5 – Bonding and Structure Revision Notes 1) Introduction • Atoms form bonds to get a full outer shell of electrons • There are three types of bonding: ionic‚ covalent and metallic • The structures produced by forming bonds are either giant or simple • The possible combinations of structure and bonding are giant ionic‚ simple covalent‚ giant covalent and giant metallic • Simple covalent is sometimes called simple molecular • Giant covalent is sometimes called giant molecular
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valence electrons do atoms of each element have? a. nitrogen d. barium b. lithium e. bromine c. phosphorus f. carbon 37. Name each ion in Problem 36. Identify each as an anion or a cation. 7.2 Ionic Bonds and Ionic Compounds 38. Define an ionic bond. 39. Explain why ionic compounds are electrically 29. Write electron dot structures for each of the fol- lowing elements: a. Cl b. S c. Al d. Li neutral. *40. 30. Describe two ways that an ion forms from an atom
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negative anions. IONS Are charges particles. EXMAPLES Atomic Notation and Bohr Diagrams Lewis Dot Diagram Examples Lewis Dot Diagrams of an Negative ION (NON-METAL) Negative ions have 8 valence electrons! Lewis Dot Diagram of an Ionic Compound Lewis Dot Diagrams of an Positive ION (METAL) Positive Ions have no valence electrons! The Octet Rule REMEMBER! All elements want to be like the noble gases. All elements want full electron shells. All elements want 8 valence
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Biology Notes 1.02 Sometimes a practice or belief claims to be science but does not follow the scientific method or cannot be proven reliable through experimentation. These practices are examples of pseudoscience‚ which literally means "fake science." Charms‚ astrology = stars‚ and phrenology= reading the bump on skull 1.03 * In the mid 1600s in the Netherlands‚ the scientist Antonie van Leeuwenhoek developed the first known microscope using a single magnifying lens. He was the first person
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HKDSE Chemistry – A Modern View 1 (SAMPLE) Suggested Answers (Coursebook) |Chapter 1 The fundamentals of chemistry | |Class Practice |1 | |Chapter Exercises |3 | |Chapter 2 The atmosphere
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around the atoms and lines. c) Octet rule: It is referring to the principle that bonded atoms share their eight outer electrons. There rule of the octet is sometimes broken. d) Cations/Anions: It is an ionic species with a positive charge‚ example of Cation/Anions: Anion is an ionic species having a negative charge. e) Electronegativity: It is a property of an atom which increases with its tendency to attract the electron of a bond. f) Polar covalent bond: Polar covalent bonds act
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Lipids are used for energy storage and for hormones. Question 9. Question : The instructions for growth‚ development‚ metabolism‚ and reproduction of a cell are contained in: DNA Question 10. Question : The ’sequence’‚ or order of amino acids in a protein is termed its ____________‚ whereas the 3-dimensional structure of a two proteins interacting with each other is termed its ____________. Student Answer: primary structure‚ quaternary structure Question 11
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students define the following terms: compound‚ metal‚ non-metals‚ ionic compound‚ covalent compound‚ ion‚ cation‚ anion‚ polyatomic ion‚ oxidation no. ‚ chemical formula‚ binary compounds‚ ternary compounds. 2. Ask the importance of giving chemical formulas to compounds. 3. Classify compounds as ionic or covalent. If ionic‚ identify whether binary or ternary. 4. Specify the rules in writing chemical formulas of binary ionic compounds using the Stock and classical method. 5. Specify the rules
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is to learn to demonstrate a double-replacement reaction of ionic compounds. To accomplish this‚ two ionic compounds will be mixed together and the product will precipitate out of solution. In this procedure‚ the product must be precipitated out of the solution and then weighed. For this lab‚ lead (II) nitrate (Pb(NO3)2) and potassium chromate (K2CrO4) will be reacted together to demonstrate double replacement reaction between 2 ionic compounds. This was shown when chromate replaced the nitrate
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called electrolytes and those that do not conduct electricity are called nonelectrolytes. Also electrolytes can be strong or weak. Under strong electrolytes we have NaCl and CaCl2 which are ionic compounds‚ HCI‚ HNO3‚ HBr and H2SO4 are under acids and NaOH‚ KOH‚ and LiOH are under bases. Weak electrolytes are ionic compounds and slightly soluble such as CH3COOH‚ under acids we have HF‚ H2CO3‚ H2SO3‚ and NH3.While nonelectrolytes are nonpolar covalent compounds such as O2 and H2O‚ and under acids we
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