learned regarding periodic trends. DO NOT base your answer on tabulated values since exceptions may occur. | germanium smallest arsenic selenium bromine largest Feedback: Electronegativity is the ability of an atom in a molecule to attract electrons to itself. In general‚ electronegativity increases as the atomic radius decreases. Smaller atoms have higher electronegativities. Notice that all of these elements are in row 4. Across a row of the periodic table‚ atomic radius decreases
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Valence Electrons The valence electrons are the electrons in the last shell or energy level of an atom. They do show a repeating or periodic pattern. The valence electrons increase in number as you go across a period. Then when you start the new period‚ the number drops back down to one and starts increasing again. For example‚ when you go across the table from carbon to nitrogen to oxygen‚ the number of valence electrons increases from 4 to 5 to 6. As we go from fluorine to neon to sodium‚ the
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Name _________________________________________ Date _________________________ Period ____ Homework Chapter 7: Electronic Structure of Atoms Exercises: Sections 7.4‚ 7.5 : Ionization Energy and Electron Affinities 1. Write equations that show the process for (a) The first two ionization energies of gallium; first: Ga(g) → Ga+(g) + 1 e– second: Ga+(g) → Ga2+(g) + 1 e– (b) the fourth ionization energy of rhodium. fourth: Rh3+(g) → Rh4+(g) + 1 e–
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Sodium gives electrons when reacting with a substance such as Chloride instead of sharing electron in a reaction such as the Hydrogen and Oxygen forming water molecules can be found in the type of bond in each example reaction. Before I can identify the contrasting characteristics of each reaction‚ I must first acknowledge the reason atoms react with one another in the first place. Each element has a certain number of valence electrons‚ an example being Sodium having one valence electron. When elements
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Name: ______________________________________ Date: ________________________ Student Exploration: Covalent Bonds Vocabulary: covalent bond‚ diatomic molecule‚ Lewis diagram‚ molecule‚ noble gases‚ nonmetal‚ octet rule‚ shell‚ valence‚ valence electron Prior Knowledge Questions (Do these BEFORE using the Gizmo.) 1. There are eight markers in a full set‚ but Flora and Frank each only have seven markers. Flora is missing the red marker‚ and Frank is missing the blue marker. What
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Chapter 9 – Electrons in Atoms and the Periodic Table True/False Questions 1) When the elements are arranged in order of increasing number of protons‚ certain sets of properties recur periodically. 5) A particle of light is called a packet. 9) Ultraviolet light produces suntans and sunburns. 13) Electrons behave like particles and we can describe their exact paths. 17) The ground state is when an electron in an atom is excited into the lowest possible vacant orbital. 21) Bromine has 17 valence electrons
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03.04 Valence Electrons and Bonding Individual neutral atoms are rarely found in nature. The noble gases are the only elements that are found as single atoms more often than they are found in compounds. Atoms are held together in compounds by electrostatic attraction between positive nuclei and negative electrons. This attraction holds atoms together in a chemical bond‚ a link between two atoms resulting from the mutual attraction of their nuclei for valence electrons. All chemical bonds involve
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Energy and Electron Affinity Ionization Energy is removing an electron Electron Affinity is adding an electron Ionization Energy • Energy required to remove an electron from a ground state atom Ionization Energy of Noble Gases • Noble gases have full orbitals‚ so it is difficult to remove an electron from them. But‚ it does become easier the further away the electrons get from the nucleus. Ionization Energy of Alkali Metals • Alkali Metals only have one valence electron‚ so it does
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VALENCE BOND THEORY The ‘mixing’ or ‘blending’ of atomic orbitals to accommodate the spatial requirements in a molecule is known as hybridization. Hybridization occurs to minimize electron pair repulsions when atoms are brought together to form molecules. Possible hybridization schemes: 2nd row elements: sp sp2 sp3 3rd row elements also have: dsp3 d2sp3 Each of these hybridzation schemes corresponds to one of the five fundamental VSEPR geometries. Bonding arises from the overlap
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FREE ELECTRON THEORY Classical free electron theory of metals This theory was developed by Drude and Lorentz and hence is also known as Drude-Lorentz theory. According to this theory‚ a metal consists of electrons which are free to move about in the crystal like molecules of a gas in a container. Mutual repulsion between electrons is ignored and hence potential energy is taken as zero. Therefore the total energy of the electron is equal to its kinetic energy. Drift velocity If no electric
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