Calculate M+ (using the lower mass number isotope of the halogen) and M+2 (using the higher mass number isotope of the halogen) for each of the molecular formulas given below. 1. C3H5Br 2. C6H5Cl 3. C2H3O2Cl 4. C3H4NBr

Lithium, Li, reacts with element X to form an ionic compound with the formula Li2X. a What is the formula of the compound you expect to form when aluminum, Al, reacts with element X? b Would you expect this compound to be ionic or molecular?

Atmospheric argon is a mixture of three stable isotopes. 36Ar. 38Ar, and 40Ar. Use the information in the table below to determine the atomic mass and natural abundance of 40Ar.

When mixtures of gaseous H2 and gaseous Cl2 react, a product forms that has the same properties regardless of the relative amounts of H2 and Cl2 used. a. How is this result interpreted in terms of the law of definite proportion? b. When a volume of H2 reacts with an equal volume of Cl2 at the same temperature and pressure, what volume of product having the formula HCI is formed?

Two samples of different compounds of sulfur and oxygen have the following compositions. Show that the compounds follow the law of multiple proportions. What is the ratio of oxygen in the two compounds for a fixed amount of sulfur? Amount S Amount O Compound A l.210g 1.811 g Compound B 1.783 g 1.779 g

Calculate the atomic mass of each of the following elements using the given data for the percentage abundance and mass of each isotope. a. Silver: 51.82% 107Ag (106.9 amu) and 48.18% 109Ag (108.9 amu) b. Silicon: 92.21% 28Si (27.98 amu), 4.70% 29Si (28.98 amu), and 3.09% 30Si (29.97 amu)

Reference Section 5-2 to find the atomic masses of 12C and 13C, the relative abundance of 12C and 13C in natural carbon, and the average mass (in u) of a carbon atom. If you had a sample of natural carbon containing exactly 10,000 atoms, determine the number of 12C and 13C atoms present. What would be the average mass (in u) and the total mass (in u) of the carbon atoms in this 10,000-atom sample? If you had a sample of natural carbon containing 6.0221 1023 atoms, determine the number of 12C and 13C atoms present What would be the average mass (in u) and the total mass (in u) of this 6.0221 1023 atom sample? Given that 1 g = 6.0221 1023 u, what is the total mass of I mole of natural carbon in units of grams?

Determine whether the statements given below are true or false. (a) The mass of an atom can have the unit mole. (b) In N204, the mass of the oxygen is twice that of the nitrogen. (c) One mole of chlorine atoms has a mass of 35.45 g. (d) Boron has an average atomic mass of 10.81 amu. It has two isotopes, B-10 (10.01 amu) and B-11 (11.01 amu). There is more naturally occurring B-10 than B-11. (e) The compound C6H12O2N has for its simplest formula C3H6ON1/2. (f) A 558.5-g sample of iron contains ten times as many atoms as 0.5200 g of chromium. (g) If 1.00 mol of ammonia is mixed with 1.00 mol of oxygen the following reaction occurs, 4NH3(g)+5O2(g)4NO(g)+6H2O(l)All the oxygen is consumed. (h) When balancing an equation, the total number of moles of reactant molecules must equal the total number of moles of product molecules.

For the following processes that show the formation of ions, use the periodic table to indicate the number of electrons and protons present in both theionand theneutral atomfrom which the ion is made. a.CaCa2++2e b.P+3eP3 c.Br+eBr d.FeEe3++3e e.AlAl3++3e f.N+3eN3

For each of the negative ions listed in column 1, use the periodic table to find in column 2 the total number of electrons the ioncontains. A given answer may be used more than once. Column 1 Column 2 [ 1] Se2 [a] 18 [ 21 S2 [b] 35 [ 31 P3 [c] 52 [ 4] O2 [d] 34 [ 5] N3 [e]36 [6] I [f] 54 [7] F [g] 10 [8] Cl [h]9 [9] Br [i] 53 [101 At [j] 86