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9 Cards in this Set
- Front
- Back
- 3rd side (hint)
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What are the three electron orbital rules? |
Aufbau Principle: electrons must fill each orbital in order of atomic number. Hund's Rule: Each orbital of a subshell must be singly occupied by an electron before pairing with another. Pauli Exclusion: There must only be two electrons in an orbital, and they must have opposite charge. |
Aufbau Principle: Hund's Rule: Pauli Exclusion: |
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What does VSEPR Theory stand for? What does it state? |
Valence Shell Electron Pair Repulsion. States that lone pairs repel the most out of electron pairs. Bonded electron pairs repel the least. |
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What is the equation for the formal charge of an atom? |
# of valence electrons - (bonded pairs + lone electrons) |
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What does Hess' Law state? |
Hess' Law states that you can find an unknown enthalpy through the addition of thermochemical equations to find the desired enthalpy value. |
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Energy is required to break bonds, therefore: |
It is endothermic |
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Bond making releases energy, therefore |
Exothermic |
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What is the standard enthalpies of formation? |
It is the enthalpy change of a reaction that forms one mole of a compound from its elements, with the reactants in their standard states. |
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What are the variables that affect reaction rates? |
Concentration of reactants - More reactant molecules = greater the rate of reaction Presence of a catalyst Temperature Surface Area of a solid reactant Nature of the Reactants |
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What are the strong acids? |
HI HBr HCl HNO3 HNO4 H2SO4 HCLO4 HNO3 |
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