SUMMER WORK AP Chemistry
... experiment requires 15.0 g of cyclohexane, whose density at 25 °C is 0.7781 g/mL. What volume of cyclohexane should be used? (c) A spherical ball of lead has a diameter of 5.0 cm. What is the mass of the sphere if lead has a density of 11.34 g.cm3? (The volume of a sphere is (4/3)πr3where r is the r ...
... experiment requires 15.0 g of cyclohexane, whose density at 25 °C is 0.7781 g/mL. What volume of cyclohexane should be used? (c) A spherical ball of lead has a diameter of 5.0 cm. What is the mass of the sphere if lead has a density of 11.34 g.cm3? (The volume of a sphere is (4/3)πr3where r is the r ...
Fall Final Review Honors
... W 32. Why are there small jumps in the 1st ionization energies of the elements as you move across a period? 33. Why is there a large increase in ionization energy when the 4th electron is removed from aluminum? VOCAB: ionization energy periodic law metals/nonmetals/metalloids shielding excited state ...
... W 32. Why are there small jumps in the 1st ionization energies of the elements as you move across a period? 33. Why is there a large increase in ionization energy when the 4th electron is removed from aluminum? VOCAB: ionization energy periodic law metals/nonmetals/metalloids shielding excited state ...
Glossary
... Equipartition theorem − consequence of the kinetic molecular theory that molecules have average kinetic energy proportional to the number of different types of molecular motion. Equivalent − one mol of charge (protons, electrons, ions). Exclusion principle− no two electrons can have the same set of ...
... Equipartition theorem − consequence of the kinetic molecular theory that molecules have average kinetic energy proportional to the number of different types of molecular motion. Equivalent − one mol of charge (protons, electrons, ions). Exclusion principle− no two electrons can have the same set of ...
chemistry i
... decreases. The equation E = hν means that as frequency increases, energy increases. Using this information and the reference tables, which color of visible light has the least energy? A. Red b. Yellow c. Green d. Violet 38. If an electron drops from n=6 to n=2, what type of electromagnetic radiation ...
... decreases. The equation E = hν means that as frequency increases, energy increases. Using this information and the reference tables, which color of visible light has the least energy? A. Red b. Yellow c. Green d. Violet 38. If an electron drops from n=6 to n=2, what type of electromagnetic radiation ...
Week 8 - Day 3 (End of Chapter 6)
... A chemical bond results from the overlap of two half-filled orbitals and spin-pairing of the two valence electrons (or less commonly the overlap of a completely filled orbital with an empty orbital). The geometry of the overlapping orbitals determines the shape of the molecule. ...
... A chemical bond results from the overlap of two half-filled orbitals and spin-pairing of the two valence electrons (or less commonly the overlap of a completely filled orbital with an empty orbital). The geometry of the overlapping orbitals determines the shape of the molecule. ...
chapter02_part1_lecture - bloodhounds Incorporated
... before the next higher level contains any electrons. ...
... before the next higher level contains any electrons. ...
study guide first semester chemistry
... 1. Write the balanced equation for the following: (include the state of each reactant and product) a. magnesium reacts with nitrogen to produce magnesium nitride. (3Mg(s) + N2(g) Mg3N2(s) b. silver nitrate reacts with copper to form copper(II) nitrate and silver. ...
... 1. Write the balanced equation for the following: (include the state of each reactant and product) a. magnesium reacts with nitrogen to produce magnesium nitride. (3Mg(s) + N2(g) Mg3N2(s) b. silver nitrate reacts with copper to form copper(II) nitrate and silver. ...
1 l 0 n = 1 → l = 0 n = 2 → l = 0, 1 n = 3 → l = 0, 1, 2 - Help-A-Bull
... Each line in the emission spectrum corresponds to the difference in energy between two energy states ...
... Each line in the emission spectrum corresponds to the difference in energy between two energy states ...
Chapter 8 Study Guide
... a. Chemists discovered that if two or more different compounds are composed of the same elements, the ratio of the masses of the second element is always a ratio of small whole numbers. This example illustrates the law of multiple proportions ...
... a. Chemists discovered that if two or more different compounds are composed of the same elements, the ratio of the masses of the second element is always a ratio of small whole numbers. This example illustrates the law of multiple proportions ...
Chemistry ~ Fall Final Review
... Properties of Matter: atoms/molecules, elements & compounds, chemical/physical changes History of the atom: models & scientists Wave calculations: properties of waves, energy, frequency, wavelength Electron configuration: orbital diagrams, electron configuration, shorthand notation Periodic Table: m ...
