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General Chemistry Test 2 Study Guide

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Termini in questo insieme (25)

  • What is matter and how is it classified?

    Matter is anything that has mass and occupies space. It is classified into pure substances and mixtures.

  • Define pure substances and give examples.

    Pure substances have a fixed composition and include elements (e.g., oxygen) and compounds (e.g., water).

  • What are mixtures? Differentiate homogeneous and heterogeneous mixtures.

    Mixtures contain two or more substances physically combined. Homogeneous mixtures are uniform (e.g., salt water), heterogeneous mixtures are not (e.g., salad).

  • Define physical and chemical changes with examples.

    Physical changes alter appearance but not composition (e.g., melting ice). Chemical changes alter composition (e.g., rusting iron).

  • What are physical and chemical properties? Give examples.

    Physical properties can be observed without changing composition (e.g., color). Chemical properties describe reactivity (e.g., flammability).

  • Explain intensive and extensive physical properties with examples.

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

  • List the 7 basic SI units.

    Meter (length), Kilogram (mass), Second (time), Ampere (electric current), Kelvin (temperature), Mole (amount of substance), Candela (luminous intensity).

  • How do you convert temperatures between °C, °F, and K?

    Use formulas: °F = (°C × 9/5) + 32, K = °C + 273.15, and reverse accordingly.

  • What is the Factor Label method in metric conversions?

    The Factor Label method uses conversion factors as fractions to cancel units and convert quantities.

  • Define density and its formula.

    Density is mass per unit volume, calculated as \(\rho=\frac{m}{V}\).

  • What are significant figures and why are they important?

    Significant figures indicate the precision of a measurement and affect calculation accuracy.

  • How is scientific notation used in chemistry?

    Scientific notation expresses very large or small numbers as a product of a number between 1 and 10 and a power of 10.

  • How is the periodic table organized?

    Elements are arranged by increasing atomic number and grouped by similar properties into families.

  • Name and describe properties of key element families.

    Alkali metals: very reactive metals; Alkaline earth metals: reactive metals; Halogens: reactive nonmetals; Noble gases: inert gases; Transition metals: variable properties.

  • Differentiate metals, nonmetals, and metalloids.

    Metals are conductive and malleable, nonmetals are insulators and brittle, metalloids have mixed properties.

  • How do you write and name ionic and molecular compounds?

    Ionic compounds combine metals and nonmetals with charges balanced; molecular compounds combine nonmetals with prefixes indicating atom counts.

  • What are binary and tertiary compounds?

    Binary compounds contain two elements; tertiary compounds contain three or more elements.

  • What are polyatomic ions and how do you use their charges?

    Polyatomic ions are charged groups of atoms; their charges must be balanced in formulas.

  • How do you calculate percent composition of a formula?

    Percent composition = (mass of element / total formula mass) × 100%.

  • What is a hydrate and how is it named?

    A hydrate is a compound with water molecules attached; named by adding prefixes to indicate water molecules (e.g., copper(II) sulfate pentahydrate).

  • How do you count the number of atoms in a formula?

    Multiply the subscript of each element by the number of formula units present.

  • Define Gram Formula Mass (GFM) or Molar Mass (MM).

    GFM/MM is the sum of atomic masses of all atoms in a formula, expressed in grams per mole.

  • Explain the mole concept and Avogadro's number.

    A mole is 6.02 × 10\(^{23}\) particles; it relates grams, particles, and volume (22.4 L at STP).

  • How do you use mole-to-mole and mass-to-mass ratios?

    Use mole ratios from formulas to convert between amounts of substances; convert masses to moles first for mass-to-mass calculations.

  • What is the difference between empirical and molecular formulas?

    Empirical formula shows simplest whole-number ratio; molecular formula shows actual number of atoms.