File - Grade 12 Chemistry
... Dispersion forces are very weak intermolecular forces that exist between molecules. When a carbon atom is bonded to another carbon atom, or to a hydrogen atom, the bond is not considered to be polar because the electronegativity difference between carbon atoms is zero and between carbon and hydrogen ...
... Dispersion forces are very weak intermolecular forces that exist between molecules. When a carbon atom is bonded to another carbon atom, or to a hydrogen atom, the bond is not considered to be polar because the electronegativity difference between carbon atoms is zero and between carbon and hydrogen ...
“No Score” from Exam 1??
... 3. The electron domain geometry corresponds to the number of electron domains 4. The molecular geometry is defined by the positions of only ________________ in the molecules, _______ the nonbonding pairs ...
... 3. The electron domain geometry corresponds to the number of electron domains 4. The molecular geometry is defined by the positions of only ________________ in the molecules, _______ the nonbonding pairs ...
Unit 1 Notes
... 1. All matter is composed of extremely small particles called atoms, which cannot be broken into smaller particles, created nor destroyed. 2. The atoms of any given element are all identical to each other and different from the atoms of other elements. 3. Atoms of different elements combine in speci ...
... 1. All matter is composed of extremely small particles called atoms, which cannot be broken into smaller particles, created nor destroyed. 2. The atoms of any given element are all identical to each other and different from the atoms of other elements. 3. Atoms of different elements combine in speci ...
CHAPTER 13 BONDING: GENERAL CONCEPTS
... a. This diagram represents a polar covalent bond as in HCl. In a polar covalent bond, there is an electron rich region (indicated by the red color) and an electron poor region (indicated by the blue color). In HCl, the more electronegative Cl atom (on the red side of the diagram) has a slightly grea ...
... a. This diagram represents a polar covalent bond as in HCl. In a polar covalent bond, there is an electron rich region (indicated by the red color) and an electron poor region (indicated by the blue color). In HCl, the more electronegative Cl atom (on the red side of the diagram) has a slightly grea ...
2014 Exams
... BaCl2 and no precipitate was observed upon any of those additions. b. One part was treated with NH4Cl and excess NH3 and gave a blue solution with no precipitate. Which ions are present? absent? undetermined? Explain your reasoning. (see beginning of test for all elements in Al-Ni group) ...
... BaCl2 and no precipitate was observed upon any of those additions. b. One part was treated with NH4Cl and excess NH3 and gave a blue solution with no precipitate. Which ions are present? absent? undetermined? Explain your reasoning. (see beginning of test for all elements in Al-Ni group) ...
syllabus details - hrsbstaff.ednet.ns.ca
... Students should be able to draw an energy-level diagram show transitions between different energy levels and recognize that the lines in a line spectrum are directly related to these differences. An understanding of convergence is expected. Series should be considered in the ultraviolet visible and ...
... Students should be able to draw an energy-level diagram show transitions between different energy levels and recognize that the lines in a line spectrum are directly related to these differences. An understanding of convergence is expected. Series should be considered in the ultraviolet visible and ...
The Complete Notes - Joliet Junior College
... remembering. An analogy would be this: you read all the books out there on the subject of golf, but don’t get round to swinging a club – what do you think happens when you tee off for the first time? ...
... remembering. An analogy would be this: you read all the books out there on the subject of golf, but don’t get round to swinging a club – what do you think happens when you tee off for the first time? ...
Solution Preparation Final Goueth
... 29. When FeCl3 is ignited in an atmosphere of pure oxygen, this reaction takes place. 4 FeCl3(s) + 3 O2 (g) ---> 2 Fe2O3(s) + 6 Cl2 (g) If 3.0 mol of FeCl3 are ignited in the presence of 2.0 mol of O2 gas, how much of which reagent is present in excess and therefore remains unreacted? (A) 0.33 mol F ...
... 29. When FeCl3 is ignited in an atmosphere of pure oxygen, this reaction takes place. 4 FeCl3(s) + 3 O2 (g) ---> 2 Fe2O3(s) + 6 Cl2 (g) If 3.0 mol of FeCl3 are ignited in the presence of 2.0 mol of O2 gas, how much of which reagent is present in excess and therefore remains unreacted? (A) 0.33 mol F ...
Name __KEY____________ Per. ______ Polarity and
... When examining trends in the periodic table, as we move towards the top-right the elements have a greater _electronegativity_ (atomic radius/ electronegativity), which is a measure of how much they want to _ hold onto_ (hold onto/ let go of) their electrons. For any two elements that share a chemica ...
... When examining trends in the periodic table, as we move towards the top-right the elements have a greater _electronegativity_ (atomic radius/ electronegativity), which is a measure of how much they want to _ hold onto_ (hold onto/ let go of) their electrons. For any two elements that share a chemica ...
9th class bridge course 74-112
... (i) Bohr’s model could not explain the spectra of atoms containing more than one electron. (ii) It was observed that in the presence of a magnetic field, each spectral line gets split up into closely spaced lines. This phenomenon, known as Zeeman effect, could not be explained by Bohr’s model. Simil ...
... (i) Bohr’s model could not explain the spectra of atoms containing more than one electron. (ii) It was observed that in the presence of a magnetic field, each spectral line gets split up into closely spaced lines. This phenomenon, known as Zeeman effect, could not be explained by Bohr’s model. Simil ...
