Science Chapter 2 - Analyzing Data

Study Notes

Chapter 2 – Analyzing Data

Measurements of Matter:
- Volume is measured in liters (L) or cubic meters (m³).
- Volume formulas: Cube (side³), Cylinder (πr²h).
- Mass is measured in grams (g) or kilograms (kg).
- Temperature is measured in Kelvin (K), Celsius (°C), or Fahrenheit (°F), with conversion formulas provided.
Accuracy, Precision, and Error:
- Accuracy is the closeness to the true value.
- Precision is the reproducibility of measurements.
- Percent error is a calculation of the difference between measured and true values.
SI Units and Prefixes:
- Base units: meter (m), kilogram (kg), second (s), mole (mol), Kelvin (K), liter (L).
- Prefixes (e.g., kilo-, centi-, milli-) are used to represent multiples or fractions of base units.
Dimensional Analysis:
- Use conversion factors to change units.
Density:
- Formula: Density = Mass/Volume
- Units: g/cm³, kg/m³.
Significant Figures:
- Rules for determining significant figures are presented.
Scientific Notation:
- Express numbers in the form a × 10^b, where 1 ≤ |a| < 10.
Graphing:
- Independent variable on the x-axis.
- Dependent variable on the y-axis.

Chapter 3 – Matter: Properties and Change

Physical vs. Chemical Properties:
- Physical properties are observed without changing composition (e.g., melting point, density).
- Chemical properties are observed through a chemical change (e.g., reactivity, flammability).
Physical vs. Chemical Changes:
- Physical changes alter appearance without forming new substances.
- Chemical changes form new substances.
Law of Conservation of Mass:
- Mass is conserved in chemical reactions (mass is neither created nor destroyed).
Compounds, Elements, and Mixtures:
- Compounds are substances formed by chemically combining two or more elements.
- Elements are pure substances composed of one type of atom.
- Mixtures are combinations of two or more components that are not chemically bonded.
  - Homogeneous mixtures are uniform throughout.
  - Heterogeneous mixtures are not uniform.
Separation Methods:
- Common methods include filtration, distillation, chromatography, and evaporation.
Intensive vs. Extensive Properties:
- Intensive properties are independent of the amount of substance.
- Extensive properties depend on the amount of substance.

Chapter 4 – The Structure of the Atom

Historical Models:
- Dalton: Atoms are indivisible.
- Rutherford: Atoms have a dense, positively charged nucleus.
Subatomic Particles:
- Proton: positive charge, mass ≈ 1 amu.
- Neutron: neutral charge, mass ≈ 1 amu.
- Electron: negative charge, negligible mass.
Isotopes:
- Atoms of the same element with different numbers of neutrons.
- Average atomic mass is calculated using abundance of isotopes.
Nuclear Decay:
- Types include alpha (α), beta (β), and gamma (γ) decay.
Half-Life:
- Formula for calculating half-life is presented.

Chapter 5 – Electrons in Atoms

Bohr Model:
- Electrons orbit in specific energy levels.
Energy of a Photon:
- Formula for calculating the energy of a photon is provided.
Orbitals:
- Types of orbitals (e.g., s, p) and their shapes are discussed.
Electron Configuration:
- Principles (Aufbau, Pauli Exclusion, Hund's) used to predict electron arrangement.

Chapter 6 – The Periodic Table

Groups/Families:
- Classification of elements based on their properties (e.g., alkali metals, halogens).
Periodic Trends:
- Discussion of trends in atomic radius, ionization energy, and electronegativity across periods and down groups.
Coulomb's Law:
- Formula for calculating the force between charged particles is provided.

Chapter 7 – Ionic Compounds and Metals

Octet Rule:
- Atoms tend to gain or lose electrons to achieve a stable octet of valence electrons.
Formulas for Ionic Compounds:
- Cations and anions combine to create neutral compounds.

Chapter 8 – Covalent Bonding

Naming Binary Covalent Compounds:
- Prefixes (mono-, di-, tri-, tetra-, penta-) used to indicate the number of atoms of each element.
Acids:
- Naming of binary and oxyacids.

Description

Explore key concepts of data analysis in this quiz covering measurements of matter, accuracy, precision, and significant figures. You'll learn about SI units, dimensional analysis, density calculations, and error measurement. This quiz is designed to reinforce your understanding of scientific measurement principles.