of the periodic table in terms of periods (1 – 7 )‚ Groups (1 – 18)‚ and metals/non-metals * Describe the trends in atomic size and down a Group and across a Period. * Describe the trend in MP across period 3. | Atomic structure and bonding I can | | | Atomic structure * State that matter is built up from minute particles called atoms. * Write the symbols and names of the following elements:
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Experiment 3: Electronic structure‚ bonding and shape of some simple inorganic molecules. Introduction: In quantum chemistry‚ electronic structure is the state of motion of electrons in an electrostatic field created by stationary nuclei. The term encompass both the wave functions of the electrons and the energies associated with them. Electronic structure is obtained by solving quantum mechanical equations for the aforementioned clamped-nuclei problem. Electronic structure problem arise from the
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Describe the difference between a mixture and a compound. A compound is a substance in which atoms of different elements are chemically held to one another. A mixture is a substance made by combining two or more different materials in such a way that no chemical reaction occurs. A mixture can usually be separated back into its original components‚ a compound cannot. Below are some examples of the differences between each. Compounds •Compounds are pure substances. •They are made up of two or more
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writing chemical equations using Lewis structures for different reactions involving either ionic compounds or covalent compounds. Lastly‚ I will I will predict the empirical formulas of ionic and covalent compounds
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i) deduce empirical and molecular formula from suitable data Topic 1.3 Can you: a) define an ionic bond‚ covalent bond‚ metallic bond‚ and predict the type of bonding present in simple substances b) explain the difference between normal and dative covalent bonds c) define electronegativity and use it to explain why some bonds are covalent‚ others polar covalent and others ionic d) draw dot-cross diagrams to show
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light * Explain that the amount of energy needed to separate atoms in a compound is an indication of the strength of the attraction‚ or bond‚ between them The stronger the chemical bonding in a compound‚ the more energy is required to break the compound into atoms. Alternatively‚ the stronger the chemical bonding in a compound the more energy is released when the compound is formed from its
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bonds B) ionic bonds C) acid bonds D) nonpolar bonds E) none of the above 2. Most of water’s unique properties result from the fact that water molecules _____. A) are very small B) tend to repel each other C) are extremely large D) tend to stick together E) are in constant motion 3. Each water molecule is joined to _____ other water molecules by ____ bonds. A) two ... hydrogen B) four ... hydrogen C) three ... ionic D) four
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Distinguish between ionic bonds‚ covalent bonds (how are nonpolar and polar covalent bonds different)‚ and hydrogen bonds‚ noting their relative strengths and in what types of molecules they might be found. Give an example of each in a biological system. Covalent bonds are bonds that involve the sharing of a pair of valence electrons by two atoms. This type of bond is usually only between two nonmetal elements. Covalent bonds are strong bonds compared to other bonds‚ except ionic
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Current‚ Voltage and Power * Electricity is the flow of electric charge. We can describe the flow of electric charge in several ways. These include the quantities Current‚ Voltage and Power. Current * Current (I) is the rate of flow of Charge Carriers‚ such as electrons. Current is usually thought of as moving in the direction of positive charge‚ so from the positive power supply to the negative. However‚ since in metals it is electrons that carry electric charge‚ the actually flow is opposite
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HF – hydrogen fluoride is a covalent bond and shares one pair of electrons. The hydrogen end of the molecule is slightly positive and the fluorine end is slightly negative. This causes hydrogen bonding between other hydrogen fluoride molecules. KCl – potassium chloride is a metal halide salt. The bonding between potassium and chloride is an ionic bond. The potassium becomes a cation and the chloride an anion. The potassium end of the molecule becomes slightly positive and the other end slightly
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