Physical Science L to J Words Flashcards

Atom and Structure

• Atoms are the smallest units of elements, preserving the element's properties.
• Atomic Mass Unit (AMU) is defined as one-twelfth the mass of a carbon-12 atom.
• Atomic Number indicates the number of protons in an atom's nucleus, determining elemental identity.
• Atomic Radius is measured as half the distance between the nuclei of identical bonded atoms.
• Average Atomic Mass reflects the weighted average of an element's isotopes' atomic masses.

Mole Concepts

• Avogadro's Number signifies the number of particles in one mole of a substance.
• A Mole is defined as the amount of substance containing as many particles as 12 g of carbon-12.
• Molar Mass is the mass of one mole of a pure substance.

Chemical Bonding

• A Binary compound consists of two distinct elements.
• Bond Energy denotes the energy required to break chemical bonds and yield neutral atoms.
• Bond Length indicates the distance between two bonded atoms at minimum potential energy.
• Covalent Bonds involve sharing an electron pair between two atoms; nonpolar and polar distinguish the equality of electron sharing.
• Ionic Bonding results from electrostatic attraction between cations and anions.

Reaction Types

• Combustion involves a substance reacting with oxygen, producing heat and light.
• Decomposition reactions yield two or more simpler substances from a single compound.
• Double Replacement reactions occur when ions in two compounds swap places.
• Composition Stoichiometry focuses on mass relationships of elements in compounds and how to calculate them.

Formulas and Equations

• Chemical Equations represent reactants and products in a reaction using formulas.
• Chemical Formulas convey the relative number of different types of atoms in a compound using atomic symbols and subscripts.
• Coefficients in chemical equations indicate the number of molecules or moles of a substance involved.

Isotopes and Mass

• Isotopes are variations of the same element that differ in mass due to differing numbers of neutrons.
• Mass refers to the measure of matter in an object, while Mass Number is the total count of protons and neutrons in an atom's nucleus.

Energy and Stability

• Lattice Energy is the energy released when forming one mole of ionic crystal from gaseous ions.
• The Law of Conservation of Mass states that mass is conserved in chemical and physical reactions.
• The Law of Conservation of Energy dictates that energy cannot be created or destroyed in reactions.

Advanced Concepts

• Lewis Structures represent atom nuclei, bonded electron pairs, and unshared electrons.
• VSEPR Theory explains molecular geometry based on electron pair repulsion.
• Resonance Structures depict bonding that cannot be fully represented by a single Lewis structure.

Additional Definitions

• Density is the ratio of an object's mass to its volume.
• Polyatomic Ions are charged groups of covalently bonded atoms.
• Valence Electrons play a key role in chemical bonding, affecting how atoms can interact in forming compounds.
• The Octet Rule suggests that atoms tend to seek a full outer shell of electrons for stability.

Periodicity

• The Periodic Table organizes elements by increasing atomic number, showcasing periodic trends in element properties.