Term
| These bonds are arranged in order of increasing polarity C-H < N-H < O-H |
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Definition
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Term
| All atoms in a contributing structure must have a complete valence shell |
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Definition
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Term
| An electron in a 1s orbital is held closer to the nucleus than an electron in a 2s orbital. |
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Definition
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Term
| A sigma bond and a pi bond have in common that each can result from the overlap of atomic orbitals. |
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Definition
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Term
| The molecular formula of the smallest aldehyde is C3H6O, and that of the smallest ketone is also C3H6O. |
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Definition
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Term
| To predict whether a covalent molecule is polar or nonpolar, you must know both the polarity of each covalent bond and the geometry (shape) of the molecule. |
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Definition
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Term
| An orbital is a region of space that can hold two electrons. |
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Definition
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Term
| In the ground-state electron configuration of an atom, only the lowest-energy orbitals are occupied. |
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Definition
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Term
| Electronegativity generally increases with atomic number. |
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Definition
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Term
| Paired electron spins means that the two electrons are aligned with their spins North Pole to North Pole and South Pole to South Pole. |
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Definition
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Term
| According to the Lewis model of bonding, atoms bond together in such a way that each atom participating in the bond acquires on outer-shell electron configuration matching that of the noble gas nearest it in atomic number. |
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Definition
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Term
| A primary amine contains on N – H bond, a secondary amine contains two N – H bonds, and a tertiary amine contains three N – H bonds. |
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Definition
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Term
| All bond angles in sets of resonance contributing structures must be the same. |
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Definition
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Term
| Electronegativity is a measure of an atom’s attraction for electrons it shares in a chemical bond with another atom. |
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Definition
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Term
| An orbital can hold a maximum of two electrons with their spins paired. |
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Definition
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Term
| Fluorine in the upper right corner of the Periodic Table is the most electronegative element; hydrogen, in the upper left corner, is the least electronegative element. |
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Definition
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Term
| A primary alcohol has one – OH group, a secondary alcohol has two – OH groups, and a tertiary alcohol has three – OH groups. |
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Definition
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Term
| H2O and NH3 are polar molecules, but CH4 is nonpolar. |
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Definition
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Term
| Electronegativity generally increases from top to bottom in a column of the Periodic Table. |
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Definition
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Term
| The letters VSEPR stand for valence-shell electron pair repulsion. |
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Definition
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Term
| In predicting bond angles about a central atom in a covalent bond, VSEPR considers only shared pairs (pairs of electrons involved in forming covalent bonds). |
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Definition
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Term
| For a central atom surrounded by three regions of electron density, VSEPR predicts bond angles of 360 ˚/3 = 120 ˚. |
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Definition
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Term
| The three 2p orbitals are aligned parallel to each other. |
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Definition
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Term
| All molecules with polar bonds are polar |
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Definition
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Term
| Electronegativity generally increases from left to right across a period of the Periodic Table. |
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Definition
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Term
| A compound with the molecular formula C3H6O may be an aldehyde, a ketone or a carboxylic acid. |
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Definition
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Term
| Dichloromethane, CH2Cl2 is polar, but tetrachloromethane, CCl4, is nonpolar. |
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Definition
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Term
| A covalent bond is formed between atoms whose difference in electronegativity is less than 1.9 |
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Definition
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Term
| Each principal energy level can hold two electrons. |
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Definition
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Term
| Atoms that share electrons to achieve filled valence shells form covalent bonds. |
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Definition
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Term
| Contributing structures differ only in the distribution of valence electrons |
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Definition
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Term
| In creating hybrid orbitals (sp, sp², and sp³), the number of hybrid orbitals created is equal to the number of atomic orbitals hybridized. |
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Definition
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Term
| VSEPR treats the two electron pairs of a double bond and the three electron pairs of a triple bond as one region of electron density |
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Definition
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Term
| If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will not form a covalent bond. |
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Definition
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Term
| A carbon – carbon triple bond is a combination of one sigma bond and two pi bonds. |
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Definition
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Term
| A carbon – carbon double bond is a combination of two sigma bonds. |
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Definition
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Term
| An s orbital has the shape of a sphere with the center of the sphere at the nucleus |
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Definition
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Term
| A functional group is a group of atoms in an organic molecule that undergoes a predictable set of chemical reactions. |
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Definition
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Term
| In a polar covalent bond, the more electronegative atom has a partial negative charge and the less electronegative atom has a partial positive charge. |
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Definition
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Term
| Electronegativity depends on both the nuclear charge and the distance of the valence electrons from the nucleus. |
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Definition
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Term
| There are two alcohols with the molecular formula C3H8O |
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Definition
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Term
| In methanol, CH3OH, the O – H bond is more polar than the C – O bond |
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Definition
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Term
| The molecular formula of the smallest carboxylic acid is C2H6O2 |
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Definition
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Term
| Each 2p orbital has the shape of a dumbbell with the nucleus at the midpoint of the dumbbell. |
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Definition
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Term
| Atoms that lose electrons to achieve a filled valence shell become cations and form ionic bonds with anions. |
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Definition
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Term
| There are three amines with the molecular formula C3H9N. |
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Definition
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