1. Molecular Basics Flashcards
how many single bonds, double bonds and triple bonds can Carbon form
single = 4
double = 2
triple + single bond
how many single bonds & double bonds can oxygen form
single = 2
double = 1 + 2 pairs of unshared e-
how many bonds and what type can Hydrogen form
1 single bond
how many single bonds, double bonds and triple bonds can Nitrogen form
single = 3
can also form double or triple bonds depending on the compound
what is the valence of carbon
4
what is the valence of Oxygen
2
what is the valence of hydrogen
1
what is the valence of nitrogen
3
what is the valence of nitrogen
3
what do lewis structures show
all atoms and bonds in molecule
what does each bone represent in a lewis structure
represents the sharing of 2 e- between respective atoms
what do partially condensed structures show
dont show bonds between C & H, atoms are drawn beside each other
what do condensed structures show
dont show any single bonds, only shows structural arrangement of atoms
in 3D bond line structures what do wedges represent
group coming out of page towards you
in 3D bond line structures what do dashes represent
what does a positive charge on an oxygen atom indicate in terms of number of bonds and lone pairs
3 bonds and one lone pair of e-
what does a negative charge on an oxygen atom indicate in terms of number of bonds and lone pairs
one bond and 3 lone pairs
what does no charge on an oxygen atom indicate in terms of number of bonds and lone pairs
2 bonds and 2 lone pairs
what does a positive charge on an nitrogen atom indicate in terms of number of bonds and lone pairs
4 bonds and no lone pairs
what does a negative charge on an nitrogen atom indicate in terms of number of bonds and lone pairs
2 bonds and 2 lone pairs
what does no charge on an nitrogen atom indicate in terms of number of bonds and lone pairs
3 bonds and one lone pair
what are resonance structures used to show
the spread of positive charge, combination of different structures in a linear fashion
what are the 3 rules for determining significance of resonance structures (full explanation)
- structures with minimal charges are more significant than structures with several charges
- structures that have a full octet of e- on their atoms are more significant than those that do not have a full octet
- if 2 carbon atoms in a structure have opposite charges, this structure is generally insignificant
what are the 3 rules for determining significance of resonance structures (brief summary)
minimal charges, full octet of atoms and doesnt show carbon atoms with opposing charges = significant
how many atoms/groups are sp3 orbital carbons connected to
4
what is the angle between atoms/groups in a sp3 orbital carbon
109.5 degrees
how many atoms/groups are sp2 orbital carbons connected to
3
what is the angle between atoms/groups in a sp2 orbital carbon
120 degrees
how many atoms/groups are sp orbital carbons connected to
2
what is the angle between atoms/groups in a sp orbital carbon
180 degrees
what are cis and trans isomers
same molecular formula and same structural formula but the atoms are arranged differently about the C=C double bond
