Unit 3.01 - 3.02

Question 1

What are the properties of a solid?

Answer 1

Has a definite shape and a definite volume; The particles are tightly packed together and only vibrate gently around fixed positions

Question 2

What are the properties of a liquid?

Answer 2

Has no definite shape, but has a definite volume; The particles are free to move

Question 3

What are the properties of a gas?

Answer 3

Neither has definite shape nor volume; The particles spread apart, filling all the space of the container

Question 4

What properties are depended upon how the particles that make up the solid or liquid arranged, and the extent of the attraction between those particles?

Answer 4

Viscosity, surface tension, hardness, etc,.

Question 5

What does the straight line mean in a heating or cooling curve?

Answer 5

It means that the energy is being used to weaken and separate the particles from each other; transition period

Question 6

The Liquid/Gas transition line is always…

Answer 6

longer

Question 7

What does slope indicate in a heating or cooling curve?

Answer 7

Heat capacity

Question 8

What is inter bonding based on?

Answer 8

Based upon the Coulombic attraction between opposite charges

Question 9

Properties of inter bonding?

Answer 9

Usually very small, relatively very weak attraction

Question 10

Define London Dispersion (LDF)

Answer 10

Occurs when small electrostatic forces are caused by the movement of electrons within the covalent bonds of a molecule. This movement causes small, temporary dipoles

Question 11

What molecules can have LDF

Answer 11

Any molecule

Question 12

LDF increases with…

Answer 12

Surface area and with the polarizability of the atom or molecule

Question 13

Define polarizability

Answer 13

The ability to become polar

Question 14

Polarizability increases along with the number…

Answer 14

of electrons

Question 15

Larger molecules with larger surface area have more electrons, therefore

Answer 15

it has a greater polarizability and leads to greater attractions and therefore higher boiling points.

Question 16

However, isomers have

Answer 16

different surface area and boiling points

Question 17

single atoms are always…

Answer 17

nonpolar

Question 18

Number of electrons increase along with…

Answer 18

boiling point

Question 19

As the number of electrons increase, what happened to the strength of attractions?

Answer 19

Gets stronger

Question 20

Define Dipole Dipole Forces

Answer 20

When molecules that have permanent dipoles come together, they will arrange themselves so that the negative and the positive ends of the molecules attract one another.

Question 21

Define Dipole Induced Dipole Forces

Answer 21

When a polar molecule approaches a nonpolar molecule and induces (forces) a dipole.

Question 22

Define Ion-Dipole Force

Answer 22

A polar molecule interacts with an ion.

Question 23

What molecules can have Dipole Dipole?

Answer 23

Polar molecules ONLY

Question 24

Define hydrogen bonding

Answer 24

Forms a covalent bond its electron is held to one side of the nucleus leaving the other side completely exposed. This means there is a small portion that is negative and a big portion of a positive side.

Question 25

What force is the strongest

Answer 25

Hydrogen bonding

Question 26

What atoms can experience hydrogen bonding

Answer 26

F, O, or N

Question 27

What does Hydrogen have to be bonded with in hydrogen bonding?

Answer 27

To a more electronegative element that is small enough to allow a significant intermolecular interaction

Question 28

More electrons mean…

Answer 28

more polarizable