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General Chem
General Chem
General Chem
General Chem
General Chem
100
Bonds overview
What is Atoms join to form molecules because atoms like to have a full outer shell of electrons. Usually means 8 electrons in outer shell.
100
Ionic bond
What is -Solid held together by electrostatic attractions between ions that are next to one another in a lattice structure. -Often occur between metals and nonmetals. -Electrons are NOT shared. -One atom gives up electrons and becomes a positively charged ion while the other accecpts electrons and becomes a negatively charged ion. -Due to Coulomb's law, an ionic bond between +2 and -2 is stronger than +1 and -1 charges. -The smaller the ions in an atomic bond, the stronger the bond because a small electronic radius allows charges to get closer together and increases the force between them. -Each electron is localized around a particular atom, so electrons don't move around the lattice, making these solids poor conductors of electricity -These liquids do conduct electricity because the ions themselves are free to move about in the liquid phase. -Hold salts together
100
Covalent bond
What is -Two atoms share electrons. Each atom counts the shared electrons as part of their valance shell. Both atoms complete their outer shells. -An atom can form as many covalent bonds as it has numbers of electrons in its valance shell. -The first covalent bond formed between two atomsis called a sigma bond. All single bonds are sigma bonds. -If additional bonds between atoms are formed, they are called pi bonds. The second bond in a double bond is a pi bond and the second and third bonds in a triple bond are also pi bonds. Double and triple bonds are stronger and shorter than single bonds, but not 2 or 3 times as strong
100
Single bond
What is Bond designation: 1 sigma -Bond order: one -Bond length: longest -Bond energy: least
100
Double bond
What is Bond designation: 1 sigma and 1 pi -Bond order: two -Bond length: intermediate -Bond energy: intermediate
200
Triple bond
What is -Bond designation: 1 sigma -Bond order: three -Bond length: shortest -Bond energy: greatest
200
Polarity
What is separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment. Polar molecules interact through dipole–dipole intermolecular forces and hydrogen bonds.
200
Ionic bond strength
What is strength based on Coulombs law, a greater charge means more energy. smaller ions will have greater coulombic attraction.
200
Coulombic attraction
What is how much two particles are electrically attracted
200
Ionic properties
What is how much two particles are electrically attracted
300
Metallic bond properties
What is delocalized electron structure so it is a good conductor and also malleable and ductile.
300
Interstitial alloy
What is metals with two vastly different radii combine like steel (small carbon and big iron)
300
Substitutional alloy
What is Metal atoms with similar radii like brass (zinc and copper)
300
Covalent bond names
What is first is the sigma bond then additional are pi bonds. so for a triple bond thats 1 sigma and two pi bonds.
300
Polarity
What is one atom is more electronegative will pull more electrons making a dipole
400
Intermolecular forces
What is only exist in covalent bonds
400
Rate law
What is Describes the dependence of the initial rate of a reaction on the concentrations of reactants
400
Rate law form
What is RATE = k[A]^x [B]^y
400
First order reaction law
What is Ln[A] t = -kt +Ln[A]o
400
Second order reaction law
What is 1/[A] = -kt + (1/[A]o)
500
Zero order reaction law
What is [A] = kt + [A]0
500
Collision theory
What is 1. The molecules must collide 2. They must collide with enough energy to overcome the activation energy. 3. They must collide with the proper orientation of each molecule.
500
Beer's law
What is A =abc. A= Absorbance, a= molar absorbitivity (a constant) b=path length c= concentration of solution
500
Intermediates
What is chemicals that appear in the mechanism, but cancel out of the balanced equation.
500
Dipole
What is Molecular dipoles occur due to the unequal sharing of electrons between atoms in a molecule. Those atoms that are more electronegative pull the bonded electrons closer to themselves.