Physical and Chemical Properties Quiz

Physical and Chemical Properties

• Physical Properties: Characteristics that can be observed without changing the substance's composition, including color, luster, malleability, texture, brittleness, hardness, state (solid, liquid, gas), and clarity.
• Chemical Properties: Characteristics that describe how a substance reacts with other substances, including flammability, corrosion, solubility, and viscosity.
• Physical Changes: Changes in the appearance or state of a substance without altering its chemical composition. Examples: melting, dissolving. There are no new substances, and no heat, light, or sound are involved.
• Chemical Changes: Changes in a substance that result in the formation of new substances with different properties. Examples include color changes, heat/light/sound production, bubble formation, solid formation in a liquid, and changes that are difficult or impossible to reverse.

Qualitative and Quantitative Properties

• Qualitative Properties: Properties that describe a substance without using numbers, including color, texture, state, hardness, and luster.
• Quantitative Properties: Properties that describe a substance using numbers and units, including temperature, height, mass, volume, density, solubility, viscosity, melting point, and boiling point.
• Characteristic Physical Properties: Some physical properties help identify a pure substance (e.g., melting point, density, boiling point) while others (like color and shape) are not as useful.

Density Calculations

• Density Formula: Density (D) = mass (m) / volume (v). The formula allows calculation of any missing variable.
• Example: If mass = 40 g and density = 2.5 g/cm³, volume = 16 cm³.

Volume Measurement (Irregular Objects)

• Displacement Method: To find the volume of an irregular object, immerse it in water and measure the volume of water displaced in a graduated cylinder. 1 mL of water equals 1 cm³.

Elements, Compounds, and Mixtures

• Element: A pure substance consisting of only one type of atom (e.g., hydrogen, oxygen).
• Compound: A pure substance composed of two or more different elements chemically combined (e.g., water, salt).
• Mixture of Elements: Two or more elements not chemically bonded (e.g., air).
• Mixture of Compounds: Two or more compounds mixed together (e.g., salt dissolved in water).
• Mixture of Elements and Compounds: A combination of elements and compounds, not chemically bonded.

Periodic Table

• Metals, Nonmetals, Metalloids: Categorization of elements based on location on the periodic table "staircase"
• General Properties: Metals are typically ductile, conductive, and malleable; nonmetals are brittle; metalloids exhibit properties of both.
• Periodic Table Organization: Period = horizontal row; Group = vertical column.
• Element Information: Use the periodic table to find element name, symbol, atomic number, and atomic mass.
• Atomic Notation: Standard atomic notation shows atomic number (number of protons) and mass number (protons + neutrons).

Atomic Structure

• Atom: Has the same number of protons and electrons (neutral).
• Bohr-Rutherford Diagrams: Diagrams of atomic structure showing protons and neutrons in the nucleus, and electrons orbiting in shells. Note maximum electron capacity per shell (e.g., first = 2, subsequent = 8).
• Atomic Number: Number of protons in an atom.
• Atomic Mass: Number of protons + neutrons.
• Element Period: Corresponds to the number of electron shells (or orbitals)
• Ions: Atoms that have gained or lost electrons (anions = negative, cations = positive).
• Ionic Formation: Atoms become ions to achieve a stable electron configuration, gaining or losing electrons to fill their outermost shell.
• Metals and Nonmetals: Metals lose electrons to become stable, nonmetals gain electrons.
• Valence Electrons: Electrons in the outermost shell, and the group number in the periodic table often indicates the number of valence electrons.
• Reactivity: Valence electrons far from the nucleus are less tightly bound increasing reactivity.

Chemical Families (Groups):

• Group 1 (Alkali Metals): Highly reactive, good thermal and electrical conductors.
• Group 2 (Alkaline Earth Metals): Reactive but less so than alkali metals, good conductors.
• Group 17 (Halogens): Highly reactive nonmetals, combine with metals to form salts.
• Group 18 (Noble Gases): Stable, unreactive gases due to complete outermost electron shells.

Counting Atoms in Formulas

• Subscripts: Numbers inside chemical formulas tell you how many atoms (of that element) are in the molecule. The count applies to everything inside the brackets, with numbers outside the brackets affecting ALL elements inside the bracket.

History of the Atom

• Scientists and Models: Connect key scientists (Dalton, Thomson, Rutherford, Bohr, Chadwick, Mendeleev, Aristotle) with their atomic models and/or experiments.
• Highlights Key characteristics and experiments of those scientists.

Diatomic Molecules

• Diatomic Molecules: Molecules consisting of two atoms of the same element (e.g., H₂, O₂). They share electrons to achieve stability.
• Examples (7): H₂, O₂, F₂, Br₂, I₂, N₂, and Cl₂.

Molecular Compounds

• Molecular Compounds: Two or more nonmetals share electrons forming covalent bonds. These atoms are neutral.

Ionic Compounds

• Ionic Compounds: Atoms gain or lose electrons, creating positively and negatively charged ions that bond. Cations (positive) bond with anions (negative). Usually a metal and nonmetal (often).

Electricity

• Electrical Concepts: Voltage (V), current (I), resistance (R), and charge (Q). Know their meanings, units, and units' symbols.

• Ohm's Law: V = I x R

• Charge Equation: Q = I x ∆t

• Energy Equation: ∆E = ∆V x Q

• Factors Affecting Resistance: Length, cross-sectional area, material, and temperature.

• Conductors vs. Insulators: Conductors have low resistance, insulators have high resistance.

• Series vs. Parallel Circuits: Key differences in how current and voltage behave.

• Equivalent Resistance: Calculate equivalent resistance in series and parallel circuits.

• Renewable vs. Non-renewable Electricity: Know the difference. Review Gizmo work on energy conversions.

• Types of Electricity: Static vs Current Electricity (difference)

• Law of Charges: Positive charges attract negative charges; like charges repel like charges.

• Charge by Friction, Induction, Conduction: Explain the electron movement within each.

• Electrostatic Series: Can predict the charge of an object resulting from an interaction. Predict electron transfer by friction—which material will lose electrons and which gains.

• Neutral vs. Charged Object: Showing the difference in electron count in diagrams.

Diagrams

• Diagrams: Use diagrams to show electron transfer in charging by friction, induction, and conduction. Analyze diagrams to predict final charge states.

Test your knowledge on the physical and chemical properties of substances! This quiz covers key characteristics, physical and chemical changes, as well as qualitative and quantitative properties. Perfect for chemistry students looking to reinforce their understanding.