Chemistry: A Molecular Approach (Tro) Chapter 10 Chemical Bonding II: Molecular Shapes‚ Valance Bond Theory‚ and Molecular Orbital Theory 1) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A) eg=trigonal planar‚ mg=trigonal planar B) eg=tetrahedral‚ mg=trigonal planar C) eg=tetrahedral‚ mg=trigonal pyramidal D) eg=trigonal planar‚ mg=bent E) eg=trigonal bipyramidal‚ mg= trigonal bipyramidal Answer: A 2) Determine
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function with the coordinates of its 3d space position ~ A wave function is called an orbital (this is not the Bohr orbit) ~ The Hydrogen electron in a 1s orbital is not moving around the nucleus in a circular orbit ~ It is still unknown how electrons are moving 1. Principle Quantum Number ~ represented by the letter "n" ~ it can only have positive integer values ~ n determines the size of the orbital ~ it is the energy level in the electron configuration 2. Angular Momentum Quantum
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Atomic radii • Ingoing from top to bottom of a group‚ the outermost electrons are assigned to orbitals with increasingly higher values of the principal quantum number. The underlying electrons require space so the electrons of the outer shell is farther from the nucleus. • In a period‚ going across the period‚ a proton is added to each nucleus and an electron is added to each outer shell. In each‚ the effective nuclear charge increases slightly because the effect of each additional proton is more
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therefore required three coordinates‚ or three quantum numbers‚ to describe the orbitals in which electrons can be found. The three coordinates that come from Schrödinger’s wave equations are the principal (n)‚ angular (l)‚ and magnetic (m) quantum numbers. These quantum numbers describe the size‚ shape‚ and orientation in space of the orbitals on an atom. The principal quantum number (n) describes the size of the orbital. Orbitals for which n = 2 are larger than those for which n = 1‚ for example. Because
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SCH4U-C 1 UNIT Structure and Properties of Matter Unit 1 Introduction Chemisty SCH4U-C Table of Contents Unit 1: Structure and Properties of Matter Lesson 1: Atomic Structure Lesson 2: Introduction to Chemical Bonding Lesson 3: Molecular Shape and Polarity Lesson 4: Intermolecular Forces and Their Applications Unit 2: Organic Chemistry Lesson 5: Saturated Hydrocarbons Lesson 6: Unsaturated Hydrocarbons Lesson 7: Functional Groups Lesson 8: Acids‚ Esters‚ Amides
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energy level‚ there may be several orbits with different shapes and at different energy levels. Each energy sublevel corresponds to an orbital of a different shape which describes where the electron is likely to be found S orbital are spherical (circle)‚ and p orbitals are dumbbell-shaped. D orbitals have four clover leaf shapes. # and kinds of atomic orbitals depends on the energy sublevel. B. Electron Arrangement in Atom i. Electron Configurations The way in which electrons are
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class of operation χ(IR): the corresponding character in the irreducible representation ai CHEM 331 – 2014 Dr. Roland Roesler 8-4 MO Theory: Polyatomic Molecules H2 O The LCAO (Linear Combination of Atomic Orbitals) for the 2 H atoms under C2v symmetry is assessed (two 1s orbitals). Γ2H(1s) 2 0 0 2 This
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frequency 18. Calculations with energy‚ wavelength‚ and frequency 19. Dual nature of light and photoelectric effect 20. Electron’s energy is quantized‚ meaning that electrons jump by steps of QUANTA 21. Electron’s configuration a. electrons are in orbitals – place of higher probability of finding the electrons in an atom b. the four quantum numbers: n‚ l‚ m‚ s c. main energy level of an electron is
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Topic: Atomic Orbitals 1. A) B) C) D) E) In quantum mechanics a node (nodal surface or plane) is: a place where Ψ is negative. a place where Ψ is positive. a place where Ψ = 0. a place where Ψ2 is large. a place where Ψ2 is negative. Ans: C Topic: Atomic Orbitals‚ Molecular Orbitals 2. When the 1s orbitals of two hydrogen atoms combine to form a hydrogen molecule‚ how many molecular orbitals are formed? A) 1 B) 2 C) 3 D) 4 E) 5 Ans: B Topic: Atomic Orbitals 3. Which principle(s)
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Chemistry Final Study Guide Matter as anything that has mass and takes up space. Significant figures refers to digits that were measured. When rounding calculated numbers‚ we pay attention to significant figures so we do not overstate the accuracy of our answers. Rules: -All nonzero digits are significant. -Zeroes between two significant figures are themselves significant. -Zeroes at the beginning of a number are never significant. -Zeroes at the end of a number are significant if a decimal
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