoms in a lump of metal, simply by measuring the mass of the lump and doing a simple calculation. ?mol.
- You want to make a molecule that has Calcium Ca and Chloride Cl. The smallest repeating unit of a crystal lattice is the unit cell. Identify the element. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Explain your answer. The total number of atoms in a substance can also be determined by using the relationship between grams, moles, and atoms. Can crystals of a solid have more than six sides? Any atom in this structure touches four atoms in the layer above it and four atoms in the layer below it. The experimentally determined density of a material is lower than expected based on the arrangement of the atoms in the unit cell, the formula mass, and the size of the atoms. A. FeO Two adjacent edges and the diagonal of the face form a right triangle, with the length of each side equal to 558.8 pm and the length of the hypotenuse equal to four Ca atomic radii: Solving this gives r=[latex]{\frac{(558.8\;\text{pm})^2\;+\;(558.5\;\text{pm})^2}{16}}[/latex] = 197.6 pm fro a Ca radius. (c) Using the volume of a silver atom and the formula for the volume of a sphere, calculate the radius in angstroms of a silver atom. B. The fact that FCC and CCP arrangements are equivalent may not be immediately obvious, but why they are actually the same structure is illustrated in Figure 4.
How many gold atoms are contained in 0.650 grams of gold? ), Then, the density of Ca = [latex]\frac{2.662\;\times\;10^{-22}\;\text{g}}{1.745\;\times\;10^{-22}\;\text{cm}^{3}}[/latex] = 1.53 g/cm3. figs.). For example, gold has a density of 19.32 g/cm3 and a unit cell side length of 4.08 . 44 Converting moles of a substance to atoms requires a conversion factor of Avogadro's constant (6.022141791023) / one mole of substance. One mole is equal to \(6.02214179 \times 10^{23}\) atoms, or other elementary units such as molecules. D. 1.2x10^24 Atoms on a corner are shared by eight unit cells and hence contribute only \({1 \over 8}\) atom per unit cell, giving 8\({1 \over 8}\) =1 Au atom per unit cell. What are the 4 major sources of law in Zimbabwe. An atom at a corner of a unit cell is shared by all eight adjacent unit cells and therefore contributes 18 atom to each.The statement that atoms lying on an edge or a corner of a unit cell count as 14 or 18 atom per unit cell, respectively, is true for all unit cells except the hexagonal one, in which three unit cells share each vertical edge and six share each corner (Figure 12.4), leading to values of 13 and 16 atom per unit cell, respectively, for atoms in these positions. Avogadro's Number of atoms. 40% Then the number of moles of the substance must be converted to atoms. Using Avogadro's number, #6.022 xx 10^23"particles"/"mol"#, we can calculate the number of atoms present: #color(blue)(3.82# #cancel(color(blue)("mol Ca"))((6.022xx10^23"atoms Ca")/(1cancel("mol Ca")))#, #= color(red)(2.30 xx 10^24# #color(red)("atoms Ca"#, 84931 views There is only one Ca atom. 4.45 x 10 ^26 atoms. The line that connects the atoms in the first and fourth layers of the ccp structure is the body diagonal of the cube. The density of calcium can be found by determining the density of its unit cell: for example, the mass contained within a unit cell divided by the volume of the unit cell. (The mass of one mole of calcium is 40.08 g.).00498 mol. The transition temperature, the temperature at which one phase is converted to the other, is 95C at 1 atm and 135C at 1000 atm. A. Science Chemistry Chemistry questions and answers Resources How many atoms are in 197 g of calcium? Because closer packing maximizes the overall attractions between atoms and minimizes the total intermolecular energy, the atoms in most metals pack in this manner. Why was the decision Roe v. Wade important for feminists? 3 hours ago. 100% (27 ratings) for this solution. Converting moles of a substance to grams requires a conversion factor of molar mass of substance/one mole of substance. 3. Join Yahoo Answers and get 100 points today. \[10.78 \cancel{\;mol\; Ca} \left(\dfrac{40.08\; g\; Ca}{1\; \cancel{mol\; Ca}}\right) = 432.1\; g\; Ca \nonumber \]. In a cubic unit cell, corners are 1/8 of an atom, edges are 1/4 of an atom, and faces are 1/2 of an atom. C. 2 D. 3.6 x 10 ^24 Then, multiply the number of moles of Na by the conversion factor 6.022141791023 atoms Na/ 1 mol Na, with 6.022141791023 atoms being the number of atoms in one mole of Na (Avogadro's constant), which then allows the cancelation of moles, leaving the number of atoms of Na. And of course, we can also find the number of calcium atoms given a mass, and a formula for a calcium-containing material. The density of solid NaCl is 2.165 g/cm3. #6.022xx10^23# individual calcium atoms have a mass of #40.1*g#. To calculate the number of atoms in the unit cell, multiply the number of atoms on vertices times the fraction of each atom that is within the unit cell. Some metals crystallize in an arrangement that has a cubic unit cell with atoms at all of the corners and an atom in the center, as shown in Figure 2. How does the mole relate to molecules and ions? 100% (3 ratings) The molar mass of calcium is 40.078 . Approx.
