Mullis 1 Naming Compounds Binary Ionic Compounds • Cation (+ charge ) is listed first. • Name of cation is the chemical name. – For many transition metals, the ion is distinguished by the addition of a roman numeral after the chemical name. – Find charge of the anion and choose appropriate roman numeral to balance the charge. • Name of the anion ends in –ide. Examples: • Al 2 O 3 aluminum oxide • CuBr 2 copper(II) bromide
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Mullis1 Naming Compounds Binary Ionic Compounds Cation (+ charge ) is listed first. Name of cation is the chemical name. –For many transition metals, the.
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Mullis 1
Naming CompoundsBinary Ionic Compounds• Cation (+ charge ) is listed first.• Name of cation is the chemical name.
– For many transition metals, the ion is distinguished by the addition of a roman numeral after the chemical name.
– Find charge of the anion and choose appropriate roman numeral to balance the charge.
• Name of the anion ends in –ide.Examples:• Al2O3 aluminum oxide• CuBr2 copper(II) bromide
Mullis 2
Naming Molecular CompoundsBinary Molecular Compounds• If more than one atom, name the first element with
a numerical prefix.• Name the second element with a numerical prefix
and a suffix –ide.• For prefixes, drop o or a if the element name
begins with a vowel. (Examples are monoxide and pentoxide.)
Examples:• N2O4 dinitrogen tetroxide
• OF2 oxygen difluoride
Mullis 3
Numerical PrefixesNumber Prefix
1 mono-
2 di-
3 tri-
4 tetra-
5 penta-
6 hexa-
7 hepta-
8 octa-
9 nona-
10 deca-
Mullis 4
Polyatomic ions• Poly = many• Atomic = atoms• Entire group of atoms is an ion with a
positive or negative charge.• Within the polyatomic ion, atoms are
bound covalently.• Examples:
Sulfate ionSO4
2-
S
Carbonate ionCO3 2-
C
Mullis 5
Chemical Equations•Law of conservation of mass: Atoms are neither created nor destroyed (in ordinary chemical reactions).
–number of atoms on left = number of atoms on right
•The correct formula must be shown for all reactants and products.
–Use oxidation states and ionic charges to correctly write a formula–In balancing, do not split up molecules or change the formula. –Remember common polyatomic ions and diatomic molecules.
Mullis 6
Symbols used in Equations
Yields
Reversible reaction
Reactants are heated
Catalyst added
(s) solid state or precipitate
(l) liquid state
(g) gaseous state
(aq) aqueous state, or dissolved in water
heator
catalyst
Mullis 7
Order for Balancing• MINOH method (Me know chemistry, said
*An odd # on one side and even on other will require you to multiply the odd side to make it even!
Mullis 8
Steps to balance a chemical equation1. Write the formulas and symbols.Cu(s) + Ag(NO3)(aq) Ag(s) + Cu(NO3)2 (aq) 2. Count the atoms on each side of the arrow.
1 Cu 1 Cu 1 Ag 1 Ag 1 N 2 N 3 O 6 O
3. Balance by using coefficients. Do not change subscripts!
Cu(s) + 2Ag(NO3)(aq) 2Ag(s) + Cu(NO3)2 (aq) 4. Check work by counting each element.
1 Cu 1 Cu 2 Ag 2Ag 2 N 2 N 6 O 6 O
Mullis 9
Two Important Principles
1. Every chemical compound has a formula that cannot be altered.
2. A chemical reaction must account for every atom used. (Law of Conservation of Matter)
Mullis 10
Synthesis reactions(composition reactions)
A + B AB
1. Reactions with O2 or S8
Oxides or sulfides formed
16Rb + S8 8Rb2S 2Mg + O2 2MgO
2. Metals with halogensa. Ionic compounds formedb. Examples are NaF and NaCl
Mullis 11
Synthesis reactions, cont.A + B AB
3. Two compounds combine to form a single product.
N2O3 + H2O 2HNO2
4. Oxides with watera. With metal: Metal hydroxides produced
CaO + H2O Ca(OH)2
b. With nonmetal: Oxyacids produced
SO3 + H2O H2SO4
Mullis 12
Synthesis reactions, cont.A + B AB
5. Metal oxides with CO2
5. Carbonates produced
6. CaO + CO2 CaCO3
6. Metal oxides with SO2
Sulfites produced
CaO + SO2 CaSO3
Mullis 13
Decomposition reactions
AB A + B1. Binary compounds split up
a. Electrolysis is decomposition by electric current
Example: H2O 2H2 + O2
b. Electrolysis is decomposition by electric current
2. Metals with carbonatesa. Metal oxide and carbon dioxide are formed
b. Example: CaCO3 CaO + CO2
3. Metal hydroxidesa. When heated, metal hydroxides decompose to metal oxide and
water.
b. Example: Ca(OH)2 CaO + H2O
electricity
Mullis 14
Decomposition reactions
AB A + B
4. Metal chloratesa. When heated, metal chlorates decompose to
metal chloride and oxygen.
b. Example: 2KClO3 2KCl + 3O2
5. Decomposition of acidsa. Some acids decompose into nonmetal oxides
and water.
b. Example: H2CO3 CO2 + H2O
Mullis 15
Single Replacement Reactions
C + AB A + CB1. Metal replaces another metal
Replacing metal must be the more active metal!
Example: 2Al + 3Pb(NO3)2 3Pb + 2Al(NO3)3
2. Metal replaces H in water
a. Active metals produce metal hydroxide and waterb. Less reactive metals make metal oxide and hydrogen gas
Examples: 2Na + 2H2O 2NaOH + H2
3Fe + 4H2O Fe3O4 + 4H2
Mullis 16
Single Replacement Reactions
C + AB A + CB3. Metal replaces H in an acid
More active metals involved
Example: Mg + 2HCl H2 + MgCl2
4. Halogen replaces another halogenFluorine is most reactive and replaces others.