1: Notes & Gas Laws
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Questions and Answers

What does Dalton’s Atomic Theory state about elements?

  • All elements are composed of molecules.
  • All atoms of different elements are identical.
  • Atoms can be created and destroyed in reactions.
  • Each element is composed of atoms. (correct)

Dalton's Atomic Theory states that all atoms of a given element are chemically identical.

True (A)

What law states that mass is neither created nor destroyed in chemical reactions?

Law of Conservation of Mass

The law of _________ states that when two elements form different compounds, the ratios of the masses of the second element that combine with a fixed mass of the first element can be expressed in small whole numbers.

<p>Multiple Proportions</p> Signup and view all the answers

Match the following concepts to their descriptions:

<p>Law of Constant Composition = A compound always contains the same proportion of elements. Conservation of Mass = Mass is conserved in a chemical reaction. Multiple Proportions = Different compounds formed from the same elements have ratios of mass that can be expressed in whole numbers. Atoms = Building blocks of matter.</p> Signup and view all the answers

What is the correct approach to balance the equation $a H_2 + b O_2 \rightarrow c H_2O$?

<p>Set a = 1, then c = 1 and b = 2 (A)</p> Signup and view all the answers

Changing coefficients in a chemical equation affects the actual substances involved.

<p>False (B)</p> Signup and view all the answers

What is the key condition for balancing coefficients in a chemical equation?

<p>The number of atoms of each element must be equal on both sides of the equation.</p> Signup and view all the answers

To balance a chemical equation, you should change the ______ but not the ______.

<p>coefficients, subscripts</p> Signup and view all the answers

Match the term with its definition:

<p>Coefficients = Numbers placed in front of reactants and products to balance an equation Subscripts = Numbers that indicate the number of atoms in a molecule Balanced Equation = An equation where the number of each type of atom is the same on both sides Chemical Reaction = A process that leads to the transformation of one set of chemical substances to another</p> Signup and view all the answers

What is the smallest unit of an element?

<p>Atom (B)</p> Signup and view all the answers

Pure substances can have varying compositions from sample to sample.

<p>False (B)</p> Signup and view all the answers

Name a characteristic of a homogeneous mixture.

<p>It has a uniform composition.</p> Signup and view all the answers

A mixture that consists of two or more pure substances that is not uniform is known as a __________ mixture.

<p>heterogeneous</p> Signup and view all the answers

Which of the following is an example of a homogeneous mixture?

<p>Mineral water (B)</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Elements = Substances made of only one atom type Compounds = Molecules with different types of atoms Molecules = Two or more atoms joined together Mixtures = Contain two or more pure substances</p> Signup and view all the answers

Chemical changes that describe how substances react are known as __________.

<p>reactions</p> Signup and view all the answers

All substances with the same physical appearance are necessarily homogeneous mixtures.

<p>False (B)</p> Signup and view all the answers

Match the following key areas to their relevance in engineering:

<p>Hydrogen-fired turbines = Alternative energy solutions Carbon capture = Environmental engineering Biomedical devices = Healthcare technology Batteries = Energy storage systems</p> Signup and view all the answers

What is the formula weight (FW) of water (H2O)?

<p>18.0 u (D)</p> Signup and view all the answers

The empirical formula is used to determine molecular weight for ionic solids.

<p>True (A)</p> Signup and view all the answers

What does FW stand for in chemistry?

<p>Formula weight</p> Signup and view all the answers

The molecular weight of H2O is ____ u.

<p>18.0</p> Signup and view all the answers

What is the correct way to write the formula for sodium chloride?

<p>NaCl (C)</p> Signup and view all the answers

Molecular weight (Mw) and formula weight (FW) are different concepts.

<p>False (B)</p> Signup and view all the answers

How many grams of O2 can react with 2.00 g of H2?

<p>This question requires a calculation based on stoichiometry.</p> Signup and view all the answers

Match the following chemical terms with their definitions:

<p>Formula Weight = Sum of atomic weights in a formula Molecular Weight = Another term for formula weight Ionic Solid = Compound consisting of ions Empirical Formula = Simplest whole-number ratio of atoms</p> Signup and view all the answers

Flashcards

Moodle

The digital platform used to provide all course information for Chemistry.

