Chapter 11: States of Matter and Intermolecular Forces
Note: I will be focusing on the concepts in a qualitative manner. You will not need to do any
calculations in this chapter.
11.1 And 11.2: Solids, liquids, gases and their phase transitions.
First a r
Chapter 10 notes part 3 and bonds - bonds are made from hybrid orbitals. There can only be ONE sigma bond between two atoms. - bonds are made from the overlap of unhybridized p orbitals. In a double bond (like the C-C double bond in ethene), one of the bo
Chapter 10 notes part 2 10.2 dipole moment and molecular geometry - dipole moment: a quantitative measure of charge separation in a molecule. - e-'s are polarized in the direction of the more electronegative atom in a chemical bond (ie closer to the more
Chapter 1 Notes-Chemistry and Measurement Ebbing and Gammon 9th Edition I. What is chemistry? A. The study of matter and the changes which matter undergoes.
Fall 2101 Chem 0110
1. Elements are the simplest form of pure matter as defined in chemistry. 2. E
11.4 Surface Tension and Viscosity Surface tension: The energy needed to increase the surface area of a liquid by a unit amount (J/m2) Examine figure 11.16 in your text. - A molecule beneath the surface of a liquid is attracted to liquid molecules in all
Chapter 9: Ionic and Covalent Bonding
9.1 Ionic Bonds: electrostatic attractions between ions (+ and -)
Anions: Lewis dot structures: show the number of valence electrons around an atom. (see table
- For the Main Group elements, the number
9.10 Bond Length and Bond Order
Bond Length: the distance between two nuclei (of two atoms)
Covalent Radii: are values (in picometers) assigned to atoms for single bonds (see table
9.4) on page 358. The sum of two covalent radii is equivalent to the appro
9.5 Polar Bonds and Electronegativity
- Polarity refers to the separation of charge, and in the class we will be refering to covalent
- Electrons are not always shared equally in covalent bonds
- if the electrons are shared equally, then the covale
Chapter 8 Electron Configurations and Periodicity Electrons form bonds and therefore the study of their spacial distribution around an atom is extremely important in forming bonds, namely the valence electrons (the electrons in the outermost orbital (subs
Chapter 7: The Quantum Theory of the Atom
To understand the formation of chemical bonds we need to have an understanding of electrons,
the sub-atomic particles that create them. Light gives us information about chemical and
molecular structure so we will
Chapter 6: Thermochemistry 6.1 Thermochemistry: studies the release or absorption of heat in a chemical or physical process - Energy: the potential or capacity to do work. - E is not a material thing but a property of matter and can be interconverted from
4.2 Molecular and Ionic Equations Molecular equations: a chemical equation where all reactants and products are written as molecules (even though they may exist as ions in solution) Ca(OH)2 (aq) + Na2CO3 (aq) CaCO3 (s) + 2NaOH (aq) Complete Ionic Equation
Chapter 3 notes part 2
3.6 Molar Interpretation of a chemical equation
Mole Relationships in Chemical Equations
o The Law of Conservation of Mass says Matter is neither created or destroyed in
chemical reactions. There fore, the total mass of reactants m
Chapter 2 notes part 3 /Chapter 3 notes part 1 Hydrates and naming Chemical compounds (mostly ionic) that contain H2O water in weakly bound to it's solid crystalline structure. See table 2.8n in your textbook MgSO4 * 5H2O Magnesium sulfate pentahydrate o
CHEM 0110 General Chemistry I
1.1 Introduction: The world around us has been changed by chemistry and chemicals.
1. The Discovery of the New World (nutmeg, pepper and cloves)
Preservation of perishable food was difficult.
Chapter 2: Water and Carbon Chemical Evolution-leading scientific explanation for the origin of life -Pattern Component: simple chemical compounds combined to form more complex carbon containing substances -Process Component: complex carbon containing com