Compound NaF CaO BaO in Visual C#

Scanner Data Matrix in Visual C# Compound NaF CaO BaO

Compound NaF CaO BaO
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Ionic radius of cation (pm) 116 114 149
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Ionic radius of anion (pm) 119 126 126
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Lattice energy (kJ/mole) 911 3566 3202
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U Answers and Explanations
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Notice that all the answers are very short Do not try to fill all the space provided on the exam You score points by saying specific things, not by the bulk of material The graders look for certain keywords or phrases The answers should not contain statements that contradict each other
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2+ 3+ a The observed trend of radii is: Fe > Fe > Fe There is an increase in the effective nuclear charge in this series As electrons are removed, the repulsion between the electrons decreases The larger the effective nuclear charge, the more the electrons are pulled towards the nucleus and the smaller the atom or ion becomes Give yourself 1 point for effective nuclear charge, and 1 point for explaining the effective nuclear charge discussion
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b When moving across a period on the periodic table, the value of the effective nuclear charge increases with atomic number This causes a general increase from Li to Be to B This effective nuclear charge argument is worth 1 point The even higher value of Be (greater than B) is due to the increased stability of the electron configuration of Be Beryllium has a filled s-subshell Filled subshells have an increased stability, and additional energy is required to pull an electron away Give yourself 1 point for the filled subshell discussion c The effective nuclear charge in F is greater than the effective nuclear charge in O This causes a greater attraction of the electrons You get 1 point for this answer d Because all the solids adopt the same structure, the structure is irrelevant The sizes of the anions are similar; thus, anion size arguments are not important Two factors, other than structure, are important here The two compounds with the highest lattice energies contain divalent ions (+2 or 2) while NaF contains
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Basics 65
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univalent ions (+1 or 1) The higher the charge is, the greater the attraction between the ions is The lattice energy increases as the attraction increases You get 1 point for correctly discussing the charges The difference between the CaO and BaO values is because the larger the ion is, the lower the attraction is (greater separation) The lower attraction leads to a lower lattice energy This size argument will get you 1 point Total your points The maximum is 7
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U Rapid Review
Here is a brief review of the most important points in the chapter If something sounds unfamiliar, study it in the chapter and your textbook
Know the metric measurement system and some metric/English conversions Know how to convert from any one of the Fahrenheit/Celsius/Kelvin temperature scales to the other two The density of a substance is mass per unit volume Know how to determine the number of significant figures in a number, the rules for how many significant figures are to be shown in the final answer, and the round-off rules Know how to set up problems using the factor label method Know the differences between a solid, a liquid, and a gas at both the macroscopic and microscopic levels Know what part Dalton, Thompson, Millikan, and Rutherford had in the development of the atomic model Know the three basic subatomic particles proton, neutron, and electron their symbols, mass in amu, and their location Isotopes are atoms of the same element that have differing numbers of neutrons Electrons are located in major energy levels called shells Shells are divided into subshells, and there are orbitals for each subshell Know the electron capacity of each orbital (always 2) Be able to write both the energy-level diagram and the electronic configuration of an atom or ion by applying both the Aufbau build-up principle and Hund s rule Know how the modern periodic table was developed, including the differences between Mendeleev s table and the current table Periods are the horizontal rows on the periodic table; the elements have properties unlike the other members of the period Groups or families are the vertical rows on the periodic table; the elements have similar properties Know the properties of metals, nonmetals, and metalloids and which elements on the periodic table belong to each group Valence electrons are outer-shell electrons
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