Chemistry: The Central Science in SI Units

The assigned textbook for Chemistry.

Office Hours

Regular sessions where students can ask questions and get help with the material.

Prof. David J. Norris

The professor teaching the Chemistry course.

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Thursdays, 17:00-18:00

The specific day and time when the professor will be available during office hours.

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0.25 point bonus on final grade

A bonus point awarded to students who pass at least two out of three graded problem sets.

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PS #1

The name of the first problem set assigned in the course.

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Friday, Sept. 27, 14:00

The deadline for submitting the first problem set.

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MAVT Engineers and Chemistry

Engineers graduating from the MAVT department at ETH Zurich are now expected to work in diverse fields requiring a solid base in chemistry.

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Why Chemistry for Engineers?

Learning chemistry is essential for modern engineering, especially for engineers facing critical global challenges.

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MAVT and the Regret of Neglecting Chemistry

Engineers from the MAVT department at ETH Zurich were previously advised to neglect chemistry, a decision they later came to regret.

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Goals of the Introductory Chemistry Course

This introductory chemistry course aims to provide students with a broad foundation in basic chemical concepts.

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Engaging Students in Chemistry

The course facilitator strives to keep all students engaged and actively involved in learning the material.

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Lifelong Learning in Chemistry

Learning chemistry is an ongoing process. Even experts continue to learn and expand their knowledge.

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Experts: Continuous Learning

Even those with extensive knowledge in chemistry continue to actively engage in learning and new discoveries.

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Tutorials in Early Exercises

The course will incorporate practical tutorials into the early exercises to reinforce learning.

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What is an atom?

The smallest unit of an element, the building blocks of matter.

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Elements

Substances made of only one type of atom. Examples: gold (Au), oxygen (O2).

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Molecules

Two or more atoms joined together by chemical bonds. Examples: water (H2O), carbon dioxide (CO2).

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Compounds

Molecules made up of two or more different types of atoms. Examples: water (H2O), sodium chloride (NaCl).

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Chemical Reactions

A description of how matter changes during chemical reactions.

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Pure Substances

Substances with a fixed composition that doesn't change from sample to sample. Examples: pure water, gold.

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Homogeneous Mixture

A mixture with uniform composition throughout. Examples: salt water, air.

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Heterogeneous Mixture

A mixture with non-uniform composition, different parts have different properties. Examples: sand and water, oil and water.

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What is Dalton's Atomic Theory?

Dalton's Atomic Theory states that all matter is composed of tiny, indivisible particles called atoms. These atoms are the fundamental building blocks of elements, and they cannot be created or destroyed in chemical reactions.

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What makes atoms of different elements unique?

Each element is made up of a unique type of atom. For instance, all gold atoms are identical, while all silver atoms are distinct from gold atoms.

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Are all atoms of the same element the same?

Atoms of the same element are chemically identical, meaning they have the same properties and mass. For example, all hydrogen atoms are alike.

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What happens to atoms in chemical reactions?

Atoms cannot be changed, created, or destroyed during ordinary chemical reactions. They simply rearrange themselves to form new substances.

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How are compounds formed?

Compounds are formed when atoms of different elements combine in fixed ratios. For example, water (H2O) always consists of two hydrogen atoms and one oxygen atom.

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What are chemical equations?

A method of representing chemical changes using symbols and formulas that demonstrates the conservation of matter.

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What are coefficients in chemical equations?

Numbers placed in front of chemical formulas in an equation to balance the number of atoms of each element on both sides.

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What does it mean to balance a chemical equation?

To adjust the coefficients in a chemical equation so that the number of atoms of each element is the same on both sides.

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What are chemical reactions?

The rearrangement of atoms to form new substances, indicated by changes in chemical composition.

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What are subscripts in chemical formulas?

Subscripts within chemical formulas indicate the number of atoms of a particular element in a molecule or compound. They cannot be changed to balance an equation.

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Formula Weight (FW)

The sum of the atomic weights of all atoms in a chemical formula.

