BackGeneral Chemistry - Atomic Structure and Chemical Bonding
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Terms in this set (18)
Dalton's hypothesis states that matter is composed of indivisible atoms, which combine in fixed ratios to form compounds.
Thomson's model proposed the atom as a sphere of positive charge with embedded electrons, known as the 'plum pudding' model.
Rutherford's model described the atom with a dense, positively charged nucleus and electrons orbiting around it.
Bohr's model introduced quantized electron orbits with fixed energy levels around the nucleus.
Wave-particle duality means particles like electrons exhibit both wave and particle properties.
Heisenberg's principle states it is impossible to simultaneously know both the exact position and momentum of an electron.
Atomic orbitals are regions in space where there is a high probability of finding an electron.
Quantum numbers describe the size, shape, orientation, and spin of atomic orbitals and electrons.
The periodic table was developed to organize elements by increasing atomic number and recurring chemical properties.
Effective nuclear charge is the net positive charge experienced by an electron after accounting for shielding by other electrons.
Periodic properties include atomic radius, ionization energy, and electronegativity, which vary predictably across periods and groups.
Ionic bonds form by electrostatic attraction between positively and negatively charged ions.
Covalent bonds involve sharing of electron pairs between atoms.
Valence Shell Electron Pair Repulsion (VSEPR) theory predicts molecular geometry based on repulsions between electron pairs.
Molecular geometry is the three-dimensional arrangement of atoms in a molecule determined by VSEPR theory.
Molecular polarity depends on the shape of the molecule and the difference in electronegativity between atoms.
Inorganic compounds include salts, metals, and minerals, typically lacking C-H bonds.
Chemical reactions involve the rearrangement of atoms to form new substances with different properties.