Questions and Answers
What is accuracy?
Closeness of measurements to the true value of what is being measured.
What is precision?
Closeness of a set of measurements.
How do you calculate Percent Error?
| experimental - accepted | / accepted value x 100
Are zeros in front of non-zero digits significant?
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Are zeros at the end of a number and to the right of the decimal significant?
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What is the rule for addition/subtraction in regards to significant figures?
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What is the rule for multiplication/division in regards to significant figures?
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How many electrons are equivalent to the number of protons?
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What is atomic mass?
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What is atomic mass number?
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What is an isotope?
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Do columns or rows in the Periodic Table have similar patterns?
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Which area of the Periodic Table has greater metallicness?
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Which area of the Periodic Table has greater atomic size?
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Which area of the Periodic Table has greater ionization energy?
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Which area of the Periodic Table has greater electronegativity?
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What is ionic bonding?
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What is covalent bonding?
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What is VSEPR theory?
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How do you determine polarity?
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Is water polar?
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What is a combination reaction?
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What is a decomposition reaction?
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What is a single replacement reaction?
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What is a double replacement reaction?
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What is a combustion reaction?
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What is Avogadro's number?
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What is molar mass?
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What is the volume of one mole?
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What is the difference between empirical formula and molecular formula?
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What is percent composition?
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What is a limiting reactant?
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Which state of matter has the greatest kinetic energy?
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What are the three types of intermolecular forces?
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What do you call a solid changing to a gas?
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What are the values for STP?
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Why is the pressure of a gas directly proportional to the number of particles?
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Study Notes
Measurement and Significant Figures
- Accuracy: Closeness of measurements to the true value of what is being measured.
- Precision: Closeness of a set of measurements to each other.
- Percent Error Calculation: (|\text{experimental} - \text{accepted}| / \text{accepted} \times 100)
- Significant Zeros: Zeros in front of non-zero digits are not significant (e.g., 0.0071 has 2 significant figures).
- Trailing Zeros: Zeros at the end of a number and to the right of the decimal are significant (e.g., 9.100 has 4 significant figures).
- Addition/Subtraction: Round results to the least number of decimal places in the calculation.
- Multiplication/Division: Round results to the least number of significant figures.
Atomic Structure
- Electrons: The number of electrons equals the number of protons in a neutral atom.
- Atomic Mass: Number of protons in the nucleus, indicated at the bottom left of the chemical symbol.
- Atomic Mass Number: Total number of protons and neutrons, indicated at the top left of the chemical symbol.
- Isotopes: Atoms of the same element with different masses due to a varying number of neutrons.
Periodic Table Trends
- Columns in Periodic Table: Groups show repeating patterns in properties.
- Metallic Character: Increases as you move left and down the Periodic Table.
- Atomic Size: Increases as you move left and down the Periodic Table.
- Ionization Energy: Increases as you move right and up the Periodic Table.
- Electronegativity: Increases as you move right and up, with noble gases exhibiting zero electronegativity.
Bonding
- Ionic Bonding: Involves a metal and a nonmetal; electrons are transferred.
- Covalent Bonding: Involves nonmetals; electrons are shared between atoms.
- VSEPR Theory: Valence Shell Electron Pair Repulsion; electron pairs arrange themselves to minimize repulsion.
Chemical Reactions
- Polarity Determination: Subtract electronegativity values of atoms in a compound.
- Water: Exhibits polar characteristics.
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Reaction Types:
- Combination Reaction: ( A + B \rightarrow AB )
- Decomposition Reaction: ( AB \rightarrow A + B )
- Single Replacement Reaction: ( AB + C \rightarrow AC + B )
- Double Replacement Reaction: ( AB + CD \rightarrow AD + CB )
- Combustion Reaction: Always produces water and carbon dioxide, represented as ( C + H + O \rightarrow H_2O + CO_2 ).
Stoichiometry and Moles
- Avogadro's Number: ( 6.022 \times 10^{23} ) particles per mole.
- Molar Mass: Expressed in grams per mole (g/mol).
- Mole to Volume: One mole of gas occupies 22.4 liters at STP.
- Empirical vs Molecular Formula: Molecular formulas show actual atom counts while empirical formulas show the simplest ratio.
- Percent Composition: Calculated as ( \text{mass of element} / \text{mass of compound} \times 100 ).
- Limiting Reactant: The reactant that runs out first and restricts product formation.
Kinetic Theory and States of Matter
- Kinetic Energy: Gases have the greatest kinetic energy due to particles being widely spaced and fast-moving.
- Intermolecular Forces: Include hydrogen bonding, dipole attraction, and dispersion forces.
- Phase Change: Transition from solid to gas is called sublimation.
Standard Temperature and Pressure (STP)
- Values for STP: 0°C (273 K); pressure is 1 atm (101.3 kPa or 760 mmHg).
Gas Behavior
- Pressure and Particle Count: Gas pressure is directly proportional to the number of particles, with more particles causing more frequent collisions.
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Prepare for your Chemistry final with these comprehensive flashcards covering key concepts like accuracy, precision, and percent error. Each card provides clear definitions to help reinforce your understanding of essential chemistry principles.