Chemistry-VSEPR/Polarity/IMF's

In polar compounds how are electrons shared

unequally

electronegativity

how much electrons are pulled and therefore one molecule holds on to the electrons longer creating a negative charge

= sharing of electrons

non-polar

un = sharing of electrons

polar

Dipole

has 2 poles

0-0.5

nonpolar

0.5-2

polar

2.0-3.3

ionic compound

how does shape affect polarity

a bent shape means a polar molecule

a linear shape most likely means nonpolar

How are nonbonded (unpaired) electrons different from bonded electrons

they take up more space

What are the 4 types of electrons

1. non bonded (lone pairs)

2. single bond

3. double bond

4. tripple bond

what are electrons domains

the type of electrons that exist around the central atom/ space where electrons exist

How many e.d. are present

2

How many e.d. are present

4

How many e.d. are present

6

How many e.d. are present

2

how many electrons can the s orbital hold

2

how many electrons can the p orbital hold

6

what is the hybridization of this atom?

sp3d2

what is the hybridization of this atom?

sp

what is the hybridization of this atom?

sp3

what is the hybridization of this atom?

sp

true or false: lone pairs repel more strongly than bonded pairs

true

What is VSEPR notation

AXaEb

What does A stand for in AXaEb

the central atom

What does X stand for in AXaEb

the number of bonded pairs (this goes to a)

What does E stand for in AXaEb

the number of lone pairs (this goes to b)

Do you write the subscript for 1 in VSPER notation?

no, just the letter

Where there are 0 lone pairs or bonds do you write the letter in VSPER notation?

no

True or false: lone pairs affect bond angles

True

What is the difference between intramolecular forces and intermolecular forces

INTRAmolecular forces-connects chemical bonds (like super glue)

INTERmolecular- forces that bine compounds

examples of INTRAmolecular forces

ionic and covalent bond

what are INTERmolecular forces represented by?

a dotted line

What do intermolecular forces affect?

Physical properties: melting point, boiling point, and surface tension

what is surface tension

the ability for an object to rest on top of a liquid.

What IMF can every molecule make

LDF

What are the strongest IMF’s

ionic forces

Ion-ion

forces between ionic compounds

ion-dipole

force of attraction between ion and covalently bonded polar molecule.

example of ion-dipole

ionic compound being dissolved in a polar solvent.

Dipole-dipole

attraction between oppositely charged regions of polar molecules

what bond does every polar molecule have

dipole-dipole

Hydrogen bond

1. molecule must have hydrogen covalently bonded to Nitrogen,Oxygen, or Fluoride

2. Nitrogen,Oxygen, or Fluoride must have a lone pair attached to it.

Are hydrogen bonds strong

yes

do hydrogen bonds have a high melting point

yes

weakest IMF

LDF

LDF

molecule with an instantaneous dipole

instantaneous dipole

all electrons move to 1 side at some point (even if not a dipole)

induced dipole

follows after an instantaneous dipole

Do LDF’s last long

no, they end just as quickly as they start

What are factors that affect LDF’s

size of the molecule (the larger the molecule the stronger the LDF

True or false: the more polar the molecule, the stronger the dipole-dipole force

True

True or false: the more polar a molecule is the higher the boiling point

true

Cl combinding with H2O is an example of what IMF

Ion-Dipole

This is an example of what IMF

ion-ion

This is an example of what IMF

dipole-dipole

This is an example of what IMF

hydrogen bonding

what does the symbol for a dipole look like (positive or negative)

δ

the stronger the IMF, the high the what?

melting and boiling point or higher surface tension.