Atomic Structure Quiz

Atomic Structure

• Atomic model:
  • Rutherford's nuclear model: nucleus (protons and neutrons) surrounded by electrons
  • Electron cloud: region where electrons are likely to be found
• Subatomic particles:
  • Proton: positive charge, found in nucleus
  • Neutron: no charge, found in nucleus
  • Electron: negative charge, found in electron cloud
• Atomic number (Z): number of protons in an atom
• Mass number (A): total number of protons and neutrons in an atom
• Isotopes: atoms of the same element with different mass numbers
• Ions: atoms or groups of atoms with a charge (gained or lost electrons)

Periodic Table

• Arrangement:
  • Rows: periods
  • Columns: groups (families)
  • Metals: left side and center of the table
  • Non-metals: right side of the table
• Periodic trends:
  • Atomic radius: decreases from left to right, increases down a group
  • Electronegativity: increases from left to right, decreases down a group
  • Ionization energy: increases from left to right, decreases down a group
• Blocks:
  • s-block: first two columns (groups 1 and 2)
  • p-block: last six columns (groups 13 to 18)
  • d-block: middle ten columns (groups 3 to 12)
  • f-block: lanthanides and actinides (bottom two rows)

Chemical Bonding

• Types of bonds:
  • Ionic bond: transfer of electrons between atoms
  • Covalent bond: sharing of electrons between atoms
  • Polar covalent bond: unequal sharing of electrons between atoms
• Bonding theories:
  • Electronegativity: ability of an atom to attract electrons
  • VSEPR theory: shape of molecules based on electron pairs
• Molecular shape:
  • Linear
  • Bent
  • Trigonal planar
  • Tetrahedral
  • Trigonal bipyramidal
  • Octahedral

Acid-base Chemistry

• Arrhenius theory:
  • Acid: substance that donates a proton (H+)
  • Base: substance that accepts a proton
• Bronsted-Lowry theory:
  • Acid: substance that donates a proton (H+)
  • Base: substance that accepts a proton
• pH scale:
  • Acidic: pH < 7
  • Neutral: pH = 7
  • Basic: pH > 7
• Strong and weak acids and bases:
  • Strong acids: completely ionize in water
  • Weak acids: partially ionize in water
  • Strong bases: completely ionize in water
  • Weak bases: partially ionize in water

Stoichiometry

• Mole concept:
  • Mole (mol): 6.022 x 10^23 particles (atoms, molecules, ions, etc.)
  • Molar mass: mass of one mole of a substance
• Empirical and molecular formulas:
  • Empirical formula: simplest whole number ratio of atoms in a compound
  • Molecular formula: actual number of atoms in a molecule
• Stoichiometric calculations:
  • Moles of reactants and products
  • Amount of substance (mass or volume) of reactants and products
  • Yield calculations: actual amount of product formed

Atomic Structure

• Atomic model consists of a nucleus (protons and neutrons) surrounded by an electron cloud, where electrons are likely to be found
• Protons have a positive charge and are found in the nucleus
• Neutrons have no charge and are found in the nucleus
• Electrons have a negative charge and are found in the electron cloud
• Atomic number (Z) is the number of protons in an atom
• Mass number (A) is the total number of protons and neutrons in an atom
• Isotopes are atoms of the same element with different mass numbers
• Ions are atoms or groups of atoms with a charge (gained or lost electrons)

Periodic Table

• The periodic table is arranged in rows (periods) and columns (groups or families)
• Metals are found on the left side and center of the table
• Non-metals are found on the right side of the table
• Atomic radius decreases from left to right and increases down a group
• Electronegativity increases from left to right and decreases down a group
• Ionization energy increases from left to right and decreases down a group
• The periodic table is divided into blocks: s-block, p-block, d-block, and f-block

Chemical Bonding

• Ionic bonds are formed by the transfer of electrons between atoms
• Covalent bonds are formed by the sharing of electrons between atoms
• Polar covalent bonds are formed by the unequal sharing of electrons between atoms
• Electronegativity is the ability of an atom to attract electrons
• VSEPR theory predicts the shape of molecules based on electron pairs
• Molecular shapes include linear, bent, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral

Acid-base Chemistry

• Arrhenius theory defines acids as substances that donate a proton (H+) and bases as substances that accept a proton
• Bronsted-Lowry theory defines acids as substances that donate a proton (H+) and bases as substances that accept a proton
• pH scale: acidic (pH < 7), neutral (pH = 7), and basic (pH > 7)
• Strong acids completely ionize in water, while weak acids partially ionize in water
• Strong bases completely ionize in water, while weak bases partially ionize in water

Stoichiometry

• One mole (mol) is equal to 6.022 x 10^23 particles (atoms, molecules, ions, etc.)
• Molar mass is the mass of one mole of a substance
• Empirical formula is the simplest whole number ratio of atoms in a compound
• Molecular formula is the actual number of atoms in a molecule
• Stoichiometric calculations involve moles of reactants and products, amount of substance (mass or volume) of reactants and products, and yield calculations