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Theories - doubly occupied and all electrons singly...

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Kinetic Molecular Theory: all matter consists of extremely tiny particles (atoms, molecules, or ions). The higher the temperature the faster the particles move. Their kinetic energy acts to overcome the forces of attraction between particles. De Broglie proposed that a free electron of mass m moving with a velocity v should have an associated wavelength. Electrons can be described as having wave-like properties. Uncertainty Principle – it is impossible to fix the position of an electron in an atom and its energy with any degree of certainty. Pauli Exclusion Principle – no two electrons can have the same set of quantum numbers. No atomic orbital can contain more than two electrons. Auf Bau Principle – how atom is built - build up an electronic configuration by putting each electron in the lowest energy orbital possible. Electrons will enter lower energy orbitals first, and then will fill higher energy orbitals as the lower energy ones are already taken. Hund’s Rule – every orbital in a subshell is singly occupied with one electron before any one orbital is
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Unformatted text preview: doubly occupied, and all electrons singly occupied have the same spin. Isoelectronic – having the same number of valence electrons and the same lewis dot structures. Theory of resonance – different ways of drawing the lewis dot structure. Valence Shell Electron Pair Repulsion (VSEPR) – bond and lone electron pairs in the valence shell of an element repel each other and seek to be as far apart as possible. Valence Bond Theory – qualitative, visual picture of molecular structure and bonding. Describe molecules in lower energy states. Molecular Orbital Theory – used when a more quantitative picture of bonding is needed. Describe molecules in higher energy states. Boyle’s Law – pressure and volume, number of moles is constant. Inverse relationship between P and V. Charles’s Law – volume and temperature. Direct relationship. Avogadro’s Law – n1/v1=n2/v2...
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