Ch. 8 Ionic Compounds Flashcards
Chemical bond
- The force that holds two atoms together
- an attachment may form by the attraction of the positively charged nucleus of one atom for the negatively charged electrons of another atom or by the attraction of charged atoms which are called ions
Valence electrons
- the electrons in the outermost energy level
- also in the chemical bond attraction
Noble gasses
Are a family of elements that have very little tendency to react
Stable Octet
Elements have a set of eight outermost electrons
Pseudo- noble gas formations
Relatively stable electrons structures developed by loss of electrons in certain elements of groups 1B, 2B, 3A, and 4A
True or false ?
A positively charged ion is called an anion
False
True or false ?
Elements in group 1A lose the I one valence electron, forming an ion with a 1+ charge
True
True or false ?
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 (Zn2+) is an example of a pseudo noble gas formation
True
True or false ?
A CI- ion is an example of a cation
False
True or false ?
The ending -ide is used to designate an anion
True
True or false ?
Non metals form a stable outer electron configuration by losing electrons and becoming anions
False
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 of an ionic compound
Is always zero
Ionic bonds generally occur between
A metal and a non metal
salts are ex’s of
Ionic compounds
Crystal lattice
A three dimensional arrangement of particles In an ionic solid
In a crystal lattice of an ionic compound
Ions are surround by ions of the opposite charge
What is the relationship between lattice em where 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, _________________________________________
The nonmetallic atom gains electrons from the metallic atom
Melting point
High
Boiling point
High
Hardness
Hard
Brittleness
Brittle
Electrical conductivity in a sold state
Poor
Electrical conductivity in the liquid state
Good
Electrical conductivity when dissolved in water
Good
True or false ?
The crystal lattice of an ionic compound 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 that formed it
False
True or false ?
Large ions tend to produce more negative value for the lattice energy thanthe 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
Monatomic ion
A one atom ion
Oxidation number
- The number of electrons transfers to or from the atom to form the ion
- the charge of such an ion is equal to the atoms^
In ionic compounds the sum of the charges of all the ions equals ________
0
Polyatomic ions
Ions made up of more than one atom
Oxyanion
An ion negatively charged and includes one or more oxygen atoms
Suffix - ate
Two such ions can be formed that contain different number of oxygen atoms, the name for the ion with more oxygen atoms
Suffix - ite
The name for the ions with fewer oxygen atoms
Chemical formula for any ionic compound
The chemical symbol for the CATION is written first followed by the chu kcal symbol for the ANION
Subscript
- Is a small number used to represent the number of ions of a given element in a chemical formula
- these numbers are written to the lower right of symbol for the element
Chlorate
C1O¥3-
Hypochlorite
C1O-
Chloride
C1-
Perchlorate
C1O¥4-
Chlorite
C1O¥2-
NaI
Sodium Ludide
CaC1,2
Calcium chloride
K,2S
Potassium sulfide
MgO
Magnesium oxide
LiHSO
Lithium hydrogen sulfate
NH,4Br
Ammonium bromide
Ca,3N,2
Calcium nitride
Cs,3P
Cesium phosphide
KBrO,3
Potassium bromate
Mg(CIO),2
Magnesium hypo chloride
Li,2O,2
Lithium peroxide
Be,3(PO,4),2
Beryllium carbonate
(NH,4),2CO,3
Amuonium carbonate
NaBrO,3
Sodium bromate
Fr,2O,3
Iron (111) oxide
Fe(IO,3),2
Iron (111) lodate
Beryllium nitride
Be,3N,2
Nickel (11) chloride
NiCI,2
Potassium chlorite
KcIO,2
Copper (1) oxide
Cu,2O
Magnesium sulfite
MgSO,3
Ammonium sulfide
(NH,4) ,2S
Calcium iodate
Ca (IO,3) ,2
Iron (111) perchlorate
Iron (CIO,4),3
Sodium nitride
Na,3N
Why are the electrons in a metallic solid described as delocalized?
They move from one atom to another