Untitled Flashcards Set

CHAPTER 1

Know your definitions for the following.

Chemistry - the study of matter and the changes it undergoes.

Matter - anything that has mass and takes up space

Mass - a measurement that reflects the amount of matter.

Weight - a measure of mass and the force of gravity on an object.

Weight can change from place to place, but mass is constant.

Scientific Method

Law - a relationship in nature that is supported by many experiments, and no exceptions to these relationships are found.

Theory -  an explanation that has been repeatedly supported by many experiments.

Quantitative data - Data observed through numerical observations. 

Qualitative data - Data observed through observations such as color small or shape. 

Independent variable - A variable you can change.

Dependent Variable - An outcome variable as a result of the independent variable. 

The purpose of a control in an experiment - The standard for comparison.

Pure Research - research to gain knowledge for the sake of knowledge itself.

Applied Research - research undertaken to solve a specific problem.

Chance Discoveries - Chance discoveries occur when scientists obtain results that are far different from what they expected.

CHAPTER 2

X7 SI Base Units

How to use Metric Prefixes to do conversions. 

Temperature Conversions 

• K = C + 273

• F = (°C x 1.8) + 32

• C = (°F - 32) x 59

Derived units such as density (know how to solve for either density, mass or volume).

Writing numbers in scientific notation and standard form

Accuracy - ​​how close a measured value is to an accepted value.

Precision - how close a series of measurements are to one another.

Significant Figures (application in addition, subtraction, multiplication and division).

• All numbers in between #s 1-9

• Zeros after #s 1-9 if decimal point is present(even past decimal point)

• No zeros before #s 1-9

CHAPTER 3

States of Matter (difference between a gas and a vapor)

• Solid, Liquid, Gas

• Gas - no definite shape or volume. They expand to fill their container.

• Vapor - the gaseous state of a substance that is a solid or liquid at room temperature.

Physical properties - ​​characteristics that can be observed or measured without changing the sample’s composition.

Chemical properties - The ability of a substance to combine with or change into one or more other substances

Intensive vs Extensive properties

Physical change - A change that alters a substance without changing its composition 

Chemical Changes - A change that involves one or more substances turning into new substances

Law of Conservation of Mass - states that mass is neither created nor destroyed in a chemical reaction, it is conserved.

Compound - two or more elements combined chemically.
Element - a pure substance that cannot be separated into simpler substances by physical or chemical means.

Mixture - a combination of two or more pure substances in which each pure substance retains its individual chemical properties.

Homogeneous (solution) - a mixture where the composition is constant throughout.

Heterogeneous - a mixture where the individual substances remain distinct.

Separation of Mixtures (filtration, crystallization, distillation, sublimation, chromatography)

Law of definite proportions and Law of Multiple Proportions (Honors Only)

CHAPTER 4

The contributions of the following: Democritus, Dalton, Thompson, Rutherford, Chadwick (also Bohr and Schrodinger in the next chapter). What they discovered along with the experiments discussed in the lecture notes.

For protons, neutrons and electrons know their charge, mass and location in the atom.

Atomic Numbers and Mass Numbers

Isotopes, what are they and how to find the average atomic mass.

Calculate the % abundance of different isotopes.

CHAPTER 5

Know how to label a wave (amplitude, wavelength, trough, crest/peak, node)

Know how to solve for frequency, wavelength or the energy of a photon (the formulas will the provided) the c and h constant values will also be provided.

You must know the order of the electromagnetic spectrum and be able to compare which form of light has higher energy, frequency and wavelength.

Ground State vs Excited State of an atom.

Schrodinger’s quantum mechanical model of the atom

Know what an orbital is.

Know how to draw an Aufbau Principle Diagram

Also know Aufbau’s, Pauli’s and Hund’s rules.

How to write long-hand and short-hand electron configurations

Also, how to draw orbital diagrams.

Know the s²d⁴ becoming s¹d⁵ and s²d⁹ becoming s¹d¹⁰ exceptions.

CHAPTER 6

Familiarity with The Periodic Table, know the labeling of the 7 periods, 18groups / columns, along with the Main Group elements (1A-8A)

Know the nicknames (alkali, alkaline earth, chalcogens, halogens, noble gases, transition metals, lanthanides, actinides)

Know the location of metals, non-metals and metalloids. 

Know what valence electrons are and be able to identify them.

s,p,d,f block elements

Periodic Trends

INFORMATION PROVIDED ON YOUR TEST

You will be provided with the following information for your final exams.

A periodic table

Formula to solve for frequency, wavelength and energy of a photon along with the constants c and h.

Braden GPT⬆

Chat GPT⬇

CHAPTER 1: Fundamentals of Chemistry

1. Definitions:

   • Chemistry: Study of matter, its properties, and the changes it undergoes.

   • Matter: Anything that has mass and takes up space.

   • Mass vs. Weight:

     • Mass: Measure of the amount of matter.

