Chemistry Final Exam Flashcards

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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?

False Signup and view all the answers

Are zeros at the end of a number and to the right of the decimal significant?

True Signup and view all the answers

What is the rule for addition/subtraction in regards to significant figures?

Round numbers to the least number of decimal places. Signup and view all the answers

What is the rule for multiplication/division in regards to significant figures?

Round answers to the least amount of significant figures. Signup and view all the answers

How many electrons are equivalent to the number of protons?

The number of electrons equals the number of protons. Signup and view all the answers

What is atomic mass?

Number of protons in the nucleus. Signup and view all the answers

What is atomic mass number?

Number of protons and neutrons. Signup and view all the answers

What is an isotope?

Atoms of the same element with different masses. Signup and view all the answers

Do columns or rows in the Periodic Table have similar patterns?

Columns have repeating patterns. Signup and view all the answers

Which area of the Periodic Table has greater metallicness?

Left and down. Signup and view all the answers

Which area of the Periodic Table has greater atomic size?

Left and down. Signup and view all the answers

Which area of the Periodic Table has greater ionization energy?

Right side and up. Signup and view all the answers

Which area of the Periodic Table has greater electronegativity?

Right side and up, except for the Noble Gases. Signup and view all the answers

What is ionic bonding?

A metal and a nonmetal giving/taking electrons. Signup and view all the answers

What is covalent bonding?

Nonmetals sharing electrons. Signup and view all the answers

What is VSEPR theory?

Valence Shell Electron Pair Repulsion. Signup and view all the answers

How do you determine polarity?

Subtract the electronegativity values of the elements in the compound. Signup and view all the answers

Is water polar?

True Signup and view all the answers

What is a combination reaction?

A + B --> AB Signup and view all the answers

What is a decomposition reaction?

AB --> A + B Signup and view all the answers

What is a single replacement reaction?

AB + C --> AC + B Signup and view all the answers

What is a double replacement reaction?

AB + CD --> AD + CB Signup and view all the answers

What is a combustion reaction?

C + H + O --> H2O + CO2 always. Signup and view all the answers

What is Avogadro's number?

6.022 x 10^23 particles = 1 mole. Signup and view all the answers

What is molar mass?

Gram/mole. Signup and view all the answers

What is the volume of one mole?

1 mole = 22.4 L. Signup and view all the answers

What is the difference between empirical formula and molecular formula?

Molecular = actual number of atoms; Empirical = smallest ratio of atoms. Signup and view all the answers

What is percent composition?

Mass element/mass compound x 100. Signup and view all the answers

What is a limiting reactant?

The reactant which runs out first. Signup and view all the answers

Which state of matter has the greatest kinetic energy?

Gas. Signup and view all the answers

What are the three types of intermolecular forces?

Hydrogen bonding, dipole attraction, dispersion forces. Signup and view all the answers

What do you call a solid changing to a gas?

Sublimation. Signup and view all the answers

What are the values for STP?

0 Celsius or 273 Kelvin, 1 atm = 101.3 kPa = 760 mmHg. Signup and view all the answers

Why is the pressure of a gas directly proportional to the number of particles?

Because pressure is caused by collisions of gas. Signup and view all the answers

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.
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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Description

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.