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Questions and Answers
The formula for the number of electrons that an energy level can hold is n^2 * ______.
The formula for the number of electrons that an energy level can hold is n^2 * ______.
2
Electrons located in the outermost energy level of an atom are called ______ electrons.
Electrons located in the outermost energy level of an atom are called ______ electrons.
valence
The ______ principle states that no two electrons in an atom can have the same set of four quantum numbers.
The ______ principle states that no two electrons in an atom can have the same set of four quantum numbers.
Pauli Exclusion
The ______ rule states that electrons fill orbitals in a subshell in a way that maximizes the total spin.
The ______ rule states that electrons fill orbitals in a subshell in a way that maximizes the total spin.
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According to the ______ principle, electrons fill lower-energy orbitals before higher-energy ones.
According to the ______ principle, electrons fill lower-energy orbitals before higher-energy ones.
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Matter is made up of tiny, indivisible particles called ______
Matter is made up of tiny, indivisible particles called ______
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In the Plum Pudding Model, negatively charged electrons are embedded in a uniform sphere of positive ______
In the Plum Pudding Model, negatively charged electrons are embedded in a uniform sphere of positive ______
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The Nuclear Model proposes that electrons orbit a tiny, dense ______ at the center of the atom.
The Nuclear Model proposes that electrons orbit a tiny, dense ______ at the center of the atom.
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In the Planetary Model, electrons move in specific allowable paths called ______.
In the Planetary Model, electrons move in specific allowable paths called ______.
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The Quantum Mechanical Model describes the electron as a wave portrayed by a nucleus surrounded by an electron ______.
The Quantum Mechanical Model describes the electron as a wave portrayed by a nucleus surrounded by an electron ______.
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Quantum numbers describe properties of electrons, including energy levels, orbital shapes, and their ______.
Quantum numbers describe properties of electrons, including energy levels, orbital shapes, and their ______.
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The Principal quantum number (n) represents the energy level and orbital ______.
The Principal quantum number (n) represents the energy level and orbital ______.
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The Azimuthal quantum number (l) indicates the type of ______ and the shape of the orbital.
The Azimuthal quantum number (l) indicates the type of ______ and the shape of the orbital.
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Electrons will first occupy all the available orbitals in a subshell with parallel spins before pairing up with other ______.
Electrons will first occupy all the available orbitals in a subshell with parallel spins before pairing up with other ______.
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Noble gas configuration consists of the elemental symbol of the last noble gas prior to that atom, followed by the configuration of the remaining ______.
Noble gas configuration consists of the elemental symbol of the last noble gas prior to that atom, followed by the configuration of the remaining ______.
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Unpaired electrons show that a substance is ______; paired electrons show that a substance is diamagnetic.
Unpaired electrons show that a substance is ______; paired electrons show that a substance is diamagnetic.
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The tendency of atoms to prefer to have eight electrons in the valence shell is known as the ______ rule.
The tendency of atoms to prefer to have eight electrons in the valence shell is known as the ______ rule.
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Lewis structures are diagrams that show the bonding between a molecule's atoms and the lone pairs of ______ that may exist in the molecule.
Lewis structures are diagrams that show the bonding between a molecule's atoms and the lone pairs of ______ that may exist in the molecule.
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Cations are ions with a ______ charge.
Cations are ions with a ______ charge.
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In a polar covalent bond, electrons are ______ shared between the two bonded atoms.
In a polar covalent bond, electrons are ______ shared between the two bonded atoms.
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VSEPR theory states that electron pairs around a central atom repel each other, arranging themselves to be as far apart as ______.
VSEPR theory states that electron pairs around a central atom repel each other, arranging themselves to be as far apart as ______.
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Study Notes
Models of Atomic Structure
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Solid Sphere Model (Dalton, 1803): Atoms are solid, indivisible spheres. Atoms of the same element are identical, and different elements have different atoms. Atoms combine in fixed ratios to form compounds.
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Plum Pudding Model (Thomson, 1904): Atoms consist of a uniform positive sphere with negatively charged electrons embedded within it, like plums in a pudding. The positive and negative charges balance, making the atom neutral.
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Nuclear Model (Rutherford, 1911): The atom has a tiny, dense, positively charged nucleus at its center containing most of the atom's mass. Negatively charged electrons orbit the nucleus like planets orbiting the sun.
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Planetary Model (Bohr, 1913): Electrons orbit the nucleus in specific, fixed energy levels or shells. Electrons can change energy levels by absorbing or emitting energy.
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Quantum Mechanical Model (Schrödinger, 1926): Electrons are described as waves. They exist in orbitals, defined regions of space where there's a high probability of finding an electron. Electrons exist in specific energy levels. Electrons can only move between energy levels by absorbing or emitting energy in the form of photons.
Quantum Numbers
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Principal (n): Describes the energy level and size of the electron's orbital.
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Azimuthal/Angular Momentum (l): Describes the shape of the electron's orbital (s, p, d, f).
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Magnetic (ml): Describes the orientation of the electron's orbital in space.
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Spin (ms): Describes the intrinsic angular momentum (spin) of the electron (up or down).
Electron Configuration
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Atomic orbitals: Electrons fill lower energy levels before higher levels.
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Pauli Exclusion Principle: No two electrons in an atom can have the same set of four quantum numbers.
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Hund's Rule: Electrons fill orbitals in a subshell such that the total electron spin is maximized before pairing up. A different way of stating the same idea - each orbital in a subshell is singly occupied before any one orbital is doubly occupied.
Valence Electrons
- Valence electrons: Electrons in the outermost energy level of an atom. They are responsible for the chemical properties of an element. The number of valence electrons determines how atoms interact with each other.
Molecular Geometry
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Molecular geometry: The 3-D structure of atoms in a molecule. This is dependent on valence shell electron pair repulsion (VSEPR) theory. The valence shell electron pair repulsion (VSEPR) theory predicts that molecules will arrange themselves so that the electron clouds ( bonds and lone pairs of electrons) are as far from each other as possible. Common geometries include linear, trigonal planar, bent, tetrahedral, trigonal pyramidal, and octahedral. The shape of a molecule determines its polarity.
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Octet Rule: The tendency of atoms to prefer to have eight electrons in their valence shell. This rule helps predict the bonding patterns in many molecules.
Bond Types
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Ionic Bonds: Atoms transfer electrons to form ions (positive and negative). Oppositely charged ions are attracted to form an ionic bond.
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Covalent Bonds: Atoms share electrons to achieve a more stable electron configuration. Shared electrons form a covalent bond. The number of shared electron pairs determines the bond type (single, double, triple bond). Single bonds share one pair, double bonds share two pairs and triple bonds share three pairs.
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Polarity: A molecule is polar if the electrons are not shared equally between the atoms in a covalent bond; if there is an uneven distribution of charge.
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Description
Test your knowledge on the various models of atomic structure, including Dalton's solid sphere, Thomson's plum pudding, Rutherford's nuclear model, Bohr's planetary model, and Schrödinger's quantum mechanical model. Each model represents a significant development in our understanding of atomic theory. How well do you grasp these foundational concepts in chemistry?
