Lesson 3.01: History of the Periodic Table 1. Explain how scientific observations led to the development of‚ and changes to‚ the periodic table. Dmitri Mendeleev- first periodic table‚ organized 63 known elements according to properties‚ organized into rows and columns. He wrote names‚ mass and chemical properties on each. Julius lothar Meyer- independently worked in German ‚ similar to Mendeleev Henry Gwyn Jeffrey’s Moseley: worked with Ernest Rutherford experimented with 38 metals‚ he found that
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electrons. There are three types of bonds that I have learned about in the bonding comparison lab. These bonds include ionic‚ polar covalent‚ and non-polar covalent. Each of these bonds and the element compounds connected to them has individual solubility‚ conductivity‚ melting point‚ and volatility levels. The three element compounds that will follow are sodium chloride‚ sucrose‚ and p-dichlorobenzene. Sodium chloride is an ionic bond. It is soluble in water‚ but is not soluble in heptane. Sodium chloride
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wiki.answers.com 4. In ionic bonding‚ the atoms are bound by attraction of opposite ions‚ whereas‚ in covalent bonding‚ atoms are bound by sharing electrons to attain stable electron configurations. Found @ http://en.wikipedia.org/wiki/Ionic_bond#Comparison_with_covalent_bonding 5. There are many types of chemical bonds and forces acting together to bind molecules together. The two most basic types of bonds are characterized as either ionic or covalent. In ionic bonding‚ atoms transfer electrons
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Hwa Chong Institution (High School) Secondary 4 End of Year Examinations Chemistry Revision Notes List of topics: 1. Atomic Structure 2. Separation Techniques 3. Chemical Bonds and Bonding (Ionic‚ Covalent) 4. Metals 5. Properties and structures of compounds 6. Qualitative Analysis 7. Acids‚ Bases and Salts 8. Chemical Periodicity 9. Chemical Calculations 10. Air and Environment 11. Electrochemistry (Including Redox reactions) 12. Thermochemistry 13. Rates of Reaction 14. Chemical
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observations in the lab‚ categorize each unidentified compound as ionic or covalent. Explain in one or two sentences why you categorized the compounds the way that you did. (5 points) Based on my observations in the lab I categorized Substance A and Substance C as an ionic bonds because the solids don‘t conduct electricity but when in liquid state and aqueous solutions‚ electricity was conducted. I categorized substances B and D as covalent bonds because the solids conduct electricity but the liquid
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type of compound usually has higher melting points‚ ionic compounds or covalent compounds? What is the reason for this difference in melting points? (3 points) 2. Do ionic compounds conduct electricity as: (3 points) a. Solids? b. Liquids? c. Aqueous solutions (when the ionic compounds are dissolved in water)? 3. Do covalent compounds conduct electricity as: (3 points) a. Solids? b. Liquids? c. Aqueous solutions (when the covalent compounds are dissolved in water)? Part II: Lab
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in chemical bonding? What is the octet rule? What does the period on the periodic table tell you about an atom? What does the group/family on the periodic table tell you about a Group A element? Define molecule Define compound Define ionic bond and describe how they are formed Define ion Define cation Define anion Define polyatomic ion Define covalent bond and describe how they are formed Define electronegativity and describe how it is used to determine if a bond is ionic‚ polar covalent or nonpolar
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broadly classified into two types: Ionic and Covalent. Ionic: metal & nonmetal Metals have a tendency to lose electrons and nonmetals have a tendency to gain them. The metal atom becomes a cation and a nonmetal becomes an anion. The oppositely charged ions attract one another and form an ionic compound Covalent: nonmetal & nonmetal Covalent bonds are shared; Ionic bonds are distributed Covalent bonds are stronger than Ionic bonds Ionic Compounds: Ionic compounds consist of positive and
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C2.1.1 Structure and bonding a) Compounds are substances in which atoms of two or more elements are chemically combined. b) Chemical bonding involves either transferring or sharing electrons in the highest occupied energy levels (shells) of atoms in order to achieve the electronic structure of a noble gas. c) When atoms form chemical bonds by transferring electrons‚ they form ions. Atoms that lose electrons become positively charged ions. Atoms that gain electrons become negatively charged
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That is why chemists use some sort of classification in which each substance would fit into their discrete groupings. Chemist use bonding types‚ electrical conductivity‚ melting and boiling point and physical properties to classify substances into four main groups‚ which are: • Metallic substances • Ionic compounds • Covalent molecular and; • Covalent network substances Metallic substances are substances that are made up of one or more metal. They have regular 3D lattice of positively
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