Download Vocabulary CHEM121

Chemical Vocabulary for CHEM121
Lesson 1:
The elements on the extreme right of the periodic chart are the Noble Gases (Group VIIIA). They are
called “Noble” because they do not normally form compounds.
On the extreme left of the chart are the Alkali Metals (Group IA). These elements are also
called “active metals” because of their high degree of reactivity. Element #1 (Hydrogen) is
included in this group, but it is not a metal. The alkali metals are all solids (hydrogen is a
gas). In compounds, the alkali metals become cations (positive ions) with a charge
(oxidation number) of +1.
Group IA: Alkali Metals
Group VIIIA: Noble Gases
symbol
H
Li
Na
K
Rb
Cs
Fr
symbol
He
Ne
Ar
Kr
Xe
Rn
name
Hydrogen* (is a non-metal)
Lithium*
Sodium*
Potassium*
Rubidium
Cesium
Francium
name
Helium*
Neon*
Argon*
Krypton*
Xenon*
Radon*
*denotes element you should know
Lesson 2:
The other group of “active metals” is the Alkaline Earth Metals, found in the 2nd column (Group IIA).
These elements are all solids. In compounds, these elements become cations with a charge of +2.
The group next to the noble gases is the Halogens (Group VIIA). Hydrogen is included in
this group on some charts. Hydrogen, fluorine and chlorine are gases, bromine is a liquid (one
of only 2 on the chart—the other is Mercury, Hg*), and iodine & astatine are solids.
Group IIA: Alkaline
Earth Metals
Be
Mg
Ca
Sr
Ba
Ra
symbol name
Beryllium*
Magnesium*
Calcium*
Strontium*
Barium*
Radium*
Group VIIA: Halogens
H
F
Cl
Br
I
At
symbol name
Hydrogen*
Fluorine*
Chlorine*
Bromine*
Iodine*
Astatine
All the elements in this group exist as homonuclear diatomic molecules: H2, F2, Cl2, Br2, I2.
Only the elements in air (Oxygen*, O2 and Nitrogen*, N2) do the same.
When the halogens form monatomic anions (negative ions), they have a charge of -1. The suffix “-ide” is used to
indicate when this is the case: fluoride, chloride, bromide, iodide.
Note: Hydrogen is +1 in the vast majority of its compounds; it can be a hydride only when combined with the
active metals.
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Lesson 3:
Continuing from the left, the next tall column is:
Group IIIA
symbol
name
B
Boron*
Al
Aluminum*
Ga
Galium
In
Indium
Tl
Thallium
These have oxidation numbers of +3 when combined.
The Group VIA elements are:
symbol
name
O
Oxygen*
S
Sulfur*
Se
Selenium
Te
Tellurium
Po
Polonium
When these are the negative parts of 2-element
(binary) compounds, they have an oxidation
number of -2.
Note the heavy stair-step line drawn between elements B & Al, etc. This line separates the metals (lower left) from
the non-metals (upper right).
 Metals can only form cations.
 Non-metals form anions when combined with metals.
 Elements that touch the line are called metalloids (except Al, which is a metal).
Oxygen combines with all elements except Noble Gases. Oxygen usually forms the oxide (O2-) ion in compounds,
but also may form a homunuclear diatomic anion called peroxide (O22-) —it does this only with active metals and
hydrogen.
Chemical formulas are representations of a chemical species that identify the number and type of atoms that make
up a chemical unit (compound, ion, etc.). The formula includes symbols of each element and numerical subscripts
to show the number of each atom present. If only one atom is present, no subscript is used.
Formulas of binary salts: (two-element compounds formed from a metal and a non-metal) Remember that the
compound is neutral (the positive and negative charges must add up to zero). The symbol for the metal is listed
first and subscripts are used to indicate the number of ions (if more than 1). The name is that of the metal followed
by that of the non-metal with the “-ide” ending to indicate the homonuclear anion.
2+
Example: Ca
and F -two fluoride ions are needed to combine with one calcium ion to give
CaF2
calcium fluoride
Writing formulas using the cross-charge method:
3+
2Example: Al
and O -the charge on the cation becomes the
subscript for the anion
Lesson 4
Al2O3
aluminum oxide
Group VA
symbol
name
N
Nitrogen*
P
Phosphorus*
As
Arsenic
Sb
Antimony
Bi
Bismuth
The non-metals (N, P) in this group have a -3 charge
when they form monatomic anions.
