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Ionic Bonds
Bonds formed from the transfer of electrons from a metallic element to a non-metallic element.
Cation
A positively charged ion formed when a metal loses electrons from its valence shell.
Anion
A negatively charged ion formed when a non-metal gains electrons.
Electrostatic Attractions
Strong attractions formed between oppositely charged ions (cations and anions) to form ionic compounds.
Ionic Lattice
An evenly distributed crystalline structure formed by ions arranged in a regular repeating pattern due to electrostatic forces of attraction between cations and anions.
Properties of Ionic Compounds
Different physical properties (melting/boiling points, electrical conductivity, and solubility) due to their structure and bonding.
Covalent Bonds
Bonds formed between two non-metals through the sharing of electrons in their outer shells.
Dative Covalent Bond
A type of covalent bond where one atom donates a lone pair of electrons to an electron-deficient atom.
Multiple Bonds
Non-metals can share more than one pair of electrons to form different types of covalent bonds.
Bond Energy
The energy required to break one mole of a particular covalent bond in the gaseous state.
Bond Length
The internuclear distance between two covalently bonded atoms.
Bond Polarity
The polarity of a covalent bond determined by the difference in electronegativity between the atoms involved.
Lewis Structures
Simplified electron shell diagrams that show pairs of electrons around atoms.
Octet Rule
The tendency of atoms to gain a valence shell with a total of 8 electrons.
Incomplete Octets
Exceptions to the octet rule where elements below atomic number 20 can achieve stability with fewer than 8 electrons in their valence shells.
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