Name____________________________________________Period_________Date__________________ The Nuts and Bolts of Chemistry Atoms of different elements combine in simple, whole number ratios to form chemical compounds. The same two elements may combine in different ratios to form various compounds. We will use nuts and bolts to practice the math involved in this chemical concept. I. Determine the following masses: a. Mass of bolt (Bt) = __________ d. Mass of BtNt2 = ___________ b. Mass of nut (Nt) = __________ e. Mass of Bt2Nt = __________ c. Mass of BtNt = __________ II. Compose your own compound and record its mass: f. Mass of BtxNty = __________ Your compound ____________ III. Find the % Bt and % Nt for each of the compounds. BtNt BtNt2 Bt2Nt BtxNty % Bt % Nt IV. Calculate the empirical formula for each of the compounds by taking the % of one element and dividing it by the mass of that element. Repeat this calculation with the other element. Divide the smallest of the two resulting numbers into the larger number. The resulting ratio is the empirical formula. BtNt BtNt2 Bt2Nt BtxNty Empirical formula V. Questions a. Using your measured masses, calculate the composition of Bt2Nt2. Compare it with the % composition of BtNt. assuming you can’t see the true combination of bolts and nuts what information could you use to determine what your compound was? b. Obtain the % composition of BtxNty from another lab group. Calculate the empirical formula of their compound and see if it agrees. c. Determine the empirical formula for the following compounds: i. H = 6.0%, S = 94.0% ii. Na = 21.7%, Cl = 33%, O = 45% d. What is the empirical formula for 2.3g of Na, 1.2g of C, and 1.6g of O?