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(1) Describe the Rutherford's model of the atom and compare it with the model proposed by his student Niels Bohr.
(2) How many electrons are in the second energy level of an atom of each element?
a. chlorine
b. phosphorus
c. potassium
Calculate the wavelength of the light in nanometers corresponding to this transition. You can use the following values for your calculations: Planck's constant (h) = 6.626x10^-34 Jxs, speed of light (c) = 2.998x10^8 m/s, and 1m=10^9nm.
The atomic mass of boron is 10.81 g/mol. The two naturally occuring isotopes are B-10 with a mass of 10.0129 amu and B-11 with a mass of 11.0093 amu. Determine the percent of naturally occuring B-10.
A water sample is found to contain 23ppm iodine(I). If you drank 1399mL of this water, how many moles of Iodine(I) would you ingest
What is the pH of a solution that mixes 30mL of 0.01M CH3COOH with 30mL 0.0075M NaCH3CO2? (Assume the volumes are additive
Find the pH during the titration of 20.00 mL of .1000 M butanoic acid CH3CH2CH2COOH (kA = 1.54E-5), with .1000 M NaOh solution after the following additions of titrant. a. 20.40 mL b. 26.00 mL
Suppose you were instructed to add 38 g of sodium chloride (NaCl) to 100 mL of water. a. prepared as instructed at 20°C b. heated the mixture in (a) to 100°C. Describe what you would observe under the following conditions.
Which metal is associated with the synthesis of cyclopropanes?
If a raindrop weighs 53 mg on average and 5.1 105 raindrops fall on a lawn every minute, what mass (in kg) of rain falls on the lawn in 3.0 h.
Find the pH solution & Hydronium ion concentration and What is the pH of a solution of 0.17 M acid and 0.81 M of its conjugate base if the pKa = 8.62?
Give the systematic names for the formulas, or the formulas for the names. (using the format copper(II) chloride for CuCl2, and using the format CO2 for CO2. Omit the centered dot for hydrates.)
Carbon-14 is a radioactive isotope which decays with a half-life of 5730 years. What is the first-order rate constant for its decay, in units of years^-1
Calculate the maximum number of moles and grams of H2S that can form when 152 g aluminum sulfide reacts with 147 g water.
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