sch3u unit 1 test: matter
... 9. When fluorine forms an ionic bond it tends to a. lose electrons b. gain electrons c. share electrons d. lose protons 10. Copper (II) hydroxide is composed of a. 2 elements, 2 atoms b. 2 elements, 3 atoms c. 3 elements, 4 atoms d. 3 elements, 5 atoms ...
... 9. When fluorine forms an ionic bond it tends to a. lose electrons b. gain electrons c. share electrons d. lose protons 10. Copper (II) hydroxide is composed of a. 2 elements, 2 atoms b. 2 elements, 3 atoms c. 3 elements, 4 atoms d. 3 elements, 5 atoms ...
Chemical Bonding and Molecular Structure
... molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms. Electron pairs are assumed to be localized on a particular atom [lone pairs] or in the space between two atoms [bonding pairs]. Lewis Structures describe the valence elec ...
... molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms. Electron pairs are assumed to be localized on a particular atom [lone pairs] or in the space between two atoms [bonding pairs]. Lewis Structures describe the valence elec ...
Review Questions
... 5. Find the percent composition of Oxygen in Na2S2O3 __________________________ ...
... 5. Find the percent composition of Oxygen in Na2S2O3 __________________________ ...
Atomic Structure Study Guide
... the times of _____________________. However, these speculations were not scientific theories, because they were not based on any experimental ____________. The first scientific theory of atoms was developed by ___________ in the 18th Century. He based his theory on 3 scientific _____ which he had ob ...
... the times of _____________________. However, these speculations were not scientific theories, because they were not based on any experimental ____________. The first scientific theory of atoms was developed by ___________ in the 18th Century. He based his theory on 3 scientific _____ which he had ob ...
Ground State
... Pieter Zeeman, Lorentz “spectra line splitting” in magnetic filed 1902 Nobel Prize ...
... Pieter Zeeman, Lorentz “spectra line splitting” in magnetic filed 1902 Nobel Prize ...
ATOMS
... • Most matter is in the form of COMPOUNDS or mixtures of compounds. For example: salt (NaCl), water (H20), carbon dioxide (CO2) • Compounds have properties UNLIKE those of their elements. For example: Salt—Sodium (Na) is a shiny, soft, gray, explosive metal with water & Chlorine (Cl) is a yellowish- ...
... • Most matter is in the form of COMPOUNDS or mixtures of compounds. For example: salt (NaCl), water (H20), carbon dioxide (CO2) • Compounds have properties UNLIKE those of their elements. For example: Salt—Sodium (Na) is a shiny, soft, gray, explosive metal with water & Chlorine (Cl) is a yellowish- ...
Valence electrons and Lewis Dot Structures
... Means that one or more electrons are ____________ from the metal to the nonmetal (no longer neutral) these are now ions ...
... Means that one or more electrons are ____________ from the metal to the nonmetal (no longer neutral) these are now ions ...
Final exam 2007
... 6. (7) How many L of oxygen, measured at 0 oC and 1.00 atm, are required for the complete combustion of 5.00 g of ethane (C2H6)? ...
... 6. (7) How many L of oxygen, measured at 0 oC and 1.00 atm, are required for the complete combustion of 5.00 g of ethane (C2H6)? ...
Chemistry of Life
... • To do work or cause change • ____________________________: Energy is not created or destroyed it only changes forms • _______________(exothermic)- releasing of energy • _______________(endothermic)-absorption of energy • Activation energy: Energy needed to start the reaction • ____________: someth ...
... • To do work or cause change • ____________________________: Energy is not created or destroyed it only changes forms • _______________(exothermic)- releasing of energy • _______________(endothermic)-absorption of energy • Activation energy: Energy needed to start the reaction • ____________: someth ...
When we solve the Schrödinger equation for the hydrogen molecule
... electrons about the inter-nuclear axis. 2. As defined, S is the total spin angular momentum quantum number, formed from the individual electron. Spin quantum number of single electron s = 1/2 , and ms = ±1/2. For one unpaired electron, S = s = 1/2 (a doublet state with 2S + 1 = 2). For two unpaired ...
... electrons about the inter-nuclear axis. 2. As defined, S is the total spin angular momentum quantum number, formed from the individual electron. Spin quantum number of single electron s = 1/2 , and ms = ±1/2. For one unpaired electron, S = s = 1/2 (a doublet state with 2S + 1 = 2). For two unpaired ...
Physics 361 Principles of Modern Physics
... present in each atomic orbital that creates the molecular orbitals. ...
... present in each atomic orbital that creates the molecular orbitals. ...
