pls help q(A) and (D) Table 1: Cubic Unit Cell SystemSimpleBodyFaceDescription of table entryCubicCenteredCentered(1) # of corner atoms in one unit cell88.(2) Fraction of a single corner atom inside one unit cell 1/81/81/8Total # of 'equivalent corner atoms inside one unit cellHint: multiple (1) x (2)(3) # of atoms in the center (body) of one unit cell 011.11(4) Fraction of a single body atom inside one unit cell1.Total # of 'equivalent body atoms inside one unit cell1Hint: multiple (3) x (4)(5) # of atoms in all faces of one unit cell6(6) Fraction of each face atom inside one unit cellTotal # of 'equivalent face atoms inside one unit cell.Hint: multiple (5) x (6)1/23a) Find the total # of 'equivalent atoms in each unit cell (sum1.24equivalent # of corner, body, and face atoms)b) Coordination number for an atom in this unit cell6.812c) Along which length do atoms touch in this unit cell, a, c or d?lad.d) Express the above length in terms of atomic radius, 'T'Keep 'r' as a variable in your answer (e.g., '2r')a= 2rd=4rc=4re) Use the answer above to find the unit cell edge length, a in terms ofTr'. Round to 3 sig figs & keep 'r' as a variable, e.g. "3.14r". Show2.00r2.31r2.83ryourworkf) Using the answer above for 'a', determine the unit cell volume (a®) in 8.00r^312.3г^322.6r^3terms of atomic radius, 'r³'. Round your answer to 3 sig figs andkeep 'r' as a variable. Showyour .work Sketch one 'face' of a unit cell for SC, FCC and BCC. A total of 3 sketches are required forthis question.Calculate the percent empty space in each of the unit cells, SC, BCC and FCC. This is the ratioof space filled by atoms inside the unit cell to the total volume of the unit cell, given as a percentage.Remember that the volume of a sphere with radius, r, is tr³.А.В.(volume of unit cell – volume of atoms inside unit cell)volume of unit cell% Empty spacex 100%a) Calculate the volume of ONE unit cell, keep the 'r' term in your result.b) Calculate the volume of all atoms inside ONE unit cell, again keep the 'r term in your result.c) Use the equation above and your previous two answers to calculate the % empty space in theunit cell. You should find the r' terms cancel! Simplify and report your answer to 3 sig. figs.С.Density is an intensive property, meaning any sample size will give the same value. Hence,even a sample as small as a unit cell can be used to determine a substance's density:mass of atoms inside unit cell (in grams)volume of the unit cell, a³ (in cm³)density (using unit cell)Using the density formula above, calculate the density (in g/cm³) for each of the three crystalstructures (SC, FcC, & BCC) when they contain atoms with a mass of 105.00 amu and a radius of0.125 nm.For each unit cell type, label and show how a calculation for the mass of the unit cell, thevolume of the unit cell and the density of the unit cell.Show all necessary work, including units for each numeric value used in these calculations!HINT: Be careful with your unit conversions.if your density values are not between 0.5 and30 g/cm?, you've likely made a unit conversion error.Which one of the three types of cubic unit cells (SC, BCC, FCC) corresponds to what is called"cubic closest packing"? Use two pieces of evidence from Table 1 and the previous questions toexplain and support your selection. (just listing them is not an explanation and earns no points)

Question

pls help q(A) and (D) Table 1: Cubic Unit Cell SystemSimpleBodyFaceDescription of table entryCubicCenteredCentered(1) # of corner atoms in one unit cell88.(2) Fraction of a single corner atom inside one unit cell 1/81/81/8Total # of 'equivalent corner atoms inside one unit cellHint: multiple (1) x (2)(3) # of atoms in the center (body) of one unit cell 011.11(4) Fraction of a single body atom inside one unit cell1.Total # of 'equivalent body atoms inside one unit cell1Hint: multiple (3) x (4)(5) # of atoms in all faces of one unit cell6(6) Fraction of each face atom inside one unit cellTotal # of 'equivalent face atoms inside one unit cell.Hint: multiple (5) x (6)1/23a) Find the total # of 'equivalent atoms in each unit cell (sum1.24equivalent # of corner, body, and face atoms)b) Coordination number for an atom in this unit cell6.812c) Along which length do atoms touch in this unit cell, a, c or d?lad.d) Express the above length in terms of atomic radius, 'T'Keep 'r' as a variable in your answer (e.g., '2r')a= 2rd=4rc=4re) Use the answer above to find the unit cell edge length, a in terms ofTr'. Round to 3 sig figs & keep 'r' as a variable, e.g. &#34;3.14r&#34;. Show2.00r2.31r2.83ryourworkf) Using the answer above for 'a', determine the unit cell volume (a®) in 8.00r^312.3г^322.6r^3terms of atomic radius, 'r³'. Round your answer to 3 sig figs andkeep 'r' as a variable. Showyour .work Sketch one 'face' of a unit cell for SC, FCC and BCC. A total of 3 sketches are required forthis question.Calculate the percent empty space in each of the unit cells, SC, BCC and FCC. This is the ratioof space filled by atoms inside the unit cell to the total volume of the unit cell, given as a percentage.Remember that the volume of a sphere with radius, r, is tr³.А.В.(volume of unit cell – volume of atoms inside unit cell)volume of unit cell% Empty spacex 100%a) Calculate the volume of ONE unit cell, keep the 'r' term in your result.b) Calculate the volume of all atoms inside ONE unit cell, again keep the 'r term in your result.c) Use the equation above and your previous two answers to calculate the % empty space in theunit cell. You should find the r' terms cancel! Simplify and report your answer to 3 sig. figs.С.Density is an intensive property, meaning any sample size will give the same value. Hence,even a sample as small as a unit cell can be used to determine a substance's density:mass of atoms inside unit cell (in grams)volume of the unit cell, a³ (in cm³)density (using unit cell)Using the density formula above, calculate the density (in g/cm³) for each of the three crystalstructures (SC, FcC, & BCC) when they contain atoms with a mass of 105.00 amu and a radius of0.125 nm.For each unit cell type, label and show how a calculation for the mass of the unit cell, thevolume of the unit cell and the density of the unit cell.Show all necessary work, including units for each numeric value used in these calculations!HINT: Be careful with your unit conversions.if your density values are not between 0.5 and30 g/cm?, you've likely made a unit conversion error.Which one of the three types of cubic unit cells (SC, BCC, FCC) corresponds to what is called&#34;cubic closest packing&#34;? Use two pieces of evidence from Table 1 and the previous questions toexplain and support your selection. (just listing them is not an explanation and earns no points)

Accepted Answer

The SC unit cell is shown below.

The FCC unit cell is shown below.

The BCC unit cell is shown…