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The most active nonmetallic element is:
fluorine (F)
The insertion of a burning paraffin taper into a bottle of chlorine will result in:
the production of carbon.
The bromide iron is:
colorless.
When chlorine water and carbon tetrachloride are mixed with an unknown,
a violet layer is produced.

The unknown is:
an iodide.
The order of decreasing activity of the halogens is:
F, Cl, Br, I
A light-sensitive substance used on photographic films has the formula:
AgBr
Halides used on photographic film are silver bromide and silver iodide.
Aqua regia is:
HCl and HNO3
The metal that has an orange sulfide is:
Sb (Antimony)
a member of the Nitrogen family (Group 15),
a metalloid,
forms very weak acid, mostly basic solutions
Sulfur dioxide is the anhydride of:
sulfurous acid.
Anhydride means:

a compound derived from another compound by the removal of water;
it will combine with water to form
an acid (acid anhydride) or a base (basic anhydride).
The charring action of sulfuric acid is due to its being:
a dehydrating agent.
Dehydrating agent means:

a substance able to withdraw water from another substance, thereby drying it.
Sulfuric acid is used in the manufacture of many other acids because of its:
high boiling point.

(338 degrees Celsius)
Nitrogen for commercial use is generally obtained from:
liquid air.
Nitrogen is a colorless, odorless, tasteless, and rather inactive gas
that makes up 4/5ths of the air in our atmosphere.
Ammonia is prepared commercially by the:
Haber process.
Haber process:
a catalytic method for the union of atmospheric nitrogen with hydrogen to form ammonia.
A nitrogen compound that has a color is:
nitrogen dioxide.
Nitrogen dioxide is a reddish-brown gas,
1.6 times heavier than air,
very soluble in water,
and extremely poisonous.
It has a very unpleasant odor.
If a student heats a mixture of ammoniom chloride and calcium hydroxide in a test tube,
he or she will detect:
the odor of ammonia.
Chlorine has the ability to:
withdraw hydrogen from hydrocarbons.
The halogen chlorine is used to:
1. purify water supplies
2. bleach
3. prepare pure hydrochloric acid
Chlorine is used in many industrial applications.
Uses for fluorides include:
added to drinking water and toothpaste to reduce tooth decay
How does hypochlorous acid bleach?
by oxidation.
List uses for the halogen bromine.
1. as ethylene dibromide in antiknock gasolines to remove the lead deposits
that form from the other additive, tetraethyl lead.
2. as a bromide in many nerve sedatives.
List the most widely known use of iodine.
As an antiseptic in an alcohol solution of iodine called tincture of iodine.
Iodine is also used in small amounts to treat goiter conditions.
The difference between ammonia and ammonium is:
a proton.
An important ore of iron is:
hematite.
Hematite = Fe2O3
The material added to the charge of a blast furnace to react with the sand is:
calcium carbonate.
A reducing agent used in the blast furnace is:
CO
The most abundant of all metals in the earth's crust is:
aluminum.
List the outstanding properties of aluminum.
1. light-weight with high strength
2. ability to form an aluminum oxide coating that protects this metal from further oxidation
3. ability to conduct an electric current
The solvent used in obtaining aluminum from its ore is:
cryolite
The Hall process is the electrolytic method of preparing aluminum.
It uses molten cryolite (Na3AIF6) as the solvent for bauxite ore (Al2O3 * 2H2O).
The process of extracting aluminum is called:
the Hall process.
Aluminum is extracted from its oxide by:
electrolysis.
The Dow process extracts magnesium from:
seawater.
Dow Process:

an electrolytic method of preparing magnesium from seawater.

The magnesium salts are precipitated with Ca(OH)2 solution to form Mg(OH)2.

The hydroxide is then converted to a chloride by adding hydrochloric acid to the hydroxide.

