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Brown and Poon O-Chem chapter 1 True False
Chapter 1 True/False Flash Cards
46
Organic Chemistry
Undergraduate 3
01/19/2012

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Cards

Term
These bonds are arranged in order of increasing polarity C-H < N-H < O-H
Definition
True
Term
All atoms in a contributing structure must have a complete valence shell
Definition
False
Term
An electron in a 1s orbital is held closer to the nucleus than an electron in a 2s orbital.
Definition
True
Term
A sigma bond and a pi bond have in common that each can result from the overlap of atomic orbitals.
Definition
True
Term
The molecular formula of the smallest aldehyde is C3H6O, and that of the smallest ketone is also C3H6O.
Definition
False
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.
Definition
True
Term
An orbital is a region of space that can hold two electrons.
Definition
True
Term
In the ground-state electron configuration of an atom, only the lowest-energy orbitals are occupied.
Definition
True
Term
Electronegativity generally increases with atomic number.
Definition
False
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.
Definition
False
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.
Definition
True
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.
Definition
False
Term
All bond angles in sets of resonance contributing structures must be the same.
Definition
False
Term
Electronegativity is a measure of an atom’s attraction for electrons it shares in a chemical bond with another atom.
Definition
True
Term
An orbital can hold a maximum of two electrons with their spins paired.
Definition
True
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.
Definition
False
Term
A primary alcohol has one – OH group, a secondary alcohol has two – OH groups, and a tertiary alcohol has three – OH groups.
Definition
False
Term
H2O and NH3 are polar molecules, but CH4 is nonpolar.
Definition
True
Term
Electronegativity generally increases from top to bottom in a column of the Periodic Table.
Definition
False
Term
The letters VSEPR stand for valence-shell electron pair repulsion.
Definition
True
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).
Definition
False
Term
For a central atom surrounded by three regions of electron density, VSEPR predicts bond angles of 360 ˚/3 = 120 ˚.
Definition
True
Term
The three 2p orbitals are aligned parallel to each other.
Definition
False
Term
All molecules with polar bonds are polar
Definition
False
Term
Electronegativity generally increases from left to right across a period of the Periodic Table.
Definition
True
Term
A compound with the molecular formula C3H6O may be an aldehyde, a ketone or a carboxylic acid.
Definition
False
Term
Dichloromethane, CH2Cl2 is polar, but tetrachloromethane, CCl4, is nonpolar.
Definition
True
Term
A covalent bond is formed between atoms whose difference in electronegativity is less than 1.9
Definition
True
Term
Each principal energy level can hold two electrons.
Definition
False
Term
Atoms that share electrons to achieve filled valence shells form covalent bonds.
Definition
True
Term
Contributing structures differ only in the distribution of valence electrons
Definition
True
Term
In creating hybrid orbitals (sp, sp², and sp³), the number of hybrid orbitals created is equal to the number of atomic orbitals hybridized.
Definition
True
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
Definition
True
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.
Definition
False
Term
A carbon – carbon triple bond is a combination of one sigma bond and two pi bonds.
Definition
True
Term
A carbon – carbon double bond is a combination of two sigma bonds.
Definition
False
Term
An s orbital has the shape of a sphere with the center of the sphere at the nucleus
Definition
True
Term
A functional group is a group of atoms in an organic molecule that undergoes a predictable set of chemical reactions.
Definition
True
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.
Definition
True
Term
Electronegativity depends on both the nuclear charge and the distance of the valence electrons from the nucleus.
Definition
False
Term
There are two alcohols with the molecular formula C3H8O
Definition
True
Term
In methanol, CH3OH, the O – H bond is more polar than the C – O bond
Definition
True
Term
The molecular formula of the smallest carboxylic acid is C2H6O2
Definition
False
Term
Each 2p orbital has the shape of a dumbbell with the nucleus at the midpoint of the dumbbell.
Definition
True
Term
Atoms that lose electrons to achieve a filled valence shell become cations and form ionic bonds with anions.
Definition
True
Term
There are three amines with the molecular formula C3H9N.
Definition
False
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