Oakland Schools Chemistry Resource Unit Intermolecular Forces Brook R. Kirouac David A. Consiglio‚ Jr. Southfield‐Lathrup High School Southfield Public Schools Bonding: Intermolecular Forces Content Statements: C2.2: Chemical Potential Energy Potential energy is stored whenever work must be done to change the distance between two objects. The attraction between the two objects may be gravitational‚ electrostatic‚ magnetic‚ or strong force. Chemical potential energy is the result
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are the covalent bonds and ionic bonds. Covalent bonds are bonds in which one or more pairs of electrons are shared by two atoms. Covalent bonds‚ in which the sharing of the electron pair is unequal‚ with the electrons spending more time around the more non-metallic atom‚ are called polar covalent bonds. In such a bond there is a charge separation with one atom being slightly more positive and the other more negative‚ i.e.‚ the bond will produce a dipole moment. On the other hand‚ Ionic bonds are
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classified as metals. The following are examples of heteronuclear diatomic molecules with ionic bonding: Let us take NaCl‚ for example‚ sodium (Na) is on the far left side of the periodic table‚ indicating it is a metal‚ and chlorine (Cl) is a nonmetal‚ so NaCl is a heteronuclear diatomic molecule with an ionic bond. The following are examples of heteronuclear diatomic molecules with covalent bonding: Let us look at HBr‚ for example. Hydrogen is on the left side of the stairs that divide
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Lesson 03.01: History of the Periodic Table Explain how scientific observations led to the development of‚ and changes to‚ the periodic table. Russian chemist Dmitri Mendeleev set out to organize the 63 known elements according to their properties. Mendeleev wrote the name‚ mass‚ and chemical properties of each element on a separate card and arranged the cards by various properties‚ looking for trends and patterns. When he arranged the elements by increasing atomic mass‚ Mendeleev noticed that similar
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elements are in their highest oxidation states. In these oxides‚ all the outer electrons in the Period 3 element are being involved in the bonding - from just the one with sodium‚ to all seven of chlorine’s outer electrons. The structures The trend in structure is from the metallic oxides containing giant structures of ions on the left of the period via a giant covalent oxide (silicon dioxide) in the middle to molecular oxides on the right. Melting and boiling points The giant structures (the metal oxides
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Chemistry Summary The particle theory: 1. Matter is made of tiny particles 2. Particles of matter are in constant motion 3. Particles of matter are held together by very strong electric forces 4. There are empty spaces between the particles of matter that are very large compared to the particles themselves. 5. Each substance has unique particles that are different from the particles of other substances 6. Temperature affects the speed of the particles. The
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all of these behaviors merge into each other seamlessly in various bonding situations so that there is no clear line to be drawn between them‚ nevertheless behaviors of atoms become so qualitatively different as the character of the bond changes quantitatively‚ that it remains useful and customary to differentiate between the bonds that cause these different properties of condensed matter. In the simplest view of a so-called ’covalent’ bond‚ one or more electrons (often a pair
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Diatomic elements (ogens or ines) H2‚ N2‚ O2‚ F2‚ Cl2‚ Br2 (liquid)‚ I2 (solid)‚ At2 Common valencies: NH4 (Ammonium) 1+ Zn 2+ NO3 1 OH 1 CO3 2 SO4 2 PO4 (phosphate) 3 Combustion reaction: compound + oxidant → heat + product hydrocarbon + O2 → CO2 + H2O Ionic equation: Metal + Non metal Law of conservation of Mass: In all chemical reactions‚ mass is conserved. The total mass of all the reactants equals the total mass of all the products. ● identify the difference between elements‚ compounds and mixtures in terms of
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MODULE 1: THE CHEMICAL EARTH 3.1.1: Elements in Earth are present mostly as compounds because of interactions at the atomic level * Identify that matter is made of particles that are continuously moving and interacting Matter: anything that has mass and occupies space. Exists in three different states: solid (s)‚ liquid (l) and gas (g) The Particle Theory: “All matter is made up of small‚ indivisible particles called atoms that are continuously moving” | Solid | Liquid | Gas | Particle
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mobile delocalised valence electrons. • Metallic bonding is the electrostatic attraction between the delocalised electrons and the positive ions in the metallic lattice. Properties of metals: Property Explanation Relatively high density The particles are very close together. This is because of high electrostatic forces between the sea of valence electrons and the positively charged nucleus. Malleability and Ductility Because metallic bonding is non-directional-meaning that the bonds don’t have
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