This chloride is mixed with potassium chloride, melted, and electrolyzed
to release the magnesium at the cathode and chlorine at the anode.
An alloy of bismuth is used in automatic fire sprinklers because:
it has a low melting point.
List the important properties of magnesium.
1. light weight
2. rigid
3. inexpensive metal
4. can form a protective adherent oxide coating
Name 3 important metals that can be prepared by electrolysis.
1. aluminum
2. magnesium
3. copper
Which metal is refined by reduction in a blast furnace?
iron ore
The molten iron from the blast furnace is called:
pig iron.
Define Alloy.
Alloy means:

a substance composed of 2 or more metals, which are intimately mixed;
usually made by melting the metals together.
Define acid salt.
Acid salt:

a salt formed by replacing part of the hydrogen ions
of a dibasic or tribasic acid with metallic ions.
Define allotropic forms.
Allotropic forms:

forms of the same element that differ
in their crystalline structures.
Allotropic forms of sulfur:
1. rhombic
2. monoclinic
3. amorphous
Define alloy.
Alloy:

a substance composed of two or more metals,
which are intimately mixed;
usually made by melting the metals together.
Define aqua regia.
Aqua regia:

a mixture of 3 vol of concentrated HCl (hydrogen chloride) and
1 vol of concentrated HNO3 (nitric acid).
that can dissolve gold or platinum.
Name the colorless gas that has an odor of rotten eggs.
hydrogen sulfide
Hydrogen sulfide:

1. odor of rotten eggs
2. fairly soluble in water
3. poisonous in rather small concentrations
4. can be prepared by reacting ferrous sulfide with an acid, such as dilute HCl
5. burns in excess oxygen to form compounds of water and sulfur dioxide
6. a weak acid in water solution
7. widely used in qualitative lab tests since many metallic sulfides precipitate with recognizable colors (sometimes used as paint pigments)
Name the compound of sulfer that is a colorless gas with a suffocating oor.
sulfur dioxide
The acid anhydride of sulfurous acid.

Used as a bleach on moist straw, silk, wool, and paper
because of its ability to reduce the coloring agent.
Describe the test for fluoride.
Add sulfuric acid and test if the gas released,
which will be hydrogen fluoride (HF),
will etch glass.
CAUTION: do NOT get on hands.
Describe the test for chloride.
Add a solution of silver salt (usually silver nitrate)
and look for a white precipitate that is soluble in ammonium hydroxide
but insoluble in nitric acid.
List some important halides and their uses.
1. hydrochloric acid: used in many important industrial processes.
2. silver bromide and silver iodide: used on photographic film.
3. hydrofluoric acid: used to etch glass by reacting with
SiO2 to release silicone fluoride gas.
Also used to frost glass.
Explain the inactivity of N2 gas.
Two atoms of nitrogen are bonded by three covalent bonds
that require a great deal of energy to break.
Since nitrogen must be "pushed" into combining with other elements,
many of its compounds tend to decompose violently
with a release of the energy that went into forming them.
List some physical properties of metals.
1. metallic luster
2. conductors of heat and electricity
3. malleable (can be pounded into sheets)
4. ductile (can be drawn into wires)
5. most have a silvery color
6. densities between 7 and 14 g/cm to the thirdpower
7. none is soluble in any ordinary solvent without a chemical change
List the general chemical properties of metals.
1. electropositive
2. the more active metallic oxides form bases, although some metals form amphoteric hydroxies can react as both acid and base
Define roasting.
Roasting:

heating an ore (usually a sulfide) in an excess of air
to convert the ore to an oxide,
which can then be reduced.
Used to convert sulfide or carbonate ores to oxides.
Define anode.
Anode:

the electrode in an electrolytic cell
that has a positive charge and attract negative ions;

the electrode at which oxidation occurs in an electrochemical cell.
What is the Dow process.
An electrolytic method of preparing magnesium from seawater.
Define metalloids.
Metalloids:

