5: LAB 5 - PHYSICAL AND CHEMICAL PROPERTIES
- Page ID
- 506153
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)The purpose of this experiment is to:
- Record the appearance of several metals and nonmetals.
- State whether a solid is soluble or insoluble in water.
- State whether a liquid is soluble or insoluble in water.
- Explain whether a substance is undergoing a physical or chemical change.
- Measure boiling points and record test tube reactions.
INTRODUCTION
Chemistry is the study of matter and any changes it undergoes. Matter is defined as anything that occupies space and has mass. Matter can be classified into three states: solid, liquid, and gas. These properties indicate that matter has specific physical characteristics, which correspond to the three phases of matter. A solid has a definite shape and volume. Solids are tightly packed, with atoms having a fixed volume and a definite shape. Liquids have a fixed volume but not a definite shape and take the shape of their containers. Gases have neither a definite shape nor a definite volume, and they expand to fill the space within their containers.
Matter can also be classified into mixtures and pure substances. A pure substance has a constant composition. All have the same composition and properties. Pure substances are divided into two classes: elements and compounds. Pure substances that cannot be broken down into simpler substances by chemical changes are called elements. Some examples are iron, silver, gold, aluminum, sulfur, oxygen, and copper. Pure substances that can be broken down to produce either elements or other compounds, or both, by chemical changes are called compounds.
Although there are 118 elements, tens of millions of chemical compounds result from different combinations of these elements. Each compound has a specific composition and definite chemical and physical properties that distinguish it from all other compounds. And, of course, there are innumerable ways to combine elements and compounds to form different mixtures.
Scientists use the periodic table to reference information about an element, such as atomic mass and chemical symbols. The periodic table's arrangement also allows scientists to discern trends in element properties, including electronegativity, ionization energy, and atomic radius. The periodic law states that the physical and chemical properties of the elements recur systematically and predictably when the elements are arranged in order of increasing atomic number.
The periodic table organizes elements based on their increasing atomic numbers, which allows for the prediction of their chemical and physical properties. Elements within the same group or column often share similar properties due to their similar outer electron configurations.
The properties that chemists use to describe matter fall into two general categories.
Physical properties are characteristics that describe matter. They include size, hardness, state, shape, color, density, melting, boiling, freezing, solubility, and mass.
Chemical properties describe how matter changes its chemical structure or composition. Flammability, toxicity, acidity, the reactivity of various types, and the heat of combustion
EQUIPMENT* AND CHEMICALS NEEDED
| Equipment | Equipment | Chemicals |
|---|---|---|
| Safety goggles | Thermometer | 1.0 M Hydrochloric Acid (HCl) |
| Spatula | Large test tube and split cork | Alcohol (ethanol/methanol) |
| Hot plate | Test tube holder | Sodium chloride \(\ce{(NaCl)}\) |
| 10 mL graduated cylinder | Medium-sized test tubes | Sodium carbonate \(\ce{(Na2CO3)}\) |
| Glass Stirring Rod | Test tube rack | Calcium carbonate \(\ce{(CaCO3)}\) |
| 250 ml beaker | Boiling chip | starch |
| Deionized water | Hexane |
* Images of equipment needed in this lab can be found in the appendix (the equipment may differ or be subject to changes; follow your instructor’s directions).
- Always wear chemical splash goggles during the experiment.
- Gloves are provided for those who wish to wear them.
- Exercise extreme caution when using a hot plate or Bunsen burner to heat water.
- Water used for boiling point determination can be discarded in the sink. Other chemical waste solutions should be placed in appropriate waste containers as advised by the instructor.
- Ensure all glassware is clean, and all equipment is returned to its designated place.
- Thoroughly clean your work area and return chemicals and equipment to their designated places after the experiment.
- Clean the lab benches and verify all equipment is in your lab drawer before leaving.
- Wash your hands as soon as you leave the lab.
EXPERIMENTAL PROCEDURE
A. Identification, appearance, and observations of several metals, metalloids, and nonmetals.
Using the virtual periodic table and answering the questions in the data table below in data and observations part A.
- Classify the following: Carbon, Calcium, Sodium, Nitrogen, Oxygen, Phosphorus, Neon, Vanadium, Lithium, as metals, metalloids, and nonmetals in the data sheet.
- Identify the elements and group numbers of named groups: Alkali Metals, Alkaline earth metals, halogens, and noble gases.
- Which group of elements is considered transition metals?
- Which elements are considered Metalloids?
B. Physical and Chemical Properties and Changes
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Take a 250.0 mL beaker and add approximately 175 mL of distilled water to it. Bring the mixture to a boil on a hot plate*.
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While waiting for the water to boil, take a test tube large enough not to be immersed in the above 250.0 mL beaker and add 25 drops of alcohol, along with a boiling chip. Note the alcohol's identity. Suspend the thermometer in the test tube using a split cork. Ensure the tip of the thermometer is at least 1.0 cm above the alcohol level in the test tube. Place the test tube in the test tube rack.
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When the water starts boiling, record the boiling point in part B of the data table and observations. Identify whether this is a chemical or physical change. After recording the boiling point, turn off the hot plate.
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Place the test tube with alcohol into the above beaker with hot water. Record the temperature as the alcohol starts to boil. If your water has cooled down and the alcohol does not boil, turn on your hot plate to warm the water.
