Checkpoint 4 Flashcards
A bond in which 2 electrons are shared by 2 atoms
Covalent bonds
Pairs of electrons localized on one atom
Lone pair
Pairs of electrons shared between atoms
Bonding pairs
As the number of bonds increase, bond energy ____
Increases
As the number of bonds decrease, bond length _____
Decreases
Electrons are negatively charged and therefore repel each other. Distances between electron pairs are maximized
VSEPR Theory
How is the number of bonding pairs determined?
How many elements are bonded to the central atom
Multiple bonds make a ____ distance
Shorter
How are the number of lone pairs determined?
How many pairs of atoms are attached to the central atom
What is correlated to bond angle?
Total number of electron areas
How do you find the total electron area?
Bonding area + lone pairs
How do you determine electron pair geometry?
Total electron areas
How do you determine the molecular geometry?
Bonding areas
Electrons are not shared equally in a covalent bond
Polar covalent
Electrons are shared equally in a covalent bond
Nonpolar covalent
What is the trend of electronegativity on the periodic table?
Left to right increases, up and down decreases
When dipoles cancel out it is (polar or nonpolar)
Nonpolar
When dipoles do not cancel out it is (polar or nonpolar)
Polar
If the molecule is symmetric it is usually (polar or non polar)
Nonpolar
If the molecule is nonsymmetric, it is usually (polar or non polar)
Polar
Only contains carbon carbon single bonds
Alkanes
Contains at least one carbon carbon double bonds
Alkenes
Contains at least one carbon carbon triple bonds
Alkynes
Organic compounds that contain an -OH group
Alcohol
Organic compounds that contain a -COOH group
Carboxylic acid
Two hydrocarbons are bonded in an oxygen atom
Ether
Organic compounds that contain a -CONH2 group
Amides
Method of describing the delocalized electrons in some molecules where the bonding cannot be explicitly expressed by a single Lewis structure
Resonance
