Chapter 8 - Ionic Compounds

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62 terms

chemical bond

the force that holds two atoms together


a negatively charged ion


a positively charged ion

ionic bond

the electrostatic force that hold oppositely charged particles together in an ionic compound


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


True or False: the elements in group 1A lose their one valence electron, forming an ion with a 1+ charge


True or False: the elements tend to react so that they acquire the electron structure of a halogen


True or False: A sodium atom tends to lose one electron when it reacts


True or False: The electron structure of a zinc ion is an example of pseudo noble gas formation


True or False: A Cl- ion is an example of a cation


True or False: The ending -ide is used to designate an anion


True or False: Nonmetals form a stable outer electron configuration by losing electrons and becoming anions


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


In ionic compounds, the boiling point is


In ionic compounds,electrical conductivity in the solid state is


In ionic compounds, the electrical conductivity in a liquid state is


In ionic compounds, the electrical conductivity when dissolved in water is


True or False: The crystal lattice of ionic compounds affects their melting and boiling points


True or False: the lattice energy is the energy required to separate the ions of an ionic compound


True or False: the energy of an ionic compound is higher than that of the separate elements formed in it


True or False: the large ions tend to produce a more negative value for lattice energy than smaller ions do


True or False: ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do.


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


Silver has the charge of


What are the 5 metals that could have different charges?

Iron, copper, tin, lead, and mercury


NH4 1+


C2H302 1-


ClO4 1-


ClO2 1-

Hydrogen carbonate or bicarbonate

HCO3 1-


OH 1-


NO3 1-


NO2 1-


CO3 2-


SO4 2-


SO3 2-


PO4 3-


ClO 1-


ClO3 1-


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


The name for the in with fewer oxygen atoms ends with



a one-atom ion


ions made up of more than one atom


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

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