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41 Cards in this Set
- Front
- Back
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Elements form ______ and are held together by _______ |
*Molecules *Chemical bonds (by interaction of valence electrons) |
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Which are weaker intermolecular forces or intramolecular foces |
Intermolecular foces are wekaer than intramolecular chemical bonds |
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What does the octet rule state |
Bonds will ahve 8 electrons in the outermost shell Except: H, He (2 valence electrons), Li and Be (2 and 4 valence electrons), B (6 valence electrons) and elements beyond the 2nd row (IE P and S)expand octet to more than 8 to incorporate d orbitals |
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What are ionic bonds |
1 or more electrons from an atom with a smaller IE are transferred to an atom with a higher electron affinity and held together by electrostatic force (Difference in EM is greater than 1.7) The one which loses an electron = cation The one who gains an electron = anion |
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What is covalent bonding |
Electrons are shared between 2 atoms |
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What is polar covalent |
Partially covalent and ionic |
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What are the physical properties of ionic bonds |
Form crystal lattices in which attractive forces between ions are maximum and repulsive forces are minimum High melting point and high boing point because of strong electrostatic forces can conduct electricity in liquid and aqueous states |
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Do covalen bonds have stronger or weaker intermolecular forces than ionic bonds |
Weaker |
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Do covalent bonds have high or low melting points |
Low |
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Do covalent bonds conduct electricity? |
No |
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What is bond length |
Average distance between nuclei of atoms |
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When there is a higher amount of shared electrons are atoms pulled closer together or further apart? |
Closer together |
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Which is longer single, double or triple bond?
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Single |
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Which is shorter single, double or triple bond?
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Triple |
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What is bond energy? |
Energy to separate bond? |
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If there are more shared electrons does that lead to a higher or lower bond energy? |
Higher |
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Practice drawing lewis structure |
X |
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How do you find the formal charge |
VE - (1/2 Bonding) - Non bonding electrons |
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How do you find the formal charge of the molecule |
Sum of the formal charges of all of the element |
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The more stable the resonance structure does it have less or more contribution |
More |
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What sort of resonance structure is preferred
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A lewis structure with small or no formal charge perferred Negative formal charge on electronegative atoms |
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What are the types of covalent bonds
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Polar covalent Nonpolar Coordinate covalent |
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What is a polar covalent bond |
Small difference in electronegativity Electrons are pulled towards the more electronegative and other atom has a partial positive |
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How do you calculate the dipole moment of a polar covalent molecule |
(charge)(radius between the two atoms) |
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What is a nonpolar covalent bond |
Same electronegativity between elements (O2) |
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What is a coordinate covalent bond? |
Lewis acid (accepts an electron pair) and lewis base |
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What does polar mean? |
Molecule with dipole moment |
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If a polar molecule is oriented so the dipole moments cancel out what is it |
Nonpolar |
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If a polar molecule is oriented so that the dipole moment doesn't cancel out what is it?
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Polar |
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What is the aximuthal quantum number |
l |
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How many possible orbitals does l = 1 have |
3 possible orbitals (-1, 0, +10 Px, Py, Pz which are perpendicular to each other |
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When two atoms are bundled what do the atomic orbitals interact to form? |
Molecular orbitals |
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If the signs of 2 atomic orbitals are the same what does it create |
Bonding orbital |
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If the signs of 2 atomic orbitals are not the same what does it create? |
Antibonding orbital |
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A head to head p orbital overlap creates what |
Sigma bond |
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A parallel p orbital overlap creates what |
Pi bond |
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What is the ranking for intermolecular forces |
Dipole-ion > H bond > Dipole-dipole > LDF |
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What is dipole-dipole interactions |
Polar molecules orient so positive is to negative of other atom so attractive dipole forms In solid and liquid phase Polar molecules have high boiling points than nonpolar molecules |
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What is hydrogen bonding |
Hydrogen bonded to F, O or N interacts with the partially negative EN atoms such as F, N or O |
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Yes |
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What is dispersion force |
Bonding electrons located randomly through orbitals have unequal sharing of electrons These dipoles interact with electrons of neighboring molecules Short lived and weaker |
