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Definitions
General Knowledge
Bonds
SP and Dipole
Formal Charges
100
An electron goes into an empty degenerate orbital rather than pairing up
What is Hund's Rule
100
Primary Carbocation
What is the carbocation that does not exist?
100
As bond length increases, bond strength _____
decreases
100
Indicate the dipole direction: H-Cl
---> (towards Cl)
100
What is the Formal Charge of the right nitrogen?
-1
200
An atomic orbital can contain no more than 2 electrons
What is the Pauli exclusion principle?
200
the most electronegative atom
What is Fluorine?
200
This bond contains only 1 sigma bond and 0 pi bonds
What is a single bond?
200
indicate the dipole moment: O=C=O
There is none, the oxygens equally pull the dipole
200
What is the formal charge of the carbon atom?
-1
300
An electron will go into the atomic orbital that has the lowest energy
What is the Aufbau Principle
300
This increase from left to right and from the bottom up
What is the electronegativity trend?
300
This bond contains 2 pi bonds and 1 sigma bond
What is a triple bond?
300
Indicate which atoms on this compound have sp2 hybridization: CH3-CH=O
C on CH and O
300
What is the formal charge of the right oxygen?
0
400
Bonded atoms are the same
What is a non-polar covalent bond?
400
The smaller the pKa, the ____ the acid is
stronger
400
This bond contains 1 sigma bond and 1 pi bond
What is a double bond?
400
Indicate which atoms on this compound has sp3 hybridization: O=Cl-CH2-CH3 | OH
C on CH2, C on CH3, and O on OH
400
What is the formal charge of the right sulfur?
+1
500
bonded atoms are different
What is a polar covalent bond?
500
A _____ loses a proton, a _____ gains a proton
acid, base
500
This is defined when a bond is short and strong and has a large bond angle.
What is a large S character
500
What bond has SP hybridization?
a triple bond
500
What is the formal charge of the nitrogen atom?
-2