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Molecular Weight (Mw)

The formula weight of a molecule.

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Empirical Formula

The smallest whole-number ratio of atoms in a compound.

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Study Notes

Chemistry Lecture 1 Notes

  • The lecturer is Prof. David J. Norris
  • Email: [email protected]
  • Office: LEE P210
  • Office hours: Thursdays 17:00-18:00 or by appointment
  • The course uses American English
  • Chalkboard and slides will be used for teaching
  • Lecturer is from Chicago
  • Teaching assistants are listed on page 2
  • All course information is available on Moodle: https://moodle-app2.let.ethz.ch/course/view.php?id=22903
  • Textbook: Chemistry: The Central Science in SI Units, 15th Edition, ©2022, by Theodore E. Brown, et al.
  • Exercises are held Fridays 14:00-16:00
  • Problem sets are weekly, and 3 are randomly graded
  • Pass 2 out of 3 problem sets for bonus
  • Problem set 1 is due Friday, Sept. 27, 14:00
  • Required textbook is available in the ETH Store (Orell Füssli) and online.
    • ISBN: 978-1-292-40761-6
    • Price: CHF 88.90

Why Chemical Knowledge is Important

  • Some engineering students initially underestimate the need for chemistry
  • Many fields of engineering rely on chemistry, including mechanical and process engineering
  • Students are urged to develop strong chemical knowledge
  • Students may regret skipping basic chemistry
  • Chemical knowledge is crucial in important engineering and technological areas including, but not limited to:
    • batteries
    • Hydrogen-fired turbines
    • Carbon capture
    • Transportation
    • Biomedical devices

Goals for the Course

  • Introductory chemistry course designed for engineering students
  • Goal of the course is to provide a foundation in basic chemistry
  • The lecturer wants to engage all students, even experts

Your Challenge

  • The lecturer expects students to ask questions
  • The lecturer will do everything possible to clarify any questions
  • Students should stay engaged during the lecture and in doing the exercises/problem sets

Apologies in Advance

  • There may be some handwriting-related problems with the lecture slides
  • German translations to specific lecture slides/exercises can be requested if necessary
  • Students can provide feedback

Lecture Content - What is Chemistry, Atoms, and the Periodic Table

  • Chemistry is defined as the study of matter and its properties and behavior

  • Elements are substances made up of one type of atom

  • Molecules are made from atoms of different elements

  • Compounds contain atoms from different elements joined together

  • The study of chemical changes forms the heart of chemical reactions (and this is distinct from physical changes, like melting ice)

    • During chemical reactions, energy is either absorbed or released
    • Atoms are neither created nor destroyed during chemical reactions (this is important)

  • Atoms are composed of smaller particles

  • Protons, neutrons, and electrons are the main subatomic particles and have different properties each

  • Structure of the atom has the nucleus at the center with electrons circulating

  • Atoms in an element are identical chemically

  • Atoms from different elements combine to produce compounds

  • Periodic table organizes elements by atomic number (that determines the properties, and it is often already in order)

  • The number of protons determines the type of atom, and also the behaviour

    • elements in the same column (group) of the periodic table display similar properties

More Lecture Content

  • Chemical equations describe chemical changes
  • Atom types must be balanced on the reactant and product sides
  • Some important laws of chemical reactions are constant composition, conservation of mass, and multiple proportions.
  • Definition and examples of Polyatomic ions
  • Names and formulas for important cations and anions are essential in naming and understanding ionic compounds.

Further Lecture Content:

  • The mole is a standard that equals 6.02 x 1023
  • The atomic mass of an element expressed in grams contains one mole of atoms.
  • Formula weight is sum of the atomic weights of the atoms in a molecule
  • The concept of molar mass is defined as grams per mole, and molar mass is determined from the molecular formula

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ETH Zurich Chemistry Lecture 1 PDF Fall 2024

Description

Explore the foundational concepts presented in the first lecture of the Chemistry course led by Prof. David J. Norris. This lecture highlights important course information, textbooks, and the significance of chemical knowledge in engineering. Ideal for students looking to enhance their understanding of chemistry in a practical context.

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