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Chem Exam 4
Chapters 7-9
| Question | Answer |
|---|---|
| What are the 3 types of chemical bonding | Ionic, Covalent, Polar Covalent |
| Ionic Bonding | Complete transfer of valence electrons between atoms |
| Covalent Bonding | equal sharing of valence electrons between atoms |
| Polar Covalent | Mix of Ionic and Covalent Bonding |
| Electronegativity | Ability of atom to attract atoms towards it |
| Covalent Electronegativity | 0-0.4 |
| Polar Covalent Electronegativity | 0.4-2 |
| Ionic Electronegativity | 2- infinity |
| What is the primary consideration in determining bond type | Electronegativity |
| Br2 | Non-Poplar Covalent |
| CsCl difference 2.6 | Ionic |
| H2S Difference .4 | Non polar covalent |
| Metallic | 2 of the same metal combined |
| ionic Compound | Bond via electrostatic Forces |
| Isoelectronic | What element e- adds up to |
| Isoelectronic Li+ and F- | [He][Ne] |
| Lattice Energy (u) | energy required to completely separate one mole of a solid ionic compound into gaseous ions |
| Covalent bond occurs | when 2 identical nonmetals bond together |
| Why would 2 atoms want to share e- | to fill e- configuration and get the octet rule |
| Electronegativity increases | Up and to the Right |
| Group 4A Lewis Dot Structure | 4 single bonds |
| Group 5A Lewis Dot Structure | 3 single bonds and 1 lone pair |
| Group 6A Lewis Dot Structure | 2 single bonds and 2 lone pairs |
| Group 7A Lewis Dot Structure | 1 single bond and 3 lone pairs |
| Exceptions to the Octet Rule | Incomplete and Expanded |
| Incomplete Exception | Be:4 B: 6 |
| Expanded | period 3 and down can have more electrons than 8 |
| Resonance Structure | 1 of 2+ Lewis Structures for a single molecule that cant be represented accurately by only one Lewis Structure |
| How do you create a different resonance structure | by moving a bond and lone pair |
| Formal Charge | Charge on an atom in a molecule |
| Sum of All formal charges equals | the overall charge of the molecule/ Polyatomic Ion |
| Formal Charge Formula | (# of Valence E-) minus (#of unpaired e-) minus (1/2* number of paired e-) |
| Bond Enthalpy | enthalpy charge for breaking a particular bond in a mole of gaseous substance |
| What is bond enthalpy used for | approximate value for change in H |
| Bond Enathlpy formula | Bond Energy reactants- Bond energy products |
| 2 regions | Linear |
| 3 regions | Trigonal Planar |
| 4 regions | Tetrahedral |
| 5 regions | Trigonal Bipyramid |
| 6 regions | Octahedral |
| 2 single bonds and 1 lone pair | Bent |
| 3 regions and one lone pair | Trigonal Pyramid |
| Non Polar | Even distribution |
| Polar | Uneven distribution |
| Vesper predicted geometric shapes is the same as | Base Geometry |
| Valence Bond Theory | describes covalent bond as the overlap of half-filled atomic orbitals (each contain single electron) that yield a shared pair of electrons |
| 3 Types of Hybridization of Atomic Orbitals | SP3, SP2, SP |
| SP3 | 1s and 3P mixed to form 4 different hybrids |
| SP2 | 1s and 2P mixed to form 3 different hybrids |
| SP | 1s and 1P mixed to form 2 different hybrids |
| Linear Vesper | SP |
| Trigonal Planar Vesper | SP2 |
| Tetrahedral Vesper | SP3 |
| Sigma Bond | e- density between 2 atoms |
| pi bond | e- density up and down plane of nuclei of bonding atoms |
| Single bond has | 1 sigma bond |
| Double Bonds has | 1 sigma bond and 1 pi bond |
| Triple Bond has | 1 sigma bond and 2 pi bonds |
| What is the most excitable and chaotic state of matter | Gas |
| What is the most compressive state of matter | gas |
| Which state of matter has the highest density | solid |
| 4 variables gas properties depend on | Volume (mL or L), Temperature (K), Amount of gas (moles), Pressure (atm, kPa, mmHg) |
| Pressure equals | force/area |
| Force equals | mass * acceleration |
| combined Gas Law Formula | PV/T=PV/T |
| Polarity | distribution of e- around a central atom |
| Ideal Gas Law | PV=nRT |
| Ideal Gas law variables explained PVnRT | Pressure, Volume, Moles, Temp, Ideal Law Constant |
| Density | mass per liter of volume |
| STP | gas is 0 degrees Celsius and 1atm |
| Daltons Law of Partial Pressure | at a constant Volume and Temp, P1 + P2 = Ptotal |
| Kinetic Molecular Theory 4 rules ( distance, motion/collision, forces, Kinetic Energy) | gas molecules far apart, Molecules in constant motion in random directions-collisions are perfect elastic, gas molecules exert neither attractive nor repulsive forces on eachother, Average KE of the molecules are proportional to temp of gas in Kelvin |
| Diffusion | Gradual mixing of molecules of different gases such as Skunk Spray |
| Effusion | Movement of molecules through a small hole (balloon) |
| Velocity of Gas | smaller the mass the faster the molecules move |
| Deviations from Ideal Gas Law | Pressure and Temp |
| Phase Diagram | conditions at which a substance exists as solid, liquid, or gas |
| Non Ideal | High Pressure and Low Temperature |
Created by:
brkolstoe
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