LESSON 4: NAMING CHEMICAL FORMULA Flashcards
• Nearly 70% of known elements
• Lustrous
• Good conductor of heat &electricity
• Malleable
METALS
• Lower melting points and densities
• Form brittle solids
• Poor conductor of heat and electricity
• Reactive nonmetals and noble gases
NONMETALS
• Properties fall somewherebetween metals and nonmetals
• Have metalic apperance
• usually brittle
• not as good as metals in conducting electricity
METALLOIDS
Larger particle or structure formed when ______________________________
two or more atoms are bonded together.
single atom molecule (ex: diamond, pure gold)
Monatomic
molecule with 2 atoms (ex: Cl2, I2, Br2)
Diatomic
molecule with 3 or more atoms (ex: C6H12O6, CaCO3)
Polyatomic
particles that have a NET CHARGE (formed when an atom loses or gains electrons)
IONS
positively (+) charged
Cations
negatively (-) charged
Anions
formed from the TRANSFER of electrons between cation and anion COMBINE
IONIC COMPOUND
• Form from the SHARING of electrons between REACTIVE NONMETALS
• Gases, low-boiling liquids, low-melting solids
• Ex: methane gas, water, alcohols, chewing gum
MOLECULAR COMPOUNDS
Actual number of atoms of each element
MOLECULAR
Simplest whole number ratio
EMPIRICAL
How atoms are bonded to one another
STRUCTURAL
TYPES OF CHEMICAL FORMULA
MOLECULAR, EMPIRICAL, STRUCTURAL
MOLECULAR MODELS
Ball-and-stick-models, Ball-and-stick-models
• shows atoms as spheres and bonds as sticks
• accurately represent the bonds and bond angles at which atoms are attached to one another within the molecule, but not the actual size of the atom
Ball-and-stick-models
gives more realistic representation of the space
occupied by the atoms since it shows the relative sizes of the atoms
Space-filling model
denote the numbers of atom present.
Prefixes
The name of the other component, which will be used as the second word, would be modified to accommodate the suffix
–ide.
MONO
1
DI
2
TRI
3
TETRA
4
PENTA
5
HEXA
6
OCTA
8
NONA
9
DECA
10
occur when atoms gain, lose, or share electrons.
Chemical reactions
Sharing electrons creates a _______
covalent bond
Nonmetals can _______ electrons to form a covalent bond. This creates a ___________.
share, molecule
_______ can act as either a
metal or a nonmetal!
HYDROGEN
What elements exist as diatomic molecules?
H2, N2, O2, F2, Cl2, Br2, I2
Nonmetals _____________ electrons.
This gives them a ____ charge.
gain/accept, -
Negative ions are called ___________.
anions
Metals ________________ electrons.
This gives them a ____ charge
lose/donate, +
Positive ions are called ___________.
cations
Positive ions are called ___________.
cations
the names of metal do not change
naming ions
rules for naming ions for non metals
root of element name + ide
naming ionic compounds
- write the name of metal ion
- write the name of the nonmetal ion
Ionic Compounds:
CaBr2
calcium bromide
Ionic Compounds:
NaF
sodium fluoride
Ionic Compounds:
MgO
magnesium oxide
Ionic Compounds:
SrCl2
strontium chloride
Li2S
lithium sulfide
Ionic Compounds:
CaO
calcium oxide
Ionic Compounds:
Kl
potassium iodide
naming ions:
sulfur
sulfide
naming ions:
nitrogen
nitride
naming ions:
potassium
potassium
naming ions:
oxygen
oxide
naming ions:
lithium
lithium
naming ions:
bromine
bromide
naming ions:
chlorine
chloride
naming ions:
hydrogen
hydrogen, hydride
Name the ionic compounds:
CaCl2
calcium chloride
Name the ionic compounds:
K2S
potassium permanganate
Name the ionic compounds:
BaO
barium oxide
Name the ionic compounds:
NH4Cl
ammonium chloride
Name the ionic compounds:
CsCl
cesium chloride
Name the ionic compounds:
MgSO4
magnesium sulfate
Name the ionic compounds:
NaBr
sodium bromide
Name the ionic compounds:
AlP
aluminum phosphide
These are ionic compounds that consist of two or more atoms chemically bonded together and have net electrical charge instead of being neutral
POLYATOMIC IONS
nonmetal bonded to one or more
oxygen atoms
OXOANIONS/OXYANIONS
ion with fewer oxygen atoms ends in
ite
ion with more oxygen atoms ends in
ate
HF
HYDROFLUORIC ACID
HCI
HYDROCHLORIC ACID
HBr
HYDROBROMIC ACID
HI
HYDROIODIC ACID
HCN
HYDROCYANIC ACID
H2S
HYDROSULFURIC ACID
HNO3
NITRIC ACID
HNO2
NITROUS ACID
H2SO4
SULFURIC ACID
H2SO3
SULFUROUS ACID
H3PO4
PHOSPORIC ACID
HC2H3O2
ACETIC ACID
is an assembly of two or more non-metal atoms
tightly bonded together.
