Ch. 1 Flashcards
Cation
Positively charged, has fewer electrons than protons
Anion
Negatively charged, has more electrons than protons
Elements in the same ____ have similar size
row
Elements in the same _____ have similar electronic and chemical properties
column
What shape are s orbitals? p orbitals?
S orbitals are spherical, P orbitals are dumbbell shaped
Where does electronegativity trend?
Top right corner (towards fluorine)
When does ionic bonding occur?
Elements on the far left side bond with elements on the far right side. Usually when the electronegativity difference is 1.5 or higher
When does covalent bonding occur?
Occurs between two of the same elements from the sides of the table (ex. H2, Cl2)
What is a formal charge? How do you calculate it?
A formal charge is the charge assigned to individual atoms in a Lewis structure. Calculated by subtracting the number of electrons an atoms “owns” from the number of valence electrons
What four things can you use to compare resonance structures?
- Has as many bonds as possible
- Every atom has an octet
- Has the negative charge on the most electronegative atom
- Has as little charge separation as possible
What is a major contributor (resonance)? minor contributor?
the major contributor is the better resonance structure and all of the other “worser” structures are the minor contributors
What is a resonance hybrid and what contributor does it reflect?
A resonance hybrid is a composite of all possible resonance structures. It looks like the major contributor
Triple Bond Hybridization
A side-by-side overlap of two 2p orbitals on one carbon with two 2p orbitals on the other carbon creates the second and third bonds of the triple.
Double Bond Hybridization
Overlap of the two sp2 orbitals from the C-C sigma bond and overlap of the two 2p orbitals forms the pi bond.
Hybridization of an atom based on groups/orbitals
2 groups/orbitals –> two sp hybrid orbitals
3 groups/orbitals –> three sp2 hybrid orbitals
4 groups/orbitals –> four sp3 hybrid orbitals
