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Definitions
Elements/ # of Atoms
Ionic/ Covalent Compounds
Formulas
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100
binary compound
compound composed of two elements
100
NaCl
1 sodium, 1 chlorine
100
Usual state of ionic compounds at room temperature
solid
100
calcium chloride
CaCl2
100
Atoms form compounds when the compound is more ________ than the separate atoms.
stable
200
ionic bond
the force of attraction between the opposite charges of the ions in an ionic compound
200
NaOH
1 sodium, 1 oxygen, 1 hydrogen
200
Usual state of covalent compounds at room temperature
liquid or gas
200
iron (II) oxide
FeO
200
A(n) _______ is a charged particle because it has more or fewer electrons than protons.
ion
300
covalent bond
the attraction that forms between atoms when they share electrons
300
NH3
1 nitrogen, 3 hydrogen
300
Smallest particle of ionic compounds
ions
300
copper (I) oxide
Cu2O
300
_______ are neutral particles formed as a result of sharing electrons.
molecules
400
polyatomic ion
positively or negatively charged, covalently bonded group of atoms
400
SiO2
1 silicon, 2 oxygen
400
Smallest particle of covalent compounds
molecule
400
sodium sulfide
Na2S
400
__________-- compound with water chemically attached to its ions.
hydrate
500
oxidation number
number that indicates how many electrons an atom must gain, lose or share to become stable
500
H2SO4
2 hydrogen, 1 sulfur, 4 oxygen
500
How is a covalent compound formed
two non-metals
500
magnesium sulfate heptahydrate
MgSO4 • 7 H2O
500
Name binary covalent compounds by using ______ to indicate how many atoms of each element are in the compound.
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