Skip to main content
Indietro

General Chemistry Chapter 1 & E Study Flashcards

I pulsanti di controllo sono stati cambiati in modalità "navigazione".
1/26

Termini in questo insieme (26)

  • Difference between accuracy and precision

    Accuracy refers to how close measurements are to the true value, while precision refers to how close measurements are to each other.

  • How to determine the number of significant figures in 3.04 cm

    3.04 cm has 3 significant figures because all nonzero digits and zeros between them count.

  • How to write 7,600,000 kg with three significant figures

    Write as \(7.60\times10^{6}\) kg to show three significant figures.

  • Conversion between cm³ and mL

    1 cm³ = 1 mL, so volume in cubic centimeters equals volume in milliliters.

  • Conversion between dm³ and L

    1 dm³ = 1 L, so volume in cubic decimeters equals volume in liters.

  • Definition of intensive vs extensive properties

    Intensive properties do not depend on amount (e.g., density, color). Extensive properties depend on amount (e.g., mass, volume, length).

  • How to perform dimensional analysis

    Use conversion factors with units to cancel and convert quantities step-by-step, always including units throughout.

  • Number of protons in an atom

    The number of protons equals the atomic number of the element from the periodic table.

  • Number of neutrons in an isotope

    Neutrons = mass number - atomic number.

  • Definition of a cation and anion

    Cations are positively charged ions; anions are negatively charged ions.

  • How to calculate average atomic mass

    Average atomic mass = sum of (isotope mass × fractional abundance) for all isotopes.

  • How to convert moles to grams

    Use molar mass as a conversion factor: \(\text{grams} = \text{moles} \times \text{molar mass}\\).

  • How to convert grams to number of atoms

    Convert grams to moles using molar mass, then moles to atoms using Avogadro's number.

  • How to determine the charge of an ion

    Charge = number of protons - number of electrons.

  • How to identify significant figures in 5200 m

    5200 m has 2 significant figures if no decimal is shown; trailing zeros without a decimal are not significant.

  • How to add measurements with significant figures

    Result should be rounded to the least number of decimal places among the numbers added.

  • How to multiply measurements with significant figures

    Result should be rounded to the least number of significant figures among the numbers multiplied.

  • Density formula

    Density = mass / volume, often expressed in g/mL or g/cm³.

  • How to convert 3.4 L to mL

    Multiply by 1000: \(3.4\,\text{L} \times 1000 = 3400\,\text{mL}\).

  • How to calculate volume of a room in liters

    Calculate volume in cubic feet, convert to cubic meters, then to liters (1 m³ = 1000 L).

  • How to convert fuel efficiency from mi/gal to km/L

    Convert miles to kilometers and gallons to liters using conversion factors, then divide.

  • How to calculate number of electrons in Mg2+ ion

    Mg atomic number is 12, Mg2+ has lost 2 electrons, so electrons = 10.

  • How to calculate mass from number of atoms

    Convert atoms to moles using Avogadro's number, then moles to grams using molar mass.

  • How to determine if a measurement is precise but inaccurate

    Measurements are close to each other but far from the true value.

  • How to express 5.200 x 10³ m in significant figures

    It has 4 significant figures because all digits including zeros after decimal count.

  • How to calculate mass consumed given volume and density

    Mass = volume × density; convert units as needed.