... Properties of Matter: atoms/molecules, elements & compounds, chemical/physical changes History of the atom: models & scientists Wave calculations: properties of waves, energy, frequency, wavelength Electron configuration: orbital diagrams, electron configuration, shorthand notation Periodic Table: m ...
Pure Substances and Mixtures
... • Pure substances contain only one kind of molecule. – Molecules are small groups of atoms that make up matter. Example: Water is a molecule of two hydrogen atoms, and one oxygen atom • Atoms are the smallest particles of elements ...
... • Pure substances contain only one kind of molecule. – Molecules are small groups of atoms that make up matter. Example: Water is a molecule of two hydrogen atoms, and one oxygen atom • Atoms are the smallest particles of elements ...
Chem 222 Intro to Inorganic Chemistry Summer 2011 Problem Set 3
... bonding interaction and a longer He-He distance. (c) Is either of these ions paramagnetic? The monocation [He2]+ has one unpaired electron, so it is paramagnetic. 11. (H&S 2.25c) Account for the observation that, in the salt formed from the reaction of Br2 and SbF5, the Br-Br bond distance in the Br ...
... bonding interaction and a longer He-He distance. (c) Is either of these ions paramagnetic? The monocation [He2]+ has one unpaired electron, so it is paramagnetic. 11. (H&S 2.25c) Account for the observation that, in the salt formed from the reaction of Br2 and SbF5, the Br-Br bond distance in the Br ...
Ch 8 AP Practice
... (a) Write the equation for the ionization of atomic fluorine that requires 1,681.0 kJ mol-1. (b) Account for the fact that the first ionization energy of atomic fluorine is greater than that of atomic oxygen. (You must discuss both atoms in your response.) (c) Predict whether the first ionization en ...
... (a) Write the equation for the ionization of atomic fluorine that requires 1,681.0 kJ mol-1. (b) Account for the fact that the first ionization energy of atomic fluorine is greater than that of atomic oxygen. (You must discuss both atoms in your response.) (c) Predict whether the first ionization en ...
Atoms and Elements Notes
... • An ion is formed when an atom gives up an electron and becomes positive (+) or an atom gains an electron an becomes negative (–) • An ionic bond is formed when two opposite charged atoms come in contact and stick to together. • This the strongest of the chemical bonds ...
... • An ion is formed when an atom gives up an electron and becomes positive (+) or an atom gains an electron an becomes negative (–) • An ionic bond is formed when two opposite charged atoms come in contact and stick to together. • This the strongest of the chemical bonds ...
Fall Exam 4 - Chemistry - University of Kentucky
... Starting with answer "1" on SIDE 1, fill in the circle indicating the one best answer for each of the 60 questions in this examination. Your score is the sum of the appropriate credit for each response. Soon after the examination is finished, an examination key will be posted on Blackboard. Grading ...
... Starting with answer "1" on SIDE 1, fill in the circle indicating the one best answer for each of the 60 questions in this examination. Your score is the sum of the appropriate credit for each response. Soon after the examination is finished, an examination key will be posted on Blackboard. Grading ...
Topic 1 Atomic Structure and Periodic Properties Atomic Structure
... Due to the high nuclear charge of heavy elements electrons close to the nucleus (s orbitals!) have a big velocity –> mass of electron increases –> effective size of orbital decreases (relativistic orbital contraction) –> energy of of electron is lowered The contraction of the s orbitals (and somewha ...
... Due to the high nuclear charge of heavy elements electrons close to the nucleus (s orbitals!) have a big velocity –> mass of electron increases –> effective size of orbital decreases (relativistic orbital contraction) –> energy of of electron is lowered The contraction of the s orbitals (and somewha ...
Molecular Geometry and Chemical Bonding Theory
... valence bond (VB) theory (Linus Pauling) and molecular orbital (MO) theory (Robert S. Mulliken). The molecular orbital theory does a better job of describing molecules in their ...
... valence bond (VB) theory (Linus Pauling) and molecular orbital (MO) theory (Robert S. Mulliken). The molecular orbital theory does a better job of describing molecules in their ...
Name: Period
... 3. What are the shapes of an s and p orbitals? 4. What is a principal energy level, sublevel and atomic orbital? 5. What is the maximum number in each s, p, d and f orbitals? 6. What types of atomic orbitals are in the 1st, 2nd and 3rd principal energy levels? 7. If the spin of one electron is clock ...
... 3. What are the shapes of an s and p orbitals? 4. What is a principal energy level, sublevel and atomic orbital? 5. What is the maximum number in each s, p, d and f orbitals? 6. What types of atomic orbitals are in the 1st, 2nd and 3rd principal energy levels? 7. If the spin of one electron is clock ...
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.