Energy due to motion, occurs as a result of vibration, rotation, or translation

Energy due to position, is contained in bonds and intermolecular forces

Forms between a metal and a nonmetal, an electrostatic attraction between ions, occurs when electrons are transferred

Forms between 2 or more nonmetals, the sharing of electrons

When atoms bond, they lose, gain, or share electrons to attain a filled outer layer of eight electrons

The observation that atoms will tend to gain, lose, or share electrons until they are surrounded by 8 valence electrons

Used to indicate the number of valence electrons an atom has, represented as dots

Ratio of ions based on charge balance

The energy required to completely separate a mole of a solid ionic compound into its gaseous ions

Lattice energies are impacted by two primary factors:

Atomic orbitals overlap to share electrons

When the bond order=1 and one pair of electrons are shared between atoms

When there are unequally shared electrons between 2 or more nonmetals

An unequal sharing of electrons between atoms (a polar covalent bond)

When electrons are shared equally between 2 or more nonmetals

Covalently bonding groups of ions that carry an overall charge

Anions containing oxygen and another element

Hydrogen carbonate or bicarbonate

The percentage by mass contributed by each element in a sample

Contains the simplest whole number ratio of the types of atoms present in a compound

Describes actual numbers of atoms of each element in a molecule, and it can be the same as the empirical formula

The number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the Lewis Structure

When there is more than one Lewis Structure for a molecule that differs only in the position of the electrons

Regions about a central atom where electrons are located

Defined by the positions of only the atoms in the molecules, not in the nonbonding pairs

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chem exam 2

Term	Definition
KineticEnergy	Energy due to motion, occurs as a result of vibration, rotation, or translation
PotentialEnergy	Energy due to position, is contained in bonds and intermolecular forces
Bonded	Atoms are more stable when...
IonicBond	Forms between a metal and a nonmetal, an electrostatic attraction between ions, occurs when electrons are transferred
CovalentBond	Forms between 2 or more nonmetals, the sharing of electrons
MetallicBond	Forms between 2 metals
LewisTheory	When atoms bond, they lose, gain, or share electrons to attain a filled outer layer of eight electrons
OctetRule	The observation that atoms will tend to gain, lose, or share electrons until they are surrounded by 8 valence electrons
LewisSymbols	Used to indicate the number of valence electrons an atom has, represented as dots
Cation	Positive ion
Anion	Negative ion
ChemicalFormula	Ratio of ions based on charge balance
LatticeEnergy	The energy required to completely separate a mole of a solid ionic compound into its gaseous ions
SizeAndCharge	Lattice energies are impacted by two primary factors:
ValenceBondTheory	Atomic orbitals overlap to share electrons
SingleCovalentBond	When the bond order=1 and one pair of electrons are shared between atoms
PolarCovalentBond	When there are unequally shared electrons between 2 or more nonmetals
Dipole	An unequal sharing of electrons between atoms (a polar covalent bond)
NonpolarCovalentBond	When electrons are shared equally between 2 or more nonmetals
PolyatomicIons	Covalently bonding groups of ions that carry an overall charge
Oxyanions	Anions containing oxygen and another element
CH3COO-	Acetate
C2H3O2-	Acetate
CO3^2-	Carbonate
HCO3-	Hydrogen carbonate or bicarbonate
NO2-	Nitrate
NO3-	Nitrite
PO4^3-	Phosphate
PO3^3-	Phosphite
CrO4^2-	Chromate
SO4^2-	Sulfate
SO3^2-	Sulfite
HSO3-	Hydrogen sulfite
OH-	Hydroxide
CN-	Cyanide
MnO4-	Permanganate
NH4+	Ammonium
Cr2O7^2-	Dichromate
PercentComposition	The percentage by mass contributed by each element in a sample
EmpiricalFormula	Contains the simplest whole number ratio of the types of atoms present in a compound
MolecularFormula	Describes actual numbers of atoms of each element in a molecule, and it can be the same as the empirical formula
FormalCharge	The number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the Lewis Structure
ResonanceStructure	When there is more than one Lewis Structure for a molecule that differs only in the position of the electrons
ElectronDomain	Regions about a central atom where electrons are located
MolecularGeometry	Defined by the positions of only the atoms in the molecules, not in the nonbonding pairs

Created by: odetteschnell7

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