metals but more like nonmetals Identify groups and sections of the periodic table by group name and common properties. 3.02 notes Lesson 03.03: Periodic Trends Describe and explain the trends for effective nuclear charge‚ atomic radius‚ ionic radius‚ and ionization energy across a period and down a group. -Effective Nuclear Charge- the charge (from the nucleus) felt by the valence electrons after you have taken into account the number of
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This is called bonding which is pretty much the realm of the electrons. It is the sharing of electrons from each atom that define the chemical bond. Because all bonds involve the sharing of electrons‚ we can say that all bonds are covalent. It’s just that some are more polar that others and some are very‚ very polar. It is the latter which take on some of the characteristics of an ionic bond. The ionic and covalent bonds are known to be the strongest chemical bonds. An ionic bond forms when
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2013 I. Learning Objectives At the end of the sessions‚ the students of III- 15‚ and III – 10 must be able to: 1. Students will be able to interpret and draw Lewis dot diagrams for individual atoms and both covalent and ionic compounds. II. Subject Matter A. Topic: Chemical Bonding B. References 1. Department of Education‚ Culture and Sports. (1991). Science and Technology III. Quezon City: Book Media Press‚ pp. 273. 2. Estrella‚ Mendoza E. Chemistry.2003. Phoenix Publishing House. Quezon
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molecules. If you are interested in electronegativity in an organic chemistry context‚ you will find a link at the bottom of this page. What is electronegativity Definition Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The Pauling scale is the most commonly used. Fluorine (the most electronegative element) is assigned a value of 4.0‚ and values range down to caesium and francium which are the least electronegative at 0.7. What happens if two
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within types of covalent and non-covalent bonding. Covalent bonding involves the pairing of electrons that are shared between atoms‚ whereas non-covalent bonding involves the attraction of electromagnetic forces between atoms. Covalent bonds are strong and non-covalent bonds are weak. Both covalent and non-covalent bonds relate in a sense of stability as covalent bonds are most stable when its outmost electron shell filled‚ typically octet (or eight electrons)‚ and non-covalent bonds are stable
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particles of a substance. Intramolecular forces: covalent and ionic bond within compounds. Attractive forces between molecules are mainly due to hydrogen bonding. Ion-ion attraction The energy of attraction between two oppositely charged ions is directly proportional to the charges on the ions and inversely proportional to the distance of separation. Ionic compound has high melting points. The product q+ q- increases as the charges on ions increase. Ionic substances containing multiply charged ions
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Chemistry Review sheet: Unit 1- Lesson 1‚ 2 *Key notes to keep in mind* ü Metals have a high low ionization energy ü Non-metals have a high electron affinity · Atom: The basic unity of an element which still retains the elements properties · Atomic number: the unique number of protons in the nucleus of a particular element · Isotope: Atoms of the same element which contain a different number of neutrons · Periodic law: The chemical
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and Bunsen burner. The substances were identified according to their properties. Paraffin wax was identified as a non-polar covalent solid‚ sucrose is a polar covalent‚ sodium chloride was acknowledged as an ionic solid‚ tin is a metallic solid‚ sand is a network covalent‚ unknown#1 is a non-polar covalent solid‚ unknown#2 is an ionic solid‚ and unknown#3 is a polar covalent solid. These conclusions were made based on their physical and chemical properties. Introduction Solid substances are classified
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IB Chemistry Summary- By Paul Li & Silvia Riggioni TABLE OF CONTENTS Table of Contents............................................................................................................................................................ 1 Atomic Theory................................................................................................................................................................ 3 The Electromagnetic Spectrum.............................................
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balanced chemical equations (2.2‚ 2.3) Interpret balanced chemical equations in terms of chemical amount (in moles) (2.3) Convert between chemical amount and mass (2.4) Classify chemical reactions (2.5‚ 2.6) Predict the solubility of elements and ionic and molecular compounds in water (2.6) Predict products for chemical reactions (2.5‚ 2.6) Memorized molecular compounds pg. 34 Sample Questions: Chapter One Review pg. 40 #11-19‚ 25 Chapter Two Review pg. 66 #5-7‚ 9 Unit Review pg. 68
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