Chemistry Chapter 7
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
-ate
The name for the ion with fewer oxygen atoms ends with
-ite
What is the formula of calcium phosphate, which is made up of the ions Ca^2+ and PO4^3-?
Ca3(PO4)2
Are the metal atoms that are shown cations or anions? How can you tell?
Cations- they are positively charged
Why are the electrons in a metallic solid described as delocalized?
Electrons are free to move from one atom to another.
Larger ions tend to produce a more negative value for lattice energy than smaller ions do.
False
The energy of an ionic compound is higher than that of the separate elements that formed it.
False
The overall charge of a formula unit for a compound is never zero.
False/always
When a metal reacts with a nonmetal, the metal tends to gain electrons.
False/lose
Delocalized valence electrons are typical of ionic compounds.
False/metals
A sulfate ion contains fewer oxygen atoms than a sulfate ion does.
False/more
The more negative the lattice energy is, the stronger is the force of attraction between the ions of an ionic compound.
False/positive
An ionic bond is
a force that holds together atoms that are oppositely charged
Ionic bonds generally occur between
a metal and a nonmetal
Be3(PO4)2
beryllium phosphate
K2S
potassium sulfide
the name for most ionic compounds other than oxides
salts
Where does a subscript that indicated the number of atoms appear, relative to a chemical symbol in a formula?
to the lower right
How many chloride ions are present in a formula unit of magnesium chloride, given that the charge on a Mg ion is 2+?
two
In ionic compounds, the sum of the charges of all the ions equals
zero
(Word that correctly describes each property in ionic compounds) Electrical conductivity in the solid state
poor
KBrO3
potassium bromate
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Brittle
No
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Low melting point
No
(Is the property a characteristic of most metals? If yes, explain how metallic bonding accounts for the property.) Poor conduction of heat
No
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.
a charged particle containing more than one atom
polyatomic ion
Explain what holds the atom together in the solid.
They are bonded by oppositely charged electron sea that surrounds them.
In a crystal lattice, each positive ion is surrounded by negative ions.
True
In naming a monatomic anion, the suffix -ide is used.
True
In naming ionic compounds, the cation is first.
True
Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller chargers do.
True
Metals tend to be malleable and ductile and to have relatively high melting points.
True
The crystal lattice of ionic compounds affects their melting and boiling points.
True
The lattice energy is the energy required to separate the ions of an ionic compound.
True
The prefix per- is used in naming the anion with the most oxygen atoms.
True
Which electrons from the metal make up the delocalized electrons?
Valence electrons
(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.) Good conduction of electricity
Yes, the delocalized electrons are mobile
(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.) 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.) Ductile
Yes, when the metal is pulled, the delocalized electrons move, keeping the metallic bonds intact
a mixture of elements that has metallic properties
alloy
NH4Br
ammonium bromide
(NH4)2CO3
ammonium carbonate
a negatively charged ion
anion
Ions made up of more than one atom are called
polyatomic ions
(Word that correctly describes each property in ionic compounds) Brittleness
brittle
CaCl2
calcium chloride
Ca3N2
calcium nitride
Which of the following is an example of an interstitial alloy?
carbon steel
a positively charged ion
cation
In the chemical formula for any ionic compound, the chemical symbol for the ___ is written first, followed by the chemical symbol for the ___.
cation, anion
Cs3P
cesium phosphide
the force that holds two atoms together
chemical bond
CIO3-
chlorate
Cl-
chloride
CIO2-
chlorite
A three dimensional arrangement of particles in an ionic solid is called a
crystal lattice
electrons that are free to move in metals
delocalized electrons
an ionic compound whose aqueous solution conducts electricity
electrolyte
What is the name of the model of metallic bonding that is illustrated?
electron sea model
represents the way electrons exist in metals
electron sea model
shows the simplest ratio of ions in an ionic compound
formula unit
(Word that correctly describes each property in ionic compounds) Electrical conductivity in the liquid state
good
(Word that correctly describes each property in ionic compounds) Electrical conductivity when dissolved in water
good
(Word that correctly describes each property in ionic compounds) Hardness
hard
(Word that correctly describes each property in ionic compounds) Boiling point
high
(Word that correctly describes each property in ionic compounds) Melting point
high
CIO-
hyperchlorite
The anion that has the formula CIO- is called the
hypochlorite ion
the electrostatic force that holds oppositely charged particles together
ionic bond
Salts are examples of
ionic compounds
In a crystal lattice of an ionic compound
ions are surrounded by ions of the opposite charge
Fe2O3
iron (III) oxide
The overall charge of a formula unit for an ionic compound
is always zero
the energy needed to separate the ions of an ionic compound
lattice energy
LiHSO4
lithium hydrosulfate
Li2O2
lithium peroxide
Such numbers are written to the ___ of the symbol for the element
lower right
Mg(CIO)2
magnesium hypochlorite
MgO
magnesium oxide
The formation of a stable ionic compound from ions
may be either exothermic or endothermic
the attraction of a metallic cation for delocalized electrons
metallic bond
A one atom ion is called a
monatomic ion
a charged particle containing only one atom
monatomic ion
What is the electron configuration for the noble gases other than helium?
na^2np^6
If no number appears, the assumption is that the number equals
one
for a monatomic ion, is equal to the charge
oxidation number
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
If such an ion is negatively charged and includes one or more oxygen atoms, it is called an
oxyanion
a polyatomic ion composed of an element bonded to at least one oxygen atom
oxyanion
CIO4-
perchlorate
NaBrO3
sodium bromate
NaI
sodium iodide
A ___ is a small number used to represent the number of ions of a given element in a chemical formula
subscript
How many outermost d electrons are there in an ion that has achieved a pseudo-noble gas configuration?
ten
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
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
The formula unit of an ionic compound shows
the simplest ratio of the ions
