polar and nonpolar test

Ionic Compounds are between what

metal and nonmetal

general properties of ionic compound?

brittle, high boiling point, good insulators as solids, between metal/ nonmetal

Ionic compounds are dissolved by what kind of covalent compound?

polar

What are the factors of lattice energy?

Higher charge= higher Lattice energy…more distance= higher Lattice energy.. size of ion decreases when there is more lattice energy

What are hydrocarbons? Are they polar or nonpolar?

Organic compounds made up of hydrogen and carbon; nonpolar

Which ones dissolved by water?

Propanol, ethanol, methanol

What is IMF???

Attractive forces that act between molecules, atoms or ions to determine substances physical properties

What is the main IMF for polar molecules?

Dipole- Dipole

What is the main IMF for nonpolar forces?

London Dispersion Forces

Noble gases have which IMF?

only London Dispersion

Which Noble gas has the highest IMF?

Xenon; largest atomic radius, high number of electrons, high polarazibility

Which halogen molecule has the largest IMF?

I2;solid state at room temperature, highest melting point

How does having a higher IMF affect boiling points and melting points???

More thermal energy is required to overcome stronger attractions between molecules .. particles are held together more tightly , making it harder to transition from solid to liquid, a liquid to gas

Rank IMF from strongest to weakest

1. LDF

2. . Dipole- Dipole

3. Hydrogen Bonding

examples of molecules w LDF

Ch4, CO2, O2, He

examples of molecules with Dipole- Dipole

HCl, SO2, CH2Cl2

molecules w Hydrogen bonding

H2O, NH3, CH3OH

Polar covalent compound definition

Shares electrons unequally; has CHARGED ENDS

Nonpolar covalent compound

shares electrons equally or almost equally; NO CHARGED ENDS

example of polar covalent compounds

H2O, NH3

example of nonpolar covalent compounds

H2, O2

Describe soap’s structure. Why does it help remove grease from pots and pans?

Soap has a nonpolar end and polar end; polar end attached to water while th oil (or other nonpolar molecule) attaches to the nonpolar end.

What are the factros that affect boiling point and melting point?

molecular size, shape, polarity., external pressure

prefixes

1- mono

2- di

3-tri

4-tetra

5-penta

6-hexa

7-hepta

8-octa

9-nona

10-deca

Roman Numerals

1- I

2- II

3- III

4- IV

5-V

6-VI
7-VII

8-VIII

9- IX

10- X

When lattice energy is up boiling point is ____________

UP

whihc alkyne has highest boiling point and why

Decane has the highest boiling point from alkanes because it has more bonds, therefore it has more opportunities for London Dispersion Forces. Since it has a greater IMF, the atoms are more tightly packed and harder to pull apart, increasing the boiling point.

A substance will form hydrogen bonds if it

1. contains hydrogen atoms and either O, F, or N.

Lattice energy is

1. the amount of energy required to pull apart a lattice structure until both elements transform into gases. Lattice energy increases with higher ion charges and decreases as the distance between ions increases.

Characteristics of ionic compounds include

high melting points, good insulators as solids, good conductors in an aqueous or molten state, production of electrolytic solutions when dissolved in water, hardness, brittleness, and between a metal and non-metal

Adhesion is

the attraction and "sticking" of water molecules to molecules of different substances, driven by water's polarity (uneven charge) creating weak bonds with other charged or polar surfaces, explaining phenomena like water climbing glass (capillary action) or sticking to plant leaves.

Cohesion

 water is the attraction of water molecules to other water molecules, caused by hydrogen bonds due to their polar nature, allowing for surface tension.

Substances with stronger intermolecular forces or more surface area will have

higher melting/boiling points.

• Electronegativity difference in covalent bonds

• Less than 0.5 - nonpolar

• In between 0.5 and 1.7 - polar

• Above 1.7 - ionic

• Physical properties of polar molecules

• High specific heat (heats up slowly and requires a lot of energy to change the temperature)

• Able to be dissolved in water (like dissolves like)

  • Water can dissolve polar and ionic compounds

• Examples of polar molecules: sugar

Nonpolar molecules

• Do not dissolve in water

• Oil, gasoline, acetone

• Isomers - molecules with the same formula but different structures 

• N-pentane and neo-pentane

• Intermolecular force - holds molecules together

• LDF, dipole-dipole

• Intramolecular force - holds atoms together in molecule

• Metallic, ionic, and covalent bonds