4 - College of Arts and Sciences
... C (graphite) + O2 (g) CO2 (g) ∆ H = -393.5 kJ ∆ H = -285.5 kJ H2 (g) + ½ O2 (g) H2O C2H2 (g) + 5/2 O2 (g) 2 CO2 (g) + H2O ∆ H = -1299.4 2 CO2 (g) + H2O C2H2 (gas) + 5/2 O2 (g) ∆ H = +1299.4 ...
... C (graphite) + O2 (g) CO2 (g) ∆ H = -393.5 kJ ∆ H = -285.5 kJ H2 (g) + ½ O2 (g) H2O C2H2 (g) + 5/2 O2 (g) 2 CO2 (g) + H2O ∆ H = -1299.4 2 CO2 (g) + H2O C2H2 (gas) + 5/2 O2 (g) ∆ H = +1299.4 ...
chemical bond
... covalent bonds (sharing). i.e. must be a non-metal and a non-metal Molecular compound – a chemical compound whose simplest units are molecules. ...
... covalent bonds (sharing). i.e. must be a non-metal and a non-metal Molecular compound – a chemical compound whose simplest units are molecules. ...
4 - College of Arts and Sciences
... What is the oxidation number ? What is oxidized ? What is causing oxidation? What is reduced ? What is causing reduction ? ...
... What is the oxidation number ? What is oxidized ? What is causing oxidation? What is reduced ? What is causing reduction ? ...
Chapter 7
... Follow 3 rules to configure the electrons 1. Aufbau Principle - electrons fill orbitals starting at the lowest available (possible) energy states before filling higher states 2. Pauli Exclusion Principle - two electrons cannot share the same set of quantum numbers within the same system. Therefore, ...
... Follow 3 rules to configure the electrons 1. Aufbau Principle - electrons fill orbitals starting at the lowest available (possible) energy states before filling higher states 2. Pauli Exclusion Principle - two electrons cannot share the same set of quantum numbers within the same system. Therefore, ...
Slide 1
... The symbol for the magnetic quantum number is m which defines the orbital. m = - , (- + 1), (- +2), .....0, ......., ( -2), ( -1), The last quantum number is the spin quantum number which has the symbol m s which characterizes the single electron. The spin quantum number only has two pos ...
... The symbol for the magnetic quantum number is m which defines the orbital. m = - , (- + 1), (- +2), .....0, ......., ( -2), ( -1), The last quantum number is the spin quantum number which has the symbol m s which characterizes the single electron. The spin quantum number only has two pos ...
A COMPUTATIONAL STUDY OF -SCN
... 8. In the Surfaces window, click the Add button. Choose HOMO. Move the window out of the way, but leave it open. 9. On the menu bar, click Setup, and then Calculations. a. Calculate: Equilibrium Geometry with Hartree-Fock 3-21G should already be selected (both are default settings). b. Determine how ...
... 8. In the Surfaces window, click the Add button. Choose HOMO. Move the window out of the way, but leave it open. 9. On the menu bar, click Setup, and then Calculations. a. Calculate: Equilibrium Geometry with Hartree-Fock 3-21G should already be selected (both are default settings). b. Determine how ...
Chapter 10 - HCC Learning Web
... The number of molecular orbitals formed is always equal to the number of atomic orbitals combined. A molecular orbital can accommodate up to two electrons. When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by Hund's rule. Low-energy molecular orbitals ...
... The number of molecular orbitals formed is always equal to the number of atomic orbitals combined. A molecular orbital can accommodate up to two electrons. When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by Hund's rule. Low-energy molecular orbitals ...
Atomic Structure: SOL Review #1 Name: Historical Developments 1
... 26) How does the following orbital box diagram for Nitrogen violate Hund’s rule? The electrons are not “singly before pairing.” Electrons repel each other, so they do want not pair until there is no more “space” left in the sublevel. Periodic Table and Periodic Trends 27) Which elements would have s ...
... 26) How does the following orbital box diagram for Nitrogen violate Hund’s rule? The electrons are not “singly before pairing.” Electrons repel each other, so they do want not pair until there is no more “space” left in the sublevel. Periodic Table and Periodic Trends 27) Which elements would have s ...
Chemical Bonding
... • The subatomic particles that make up atoms are protons, neutrons, and electrons. • Protons=Positive charge • Neutrons=Neutral charge • Electrons=Negative charge ...
