(a) Three spheres of equal size are composed of aluminum1density = 2.70 g>cm32, silver 1density = 10.49 g>cm32,and nickel 1density = 8.90 g>cm32. List the spheres fromlightest to heaviest. (b) Three cubes of equal mass arecomposed of gold 1density = 19.32 g>cm32, plat inum1density = 21.45 g>cm32, and lead 1density = 11.35 g>cm32.List the cubes from smallest to largest. [Section 1.5]

As you move down a family (group) of the periodic table the size of atoms increases from period 2 to period 3 by about 30-40 pm.  For example, the radius of B is 84 pm and the radius of Al is 121 pm.  However, as you move from aluminum (radius of 121 pm) to gallium (radius of 122 pm) the radius only increases by 1 pm.  Which of the following explains this small increase in radius from Al to Ga? Select one: a. the scandide contraction b. the lanthanide contraction c. the mercurate elongation d. the zincate elongation e. Aluminum is just larger than you might expect.

A sample of a gaseous binary compound of boron and chlorine weighing 2.842 g occupies 0.153 L. This sample is decomposed to give 0.664 g solid boron and enough gaseous chlorine (Cl2) to occupy 0.688 L at the same temperature and pressure. Determine the number of atoms of boron and the number of atoms of chlorine in a molecule of this compound.

Determine the mass (in grams) of exactly 100 millionatoms of fluorine if the relative atomic mass of fluorine is18.998403 on a scale on which exactly 12 is the relativeatomic mass of 12C.

2.) Suppose you're attempting to measure the density of a liquid that is highly volatile (it evaporates quickly). If you first measure the volume and then several minutes later you measure the mass of the liquid will the measured density be higher than the true value, lower than the true value, or the true density of the liquid. [It helps to understand this problem with the density equation.]

How much does 60.2 L of Al(NO3)3 weigh in grams?

6 A compound of iodine and cesium contains 74.85 g of metal and 61.30 g of nonmetal. How many grams of cesium are in 34.88 g of compound?

(a) You are given a cube of silver metal that measures 1.000cm on each edge. The density of silver is 10.5 g/cm3. Howmany atoms are in this cube? (b) Because atoms are spherical,they cannot occupy all of the space of the cube. Thesilver atoms pack in the solid in such a way that 74% of thevolume of the solid is actually filled with the silver atoms.Calculate the volume of a single silver atom. (c) Using thevolume of a silver atom and the formula for the volume of asphere, calculate the radius in angstroms of a silver atom

A one carat diamond which is made of the element carbon, weighs 0.200 grams. The average mass of a carbon atom is 12.0 atomic mass units(Amu). If 1 amu= 1.661*10^-24 grams, how many carbon atoms are present in a one carat diamond?

Although carbon-12 is now used as the standard for atomic weights, this has not always been the case. Early attempts at classification used hydrogen as the standard, with the weight of hydrogen being set equal to 1.0000. Later attempts defined atomic weights using oxygen (with a weight of 16.0000 ). In each instance, the atomic weights of the other elements were defined relative to these masses. (To answer this question, you need more precise data on current atomic weights: H,1.00794 u; O, 15.9994 u.) (a) If H=1.0000 u was used as a standard for atomic weights, what would the atomic weight of oxygen be? What would be the value of Avogadro's number under these circumstances?(b) Assuming the standard is O=16.0000 u, determine the value for the atomic weight of hydrogen and the value of Avogadro's number.