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Unit 11: Bonding
Guiding Questions:
- What is that?
- How do we figure out what the chemical formula is?
- What does it mean to be "free of chemicals"?
- Why are some thing liquids at room temperature and other things gases or solids?
- How are shapes of molecules determined?
- How do Splenda and other artificial sweeteners work?
- How do bees tell the difference between a worker and the queen?
What you should learn:
- Chemical formulas can be predicted from the periodic table and allow chemists to classify and predict properties of compounds
- The general trend in the universe to strive for lower energy explains and allows for prediction of chemical properties of elements
- Elements combine in whole number ratios and these molar ratios can be used to determine chemical formulas
- The shape of a molecule can be used to predict the properties of that molecule.
- The shape of a molecule is determined by the electron arrangement of the atoms that make up the molecule
More Specifically...:
IB Objectives: SL
Option
HL
- Covalent Bonding Model
- Define covalent bonding as a bond in which electrons are shared
- Use electronegitivity difference to distinguish between ionic, polar and non-polar bonds
- Contrast the intermolecular forces exhibited by ionic, polar, and non-polar bonds (all are weaker than covalent bonds. For similar molar mass, h-bonds are stronger than dipole-dipole which are stronger than Van der Waals)
- a. ion-dipole interactions,
- b. dipole-dipole interactions,
- c. Hydrogen bonds and
- d. London dispersion forces
- Use intermolecular forces to explain and predict IBH 4.5.1-2
- a. state of matter at room temperature
- b. viscosity
- c. volatility
- d. boiling point IBH 4.3.2
- i. Compare H2O and H2S,
- ii. NH3 and PH3,
- iii. C3H8, CH3CHO, and C2H5O5
- e. freezing point
- f. vapor pressure
- g. solubility and miscibility using the rule "Like dissolves like"
- Draw Lewis structures for covalent compounds including resonance structures. Specifically O2, N2 CO2, C2H4, C2H2
- State and explain the relationship between the number of bonds, bond length, and bond strength. The comparison should include bond length and bond strings of IBH 4.2.3
- a. Two carbon atoms joined by single, double, and triple bonds
- b. The carbon atom and the two oxygen atoms in the carboxyl group of carboxylic acid
- State that bonds form when orbitals overlap
- Briefly describe hybridization of orbitals in methane
- Use the VSEPR (Valence Shell Electron Pair Repulsion) model to predict the geometric shape and bond angles of simple molecules and polyatomic ions
- a. bent, linear, trigonal planar, tetrahedral, and trigonal pyramidal
- Construct models of molecules and polyatomic ions to illustrate their predicted geometric shapes
- Predict the polarity of molecules by using the VSEPR model for molecules containing polar covalent bonds
- Ionic Bonding Model
- Use physical and chemical properties to distinguish between ionic and covalent compounds
- Describe energy changes as elements combine to form an ionic compound
- Describe ionic bonding as the transfer of electrons and the formation of a crystal lattice due to electrostatic attraction between ions of opposite charge
- Predict the formation of cations and anions based on placement on periodic table
- State that transition metals can form more than one ion
- Relate formation of anion or cation with ionization energy and electron affinity
- State that bonding occurs to increase stability
- Contrast metallic and ionic bonding
- Describe the metallic bond formation and explain the physical properties of metals (delocalized electrons = high conductivity, malleability, ductility)
Lecture Notes:
Assignments:
Labs:
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