... • The subatomic particles that make up atoms are protons, neutrons, and electrons. • Protons=Positive charge • Neutrons=Neutral charge • Electrons=Negative charge ...
Unit 4 Chap. 4 Arrangement of Electrons in Atoms
... IN THE ELECTRON DOT DIAGRAM, THE SYMBOL REPRESENTS THE NUCLEUS AND ALL ELECTRONS EXCEPT THOSE IN THE OUTER LEVEL. IN THE ELECTRON DOT DIAGRAM, DOTS INDICATE OUTER LEVEL PAIRED OR UNPAIRED ELECTRONS. ELECTRON-DOT NOTATION (LEWIS DOT FORMULAS) ...
... IN THE ELECTRON DOT DIAGRAM, THE SYMBOL REPRESENTS THE NUCLEUS AND ALL ELECTRONS EXCEPT THOSE IN THE OUTER LEVEL. IN THE ELECTRON DOT DIAGRAM, DOTS INDICATE OUTER LEVEL PAIRED OR UNPAIRED ELECTRONS. ELECTRON-DOT NOTATION (LEWIS DOT FORMULAS) ...
Notetakers
... • electrons in an orbital spin in opposite directions; these directions are designated as + ½ and – ½ Pauli Exclusion Principle: states that no 2 electrons have an identical set of four quantum #’s; ensures that no more than 2 electrons can be found within a particular orbital. Hund’s rule: orbitals ...
... • electrons in an orbital spin in opposite directions; these directions are designated as + ½ and – ½ Pauli Exclusion Principle: states that no 2 electrons have an identical set of four quantum #’s; ensures that no more than 2 electrons can be found within a particular orbital. Hund’s rule: orbitals ...
Learning Standards vocab chemical basis and molecules of life 09
... Given the number of protons, identify the element using a Periodic Table. Explain the arrangement of the elements on the Periodic Table, including the significant relationships among elements in a given column or row. Explain how ions and ionic bonds are formed (e.g., sodium atoms lose an elec ...
... Given the number of protons, identify the element using a Periodic Table. Explain the arrangement of the elements on the Periodic Table, including the significant relationships among elements in a given column or row. Explain how ions and ionic bonds are formed (e.g., sodium atoms lose an elec ...
3. atomic structure
... In this class we will be performing an experiment called the “Flame Test”. We will be heating up metal powders in order to excite the electrons to jump from a lower energy level to a higher energy level. When an electron returns from a higher energy state to a lower energy state, it emits a specific ...
... In this class we will be performing an experiment called the “Flame Test”. We will be heating up metal powders in order to excite the electrons to jump from a lower energy level to a higher energy level. When an electron returns from a higher energy state to a lower energy state, it emits a specific ...
water, h2o
... When molecules form the atomic orbitals get re-arranged into new molecular orbitals to satisfy symmetry requirements. The oxygen atom 16O8 has the following atomic orbitals: 2(1s), 2(2s), 4(2p). The s orbitals are of course spherically symmetric, while the p orbitals are of the form: px = sinθ∙cosφ; ...
... When molecules form the atomic orbitals get re-arranged into new molecular orbitals to satisfy symmetry requirements. The oxygen atom 16O8 has the following atomic orbitals: 2(1s), 2(2s), 4(2p). The s orbitals are of course spherically symmetric, while the p orbitals are of the form: px = sinθ∙cosφ; ...
CHEM 1211K Test IV MULTIPLE CHOICE. (3 points each) 1) The
... among different I2 molecules in the solid? A) London dispersion forces B) ionic-dipole interactions C) dipole-dipole attractions D) dipole-dipole rejections E) covalent-ionic interactions 22) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.2 J/mol(K) the conversio ...
... among different I2 molecules in the solid? A) London dispersion forces B) ionic-dipole interactions C) dipole-dipole attractions D) dipole-dipole rejections E) covalent-ionic interactions 22) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is 75.2 J/mol(K) the conversio ...
General Chemistry - Review for final exam: (Make sure you bring
... 72. In the activity series of metals are the more reactive metals found on the top or the bottom of the chart? 73. What conditions in the reactants must be present in order for a double-replacement to take place? 74. What types of products are you likely to find in a double-replacement reaction? 75. ...
... 72. In the activity series of metals are the more reactive metals found on the top or the bottom of the chart? 73. What conditions in the reactants must be present in order for a double-replacement to take place? 74. What types of products are you likely to find in a double-replacement reaction? 75. ...
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.