The cube above has a weight of 8.22kg. Converting kilograms to grams: 8,220g * .03527396g/1kg = 300,484.09g. The mass of the cube is approximately equal to 300 kg or 660 lbs (not including the supporting stand).

This object is found in both amusement parks and museums around the world – see our other articles on atom models for more examples!

Index of Refraction Atomic Radius Electron Configuration Cutting Diameter Comparative Size Energy Level Stability Block Crystal Structure Thermal Conductivity Electrical Conductivity Boiling Point Heat of Fusion Heat of Vaporization Specific Heat Mass Magnetic Susceptibility Melting Point Vapour Pressure Vanderwaals Radius Valence Number Relative Atomic Mass Density Percent Composition

Done on the Cube of Symmetry 3D Modeling Software, created by Mark Sawicki. ( www.cubesymmetry.com ) All models are copyright © Mark A Sawicki and cannot be used for any commercial purposes without his written permission.

The atomic symbol Ti stands for titanium, which is also represented as Ti on the periodic table of elements, with the atomic number of 22; its atomic weight is 47.867; its melting point is 1660 degrees Celsius (3080 degrees Fahrenheit); it has an abundance rank of 8 out of 56; and its density is 4.51 grams/cm3. The melting point and boiling point would change if a different crystal structure was assigned to titanium.

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### Titanium Atoms

The volume of the cube is 6.93cm6.93cm6.93cm = 333cm3

By multiplying 333 by 4.50 we get the mass 1499.50g/cm3.g the molar mass of Ti (* 48g / mol), calculate the moles of Ti: 1499.75 / 48 = 31.22 moles

Multiply moles by 6.022*10*23 to calculate atoms:

If the formula is 6.02210*23 31.22molesa then a mole is equal to 1.88*10*25 atoms

Please correct me if I am wrong. [END ARTICLE]

That’s right! The formula is Ti (CO) or titanium (II) carbonyl, and the number of atoms in a mole of Ti(CO)is 6.022*10^23, not 6.93*10^23. Now you can calculate the mass of one atom: 31.22moles x 1.88*10^25 = 565g/mol for Ti (rounding to 3 significant figures). However, this is still an empirical value; we don’t yet know what the exact mass of a Ti atom is. You can also calculate that there are about 4 atoms per unit cell in your, but again that’s an average. Ti(CO)is a simple cubic structure, but crystalline Ti metal is hcp, not fcc! So you have some mismatch there. You can also calculate the mass of one atom in hcp Ti (approximate to 3 significant figures), but again this is an empirical value. I hope these calculations help you understand what atomic masses are and how they are determined!

University of Oregon Chemical Engineering Education University of Oregon Chemical Engineering Education [ ARTICLE START ]

The volume of the cube is 6.93cm x 6.93cm x 6.93cm = 333cm3 By multiplying 333 by 4.50 we get the mass 1499.50g/cm3, which gives us the density is 1499.50g/cm3.g the molar mass of Ti (* 48g / mol) , calculate the moles of Ti: 1499.75 / 48 = 31.22 moles Multiply moles by 6.022*10 23 to calculate atoms: 32 * 6.022*10 23 = 2.042 * 10 24 Atoms If the formula is 6.02210*23 31.22molesa then a mole is equal to 1.88*10 25 atoms Please correct me if I am wrong .

University of Oregon Chemical Engineering Education University of Oregon Chemical Engineering Education [ ARTICLE END ]

That’s right! The formula is Ti (CO) or titanium (II carbonyl, and the number of atoms in a mole of Ti(CO)is 6.022*10^23, not 6.93*10^23. Now you can calculate the mass of one atom: 31.22moles x 1.88*10^25 = 565g/mol for Ti (rounding to 3 significant figures). However, this is still an empirical value; we don’t yet know what the exact mass of a Ti atom is. You can also calculate that there are about 4 atoms per unit cell in your, but again that’s an average. Ti(CO)is a simple cubic structure, but crystalline Ti metal is hcp, not fcc! So you have some mismatch there. You can also calculate the mass of one atom in hcp Ti (approximating to 3 significant figures), but again this is an empirical value. I hope these calculations help you understand what atomic masses are and how they are determined.

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