Chemistry Quiz: Properties and Ions

Chemistry Eighth Edition - Chapter 2: Atoms, Molecules, and Ions

• Chapter 2 of the Chemistry textbook, Eighth Edition, focuses on atoms, molecules, and ions.
• Table 2.1 details names and symbols of some common elements, including their Latin origins.
• The periodic table positions elements in specific rows (periods) and columns (groups).
• International standard groups are numbered 1-18, while US system uses 1A-8A, 1B-8B designations.
• There are main groups (1A-2A & 3A-8A) and transition elements (3B-2B), and inner transition elements (14 groups between 3B & 4B).
• The elements in the periodic table are categorized as metals, semimetals, and non-metals.
• Metals are primarily on the left side of the periodic table's zig-zag line (excluding Hydrogen)
• Nonmetals are primarily on the right side of the zig-zag line.
• Semimetals lie along the zig-zag line of the periodic table.
• Intensive properties do not depend on sample size, such as temperature and melting point, while extensive properties, like length & volume, do depend on the sample size.
• Physical properties describe sample characteristics without chemical changes (e.g., color, melting point).
• Chemical properties describe characteristics tied to chemical changes (e.g., rusting, combustion).
• The law of conservation of mass states mass is conserved in chemical reactions.
• The law of definite proportions dictates that pure chemical substances always have the same element proportion by mass.
• Law of multiple proportions shows elements can combine in different ways, forming substances with small whole-number mass ratios.
• Dalton’s atomic theory suggests atoms of the same element have the same mass, while those from different elements have different masses.
• Atoms joining in whole-number ratios form compounds.
• Rutherford's gold foil experiments demonstrated an atom's mostly empty space, with a dense nucleus.
• Subatomic particles are electron, proton, and neutron, each with distinct mass and charge.
• Atomic number (Z) is the number of protons (same as number of electrons) inside the nucleus.
• Mass number (A) is the sum of protons and neutrons.
• Isotopes are atoms with the same atomic number but different mass numbers.
• The mass of an atom is primarily concentrated in its nucleus.
• The mass of one carbon-12 atom is 12 amu.
• The atomic weight of an element is the weighted average of its naturally occurring isotopes.
• Avogadro's Number (NA) is 6.022×10²³.
• Molar mass, in grams, is numerically equal to the atomic weight of an element.
• Mass spectrometry is a common method for measuring atomic weights. The resulting ions are deflected based on their mass-to-charge ratio. A mass spectrum presents measured intensities of ions.
• Mixtures are categories of matter composed of two or more pure substances.
• Covalent bonds involve electron sharing between two atoms (typically between nonmetals).
• A molecule forms when two or more atoms are bound by covalent bonds.
• An ionic bond involves the electron transfer from one atom to another creating oppositely charged particles (ions).
• Cations are positively charged ions (metals tend form them), and anions are negatively charged ions (nonmetals form them).
• Ions combine to form neutral compounds where the number of positive charges equals the number of negative charges.
• In naming ionic compounds, simple charges are used and roman numerals are used for compounds with more than one cation.
• Polyatomic ions are charged groups containing multiple atoms
• Covalent compounds often use prefixes to indicate the number of each element (e.g., "monoxide", "dioxide").