F F Kr F Se in C#.NET

Scanning DataMatrix in C#.NET F F Kr F Se

F F Kr F Se
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KrF2: two bonding pairs and three nonbonding pairs
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SeF2: two bonding pairs and two nonbonding pairs
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SnF2: ionic
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The Lewis structure indicates that KrF2 is nonpolar Thus, it only has very weak London dispersion forces between the molecules SeF2 is polar and the molecules are attracted by dipole dipole attractions, which are stronger than London SnF2 has the highest melting point, because of the presence of strong ionic bonds You get 1 point for the order, and 1 point for the discussion c The following resonance structures may be drawn for the oxalate ion The presence of resonance equalizes the bonds
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2 You get 1 point for any correct Lewis structure for C2O4 ,and 1 point for showing or discussing resonance
d PCl5 must ionize There are two acceptable equations 2 PCl 5
PCl 4 + + PCl 6 or PCl 5
PCl 4 + + Cl
You get 1 point for the explanation, and you get 1 point for either of the equations Total your points for the different parts There are 10 points possible
U Rapid Review
Compounds are pure substances that have a fixed proportion of elements Metals react with nonmetals to form ionic bonds, and nonmetals react with other nonmetals to form covalent bonds The Lewis electron-dot structure is a way of representing an element and its valence electrons Atoms tend to lose, gain, or share electrons to achieve the same electronic configuration (become isoelectronic to) as the nearest noble gas Atoms are generally most stable when they have a complete octet (eight electrons) Ionic bonds result when a metal loses electrons to form cations and a nonmetal gains those electrons to form an anion
Bonding 165
Ionic bonds can also result from the interaction of polyatomic ions The attraction of the opposite charges (anions and cations) forms the ionic bond The crisscross rule can help determine the formula of an ionic compound In covalent bonding two atoms share one or more electron pairs If the electrons are shared equally, the bond is a nonpolar covalent bond, but unequal sharing results in a polar covalent bond The element that will have the greatest attraction for a bonding pair of electrons is related to its electronegativity Electronegativity values increase from left to right on the periodic table and decrease from top to bottom The N A = S rule can be used to help draw the Lewis structure of a molecule Molecular geometry, the arrangement of atoms in three-dimensional space, can be predicted using the VSEPR theory This theory says the electron pairs around a central atom will try to get as far as possible from each other to minimize the repulsive forces In using the VSEPR theory, first determine the electron-group geometry, then the molecular geometry The valence bond theory describes covalent bonding as the overlap of atomic orbitals to form a new kind of orbital, a hybrid orbital The number of hybrid orbitals is the same as the number of atomic orbitals that were mixed together There are a number of different types of hybrid orbital, such as sp, sp2, and sp3 In the valence bond theory, sigma bonds overlap on a line drawn between the two nuclei, while pi bonds result from the overlap of atomic orbitals above and below a line connecting the two atomic nuclei A double or triple bond is always composed of one sigma bond and the rest pi In the molecular orbital (MO) theory of covalent bonding, atomic orbitals form molecular orbitals that encompass the entire molecule The MO theory uses bonding and antibonding molecular orbitals The bond order is (# electrons in bonding MOs # electrons in anti-bonding MOs)/2 Resonance occurs when more than one Lewis structure can be written for a molecule The actual structure of the molecule is an average of the Lewis resonance structures The higher the bond order, the shorter and stronger the bond Paramagnetism, the attraction of a molecule to a magnetic field, is due to the presence of unpaired electrons Diamagnetism, the repulsion of a molecule from a magnetic field, is due to the presence of paired electrons
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