3.6: End of Chapter Key Terms
- Page ID
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Atomic Theory and the Periodic Table Key Terms
- Atom: The smallest unit of an element that retains the properties of that element, consisting of protons, neutrons, and electrons.
- Nucleus: The dense central core of an atom, containing protons and neutrons.
- Proton: A positively charged subatomic particle found in the nucleus of an atom.
- Neutron: A neutral subatomic particle found in the nucleus of an atom.
- Electron: A negatively charged subatomic particle that orbits the nucleus of an atom.
- Atomic Number (Z): The number of protons in the nucleus of an atom, which determines the element's identity.
- Mass Number (A): The total number of protons and neutrons in the nucleus of an atom.
- Isotope: Atoms of the same element with the same number of protons but different numbers of neutrons.
- Atomic Mass Unit (amu): A unit of mass used to express atomic and molecular weights, approximately equal to the mass of a proton or neutron.
- Atomic Mass: The weighted average mass of the isotopes of an element, typically expressed in atomic mass units (amu).
- Electron Cloud: The region around the nucleus where electrons are likely to be found.
- Orbital: A region of space around the nucleus where an electron is likely to be found, described by quantum numbers.
- Quantum Numbers: Numbers that describe the properties of atomic orbitals and the properties of electrons in orbitals.
- Principal Quantum Number (n): Indicates the relative size and energy of atomic orbitals; larger nnn values correspond to higher energy levels.
- Angular Momentum Quantum Number (l): Describes the shape of an atomic orbital; values range from 0 to n−1n-1n−1.
- Magnetic Quantum Number (m_l): Describes the orientation of the orbital in space; values range from −l-l−l to +l+l+l.
- Spin Quantum Number (m_s): Describes the spin of an electron; can be +12+\frac{1}{2}+21 or −12-\frac{1}{2}−21.
- Electron Configuration: The arrangement of electrons in an atom's orbitals, described by the distribution of electrons among energy levels and orbitals.
- Aufbau Principle: States that electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels.
- Pauli Exclusion Principle: States that no two electrons in an atom can have the same set of four quantum numbers.
- Hund's Rule: States that electrons will fill degenerate orbitals (orbitals of the same energy) singly before pairing up.
- Periodic Table: A tabular arrangement of elements in order of increasing atomic number, with elements having similar properties placed in vertical columns (groups).
- Period: A horizontal row in the periodic table, where elements have the same number of electron shells.
- Group (Family): A vertical column in the periodic table, where elements have similar chemical properties and the same number of valence electrons.
- Valence Electrons: Electrons in the outermost shell of an atom, which determine the chemical properties and reactivity of the element.
- Alkali Metals: Elements in Group 1 of the periodic table (excluding hydrogen), characterized by having one valence electron.
- Alkaline Earth Metals: Elements in Group 2 of the periodic table, characterized by having two valence electrons.
- Transition Metals: Elements in Groups 3-12 of the periodic table, characterized by having d electrons.
- Halogens: Elements in Group 17 of the periodic table, characterized by having seven valence electrons.
- Noble Gases: Elements in Group 18 of the periodic table, characterized by having a full valence shell of electrons, making them very stable and unreactive.
- Lanthanides: A series of elements from atomic numbers 57 to 71, characterized by filling of 4f orbitals.
- Actinides: A series of elements from atomic numbers 89 to 103, characterized by filling of 5f orbitals.
- Metals: Elements that are typically shiny, conductive, malleable, and ductile.
- Nonmetals: Elements that are typically not shiny, poor conductors, and brittle in solid form.
- Metalloids: Elements with properties intermediate between metals and nonmetals.
- Atomic Radius: The distance from the nucleus to the outermost electron shell of an atom.
- Ionization Energy: The energy required to remove an electron from a gaseous atom or ion.
- Electron Affinity: The energy change that occurs when an electron is added to a neutral atom in the gas phase.
- Electronegativity: A measure of the ability of an atom in a chemical compound to attract electrons.
- Periodic Trends: Patterns observed in the periodic table for properties such as atomic radius, ionization energy, electron affinity, and electronegativity.