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After the remaining alcohol has cooled, pour it into the organic waste container, and the water can be discarded down the drain. Clean your work area and all glassware before moving on to the next step of the experiment.
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Obtain six test tubes and place them on a test tube rack. Add 10 mL of distilled water to each. Add half a spatula or 25 drops of the mentioned chemicals to the test tubes. Into the Test tube: 1 Sodium chloride \(\ce{(NaCl)}\), 2 Sodium carbonate \(\ce{(Na2CO3)}\), 3 Calcium carbonate \(\ce{(CaCO3)}\), 4 Starch, 5 twenty five drops of ethanol (or methanol), 6 25 drops of hexane, respectively (add only one compound into each test tube of distilled water). Swirl the liquid in the test tubes, and if necessary, use the glass rod to stir the solid in all three test tubes. Record the observations and solubilities and identify the type of change involved. Chemical waste solutions should be placed in appropriate waste containers.
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Obtain four test tubes, place them on a test tube rack, and add 10 mL of 1 M HCl to each. In each test tube, add a small amount, around half a spatula each of Sodium carbonate Na2CO3, Calcium carbonate CaCO3, 25 drops of ethanol (or methanol), and 25 drops of hexane, respectively. Stir using the glass rod. (Remember to clean the glass rod after mixing it into each test tube.) Record the observations and solubilities and identify the type of change involved.
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As instructed by your instructor, discard the contents of the test tubes into the designated waste container. Thoroughly clean all glassware with soap and water. Return all equipment and chemicals to their appropriate place. Before leaving the lab, clean the bench and your work area.
PRE-LAB QUESTIONS
Name: ____________________________________
- How are the elements in the periodic table arranged? Why is it important?
- The columns and rows of the periodic table are called:
- The elements in the two rows at the bottom of the periodic table are called:
- Define what a Physical property is and give five examples.
- Define Chemical property and give five examples.
DATA AND OBSERVATIONS
Name: _________________________Lab Partner(s): ______________________________
A. Identification, appearance, and observations of several metals, metalloids, and nonmetals.
- Classify the following as metals, metalloids, and nonmetals.
Element Name |
Symbol of Element |
Identify whether Metal / Nonmetal / Metalloid |
Group # |
State (s, l, g) |
|---|---|---|---|---|
Carbon |
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Calcium |
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Sodium |
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Nitrogen |
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Oxygen |
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Phosphorous |
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Neon |
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Vanadium |
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Lithium |
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Germanium |
- Identify the elements and group numbers of named groups: Alkali Metals, Alkaline earth metals, halogens, and noble gases.
a) Alkali Metals Group Number:
Names and Symbols of Alkali Metals:
b) Alkaline Earth Metals Group Number:
Names and Symbols Alkaline Earth Metals:
c) Halogens Group Number:
Names and Symbols of Halogens:
d) Nobel Gases Group Number:
Names and Symbols of Nobel Gases:
e) Transition metals, Group Numbers:
Names and Symbols of five Transition metals:
f) Names and Symbols of five of the Metalloids:
B. Physical and Chemical Properties and Changes
1. Boiling Point:
i) Boiling Point of Water:
Identify whether the boiling point of water is a Physical or Chemical change:
ii) Boiling Point Alcohol:
Identify whether the boiling point of Alcohol is a Physical or Chemical change:
2. Determine whether a change is chemical or physical using Water.
Test tubes # |
Observation |
Soluble / Insoluble |
Physical /Chemical Change |
|---|---|---|---|
|
1. Sodium chloride + water (NaCl + H2O) |
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2. Sodium Carbonate + water (Na2CO3 + H2O) |
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3. Calcium Carbonate + water (CaCO3 + H2O) |
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4. Starch + water |
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5. 25 drops of ethanol + water or (25 drops of methanol + water) |
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6. 25 drops of hexane + water |
3. Identify if a Chemical or Physical change using Hydrochloric acid.
Test Tubes # |
Observation |
Soluble / Insoluble |
Physical /Chemical Change |
|---|---|---|---|
|
1. Sodium chloride + HCl (aq) (NaCl + HCl (aq)) |
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2. Sodium Carbonate + HCl (aq) Na2CO3 + HCl (aq) |
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3. Calcium Carbonate + HCl (aq) CaCO3+ HCl (aq) |
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4. Starch+ HCl (aq) |
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5. 25 drops of ethanol + HCl (aq) (or methanol + HCl (aq)) |
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6. 25 drops of hexane + HCl (aq) |
POST-LAB QUESTIONS
1. Classify the following elements and complete the table below.
Name of Element |
Symbol of Element |
Identify whether Metal / Nonmetal/Metalloid |
Group Number |
Period |
|---|---|---|---|---|
|
Lithium |
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Si |
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Zinc |
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Mg |
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Copper |
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I |
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Uranium |
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Cl |
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Tin |
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Ge |
2. Identify whether a chemical or physical change.
Chemical or Physical Change |
|
|---|---|
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1. The density of zinc is 7.41 g/cm3 |
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2. Zinc combines with Hydrochloric acid to give zinc chloride and hydrogen gas |
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3. Silver tarnishes to silver oxide when exposed to moisture |
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4. Melting of polar ice caps due to global warming |
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5. Copper can be drawn into a thin wire and wrapped into a cord |
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6. An iron nail rusts when exposed to moisture |
Please click here to access the Pre-Lab, Data Tables, and Post-Lab in Word or PDF format. Complete them and upload according to your instructor's instructions.