Lecture Notes: Atoms and Bonding - Vocabulary Flashcards

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Vocabulary flashcards covering atomic structure, electron configurations, periodic trends, bonding types, and properties derived from bonding.

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42 Terms

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Atom

The basic unit of matter composed of electrons, protons, and neutrons; bonding depends on its structure.

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Electron

Negatively charged subatomic particle with mass about 9.11×10^-31 kg; orbits the nucleus.

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Proton

Positively charged subatomic particle with mass about 1.67×10^-27 kg; located in the nucleus.

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Neutron

Electrically neutral subatomic particle with mass about 1.67×10^-27 kg; located in the nucleus.

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Atomic Number (Z)

Number of protons in the nucleus; equal to the number of electrons in a neutral atom.

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Atomic Mass Unit (amu)

Defined as 1/12 the mass of a carbon-12 atom.

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Atomic Weight

The mass of one mole of atoms (6.022×10^23 atoms) of an element.

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Isotopes

Atoms of the same element with the same Z but different neutron numbers (e.g., Carbon-12, Carbon-13, Carbon-14).

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Bohr Model

Electrons revolve around the nucleus in discrete shells with quantized energy levels.

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Wave-Mechanical Model

Electrons exhibit wave-particle duality and occupy orbitals—regions of probability.

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Principal Quantum Number (n)

Defines the shell or energy level (K, L, M… or 1, 2, 3…).

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Subsidiary Quantum Number (l)

Defines orbital shape (s, p, d, f).

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Magnetic Quantum Number (ml)

Orientation of the orbital in space.

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Spin Quantum Number (ms)

Direction of electron spin (+1/2 or −1/2).

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Orbital

Region in space where there is a high probability of finding an electron; defined by n, l, ml.

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Energy Level / Shell

Group of orbitals with similar energy, defined by the principal quantum number n.

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s, p, d, f Orbitals

Types of atomic orbitals with characteristic shapes used to describe electron locations.

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Electron Configuration

Distribution of electrons among orbitals, filling lowest energy levels first.

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Hydrogen 1s1

Hydrogen electron configuration: 1s1.

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Helium 1s2

Helium stable configuration: 1s2.

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Carbon 1s2 2s2 2p2

Carbon electron configuration with 4 valence electrons.

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Noble Gases

Elements with completely filled outer shells; chemically stable.

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Valence Electrons

Electrons in the incomplete outer shell that participate in bonding.

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Periodic Table

Organization of elements by electron structure and electronegativity trends.

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Metals

Electropositive elements that tend to lose electrons to form cations.

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Nonmetals

Electronegative elements that tend to gain electrons to form anions.

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Electronegativity

Atom’s tendency to attract electrons in a bond; measured on scales like Pauling’s.

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Pauling Scale

Common electronegativity scale (approximately 0.7 to 4.0).

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Ionic Bonding

Bonding via transfer of electrons from metals to nonmetals; strong Coulombic attraction; examples: NaCl, MgO, CaF2.

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Covalent Bonding

Bonding via sharing of valence electrons between atoms with similar electronegativity; directional bonds.

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Metallic Bonding

Bonding in metals with delocalized valence electrons forming an electron cloud around positive ion cores.

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Mixed Ionic-Covalent Bonding

Bonds that have both ionic and covalent character; ionic character estimated from electronegativity differences.

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Secondary Bonding (Van der Waals Forces)

Weaker dipole-based interactions (permanent, induced, fluctuating) important in polymers and molecular solids.

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Hydrogen Bonding

A strong type of dipole-dipole interaction involving hydrogen and a highly electronegative partner.

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Bond Energy (Eo)

Energy required to break a bond; higher bond energy indicates greater stability and higher melting point.

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Bond Length (r)

Distance between the centers of two bonded atoms at equilibrium.

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Melting Temperature (Tm)

Temperature at which a solid becomes a liquid; higher for stronger bonds.

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Thermal Expansion (α)

Coefficient describing how a material’s size changes with temperature; weaker bonds expand more.

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Primary Bonding Types

Ionic, covalent, and metallic bonds—the main, strong interatomic bonds.

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Secondary Bonding

Weaker, dipole-based interactions such as van der Waals forces.

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Bonding and Properties

Bond type and strength influence melting point, strength, conductivity, and thermal expansion.

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Periodicity of Bonding Trends

Element groups and electronegativity trends in the Periodic Table influence bonding behavior.