Chem 101 Lab Final

Front 1

A double replacement reaction in which an acid and a base react to form salt and water.

Back 1

Neutralization

Front 2

The process of measuring the volume of one reagent required to react with a measured volume or mass of another reagent.

Back 2

Titration

Front 3

The point of neutralization in which the solution becomes “neutral” due to the addition of acid to a basic solution or base to an acidic solution.

It is the point when the number of moles of base are equivalent to the number of moles of acid in the solution.

Back 3

End-point

Front 4

The measure of relative proportions of two or more quantities in a mixture.

A concentrated solution = a large number of solute particles in the solvent.

A dilute solution = a small number of solute particles in the solvent.

Back 4

Concentration

Front 5

What indicator was used during the titration lab?

Back 5

Phenolphthalein

Front 6

KHP is an abbreviation for what compound?

Back 6

Potassium hydrogen phthalate with a molecular formula of HKC8H4O4

Front 7

What acid was used during the titration lab?

Back 7

KHP

Front 8

What base was used during the titration lab?

Back 8

NaOH

Front 9

What two compounds are produced as a result of a neutralization reaction?

Back 9

Salt and water (H2O)

Front 10

Identify the units for molarity.

Back 10

Molarity (M) = mol/L

Front 11

Convert mL to L?

Back 11

Divide by 1000

Front 12

Electrons in the outer most energy level that are involved in bonding atoms together to form compounds.

Back 12

Valence electrons

Front 13

- Groups of electrons arranged around the central atom due to repulsion.

- Includes: lone pairs,single bonds, double bonds, triple bonds, and a single electron.

Back 13

Electron group geometry

Front 14

- Groups of bonded atoms arranged around the central atom.

Back 14

Molecular group geometry

Front 15

- The charge Lewis structures would have if all bonding electrons were shared equally between the bonded atoms.

- It is useful to distinguish between multiple possible Lewis structures by determining the most stable orientation.

Back 15

Formal charge

Front 16

- Molecules that have the same molecular formula but different chemical structures.

Back 16

Isomer

Front 17

- It depicts two or more structures with the electrons in different places to more accurately reflect the delocalization of electrons.

Back 17

Resonance

Front 18

Carbon, Oxygen, Nitrogen, and Fluorine

Back 18

What elements always follow the octet rule?

Front 19

What elements are capable of violating the octet rule by forming expanded octets?

Back 19

Elements in the 3rd period or higher due to hybridization of the d-orbital.

Front 20

Hydrogen (2), Helium (2), Lithium (2), Berylium(4), and Boron (6)

Back 20

What elements violate the octet rule by forming incomplete octets?

Front 21

The central atom is usually the _____ electronegative atom in a compound.

Back 21

LEAST

Front 22

What two atoms are always terminal atoms?

Back 22

Hydrogen and Fluorine

Front 23

What types of atoms do not form multiple (ie. Double or Triple) bonds?

Back 23

Hydrogen and the Halogens (Fluorine, Chlorine,Bromine, Iodine, etc.)

Front 24

- Substance that form ions that are free to move in solution when dissolved in solvent (ie. water)

- Substances whose aqueous solutions conduct electricity.

- Includes: acids, bases, and salts.

Back 24

Electrolytes

Front 25

- Substances whose aqueous solutions do not conduct electricity.

- Examples include: sugars and alcohols.

Back 25

Non-electrolytes

Front 26

- Process in which compounds break down into component ions in solution.

Back 26

Ionization/Dissociation

Front 27

- Substances that COMPLETELY ionize in water.- Includes: salts and some acids and bases.

Back 27

Strong electrolytes

Front 28

- Substances that PARTIALLY ionize in water. - Includes: some acids and bases.

Back 28

Weak electrolytes

Front 29

- Substances that yield H+ions (specifically H3O+ ions) when dissolved in water.

- A proton (H+)donor.

Back 29

Acids

Front 30

- A non-metal oxide.

- Acids in which WATER has been removed.

Back 30

Acid Anhydride

Front 31

- Substances that yield OH-ions when dissolved in water.

- A proton (H+) acceptor.

Back 31

Base

Front 32

- A metal oxide.

- Bases in which WATER has been removed.

Back 32

Basic Anhydride

Front 33

- A solution in which the concentrations of H+ and OH- ions are equal.

Back 33

Neutral solution

Front 34

- A substance that consists of a positively charged ion (excluding H+) and a negatively charged ion (excluding O-2 and OH-).

Back 34

Salt

Front 35

An organic compound that changes color at a particular concentration of H+ and OH-ions.

Back 35

Indicator

Front 36

An instrument that measures H+ ion concentration by using an electrode that converts H+ions into an electric potential that is read by a voltmeter calibrated in pH units.

Back 36

pH meter

Front 37

- A measure of the acidity or alkalinity of a solution on a logarithmic scale.

Back 37

pH

Front 38

Mg(OH)2

Back 38

Base

Front 39

HClO4

Back 39

Acid

Front 40

KOH

Back 40

Base

Front 41

FeNO3

Back 41

Salt

Front 42

SO2

Back 42

Acid anhydride

(Non-metal oxide)

Front 43

AlCl3

Back 43

Salt

Front 44

BaO

Back 44

Basic anhydride (Metal oxide)

Front 45

H3PO4

Back 45

acid

Front 46

- States that energy cannot be created or destroyed. Instead it is converted from one form to another.

Back 46

Law of Conservation of Energy

Front 47

- The branch of physics that relates heat and temperature to energy and work.

Back 47

Thermodynamics

Front 48

- The study of heat released or absorbed as a result of a chemical reaction.

Back 48

Thermochemistry

Front 49

- States that heat energy lost by one body is gained by another body.

Back 49

First Law of Thermodynamics

Front 50

- Measurement of the amount of heat evolved or absorbed in a chemical reaction, change of state, or formation of a solution.

Back 50

Calorimetry

Front 51

- An instrument that measures the amount of heat transferred as a result of a chemical reaction.

Back 51

Calorimeter

Front 52

- The amount of heat energy required to raise the temperature of one gram of any substance by one degree Celsius.

Back 52

Specific Heat Capacity

Front 53

- A unit of heat (thermal)energy equal to 4.184 Joules.

- It is the amount of energy required to raise the temperature of one gram of water by one degree Celsius at standard pressure.

Back 53

calorie

Front 54

- A unit of heat used tomindicate the energy content in food or the energy that foods will produce in the human body. - 1 Calorie = 1 kilocalorie =1000 calories

Back 54

Calorie

Front 55

1. What is the formula for the calculation of heat energy?

Back 55

heat = (mass)(specific heat)(change in temperature, T final – T initial)

Front 56

1. What instrument measures the transfer of heat energy from one substance or object to another?

Back 56

Calorimeter