The last valence electron in Br is 4p5. What are the quantum numbers for this electron. n is _______ l is  _______ ml is _______ and ms is _______

A 35.0 g sample of nickel metal is heated to 100.°C and dropped into 100.0 g of water, initially at 22.0°C. Assuming that all of the heat lost by the nickel is absorbed by the water, calculate the final temperature of the nickel and the water. The specific heat of nickel is 0.444J/g°C)

Calculate the energy of light emitted when the following transition occurs in a hydrogen atom: n=6 to n=3 Enter your value as a positive.

Given the following data: 2C2H2(g) + 5 O2(g) –> 4CO2(g) + 2H2O(l)      ΔH= -2600.kJ CO2(g) –> C(s) + O2(g)                                  ΔH= 394kJ 2H2(g) + O2(g) –> 2H2O(l)                                 ΔH= -572kJ Use Hess’s Law to calculate ΔH for the reaction 2C(s) + H2(g) –> C2H2(g)

In a well insulated container, 50.0 g of water at 5.0 degrees celsius is added to 350 g of water at 32.0 degrees celsius. What is the final temperature when the ice mixture reaches equilibrium?

The specific heat capacities of three metals are given below. Metal Fe Pb Zn Specific Heat, j/g°C 0.470 0.130 0.388 If 1.00 gram of each metal is heated to 100 degrees celsius and added to 10 grams of water at 25 degrees celsius, what is the order of the temperatures of the final mixtures from the lowest to the highest?

Consider the reaction: B2H6(g) + 3O2(g) –>B2O3(s) + 3H2O(g)             ΔH = -2035 kJ Calculate the amount of heat released when each of the following amounts of diborane (B2H6) is burned A mixture of 20.0 g B2H6 and 10.0 g O2

Nitrogen has a greater first ionization energy than oxygen. What is the best explanation for this observation?

Calculate the energy released by the reaction 4Fe(s) + 3O2(g) –> 2Fe2O3 when a 55.8 gram sample of iron reacts completely with 1.00 mol of oxygen. The enthalpy of formation (ΔH°f) of Fe2O3 (s) is -826 kj/mol.

Given the enthalpy changes: A +B –> C ΔH= -35 kj/mol A + D –> E + F ΔH= 20 kj/mol F –> C + E ΔH= 15 kj/mol