Other common metals that are monovalent:
Ag
Silver*
is +1 in compounds
Zn
Zinc*
is +2 in compounds
Cd
Cadmium* is +2 in compounds
Group IVA
symbol
name
C
Carbon*
Si
Silicon*
Ge
Germanium
Sn
Tin*
Pb
Lead*
These elements can have oxidation numbers from -4
to +4
2
Lesson 5:
Type II Metals: Metals that form more than one cation (have multiple oxidation states)
Salts of metals that form more than one cation can be named:
1. By including the charge as a Roman numeral in parentheses (IUPAC nomenclature)*
Fe2+
iron(II)
Fe3+
iron(III)
2. By using the suffixes “-ous” and “-ic” for the lower and higher oxidation states (common nomenclature)
Fe2+
ferrous
Fe3+
ferric
You should know the following type II metal ions*:
Au+
gold(I)
Au3+
gold(III)
Cu+
copper(I)
2+
Cu
copper(II)
Hg2+
mercury(II)
Fe2+
iron(II)
Fe3+
iron(III)
Ni2+
nickel (II)
Ni3+
nickel(III)
2+
Pb
lead(II)
Pb4+
lead(IV)
Sn2+
tin(II)
Sn4+
tin(IV)
A few more transition metals to know*:
Co
Cobalt
Pd
Palladium
Pt
Platinum
U
Uranium
Elements to know:
Cr
Mn
B
Co
Pd
Pt
C
Si
He
Ne
Ar
Kr
Xe
Rn
Ra2+
Lesson 6:
Polyatomic ions: (group of atoms with a charge)
formula
name
OHhydroxide
CN
cyanide
NH4+
ammonium
+
[H3O
hydronium is an ion we will learn about in the chapter on acids]
Note that parentheses may now be needed for subscripts:
ammonium sulfide is (NH4)2S
3
Oxyanions: (anions made up from an atom covalently bonded to one or more oxygens) Compounds containing
these anions are named with the suffix “-ate”. When two oxyanions are possible, the one with fewer oxygens is
named “-ite”.
formula
name
formula “ite”
CO32carbonate
NO3nitrate
NO2- nitrite
PO43phosphate
PO33- phosphite
2SO4
sulfate
SO32- sulfite
Some elements can form more than 2 oxyanions. For example, chlorine forms the following 4 oxyanions:
ClOhypochorite
(hypo = below)
ClO2chlorite
ClO3chlorate
ClO4perchlorate
(from hyper = above)
Some metals also form oxyanions:
MnO4permanganate (also uses the per prefix)
CrO42chromate
Cr2O72dichromate
Mixed Salts: Some polyatomic ions (having a -2 or higher charge) can form a related ion in which a hydrogen (H+)
is attached to the anion, the charge becomes -1 and the prefix “bi-“ is used.
formula
name
HCO3bicarbonate
(or hydrogen carbonate)
HSO4
bisulfate
(or hydrogen sulfate)
HSO3
bisulfite
(or hydrogen sulfite)
2HPO4
hydrogen phosphate
H2PO4dihydrogen phosphate
Organic anions:
C2H3O2
-
(or CH3COO-) acetate
Lesson 7:
Molecular vs. Ionic Compounds
Compounds may be divided into 2 general types:
1. Molecular (covalent) compounds are combinations of non-metals
2. Ionic (contains ions) includes:
Acids: anything giving H+ when dissolved in water
Bases: anything giving OH- when dissolved in water
Salts: all other ionic materials
Formulas of molecular/covalent compounds:
Non-metals can combine with other non-metals to form molecules. Molecules are covalently bonded groups of
atoms—they do not have a charge like polyatomic ions, but are neutral. Since more than one combination is
possible, the names must be more explicit. The number of atoms is given by a Greek prefix (mono-, di-, tri-, tetra-,
penta-, hexa-, hepta-, octa-, nona-, deca-).
Note: a prefix is not used if there is only one of the first
example
name
element listed. Also, the prefix is usually omitted when H
CO
carbon monoxide
is the first element.
CO2
carbon dioxide
HF
hydrogen fluoride
N2O5
dinitrogen pentoxide
*Know the Greek prefixes for 1-6
SF6
sulfur hexafluoride
H2S
hydrogen sulfide
4
More on Hydrogen:
Hydrogen compounds of the second period elements
frequently have common names:
Ionic Compounds:
-Crystalline array of cations/anions
BH3
CH4
NH3
H2O
H2O2
borane*
methane*
ammonia*
water*
hydrogen peroxide*
Molecular/Covalent Compounds:
-Group of atoms joined by covalent bonds
CH4
methane is a molecular
compound
NaCl is an
ionic compound
Lesson 8:
Binary Acids:
When some hydrogen-containing compounds are dissolved in water, an ionic substance, called an acid, is formed.
The name changes to hydro[nonmetal]ic acid for these binary acids.
HF(aq)
HCl(aq)
HBr(aq)
HI(aq)
hydrofluoric acid*
hydrochloric acid*
hydrobromic acid*
hydroiodic acid*
Note that: HF(g) is hydrogen fluoride, but when it is
dissolved in water, it is called hydrofluoric acid HF(aq)
Also note:(aq) stands for aqueous solution
(s) stands for solid
(l) stands for liquid
(g) stands for gas
Ternary Acids:
Oxyacids are formed by combining an oxyanion with hydrogen as the cation (and dissolving it in water). They are
named by stating the name of the oxyanion, but changing “-ate” to “-ic” or changing “-ite” to “-ous” and adding
acid.
