LEWIS DOT STRUCTURES , MOLECULAR SHAPES, AND
... 5. Add connect the atoms by adding electron pair bonds. 6. Add unshared electron pairs around the remaining atoms so that everything is satisfied with an octet (note some atoms like hydrogen are satisfied when they have 2 valence electrons). 7. Count to make sure that the number of electrons used eq ...
... 5. Add connect the atoms by adding electron pair bonds. 6. Add unshared electron pairs around the remaining atoms so that everything is satisfied with an octet (note some atoms like hydrogen are satisfied when they have 2 valence electrons). 7. Count to make sure that the number of electrons used eq ...
Summarised Notes
... b) Compare the structure of simple molecular substances, eg methane; iodine, with those of giant molecular substances, eg poly(ethene); sand (silicon dioxide); diamond; graphite in order to deduce their properties ...
... b) Compare the structure of simple molecular substances, eg methane; iodine, with those of giant molecular substances, eg poly(ethene); sand (silicon dioxide); diamond; graphite in order to deduce their properties ...
Let’s talk Chemistry!
... compound contains Two nitrogen atoms and 4 oxygen atoms Formaldehyde, CH2O, and acetic acid, C2H4O2, have the same empirical formula but different ...
... compound contains Two nitrogen atoms and 4 oxygen atoms Formaldehyde, CH2O, and acetic acid, C2H4O2, have the same empirical formula but different ...
Eighth Grade Review - PAMS-Doyle
... several ways, including: • acids, bases, salts • inorganic and organic compounds. (All organic compounds contain carbon). ...
... several ways, including: • acids, bases, salts • inorganic and organic compounds. (All organic compounds contain carbon). ...
Chapter 9
... decrease by one electron and a negative charge means we would increase by one electron. ...
... decrease by one electron and a negative charge means we would increase by one electron. ...
Lecture#2
... Drawing Lewis Structures Our goals are to predict: a) the lowest energy structure (most thermodynamically stable) b) its properties (bond lengths, atomic charges, dipole moment, chemical reactivities) General rules: 1. Show ALL the valence electrons with dots 2. Provide octet (8 electrons) for each ...
... Drawing Lewis Structures Our goals are to predict: a) the lowest energy structure (most thermodynamically stable) b) its properties (bond lengths, atomic charges, dipole moment, chemical reactivities) General rules: 1. Show ALL the valence electrons with dots 2. Provide octet (8 electrons) for each ...
ChLM Final Review Name: Period: Base Knowledge 1. Classify the
... 22. Draw arrows showing where periods and groups are on the periodic table. ...
... 22. Draw arrows showing where periods and groups are on the periodic table. ...
Unit 4 - Dorman High School
... Now for more complicated models: 1. All valence electrons must be included for all atoms in the compound. 2. Atoms that are bonded share one or more pairs of electrons. 3. Each atom must have a full valence shell. Know the steps ...
... Now for more complicated models: 1. All valence electrons must be included for all atoms in the compound. 2. Atoms that are bonded share one or more pairs of electrons. 3. Each atom must have a full valence shell. Know the steps ...
Chapter 4 – Matter - Chemistry at Winthrop University
... Formed between metals and non-metals, and also with polyatomic ions (electrically charged molecules) ...
... Formed between metals and non-metals, and also with polyatomic ions (electrically charged molecules) ...
Review Sheet Filled Out
... Electrons closest to the nucleus have the least amount of energy Electrons farthest away from the nucleus have the most energy – valence e Have a negative charge Have insignificant mass and volume Reside in the 99.996% of the atom outside the nucleus Can’t tell where an electron is at any ...
... Electrons closest to the nucleus have the least amount of energy Electrons farthest away from the nucleus have the most energy – valence e Have a negative charge Have insignificant mass and volume Reside in the 99.996% of the atom outside the nucleus Can’t tell where an electron is at any ...
the atomic theory
... 3. Ernest Rutherford 4. James Chadwick 5. Neils Bohr 6. nucleus 7. proton 8. neutron 9. electron 10. shell 11. atomic number 12. atomic mass 13. Bohr Model 14. subatomic particle 15. isotope 16. empty bus seat rule B/ THE HISTORY OF THE ATOM: - John Dalton ...
... 3. Ernest Rutherford 4. James Chadwick 5. Neils Bohr 6. nucleus 7. proton 8. neutron 9. electron 10. shell 11. atomic number 12. atomic mass 13. Bohr Model 14. subatomic particle 15. isotope 16. empty bus seat rule B/ THE HISTORY OF THE ATOM: - John Dalton ...
