Describe how the ionization energies of main group elements vary across a period in the periodic table, using a diagram if necessary.

a, Write the equation for the first ionization of potassium

What are the major developments in Novel hybrid inorganic - organic polymer systems in the last 10 years?

A)   When 155 mL of water at 26 degrees Celsius is mixed with 25 mL of water at 85 degrees Celsius what is the final temperature? (Assume that no heat is released to the surroundings, d of water = 1.00 g/mL

B) Use twice the volume of each water sample. Calculate final temperature.

C) Instead of 75 mL, use 150 mL.  Calculate final temperature.

D) Instead of 75 mL, use 25 mL.  Calculate final temperature.

E) Discuss your results. How did the different volumes affect the final temperature?

A buffer is made from 3.7 ?? 10?1 M of HC2H3O2 and 2.9 ?? 10?1 M of NaC2H3O2

a. What is the pH?

b. If you added 3.0 ?? 10?3 moles of NaOH to 0.100 L of buffer what is the final pH. (assume that any change in volume is negligible.)

How long would it take to deposit 500 g of silver metal from a solution containing Ag+ ions using a current of 3.00 amperes? If the same time was spent depositing gold metal from a solution containing Au3+ ions using the same current, how much weight would of gold would be deposited? If you had 23 spoons that you wanted to coat with either silver or gold, and each spoon had a surface area of 150 mm2, how thick a coating could you make with each metal (for the same time spent in the electrolysis bath)? The density of silver is 10.5 g/mL and the density of gold is 19.3 g/mL.

3).The photosynthesis reaction is 6CO2 (g) + 6H2O (g) (Arrow) C6H12O6(s) + 6O2 (g). If the reaction requires 2.82 x 10^3 kJ/ mole of C6H12O6 formed: a.) How many grams of C6H12O6 can be produced from 4.20 x 10^4 kJ? b). How much energy is required to produced 250g of C6H12O6? c.)How many liters (at STP) of O2 are produced with 250g of C6H12O6? ͢͢͢͢͢

4.) Given the equation; N2 (g) + 3H2(g) (arrow) 2NH3(g). If 7.00L of N2 ( at STP) reacts with 15.0 L of H2, A.) How many L of NH3 is formed? B.) How many L of the excess gas remains unreacted? C.) How many grams of NH3 are formed?

2.) Place the following sets of elements in order of increasing size and give rational for answer . [Al, P, Na, Ar], [Ca, I , P, Br].

3.) Lead and Carbon are in the same column and therefore have the same electron configuration ending. Briefly explain why Carbon is a non metal and Lead is a metal.

One deciliter of a .9% nickel (II) nitrate solution is diluted to a volume of 500 mL. Calculate the final [NO3-] of the resultant solution. Answer in M please.

Consider the methanol(1) + ethanol(2) system at 101.325 kPa. Using Raoult's Law, predict the system temperature and vapor-phase composition for this mixture.

1) The data below apply to the formation of urea (NH2CONH2) from ammonium cyanate (NH4CNO). Initially, 22.9 grams of ammonium cyanate was dissolved in enough water to prepare 1.00 L solution. The reaction is NH4CNO----> NH2CONH2. Time (minutes) 0, 20.0, 50.0, 65.0, 150.0

Mass of urea formed (grams) 0, 7.0, 12.1,13.8, 17.7

From this data and using Excel, (a) determine the order of the reaction, (b) determine the rate constant (along with units), and (c) determine the mass of ammonium cyanate left after 300 minutes.

Discuss effects of structure and of the medium on the strengths of acids and bases. Use examples to illustrate your explanation.

You may have heard that ice skaters actually skate on a thin layer of water rather than solid ice (which reduces friction on the blade and allows them to skate faster). Let’s work through a calculation to determine if this statement is reasonable. Estimate the pressure exerted by a 200-lb hockey player, standing on two blades that are 0.1 mm x 20 cm. Calculate the melting point of ice below the player, assuming that the density of ice under these conditions is approximately 0.915 g cm^–3 and that of liquid water is 0.998 g cm^–3. Assuming a typical temperature of ice in a skating rink is 27 °F, does a hockey player skate on ice or water?

Write the half reaction for the anode and cathode for the following electrochemical cells. which metal acts as the anode and which acts as the cathode. For each cell, combine the half reactions and write the overall cell reaction.

a. Zn/Cu

b. Fe/Cu

c. Mg/Cu

d. Pb/Cu

e. Sn/Cu

A solution contains 8.28×10-3 M magnesium nitrate and 1.47×10-2 M calcium acetate. Solid ammonium fluoride is added slowly to this mixture. What is the concentration of calcium ion when magnesium ion begins to precipitate?

The volume of a sample of pure HCl gas was 277 mL at 20°C and 189 mmHg. It was completely dissolved in about 70 mL of water and titrated with an NaOH solution; 16.5 mL of the NaOH solution was required to neutralize the HCl. Calculate the molarity of the NaOH solution.