Step 1: Find the Molar Mass of the Formula Find a periodic table of elements to find the molar mass of your sample.
Types of Unit Cells: Body-Centered Cubic and Face-Centered - Unizin Shockingly facts about atoms. My avg. The atomic mass of Copper is 63.55 atomic mass units. How many moles of potassium (\(\ce{K}\)) atoms are in 3.04 grams of pure potassium metal? Explanation: To calculate the n of moles of Ca that they are in 137 g, we can use the next relation: n = mass/atomic mass = (137 g)/ (40.078 g/mol) = 3.4 mol. Then, we need to convert moles to atoms which we do with Avogadro's constant which is 6.022*10^23atoms/mol. Step-by-step solution. C) HCO D) CO, The analysis of a compound shows it contains 5.4 mol C, 7.2 mol H, and 1.8 mol N. What is the empirical formula of the compound? Solution: 1) Calculate the average mass of one atom of Fe: 55.845 g mol1 6.022 x 1023atoms mol1= 9.2735 x 1023g/atom 2) Determine atoms in 1 cm3: 7.87 g / 9.2735 x 1023g/atom = 8.4866 x 1022atoms in 1 cm3 3) Determine volume of the unit cell: 287 pm x (1 cm / 1010pm) = 2.87 x 108cm The structures of many metals depend on pressure and temperature. 1 point How many chlorine atoms are there in 20.65 moles of aluminum chloride? This means that #"Avogadro's number"# of calcium atoms, i.e. mph. The arrangement of atoms in a simple cubic unit cell. A. Electron Configurations, Orbital Box Notation (M7Q7), 41. consumption of carbohydrates is limited to 65 grams x 3 meals, or a total of 195 grams. 5. Number of atoms = Mass Molar mass Avogadro's number. Amounts may vary, according to . (1 = 1 x 10-8 cm. Using the Pythagorean Theorem, we determine the edge length of the unit cell: We conclude that gold crystallizes fcc because we were able to reproduce the known density of gold. 1) Calculate the average mass of one atom of Fe: 287 pm x (1 cm / 1010 pm) = 2.87 x 108 cm. No packages or subscriptions, pay only for the time you need. Any intensive property of the bulk material, such as its density, must therefore also be related to its unit cell. A single layer of close-packed spheres is shown in part (a) in Figure 12.6.
How many atoms are in 149 g of calcium? | Wyzant Ask An Expert Each unit cell has six sides, and each side is a parallelogram. Solutions and Solubility (part 2) (M3Q2), 12. For instance, consider methane, CH4. Figure 3. The number of moles in a system can be determined using the atomic mass of an element, which can be found on the periodic table. The idea of equivalent mass, the use of mass to represent a NUMBER of combining particles, is fundamental to the study of chemistry, and should not require too much angst to incorporate. (CC BY-NC-SA; anonymous by request). 25% If the cubic unit cell consists of eight component atoms, molecules, or ions located at the corners of the cube, then it is called simple cubic (part (a) in Figure 12.5). When we count atoms or ions in a unit cell, however, those lying on a face, an edge, or a corner contribute to more than one unit cell, as shown in Figure 12.5. B.
