BIOC 1303 Study Guide - Midterm Guide: Vsepr Theory, Noble Gas, Lone Pair
28 Jun 2018
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Organic and Biology Chemistry for Health Sciences - Chapter Definitions
Week One: Chapter 5 Compounds and Their Bonds
Anion: A negatively charged ion (ie. Cl-)
Bent: The shape of a molecule with two bonded atoms and two lone pairs (ie. H20)
Cations: A positively charged ion. (ie. Na+)
Covalent Bond: A bond created by the sharing of valence electrons.
Covalent Compound: A combination of atoms in which noble gas configurations are attained by
sharing electrons.
Dipole: A pair of equal and oppositely charged or magnetized poles separated by a distance.
Dipole-Dipole Attractions: Attractive forces between oppositely charged ends of polar
molecules.
Double Bond: A sharing of two pairs of electrons by two atoms
Electronegativity Value: The relative ability of an element to attract electrons in a bond.
Formula: The group of symbols and subscripts that represent the atoms or ions in a compound.
Ion: Atom(s) having an electrical charge because of a loss or gain of electrons.
Ionic Charge: The difference between the number of protons and number of electrons.
Molecule: The smallest unit of two or more atoms held together by covalent bonds.
Non-Polar Covalent Bond: A covalent bond in which the electrons are shared equally.
Nonpolar Molecule: A molecule that has only nonpolar bonds or in which the dipoles cancel.
Octet Rule: Elements in groups 1A-7A (1,2,13-17) react with other elements by forming ionic or
covalent bonds to produce a noble gas configuration.
Polar Covalent Bond: A covalent bond in which the elements are shared unequally between
atoms.
Polar Molecule: A molecule containing dipoles that do not cancel.
Polyatomic Ion: A group of covalently bonded non metal atoms that has an overall electrical
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Document Summary
Organic and biology chemistry for health sciences - Week one: chapter 5 compounds and their bonds. Bent: the shape of a molecule with two bonded atoms and two lone pairs (ie. h20) Covalent bond: a bond created by the sharing of valence electrons. Covalent compound: a combination of atoms in which noble gas configurations are attained by sharing electrons. Dipole: a pair of equal and oppositely charged or magnetized poles separated by a distance. Dipole-dipole attractions: attractive forces between oppositely charged ends of polar molecules. Double bond: a sharing of two pairs of electrons by two atoms. Electronegativity value: the relative ability of an element to attract electrons in a bond. Formula: the group of symbols and subscripts that represent the atoms or ions in a compound. Ion: atom(s) having an electrical charge because of a loss or gain of electrons. Ionic charge: the difference between the number of protons and number of electrons.
