# Samuels CHEM Quantum Numbers: Question Preview (ID: 31587)

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How many quantum numbers are there? |
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a) 4 | b) 3 | c) 2 | d) 1 | |

The principle quantum number is symbolized by ______. |
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a) n | b) l | c) m | d) +½ or -½ | |

The angular momentum quantum number is symbolized by ______. |
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a) l | b) m | c) n | d) +½ or -½ | |

The magnetic quantum number is symbolized by ______. |
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a) m | b) l | c) n | d) +½ or -½ | |

The spin quantum number is symbolized by ______. |
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a) +½ or -½ | b) m | c) l | d) n | |

This states that each electron occupies the lowest energy orbital available first. |
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a) Aufbau principle | b) Pauli exclusion principle | c) Hund’s rule | d) Heisenberg's principle | |

This states that a maximum of two electrons may occupy a single orbital sublevel only if electrons have opposite spins. |
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a) Pauli exclusion principle | b) Aufbau principle | c) Hund’s rule | d) Heisenberg's principle | |

This states that single electrons with same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy same orbital. |
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a) Hund’s rule | b) Pauli exclusion principle | c) Aufbau principle | d) Heisenberg’s principle | |

This indicates the main energy level occupied by the electron (1, 2, 3, 4…) |
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a) principle quantum number | b) angular momentum quantum number | c) magnetic quantum number | d) spin quantum number | |

This represents shape or type of orbital that corresponds to particular suborbital (s, p d, f) |
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a) angular momentum quantum number | b) magnetic quantum number | c) principle quantum number | d) spin quantum number | |

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