1. elements that are not distinctly metals nor nonmetals.
2. semiconductors (conuct electricity poorly)
3. may form ionic or covalent bonds
4. are located in the periodic table along the heavy dark line that starts with boron (B) and drops down steplike between the elements found lower in the table.
Boron (B), Silicon (Si), Arsenic (As), Tellurium (Te), Astatine (At)
Define nitrogen fixation.
Nitrogen fixation:

any process by which atmospheric nitrogen is converted into a compound
such as ammonia or nitric acid.
Define normal salt.
Normal salt:

a salt in which all the hydrogen or the acid has been displaced by a metal.
Define resonance.
Resonance:

the phenomenon in a molecular structure
that exhibits properties between those of a single bond and those of a double bond
and thus possesses two or more alternate structures.
Which of the following when dissolved in water
and placed in the conductivity apparatus
will cause the light to glow?

A. table salt
B. ethyl alcohol
C. sugar
D. glycerine
A. table salt
The reason that a current can flow is because:

A. ions combine to form molecules.
B. molecules migrate to the charge plate.
C. ions migrate to the charge plates.
D. sparks cross the gap.
C. ions migrate to the charge plates.
Positive ions migrate to the cathode, so they are referred to as cations.

Negative ions migrate toward the positive anode, so they are called anions.
The extent of ionization depends on the:

A. nature of the solvent.
B. nature of the solute.
C. concentration of the solution.
D. temperature of the solution.
E. all of the above.
E. all of the above.
Ionization:

the process in which ions are formed from neutral atom.
Which of the following is true?

A. The number of positive ions in solution equals the number of negative ions.
B. The positive ions are called anions.
C. The positive ions are called cathodes.
D. The total positive charge equals the total negative charge.
E. None of the above.
D.The total positive charge equals the total negative charge.
The hydronium ion is represented as:

A. H2O+
B. H3O+
C. HOH+
D. H-
B.H3O+
In the electrolysis of copper chloride,
the substance liberated at the anode is:

A. copper
B. chlorine
C. hydrogen
D. copper chloride
B. chlorine.
Ions are particles that exist:

A. only in water solutions.
B. in some crystals.
C. in polar covalent compounds.
D. in covalent compounds that are not polar.
B. in some crystals.
Ionic compounds conduct an electric current when they are:

A. solidified.
B. melted.
C. frozen.
D. dehydrated.
B. melted.
The cathode in a direct-circuit is an electrode that is:

A. always negative.
B. always positive.
C. always neutral.
D. sometimes negative and sometimes positive.
A. always negative.
Electrolysis of a dilute solution of sodium chloride results in the cathode product:

A. sodium.
B. chlorine.
C. hydrogen
D. oxygen
C. hydrogen.
If the reaction potential is positive, this indicates that:

A. the reaction will not occur.
B. the reaction will occur and give off energy.
C. the reaction will occur if heat or energy is added.
D. the reaction will power an outside alternating electric current.
B. the reaction will occur and give off energy
Define anion.
Anion:

an ion or particle that has a negative charge,
and thus is attracted to a positively charged anode.
Define cation.
Cation:

an ion that has a positive charge.
Define anode.
Anode:

the electrode in an electrolytic cell that has a positive charge
and attracts negative ions.
Define cathode.
Cathode:

the electrode in an electrolytic cell that is negatively charged and attracts positive ions.
Define dissociation (ionic).
Dissociation (ionic):

The separation of the ions of an electrovalent compound
as a result of the action of a solvent.
Define electrode potential.
Electrode potential:

The difference in potential between an electrode
and the solution in which it is immersed.
Define electrolyte.
Electrolyte:

a liquid that will conduct an electric current.
Define electrolytic reaction.
Electrolytic reaction:
Define electromotive series.
Elecromotive series:
Define ionization.
Ionization:

the process in which ions are formed from neutral atoms.
Define Nernst equation.
Walter Nernst developed a mathematical relationship that enables us to calculate
the cell voltages and direction of a spontaneous reaction at their than standard-state
Define oxidation.
Oxidation:

the chemical process by which oxygen is attached to a substance;
the process of losing electrons.
Define reduction.
Reduction:
Define standard voltage.
Standard voltage:
Define electrolytes.
Electrolytes:

