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62 terms

Chapter 8 - Ionic Compounds

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chemical bond
the force that holds two atoms together
anion
a negatively charged ion
cation
a positively charged ion
ionic bond
the electrostatic force that hold oppositely charged particles together in an ionic compound
octet
elements that have a set of eight outermost electrons
pseudo-noble gas formations
the relatively stable electrons structures developed by loss of electrons in certain elements in groups 1B, 2B, 3A, and 4A.
noble gases
the family of elements that have little tendency to react
True or False: A positively charged ion is called an anion
False
True or False: the elements in group 1A lose their one valence electron, forming an ion with a 1+ charge
True
True or False: the elements tend to react so that they acquire the electron structure of a halogen
False
True or False: A sodium atom tends to lose one electron when it reacts
True
True or False: The electron structure of a zinc ion is an example of pseudo noble gas formation
True
True or False: A Cl- ion is an example of a cation
False
True or False: The ending -ide is used to designate an anion
True
True or False: Nonmetals form a stable outer electron configuration by losing electrons and becoming anions
False
The formula unit of an ionic compound shows the
simplest ratio of the ions
The overall charge of a formula unit for an ionic compound is
always zero
ionic bonds generally occur between a
metal and nonmetal
salts are an example of
ionic compounds
in the crystal lattice of an ionic compound,
ions are surrounded by ions of the opposite charge.
what is the relationship between lattice energy and the strength of the attractive force holding ions in place?
the more negative the lattice energy is, the greater the force.
the formation of a stable ionic compound from ions is
always exothermic
in electron transfer involving a metallic atom and a nonmetallic atom during ion formation - what happens?
the nonmetallic atom gains electrons from the metallic atom.
In ionic compounds, the melting point is
high
In ionic compounds, the boiling point is
high
In ionic compounds,electrical conductivity in the solid state is
poor
In ionic compounds, the electrical conductivity in a liquid state is
good
In ionic compounds, the electrical conductivity when dissolved in water is
good
True or False: The crystal lattice of ionic compounds affects their melting and boiling points
true
True or False: the lattice energy is the energy required to separate the ions of an ionic compound
true
True or False: the energy of an ionic compound is higher than that of the separate elements formed in it
false
True or False: the large ions tend to produce a more negative value for lattice energy than smaller ions do
false
True or False: ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do.
true
Copper has the charge of
+1, +2
Iron has the charge of
+2, +3
Lead has the charge of
+2, +4
Mercury has the charge of
+1, +2
Tin has the charge of
+2, +4
Zinc has the charge of
+2
Silver has the charge of
+1
What are the 5 metals that could have different charges?
Iron, copper, tin, lead, and mercury
Ammonium
NH4 1+
Acetate
C2H302 1-
Perchlorate
ClO4 1-
Chlorite
ClO2 1-
Hydrogen carbonate or bicarbonate
HCO3 1-
Hydroxide
OH 1-
Nitrate
NO3 1-
Nitrite
NO2 1-
Carbonate
CO3 2-
Sulfate
SO4 2-
Sulfite
SO3 2-
Phosphate
PO4 3-
Hypochlorite
ClO 1-
Chlorate
ClO3 1-
oxyanion
when a negatively charged ion includes one or more oxygen atoms
If two ions can be formed that contain different numbers of oxygen atoms, the name of the ion with more oxygen atoms ends with the suffix
-ate
The name for the in with fewer oxygen atoms ends with
-ite
monatomic
a one-atom ion
polyatomic
ions made up of more than one atom
subscript
is a small number used to represent the number of ions of a given element in a chemical formula
the charge of an ion is equal to the atoms
oxidation number