Unit 2 + 3.1 Flashcards
ability of atom to form a temporary or induced dipole
polarizability
weak to strong van der waals forces + other two strong forces
LDF, Dipole-Dipole, Hydrogen (which is a type of D-D); ionic and metallic both similarly strong
when are LDFs stronger?
1) when an atom or molecule has more total electrons (it is more polarizable) and
2) when the shape of the molecule is flatter/longer/thinner so there is more surface area
when are hydrogen bonds strongest?
1) H-F, then H-O, then H-N b/c diff. in electronegativity (far apart on periodic table) and
2) when there are multiple sites for hydrogen bonding (which is not a bond but a force)
when are ionic bonds strongest?
1) when charges are larger and
2) ions are smaller (both of which must be stated in answer), which is according to coulomb’s law
when are metallic bonds strongest
1) smaller metallic cations and
2) more valence electrons
what does the sum of superscripts of hybrid orbitals equal?
no. of electron clouds around central atom (no. of electron regions, not bonds)
when is a molecule w/ a central atom nonpolar?
1) C and H only elements present
2) central atom has no lone pairs + all other atoms are identical
2 electron regions + 2 bonding regions molecular geometry and bond angle
linear 180°
3 electron regions + 3 bonding regions molecular geometry and bond angle
trigonal planar 120°
3 electron regions + 2 bonding regions molecular geometry and bond angle
bent <120°
4 electron regions + 4 bonding regions molecular geometry and bond angle
tetrahedral 109.5°
4 electron regions + 3 bonding regions molecular geometry and bond angle
trigonal pyramidal <109.5°
4 electron regions + 2 bonding regions molecular geometry and bond angle
bent <109.5°
5 electron regions + 5 bonding regions molecular geometry and bond angle
trigonal bipyramidal 90°, 120°
5 electron regions + 4 bonding regions molecular geometry and bond angle
seesaw <90°, 120°, 180°
5 electron regions + 3 bonding regions molecular geometry and bond angle
T-shaped <90°, 180°
5 electron regions + 2 bonding regions molecular geometry and bond angle
linear 180°
6 electron regions + 6 bonding regions molecular geometry and bond angle
octahedral 90°
6 electron regions + 5 bonding regions molecular geometry and bond angle
square pyramidal 90°, 180°
6 electron regions + 4 bonding regions molecular geometry and bond angle
square planar 90°, 180°
6 electron regions + 3 bonding regions molecular geometry and bond angle
T-shaped 90°, 180°
6 electron regions + 2 bonding regions molecular geometry and bond angle
linear 180°
what are the exceptions to the octet rule?
1) H only needs 1 pair
2) Be only needs 2 pairs
3) B and Al only need 3 pairs
4) NM in period 3+ b/c d orbitals