     • Weight: Force of gravity acting on an object.

   • Scientific Method Steps:

     • Observation, Hypothesis, Experiment, Data Analysis, Conclusion.

   • Law vs. Theory:

     • Law: Describes a consistent natural phenomenon.

     • Theory: Explains why or how a phenomenon occurs.

   • Quantitative vs. Qualitative Data:

     • Quantitative: Numerical data (e.g., mass, volume).

     • Qualitative: Descriptive data (e.g., color, texture).

   • Independent vs. Dependent Variables:

     • Independent: The variable manipulated in an experiment.

     • Dependent: The variable measured in response to changes.

   • Control: Ensures experimental results are due to the independent variable.

   • Pure vs. Applied Research:

     • Pure: Knowledge for its own sake.

     • Applied: Solves specific problems.

   • Chance Discoveries: Unexpected results leading to new knowledge.

CHAPTER 2: Measurement and Calculations

1. SI Base Units: Length (meter), Mass (kilogram), Time (second), Temperature (Kelvin), Amount of substance (mole), Electric current (ampere), Luminous intensity (candela).

2. Metric Prefixes and Conversions: Practice converting (e.g., kilo-, centi-, milli-).

3. Temperature Conversions:

   • C=59(F−32)C = \frac{5}{9}(F - 32)

   • F=95C+32F = \frac{9}{5}C + 32

   • K=C+273.15K = C + 273.15

4. Density Formula: Density=MassVolume\text{Density} = \frac{\text{Mass}}{\text{Volume}}.

5. Scientific Notation and Standard Form: Convert between formats.

6. Accuracy and Precision:

   • Accuracy: How close a measurement is to the true value.

   • Precision: Consistency of repeated measurements.

7. Significant Figures: Rules for addition, subtraction, multiplication, and division.

CHAPTER 3: Matter and Its Properties

1. States of Matter:

   • Gas: No fixed shape or volume.

   • Vapor: Gaseous state of a substance typically liquid or solid.

2. Properties:

   • Physical: Observable without changing composition.

   • Chemical: Observed during chemical changes.

3. Intensive vs. Extensive Properties:

   • Intensive: Independent of amount (e.g., density).

   • Extensive: Dependent on amount (e.g., mass, volume).

4. Changes:

   • Physical: No change in composition.

   • Chemical: New substances formed.

5. Law of Conservation of Mass: Mass is conserved in chemical reactions.

6. Classification of Matter:

   • Pure Substances: Elements and compounds.

   • Mixtures: Homogeneous (uniform) and heterogeneous (non-uniform).

7. Separation Techniques: Filtration, distillation, sublimation, etc.

8. Laws of Proportions (Honors):

   • Definite Proportions: Same composition for a compound.

   • Multiple Proportions: Elements combine in ratios of small whole numbers.

CHAPTER 4: Atomic Structure

1. Contributions of Scientists:

   • Democritus: Atoms are indivisible.

   • Dalton: Atomic theory.

   • Thomson: Electron discovery (Cathode Ray Tube).

   • Rutherford: Nucleus (Gold Foil Experiment).

   • Chadwick: Neutron discovery.

2. Subatomic Particles:

   • Protons (+, nucleus), Neutrons (0, nucleus), Electrons (-, orbitals).

3. Atomic and Mass Numbers: Atomic number = protons; Mass number = protons + neutrons.

4. Isotopes and Atomic Mass:

   • Isotopes: Atoms of the same element with different neutrons.

   • Average Atomic Mass Calculation: Weighted Average=∑(Mass×%Abundance)\text{Weighted Average} = \sum (\text{Mass} \times \% \text{Abundance}).

CHAPTER 5: Electrons in Atoms

1. Wave Properties:

   • Diagram: Amplitude, wavelength, crest, trough.

   • Calculations: Frequency (ff), wavelength (λ\lambda), and energy (EE).

2. Electromagnetic Spectrum: Know order and energy relationships.

3. Quantum Model:

   • Ground vs. Excited States.

   • Schrödinger’s Model: Electrons in orbitals.

4. Electron Configuration:

   • Aufbau Principle, Pauli Exclusion, Hund's Rule.

   • Long-hand/short-hand configurations.

   • Orbital Diagrams.

5. Exceptions: s1d5s^1d^5, s1d10s^1d^{10}.

CHAPTER 6: The Periodic Table

1. Structure:

   • 7 Periods, 18 Groups (Main Groups: 1A-8A).

   • Block Elements: s,p,d,fs, p, d, f.

2. Nicknames:

   • Alkali Metals, Alkaline Earth, Halogens, etc.

3. Metals, Non-Metals, Metalloids: Locations on the table.

4. Valence Electrons: Outer electrons in chemical bonding.

5. Periodic Trends: Atomic size, ionization energy, electronegativity.

TEST HINTS:

• Use the periodic table provided.

• Use constants and formulas for photon energy calculations.