How many calcium atoms can fit between the Earth and the Moon? What is the atomic radius of platinum? Why is the mole an important unit to chemists? C) CH E. 1.4 x 10^24, What is the amss of 1.5 x 10^21 water molecules? What is the length of the edge of the unit cell? Also, one mole of nitrogen atoms contain, Example \(\PageIndex{1}\): Converting Mass to Moles, Example \(\PageIndex{2}\): Converting Moles to mass, constant, it is also easy to calculate the number of atoms or molecules present in a substance (Table. Why is the mole an important unit to chemists? (The mass of one mole of arsenic is 74.92 g.). Protons, Neutrons, and Electrons (M2Q1), 6.
Answered: 6. You need to prepare 825. g of a | bartleby The unit cell has an edge of 546.26 pm and has a density of 3.180 g/cm3. The total number of Au atoms in each unit cell is thus 3 + 1 = 4. We specify this quantity as 1 mol of calcium atoms. .5 By definition, a hurricane has sustained winds of at least 74 What we must first do is convert the given mass of calcium to moles of calcium, using its molar mass (referring to a periodic table, this is #40.08"g"/"mol"#): #153# #cancel("g Ca")((1"mol Ca")/(40.08cancel("g Ca"))) = color(blue)(3.82# #color(blue)("mol Ca"#. C. SO3 I'll call it the reference cube. A. A 1.000-g sample of gypsum contains 0.791 g CaSO4. Using 316 pm for d and 548 pm for 4r, we have this: We find 199712 for the left and 300304 for the right, so the idea that tungsten is fcc fails. Above any set of seven spheres are six depressions arranged in a hexagon. As indicated in Figure 12.5, a solid consists of a large number of unit cells arrayed in three dimensions. cubic close packed (identical to face-centered cubic). How to find atoms from grams if you are having 78g of calcium? .25 B. NO3 (Elements or compounds that crystallize with the same structure are said to be isomorphous.). Metallic rhodium has an fcc unit cell. Answer (1 of 5): It's not fix like no. B. For body-centered, please see problem #2 here for this equation: Due to the fact that these numbers are roughly equivalent, we can conclude that tungsten is being body-centered cubic. What are the Physical devices used to construct memories? Explain your answer. (b) Because atoms are spherical, they cannot occupy all of the space of the cube. Gold does not crystallize bcc because bcc does not reproduce the known density of gold. Core and Valence Electrons, Shielding, Zeff (M7Q8), 43. Thus, an atom in a BCC structure has a coordination number of eight. 197 g Actiu Go to This problem has been solved! D. 4.5g Each packing has its own characteristics with respect to the volume occupied by the atoms and the closeness of the packing. There are two atoms in a body-centered cubic. What is are the functions of diverse organisms? Figure 12.7 Close-Packed Structures: hcp and ccp. A We know from Example 1 that each unit cell of metallic iron contains two Fe atoms. Predicting Molecular Shapes: VSEPR Model (M9Q1), 50. 0.134kg Li (1000g/1kg)= 134g Li (1mol/6.941g)= 19.3 mols Li, 19.3 (6.022x1023 atoms/ 1mol) = 1.16x1025 atoms of Li. Similarly, if the moles of a substance are known, the number grams in the substance can be determined. Which of the following is this compound?
