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31 Cards in this Set
- Front
- Back
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Bond Length
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is the separation between two bound atoms at the position of minimum energy.
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The H-H bond is short because the atoms are ______, whereas the I-I bond is long because the atoms are ______.
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The H-H bond is short because the atoms are small whereas the I-I bond is long because the atoms are larger.
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Most bond lengths lie between ____ and _____ angstroms
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1 and 3 angstroms
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If the electronegativities of two atoms in a bond are different, then the bond is ____.
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polar
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The presence of a positive and a negative pole in a covalent bond produces a ___________.
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bond dipole.
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A covalent bond with a bond dipole is said to be a ____________.
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polar covalent bond.
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A covalent bond with no bond dipole is a _________________.
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purely covalent bond.
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Polar bonds have bond dipoles, which are represented with arrows pointing from the poitive pole (_____electronegative atom) toward the negative pole (______electronegative atom) with a line is through the positive end.
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less, more
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percent ionic character
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increases as the electronegativity difference between the bound atoms increases.
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Ionic bonds form between metals (___________) and nonmetals (______________)
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low electronegativity, high electronegativity
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How to measure a covalent bond?
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0.0-0.4 = nonpolar covalent bond
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how to measure polar covalent bond?
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0.4-1.7 = polar covalent bond
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how to measure ionic bond
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electronegativity greater than 1.7
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Lewis structures should never show double or triple bonds to _______ or to a ________
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hydrogen, halogen
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compounds with _________ usually have ______ boiling points than similar compounds without hydrogen bonding
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compounds with hydrogen usually have higher boiling points than similar compounds without hydrogen bonding
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____________ usually have _________that have greater dispersion forces than lighter compounds
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heavier compounds usually have higher boiling points that have greater dispersion forces than lighter compounds
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___________ usually have _______ boiling points than non-polar compounds
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polar compounds usually have higher boiling points than non-polar compounds
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bond order = ________/_______________
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number of shared pairs/number of bonding regions
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A common misconception among students is that molecules have bond orders. They do not; bonds have bond orders
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A common misconception among students is that molecules have bond orders. They do not; bonds have bond orders
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When do resonance structures form?
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when the number of shared pairs exceeds the number of identical bonding regions in which they can be placed.
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It is incorrect to state that the bond order of SO2 is 1.5. Restate this sentence correctly.
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The bond order of each bond in SO2 is 1.5.
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if the bonds are covalent the resulting charge on the atom is called its _______ _______.
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formal charge
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If the bonds are assumed to be ionic the charge is the atom's _______ ______
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oxidation state
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The boiling point of a liquid ________ as the ________ increases.
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The boling point of a liquid increases as the pressure increases.
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Describe the relative strengths of the intermolecular forces.
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dispersion forces < dipole-dipole interactions < hydrogen bonds
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dipole dipole interaction only occurs between molecules that are _____
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polar
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The bond angles are the __________around the atom with the smaller number of electron groups
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greatest
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The bond angles are the greatest around the atom with the ________ number of electron groups
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smaller
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what do solid thin lines represent?
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bonds that lie in the plain of the paper
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what do dashed wedges indicate?
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bonds that extend behind the plane of the paper
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what do solid wedges show?
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bonds that extend outside of the plane of the paper
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