Polarity of covalent bonds
... form of representation has bond-forming electron pairs represented as solid lines. While the idea of shared electron pairs provides an effective qualitative picture of covalent bonding, quantum mechanics is needed to understand the nature of these bonds and predict the structures and properties of ...
... form of representation has bond-forming electron pairs represented as solid lines. While the idea of shared electron pairs provides an effective qualitative picture of covalent bonding, quantum mechanics is needed to understand the nature of these bonds and predict the structures and properties of ...
CHM 101 - Academic Computer Center
... high, positive or slightly negative low, positive or slightly negative high, very negative None of these is generally correct. ...
... high, positive or slightly negative low, positive or slightly negative high, very negative None of these is generally correct. ...
AP Biology chap 2 HW - yhs
... different chemical properties, because they have different atomic numbers. b. the same chemical properties, because they have the same number of valence electrons. c. different chemical properties, because they differ in their number of protons and electrons. d. the same chemical properties, because ...
... different chemical properties, because they have different atomic numbers. b. the same chemical properties, because they have the same number of valence electrons. c. different chemical properties, because they differ in their number of protons and electrons. d. the same chemical properties, because ...
CHAPTER 9 : CHEMICAL BONDING I
... 9.92 The amide ion, NH-2 , is a Bronsted base, Represent the reaction between the amide ion and water. 9.94 The triiodide ion (I-3) in which the I atoms are arranged in a straight line is stable, but the corresponding F-3 ion does not exist. Explain. 9.96 Methyl isocyanate (CH3NCO) is used to make c ...
... 9.92 The amide ion, NH-2 , is a Bronsted base, Represent the reaction between the amide ion and water. 9.94 The triiodide ion (I-3) in which the I atoms are arranged in a straight line is stable, but the corresponding F-3 ion does not exist. Explain. 9.96 Methyl isocyanate (CH3NCO) is used to make c ...
here
... Intrinsic Semiconductors – No impurities and lattice defects in its crystal structure – If thermal or optical energy (E > Eg) break covalent bond free electron and hole – Electrons and holes are created in pairs, so no = po ≡ ni (at thermal equilibrium) o no = electron concentration at thermal e ...
... Intrinsic Semiconductors – No impurities and lattice defects in its crystal structure – If thermal or optical energy (E > Eg) break covalent bond free electron and hole – Electrons and holes are created in pairs, so no = po ≡ ni (at thermal equilibrium) o no = electron concentration at thermal e ...
quantum number
... Orbitals within a shell are divided into subshells that have the same value of the ...
... Orbitals within a shell are divided into subshells that have the same value of the ...
CHEMISTRY FINAL EXAM REVIEW SHEET
... Hydrogen is usually +1. Oxygen is usually –2. In a compound, the more electronegative element is given an oxidation number equal to its usual ionic charge. The sum of the oxidation numbers must equal the overall charge on the compound or ion. ...
... Hydrogen is usually +1. Oxygen is usually –2. In a compound, the more electronegative element is given an oxidation number equal to its usual ionic charge. The sum of the oxidation numbers must equal the overall charge on the compound or ion. ...
Chemical bond
A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are ""strong bonds"" such as covalent or ionic bonds and ""weak bonds"" such as Dipole-dipole interaction, the London dispersion force and hydrogen bonding.Since opposite charges attract via a simple electromagnetic force, the negatively charged electrons that are orbiting the nucleus and the positively charged protons in the nucleus attract each other. An electron positioned between two nuclei will be attracted to both of them, and the nuclei will be attracted toward electrons in this position. This attraction constitutes the chemical bond. Due to the matter wave nature of electrons and their smaller mass, they must occupy a much larger amount of volume compared with the nuclei, and this volume occupied by the electrons keeps the atomic nuclei relatively far apart, as compared with the size of the nuclei themselves. This phenomenon limits the distance between nuclei and atoms in a bond.In general, strong chemical bonding is associated with the sharing or transfer of electrons between the participating atoms. The atoms in molecules, crystals, metals and diatomic gases—indeed most of the physical environment around us—are held together by chemical bonds, which dictate the structure and the bulk properties of matter.All bonds can be explained by quantum theory, but, in practice, simplification rules allow chemists to predict the strength, directionality, and polarity of bonds. The octet rule and VSEPR theory are two examples. More sophisticated theories are valence bond theory which includes orbital hybridization and resonance, and the linear combination of atomic orbitals molecular orbital method which includes ligand field theory. Electrostatics are used to describe bond polarities and the effects they have on chemical substances.