Term
|
Definition
Chapter 1
Bonds held together by electrostatic attraction |
|
|
Term
|
Definition
| [image] Contains carbon-hydrogen bonds only, NOT a functional group |
|
|
Term
|
Definition
| [image] Contains a carbon-carbon double bond |
|
|
Term
|
Definition
[image]
Contains carbon-carbon triple bond |
|
|
Term
|
Definition
| [image] Contains six-member carbon ring with alternating single and double bonds |
|
|
Term
|
Definition
| [image] carbon bonded to a halogen |
|
|
Term
|
Definition
| [image]carbon bonded to hydroxyl group |
|
|
Term
|
Definition
| [image] two carbons bonded to single oxygen |
|
|
Term
|
Definition
| [image] carbon bonded to nitrogen |
|
|
Term
|
Definition
| [image]carbon bonded to sulfide (-SH) |
|
|
Term
|
Definition
| [image] two carbons bonded to one sulfur |
|
|
Term
|
Definition
| [image] carbon double bonded to oxygen |
|
|
Term
|
Definition
| [image] one carbon and one hydrogen bonded to carbonyl group |
|
|
Term
|
Definition
| [image] two carbons bonded to a carbonyl group |
|
|
Term
|
Definition
| [image] hydroxyl group bonded to a carbonyl group (carboxylic acid derivative) |
|
|
Term
|
Definition
| [image] one carbon and one oxygen bonded to a carbonyl group, a carboxylic acid derivative |
|
|
Term
1. Amide
2. Acid Chloride
3. Acid Anhydride
4. Ester
5. Carboxylic Acid |
|
Definition
Name the 5 carboxylic acid derivatives |
|
|
Term
|
Definition
| [image] one nitrogen bonded to a carbonyl group, a carboxylic acid derivative |
|
|
Term
|
Definition
| [image] one chlorine bonded to a carbonyl group, a carboxylic acid derivative |
|
|
Term
|
Definition
| [image] one oxygen bonded to two carbonyl groups, a carboxylic acid derivative |
|
|
Term
|
Definition
| [image] carbon double bonded to a nitrogen |
|
|
Term
|
Definition
| [image]carbon triple bonded to one nitrogen |
|
|
Term
|
Definition
| [image] one sulfur bonded to a carbonyl group |
|
|
Term
| Saturated / Aliphatic Compounds |
|
Definition
Chapter 12
Term for a carbon with all four bonds established and filled |
|
|
Term
1: meth-
2: eth-
3: prop-
4: but-
5: pent-
6: hex-
7: hept-
8: oct-
9: non-
10: dec- |
|
Definition
Name all the parent numbers for systematic nomenclature |
|
|
Term
|
Definition
Term for organic chemistry nomenclature |
|
|
Term
| Bronstead Acid-Base Equilibrium |
|
Definition
Chapter 3
Idea of acid-base equilibrium where acids donate protons and bases accept protons |
|
|
Term
| Lewis Acid-Base Equilibrium |
|
Definition
Chapter 3
Idea of acid-base equilibrium where acid accepts electron pair and base donates electron pair |
|
|
Term
T = (Io/I1) x 100%
% transmittance = (original infared light/remaining infared light) x 100% |
|
Definition
Chapter 12
Formula for calculating percent transmittance |
|
|
Term
|
Definition
Chapter 1
Neutral collection of atoms |
|
|
Term
|
Definition
Chapter 1
Bond between two atoms formed by sharing a pair of electrons |
|
|
Term
| Electon-Dot / Lewis Structure |
|
Definition
Chapter 1
Style of molecular structure drawing where valence electrons are represented with dots and covalent bonds are represented by lines |
|
|
Term
| Line-Bond / Kekule Structure |
|
Definition
Chapter 1
Style of molecular structure drawing where covalent bonds are represented by lines between atoms but valence electrons are not represented |
|
|
Term
|
Definition
Chapter 1
Style of molecular structure drawing where carbons and hydrogens are not shown. The intersections between two lines are recognized as carbons. Heteroatoms are depicted and in order facing the carbon they would be bonded to. |
|
|
Term
|
Definition
Chapter 1
Theory that covalent bonds are formed when two atoms approach each other closely and a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom
|
|
|
Term
|
Definition
Chapter 1
Style of molecular structure drawing where carbon-hydrogen and carbon-carbon bonds are not illustrated but understood |
|
|
Term
|
Definition
Chapter 1
A bond characterized by head-on overlapping of two atomic orbitals along the line between the nuclei |
|
|
Term
|
Definition
Chapter 1
A bond made up solely of unhybridized p orbitals, bonds overlap above and below nuclei |
|
|
Term
1. Bond Strength
2. Bond Length
3. Bond Angle |
|
Definition
Chapter 1
Name the three unique characteristics of every covalent bond |
|
|
Term
|
Definition
Chapter 1
The combination of an s and p orbital on an atom |
|
|
Term
|
Definition
| [image]Type of hybridization where four sp hybridized orbitals are present to form a tetrahedral shape, only sigma (σ) bonds present |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
Chapter 1
Theory of covalent bond formation where a mathematical combination of atomic orbitals (wave functions) on different atoms form a molecular orbital |
|
|
Term
|
Definition
Chapter 1
Idea that orbitals belong to an entire molecular, not just a single atom |
|
|
Term
| Bonding Molecular Orbital |
|
Definition
Chapter 1
Type of molecular orbital characterized by the additive combination of two atomic orbitals to form a single, egg-shaped orbital. Electrons spend most of their time in the region between the two nuclei, lower in energy than the other type of molecular orbital. |
|
|
Term
| Antibonding Molecular Orbital |
|
Definition
Chapter 1
Type of molecular orbital characterized by the subtractive combination of two atomic orbitals to form one single orbital shaped like an elongated dumbbell. Electrons cannot occupy region between the two nuclei, higher in energy than the other type of molecuar orbital. |
|
|
