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Questions and Answers
Which of the following correctly defines chemistry?
Which of the following correctly defines chemistry?
Which of the following is a characteristic feature of a homogeneous mixture?
Which of the following is a characteristic feature of a homogeneous mixture?
What is the Kelvin equivalent of 25 degrees Celsius?
What is the Kelvin equivalent of 25 degrees Celsius?
What does the atomic number of an element represent?
What does the atomic number of an element represent?
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How do you calculate the mass number of an atom?
How do you calculate the mass number of an atom?
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Which of the following best describes an isotope?
Which of the following best describes an isotope?
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What is the relationship between atomic mass unit (amu) and grams?
What is the relationship between atomic mass unit (amu) and grams?
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Which of the following represents a cation?
Which of the following represents a cation?
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What is the likely charge of an ion formed by an element in group 1 of the periodic table?
What is the likely charge of an ion formed by an element in group 1 of the periodic table?
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Which of the following best describes the difference between ionic and molecular compounds?
Which of the following best describes the difference between ionic and molecular compounds?
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Which of the following statements accurately defines Avogadro's number?
Which of the following statements accurately defines Avogadro's number?
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How can the empirical formula of a compound be determined from percent composition?
How can the empirical formula of a compound be determined from percent composition?
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What is the main difference between molar mass and molecular weight?
What is the main difference between molar mass and molecular weight?
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Study Notes
Chemistry Definition
- Chemistry studies the composition, structure, properties, and reactions of matter
Matter & Non-Matter
- Matter has mass and takes up space
- Non-matter lacks mass and does not occupy space
SI Units of Measurement
- Length: meter (m)
- Mass: kilogram (kg)
- Time: second (s)
- Temperature: Kelvin (K)
- Amount of substance: mole (mol)
- Electric current: ampere (A)
- Luminous intensity: candela (cd)
SI/Metric Unit Prefixes
- Kilo (k): 1000
- Hecto (h): 100
- Deka (da): 10
- Deci (d): 0.1
- Centi (c): 0.01
- Milli (m): 0.001
- Micro (µ): 0.000001
- Nano (n): 0.000000001
Scientific Notation
- Expressing very large or very small numbers using powers of 10
Density & Calculations
- Density: mass per unit volume
- Formula: Density = Mass/Volume
Dimensional Analysis
- Converting between different units using conversion factors
Temperature Conversions
- Celsius to Fahrenheit: °F = (°C × 9/5) + 32
- Fahrenheit to Celsius: °C = (°F - 32) × 5/9
- Kelvin to Celsius: K = °C + 273.15
- Celsius to Kelvin: °C = K - 273.15
Matter Classifications
- Pure substances: elements and compounds
- Mixtures: homogeneous and heterogeneous
Homogeneous vs. Heterogeneous Mixtures
- Homogeneous: uniform composition
- Heterogeneous: non-uniform composition
States of Matter
- Solid: fixed shape and volume
- Liquid: fixed volume, but takes the shape of its container
- Gas: no fixed shape or volume, expands to fill its container
Phase Changes
- Solid to liquid: melting
- Liquid to solid: freezing
- Liquid to gas: vaporization
- Gas to liquid: condensation
- Solid to gas: sublimation
- Gas to solid: deposition
Physical and Chemical Changes
- Physical change: alters the form or appearance of a substance, but not its chemical composition
- Chemical change: results in the formation of new substances with different chemical properties
Physical and Chemical Properties
- Physical property: can be observed without changing the substance's composition
- Chemical property: describes how a substance reacts with other substances
Atomic Structure
- Composed of protons, neutrons, and electrons
- Protons: positive charge, located in the nucleus
- Neutrons: no charge, located in the nucleus
- Electrons: negative charge, located in the electron cloud surrounding the nucleus
Atomic Number
- Number of protons in an atom's nucleus, defining the element
Chemical Symbols
- One or two letters representing an element
Isotopes
- Atoms of the same element with different numbers of neutrons
- Same atomic number, but different mass numbers
Average Atomic Mass
- Weighted average of the masses of all naturally occurring isotopes of an element
Ions
- Atoms that have gained or lost electrons
- Cations: positively charged ions
- Anions: negatively charged ions
Polyatomic Ions
- Groups of atoms with an overall charge
Ionic Compounds
- Formed by the electrostatic attraction between oppositely charged ions
Molecular Compounds
- Formed by the sharing of electrons between atoms
Mole & Avogadro's Number
- Mole: a unit of amount of substance
- Avogadro's number: 6.022 × 10^23 particles per mole
Atomic Weight, Molecular Weight, & Molar Mass
- Atomic weight: mass of one atom of an element
- Molecular weight: mass of one molecule of a compound
- Molar mass: mass of one mole of a substance
Percent Composition
- Percentage by mass of each element in a compound
Empirical & Molecular Formulas
- Empirical formula: simplest whole-number ratio of atoms in a compound
- Molecular formula: actual number of atoms of each element in a molecule
Finding Empirical & Molecular Formulas
- Empirical formula from percent composition: convert percentage to mass, then to moles, and find the simplest whole-number ratio of moles
- Molecular formula from empirical formula: calculate the molar mass of the empirical formula, and divide the molar mass of the compound by the molar mass of the empirical formula to determine the multiplier for the empirical formula
Practice Problems
- Chapter 1 (Page 50): 9, 11, 13, 19, 25, 29, 39, 45, 57, 65, 67, 75, 81, 87, 89, 93, 95, 97
- Chapter 2 (Page 107): 7, 19, 25, 29, 33, 39, 41, 47
- Chapter 3 (Page 151): 1, 5, 9, 13, 17, 19, 25, 27, 31, 39, 43
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Description
Test your knowledge on fundamental chemistry concepts including matter, SI units, and density calculations. This quiz will also cover scientific notation and temperature conversions, helping you solidify your understanding of essential measurement principles in chemistry.
