CHEM 113 General & Quantitative Chemistry I – Matter and Measurement (Lecture Notes)

Matter and Measurement

  • This course introduces two fundamental ways to engage with chemistry:

    • Understanding: What rules (laws) does the universe follow?

    • Application: How can we use these rules to solve practical problems?

  • Example referenced: Electrolysis and Fuel Cells as applications of chemical principles.

  • Course context: CHEM-113 is the first in a two-term sequence focused on foundational chemistry topics.

Course Logistics and Syllabus

  • Course code and section: CHEM-113-02, 4 credits

  • Instructor: Dr. Joe Elias (he/him/his)

    • Email: joseph.elias@simmons.edu

    • Office: E-480A

    • Office Hours: Mon/Thu/Fri 2:00-4:00 PM; Tue 3:00-4:00 PM (in person or via Zoom)

    • Open-door policy: encourage students to ask questions; best questions are specific.

  • Moodle site: Course materials and announcements available online

  • Prerequisites: MATH 101 or a satisfactory score on math placement exam

  • Course type and meeting time: SCI; M/W/F 1:00-1:50 PM

  • Meeting location: School of Management - C-221

  • Course description (overview):

    • This is the first semester of a two-semester sequence for students whose major interest is science, medicine, or engineering.

    • Topics include: stoichiometry, states of matter, electronic structures of atoms, periodic properties, chemical bonding, molecular geometry, introduction to quantum mechanics and atomic theory, introduction to organic and biological chemistry, solid state and materials science, macromolecular structures, thermochemistry, and energy.

    • Although CHEM-113 and CHEM-216 are separate courses, students are expected to take both terms sequentially.

    • The laboratory portion correlates with and amplifies lecture material and presents fundamental laboratory techniques as well as descriptive chemistry and instrumental methods.

What is Chemistry?

  • Chemistry, broadly speaking, is the study of:

    • Matter

    • How matter changes

    • The role of energy in these two processes

Matter: Properties, Composition, and Structure

  • Matter has mass (m) and occupies a volume (V).

  • The properties of matter arise from its composition and its structure:

    • Example: Ice vs. Water

    • Composition: H$_2$O

    • Structure: different arrangements of the same composition can yield different phases

  • Composition vs. Structure illustrated:

    • Ice:

    • Composition: H$_2$O

    • Structure: solid lattice arrangement

    • Water:

    • Composition: H$_2$O

    • Structure: liquid arrangement

Phase and Phase State

  • A phase is a piece of matter with uniform properties.

  • Phases are specified by:

    • Physical state (solid, liquid, gas, plasma)

    • Composition (pure substance vs. mixture, e.g., water vs. saline solution)

Physical States

  • Gas

    • Fixed volume? No

    • Assumes shape of container? Yes

    • Compressible? Yes

  • Liquid

    • Fixed volume? Yes

    • Shape of container? Yes

    • Compressible? No

  • Solid

    • Fixed volume? Yes

    • Shape of container? No

    • Compressible? No

  • Examples noted on the slide (illustrative): Helium (gas), water (liquid), NaCl (solid salt)

Plasma

  • Fourth state of matter; formed when a gas is exposed to high energies, creating a soup of ions and electrons

  • Example: Discharged neon (as in neon signs) showcases plasma behavior

Changes of State and Phase Diagram for Water

  • Changes of state depend on environmental conditions (pressure and temperature)

  • Phase Diagram for Water (key features):

    • Axes: Pressure (Pvap, atm) vs Temperature (°C)

    • Regions/phases: ice (solid), water (liquid), water vapor (gas)

    • Points of interest:

    • Normal freezing point: 0°C

    • Normal boiling point: 100°C

    • Triple point: where solid, liquid, and gas coexist; values shown on the diagram include Pvap ≈ 0.006 atm at T ≈ 0.01°C

    • Critical point: around 374°C (and corresponding Pvap not shown in the snippet)

  • The diagram helps explain phase transitions and why water behaves unusually (e.g., expands on freezing)

Chemical Composition

  • Chemical composition describes the elemental makeup of matter

  • Example: Glucose, C$6$H${12}$O$_6$ (a specific molecular formula)

The Periodic Table and Elements

  • The 118 elements are organized in the periodic table by atomic number and properties

  • Sample elements and classifications from the slide:

    • Hydrogen (H): Nonmetal; Group/Block information shown as part of the table

    • Helium (He): Noble Gas

    • Lithium (Li): Alkali Metal

    • Sodium (Na): Alkali Metal

    • Potassium (K): Alkali Metal

    • Rubidium (Rb): Alkali Metal

    • Cesium (Cs): Alkali Metal

    • Beryllium (Be): Alkaline Earth Metal

    • Magnesium (Mg): Alkaline Earth Metal

    • Silicon (Si): Metalloid

    • Phosphorus (P): Nonmetal

    • Sulfur (S): Nonmetal

    • Chlorine (Cl): Halogen

    • Argon (Ar): Noble Gas

  • The table includes grouping and block information (s, p, d, f blocks) and various metal/nonmetal classifications (e.g., Alkali Metal, Noble Gas, Halogen, Metalloid, Transition Metal, Post-Transition Metal, etc.)

