IGC Chemistry Learning Outcomes - Vocabulary Flashcards
Matter and Measurement Foundations
Recognize the steps of the scientific method.
Observation, hypothesis, experiment, analysis, and conclusion (and iteration as needed).
Identify and describe the three states of matter.
Solid, liquid, gas; particle arrangement and energy differ by state.
Distinguish between substances and mixtures.
Substances: elements or compounds with fixed composition.
Mixtures: combinations of substances (can be homogeneous or heterogeneous).
Identify substances as elements or compounds.
Elements: pure substance consisting of one type of atom.
Compounds: pure substance composed of two or more elements in fixed ratio.
Identify mixtures as homogeneous or heterogeneous.
Homogeneous: uniform composition throughout.
Heterogeneous: non-uniform composition with visually distinguishable parts.
Identify and provide examples of properties of matter.
Physical properties: color, odor, density, melting/boiling point, solubility, etc. (examples: gold is dense; water boils at 100°C at 1 atm).
Chemical properties: reactivity, flammability, acidity, etc.
Distinguish between physical and chemical changes.
Physical change: alters state or appearance without changing composition (e.g., melting ice).
Chemical change: transforms into new substances with new properties (e.g., burning wood).
Identify properties as physical or chemical; give examples.
Physical: color, melting point, solubility in a given solvent.
Chemical: reactivity with acid, rust formation.
Distinguish between intensive and extensive properties.
Intensive: independent of amount (e.g., density, boiling point).
Extensive: depends on amount (e.g., mass, volume).
Produce examples of intensive and extensive properties.
Intensive: density of copper, melting point of ice.
Extensive: mass of a sample, volume of a liquid.
Demonstrate knowledge of units, their abbreviations, and relationships among them.
Identify the SI base units, including the symbol, and the quantity they are used to measure.
Length: meter (m)
Mass: kilogram (kg)
Time: second (s)
Electric current: ampere (A)
Temperature: kelvin (K)
Amount of substance: mole (mol)
Luminous intensity: candela (cd)
Recognize metric prefixes, their symbol, and their meaning.
e.g., kilo (k, 10^3), centi (c, 10^-2), milli (m, 10^-3), micro (μ, 10^-6), nano (n, 10^-9).
Write relationships between quantities with different metric prefixes.
Example: 1 km = 10^3 m, 1 m = 10^3 mm, etc.
Recall the difference between mass and weight.
Mass: amount of matter (in kg or g).
Weight: force due to gravity acting on mass. W = m g.
Determine when and how to use numbers in scientific notation.
Convert numbers between standard and scientific notations.
Use numbers in scientific notation in calculations.
Describe and use derived units.
Identify the SI-derived unit for volume.
Volume: derived unit liter (L) or cubic meter (m^3).
Give examples of common units of volume.
L, mL, cm^3.
Define density.
Calculate density from given values of mass and volume.
Density \rho = \frac{m}{V}
Convert temperatures between Celsius and Kelvin.
Identify the common scales used for temperature.
Relate how the temperature scales compare to each other.
Apply rules of significant figures.
Summarize the importance of significant figures.
Label numbers in a quantity as significant or not.
Define exact number.
Classify numbers as exact or not.
State the rule for determining significant figures in addition and subtraction.
Complete calculations with addition and subtraction using the rules for significant figures.
State the rule for determining significant figures in multiplication and division.
Complete calculations with multiplication and division using the rules for significant figures.
Complete calculations that involve both addition/subtraction and multiplication/division.
Distinguish between precision and accuracy.
Define precision and accuracy.
Analyze data to label as precise, accurate, neither, or both.
Solve problems using dimensional analysis.
Build a problem solving plan by analyzing what is given in a chemical problem and construct a path to obtain an answer.
Apply dimensional analysis methods to convert between units in a one step process.
Apply dimensional analysis in a multi step conversions.
Apply dimensional analysis involving units raised to a power.
Learning Outcomes: Classify matter. Exam 1 Material
Atomic Theory and Structure
Explain atomic theory and how the structure of the atom was determined.
State the law of definite proportions.
Describe Dalton's Atomic Theory and identify which statements are no longer accurate and why.
State the law of conservation of mass; perform simple problems using this law.
Explain how the cathode ray tube led to the understanding of electrons.
Describe the mass-to-charge ratio of the electron.
Explain the measurement of the electron's charge using Millikan's Oil Drop Experiment.
Describe Rutherford's gold foil experiment.
Interpret results that lead to the conclusion that the nucleus exists as a small dense core.
Explain how the mass deficit led to the proposal that neutrons exist.
Describe the structure of an atom and its components; define the atomic mass unit (amu).
Compare the relative mass and charge of subatomic particles.
Define atomic number; describe its relationship to the number of protons.
Determine the atomic number for an element using the periodic table.
Compare properties of isotopes; define isotope and mass number.
Symbolize isotopes using chemical symbols, mass number, and atomic number.
Determine the number of protons, neutrons, and electrons in an atom given the isotopic symbol.
Construct the isotope symbol for atoms.
Use isotopic masses and natural abundance in calculations.
Define natural abundance; locate the average atomic mass on the periodic table.
Calculate the average atomic mass of an element given abundance and isotope masses.
Calculate the relative abundance of isotopes of an element.
Recognize the difference among the terms "atomic number", "mass number", and "atomic mass".
Describe characteristics of cations and anions; define cation and anion.
Determine the number of protons and electrons in an ion; determine the charge of an ion given the numbers of protons and electrons.
Construct the isotope symbol for ions.
Memorize periodic properties related to isotopes and ions.
Understand the concept of ionization states and isoelectronic species.
Know how to identify isoelectronic species and rank them by size.
Distinguish between atomic and molecular elements.
Use periodic table to classify elements as main-group or transition elements.
Locate noble gases, alkali metals, alkaline earth metals and halogens on the periodic table.
Use the periodic table to classify elements as metal, nonmetal, metalloid, transition metal, lanthanide or actinide.
Chemical Formulas, Nomenclature, and Isotopes
Express chemical compounds using empirical, molecular and structural formulas.
Differentiate between atomic and molecular elements.
Memorize periodic relationships and element symbols on the Concepts to Memorize sheet.
Distinguish between ionic and covalent bonds; recall that ionic bonds generally occur between metals and nonmetals, covalent between nonmetals.
Identify characteristics of monatomic and polyatomic ions; use periodic table to predict common charges of main-group elements.
Memorize polyatomic ions and charges; recall the formula of the hydronium ion (H3O+, also H+).
Write formulas and names for compounds:
Construct chemical formulas for ionic compounds from known ion charges.
Construct chemical formulas for ionic compounds from the name of the compound.
Name ionic compounds from the chemical formula.
Name covalent compounds from the chemical formula.
Construct a chemical formula of covalent compounds from the name.
Name binary acids and provide formulas from the name; distinguish binary acids and oxyacids (oxoacids).
Define mole and relate it to the mass of an atom; Avogadro's number: N_A = 6.022 \times 10^{23}.
Convert between moles and atoms; convert between grams and moles; calculate formula and molar masses and relate to moles.