Chp 7 - Chemical Bonding Flashcards
What happens when dealing with an ion that is a transition metal when u want to know the elec. config.
Take away electrons from highest principle quantum number.
ns2 wld lose first.
What’re the differences in atomic radii when dealing with cation/anion and original?
Cations are always smaller than original. Anions are always larger than original.
What is lattice energy?
Energy = (kQ1Q2)/r
Q1- charge of cation
Q2- charge of anion
What is a covalent bond?
2 or more electrons are shared by 2 atoms.
How do the lengths of single, double, & triple bonds differ?
- Single- longest, least stable
- Double- in the middle
- Triple- shortest, most stable
Compare ionic and covalent bonds.
Ionic bonds are more stable than covalent
What is a polar bond?
Greater amount of electrons on one side while the other has poor amount.
Electronegativity in periodic table?
The more top right you go, the greater the electronegativity.
What does it mean to be isoelectronic?
Having same number of electrons and same electron configuration.
Ex- ions
How to tell what kind of bond by electronegativity?
If difference of electronegativity is:
- 0-0.5=covalent
- 0.5-1.5=polar covalent
- 1.5-=ionic
Rules for drawing Lewis Structures?
- Put least electronegative in middle.
- Count valence
- Complete octet
- If structure contains many electrons, double triple bonds
What is a resonance structure?
2 or more Lewis structures for single molecule that can’t be represented by one Lewis structure.
of hybrid orbitals = # of atomic orbitals mixed.
Ok………….
How to tell between sigma and PI bonds?
Sigma- single bonds
Pi- double, triple only p orbitals
*Double has 1 pi and 1 sigma
*Triple has 2 pi and one sigma- stronger shorter.
What happens to bond angle when lone pairs are present?
Bond angle decreases.