  • There are additional elements listed (e.g., Ba, Hf, Ta, W, Os, Pt, Xe, Au, Hg, Pb, Bi, Po, Rn, Th, Pa, U, etc.) illustrating broad coverage across groups

  • The periodic table serves as a framework to understand element properties, trends, and chemical behavior

Compounds and the Law of Definite Proportions

  • Compounds are chemically-distinct substances composed of at least two different elements

  • Law of Definite Proportions: A compound always contains its component elements in a fixed ratio by mass

    • This means that, regardless of how a compound is prepared, its elemental mass composition is fixed

  • Example highlight: Water splitting demonstrates that H and O exist in a fixed proportion in the compound H$_2$O, which can be decomposed into its elements via processes like electrolysis

Water Splitting and Related Applications

  • Water splitting (electrolysis) is the process of decomposing water into its elements:

    • Chemical equation (example):
      H<em>2O(l)→H</em>2(g)+12O2(g)\mathrm{H<em>2O(l)} \rightarrow \mathrm{H</em>2(g)} + \tfrac{1}{2} \mathrm{O_2(g)}

  • This concept underpins practical technologies such as electrolysis and fuel cells, where electrical energy drives chemical changes in water and related systems

Kahoot! and Classroom Engagement

  • Informal quiz activity mentioned: Kahoot! with a provided link

  • Link: https://play.kahoot.it/#/?quizld=a35cfff8-f75b-4ebb-9ccb-c077ce86272b

  • Note: Described as never graded and for bragging rights in the session

Connections and Relevance

  • Foundational principles connect to broader topics in chemistry:

    • Stoichiometry and chemical proportions tie to the Law of Definite Proportions

    • States of matter and phase diagrams underpin thermodynamics and energy changes

    • Electronic structure and periodic trends (periodic table) relate to chemical bonding and molecular geometry

  • Real-world relevance: understanding how phase changes, chemical composition, and energy exchanges govern material behavior in everyday substances and advanced technologies (electrolysis, fuel cells, materials science)

Quick Reference Formulas and Key Points

  • Water formula: extH2extOext{H}_2 ext{O}

  • Water splitting (example equation): H<em>2O(l)→H</em>2(g)+12O2(g)\mathrm{H<em>2O(l)} \rightarrow \mathrm{H</em>2(g)} + \tfrac{1}{2} \mathrm{O_2(g)}

  • Phase points for water (typical values):

    • Normal freezing point: 0∘C0^{\circ}\mathrm{C}

    • Normal boiling point: 100∘C100^{\circ}\mathrm{C}

    • Triple point: T≈0.01∘C,  P≈0.006  atmT \approx 0.01^{\circ}\mathrm{C},\; P \approx 0.006\ \, \text{atm}

    • Critical point: T≈374∘CT \approx 374^{\circ}\mathrm{C}

End of notes from transcript content

This chemistry course (CHEM-113) focuses on understanding the universe's chemical rules and applying them to solve problems. It is the first in a two-term sequence.

Course Logistics

  • Instructor: Dr. Joe Elias

  • Office Hours: Mon/Thu/Fri 2:00-4:00 PM; Tue 3:00-4:00 PM

  • Meeting Time/Location: M/W/F 1:00-1:50 PM in C-221

  • Prerequisites: MATH 101 or satisfactory math placement

  • Topics: Stoichiometry, states of matter, atomic structure, periodic properties, bonding, molecular geometry, quantum mechanics, organic chemistry, thermochemistry.

What is Chemistry?

  • The study of matter, its changes, and the role of energy in these processes.

Matter: Properties, Composition, and Structure

  • Matter has mass (m) and volume (V).

  • Properties stem from composition (e.g., H2_2O) and structure (e.g., solid ice vs. liquid water arrangements).

Phase and Physical States

  • A phase is matter with uniform properties, defined by its physical state (solid, liquid, gas, plasma) and composition.

  • Gas: No fixed volume, assumes container shape, compressible.

  • Liquid: Fixed volume, assumes container shape, incompressible.

  • Solid: Fixed volume, fixed shape, incompressible.

  • Plasma: Fourth state, formed when high energy ionizes a gas.

Changes of State and Phase Diagram for Water

  • Phase changes depend on pressure (P) and temperature (T).

  • Water's Phase Diagram Key Points:

    • Normal freezing point: 0∘C0^{\circ}\mathrm{C}

    • Normal boiling point: 100∘C100^{\circ}\mathrm{C}

    • Triple point: T≈0.01∘C,  P≈0.006  atmT \approx 0.01^{\circ}\mathrm{C}, \; P \approx 0.006\ \ \text{atm}

    • Critical point: T≈374∘CT \approx 374^{\circ}\mathrm{C}

Chemical Composition and Elements

  • Chemical composition: Describes elemental makeup (e.g., Glucose, C<em>6H</em>12O∗6\text{C}<em>6\text{H}</em>{12}\text{O}*6).

  • Periodic Table: Organizes 118 elements by atomic number and properties (e.g., Alkali Metals, Halogens, Noble Gases).

Compounds and the Law of Definite Proportions

  • Compounds: Chemically distinct substances of at least two different elements.

  • Law of Definite Proportions: A compound always contains its elements in a fixed ratio by mass, regardless of preparation.

Water Splitting and Applications

  • Water Splitting (Electrolysis): Decomposes water into its elements:
    H<em>2O(l)→H</em>2(g)+12O2(g)\mathrm{H<em>2O(l)} \rightarrow \mathrm{H</em>2(g)} + \tfrac{1}{2} \mathrm{O_2(g)}

  • This principle is crucial for technologies like fuel cells.