12.2: The Arrangement of Atoms in Crystalline Solids complete transfer of 2 electrons from Ca to Cl. What we must first do is convert the given mass of calcium to moles of calcium, using its molar mass (referring to a periodic table, this is 40.08 g mol ): 153 g Ca( 1mol Ca 40.08g Ca) = 3.82 mol Ca What are the answers to studies weekly week 26 social studies? (ac) Three two-dimensional lattices illustrate the possible choices of the unit cell. As shown in Figure 12.5, a face-centered cubic unit cell has eight atoms at the corners of the cube and six atoms on the faces. For each mole of a molecule contains Avogadro's number of molecules (NA = 6.022 x 10). The atoms at the corners touch the atoms in the centers of the adjacent faces along the face diagonals of the cube. \[3.5\; \cancel{g\; Na} \left(\dfrac{1\; mol\; Na}{22.98\; \cancel{g\; Na}}\right) = 0.152\; mol\; Na \nonumber \], \[0.152\; \cancel{mol\; Na} \left(\dfrac{6.02214179\times 10^{23}\; atoms\; Na}{1\;\cancel{ mol\; Na}}\right) = 9.15 \times 10^{22}\; atoms\; of\; Na \nonumber \].
Chapter 3 Practice Test Flashcards | Quizlet To calculate the density of a solid given its unit cell. Answer (1 of 4): Well, what is the molar quantity of carbon atoms in such a mass? Just as a pair can mean two shoes, two books, two pencils, two people, or two of anything else, a mole means 6.022141791023 of anything. E. H2O2, The empirical formula of a compound is CH and molecular weight = 78amu. The molar mass is used to convert grams of a substance to moles and is used often in chemistry. Types of Unit Cells: Primitive Cubic Cell (M11Q4), 61. 1 atom. 1) Calculate the average mass of one atom of Na: 4) Determine number of unit cells in 1 cm3: Problem #2: Metallic iron crystallizes in a type of cubic unit cell. Finally, if you are asked to find the number of atoms in one mole, for example, the number of H atoms in one mole of H2O, you multiply the number of atoms by.
CHEM 1411 - chapter 3 quiz Flashcards | Quizlet C) C.H.N. 22% A face-centered cubic solid has atoms at the corners and, as the name implies, at the centers of the faces of its unit cells. Cl gains 1 electron each. 10 C. 126 The cubic hole in the middle of the cell has a barium in it. 3. A link to the app was sent to your phone. B. S2O3 C. N2O If all the people who have existed in Earth's history did nothing but count individual wheat grains for their entire lives, the total number of wheat grains counted would still be much less than Avogadro's constant; the number of wheat grains produced throughout history does not even approach Avogadro's Number. How can I calculate the moles of a solute. A body-centered cubic (bcc) unit cell contains one additional component in the center of the cube. 3) Calculate the mass of NaCl inside the cube: 4) The molar mass divided by the mass inside the cube equals Avogadro's Number. Map: General Chemistry: Principles, Patterns, and Applications (Averill), { "12.01:_Crystalline_and_Amorphous_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
b__1]()", "12.02:_The_Arrangement_of_Atoms_in_Crystalline_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.03:_Structures_of_Simple_Binary_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.04:_Defects_in_Crystals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.05:_Bonding_and_Properties_of_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.06:_Metals_and_Semiconductors" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.07:_Superconductors" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.08:_Polymers" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12.09:_Modern_Materials" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Introduction_to_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Molecules_Ions_and_Chemical_Formulas" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Reactions_in_Aqueous_Solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Energy_Changes_in_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_The_Structure_of_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_The_Periodic_Table_and_Periodic_Trends" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Ionic_versus_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Molecular_Geometry_and_Covalent_Bonding_Models" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Fluids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Chemical_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Aqueous_AcidBase_Equilibriums" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Solubility_and_Complexation_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Chemical_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Periodic_Trends_and_the_s-Block_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_The_p-Block_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "22:_The_d-Block_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "23:_Organic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "24:_Nuclear_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 12.2: The Arrangement of Atoms in Crystalline Solids, [ "article:topic", "showtoc:no", "license:ccbyncsa", "authorname:anonymous", "program:hidden", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FBook%253A_General_Chemistry%253A_Principles_Patterns_and_Applications_(Averill)%2F12%253A_Solids%2F12.02%253A_The_Arrangement_of_Atoms_in_Crystalline_Solids, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 12.3: Structures of Simple Binary Compounds, Hexagonal Close-Packed and Cubic Close-Packed Structures, status page at https://status.libretexts.org.