H3BO3(aq)
boric acid
H2CO3(aq)
carbonic acid*
HNO3(aq)
nitric acid*
HNO2(aq)
nitrous acid
Organic Acids:
H2SO4(aq)
sulfuric acid*
HC2H3O2(aq) acetic acid*
H3PO4(aq)
phosphoric acid*
HClO4(aq)
perchloric acid*
Strong acids are acids that dissociate completely when dissolved in water. The 6 strong laboratory acids are:
hydrochloric, hydrobromic, hydroiodic, nitric, sulfuric & perchloric acids (they are underlined above).
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Exercises: use only a plain periodic table when answering the following.
Lesson 1:
1. Write the name & symbol for the each of the Noble Gases.
2. Write the name, symbol & oxidation number (ionic charge) for each of the Alkali Metals.
Lesson 2:
1. Write the name, symbol & oxidation number for each of the Alkaline Earth Metals.
2. Write the name, symbol & oxidation number for each of the Halogens.
3. Define: Cation; Anion
4. Write the formulas for each of the (6) diatomic elements.
Lesson 3:
1. Write the name, symbol & oxidation number for all the metals learned so far.
2. Write the name, symbol & oxidation number for all the nonmetals.
3. Write the formulas for:
sodium fluoride
sodium sulfide
magnesium fluoride
magnesium sulfide
aluminum fluoride
aluminum sulfide
4. Define: Binary salt
Lesson 4:
1. Write the names and formulas for all of the binary salts formed from the following combinations of cations and
anions.
Cl -
S2-
P3-
K+
Ba2+
Al3+
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Lesson 5:
1. Write the names & formulas for all of the salts formed from the following combinations of cations and anions.
Cl -
S2-
N3-
Cu+
Pb2+
Fe3+
Lesson 6:
1. Write the names & formulas for all of the salts formed from the following combinations of cations and anions.
OH Ag+
CO32-
PO43-
SO32-
HCO3-
Ca2+
Al3+
Fe2+
Pb4+
Au+
Lesson 7:
1. Give the formula or name:
oxygen dichloride
sulfur hexafluoride
hydrogen sulfide
dinitrogen monoxide
SO2
SO3
CS2
CH4
Lesson 8:
1. Write the names and formulas of the (4) binary acids you have learned. Identify which ones are weak which
ones are strong acids.
2. Write the formulas of the following acids:
carbonic acid
sulfuric acid
nitric acid
acetic acid
Additional Practice: Do the Vocabulary Worksheets posted on Canvas
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Element List
Al
Ar
Ba
Be
B
Br
Cd
Ca
C
aluminum
argon
barium
beryllium
boron
bromine
cadmium
calcium
carbon
Cl
Cr
Co
Cu
F
Au
He
H
I
chlorine
chromium
cobalt
copper
fluorine
gold
helium
hydrogen
iodine
Fe
Kr
Pb
Li
Mg
Mn
Hg
Ne
Ni
iron
krypton
lead
lithium
magnesium
manganese
mercury
neon
nickel
N
O
Pd
P
Pt
Pu
K
Ra
Rn
nitrogen
oxygen
palladium
phosphorus
platinum
plutonium
potassium
radium
radon
Si
Ag
Na
Sr
S
Sn
U
Xe
Zn
silicon
silver
sodium
strontium
sulfur
tin
uranium
xenon
zinc
Ions of Representative Elements
(+1 cations)
IA
+
H
Li
hydrogen/proton
+
+
Na
K+
lithium
sodium
potassium
IIA
2+
Be
2+
Mg
2+
Ca
Sr2+
2+
Ba
(+2 cations)
IIIA
beryllium
Al3+ aluminum
magnesium
(+3 cations)
VA
(-3 anions)
N3- nitride
3-
P
phosphide
VIA
(-2 anions)
O2-
oxide
2-
S
F
Cl
-
Br
I-
calcium
strontium
barium
sulfide
VIIA
-
(-1 anions)
fluoride
chloride
bromide
iodide
Polyatomic Ions
Transition Metal Ions
monovalent
Ag+
Zn
2+
Cd2+
silver
zinc
cadmium
variable charge
Au
+
gold (I)
Au
2+
gold (III)
Cu
+
copper (I)
Cu
2+
copper (II)
2+
mercury (II)
Hg
Fe
2+
iron (II)
Fe
3+
iron (III)
Ni
2+
nickel (II)
Ni
3+
nickel (III)
Pb
2+
lead (II)
Pb
4+
lead (IV)
Sn
2+
tin (II)
Sn
4+
tin (IV)
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