Molecule or molecular compound
is a molecule made from two atoms of the same element.
diatomic molecule
is one of two or more distinct forms of an element, such as: graphite and diamond (for carbon) and dioxygen (O2 - usually referred to simply as oxygen) and ozone (O3).
allotrope
are composed of nonmetal elements that bond together into larger particles using covalent bonds (bonds created by the sharing of their valence electrons.
Molecular compounds (also known as covalent compounds)
show the exact number of atoms of each element in the molecule
Molecular formulas
are the simplest whole-number ratio of the atoms in a molecular compound or an ionic compound..
Empirical formulas
are composed of ions and usually contain both metals and non-metals.
Ionic compounds
A molecular compound contains ALL _________
non-metal elements
molecular compound:
CO
CARBON MONOXIDE
molecular compound:
CO2
CARBOIN DIOXIDE
molecular compound:
NO2
NITROGEN DIOXIDE
molecular compound:
N2O4
DINITROGEN TETRAOXIDE
will start with a metal element or ammonium (NH4) and end with a non-metal or polyatomic ion
IONIC COMPOUND
three main types of ionic compound
binary
polyatomic ion
transition metal
Ionic Compound:
BaCl2
barium chloride
Ionic Compound:
(NH4)SO4
ammonium sulfate
Ionic Compound:
Cu2S
copper I sulfide
Mn(NO3)4
manganese IV nitrate
is the simplest kind of ionic compound. It has only two elements in it (one metal and one nonmetal).
binary ionic compound
naming binary ionic compounds
- write the name of metal ion (same name)
- if non metal, change the ending to -ide
is an ion made from a charged group of bonded atoms consisting of more than
one element.
polyatomic ion
Polyatomic Ion:
NH4 1+
ammonium
Polyatomic Ion:
C2H3O2 1-
acetate
Polyatomic Ion:
CN 1-
cyanide
Polyatomic Ion:
BrO 1-
hypobromite
Polyatomic Ion:
BrO2 1-
bromite
Polyatomic Ion:
BrO3 1-
bromate
Polyatomic Ion:
BrO4 1-
perbromate
Polyatomic Ion:
ClO 1-
hypochlorite
Polyatomic Ion:
ClO2 1-
chlorite
Polyatomic Ion:
ClO3 1-
chlorate
Polyatomic Ion:
ClO4 1-
perchlorate
Polyatomic Ion:
IO 1-
hypoiodite
Polyatomic Ion:
IO2 1-
iodite
Polyatomic Ion:
IO3 1-
iodate
Polyatomic Ion:
IO4 1-
periodate
Polyatomic Ion:
HCO3 1-
hydrogen carbonate
Polyatomic Ion:
H2PO4 1-
dihydrogen phosphate
Polyatomic Ion:
HSO4 1-
hydrogen sulfate
Polyatomic Ion:
NO2 1-
nitrite
Polyatomic Ion:
NO3 1-
nitrate
Polyatomic Ion:
OH 1-
hydroxide
Polyatomic Ion:
MnO4 1-
permanganate
Polyatomic Ion:
SCN1-
thiocyanate
Polyatomic Ion:
CO3 2-
carbonate
Polyatomic Ion:
C2O4 2-
oxalate
Polyatomic Ion:
CrO4 2-
chromate
Polyatomic Ion:
Cr2O7 2-
dichromate
Polyatomic Ion:
HPO4 2-
hydrogen phosphate
Polyatomic Ion:
O2 2-
peroxide
Polyatomic Ion:
SO3 2-
sulfite
Polyatomic Ion:
SO4 2-
sulfate
Polyatomic Ion:
S2O3 2-
thiosulfate
Polyatomic Ion:
PO3 3-
phosphite
Polyatomic Ion:
PO4 3-
phosphate
An acid starts with________ and ends with a nonmetal or polyatomic ion.
hydrogen
naming Binary acids: acids made from hydrogen plus a single element
Hydro + element name + ic Acid
naming Oxyacids: acids made from hydrogen plus an oxygen-containing polyatomic ion
Polyatomic ion name* Acid
(*but change “ate” endings to “ic” and “ite” endings to “ous”)
are ionic compounds that have a specific number of water molecules
attached to them.
Hydrates
are hydrates that have had the water removed (such as through heating).
Anhydrates
common hydrates:
CuSO4 . 5H20
copper II sulfate pentahydrate
common hydrates:
LiCl . H2O
lithium chloride monohydrate
common hydrates:
BaCl2 . 2H2O
barium chloride dehydrate
common hydrates:
MgSO4 . 7H2O
magnesium sulfate heptahydrate
common hydrates:
Sr(NO3)2 . 4H2O
strontium nitrate tetrahydrate