Spring 2008
... answer D: [The first row d orbitals (trans metals) are n=3, for d orbitals, l=2 (fyi for s, l=0; for p, l=1). For d oribials,ml=-2,-1,0,1, or +1. ms for an orbital can only be -1/2, 0 or ½. Note that for an electron ms can be -1/2 or +1/2) ...
... answer D: [The first row d orbitals (trans metals) are n=3, for d orbitals, l=2 (fyi for s, l=0; for p, l=1). For d oribials,ml=-2,-1,0,1, or +1. ms for an orbital can only be -1/2, 0 or ½. Note that for an electron ms can be -1/2 or +1/2) ...
4.2 3-D Structure
... 1. The words that make up the initialism “VSEPR”—valence shell electron-pair repulsion —describe the concept of the theory very well. The main concept of the theory is that pairs of electrons, both bonding and non-bonding, will repel one another and maximize the distance between themselves around an ...
... 1. The words that make up the initialism “VSEPR”—valence shell electron-pair repulsion —describe the concept of the theory very well. The main concept of the theory is that pairs of electrons, both bonding and non-bonding, will repel one another and maximize the distance between themselves around an ...
IB Chemistry Online EQ_Ans
... energy is required to break all these bonds and hence it has a high melting point. Phosphorus (P4), sulfur (S8), chlorine (Cl2) and argon (Ar) are simple molecular covalent substances and hence are held together in the solid state by London (dispersion) forces. A small amount of thermal energy is re ...
... energy is required to break all these bonds and hence it has a high melting point. Phosphorus (P4), sulfur (S8), chlorine (Cl2) and argon (Ar) are simple molecular covalent substances and hence are held together in the solid state by London (dispersion) forces. A small amount of thermal energy is re ...
Topic 1: Quantitative chemistry (12
... Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively charged nuclei. Describe how the covalent bond is formed as a result of electron sharing. Deduce the Lewis (electron dot) structures of molecules and ions for up to four electron pairs on each atom. ...
... Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively charged nuclei. Describe how the covalent bond is formed as a result of electron sharing. Deduce the Lewis (electron dot) structures of molecules and ions for up to four electron pairs on each atom. ...
Part 3 Answers Only for Questions, Exercises, and Problems in The
... 8. The particles in a solid occupy fixed positions relative to each other and cannot be poured, but different pieces of solids can move relative to each other. The slogan emphasizes that this brand of table salt has solid pieces small enough to move freely relative to one another, but not so small t ...
... 8. The particles in a solid occupy fixed positions relative to each other and cannot be poured, but different pieces of solids can move relative to each other. The slogan emphasizes that this brand of table salt has solid pieces small enough to move freely relative to one another, but not so small t ...
C:\Documents and Settings\mrh70950\My Documents
... Silicon, which is isoelectronic with carbon, can be found immediately below carbon in the periodic table. Not surprisingly, silicon is very similar to carbon: it is tetravalent, and readily makes tetrahedral analogs of alkanes. Thus, tetramethylsilane, Si(CH3)4 (bp 27EC), like 2,2dimethylpropane C(C ...
... Silicon, which is isoelectronic with carbon, can be found immediately below carbon in the periodic table. Not surprisingly, silicon is very similar to carbon: it is tetravalent, and readily makes tetrahedral analogs of alkanes. Thus, tetramethylsilane, Si(CH3)4 (bp 27EC), like 2,2dimethylpropane C(C ...
General Chemistry I - University of Toledo
... 5.12 Identify an orbital based on its shape and describe it using a set of quantum numbers. 5.13 Visualize the nodal planes in different types of orbitals and different shells. 5.14 Assign a set four quantum numbers for electrons in an atom. 5.15 Explain how electron shielding gives the order of sub ...
... 5.12 Identify an orbital based on its shape and describe it using a set of quantum numbers. 5.13 Visualize the nodal planes in different types of orbitals and different shells. 5.14 Assign a set four quantum numbers for electrons in an atom. 5.15 Explain how electron shielding gives the order of sub ...
Bent's rule
Bent's rule describes and explains the relationship between the isovalent hybridization of central atoms in molecules and the electronegativities of substituents. The rule was stated by Henry Bent as follows: ""Atomic s character concentrates in orbitals directed toward electropositive substituents"".The chemical structure of a molecule is intimately related to its properties and reactivity. Valence bond theory proposes that molecular structures are due to covalent bonds between the atoms and that each bond consists of two overlapping and typically hybridised atomic orbitals. Traditionally, p-block elements in molecules are assumed to hybridise strictly as spn, where n is either 1, 2, or 3. In addition, the hybrid orbitals are all assumed to be equivalent (i.e. the n+1 spn orbitals have the same p character). Results from this approach are usually good, but they can be improved upon by allowing hybridised orbitals with noninteger and unequal p character. Bent's rule provides a qualitative estimate as to how these hybridised orbitals should be constructed. Bent's rule is that in a molecule, a central atom bonded to multiple groups will hybridise so that orbitals with more s character are directed towards electropositive groups, while orbitals with more p character will be directed towards groups that are more electronegative. By removing the assumption that all hybrid orbitals are equivalent spn orbitals, better predictions and explanations of properties such as molecular geometry and bond strength can be obtained.Bent's rule can be generalized to d-block elements as well. The hybridisation of a metal center is arranged so that orbitals with more s character are directed towards ligands that form bonds with more covalent character. Equivalently, orbitals with more d character are directed towards groups that form bonds of greater ionic character.