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35 Terms

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Isoelectric

Having the same number of electrons per atom, ion, or molecule.

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Ionic bond

The electrostatic attraction between oppositely charged ions.

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Covalent bond

A chemical bond in which atoms share the bonding electrons.

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Bonding electron pair

An electron pair that is involved in bonding, found in the space between two atoms.

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Lewis structure

A diagram that represents the arrangement of covalent electrons and bonds in a molecule or polyatomic ion.

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Duet rule

The observation that the complete outer shell of valence electrons is stable when hydrogen and period 2 metals are involved in bonding.

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Octet rule

The observation that many atoms form the most stable substances when surrounded by 8 electrons in their valence shells.

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Lone electron pair

A pair of valence electrons that is localized to a given atom but not involved in bonding.

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Non-polar covalent bond

A covalent bond in which the electrons are shared equally between atoms.

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Polar covalent bond

A covalent bond in which the electrons are not shared equally due to one atom attracting them more strongly.

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Electronegativity

The ability of an atom in a molecule to attract shared electrons to itself.

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Dipole

A separation of positive and negative charges in a region in space.

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Polar molecule

A molecule that has a net dipole.

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Non-polar molecule

A molecule that has only nonpolar bonds or a bond dipole sum of zero.

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Valence electron theory

A theory stating that atomic orbitals overlap to form a new orbital with a pair of opposite spin electrons.

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Hybrid orbital

An orbital that forms from the combination of at least two different orbitals.

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Hybridization

The process of forming hybrid orbitals from the combination of at least two different orbitals.

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Sigma bond

A bond formed when the lobes of two orbitals directly overlap end to end.

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Pi bond

A bond formed when the sides of the lobes of two orbitals overlap.

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Intramolecular bond

The chemical bond within a molecule.

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Intermolecular force

A force that causes one molecule to interact with another molecule, occurring between molecules.

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Van der Waals forces

Types of intermolecular forces including dipole-dipole forces, London dispersion forces, and hydrogen bonding.

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Dipole-dipole force

The intermolecular force that occurs when the dipoles of polar molecules position their positive and negative ends nearby.

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Hydrogen bond

The strong dipole-dipole force that occurs when a hydrogen atom bonded to a highly electronegative atom (oxygen, nitrogen, or fluorine) is attracted to a partially negative atom on a nearby molecule.

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London dispersion forces

Intermolecular forces that exist in non-polar molecules and increase as molecular mass increases.

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Polarizability

The ability of a substance to form a dipolar charge distribution.

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Surface tension

The resistance of a liquid to increase its surface area.

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Capillary action

The spontaneous rising of a liquid in a narrow tube.

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Viscosity

The measure of a liquid’s resistance to flow.

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Composite material

A material composed of two or more distinct materials that remain separate in the solid phase.

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Metallic crystal

A solid with closely packed atoms held together by electrostatic interactions and free-moving electrons.

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Metallic bonding

The bonding that holds the nuclei and electrons of metals together.

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Molecular crystal

A solid composed of individual molecules held together by intermolecular forces of attraction.

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Covalent network crystal

A solid in which the atoms form covalent bonds in an interwoven network.

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Semiconductor

A substance that conducts a slight electric current at room temperature but has increasing conductivity at higher temperatures.