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    CATIONS and ANIONS

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    cation has fewer electrons than protons. Anions are negatively charged ions. An anion has more electron than protons. The nature and magnitude of charge on ion depend on the position of an element in the periodic table. In forming an ion‚ an atom of a main group element loses gains electrons to obtain the electronic configuration of the noble gas closest to it in the periodic table. This gives the ion on especially stable electronic arrangement with a completely filled shell of electrons; that is‚ the

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    Chem 201 /HW#10 Chapter 9 Electronegativity Table: use this table to answer Q [pic] 1. Bromine tends to form a monatomic ion which has the electronic configuration of a noble gas. What is the electron configuration of that noble gas? a. 1s2 2s2 2p6 3s2 3p6 3d10 4p6 b. 1s2 2s2 2p6 3s2 3p6 4p6 4d10 c. 1s2 2s2 2p6 3s2 3p6 4s2 4p6 d. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 e. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 2. Which ion of

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    Research Paper On Copper

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    conductor of heat and electricity. Since copper is a very good conductor of electricity‚ a lot of electrical wires are made out of copper. This helps easily transfer electricity. Electrons move candidly in copper because they are ready to bond with another atom to form an stable octet. An octet is eight valence electrons in the outer energy level. Having eight in the outer energy level will make the ion stable. Copper has a germicidal effect meaning that many germs are neutralized by it. This is why

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    (n–1) d and ns orbitals and (b) extra stability of half filled and completely filled orbitals in case of Cr and Cu in 3d series. Cr : Is 2 2s2 2p6‚ 3s2 3p6 4s1 3d5 Cu : Is2 2s2 2p6‚ 3s2 3p6 4s1 3d10 To write the electronic configuration of Mn+‚ the electrons are first removed from ns orbital and then from (n - 1) d orbitals of neutral‚ atom (if required). For example‚ the electronic configuration of Cu+‚ Cu2+ and Cr3+ are respectively 3d10 4s°‚ 3d9 4s° and 3d3 4s°. m o .c y a d with the help of above

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    the terminal ones. In the transparency‚ why are the hydrogen (H) atoms in hydrazine (N2H4) shown as the terminal atoms? 2. Step 2 in drawing a Lewis structure involves determining the total number of valence electrons in the atoms in the molecule. Explain why the total number of valence electrons in N2H4 is 14. 3. Step 3 in drawing a Lewis structure requires finding the number of bonding pairs. What must be done to the result of step 2 to find the number of bonding pairs? Verify that this is

    Free Atom VSEPR theory Chemical bond

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    Vsepr Theory

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    01.23.13 NAS102 CODE13873 VSEPR Theory VSEPR (Valence Shell Electron Pair Repulsion) theory proposes that the geometric arrangement of terminal atoms‚ or groups of atoms about a central atom in a covalent compound‚ or charged ion‚ is determined solely by the repulsions between electron pairs present in the valence shell of the central atom. The number of electron pairs around the central atom can be determined by writing the Lewis structure for the molecule

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    Vsepr Lab

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    Six-Balloon Set Octahedral B. Valence Shell Pairs: Single Bonds Fill in the table below for the corresponding compounds. Reference the tables provided in the introductory comments for Lab #16 VSEPR Theory. Molecular Shape Number of Bonds About Central Atom Shape Description BF3 3 Trigonal planar BeCl2 2 Linear CH4 4 Tetrahedral PF5 5 Trigonal bipyramidal SF6 6 Octahedral C. Valence Shell Pairs: Single Bonds and Non-Bonding electron pairs Fill in the table below

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    Bdaaaaa

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    element with a different colored candy. Each toothpick represents two electrons. A toothpick between two atoms represents a single bond‚ two toothpicks between two atoms represent a double bond‚ and three toothpicks between two atoms represent a triple bond. Remember that the lone pairs on the central atom take up space and play a role in determining the shape of the molecule. Represent each lone pair (nonbonded pairs of valence electrons) on the central atom with a nonbonded toothpick. The bonds and lone

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    gases are not reactive has to do with the outermost electron shells. Halogens are reactive because they only have seven electrons in their outermost shell and can gain another by reacting with atoms of other elements. A few examples of halogens are: fluorine‚ chlorine‚ bromine‚ iodine‚ and astatine. On the other hand alkali metals are extremely reactive because instead of gaining another electron like the halogens‚ alkali metals lose one or two electrons. Some examples of alkali metals are: lithium‚ sodium

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    Electron

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    Electromagnetic Spectrum Project Introduction: In this project you work for a company that produces and sells electromagnetic waves (Waves-R-Us). Your job is to do extensive research on the company’s products and then to design a catalog that will persuade customers to buy our product. You will also need to inform customers of the dangers of our waves.   Task:  You must design a catalog that will persuade the customers of Waves-R-Us to buy your products. Your catalog must have 1 page for each

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