Semester 1 Final Exam Study Guide
... 31. How many valence electrons do most atoms need to become as stable as possible? 32. What part of the atom is involved in compound formation? ...
... 31. How many valence electrons do most atoms need to become as stable as possible? 32. What part of the atom is involved in compound formation? ...
Ch. 2 Chemistry
... Atomic nucleus (b) An electron can move from one level to another only if the energy it gains or loses is exactly equal to the difference in energy between the two levels. Arrows indicate some of the step-wise changes in potential energy that are possible. Copyright © 2004 Pearson Education, Inc. pu ...
... Atomic nucleus (b) An electron can move from one level to another only if the energy it gains or loses is exactly equal to the difference in energy between the two levels. Arrows indicate some of the step-wise changes in potential energy that are possible. Copyright © 2004 Pearson Education, Inc. pu ...
chapter5
... circular paths. Each electron has an energy level. Each energy level of the electron can be thought of as rungs on a ladder. The energy levels closest to the nucleus are like rungs of a ladder closest to the ground. The rungs at the top of the ladder are analogous to the energy levels furthest from ...
... circular paths. Each electron has an energy level. Each energy level of the electron can be thought of as rungs on a ladder. The energy levels closest to the nucleus are like rungs of a ladder closest to the ground. The rungs at the top of the ladder are analogous to the energy levels furthest from ...
LIST OF TOPICS COVERED DURING THIS COURSE
... discussions. If you missed any notes, please get the information from a classmate, or from myself. ...
... discussions. If you missed any notes, please get the information from a classmate, or from myself. ...
Chapter Five: Many electron atom
... We can now 'build' atoms by filling the orbitals expected from a one-electron model 'perturbed' by what we know about electron-electron repulsion. This is called atomic 'Aufbau'. The first elements are easy if we postulate two 'rules': • Each electron has one of two possible 'flavors': up or down wh ...
... We can now 'build' atoms by filling the orbitals expected from a one-electron model 'perturbed' by what we know about electron-electron repulsion. This is called atomic 'Aufbau'. The first elements are easy if we postulate two 'rules': • Each electron has one of two possible 'flavors': up or down wh ...
Chapter 2 – The Structure of the Atom Since the book assumes you
... have integral values of 0 to (n - 1). Commonly, letters are used to represent this quantum number. 0 = s, 1 = p, 2 = d, 3 = f, 4 = g, ... The magnetic q.n. m, gives the number of each type of orbital and its orientation in space. There are (2 + 1) of each type of orbital and the orientations are d ...
... have integral values of 0 to (n - 1). Commonly, letters are used to represent this quantum number. 0 = s, 1 = p, 2 = d, 3 = f, 4 = g, ... The magnetic q.n. m, gives the number of each type of orbital and its orientation in space. There are (2 + 1) of each type of orbital and the orientations are d ...
1 - Hatboro
... 52. What is a covalent bond? An ionic bond? 53. Know how to subtract electronegativities to find bond type (ionic, polar and nonpolar covalent) Ex: What kind of bond is between: H-F _____ O-O _____ Ca-Cl_______ (you will need to look up their electronegativities) 54. What is the octet rule? 55. What ...
... 52. What is a covalent bond? An ionic bond? 53. Know how to subtract electronegativities to find bond type (ionic, polar and nonpolar covalent) Ex: What kind of bond is between: H-F _____ O-O _____ Ca-Cl_______ (you will need to look up their electronegativities) 54. What is the octet rule? 55. What ...
Chapter 8 & 9 PowerPoint
... Three types of bonding • Metallic bonding – results from the attraction between metal atoms and the surrounding sea of electrons • Ionic bonding – results from the electrical attraction between positive and negative ions. • Covalent bonding – results from the sharing of electron pairs between two a ...
... Three types of bonding • Metallic bonding – results from the attraction between metal atoms and the surrounding sea of electrons • Ionic bonding – results from the electrical attraction between positive and negative ions. • Covalent bonding – results from the sharing of electron pairs between two a ...
Molecular orbital diagram
A molecular orbital diagram, or MO diagram, is a qualitative descriptive tool explaining chemical bonding in molecules in terms of molecular orbital theory in general and the linear combination of atomic orbitals (LCAO) molecular orbital method in particular. A fundamental principle of these theories is that as atoms bond to form molecules, a certain number of atomic orbitals combine to form the same number of molecular orbitals, although the electrons involved may be redistributed among the orbitals. This tool is very well suited for simple diatomic molecules such as dihydrogen, dioxygen, and carbon monoxide but becomes more complex when discussing even comparatively simple polyatomic molecules, such as methane. MO diagrams can explain why some molecules exist and others do not. They can also predict bond strength, as well as the electronic transitions that can take place.