Exam 1 Flashcards
Name this functional group.
Alkane
Draw out the Alkane functional group.
Name this functional group.
Alkene
Draw out the Alkene functional group.
Name this functional group.
Alkyne
Draw out the Alkyne functional group.
Name this functional group.
Alcohol
Draw out the Alcohol functional group.
Name this functional group.
Ether
Draw the Ether functional group.
Name this functional group.
Epoxide
Draw the Epoxide functional group.
Name the functional group.
Haloalkane
Draw a haloalkane functional group.
Name the functional group.
Aldehyde
Draw a Aldehyde functional group.
Name the functional group.
Ketone
Draw a Ketone functional group.
Name the functional group.
Carboxylic Acid
Draw a Carboxylic Acid functional group.
Name the functional group.
Ester
Draw a Ester functional group.
Name the functional group.
Amide
Draw an Amide functional group.
Name the functional group.
Amine
Draw an Amine functional group.
Name the functional group.
Thiol
Draw a Thiol functional group.
What structure is this?
Isopropyl
What structure is this?
Sec-butyl
What structure is this?
Tert-butyl
What structure is this?
Isobutyl
What is the formula for calculating formal charge?
of valence electrons - (# of non-bonded electrons + # of bonds)
Why do hybrid resonance structures have lower energy/ are more stable?
There is delocalization or “spreading out” of electrons.
What are the 3 rules for bond length?
- Bond length decreases across a period.
- Bond length decreases with increasing bond order
- Bond length increases as you go down a group.
What is the bond angle for a linear electron geometry?
180*
What is the bond angle for a trigonal planar electron geometry?
120*
What is the bond angle for a tetrahedral electron geometry?
109.5
What is the equation to find the # of hybrid orbitals?
of lone pairs + # of sigma bonds
What is the equation for bond order?
(bonding orbital electrons - antibonding orbital electrons)/2
If the bond order is <1, it is ______.
Not stable
Why are staggered rotations more stable in Newman projections?
It decreases Van der Waal repulsions
What is a primary carbon?
Bonded to 1 other carbon
What is a secondary carbon?
Bonded to 2 other carbons
What is a tertiary carbon?
Bonded to 3 other carbons
What is a quaternary carbon?
Bonded to 4 other carbons
What is a primary hydrogen?
Bonded to a primary carbon
As the # of carbons increases the boiling point ________ because _______.
increases; As the molecule gets larger, the London dispersion forces increase.
As the # of carbons increases the melting point ________ because _______.
increases; As the molecule gets larger, the London dispersion forces increase.
A Lewis acid is an electron ______.
Acceptor
A Lewis base is an electron ______.
Donor
A Bronsted Acid is a species that ______ a proton.
Donates
A Bronsted base is a species that ______ a proton.
Accepts
If the product side is favored, then Keq is ____ than 1.
Greater than
If the reactant side is favored, then Keq is _____ than 1.
Less than
An electrophile is a _________.
Lewis Acid
A neutrophile is a ________.
Lewis base
