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Partial 2 Review

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  • Possible values of n
    1,2,3,4,5,6,7
  • Are ionic bonds able to make double and triple bonds?
    No, that only occurs with covalent bonds.
  • There are 3 types of intramolecular bonds. What are their names?
    Ionic, metallic, and covalent
  • Describe London dispersion forces and name at least 1 characteristic of them.
    -
  • Covalent is nonmetal + nonmetal?
    Yes! 🥳
  • Complete: There are 2 types of covalent bondings: the ______ and the ___-______.
    polar and non-polar
  • Covalent bondings are the ones where electrons are stolen?
    No, they have a healthy relationship. They always SHARE.
  • True or false: Electronegativity difference ≥ 0.5 and ≤ 1.6 is related to polar covalent compounds.
    True!
  • What is the state of matter of salts at room temperature?
    Solid
  • Possible values of quantum number "l"
    0,1,2,3 (s,p,d,f)
  • This quantum number represents the orientation of the orbital
    m (Magnetic quantum number)
  • There are 4 quantum numbers. They are:
    n, l, m, s.
  • True or false (justify): The 118 elements require to have 8 electrons in the valence shell to be stable.
    No, not all of them.
  • Possible values of The spin quantum number
    -1/2, +1/2
  • Describe dipole-dipole and name at least 1 characteristic of them.
    -
  • In electron configuration, what does the Pauli's exclusion principle indicates?
    The position of electrons within an atom cannot be the exact same (at least 1 quantum number's value will be different)
  • In the class we reviewed 3 main types of intermolecular forces. What are their names?
    Hydrogen bonds, dipole-dipole, and London dispersion forces.
  • True or false: Electronegativity difference ≤ 1.7 is related to non-polar compounds.
    True!
  • This quantum number specifies the energy level where an orbital is located.
    n (principal quantum number)
  • What is the difference between intermolecular and intramolecular bonds?
    -
  • True or false (justify): For covalent bonds, it's mandatory to previously have charges (ions).
    False, that happens in ionic and metallic bondings.
  • Describe Hydrogen bonds and name at least 1 characteristic of them.
    -
  • The type of molecule product of an ionic bond is known as...?
    Salt
  • In electron configuration, what does the Hund's rule indicates?
    The electrons must be drawn first unpaired and then paired, because they have repulsion forces and will first occupy empty orbitals
  • Complete: the electrons have 2 states: the _______ state, and the _______ state.
    ground state and excited state.
  • This quantum number specifies the shape of an orbital and is basically the path to follow for an electron.
    l (angular momentum quantum number)
  • True or false: The positions in the Aufbau diagram indicate the orbitals in an atom
    True!🥸☝️
  • True or false: Electronegativity difference ≥ 1.7 is related to ionic compounds.
    True!
  • True or false (justify): An orbital is a two-dimensional region where an electron is the 90-95% of times.
    False, because...
  • Do atoms are more stable separated or bonded to another atoms?
    When they are bonded.
  • This quantum number represents the direction the electrons move around their own axis.
    s (Spin quantum number)
  • Are non-metals less electronegative than metals?
    No, actually METALS are less electronegative🥸☝️
  • Complete: every atom is divided into: level (shell), __________, and orbitals.
    sublevel (or subshell)
  • Possible values of quantum number "m"
    -3,-2,-1,0,1,2,3
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