1A H 2A Li Be Na Mg 3B 4B 5B 68 7888 3A 4A 5A 6A 7A He BCN OF Ne S Cl Ar 1B 2B Al K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga ** Fr Ra Ac Rf Ha Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In 8A Si P Ge As Se Br Kr Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Write the complete electron configuration for the sodium atom. Using NOBLE GAS notation write the electron configuration for the beryllium atom.

1A H 2A Li Be Na Mg 3B 4B 5B 68 7888 3A 4A 5A 6A 7A He BCN OF Ne S Cl Ar 1B 2B Al K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga ** Fr Ra Ac Rf Ha Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In 8A Si P Ge As Se Br Kr Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Write the complete electron configuration for the sodium atom. Using NOBLE GAS notation write the electron configuration for the beryllium atom.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and e xplain the differences between the following terms. a. law and theory b. theory and...

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Define and e xplain the differences between the following terms. a. law and theory b. theory and experiment c. qualitative and quantitative d. hypothesis and theory
Copper atoms. (a) What is the average mass of one copper atom? (b) Students in a college computer science class once sued the college because they were asked to calculate the cost of one atom and could not do it. But you are in a chemistry course, and you can do this. (See E. Felsenthal, Wall Street Journal, May 9, 1995.) If the cost of 2.0-mm diameter copper wire (99.9995% pure] is currently 41.70 for 7.0 g, what is the cost of one copper atom?
You take three compounds, each consisting of two elements (X, Y. and/or Z), and decompose them to their respective elements. To determine the relative masses of X, Y. and Z. you collect and weigh the elements, obtaining the following data: Elements in Compound Masses of Elements 1. X and Y X = 0.4 g, Y = 4.2 g 2. Y and Z Y = 1.4 g, Z = 1.0 g 3. X and Y X = 2.0 g, Y = 7.0 g a. What are the assumptions needed to solve this problem? b. What are the relative masses of X, Y. and Z? c. What are the chemical formulas of the three compounds? d. If you decompose 21 g of compound XY, how much of each element is present?
The early alchemists used to do an experiment in which water was boiled for several days in a sealed glass container. Eventually. some solid residue would appear in die bottom of the flask, which was interpreted to mean that some of the water in the flask had been converted into earth. When Lavoisier repeated this experiment, he found that the water weighed the same before and after heating, and the mass of die flask plus the solid residue equaled the original mass of the flask. Were the alchemists correct? Explain what really happened. (This experiment is described in the article by A. F. Scott in Scientific American, January 1984.)
In 1886 Eugene Goldstein observed positively charged particles moving in the opposite direction to electrons in a cathode ray tube (illustrated below). From their mass, he concluded that these particles were formed from residual gas in the tube. For example, if the cathode ray tube contained helium, the canal rays consisted of He+ ions. Describe a process that could lead to these ions. Canal rays. In 1886, Eugene Goldstein detected a stream of particles traveling in the direction opposite to that of the negatively charged cathode rays (electrons). He called this stream of positive particles "canal rays:"
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?
Fill in the missing information in the following table.
An element X bas five major isotopes, which are listed below along with their abundances. What is the element? Isotope Percent Natural Abundance Mass (u) 46x 8.00% 45.95232 47x 7.30% 46.951764 48x 73.80% 47.947947 49x 5.50% 48.947841 50x 5.40% 49.944792
Indium oxide contains 4.784 g of indium for every 1.000 g of oxygen. In 1869, when Mendeleev first presented his version of the periodic table, he proposed the formula ln2O3 for indium oxide. Before that time it was thought that the formula was InO. What values for the atomic mass of indium are obtained using these two formulas? Assume that oxygen has an atomic mass of 16.00.