CHEM 210 Exam 2 Questions and Answers, Exam Prep. With complete solution.
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Module
CHEM 210
Institution
CHEM 210
CHEM 210 Exam 2 Questions and Answers, Exam Prep. With complete solution.
Ionic bonds
Electron transfer from metal to non-metal, forming a bond
Covalent bonds
Electron sharing between non-metals, forming a bond
Ion
Charged particle
Cation
positive ion
Anion
negative ion
wave particle d...
CHEM 210 Exam 2 Questions and Answers,
Exam Prep. With complete solution.
Ionic bonds
Electron transfer from metal to non-metal, forming a bond
Covalent bonds
Electron sharing between non-metals, forming a bond
Ion
Charged particle
Cation
positive ion
Anion
negative ion
wave particle duality
foundation of quantum mechanics
Ionization energy
Amount of energy required to remove the highest energy/outermost electron from
isolated neutral atom in gas state (E1)
Electron Affinity
isolated atom's attraction for an extra electron (a measurable quantity)
Octet Rule
Main group elements tend to undergo reactions that leave them with eight outer-shell
electrons
Diamagnetic
All electrons paired
Exothermic reaction
a reaction that releases energy
Endothermic reaction
a reaction that absorbs energy
Lattice Energy
Amount of energy that must be added to break up an ionic solid into individual gaseous
ions (U)
Alkali Metals
metallic, silvery, malleable, conductors of electricity, very reactive, occur only in salts
Alkaline Earth Metals
metallic, silvery, occur only in salts, malleable, reactive
Halogens
nonmetals, exist as diatomic, very reactive, only occur in salts and minerals
Noble Gases
colorless and odorless, nonmetals, very nonreactive, occur naturally as atomic gases
Amphoteric
A compound, usually a metal oxide or hydroxide, that is able to react as base and acid
Dipole moment
lopsided charge
, Polyatomic ions
charged, covalently bonded groups of atoms
Ionic solid
solid whos constituent particles are ions ordered into a regular 3D arrangement held
together by ionic bonds
Chemical bond
force that holds atoms together in chemical compounds
Ground state electron configuration
a description of the atomic orbitals that are occupied in the lowest-energy state of an
atom or ion
Aufbau principle
lower-energy orbitals fill before higher-energy orbitals. Orbitals have two electrons,
which have opposite spins
Effective nuclear charge
due to electron shielding of outer electrons by inner electrons and may be substantially
lower than the actual n charge (Z-eff)
Electronegativity
ability of an atom in a chemical bond to attract shared electrons (an estimated number,
cannot be measured)
Oxoanions
binary polyatomic anions in which an atom of a given element is combined with different
numbers of oxygen atoms
VSEPR
Valence shell electron pair repulsion
Formal charge
(# of valence e−)−(# of bonds)-(of nonbinding e−)
Lewis structure
Representation of distribution of valence electrons in an atom or molecule
molecule
unit of matter that results when 2 or more atoms are joined by covalent bonds
core electrons
inner-shell electrons
valence electrons
outer-shell electrons that are strongly shielded by core electrons
charge cloud
space occupied by a group of electrons, either in a bond or in a lone pair
valence bond theory
covalent bonds are formed by overlap of atomic orbitals, each of which contains one
electron of opposite spin
Sigma bond
a covalent bond formed by head-on overlap of orbitals in which the shared electrons re
centered about the axis between the 2 nuclei (σ)
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