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Chemistry Chapter 7
Terms in this set (135)
electrons that are free to move in metals
for a monatomic ion, is equal to the charge
the force that holds two atoms together
a charged particle containing more than one atom
a positively charged ion
a negatively charged ion
an ionic compound whose aqueous solution conducts electricity
the name for most ionic compounds other than oxides
represents the way electrons exist in metals
electron sea model
a charged particle containing only one atom
the energy needed to separate the ions of an ionic compound
the electrostatic force that holds oppositely charged particles together
a mixture of elements that has metallic properties
a polyatomic ion composed of an element bonded to at least one oxygen atom
shows the simplest ratio of ions in an ionic compound
the attraction of a metallic cation for delocalized electrons
What is the name of the model of metallic bonding that is illustrated?
electron sea model
Why are the electrons in a metallic solid described as delocalized?
Electrons are free to move from one atom to another.
Which electrons from the metal make up the delocalized electrons?
Are the metal atoms that are shown cations or anions? How can you tell?
Cations- they are positively charged
How do the metallic ions differ from the ions that exist in ionic solids?
The electrons are not completely lost by the metal atoms, as they are in an ionic solid.
Explain what holds the atom together in the solid.
They are bonded by oppositely charged electron sea that surrounds them.
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Malleable
Yes, when the metal is hammered the delocalized electrons move, keeping the metallic bonds intact
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Brittle
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Lustrous
Yes, delocalized electrons move, sorb, and release protons
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) High melting point
Yes, the metallic bonds are strong
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Low melting point
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Ductile
Yes, when the metal is pulled, the delocalized electrons move, keeping the metallic bonds intact
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Poor conduction of heat
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Good conduction of electricity
Yes, the delocalized electrons are mobile
An ionic bond is
a force that holds together atoms that are oppositely charged
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
How many chloride ions are present in a formula unit of magnesium chloride, given that the charge on a Mg ion is 2+?
Ionic bonds generally occur between
a metal and a nonmetal
Salts are examples of
A three dimensional arrangement of particles in an ionic solid is called a
In a 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
may be either exothermic or endothermic
In electron transfer involving a metallic atom and a nonmetallic atom during ion formation, which of the following is correct?
the nonmetallic atom gains electrons from the metallic atom
(Word that correctly describes each property in ionic compounds) Melting point
(Word that correctly describes each property in ionic compounds) Boiling point
(Word that correctly describes each property in ionic compounds) Hardness
(Word that correctly describes each property in ionic compounds) Brittleness
(Word that correctly describes each property in ionic compounds) Electrical conductivity in the solid state
(Word that correctly describes each property in ionic compounds) Electrical conductivity in the liquid state
(Word that correctly describes each property in ionic compounds) Electrical conductivity when dissolved in water
The crystal lattice of ionic compounds affects their melting and boiling points.
The lattice energy is the energy required to separate the ions of an ionic compound.
The energy of an ionic compound is higher than that of the separate elements that formed it.
Larger ions tend to produce a more negative value for lattice energy than smaller ions do.
Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller chargers do.
The overall charge of a formula unit for a compound is never zero.
In a crystal lattice, each positive ion is surrounded by negative ions.
Delocalized valence electrons are typical of ionic compounds.
A sulfate ion contains fewer oxygen atoms than a sulfate ion does.
Metals tend to be malleable and ductile and to have relatively high melting points.
The more negative the lattice energy is, the stronger is the force of attraction between the ions of an ionic compound.
In naming ionic compounds, the cation is first.
When a metal reacts with a nonmetal, the metal tends to gain electrons.
In naming a monatomic anion, the suffix -ide is used.
The prefix per- is used in naming the anion with the most oxygen atoms.
What is the electron configuration for the noble gases other than helium?
How many outermost d electrons are there in an ion that has achieved a pseudo-noble gas configuration?
The anion that has the formula CIO- is called the
Where does a subscript that indicated the number of atoms appear, relative to a chemical symbol in a formula?
to the lower right
What is the formula of calcium phosphate, which is made up of the ions Ca^2+ and PO4^3-?
Which of the following is an example of an interstitial alloy?
A one atom ion is called a
The charge of such an ion is equal to the atom's ___, which is the number of ___ transferred to or from the atom to form the ion
oxidation number, electrons
In ionic compounds, the sum of the charges of all the ions equals
Ions made up of more than one atom are called
If such an ion is negatively charged and includes one or more oxygen atoms, it is called an
If two such ions can be formed that contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends with the suffix
The name for the ion with fewer oxygen atoms ends with
In the chemical formula for any ionic compound, the chemical symbol for the ___ is written first, followed by the chemical symbol for the ___.
A ___ is a small number used to represent the number of ions of a given element in a chemical formula
Such numbers are written to the ___ of the symbol for the element
If no number appears, the assumption is that the number equals
iron (III) oxide
iron (II) iodate
nickel (II) chloride
copper (I) oxide
iron (III) perchlorate
K+ + Cl- =
Fe^3+ + O^2- =
Na+ + SO4^2- =
Al^3+ + NO3- =
Ca^2+ + PO4^3- =
iron (II) phosphate
copper (II) nitrate
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