Final

Question 1

How are ionic bonds formed?

Answer 1

An ionic bond can be formed after two or more atoms lose or gain electrons to form an ion. Ionic bonds occur between metals, losing electrons, and nonmetals, gaining electrons. Ions with opposite charges will attract one another creating an ionic bond.

Question 2

Why are polar bonds polar?

Answer 2

A polar bond is a covalent bond between two atoms where the electrons forming the bond are unequally distributed. This causes the molecule to have a slight electrical dipole moment where one end is slightly positive and the other is slightly negative.

Question 3

What factors affect the boiling point?

Answer 3

Size of particle, London dispersion forces, dipole-dipole forces, and hydrogen bonds (HO, HF, and HN).

Question 4

What do Lewis Dot Diagrams show?

Answer 4

Lone and bonding pairs. Use VSEPR shapes.

Question 5

Intermolecular forces vs intramolecular forces:

Answer 5

Intramolecular forces are the forces that hold atoms together within a molecule. Intermolecular forces are forces that exist between molecules.

Question 6

Why is VSEPR a thing?

Answer 6

The premise of the VSEPR theory is that electron pairs located in bonds and lone pairs repel each other and will therefore adopt the geometry that places electron pairs as far apart from each other as possible.

Question 7

Boyles Law:

Answer 7

The volume of a gas at constant temperature varies inversely with the pressure exerted on it.

Question 8

Charles Law:

Answer 8

Volume is proportional to Kelvin temperature.

Question 9

Gay-Lussacs Law:

Answer 9

Rising a gas’s temperature induces a relative increase in its pressure (assuming that the volume does not change). Likewise, reducing the temperature allows the strain to decrease proportionally.

Question 10

Avogadro’s Law:

Answer 10

Explained the law of combining volumes. Equal volumes of gases at the same temperature and pressure contain an equal number of molecules.

Question 11

Ideal VS Real Gasses:

Answer 11

Ideal: Gasses are far apart and the molecule size is negligible, molecules are in constant random motion with no forces in between, and their collisions are infinitely elastic.
Real: Higher pressures force the sizes of molecules to become significant, as temperature decreases, molecules slow down and intermolecular attractions are prevalent, molecule collisions result in a loss of energy.

Question 12

What do net ionic equations show?

Answer 12

The elements that are necessary within a chemical equation. Does not include spectator elements.

Question 13

What happens when a solution is diluted?

Answer 13

Decreases the concentration of the solute in the solution

Question 14

How do you do dilution calculations?

Answer 14

C1V1 = C2V2

Question 15

Concentration Equation:

Answer 15

N = C x V

Question 16

The process of creating a standard solution:

Answer 16

1. Calculate the required mass of the solute
2. Weigh the required mass and put in a clean dry beaker
3. Dissolve with half of the total volume of distilled water
4. Transfer the solution to a volumetric flask and rinse everything
5. Fill to line with an eyedropper
6. Stopper and invert

Question 17

The process of creating a diluted standard solution:

Answer 17

1. Calculate the volume of the concentrated solution required
2. Transfer the concentrated solution into a clean dry beaker using a graduated cylinder
3. Pipet solution into a clean dry 100 mL volumetric flask
4. Add distilled water to the line using an eyedropper
5. Stopper and invert

Question 18

What happens when a solute is dissolved?

Answer 18

Dissolving is when the solute breaks up from a larger crystal of molecules into much smaller groups or individual molecules.

Question 19

Properties of Acids:

Answer 19

Forms H30+, pH < 7, reacts with bases, sour, turns litmus paper red.

Question 20

Properties of Bases:

Answer 20

Forms OH-, pH > 7, doesn’t react with metals, slippery, bitter, turns litmus paper blue.

Question 21

How do you identify a strong base?

Answer 21

Groups 1&2 + OH

Question 22

What are polyprotic acids?

Answer 22

Have multiple hydrogens to give up.

Question 23

Percent Yield:

Answer 23

Experimental / Theoretical x 100 = %

Question 24

Percent Error:

Answer 24

Theoretical - Experimental | / Theoretical x 100 = %