1. substances that dissolve in water to form a solution that will conduct an electric current.
2. substances that become ions in solution and acquire the capacity to conduct electricity
Electrolytes include:
sodium, potassium, chloride, and bicarbonate.
Describe a strong electrolyte.
A strong electrolyte is:

a compound that when dissolved in water will completely ionize or dissociate into ions.

That is, the compound exists in water only as individual ions,
and there are no intact molecules at all.

This solution conducts electricity well.
Srong electrolytes fall into 3 categories:

1. strong acids: HCl, HBr, HI, HNO3, HClO3, HClO4, and H2SO4

[hydrochloric acid (HCl), hydrobromic acid (HBr), Hydriodic acid (HI), Nitric acid (HNO3), Chloric acid (HClO3), Perchloric acid (HClO4), Sulfuric acid (H2SO4)]

2. strong bases: NaOH, KOH, LiOH, Ba(OH)2, and Ca(OH)2

[Sodium hydroxide (NaOH), Potassium hydroxide (KOH), Lithium hydroxide (LiOH), Barium hydroxide ( Ba(OH)2), Calcium hydroxide (Ca(OH)2)

3.salts: NaCl, KBr, MgCl2, and many more

Describe a weak electrolyte.
A weak electrolyte is a compound that when dissolved in water
only partially ionizes or dissociates into ions.

That is, the compound exists in water
as a mixture of individual ions and intact molecules.

This solution conducts electricity weakly.
Weak electrolytes fall into 2 categories:

1. weak acids: HF (hydrogen fluoride), HC2H3O2 (acetic acid), H2CO3 (carbonic acid), H3PO4 (phosphoric acid), and many more

2. weak bases: NH3 (ammonia), C5H5N (pyridine),
several more, all containing "N"
Describe a nonelectrolyte.
Nonelectrolyte:

a compound that when dissolved in water does not ionize or dissociate into ions at all.

In water, this compound exists entirely as intact molecules.

The solution does not conduct electricity at all.
Nonelectrolytes are compounds that don't ionize when they dissolve in water.

Nonelectrolytes are limited to covalent compounds.

Many compounds of carbon such as mathane CH4, benzene C6H6, ethanol C2H5OH, ether (C2H5)2O, and formaldehyde CH2O, are nonelectrolytes.

A few inorganic compounds such as nitrous oxide N2O, phosphine PH3, and nitrogen(III) chloride NCl3, are nonelectrolytes.
Review the Six Steps for Categorizing Electrolytes.
One practical method is outlined below:

Step 1: Is it one of the seven strong acids?

Step 2: Is it of the form Metal(OH)n? Then it's a strong base.

Step 3: Is it of the form Metal(X)n? Then it's a salt.

Step 4: Does it's formula start with 'H'? It's probably a weak acid.

Step 5: Does it have a nitrogen atom? It may be a weak base.

Step 6: None of those? Call it a nonelectrolyte.
Define half-reaction.
Half-reaction:

the reaction taking place at each electrode in an electrochemical cell.
The gain of electrons by a copper ion is called:
reduction.
Reduction:

a reaction in which the atoms or ions of an element gain one or more electrons and,
hence, attain a more negative (or less positive) oxidation state.
The loss of electrons by zinc is called:
oxidation.
Oxidation:

a reaction in which the atoms or ions of an element lose one or more electrons
and, hence, attain a more positive (or less negative) oxidation state.
Reactions that do not occur spontaneously can be forced to take place
by supplying energy with an external current.

This is called:
electrolytic reactions.
Types of electrolytic reactions include:

1. electroplating
2. electrolysis of water
3. electrolysis of molten salts